Chemistry Questions

CHEMISTRY I

1. Question:The temperature at which mercury starts to freeze is -35°C. What is the temperature, in degrees Fahrenheit, at which a mercury thermometer can not be used?

a. -63 °Fb. -35 °Fc. -31 °Fd. -5.4 °F

2. Question:A piece of stone weighs 0.05 pounds. When if is submerged in a graduated cylinder containing 50 mL of H2O, the level rose to 60 mL. What is the density of the stone in g/mL?

a. 2.27b. 2.72c. 7.22d. 7.27

3. Question:A swimming pool 25m wide, 100m long, and 3m deep is filled with water up to a height of 2m. How many kilograms of water have been placed inside the pool? (The density of water is 1000 kg/m3.)

a. 5 millionb. 7.5 millionc. 10 milliond. 12.5 million

4. Question:Which of the following not an example of a compound?

a. sugarb. saltc. ashd. water

5. Question:If two pure substances have different melting points, then

a. the two substances will surely have different densities

b. the two samples are certainly different pure substances

c. the two substances are certain to have identical chemical formulas

d. the two substances are certain to be compounds and not elements

6. Question:Which of the following is a compound?

a. waterb. winec. soil d. mercury

7. Question:Which of the following processes is an example of a chemical change?

a. evaporation of sea water to form salt

b. melting of an ice cubec. filtering of paper pulp from a liquid

slurry using a sieve trayd. rusting of iron

8. Question:We know that air is a homogeneous mixture and not a compound because

a. it has no definite shape b. it has no definite volumec. it ca be compressedd. its composition can vary

9. Question:What do you call a substance that is composed of two or more elements bonded chemically?

a. an isotopeb. an elementc. a compoundd. a mixture

GENERAL ENGINEERING A2 - 1

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10. Question:Which of the following examples is a physical change?

a. crystallization of sugar from sugar can juice

b. fermenting of ethanol to form winec. burning of a piece of candled. clotting of blood

11. Question:Which of the following substances cannot be further decomposed by ordinary chemical means?

a. waterb. sugarc. aird. silver

12. Question:Which of the following not a manifestation of a chemical change?

a. reaction of a compound and an element to form a new compound and an element

b. breaking down of compound into elements

c. combining of atoms of elements to form a molecule

d. separation of the molecules in a mixture

13. Question:What do you call a nuclear reaction resulting from the interaction of two nuclei to form a bigger nucleus and an accompanying release of energy?

a. nuclear fissionb. alpha emissionc. nuclear fusiond. natural radioactive decay

14. Question:

Which of the following materials cannot be subjected to carbon dating to determine its age?

a. a trunk of wood

b. a swordc. a smear of blood on a piece of

clothd. an ancient Egyptian scroll

15. Question:What law states that the pressure of a gas is directly proportional to its absolute temperature at constant volume?

a. Charle’s Law b. Gay-Lussac’s Lawc. Boyle’s Law d. Dalton’s Law

16. Question:To what conditions does a gas behave like an ideal gas?

a. low temperature and low pressureb. low temperature and high

pressurec. high temperature and low

pressured. high temperature and high

pressure

17. Question:What law states that the pressure of gas is inversely proportional to its volume at constant temperature?

a. Charle’s Law b. Gay-Lussac’s Law c. Boyle’s Lawd. Dalton’s Law

18. Question:Which gas diffuses faster?

a. CH4 b. O2 c. CO d. He


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CHEMISTRY I

19. Question:Which of the following best describes heat?

a. the capacity to do work b. forces times distancec. sum of thermal and chemical

energyd. an energy transfer due to a

temperature difference

20. Question:What happens to water when it begins to vaporize?

a. it increases in temperatureb. it decreases in temperaturec. no change in temperatured. no change in thermal energy

21. Question:Burning of gasoline initially requires heat before it burns spontaneously. Which of the following does not give a good explanation of this phenomenon?

a. the initial heat rises the enthalpy of the reactant

b. the initial heat lowers the activation of energy of the reactants

c. the enthalpy of the reactants is lower that the enthalpy of the products

d. the enthalpy of the product is lower than the enthalpy of the reactant.

22. Question:Which of the following is an endothermic process?

a. melting of ice

b. burning of paperc. neutralization of a strong acid and

a strong based. violent reaction of sodium metal

with water

23. Question:Which of the following events is heat exchange involved?

a. when there is a phase changeb. when there is a chemical reactionc. when the gas expands

adiabaticallyd. when there is difference in

temperature

24. Question:Who first predicted the wave-particle dual property of electrons?

a. Hundb. Heisenberg c. De Broglied. Schrödinger

25. Question:Who postulated the wave equation that describes the properties of electrons in an atom?

a. Bohr b. Heisenberg c. Pauli d. Schrödinger

26. Question:Atoms of nonmetals generally reacts with atoms of metals by

a. gaining electrons to form ionic compounds

b. gaining electrons to form covalent compounds

c. sharing electrons to form ionic compounds

d. sharing electrons to form covalent compounds


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CHEMISTRY I

27. Question:The addition of a nonvolatile solute to a solvent will cause

a. the vapor pressure of the solvent to increase

b. the vapor pressure of the solvent to decrease

c. the vapor pressure of the solvent to remain unchanged

d. none of these

28. Question:Which of the following factors does not affect the rate of reaction?

a. the number of products formedb. the nature of reactantsc. temperatured. concentration of reactants

29. Question:Which of the following statements about the catalyst is not true?

a. they may slow down the reaction b. they may speed up the reactionc. they are present in living

substancesd. the may become new substances

after the reaction

30. Question:Which of the following statements about equilibrium is TRUE?

a. it exists in a closed system at varying temperature

b. it exist in an open systemc. it exists between a liquid and its

vapor in a closed system at uniform temperature.

d. it may exist between a solid and a liquid.

31. Question:According to the Bronsted-Lowry theory, an acid is

a. a proton donor b. a proton acceptor

c. a proton donor and a proton acceptor

d. neither a proton donor nor a proton acceptor

32. Question:Which is not true of bases?

a. they always contain OH- ionsb. they neutralize acidc. the pH of their solution is greater

than 7d. they react with H3O+ ions

33. Question:Organic chemistry is the chemistry of compounds containing the element

a. hydrogen b. carbon c. oxygen d. nitrogen

34. Question:What is the mass in grams of 1 liter of carbon monoxide (CO) at standard temperature and pressure (STP)? Note: The molecular weight (MW) of CO is 28 g/mole, and at STP, 1 mole of any gas occupies a volume of 22.4 liters.

a. 1.20b. 1.35c. 1.45d. 1.25

35. Question:Two-thirds of the atom in a molecule of water is hydrogen. What percentage weight of a water


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CHEMISTRY I

molecule if the weight of two hydrogen atoms? The atomic weight of hydrogen is 1.008 g/mol and oxygen is 16.00 g/mole.

a. 19.12b. 11.19c. 19.11d. 12.19

36. Question:How many protons (P) and neutrons are there in the nucleus are present in a Pb nucleus of atomic mass of 206?

a. P = 92, N = 156b. P = 85, N = 160c. P = 82, N = 124d. P = 90, N = 150

37. Question:A 0.064 kg. of octane vapor (MW = 114) is mixed with 0.91 kg of air (MW =29.0) in the manifold of an engine. The total pressure in the manifold is 86.1 kPa, and a temperature is 290 K. Assume octane behaves ideally. What is the partial pressure of the air in the mixture in kPa?

a. 46.8b. 48.6c. 84.6d. 64.8

38. Question:Hydrogen peroxide solution for hair bleaching is usually prepared mixing 5 grams of hydrogen peroxide (H2O2), Molecular weight = 34 g/mole) per 100 ml of solution. What is the molarity of this solution?

a. 1.0 Mb. 1.5 Mc. 1.95 Md. 1.8 M

39. Question:A cylinder contains oxygen at a pressure of 10 atm and a temperature of 300K. The volume of the cylinder is 10 liters. What is the mass of oxygen in grams? Molecular weight (MW) of oxygen is 32 g/mole?

a. 125

b. 130c. 135d. 120

40. Question:The molecular diameter of CO is 3.19x10-8 at 300K and pressure of 100 mmHg. What is the mean free path of the gas in cm?

a. 6.86 x 10-3

b. 6.86 x 10-5

c. 2.86 x 10-4

d. 6.86 x 10-9

41. Question:How many moles are there in one atom?

a. 3.6 x 10-23

b. 1.66 x 10-24

c. 2.86 x 10-4

d. 6.86 x 10-9

42. Question:When 0.5g of liquid is completely evaporated and collected in liter manometer, the pressure is 0.25 atm and the temperature is 27°C. Assume ideal gas behavior, find the molecular weight if the gas constant is 0.0821L.atm/mole.K.

a. 49.2 g/moleb. 12.3 g/molec. 2.2 g/moled. 64.0 g/mole

43. Question:


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CHEMISTRY I

If the atomic weight of magnesium is 24.3 g/mol, calculate how many magnesium atoms does 5g represent?

a. 1.24 x 1023 atomsb. 1.76 x 1023 atomsc. 3.44 x 1023 atomsd. 2.76 x 1023 atoms

44. Question:How many moles of iron does 25 g of Fe represent? Note: the atomic weight of iron (Fe) is 55.8 g/mol.

a. 0.356 molb. 0.564 molc. 0.448 mold. 0.247 mol

45. Question:How many oxygen atoms are present in 2.00 moles of oxygen molecules considering that is a diatomic?

a. 2.40 x 1024 atomsb. 3.43 x 1025 atomsc. 5.67 x 1026 atomsd. 1.34 x 1024 atoms

46. Question:If the atomic mass of copper (Cu) if 63.5 g/mol, compute how many grams does 0.252 mole of copper (Cu) has?

a. 16 gb. 18 gc. 20 gd. 12 g

47. Question:What is the molecular weight of calcium hydroxide or Ca(OH)2?

a. 74b. 67

c. 80d. 44

48. Question:How many molecules are there in 25 g of hydrogen Chloride, HCl?

a. 4.12 x 1023 moleculesb. 4.32 x 1023 moleculesc. 5.34 x 1023 moleculesd. 3.45 x 1023 molecules

49. Question:What is the percentage composition of a sodium in the sodium chloride compound?

a. 60.7%b. 34.6%c. 39.3%d. 50.7%

50. Question:What is the composition of oxygen of potassium sulfate, K2SO4?

a. 53.2%b. 36.7%c. 50.4%d. 43.4%

51. Question:A 1.63 g of zinc when heated in air combined with 0.40 g of oxygen to form oxide of zinc. What is the percentage composition of Zn in the compound formed?

a. 80.3%b. 76.5%c. 19.7%d. 53.4%

52. Question:Calculate how many moles of ammonia can be produced from 8 mol of hydrogen reacting with nitrogen?


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CHEMISTRY I

a. 4.53 mol NH3

b. 7.76 mol NH3

c. 5.33 mol NH3

d. 4.57 mol NH3

53. Question:How many molecules of water can be produced by reacting 0.010 mol of oxygen with hydrogen?

a. 1.20 x 1022 moleculesb. 1.32 x 1022 moleculesc. 2.34 x 1022 moleculesd. 4.15 x 1022 molecules

54. Question:If 2 liters of gas measured at STP weigh 3.23 g, what is the molecular weight of the gas?

a. 36.2 g/molb. 42.3 g/molc. 24.7 g/mold. 19.4 g/mol

55. Question:An ethyl ether 691 L weighs 1.65 g measured at 40C and 630 torr. Compute the molecular weight of ethyl ether.


