Name:Topic 1: Data Collection

What is chemistry? How do we make accurate and precise observations of our world?Vocabulary

Term Definition

Organic ChemistryInorganic ChemistryAnalytical ChemistryPhysical ChemistryBiochemistry

Qualitative ObservationQuantitative ObservationPrecision

Accuracy

Dependent VariableIndependent VariableScientific MethodMajor prefixes of the Metric System (kilo-milli)SI System

Density

Intensive propertyExtensive propertyDimensional AnalysisConversion FactorSignificant FigureUncertainty

1

Name:Topic 1: Data Collection (cont)

What is chemistry? How do we make accurate and precise ob3servations of our world?Objective Practice Problem

Identify the proper names and uses of common laboratory materials.

1. Label the following materials with their proper names and uses

Read laboratory measuring instruments to the nearest degree of precision and record data with correct number of significant figures.

2. Use the picture to the right to answer the following questions.

a. Each mark represents __________ mL.

b. The device shown is precise to what decimal place? ________

c. According to the measuring device, what is the volume of water?____________

Name and use basic SI units.

3. Label each of the following measurements with the proper SI unit.

Length _______________ Volume ______________ Mass ______________

4. Label the values below with the correct metric prefixes

___________1000 ___________1/1000 ___________1/100 ___________1/10

Distinguish between qualitative and quantitative observations.

5. Classify each of the following as either a qualitative or quantitative observation:

________________ The candle weighs 4.00 grams. ________________ The candle is round.

________________ The candle burned brightly. ________________ The candle is 2.00cm.

Perform mathematical operations involving dimensional

6. Convert using proper dimensional analysis: 25.4ft/day = ? cm/min

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Name:analysis.Determine the number of significant figures in measurements.

7. Underline and state the number of significant figures in each of the following values:

1.201 ___________ 12.0 x 104 ___________

0.012 ___________ 1200 ___________

8. Round each of the following numbers to 3 significant figures:

125.32 ________________ 124.500

________________

23.523 ________________ 0.0010101

________________

Perform mathematical operations involving significant figures.

9. Solve the following. Report answers with correct units and significant figures:

6.5 cm / 2.1 cm = _____________________

2.33 K + 18.1 K _______________________

0.00032 m x 12 m =_____________________

44.25 kg – 2.25 kg ________________________

Topic 1: Data Collection (cont)What is chemistry? How do we make accurate and precise ob3servations of our world?

Perform mathematical operations involving significant figures AND use basic SI units.

10. Convert the following (while maintaining the same number of significant figures):

42.1 g = ___________ kg 0.450 L = ___________ mL 2.25 L = ___________ mL

5.4 ft/day =___________ cm/min 3.2 °C = ___________ °F 126 K =___________ C

Perform mathematical operations involving scientific notation.

11. Express the following numbers in scientific notation:

52,000 = 0.000175 =

12. Perform the computations below expressing the answers in scientific notation

(7.1x 109)(55) = 10,500 ÷ (4.0 x 10 -4) =

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Name:Differentiate between a precise and an accurate set of data.

13.

Distinguish between intensive and extensive properties.

14. Label the following as intensive or extensive properties of matter:

Density _________________ Volume _________________

Mass _________________ Temperature_________________

4

Name:Topic 2: Chemical and Physical Properties of Substances

What are the characteristics by which matter can be classified?Vocabulary

Term Definition

matter

chemical change

chemical property

physical change

physical property

changes of state (phase change)solid, liquid, gas, plasmapure substance

atom

element

compound

mixture

heterogeneous mixturehomogeneous mixturesolution

solute

solvent

aqueous solution

density

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Name:Topic 2: Chemical and Physical Properties of Substances

What are the characteristics by which matter can be classified?Objective Practice Problem

distinguish between chemical and physical properties; chemical and physical changes.

15. Classify each of the following as either a physical or chemical change or property

Release of Odor _________________ Reactivity _________________

Paper Burning _________________ Crushing Chalk _________________

Color Change _________________ Melting Butter _________________

Cutting Paper _________________ Stirring _________________

distinguish between and classify types of matter

16.

Topic 2: Chemical and Physical Properties of Substances (continued)distinguish between and classify types of matter

17. Complete the following table using the terms element, compound, mixture, heterogeneous, homogeneous, and pure substance.

6

Name:18. A group of two or more substances that are physically combined are called a

a. mixture.b. compound.c. element.

19. Mixtures that are not evenly mixed throughout are calleda. pure substances.b. homogeneous.c. heterogeneous.

20. Classify the following substances as a: heterogeneous mixture, solution, compound, or

element.

a. iron shavings (Fe) _________________ c. brewed tea _________________

b. neon gas (Ne) _________________ d. water (H2O) _________________

e. granite _________________ f. nitrogen _________________

g. salt (NaCl) _________________ h. energy drink _________________

describe the characteristics of phase states in terms of particle arrangement and motion.

21. Which of the following has a definite shape? Circle all that applya. Solids b. Liquids c. Gases

22. Which of the following has a low density? Circle all that applya. Solids b. Liquids c. Gases

23. Label each of the following with A-I as given in the diagram to the right_____ Melting _____ Evaporation

_____ Liquid _____ Solid

_____ Gas _____

Condensation _____ Freezing

describe the relationship between energy, particle motion and change of phase.

24. Label A, B, and C with the proper phase states.25. Label 1,2,3,4 with the proper phase changes

26. At point 3 on the graph above,a. the heat added increases and the temperature increases.b. the heat added decreases and the temperature decreases.c. the heat added decreases and the temperature stays the same.

7

Name:d. the heat added increases and the temperature stays the same.

Use derived properties to identify substances

Use the diagram below to answer the next three questions27. Which line in the graph above represents lead? The density of lead is 11.4 g/mL. The

density of gold is 19.3 g/mL.e. Line Af. Line Bg. Line A if the piece of lead is larger than the piece of gold.h. Line A if the piece of gold is larger than the piece of lead.

28. Which of the following has the greatest volume?

i. 80 g of substance Aj. 