56. Question:Calculate the specific gravity of Cl2 at STP. Note: the molecular weight of Cl2 is 71 g/mol.

a. 3.45b. 1.23c. 2.46d. 1.76

57. Question:Compute the volume of oxygen at STP that can be formed from a 0.75 mole of potassium chlorate (KClO3).

a. 18.6 litersb. 16.8 litersc. 25.2 litersd. 23.2 liters

58. Question:What pressure will be exerted by a 0.50 mol of gas in a 7 L container at 23C?

a. 1.74 atmb. 2.05 atmc. 3.04 atmd. 1.32 atm

59. Question:Compute how many moles of oxygen has are in a 70 L tank at 25C if the pressure is 2000 psi?

a. 389.3 molb. 453.4 molc. 145.7 mold. 247.4 mol

60. Question:What is the molality of the solution that contains 65 g of sucrose (C12H22O11) dissolved in 300 g of water?

a. 0.89 mole/kgb. 0.78 mole/kgc. 0.54 mole/kgd. 0.63 mole/kg

61. Question:Calculate the number of moles of an ideal gas sample at 0.6 atmosphere and 87C occupies 0.450 liter.

a. 0.0091 moleb. 0.0087 molec. 0.0076 moled. 0.0056 mole

62. Question:One gram of hydrogen gas (H2) is combined with 10 g of helium (He) gas and confined at 20C and 5


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atmospheres. What is the combined volume in liters?

a. 14.4 litersb. 17.5 litersc. 16.4 litersd. 12.7 liters

63. Question:What is the molarity of the solution if 150 g of KCl is dissolved in water to make 800 mL solution?

a. 2.51 moles/Lb. 2.25 moles/Lc. 2.87 moles/Ld. 1.53 moles/L

64. Question:Compute how many grams of KCl must be dissolved in water so that it can produce a 400 L of 0.6 M (molarity) solution?

a. 17.904 gb. 14.281 gc. 11.541 gd. 12.653 g

65. Question:What is the atomic weight of calcium if 2.25 g of pure calcium metal are converted to 3.13 g of pure CaO?


66. Question:What is the equivalent weight of Sulfuric Acid (H2SO4).

a. 49b. 98c. 23d. 100

67. Question:If 60 g of H2SO4 is dissolved in water to make a 1.5 L solution, find its normality N?

a. 0.813 equiv/Lb. 0.576 equiv/Lc. 0.871 equiv/Ld. 0.765 equiv/L

68. Question:What is the equivalent weight of Mg(OH)2?

a. 23 g/molb. 29 g/molc. 58 g/mold. 20 g/mol

69. Question:How many grams of H3PO4 are confined in 700 mL container if its normality is 0.5?

a. 11.45 gb. 12.34 gc. 10.56 gd. 9.35 g

70. Question:Which of the following is the simplest balanced equation of the given reaction? Na2CO3 + HCl NaCl + H2O + CO2

a. Na2CO3 + 2HCl 2NaCl + H2O + CO2

b. Na2CO3 + 2HCl NaCl + 2H2O + CO2

c. 2Na2CO3 + HCl 2NaCl + H2O + CO2

d. 2Na2CO3 + HCl NaCl + H2O + 2CO2


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CHEMISTRY I

71. Question:If the molecular formula of water is H2O, then what is its molecular mass?

a. 18 amub. 19 amuc. 20 amud. 1 amu

72. Question:What is the molecular weight of barium chloride dehydrate BaCl22(H2O)?

a. 234.4 amub. 244.3 amuc. 270.5 amud. 298.5 amu

73. Question:Which of the following is the simplest balanced equation of the given Oxidation-Reduction Equation? P + HNO3 + H2O NO + H3PO4

a. 2P + HNO3 + H2O NO + 2H3PO4

b. 3P + HNO3 + H2O NO + 3H3PO4

c. 3P + 5HNO3 + 2H2O 5NO + 3H3PO4

d. 3P + HNO3 + 2H2O 2NO + 3H3PO4

74. Question:What type of bond results in form the sharing of electrons by two atoms?

a. atomic bondb. covalent bondc. metallic bond

d. ionic bond

75. Question:Which of the following statements regarding organic substances is FALSE?

a. Organic substances generally dissolve in high concentration acids

b. All organic matter contains carbonc. Organic matter is generally stable

at very high temperaturesd. Organic substances generally do

not dissolve in water

76. Question:What do you call a substance that dissociates in solutions to produce positive and negative ions?

a. baseb. acidc. electrolyted. solute

77. Question:During a complete or partial neutralization of acids, what is the ionic compound formed?

a. saltb. sugarc. potassiumd. sulfur

78. Question:Which of the following is most likely to prove that a substance is inorganic?

a. the substance evaporates in room temperature and pressure

b. the substance is heated together with copper oxide and the resulting gases are found to have no effect on limestone


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c. analysis shows that the substance contains hydrogen

d. the substance floats in water

79. Question:Which of the following are found in the nucleus of an atom?

a. electrons and protonsb. electrons and neutronsc. protons and neutronsd. electrons, protons and neutrons

80. Question:Which of the following elements and compounds is unstable in its pure form?

a. Helium (He)b. Neon (Ne)c. Carbon dioxide (CO2)d. Sodium (Na)

81. Question:What refers to the negatively charge component of an atom?

a. electronb. protonc. neutrond. ion

82. Question:Which of the following is the simplest type of reaction where two elements of compounds combine directly to form a compound?

a. directly combination or synthesisb. decomposition or analysisc. single displacementd. double displacement

83. Question:What do you call the bonding that occurs in inert gases and other elements with full shells, primarily due to attraction between dipole structures?

a. ionicb. metallicc. covalentd. van de waals

84. Question:If the heat of a solution is negative, heat is given off when the solute dissolves in the solvent. What type of reaction is this?

a. exothermicb. idealc. endothermic

d. efflorescent

85. Question:What do you call materials that do not conduct electric current?

a. conductorb. insulatorc. semi-conductord. intrinsic material

86. Question:What element is known as the lightest metal?

a. aluminumb. manganesec. Magnesiumd. Lithium

87. Question:Which of the following is energy removal being applied?

a. evaporation of waterb. changing water to steamc. changing water to iced. all of these


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88. Question:Halogens fall under what group in the periodic table?

a. group VIAb. group VAc. group IVAd. group VIIA

89. Question:Which of the following is added to the drinking water distribution system for disinfection?

a. Soda ashb. Chlorinec. Limed. Iodine

90. Question:What refers to the number of gram equivalent weights of solute per liter of solution?

a. molarity (M)b. normalityc. molality (m)d. formality

91. Question:Is the attraction between like molecules.

a. absorptionb. diffusionc. adhesiond. cohesion

92. Question:What do you call a substance that cannot be decomposed any further by a chemical reaction?

a. ionb. elementc. moleculed. atom

93. Question:One of the following is the standard pressure and temperature. Which one?

a. 0°C and one atmosphere pressure

b. 0°C and zero pressurec. 0°F and one atmosphered. 32°F and zero pressure

94. Question:Which of the following is the strongest type of bonds?

a. Van de Waalsb. Metallicc. Covalentd. Ionic

95. Question:Sublimation is a direct change from:

a. solid to liquid phaseb. solid to gaseous phasec. liquid to gaseous phased. gaseous phase to liquid phase

96. Question:What do you call hydrocarbons containing carbon to carbon double bonds?

a. Alkanesb. Alkenesc. Alkynesd. None of these

97. Question:How are materials containing atoms with less than 4-valence electrons classified?

a. an insulatorb. a semi-conductorc. a conductord. a compound

98. Question:


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Which of the following has the characteristics of both metals and non-metals?

a. conductorsb. insulatorsc. metalloidsd. meteors

99. Question:Which are oxidizing and reducing agents in the following reactions?2CCl4 + K2CrO4 2Cl2CO + CrO2Cl2

+ 2 KCl

a. there are no oxidizing and reducing agents in this reaction

b. oxidizing agent: chromium; reducing agent: chlorine

c. oxidizing agent: chlorine; reducing agent: carbon

d. oxidizing agent: oxygen; reducing agent: chlorine

100. Question:How are elements numbered 58 to 71 in the periodic table called?

a. Lanthanonsb. Actinonsc. Earth metalsd. Noble gas

101. Question:What type of bonding in which electrostatic attraction is predominant?

a. Ionic bondingb. Metallic bondingc. Covalent bondingd. Van der Waals bonding

102. Question:What term refers to the passage of an electric current trough an electrolyte caused by an external voltage source?

a. electrolysisb. electromechanical actionc. electrolyted. piezoelectric effect

103. Question:When all of the atoms of a molecule are the same, the substance is called _____.

a. a compoundb. a chemicalc. an elementd. an ion

104. Question:Which of the following refers to the measure of the amount of negative ions in the water?

a. acidityb. alkalinityc. turbidityd. molarity

105. Question:What device produces electrical current by way of an oxidation-reduction reaction?

a. generatorb. galvanic cellc. metallic frictiond. all of these

106. Question:What is the maximum number of electrons that can be accommodated in the valence shell of an atom?

a. 6b. 8c. 10d. 12

107. Question:


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Reactions generally proceed faster at high temperatures because of which of the following?

a. the molecules are less energeticb. the molecules collide more

frequentlyc. the activation energy is lessd. the molecules collide more

frequently and the activation energy is less

108. Question:Which component of an atom has no electric charge?

a. protonb. neutronc. coulombd. electron

109. Question:Adding more solute to an already saturated solution will cause the excess solute to settle to the bottom of the container. What is this process called?

a. precipitationb. hydrationc. dehydrationd. saturation

110. Question:What is formed when acids will react with active metals?

a. sulfurb. oxygenc. hydrogend. chloride

111. Question:How much is the pH content of an acid?

a. between 4 and 6b. between 2 and 7c. between 1 and 5d. between 0 and 7

112. Question:The condition of a liquid electrolyte is measured in terms of its:

a. specific gravityb. acid contentc. voltage outputd. current value

113. Question:What is a substance that speeds up a chemical reaction without itself undergoing a chemical change?

a. ingredientsb. reactantsc. solventd. catalyst

114. Question:How are elements numbered 90 to 103 in the periodic table called?

a. alkalib. actinonsc. earth metalsd. transition elements

115. Question:What is defined as a value equal to the number of gram moles of solute per 1000 grams of solvent?

a. Molality (m)b. Normalityc. Molarity (M)d. Formality


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116. Question:Which of the following is NOT a part of an atom?

a. electronb. protonc. neutrond. coulomb

117. Question:An element maybe defines as a substance, all atoms of which have the same:

a. number of neutronsb. radioactivityc. atomic weightd. atomic number

118. Question:How does all B families and group VII in the periodic table named?

a. light metalsb. rare earth metalsc. non-metalsd. transition metals

119. Question:The device which measures the acid content of the cell is called _____.

a. acid meterb. hydrometerc. hygrometerd. pyrometer

120. Question:The vertical columns in the periodic table are called:

a. Groupsb. Sectionsc. Batchesd. Families

121. Question:What term is used to refer to a negatively charged ion?

a. Anionb. Cathodec. Anoded. Cation

122. Question:In a copper atom, the valence ring contains:

a. no electronsb. one electronsc. two electronsd. four electrons

123. Question:The elements along the dark line in the periodic table are referred to as _____.

a. Light metalsb. Metalloidsc. Non-metalsd. Heavy metals

124. Question:What do you call an atom that loses some of its electron or accepts extra electrons from another atom?

a. Intrinsic

b. Molec. Neutrond. Ion

125. Question:A _____ is a cell designed to produce electric current and can be recharged.

a. Secondary cellb. electrolytic cellc. chemical celld. battery

126. Question:


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Which of the following groups in the periodic table the most strongly electronegative elements?

a. Group IVb. Group Vc. Group VIIAd. Group VIA

127. Question:Which of the following statement is FALSE?

a. In general, as reaction products are formed, they react with each other and reform reactants.

b. At equilibrium, the net reaction rate is zero.

c. The differential rate is the mathematical expression that shows how the rate of reaction depends on volume.

d. The net rate at which a reaction proceeds from left to right is equal to the forward rate minus the reverse rate.

128. Question:What is the smallest part of matter?

a. moleculeb. elementc. particled. atom

129. Question:The opposite of alkali

a. acidb. fluidc. substanced. none of these

130. Question:What type of reaction has two compounds as reactants and two compounds as products?

a. Direct combination or synthesis

b. Decomposition or synthesisc. Single displacementd. Double displacement

131. Question:If the heat of a solution is positive, heat is absorbed when the solute dissolves in the solvent. What type of reaction is this?

a. Exothermicb. Idealc. Endothermicd. Efflorescent

132. Question:The amount of electricity a battery can produce is controlled by

a. the thickness of the plateb. the plate surface areac. the strength of the acidd. the discharge load

133. Question:What do you call the electrons in the last orbit or shell of an atom?

a. Bound electronsb. Free electronsc. Valence electronsd. External electrons

134. Question:Which one is the positively charged ion?

a. anion

b. cathodec. anoded. cation

135. Question:It is the number of protons in the nucleus of an atom

a. Molecular numberb. Proton numberc. Mass numberd. Atomic number


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136. Question:What do you call the elements in the first two groups in the periodic table?

a. Light metalsb. Noble gasc. Non-metalsd. Heavy metals

137. Question:Which one refers to the number of gram-moles of solute per liter of solution?

a. Molality (m)b. Normalityc. Molarity (M)d. Formality

138. Question:What type of bonding is electrostatic attraction most predominant?

a. Ionicb. Metallicc. Covalentd. Van der Waals

139. Question:When the charge of an atom becomes unbalanced, the charge atom is called _____.

a. an ionb. a neutronc. a protond. an electron

140. Question:Which of the following type of reactions in which bonds within a compound are disrupted by heat or other energy to produce simpler compounds or elements?

a. direct combination or synthesisb. decomposition or analysisc. single displacementd. double displacement

141. Question:What do you call hydrocarbons containing carbon to carbon triple bonds?

a. alkanesb. alkenesc. alkynesd. non of these

142. Question:If an atom contains more than four valence electrons, the material is classified as _____.

a. insulatorb. semi-conductorc. conductord. any of these

143. Question:Which of the following refers to a measure of the quantity of an element or compound?

a. Oxidation numberb. Atomic numberc. Avogadro’s numberd. Mole

144. Question:The electrolyte is a solution of water and _____.

a. sulfuric acidb. uric acidc. nitric acidd. formic acid

145. Question:Acids will turn blue litmus paper to what color?

a. grayb. yellowc. violetd. red

146. Question:


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How much is the pH content of a base?

a. between 6 and 10 b. between 2 and 7c. between 7 and 14d. between 10 and 16

147. Question:Applying a greater pressure causes pure solvent to leave the solution. What is the name of this process?

a. cavitationb. calcinationc. purificationd. reverse osmosis

148. Question:A deuteron is

a. a neutron plus two protonsb. a nucleus containing a neutron

and a protonc. an electron with a positive changed. a helium nucleus

149. Question:Which of the following groups in the periodic table the most weakly electronegative elements?

a. Group IIAb. Group IAc. Group IIIAd. Group IVA

150. Question:What type of bonding that occurs in metals when metal atoms lose electrons and the metallic ions are attracted to a “sea” of delocalized electrons?

a. ionic bondingb. metallic bonding

c. covalent bondingd. van der waals bonding

151. Question:Which of the following elements is NOT radioactive?

a. Plutoniumb. Californiumc. Uraniumd. Cobalt

152. Question:Which of the following refers to a nucleic acid that stores genetic information?

a. Celluloseb. Codonc. DNAd. Buffer

153. Question:During chemical reactions, bonds between atoms are broken and new bonds are usually formed. What do you call the starting substances?

a. Productsb. Reactantsc. Catalystd. Ingredients

154. Question:What do you call solutions having the same osmotic pressure?

a. Isotonic solutionsb. Monohydroxic solutionsc. Dihydroxic solutionsd. Toxic solutions

155. Question:What is the term used to describe hydrocarbons containing single covalent bonds between carbon atoms?

a. alkanesb. alkenes


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c. alkynesd. allotrope

156. Question:The smallest whole unit of an element like Uranium is:

a. moleculeb. atomc. iond. electron

157. Question:What refers to the formation and collapse of minute bubbles of vapor in liquid which caused by a combination of reduced pressure and increased velocity in the fluid?

a. cavitationb. stress corrosionc. fatigue corrosiond. precipitation

158. Question:The elements in Group 0 in the periodic table is called_____.

a. light metalsb. rare earth metalsc. noble gasd. heavy metals

159. Question:A pair of electrical conductors of dissimilar materials so joined as to produce a thermal emf when the junctions are of different temperatures.

a. potentiometerb. piezoelectricc. thermocoupled. solar heating

160. Question:Bases will turn red litmus paper to what color?

a. blueb. yellowc. violetd. green

161. Question:Which of the following refers to the diffusion of a solvent into a stronger solution in an attempt to equalize the two concentrations?

a. purificationb. electrolysisc. osmosisd. hydrolysis

162. Question:The formula for Dinitrogen Pentoxide is:

a. N2O5

b. (NO)5

c. NOd. none of these

163. Question:Which of the following will occur if a substance is oxidized?

a. it absorbs energyb. it loses electronsc. it becomes more negatived. it gives off heat

164. Question:What type of reaction has one element and one compound as reactants?

a. direct combination or synthesis


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b. decomposition of analysisc. single displacementd. double displacement

165. Question:Which of the following is the atomic number of silicon?

a. 32b. 24c. 14d. 28

166. Question:Dielectric is another name for _____.

a. a conductorb. an elementc. an insulatord. a capacitor

167. Question:Which of the following refers to the change from gaseous to liquid phase?

a. condensationb. vaporizationc. sublimationd. ionization

168. Question: “At the same, pressure and temperature, equal volumes of all gasses contain equal number of molecules.” This is known as

a. Boyle’s Lawb. Faraday’s Lawc. Avogadro’s Lawd. Charles’ Law

169. Question:The galvanic cell is not dependent of which factor?

a. temperature

b. pressurec. volumed. chemical substance

170. Question:Which of the following refers to the number of protons and neutrons in the nucleus of an atm?

a. atomic weightb. atomic massc. atomic constantd. atomic number

171. Question:One of the following statements is wrong. Which one is it?

a. Electron is an elementary quantity of negative electricity

b. proton is an elementary quantity of positive electricity

c. an atom is composed of a central nucleus and orbital electrons

d. the mass of an electron is heavier than that of a proton

172. Question:During a chemical reactions, bonds between atoms are broken and new bonds are usually formed. The ending substance is called _____.

a. productsb. reactantsc. catalystd. ingredients

173. Question:What is the smallest subdivision of an element of compound that can exist in a natural state?

a. atomb. moleculec. ion

d. element

174. Question:


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The sharing of one or more electron pairs between nuclei. It usually occurs when the electronegativity difference between bonding species is less than 1.5

a. Bridge Bonding b. Ionic Bondingc. Covalent Bonding d. Valence Bonding

175. Question:The name of this group is the chalcogen (oxygen) family.

a. Group IIAb. Group IVAc. Group VIAd. Group VIIIA

176. Question:The amount of energy to change 1 g of liquid to gas at its boiling point.

a. enthalpy of formationb. enthalpy of fusionc. enthalpy of reactiond. enthalpy of vaporization

177. Question:The fragmentation of a crystal along a characteristic crystallographic direction, caused by lines of weakness in constituent atomic groups.

a. cleavageb. fracturec. lusterd. streak

178. Question:

A bond formed by the sideways overlap of two parallel p orbitals.

a. Peptide Bondb. Pi Bondc. Saturated Bondd. Delta Bond

179. Question:This indicator turns into colorless if the substance is acidic.

a. Phenolphthaleinb. Methyl orangec. Litmus paperd. Bromthymol blue

180. Question:A chemical structure with definite formula for which there exists one or more distinct structures with the same formula.

a. Isomerb. Radicalc. Groupd. Colloid

181. Question:A substance that can be decomposed into 2 or more simpler substances by ordinary chemical means.

a. Elementb. Mixturec. Compoundd. Solution

182. Question:A theory which treats bonding as an over lapping of ligand orbitals with those of the central atom.

a. Ligand Field Theoryb. Crystal Fields Theoryc. Chelate Effectd. Molecular Orbital Theory


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183. Question:Known as fool’s gold.

a. Quartzb. Cinnabarc. Feldspard. Pyrite

184. Question:It is the hardest substance known

a. Wadb. Graphitec. Diamondd. Adamantium

185. Question:The splitting of water to form hydrogen and oxygen

a. reductionb. electrolysisc. oxidationd. hydrolysis

186. Question:Which is not an open chain hydrocarbon classification?

a. alkenesb. alkanesc. cycloalkanesd. alkynes

187. Question:The process of producing ions from neutral species.

a. Fractional Distillationb. Hydrationc. Recombinationd. Ionization

188. Question:A chemical bond with “sausage roll” shape formed by the sideways overlap of two d orbitals.

a. Peptide Bondb. Pi Bondc. Saturated Bondd. Delta Bond

189. Question:Multidentate ligands have equal probability of forming a coordination bond as do monodentate ions.

a. Ligand Field Theoryb. Pauling’s Rulec. Chelate Effectd. Molecular Orbital Theory

190 Question:It has no definite composition whose members are composed of two or more substances, each retaining its own identifying properties.

a. Homogeneous Mixtureb. Heterogeneous Mixturec. Aqueous Mixtured. Ingeneous Mixture

191. Question:A chemical compound having one or more unpaired electrons which is capable of bonding with another compound.

a. Labileb. Resonance Hybridc. Free Radicald. Isodemic Crystal

192. Question:The mineral name for common table salt

a. Haliteb. Cassieritec. Aragonited. Calcite

193. Question:Any process that involves the loss of electrons.

a. Reductionb. Exsolutionc. Oxidationd. Hydrolysis


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194. Question:Elements normally found in combination with iron and nickel.

a. Noble Metalsb. Promethiumc. Tritiumd. Siderophile

195. Question:Any substances that changes the rate of a reaction without being used up.

a. Catalystb. Enzymec. Reactord. Stimulus

196. Question:A/An ____ of chemical substances is, by definition, the number in grams corresponding to the atomic or molecular mass.

a. atiomic massb. atomic weightc. moled. ion

197. Question:A reaction in which an unstable reaction intermediate is found

a. Coupled Substitutionb. Free Radical Reactionc. Polar Reactiond. Concentrated Reaction

198. Question:A reaction for which the difference between enthalpies of formation between products and reactants is positive.

a. Intrathermicb. Exothermicc. Endothermicd. Isothermic

199. Question:The ______ is the heat released of absorbed in a chemical reaction at constant pressure when simple substances combine into a more complex substance.

a. enthalpy of formationb. enthalpy of fusionc. enthalpy of reactiond. enthalpy of vaporization

200. Question:Characteristic based upon the reaction of a substance with other materials.

a. Chemical Property b. Colligative Propertyc. Nuclear Property d. Physical Property

201. Question:A symmetrical intergrowth of two or more crystals of the same substance.

a. Twinb. Isomerc. Epitaxisd. Habit

202. Question:A compound which is gaseous at ambient temperature and pressure and which is easily melted.

a. Volatileb. Solublec. Liquidusd. Solidus

203 Question:The energy required to form gaseous monatomic species.

a. Bond Energy b. Dissociation Energy


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c. Activation Energy d. Light Energy

204. Question:The amount of energy released as on mole of a given substance is burned in the presence of oxygen.

a. Nuclear Energyb. Enthalpy of Reactionc. Trans Effectd. Heat of Combustion

205. Question:The most diamagnetic naturally occurring material.

a. Ironb. Galliumc. Bismuthd. Silicon

206. Question:Any Process that involves the gain of electrons.


207. Question:The change of the thermodynamic state function enthalpy due to a chemical reaction.

a. enthalpy of formation b. enthalpy of fusionc. enthalpy of reactiond. enthalpy of vaporization

208. Question:A concept invented by Linus Pauling to measure the tendency for atoms to form ionic instead of covalent bonds.

a. Electromagnetism b. Electropositivity

c. Electronegativity d. Electrodynamism

209. Question:A substance whose particles are strongly attracted to each other (e.g., gelatin)

a. Colligativeb. Hydrophilicc. Hydrophobicd. Cohesive

210. Question:The most common form of calcium carbonate.

a. Haliteb. Cassieritec. Aragonited. Calcite

211. Question:The substance that undergoes phase change in the process of dissolving

a. Radicalb. Isomerc. Solventd. Solute

212. Question:A process in which water molecules are attracted to and form weak bonds with the solute species.

a. Hydrationb. Oxidationc. Combustiond. Reduction

213. Question:The dissociation of a chemical species resulting from its absorption of a photon.

a. Photosynthesis


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b. Photolithographyc. Photosensitization d. Photodissociation

214. Question:_____ is the mineral name for lead sulfide (PbS). It is the most important ore of lead.

a. Saltpeterb. Gypsumc. Galenad. Silicate

215. Question:A substance that does not undergo chemical reactions is said to be _____.

a. inertb. labilec. alkalined. amorphous

216. Question:Which bond strength is weak?

a. Macromolecular covalent bondsb. Ionic bondsc, Hydrogen bondsd. Van der Waals forces

217. Question:Occurs with the bonding electron pair remaining intact.


218. Question:A mixture composed of a suspended and a mobile phase.

a. Isomerb. Radicalc. Suspension

d. Colloid

219. Question:A/An _____ is a biological catalyst.

a. Amino acidsb. Genesc. DNAd. Enzyme

220. Question:The first covalent bond formed between two nuclei is always a _____. They are formed when two s orbitals, one s and one p orbital, two p orbitals, or two d orbitals overlap.

a. Peptide Bondb. Pi Bondc. Sigma Bondd. Bridge Bond

221. Question:The process by which solutions are decomposed into their components by using differences in their boiling points.

a. Fractional Distillationb. Filtrationc. Recombinationd. Ionization

222. Question:Filtration through a semi-permeable membrane used to separate colloids.

a. Dialysis b. Hydrolysisc. Electrolysis d. Chromatography

223. Question:


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In orbitals of identical energy, electrons remain unpaired if possible in order to minimize electron-electron repulsion.

a. Spin Multiplicity Ruleb. Selection Rulesc. Hund’s Ruled. Pauling’s Rules

224. Question:Elements with the same outermost shell are said to belong to the same _____.

a. spinb. periodc. valenced. slot

225. Question:An alkyl sulfate alkali.

a. Detergentb. Acetonec. Ethylened. Oil

226. Question:The process whereby an excited species transfers its energy to another excited species which subsequently undergoes a reaction

a. Photosynthesis b. Photolithographyc. Photosensitization d. Photodissociation

227. Question:_____ is the study of hydrocarbon compounds, i.e. substances consisting of the elements hydrogen, carbon, and oxygen.

a. Inorganic Chemistry b. Organic Chemistryc. Quantum Chemistry d. Biochemistry

228. Question:_____ displays all chemical elements systematically in order of increasing atomic number.

a. Phase Diagram b. Polarization Spectrumc. Periodic Table d. Elements Archive

229. Question:A substance composed of a single type of atom

a. Atomb. Compoundc. Solutiond. Colloid

230. Question:A group of elements which are gaseous at room temperature and pressure, and called so because they rarely bond with other elements.

a. Tetratomic Elementsb. Noble Gasesc. Alkalid. Lanthanide

231. Question:An element which is not found naturally on Earth. It has been found in the star HR465 in Andromeda.

a. Adamantiumb. Promethuimc. Tritiumd. Adolinium

232. Question:A form of elemental carbon which, because of its sheet structure, is an excellent lubricant.

a. graphiteb. Carbonc. Soot


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d. Coal

233. Question:Which is not one of the periodic properties?

a. electronegativityb. electron affinityc. radioactive decay coefficientd. atomic radius

234. Question:The reflection of light beam passing through a colloid which identifies the presence of suspended particles.

a. Tyndall Effect b. Brownian Movementc. Raoult’s Law d. Trans Effect

235. Question:An ionic compound containing a halogen.

a. Halideb. Lanthanidec. Alkalided. Sulfide

236. Question:A reaction for which the difference between enthalpies of information between products and reactants is negative.

a. Intrathermicb. Exothermicc. Endothermicd. Isothermic

237. Question:The quantity of energy released as one mole of bonds are produced between atoms.

a. Bond Energy b. Light Energy

c. Activation Energy d. Atomization Energy

238. Question:An ion with negative charge

a. Cationb. Anionc. Muond. Neutrino

239. Question:_____ is a measure of the acidity of alkalinity of a substance.

a. HPb. dBc. pHd. Pro-V

240. Question:Two-phase mixture composed of a dispersed and continuous phase.

a. Isomerb. Radicalc. Suspensiond. Colloid

241. Question:A solvent for atoms.

a. Fluxb. Waterc. Inert Gasesd. Kryptonite

242. Question:A class of matter with definite properties whose members are composed of two or more substances, each retaining its own identifying properties.

a. Homogeneous Mixtureb. Heterogeneous Mixturec. Solid Solution


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CHEMISTRY I

d. Ingeneous Matter

243. Question:A crystal for which all bonds have the same electrostatic valency.

a. Labileb. Resonance Hybridc. Free Radicald. Isodemic Crystal

244. Question:The ______ is a system of reference materials against whose hardness a sample is compared.

a. Richter scaleb. Mohs hardness scalec. Cavendish balanced. Brinell hardness model

245. Question:Magma with most of the gas component escaped.

a. Lavab. Cinderc. Sulphurd. Coal

246. Question:Minerals having high melting temperatures.

a. Endogenicb. andesiticc. Graniticd. Basaltic

247. Question:_____ minerals are those having low melting temperatures.

a. Endogenicb. Andesiticc. Graniticd. Basaltic

248. Question:

The transfer of one or more electrons from a metal to a nonmetal. Electron transfer usually occurs when the electronegativity difference between bonding species is 1.5 or more.

a. Bridge Bonding b. Ionic Bondingc. Covalent Bonding d. Valence Bonding

249. Question:The non-random overgrowth of two compositionally different crystalline substances.

a. Twinb. Isomerc. Epitaxis d. Habit

250. Question:The angles between equivalent faces of crystals of the same substance, measured at the same temperature, are constant.

a. Bravais Lawb. Hall Effectc. Tyndall Effectd. Steno Law

251. Question:The chemical element having the greatest binding energy per nucleon.

a. Ironb. Galliumc. Bismuthd. Platinum

252. Question:


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CHEMISTRY I

Any type of reaction that involves the pairing of unpairing of electrons.


253. Question:It is the form of oxygen consisting of three bound oxygen atoms.

a. Halogenb. Halidec. Oxided. Ozone

254. Question:A group of elements with similar properties in which the outer-most

electron shell is a partially filled f sublevel.

a. Tetratomic Elementsb. Noble Gasesc. Alkalid. Lanthanide

255. Question:A substance whose particles are only weakly attracted to each other (e.g., water)

a. Colligativeb. Hydrophilicc. Hydrophobicd. Refractory

256. Question:A class of homogeneous matter which has a definite composition by weight.

a. compoundb. mixturec. elementd. substance

257. Question:

In the periodic table, Group IA is for the:

a. Halogensb. Light metalsc. Alkaline metalsd. Alkali metals

258. Question:A covalent bond formed through a condensation reaction that involves removal of a water molecule.

a. Peptide Bondb. Pi Bondc. Sigma Bondd. Bridge Bond

259. Question:Which group is the nitrogen family?

a. Group VAb. Group IVAc. Group IIIAd. Group IIA

260. Question:Litmus paper turns into _____ is the substance is basic.

a. colorlessb. yellowc. redd. blue

261. Question:A property which depends only on the number of particles present, and not their chemical composition.

a. Chemical Propertyb. Colligative Propertyc. Nuclear Propertyd. Physical Property

262. Question:


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CHEMISTRY I

The amount of energy to change 1g of solid to liquid at its melting point.

a. enthalpy of formationb. enthalpy of fusionc. enthalpy of reactiond. enthalpy of evaporation

263. Question:The process whereby an initially homogeneous solid solution separates into two (or more) distinct crystalline minerals without the addition or removal of materials to or from the system.


264. Question:The separation of component particles from the bulk or mass.

a. Dissociationb. Atomizationc. Fissiond. Reduction

265. Question:An ion with positive charge.

a. Cationb. Anionc. Muond. Neutrino

266. Question:A cell which uses the flow of electrons from a spontaneous chemical reaction to do outside work.

a. Daniel Cellb. Gravity Cellc. Concentration Celld. Galvanic Cell

267. Question:The anion OH-.

a. Hydrideb. Oxidec. Hydroxided. Nitrate

268. Question:A measure of the tendency of a gas to escape or expand.

a. Compressibilityb. Fugacityc. Vaporizabilityd. Solubility

269. Question:An ionic theory which is an offshoot of electrostatic theory. It ignores all covalent bonding effects.

a. Ligand Field Theoryb. Crystal Fields Theoryc. Chelate Effectd. Molecular Orbital Theory

270. Question:A purple form of quartz whose color arises from Fe+4.

a. Amethystb. Rubyc. Topazd. Peridot

271. Question:A/An _____ is a hydrocarbon consisting only of single carbon-carbon bonds

a. Alkyneb. Alkene


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CHEMISTRY I

c. Alkaned. Amide

272. Question:A large polypeptide of the kind found in living organisms.

a. Amino Acidb. Proteinc. Mineralsd. Fatty Acid

273. Question:It is the code in which almost all genetic information is encoded.

a. Transfer RNAb. Ribosomal RNAc. Ribonucleic Acidd. Deoxyribonucleic Acid

274. Question:A sample of glass is a supercooled liquid rather than a true solid because it has _____.

a. a definite volumeb. no definite volumec. a crystalline structured. no crystalline structure

275. Question:Two immiscible liquids, when shaken together, may form a _______.

a. solutionb. sedimentc. hydrated solutiond. colloidal dispersion

276. Question:Which of the following is not a pure substance?

a. waterb. milkc. hydrogend. oxygen

277. Question:Which of the following is not an isotope of hydrogen?

a. hydrogenb. deuteriumc. tritiumd. uranium

278. Question:Which of the following is formed by the transfer of electrons from one atom to another?

a. allotropeb. ionc. isotoped. molecule

279. Question:The modern periodic table is based on atomic _______.

a. numberb. radiusc. charged. mass

280. Question:The gram molecular mass for H2SO4 is ______ grams.

a. 7b. 64c. 98d. 196

281. Question:The rate of chemical reaction can be increased by _______.

a. increasing the surface area of the reactants

b. decreasing the reaction temperature

c. decreasing the concentration of the reactants

d. removing the catalyst

282. Question:


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CHEMISTRY I

Which of the following is not a characteristic of a base?

a. has a bitter tasteb. feels smooth and slipperyc. turns litmus from red to blued. typically reacts vigorously with

metals

283. Question:Oxidation involves reactions in which ______.

a. a substance gains one or more electrons

b. a substance loses one or more electrons

c. oxygen has been removed from the reactants

d. oxygen is gained by the reactants

284. Question:A bleach may work if it ______.

a. adds hydrogen ions to the stainb. removes electrons during

oxidationc. adds electrons to reduce

coloration

d. moves electrons between energy levels

285. Question:An organic compound ______.

a. contains carbonb. can be produced syntheticallyc. both a and b are correctd. neither a nor b is correct

286. Question:Which of the following can be used to bombard atoms?

a. protonsb. neutronsc. electronsd. all three

287. Question:

An atom of which of the following elements has the greatest ability to attract electrons?

a. siliconb. brominec. sulfurd. nitrogen

288. Question:Given the same conditions of temperature, which nobel gas will diffuse most rapidly?

a. Krb. Hec. Ned. Ar

289. Question:When most fuels burn, the products include carbon dioxide and ______,

a. hydrogenb. hydrocarbonsc. waterd. hydroxide

290. Question:Which type of reaction is occurring when a metal undergoes corrosion?

a. neutralizationb. polymerizationc. saponificationd. oxidation-reduction

291. Question:Which part of the Periodic Table contains elements with the strongest metallic properties?

a. upper leftb. lower leftc. upper rightd. lower right

292. Question:


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CHEMISTRY I

What is the most abundant element in terms of the number of atoms?

a. Hydrogenb. Heliumc. Oxygend. Nitrogen

293. Question:Which noble gas has the smallest atomic number?

a. Argonb. Kryptonc. Neond. Helium

294. Question:What is the empirical formula of a compound that contains 85% Ag and 15% F by mass?

a. Ag2Fb. AgF2

c. Ag2F2

d. AgF

295. Question:A gas has a pressure of 300 torr, a temperature of 400 K, and a volume of 50.0 milliliters. What volume will the gas have at a pressure of 150 torr and a temperature of 200 K?

a. 25.0 mLb. 50.0 mLc. 75 mLd. 100 mL

296. Question:How many atoms are present in the formula KAl(SO4)2?

a. 6b. 8c. 10

d. 12

297. Question:How many liters of gas would 1.5 moles occupy at STP?

a. 15.0b. 4.5c. 33.6d. 44.6

298. Question:If an element has an atomic number of 11, it will combine most readily with an element that has an atomic number of _____.

a. 16b. 17c. 18d. 19

299. Question:Which of the following statements is true?

a. chlorine changes in colorb. chlorine changes in densityc. chlorine changes into liquidd. chlorine reacts explosively to form

sodium chloride

300. Question:Which of the following is a compound?

a. milkb. goldc. table saltd. ink

301. Question:Gold’s atomic number is 79. How many neutrons are there in 197 Au?

a. 79b. 118c. 197d. 276


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CHEMISTRY I

302. Question:Which of the following is an element?

a. H2Ob. O3

c. CO2

d. C2H4

303. Question:Which of the following is the empirical formula for glucose, a substance known as blood sugar, whose molecular formula is C6H12O6?

a. CH2Ob. CHOc. C2H4Od. CHO6

304. Question:Which of the following is the name of the compound K2SO4?

a. potassium sulfateb. sulphuric oxidec. potassium oxided. silver nitrate

305. Question:Which of the following balances this equation: Na(s) + H2O(l) á NaOH(aq) + H2(g)?

a. Na(s) + 2H2O(l) á NaOH(aq) + H2(g)

b. 2Na(s) + 2H2O(l) á 2NaOH(aq) + H2(g)

c. Na(s) + 2H2O(l) á NaOH(aq) + H2(g)

d. Na(s) + 2H2O(l) á NaOH(aq) + H2(g)

306. Question:What is the formula weight of C12H22O11(sucrose)? The atomic

weights of carbon, hydrogen and oxygen are 12.0 amu, 1.0 amu and 16.0 amu, respectively.


307. Question:What is the mass of 1 mol of glucose, C6H12O6? The atomic weights of carbon, hydrogen and oxygen are 12.0 amu, 1.0 amu and 16.0 amu, respectively.


308. Question:A 1M solution contains 20 grams of solute in 500 milliliters of solution. What is the mass of 1 mole of the solute?

a. 10 gb. 20 gc. 40 gd. 80 g

309. Question:What is the kinetic energy in calories of a 6.0 kg object moving at a speed of 5.0 m/s?

a. 30 calb. 18 calc. 1.2 cald. 0.16 cal

310. Question:What is the formula for a compound formed between aluminum and oxygen? (The atomic number of aluminum is 13 while that of oxygen is 8).


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CHEMISTRY I

a. Al2O3

b. Al3O5

c. AlO2

d. Al3O4

311. Question:What is the volume of exactly 1 mol of gas at 0°C (273.15 K) and exactly 1 atm pressure?

a. 27.31 Lb. 31.32 Lc. 22.41 Ld. 17.42 L

312. Question:Which of the following substances is most likely to exist as a gas at room temperature and normal atmospheric pressures?

a. P4O10

b. Cl2c. AgCld. I2

313. Question:Which of the following will happen if a gas in an enclosed container is heated?

a. pressure increasesb. temperature decreasesc. volume increases

d. volume decreases

314. Question:How can a bigger crystals of table salt be commercially produced?

a. slow solar evaporationb. fast solar heatingc. boiling in a cauldrond. heating over a sand bath

315. Question:The natural fragrance of plants is attributed to the presence of ______.

a. alkanes

b. estersc. alcoholsd. acetone

316. Question:A solution is made containing 6.9 g of NaHCO3 per 100 g of water. What is the weight percentage of solute in this solution?

a. 93.5%b. 89.7%c. 6.5%d. 10.3%

317. Question:In terms of total mass, carbon monoxide (CO) is the most abundant of all pollutant gases. The most serious source of carbon monoxide poisoning comes from ______.

a. cigarette smokingb. smoke from factoriesc. smoke from vehiclesd. smoke from forest fires

318. Question:Which of the following is not a non conventional source of biogas?

a. animal manureb. petroleumc. ipil-ipild. cassava

319. Question:When mercury is placed in a small test tube, a convex surface may be seen. This shows that ______.

a. cohesive force is stronger than adhesive force

b. cohesive force is weaker than adhesive force

c. cohesive and adhesive forces are the same

d. cohesive force is stronger at the bottom

320. Question:


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CHEMISTRY I

Which is a statement of quantitative description?

a. one bottle holds more liquid than the other

b. the color of one liquid is darker than the other

c. the liquid in one bottle is more cloudy than the other

d. the liquid in one bottle is 5 mL more than that in the other

321. Question:The mass number of an element is 16 and its atomic number is 8. How many neutrons does it have?

a. 16b. 8c. 24d. 48

322. Question:What kind of substance turns blue litmus paper into red and is classified as a proton donor?

a. a saltb. an acidc. a based. a metal

323. Question:LPG or liquefied petroleum gas is a mixture of C3H8 and C4H10. This mixture is ______ and ______.

a. propane, butaneb. ethane, methanec. propane, methaned. propane, butane

324. Question:Which unit is used to express the amount of energy absorbed or released during a chemical reaction?

a. calorieb. torrc. degreed. kilogram

325. Question:A compound with an empirical formula of CH2 has a molecular mass of 70. What is the molecular formula?

a. C2H4

b. C4H8

c. CH2

d. C5H10

326. Question:Which are the products of a fermentation reaction?

a. a soap and a glycerolb. an alcohol and carbon dioxidec. an ester and waterd. a salt and water

327. Question:The number of calories per gram required to melt ice at its melting point is called ______.

a. sublimationb. heat of fusionc. vapor pressured. heat of vaporization

328. Question:A liquid has one phase, is colorless and odorless and boils at a temperature range of 110-120°C. This liquid is called _____.

a. solutionb. colloidc. substanced. heterogenous mixture

329. Question:


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CHEMISTRY I

A white solid that melts sharply was observed to yield a colorless liquid and a black solid when burned. Which term best describes the solid?

a. elementb. mixturec. substanced. compound

330. Question:The forces of attraction that exist between nonpolar molecules are called ____.

a. ionicb. van der Waalsc. electrovalentd. atomic

331. Question:Toward which corner of the Periodic Table is located the elements that have the most pronounced nonmetallic properties?

a. upper rightb. lower rightc. upper leftd. lower left

332. Question:Which process occurs when dry ice is changed into carbon dioxide?

a. crystallizationb. sublimationc. condensationd. solidification

333. Question:What is the number of an atom which contains 25 electrons, 25 protons, and 29 neutrons?

a. 50 amub. 342.0 amuc. 25 amud. 54 amu

334. Question:

Which electron dot formula represents a nonpolar molecules?

H a. H:C:Cl:

HH

b. H:N: H

H c. H:C:H

HH

d. H:Cl:C H

335. Question:How many moles of water are contained on 0.250 mole of CuSO4 • 5H2O?

a. 62.5b. 0.5c. 1.25d. 75

336. Question:What is the mass of 3.0 x 1023 atoms of neon?

a. 10 gb. 7 gc. 30 gd. 5 g

337. Question:When a battery is in use, stored chemical energy is first changed to ______ energy.

a. lightb. electricalc. mechanicald. nuclear


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CHEMISTRY I

338. Question:In the reaction Zn(s) + Cu2+(aq) + Cu(s), the reducing agent is ______.

a. Zn(s)b. Cu(s)c. Cu2+(aq)d. Cu2+

339. Question:Which compound contains both covalent bonds and ionic bonds?

a. HCl(g)b. N2O5(g)c. NaCl(s)d. NaNO3(s)

340. Question:When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is _____.

a. constantb. halvedc. tripledd. quartered

341. Question:The number of electrons in a neutral atom of every element is always equal to the atom’s _______.

a. number of nucleonsb. number of neutronsc. number of positronsd. number of protons

342. Question:Which is a product of the hydrolysis of an animal by a strong base?

a. gasolineb. waterc. kerosened. soap

343. Question:The atom of carbon-14 contains _______.

a. 6 protons, 8 neutrons, and 8 electrons

b. 6 protons, 8 neutrons, and 6 electrons

c. 6 protons, 6 neutrons, and 8 electrons

d. 8 protons, 6 neutrons, and 6 electrons

344. Question:Which formula represents a binary compound?

a. O2

b. Nec. 2C2H5OHd. C3H8

345. Question:Which temperature represents absolute zero?

a. 0°Cb. 273°Kc. 0 Kd. 273°C

346. Question:When a salt dissolves in water, the water molecules are attracted by dissolved salt particles. This attraction is called _______.

a. atom-atomb. molecule-ionc. molecule-moleculed. atom-molecule

347. Question:An example of a heterogeneous mixture is ______.

a. stainless steelb. soilc. sugard. carbon monoxide


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CHEMISTRY I

348. Question:Water will boil at temperature of 40°C when the pressure on its surface is ______.

a. 25.5 torrb. 40 torrc. 55.3 torrd. 760 torr

349. Question:How are elements classified?

a. metals, non-metals and metalloidsb. homogeneous or heterogeneousc. suspension, colloid, solutiond. gases, solids or liquids

350. Question:Compounds are mostly classified as

a. homogeneous and heterogeneousb. acids and basesc. gases, liquids and solidsd. metals and nonmetals

351. Question:What is the property of metals that allow them to be rolled without breaking?

a. ductilityb. malleabilityc. lusterd. elasticity

352. Question:What is the property of metals that reflect the light that strikes their surfaces, making them appear shiny?

a. malleabilityb. ductilityc. lusterd. plasticity

353. Question:

An acid can react with a base to produce a _____.

a. hydrogen gasb. saltc. oxided. hydroxide

354. Question:Compounds that contain halogens are called _____.

a. aminesb. halidesc. ethersd. aldehydes

355. Question:The organic compounds that contains oxygen but not in the carbonyl group are called ___.

a. alcohols and ethersb. amines and amidesc. halidesd. aldehydes

356. Question:Which of the following is NOT a property of metals?

a. metals are neither malleable nor ductile

b. metals have high thermal conductivity

c. metals have high electrical conductivity

d. metals have more luster

357. Question:What are elements that have properties intermediate between metals and nonmetals?


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a. gasesb. solidsc. liquidsd. metalloids

358. Question:Which of the following is NOT a property of acids?

a. taste sourb. feel slippery on the skinc. turn litmus paper to redd. dissolve metals producing various

salts and hydrogen gas

359. Question:Which of the following is NOT a property of bases?

a. feel slippery on the skinb. turn litmus paper to bluec. taste bitterd. dissolve metals producing various

salts and hydrogen gas

360. Question:What organic compounds contain the hydroxyl as the functional group and are considered derivatives of water?

a. alcoholsb. ethersc. aldehydesd. ketones

361. Question:What organic compounds contain nitrogen?

a. halidesb. amines and amidesc. alcoholsd. ethers

362. Question:What organic compounds in which two hydrocarbon groups that can be

aliphatic or aromatic are attached to one oxygen atom?

a. aminesb. alcoholsc. ethersd. halides

363. Question:Vinegar is a solution of water and what acid?

a. Phosphoric acidb. Sulfuric acidc. Nitric acidd. Acetic acid

364. Question:What acid is added to carbonated drinks to produce a tart test?

a. Citric acidb. Phosphoric acidc. Sulfuric acidd. Nitric acid

365. Question:Table salt or sodium chloride may be formed by the reaction of:

a. Hydrochloric acid and sodium bicarbonate

b. Sodium and chlorinec. Hydrochloric acid and Sodium

carbonated. Hydrochloric acid and sodium

Hydroxide

366. Question: “The masses of elements in a pure compound are always in the same proportion”. This statement is known as _______.

a. Law of multiple proportionb. Law of definite proportionc. The periodic tabled. Dalton’s atomic theory

367. Question:


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How does Joseph John Thomson call his model of the atom?

a. Orbital modelb. Planetary modelc. Radioactive modeld. Plum-pudding model

368. Question:The discovery of radioactivity further confirms the existence of subatomic particles. Who discovered radioactivity?

a. Henri Becquerelb. Marie Curiec. Pierre Curied. Niels Bohr

369. Question:Atoms of the same element which have different masses are called _______.

a. moleculesb. ionsc. nuclidesd. isotopes

370. Question:What is an atom of specific isotope called?

a. Nuclideb. Ionc. Moleculed. Fermion

371. Question:The number of _____ in an atom defines what element the atom is

a. neutronsb. electronsc. protonsd. protons and electrons

372. Question:The number of _____ in an atom defines the isotopes of an element.

a. neutronsb. protonsc. electronsd. protons and neutrons

373. Question:What is the “identity number” of an atom?

a. Atomic numberb. Mass numberc. Atomic massd. Atomic weight

374. Question:“When the elements are arranged in the order of increasing atomic number, elements with similar properties appear at periodic intervals.” This statement is known as ______.

a. Law of multiple proportionb. Law of definite proportionc. The periodic lawd. Dalton’s atomic theory

375. Question:Who are the two chemists credited for the discovery of the periodic law?

a. Julius Lothar Meyer and Demitri Ivanovich Mendeleev

b. Humphrey Davy and Henri Becquerel

c. Henri Becquerel and Ernest Rutherford

d. Ernest Rutherford and Julius Lothar Meyer

376. Question:The elements with similar properties are placed in columns of the periodic table . This columns are commonly called ______.

a. Periodsb. Transitionsc. Groupsd. Groups or families


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377. Question:What are the rows in the periodic table called?

a. periodsb. transitionsc. groupsd. families

378. Question:Elements in Group 1A in the periodic table are ______.

a. Boron groupb. Alkali earth metalsc. Alkali metalsd. Carbon group

379. Question:Elements in Group IIA in the periodic table are _______.

a. Halogensb. Alkaline earth metalsc. Alkali metalsd. Nitrogen group

380. Question:The boron group is what group in the periodic table?

a. Group IIIAb. Group IVAc. Group VAd. Group VIA

381. Question:What group in the periodic table is the carbon group?

a. Group IIIAb. Group IVAc. Group VAd. Group VIA

382. Question:What is the second most abundant element in the human body?

a. Carbonb. Hydrogen

c. Oxygen

d. Nitrogen

383. Question:Which of the following is not a metalloid?

a. Antimonyb. Boronc. Magnesiumd. Silicon

384. Question:Caustic soda is used making soap, textiles and paper. What is another term for caustic soda?

a. Sodium benzoateb. Sodium hydroxidec. Potassium chlorated. Cesium bromide

385. Question:What is used for the manufacture of explosives and fireworks?

a. Magnesium hydroxideb. Potassium chloratec. Potassium perchlorated. Cesium bromide

386. Question:All alkaline metals will tarnish in air except ______.

a. Magnesiumb. Bariumc. Radiumd. Beryllium

387. Question:What alkali metal is usually used for x-ray apparatus because of its ability to allow x-rays to pass through with minimum absorption?

a. Magnesiumb. Radiumc. Berylliumd. Barium


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388. Question:What element is used as a coating for iron to make galvanized iron a corrosion-resistant material?

a. Magnesiumb. Titaniumc. Zincd. Chromium

389. Question:What element is used as electric power source for pacemakers and artificial hearts?

a. Promethiumb. Neodymiumc. Uraniumd. Plutonium

390. Question:What element is commonly used in making lasers?

a. Chromiumb. Neodymiumc. Promethiumd. Terbium

391. Question:What is regarded as the most unique element in the periodic table?

a. Hydrogenb. Oxygenc. Carbond. Uranium

392. Question:What is the most abundant element in the atmosphere?

a. Oxygenb. Nitrogenc. Heliumd. Inert gases

393. Question:

What is the only gas in Group VIA in the periodic table?

a. Hydrogen

b. Heliumc. Oxygend. Nitrogen

394. Question:What is the second most abundant element in the atmosphere?


395. Question:What element is used in advertising signs?

a. Neonb. Heliumc. Sodiumd. Xenon

396. Question:What principle stress about fundamental limitation that, for a particular as small as the electron, one cannot know exactly where it is and at the same time know its energy or how it is moving?

a. Aufbau principleb. Uncertainty principlec. Pauli exclusion principled. Kinetic molecular theory

397. Question:Who discovered the uncertainty principle?

a. Werner Karl Heisenbergb. Louie de Brogliec. Albert Einsteind. John Newlands


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398. Question:What principle states that the electrons fill the orbitals, one at a time, starting with the lowest energy orbital then proceeding to the one with higher energy?

a. Aufbau principleb. Uncertainty principlec. Pauli exclusion principled. Kinetic molecular theory

399. Question:What principle states that no two electrons in the same atom can have the same set of quantum numbers?

a. Aufbau principleb. Uncertainty principlec. Pauli exclusion Principled. Kinetic molecular theory

400. Question:What describes how the electrons and distributed among the orbitals?

a. Electronegativity of the elementb. Electron configuration of an atomc. Energy state of the atomd. Pauli exclusion principle

401. Question:The _____ of the atom describes the atom as having a nucleus at the center around which electrons move?

a. spin numberb. quantum mechanical modelc. quantum numberd. azimuthal number

402. Question:

What are the main energy level where the valence electrons belong called?

a. valence shellsb. azimuthal shellsc. spin shellsd. quantum shells

403. Question:The size of the atom is dependent on _______.

a. The size of the nucleusb. the region of space occupied by

its electronsc. the number of protons and

neutronsd. all of the choices above

404. Question:What happens to the atomic size of the elements in a group when you go from top to bottom of the group?

a. it remains the sameb. it increasesc. it decreasesd. it becomes zero

405. Question:The ionization energy is ______ to the atomic size of atom.

a. directly proportional b. inversely proportionalc. equal tod. not related

406. Question:What alkaline earth metal has the smallest atomic number?

a. Berylliumb. Magnesiumc. Calciumd. Barium

407. Question:The process of gaining or losing an electron results in the formation of a


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charged atom or molecule called ______.

a. ionb. cationc. aniond. crystal

408. Question:Aside from liquid, gas and solid, there are two other states of matter. What are they?

a. Plasma and Quarkb. Quartz and Plasmac. Quartz and Quasard. Plasma and Bose-Einstein

condensate

409. Question:Who first identified the plasma in 1879?

a. William Crookesb. Irving Langmuirc. Albert Einsteind. Eric Cornell

410. Question:Who coined the term “plasma” in 1928?

a. William Crookesb. Irving Langmuirc. Albert Einsteind. Eric Cornell

411. Question:What is made of gas atoms that have been cooled to near absolute zero at which temperature the atoms slow down, combine and forma a single entity known called a superatom?

a. Ionized gasb. Bose-Einstein condensate (BEC)c. Plasmad. Quark

412. Question:The fifth state of matter, the BEC (Bose-Einstein condensate) was first created in what year?

a. 1992b. 1993c. 1994d. 1995

413. Question:The elements of groups IA, IIA, IIIA, IVA, VA, VIA, VIIA and VIIIA are called main group elements or ______.

a. transitionsb. representativesc. inner transitionsd. metals or nonmetals

414. Question:For the representative elements, the number of valence electrons is the same as the ______.

a. number of electronsb. number of neutronsc. the rightmost digit of the group

number of elementd. number of electrons less the

number of neutrons

415. Question:For transition elements, the number of valence electrons is the same as ______.

a. the group numberb. the rightmost digit of the group

number of the elementc. the number of electrons less the

number of neutronsd. the number of electrons less the

number of protons

416. Question:What is a high-energy, electrically charged gas produced by heating the gas until the electrons in the


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outer orbitals of the atoms separate, leaving the atoms with a positive charge?

a. Quartzb. Quarkc. BECd. Plasma

417. Question:Water has the biggest density when it is in what state?

a. Liquidb. Gasc. Solidd. Vapor

418. Question:What is the temperature of water in solid state at 1 atm?

a. 4°Cb. 25°Cc. 0°Cd. 5°C

419. Question:The density of water is the largest in what temperature?

a. 2°Cb. 1°Cc. 3°Cd. 4°C

420. Question:What element has a very high melting point and ideal for filaments of light bulbs?

a. Bariumb. Aluminumc. Tungstend. Titanium

421. Question:

Metals can be drawn into wires. This illustrates what property of metals?

a. Malleabilityb. Ductilityc. Rigidityd. Plasticity

422. Question:Steel is the widely used construction material because of its high tensile strength. It is combination of what elements?

a. Iron and carbonb. Iron and aluminumc. Lead and carbond. Lead and aluminum

423. Question:What refers to the electrostatic attraction that holds together the oppositely charged ions, the cations and anions, in the solid compound?

a. Electronic bondb. Metallic bondc. Covalent bondd. Ionic bond

424. Question:What states that atoms tend to gain, lose or share electrons until they are surrounded by eight valence electrons?

a. Figure of 8 ruleb. Octet rulec. Ionic ruled. Lewis rule

425. Question:What indicates the number of valence electrons in the atom represented by dots scattered on four sides of the atomic symbol?

a. Electron dot structureb. Lewis structurec. Crystalline structure


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d. Electrons dot structure or Lewis structure

426. Question:What is the distance between the nuclei of two bonded atoms called?

a. bond lengthb. molecular lengthc. atomic distanced. atomic radius

427. Question:The overall shape of a molecule is described by which two properties?

a. bond distance and bond sizeb. bond distance and bond anglec. bond radius and bond angled. bond angle and bond size

428. Question:What is an angle made by the lines joining the nuclei of the atoms in the molecule?

a. atomic angleb. bond anglec. molecular angled. ionic angle

429. Question:“The best arrangement of a given number of shared and unshared electrons is the one that minimizes the repulsion among them.” This is known as ______.

a. valence bond theoryb. electron group theoryc. molecular polarity theoryd. valence-shell electron-pair

repulsion theory

430. Question:“A covalent bond is formed by the overlap of atomic orbitals”. This

statement is the basic idea of which theory?

a. Valence bond theoryb. Energy group theoryc. Molecular polarity theoryd. Valence-shell electron-pair

repulsion (VSEPR) theory

431. Question:The Chalcogens are elements in what group in the periodic table?

a. Group VAb. Group VIAc. Group VIIA

d. Group IVA

432. Question:Halogens belong to what group in the periodic table?

a. Group IVAb. Group VAc. Group VIAd. Group VIIA

433. Question:The elements, germanium and silicon, which are commonly used for semiconductors belongs to what group of elements?

a. Boron groupb. Carbon groupc. Nitrogen groupd. Halogens

434. Question:What group in the periodic table are the noble gases?

a. Group 0b. Group VIIIAc. Group VIIAd. Group 0 or VIIIA

435. Question:Which of the following is not a noble gas?


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CHEMISTRY I

a. Argonb. Xenonc. Radond. Antimony

436. Question:What refers to the ability of an atom in a molecule to attract shared electrons?

a. electronegativityb. electron affinityc. ionization energyd. periodic number

437. Question:What type of bond occurs when the difference in electronegativity is greater than or equal to 2?

a. ionicb. non-polar covalentc. polar covalentd. either non-polar covalent or polar

covalent

438. Question:Non polar covalent bond occurs if the difference in electronegativity ranges from

a. 0.00 to 0.40b. 0.50 to 1.90c. 1.90 to 2.00d. 2.00 and up

439. Question:When can we say that a molecule is polar?

a. when the centers of positive and negative charge do not coincide

b. when the centers of positive and negative charge coincide

c. when there is no positive nor negative charge

d. when there is only one charge, either negative or positive

440. Question:What is the sum of the masses of the atoms in the molecule of the substance called?

a. atomic massb. molecular massc. formula massd. atomic weight

441. Question:What refers to the number of atoms in exactly 12 grams of carbon-12?

a. Avogadro’s numberb. molec. molar mass

d. amu

442. Question:Which one is the Avogadro’s number?

a. 6.20 x 1023

b. 6.02 x 1023

c. 6.32 x 1023

d. 6.22 x 1023

443. Question:What is defined as the amount of substance that contains 6.02 x 1023 particles of that substance?

a. moleb. molar massc. avogadro’s numberd. amu

444. Question:What refers to the mass in grams of one mole of a substance?

a. molar massb. molecular massc. atomic massd. atomic weight

445. Question:What is the unit of molar mass?

a. amu


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b. molec. gramsd. grams per mole

446. Question:“The total pressure of a mixture of gases equals the sum of the partial pressures of each of the gases in the mixture.” This statement is known as ______.

a. Dalton’s law of partial pressureb. Gay-Lussac lawc. Boyle’s lawd. Charles’ law

447. Question:The dry air is composed of how many percent nitrogen?

a. 73.1%b. 74.4%c. 76.1%d. 78.1%

448. Question:The dry air is composed of how many percent oxygen?

a. 20.9%b. 21.2%c. 22.1%d. 23.7%

449. Question:How much carbon dioxide is present in dry air?

a. 0.003%b. 0.03%c. 0.3%d. 3%

450. Question:What is the mixing of gases due to molecular motion called?

a. diffusionb. effusion

c. fissiond. fusion

451. Question:What refers to the passage of molecules of a gas from one container to another through a tiny opening between the containers?

a. diffusionb. Effusionc. fusiond. fission

452. Question:The rate of effusion of a gas is inversely proportional to the square

root of its molar mass. Who discovered this?

a. Gilbert Lewisb. John Tyndallc. Robert Brownd. Thomas Graham

453. Question:What law states that the rate of effusion of a gas, which is the amount of gas that moves through the hole in a given amount of time, is inversely proportional to the square root its molar mass?

a. Henry’s lawb. Graham’s law of effusionc. Hund’s lawd. Lewis theory

454. Question:What is a poisonous gas generated mostly by motor vehicles?

a. carbon monoxideb. carbon dioxidec. hydroxided. nitric acid

455. Question:


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CHEMISTRY I

Who revised the atomic theory by replacing the hard, indestructible spheres imagined by John Dalton and proposed the “rain bread model” of the atom?

a. Pierre Curieb. Robert Andrews Milikanc. Joseph John Thomsond. Ernest Rutherford

456. Question:What is considered as one of the pollutants responsible for smog and acid rain?

a. sulfur dioxideb. nitrogen dioxidec. carbon dioxided. hydroxide

457. Question:What refers to the forces of attraction that exist between molecules in a compound?

a. interaction forcesb. dispersion forcesc. intermolecular forcesd. induction forces

458. Question:All are basic types of Van der waals forces except

a. Dipole-dipole interactionb. London dispersion forcesc. Heat bondingd. Hydrogen bonding

459. Question:The three types of intermolecular forces exist in neutral molecules are collectively known as van der waals forces. This is named after ____

a. Diderik van der Waalsb. Derick van der Waalsc. Doe van der Waalsd. Eric van der Waals

460. Question:a dipole has how many electrically charged poles?

a. 1b. 2c. 3d. 4

461. Question:Compounds containing hydrogen and other element are known as _______.

a. hydroxidesb. hydridesc. hydrosd. hydrates

462. Question:What is a special kind of dipole-dipole interaction formed when a hydrogen atom bounded to a highly electronegative atom is attracted to the lone pair of a nearby electronegative atom?

a. Hydride bondb. Hydro bondc. Hydrogen bondd. Hydrate bond

463. Question:What is the process of changing gas state to liquid state?

a. Sublimationb. Condensationc. Depositiond. Vaporization

464. Question:What is the process of changing liquid state to solid state?

a. Meltingb. Freezingc. Sublimation


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d. Condensation

465. Question:What is the process of changing liquid state to gas state?

a. Vaporizationb. Sublimationc. Condensationd. Deposition

466. Question:What is the process of changing solid state to gas state?

a. Vaporizationb. Depositionc. Sublimationd. Condensation

467. Question:What is the process of changing gas state to solid state?

a. Depositionb. Vaporizationc. Condensationd. Sublimation

468. Question:What is the process of changing from solid state to liquid state?

a. Freezingb. Meltingc. Condensationd. Vaporization

469. Question:What refers to the amount of heat absorbed by one mole of a substance to change from solid to liquid?

a. molar heat of vaporizationb. molar heat of solidificationc. molar heat of fissiond. molar heat of fusion

470. Question:What refers to the amount of heat required by one mole of a substance to change liquid to gas?

a. molar heat of vaporizationb. molar heat of solidificationc. molar heat of condensationd. molar heat of fusion

471. Question:Liquid that vaporizes easily are called ____ liquids.

a. volatileb. non-volatilec. surfactantd. hydrophilic

472. Question:What is the component of the solution in which the solute is dissolved?

a. solventb. catalystc. reactantd. medium

473. Question:Bronze is a solid solution of copper and tin. Which of the following is true?

a. Tin is the solventb. Copper is the solutec. Copper is the solventd. The solution is called aqueous

solution

474. Question:When the solvent of the solution is water, it is a/an ______ solution.

a. wetb. liquid


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c. aqueous d. fluid

475. Question:What is the most common solvent in medicines?

a. Paracetamolb. Acidc. Ethanold. Starch

476. Question:What is the term generally used to described the combination of solute molecules or ions with solvent molecules?

a. Solubilityb. Solvationc. Saturationd. Transformation

477. Question:What is the term used to describe the maximum amount of solute that a given solvent can dissolve to give a stable solution at a given temperature?

a. Solubilityb. Solvationc. Saturationd. Transformation

478. Question:What refers to the temperature above which a gas cannot be liquefied by an increase in pressure?

a. Absolute temperatureb. Absolute zeroc. Critical temperatured. Maximum temperature

479. Question:What is a homogeneous mixture made of particles that exist as individual molecules or ions?

a. solutionb. solutec. solventd. colloid

480. Question:What is the component of the solution that is dissolved?

a. solventb. solutec. catalystd. colloid

481. Question:When the maximum amount of solute is dissolved in the given solvent at a stated temperature, the solution formed is ________.

a. unsaturatedb. saturatedc. supersaturatedd. undersaturated

482. Question:When the solution contains less solute particles than the maximum amount the solvent can dissolve at that temperature, the solution is _______.


483. Question:When the solution contains more solute particles than the solvent can normally hold, the solution is _____.


484. Question:What is the most common solution on earth?


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CHEMISTRY I

a. airb. seawaterc. bloodd. freshwater

485. Question:Solutions composed of two or more metals are called _______.

a. saturated solutionsb. supersaturated solutionsc. unsaturated solutionsd. alloys

486. Question:The solubility of a substance in another substance is affected by the following factors except _____.

a. nature of solute and solventb. pressurec. volumed. temperature

487. Question:Liquids that do not mix are said to be _______.

a. miscibleb. immisciblec. solubled. nonsoluble

488. Question:Water and alcohol are both liquids that can be mixed in any proportion. They are said to be ____.

a. miscibleb. immisciblec. solubled. nonsoluble

489. Question:How will an increase in temperature in solids affect solubility?

a. it will cause a decrease in solubility

b. it will not affect solubility at allc. it will slightly affect solubilityd. it will cause an increase in

solubility

490. Question:How will an increase in temperature of gases dissolving in liquids affect solubility?

a. it will cause a decrease in solubility

b. it will not affect solubility at allc. it will slightly affect solubilityd. it will cause an increase in

solubility

491. Question:How does pressure affects the solubility of gases in liquids?

a. it decreases solubilityb. it does not affect solubility at allc. it slightly affects solubilityd. it increases solubility

492. Question:How does pressure affects the solubility in liquids or of liquids in another liquid?

a. it decreases solubilityb. it does not affect solubility at allc. it slightly affects solubilityd. it increases solubility

493. Question:“The solubility of gas in a liquid is directly proportional to the partial pressure of the gas above the solution”. This is known as ______.

a. Hund’s lawb. Pascal’s lawc. Henry’s lawd. Dalton’s law

494. Question:What is the common unit is used to indicate the mass of a particle?


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CHEMISTRY I

a. Atomic mass unit (amu)b. Charge unitc. Coulombd. Gram

495. Question:What is the unit for the charge of a particle?

a. Coulombb. charge unitc. atomic mass unitd. Lepton

496. Question:The protons and neutrons are not considered as fundamental particles because they consist of smaller particles called?

a. bosonsb. quarksc. leptonsd. fermions

497. Question:What refers to the measure of how fast a substance dissolves?

a. rate of solubilityb. rate of agitationc. rate of dissolutiond. rate of solution

498. Question:How can a rate of dissolution be increased?

a. reduce particle sizeb. agitationc. application of heatd. all of the above

499. Question:______ means there is only a little amount of solute dissolved in a solution.

a. concentratedb. dilutec. saturatedd. unsaturated

500. Question:______ means there is a large amount of solute dissolved in the solution.

a. concentratedb. dilutec. saturatedd. unsaturated

501. Question:What is the ratio of the number of moles of solute to the volume of the solution in liters?

a. molarityb. molalityc. formalityd. mole fraction

502. Question:What is the ratio of the number of moles of solute per kilogram of solvent?

a. molalityb. molalityc. formalityd. mole fraction

503. Question:What is the process of making a solution less concentrated as in the addition of more solvent?

a. concentrationb. dilutionc. saturationd. colligation

504. Question:


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What is the process of changing the liquid to gas that is usually accompanied by the production of bubbles of vapor in the liquid?

a. vaporizingb. boilingc. condensingd. sublimation

505. Question:What is the temperature at which the vapor pressure of the liquid equals the prevailing atmospheric pressure?

a. boiling pointb. triple pointc. saturation pointd. critical point

506. Question:What is the temperature at which liquid and solids are in equilibrium?

a. Boiling pointb. Resting pointc. Freezing pointd. Critical point

507. Question:What refers to the decrease in the freezing point of a pure liquid when another substance is dissolved in the liquid?

a. Freezing point compressionb. Freezing point extensionc. Freezing point depressiond. Freezing point dilution

508. Question:If two solutions have the same concentration of solute, they are ______.

a. hypertonicb. hypotonicc. isotonic

d. photonic

509. Question:If one or two solutions has a higher concentration of solute particles than the other, the one with the higher concentration is described as _______.

a. hypertonicb. hypotonicc. isotonicd. photonic

510. Question:What is in some aerosol products that can cause harm to the atmosphere?

a. smogb. Chloroflurocarbons (CFC)c. emulsifying agentd. hydrocarbons

511. Question:What are colloidal dispersions of gas bubbles in liquids or solids?

a. emulsionsb. aerosolsc. foamsd. sols

512. Question:What is a colloidal dispersion of a liquid in either a liquid or a solid?

a. emulsionsb. gelsc. foamsd. sols

513. Question:What is a solid dispersed in either a solid or liquid?



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CHEMISTRY I

514. Question:What is defined as a substance which, upon dissolution in or reacting with water causes an increase in the concentration of the solvent anion, OH?

a. Lewis acidb. Lewis basec. Arrhenius based. Arrhenius acid

515. Question:What is the dissolution constant of water at 25°C?

a. 1.8 x 10-15

b. 1.8 x 10-16

c. 1.8 x 10-17

d. 1.8 x 10-18

516. Question:What theory states that an acid is any substance that donates a proton to another substance, and a base is any substance that can accept a proton from any other substance?

a. Arrhenius theoryb. Bronsted-Lowry theoryc. Lewis theoryd. pH concept

517. Question:What is a colloidal system in which the dispersed phase consists of fibrous, interwoven particles called fibrils which exert a marked effect on the physical properties of the dispersing medium?


518. Question:Most cosmetics and ointments and creams used in medicines are _____.


519. Question:The substance usually used in cleaning toilets bowls and tiles is muriatic acid. What is another term for muriatic acid?

a. Nitric acidb. Sulfuric acidc. Hydrochloric acidd. Phosphoric acid

520. Question:“Upon dissociation in water, acids yield hydrogen ions while gases yield hydroxide ions”. What is this statement commonly called?

a. Arrhenius theoryb. pH conceptc. Bronsted-Lowry theoryd. Le Chatelier’s principle

521. Question:What is defined as the substance which, upon reaction with water, causes an increase in the concentration of the solvent cation, H3O+?

a. Lewis acidb. Lewis basec. Arrhenius based. Arrhenius acid

522. Question:What theory states that an acid is a substance that can accept a lone pair from another molecule, and a base is a substance that has a lone pair of electrons?

a. Arrhenius theoryb. Bronsted-Lowry theoryc. Lewis theoryd. pH concept


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CHEMISTRY I

523. Question:An acid described as an electron pair acceptor is the ______ acid.

a. Arrheniusb. Purec. Lewisd. Bronsted-Lowry

524. Question:The Bronsted-Lowry acid is:

a. a proton donorb. a proton acceptorc. an electron pair acceptord. an electron pair donor

525. Question:Acids consist of three elements, hydrogen and two nonmetals are called _______.

a. triacidsb. ternary acidsc. oxyacidsd. organic acids

526. Question:If one of two nonmetals of a ternary acid is oxygen, the acid is called _______.

a. oxideb. oxyacidc. oxide acidd. acidic oxide

527. Question:Which of thee following is the formula of sulfuric acid?

a. H2SO4

b. H2SO3

c. H4SO2

d. HNO2

528. Question:Which of the following is the formula of nitric acid?

a. HNO4

b. H2SO3

c. H4SO2

d. HNO3

529. Question:What acid is usually used in vinegars?

a. Sulfuric acidb. Acetic acidc. Nitric acidd. Carbonic acid

530. Question:What acid is used in glass itching?

a. Acetylsalicylic acidb. Hydroflouric acidc. Phosphoric acidd. Hydrochloric acid

531. Question:What acid is usually present in some fruits?

a. citric acidb. Carbonic acidc. Organic acid

d. Nitric acid

532. Question:What acid is used in carbonated drinks?

a. Carbonic acidb. Hydroflouric acidc. Nitric acidd. Citric acid

533. Question:


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CHEMISTRY I

What acid usually used to reduce pain and inflammation such as aspirin and other pain relievers?

a. Carbonic acidb. Acetylsalicylic acidc. Nitric acidd. Phosphoric acid

534. Question:The Bronsted-Lowry base is

a. a proton donorb. a proton acceptorc. an electron pair acceptord. an electron pair donor

535. Question:According to Gilbert Lewis, an acid-base reaction as the sharing of an electron pair will form what type of bond?

a. coordinate ionic bondb. coordinate covalent bondc. coordinate metallic bondd. coordinate bond

536. Question:What is the type of covalent bond in which the shared electrons are donated by one, not both, of the atoms involved?

a. synchronous covalent bondb. coordinate covalent bondc. asynchronous covalent bondd. translating covalent bond

537. Question:What is the term used for the product of a Lewis acid-base reaction?

a. oxyacidsb. binary acidsc. acibasd. adduct

538. Question:

Acids composed of only two elements, hydrogen and non metal, are called ______.

a. binary acidsb. ternary acidsc. oxyacidsd. organic acids

539. Question:What is added to hydrochloride to form hydrochloric acid?

a. oxygenb. sulfurc. waterd. carbon

540. Question:What acid is usually used in the manufacturer of fertilizers?

a. Carbonic acidb. Acetylsalicylic acidc. Sulfuric acidd. Phosphoric acid

541. Question:What acid is used in the manufacture of explosives?

a. Carbonic acidb. Acetylsalicylic acidc. Nitric acidd. Phosphoric acid

542. Question:What acid is used in the batteries of cars or automobiles?

a. Carbonic acid

b. Acetylsalicylic acidc. Sulfuric acidd. Phosphoric acid

543. Question:Bases are compounds consisting of

a. metal and oxide ionb. nonmetal and oxide ionc. metal and hydroxide ion


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CHEMISTRY I

d. nonmetal and hydroxide ion

544. Question:Which base is used to remove carbon dioxide from air?

a. Lithium hydroxideb. Sodium hydroxidec. Aluminum hydroxided. Magnesium hydroxide

545. Question:Which two substances have the same pH, which is 6.5?

a. Saliva and milkb. Orange juice and tomato juicec. Vinegar and calamansi juiced. Urine and apple juice

546. Question:Which is the most acidic?

a. vinegarb. calamansi juicec. carbonated drinkd. orange juice

547. Question:Which is the best description of strong acids?

a. They dissociate or ionize completely in water

b. They don’t dissociate or ionize completely in water

c. They are normally found in vinegars

d. They are the acids that do not contain hydrogen

548. Question:Which is the best description of weak acids?

a. They dissociate or ionize completely in water

b. They do not dissociate or ionize completely in water

c. They are normally found in hydrogen chloride form

d. They are the acids that not found in vinegars

549. Question:What is a measure of the H3O+ concentration of solution?

a. pHb. pOHc. Indicatord. OH-

550. Question:What is the measure of the OH- concentration of a solution?

a. pHb. pOHc. Indicatord. OH-

551. Question:What is the pH of neutral solution?

a. 5b. 6c. 7d. 8

552. Question:What is the pH of pure water?

a. 6.1b. 6.5c. 7d. 7.4

553. Question:What refers to the reaction between an acid and a base forming salt and water?

a. Neutralizationb. Titrationc. Hydrolysisd. Buffer

554. Question:


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CHEMISTRY I

What is the process of measuring the concentration of an acid or base in one solution by adding a base or acid solution of known concentration until the acid or base in the solution of unknown concentration is fully neutralized?

a. Neutralizationb. Titrationc. Hydrolysisd. Buffer

555. Question:What group in the periodic table is the nitrogen group?

a. Group VAb. Group VIAc. Group VIIAd. Group IVA

556. Question:What is the atomic number of oxygen?

a. 6b. 7c. 8d. 9

557. Question:What is the atomic number of germanium?

a. 14b. 32c. 18d. 23

558. Question:What is the most abundant element in the human body?


559. Question:What refers to the point at which the added base or acid solution in titration is enough to fully neutralize the acid or base?

a. Neutral pointb. Titrant pointc. Central pointd. Equivalence point

560. Question:Which of the following is the most basic?

a. pH 8b. pH 9c. pH 11d. pH 13

561. Question:What is a substance that changes at a certain pH range?

a. Litmus paperb. Indicatorc. Balancerd. Lichen

562. Question:What base is used as an antacid with no dosage restriction?

a. Magnesium hydroxideb. Sodium hydroxidec. Aluminum hydroxided. Lithium hydroxide

563. Question:What refers to the reaction between the ions of a salt and the ions of water?

a. salt titrationb. salt bufferingc. salt neutralization


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CHEMISTRY I

d. salt hydrolysis

564. Question:Magnesium hydroxide is a base used as antacid if consumed in small amounts and laxative if consumed in large dosage. What is common term for magnesium hydroxide?

a. Skim of Magnesiab. Oil of Magnesiac. Cream of Magnesiad. Milk of Magnesia

565. Question:What is the most convenient way of expressing hydronium ion concentration?

a. Hydrometer readingb. pH scalec. Alkalinityd. Basicity

566. Question:Who proposed the pH scale in 1909?

a. Albert Einsteinb. J. Willard Gibbsc. Henri Hessd. Soren Sorensen

567. Question:What does the symbol “pH” stands for?

a. the power of the hydroxide compound

b. the power of hydroxide ionc. the power of hydrogen ionsd. The power of hydrogen

568. Question:

What is a solution consisting of a weak acid and its conjugate base, or of a weak base and its conjugate acid?

a. seawaterb. saltc. bufferd. aqueous solution

569. Question:What is the most common chemical reaction, which is the reaction of materials with oxygen accompanied by the giving off of energy in the form of heat?

a. combustionb. exothermic reactionc. endothermic reactiond. kinetic reaction

570. Question:What is the area of chemistry that concerns with the rate at which chemical reactions occur?

a. Chemical collision theoryb. Chemical dynamicsc. Chemical kinematicsd. Chemical kinetics

571. Question:What is the minimum amount of energy need for a chemical reaction to occur called?

a. initial energyb. activation energyc. ignition energyd. catalystic energy

572. Question:If the energy is released as the reaction occurs, it is a ____ reaction.

a. instantaneousb. spontaneousc. exothermicd. endothermic


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CHEMISTRY I

573. Question:If the energy is absorbed as the reaction occurs, it is a ____ reaction.

a. instantaneousb. spontaneousc. exothermicd. endothermic

574. Question:Most heterogeneous catalysts are

a. liquidsb. solidsc. gasesd. plasma

575. Question:What quantity is use to determine how far from equilibrium the chemical reaction is?

a. Reaction indexb. Chemical quotientc. Equilibrium quotientd. Reaction quotient

576. Question:What states that if a change in conditions is imposed on a system at equilibrium, the equilibrium position will shift in the direction that tends to reduce the effects of that change?

a. Hess’ principleb. Catalyst effectc. Haber process principled. Le Chatelier’s principle

577. Question:What is a substance that, when added to a reaction mixture, increases the rate of the reaction but is itself unchanged after the reaction is done?

a. Hydroxide ionsb. Acceleratorsc. Catalystsd. Neutral substance

578. Question:What is a substance that slows down a chemical reaction?

a. Inhibitorsb. Retardantc. Catalystd. Decelerators

579. Question:What type of catalyst exists in the same phase as the reactants in a reaction mixture?

a. Homogeneous catalystb. Heterogeneous catalystc. Pure catalystd. Composite catalyst

580. Question:What type of catalyst exists in separate phase as the reactants in the reaction mixture?

a. Homogeneous catalystb. Heterogeneous catalystc. Pure catalystd. Composite catalyst

581. Question:What refers to the reaction of oxygen with an element or compound? It is also the loss of electron.

a. Reductionb. Oxidationc. Oxygenation


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CHEMISTRY I

d. Oxygenization

582. Question:The gain of electrons by a substance is known as _____.

a. oxidationb. covalent processc. reductiond. ionic process

583. Question:What represents the charge that the atom would have if the electrons in each bond belonged entirely to the more electronegative atom?

a. oxidation numberb. atomic numberc. atomic weightd. electron affinity

584. Question:A reduced substance is what type of agent?

a. oxidizing agentb. redox agentc. reducing agentd. nonredox agent

585. Question:The oxidized substance is what type of agent?

a. oxidizing agentb. redox agentc. reducing agentd. nonredox agent

586. Question:What reaction does not involve any change in oxidation number?

a. redox reactionb. nonredox reactionc. reducing reactiond. oxidizing reaction

587. Question:What is an apparatus that uses a spontaneous redox reaction to generate electricity?

a. voltaic cellb. fuel cellc. lead celld. nickel cadmium cell

588. Question:What is a branch of chemistry which is the study of carbon-containing molecules known as organic compounds?

a. Organic Chemistryb. Inorganic chemistryc. Stoichemistryd. Biochemistry

589. Question:It is a crystalline form of carbon.

a. diamondb. graphitec. fullerenesd. all of the above

590. Question:What crystalline carbon is soft, black, slippery solid that possess metallic luster and conduct electricity?

a. charcoalb. graphitec. diamondd. coke

591. Question:What is formed when hydrocarbons such as methane are heated in the presence of very little oxygen?

a. carbon blackb. charcoal


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CHEMISTRY I

c. coked. diamond

592. Question:Based on the type of bond existing between two carbon atoms, how do hydrocarbons classified?

a. Saturated and unsaturatedb. Pure and unpurec. Organic and inorganicd. Natural and artificial

593. Question:What hydrocarbons contain only single bond?

a. alkaneb. alkynec. alkened. benzene

594. Question:When a hydrocarbon consists of carbon links that form a long, straight or branched chain, it is classified as ____ type.

a. cyclicb. chainc. poled. linear

595. Question:When hydrocarbon consists of carbon links that form a ring, it is classified as ____ type.

a. cyclicb. chainc. poled. linear

596. Question:The aromatic hydrocarbons contain the structural unit called _____.

a. alkyneb. benzene

c. alkened. alkane

597. Question:What is a six-carbon ring with three alternating double bonds, or closely related rings or rings of similar nature where nitrogen replaces carbon in one or more ring positions?

a. alkyneb. benzenec. alkened. alkane

598. Question:What is another term for Alkanes?

a. olefinsb. acetylenec. paraffinsd. methyl

599. Question:What is the simplest alkane which is a major component of nature gas?

a. methaneb. octancec. olefind. acetylene

600. Question:What are hydrocarbons that contain one or more double bonds?


601. Question:What is another term for “alkenes”?

a. olefinsb. acetylenec. paraffins


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CHEMISTRY I

d. methyl

602. Question:What is the simplest alkene, which is a plant hormone that plays important role in the seed germination and

ripening of fruits?

a. anthraceneb. propylc. ethyned. ethene

603. Question:What are hydrocarbons that contain one or more triple bonds?


604. Question:What is the simplest alkyne which is highly reactive molecule?

a. etheneb. acetylene or ethynec. propyld. alkyl

605. Question:The compounds, benzene, naphthalene and anthracene are example of what hydrocarbon?

a. aliphatic hydrocarbonsb. aromatic hydrocarbonsc. alkenesd. alkynes

606. Question:What aromatic hydrocarbon is used as a component of mothballs?

a. benzeneb. naphthalenec. anthracened. methyl

607. Question:In 1956, the International Union of Pure and Applied Chemistry (IUPAC) devised a systematic way of naming organic compounds. What is this called?

a. System Nomenclatureb. System of Identificationc. System of Verificationd. System of Unification

608. Question:In naming of hydrocarbons, what refers to a side chain that is formed by removing a hydrogen atom from an alkane?

a. alkyl groupb. alken groupc. methyl groupd. alkyn group

609. Question:It is usually used as a refrigerant?

a. ketoneb. musconec. propyl etherd. dimethyl ether

610. Question:What are compounds with the same molecular formula but with different structural formula?

a. aldehydesb. aminesc. isomersd. esters

611. Question:


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CHEMISTRY I

What is formed when a carboxylic acid and an alcohol react, with water as a bi-product?

a. amineb. esterc. polymerd. teflon

612. Question:What common carboxylic acid is found in yogurt?

a. lactic acidb. citric acidc. tartaric acidd. lauric acid

613. Question:What carboxylic acid is found in grapes?

a. Lactic acidb. Citric acidc. Tartaric acidd. Lauric acid

614. Question:What carboxylic acid is found in coconut oil?

a. Lactic acidb. Citric acidc. Tartaric acidd. Lauric acid

615. Question:What do you call the distinct pattern in space which the atoms of metals arranged themselves when they combine to produce a substance of recognizable size?

a. space-latticeb. crystalc. graind. unit cell

616. Question:

When a solid has a crystalline structure, the atoms arranged in repeating structures called ____.

a. latticeb. unit cellc. crystald. domain

617. Question:What refers to a crystal imperfection characterized by regions of severe atomic misfit where atoms are not properly surrounded by neighbor atoms?

a. Discrystallizationb. Dislocationc. Slip stepd. Dispersion

618. Question:In electrochemistry, oxidation is a loss of _____.

a. ionb. electronc. protond. anode

619. Question:What is the process of putting back the loss electrons to convert the ions back to a metal?

a. Oxidationb. Corrosionc. Reductiond. Ionization

620. Question:Oxidation in an electrochemical call always takes place where?

a. at the anodeb. at the cathodec. at the electrond. at both cathode and anode


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CHEMISTRY I

621. Question:Reduction in an electrochemical cell always takes place where?

a. at the anodeb. at the cathodec. at the electroded. at both cathode and anode

622. Question:What is equal to the fraction of the isotope in a naturally occurring sample of the element?

a. The chemical atomic weight of the isotope

b. The relative abundance of the isotope

c. The electronegativity of the isotope

d. The quantum number of the isotope

623. Question:what refers to salts of weak bases dissolving in water to form acidic solution?

a. Hydrolysisb. Neutralizationc. Bufferizationd. Titration

624. Question:Which of the following elements has the highest atomic number?

a. Titaniumb. Plutoniumc. Uraniumd. Radium

625. Question:All are properties of gaseous state except one. Which one?

a. may be expanded or may be compressed

b. have low densitiesc. indefinite shaped. mixed uniformly when soluble in

one another

626. Question:All are properties of liquid state except one. Which one?

a. Do not expand nor compress to any degree

b. usually flow readilyc. indefinite shaped. Do not mixed by diffusion

627. Question:What type of hydrocarbons that do not contain the benzene group or the benzene ring?

a. aromatic hydrocarbonb. aliphatic hydrocarbonc. simple hydrocarbond. carbon hydrocarbon

628. Question:What is an organic compound that contains the hydroxyl group?

a. baseb. acidc. alcohold. wine

629. Question:What is a reaction in which one molecule adds to another?

a. partial reactionb. monomolecular reactionc. molecular reaction


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CHEMISTRY I

d. Additional reaction

630. Question:Oxygen comprises what percent in mass in the earth’s crust?

a. 50.5b. 49.5c. 48.5d. 47.5

631. Question:What percent of the human body is carbon?

a. 22%

b. 20%c. 18%d. 16%

632. Question:What refers to how closely individual measurements agree with each other?

a. accuracyb. precisionc. relative precisiond. relative accuracy

633. Question:What is the physical appearance of sodium?

a. silver metalb. yellowish gasc. white crystalc. reddish gas

634. Question:What is the general term that refers to an allowed energy state for an electron in the atom?

a. quantum orbital levelb. quantum energy levelc. orbitald. quantum theory

635. Question:

Who performed an experiment in 1887 that yielded the charge-to-mass ratio of the electrons?

a. Niels Bohrb. Ernest Rutherfordc. J. J. Thomsond. Max Planck

636. Question:What is an alloy of mercury with another metal or metals?

a. Amalgramb. Aminec. Allotroped. Alkynes

637. Question:A compound that contains at least one animo group and at least one carboxyl group is called _____.

a. allotropeb. animo acidc. alkenesd. alkynes

638. Question:A molecular orbit that is of higher energy and lower stability than the atomic orbitals from which it was formed is called _____.

a. main molecular orbitalb. partial molecular orbitalc. bonding molecular orbitald. antibonding molecular orbit

639. Question:What type of carbon is produced when wood is heated intensely in the absence of air? It is used to remove undesirable odors from air.

a. carbon blackb. charcoalc. coked. diamond

640. Question:


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CHEMISTRY I

What carbon is produced when coal is strongly heated in the absence of air?


641. Question:What type of carbon is used in the manufacture of car tires?


642. Question:The organic compounds are related to each other by a common feature involving a certain arrangement of atoms called _______.

a. hydrocarbonsb. chainc. functional groupsd. alkanes

643. Question:What is the simplest and most commonly encountered class of organic compounds?

a. carbidesb. oxidesc. carbon oxidesd. hydrocarbons

644. Question:A molecular orbit that is lower energy and greater stability than the atomic orbitals from which it was formed is called ____.

a. main molecular orbitalb. partial molecular orbitalc. bonding molecular orbitd. antibonding molecular orbital

645. Question:An ion containing a central metal cation bonded to one or more molecules or ions is called ____.

a. compound ionb. complex ionc. simplex iond. buffer ion

646. Question:Which one is a factor that affects the rate of chemical reactions?

a. Temperatureb. Concentration and surface area of

reactantsc. Presence of a catalystd. all of the above

647. Question:What refers to the state at which the rates of the forward and backward reactions are equal?

a. Chemical equilibriumb. Reversible equilibriumc. Reaction equilibriumd. Haber equilibrium

648. Question:What is the study of heat formed or required by the chemical reaction?

a. Stoichemistryb. Thermochemistryc. Thermodynamicsd. Enthalpy

649. Question:Who proposed the quantum theory in 1900?

a. J.J. Thompsonb. Neils Bohrc. Max Planckd. Ernest Rutherford

650. Question:Compounds containing CN ion are called _____.


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CHEMISTRY I

a. cyanidesb. cycloalkanesc. carbidesd. carboxylic acids

651. Question:A molecule that does not possess a dipole moment is called ____.

a. polar moleculeb. nonpolar moleculec. nonelectrolytic moleculed. electrolytic molecule

652. Question:What is the ratio of the equilibrium concentration of the products to the equilibrium concentrations of the reactants with each species

concentration raised to the corresponding stoichiometric coefficient found in the balanced reaction?

a. Equilibrium constantb. Equilibrium concentrationc. Chemical equilibriumd. Reaction quotient

653. Question:What term is used as a qualitative description of the extent of a chemical reaction?

a. Equilibrium positionb. Chemical equilibriumc. Equilibriumd. Reaction equilibrium

654. Question:What is the physical appearance of chlorine?

a. silver metalb. white crystalc. yellowish gasd. white metal

655. Question:

What is the physical appearance of sodium chloride?

a. silver metalb. white crystalc. yellowish gasd. white metal

656. Question:What refers to a substance that when dissolved in water, gives a solution that is not electrically conducting?

a. nonpolarb. electrolytec. nonelectrolyted. polar

657. Question:What refers to a chemical formula that shows how atoms are bonded to one another in a molecule?

a. Molecular formulab. Structural formulac. Standard formulad. Bonding formula

658. Question:What refers to ions that are not involved in the overall reaction?

a. Guest ionsb. Special ionsc. Spectator ionsd. Extra ions

659. Question:A compound distinguished by a high molar mass, ranging into thousands and millions of grams, and made up of many repeating cells is called

a. electrolyteb. polymer c. nucleotided. oxoacid


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CHEMISTRY I

660. Question:How are mixtures classified?

a. Elements and Compoundsb. Metals, Nonmetals or Metalloidsc. Homogenous or Heterogeneousd. suspension, colloids and solutions

661. Question:The mixture of soil and water is an example of what classification of a mixture?

a. homogenousb. suspensionc. colloidd. solution

662. Question:A very fine particle of soil when mixed to water will form a cloudy mixture. How is the mixture classified?

a. colloidb. suspensionc. solutiond. compound

663. Question:The particles of sugar dispersed in water are so small that a clear homogeneous mixture results. What is this homogeneous mixture called?

a. colloidb. compoundc. suspensiond. solution

664. Question:If one of the two solutions has a higher concentration of solute particles than the other, the one with the lower concentration is described as ______.

a. hypertonicb. hypotonicc. isotonicd. photonic

665. Question:The movement of solvent particles through a semi-permeable membrane from the region of lower solute concentration to the region of higher solute concentration is called _______.

a. osmosisb. hymolysisc. crenationd. dialysis

666. Question:What are suspensions of liquid or solid particles in a gas called?

a. emulsionsb. aerosolsc. foamsd. sols

667. Question:What is the atomic number of carbon?

a. 6b. 7c. 8d. 10

668. Question:Who formulated the atomic theory?

a. John Daltonb. Humphrey Davyc. Henri Becquereld. Ernest Rutherford

669. Question:


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What is the ratio of the number of moles of one component of a solution to the total number of moles of all the components?

a. molarityb. molalityc. formalityd. mole fraction


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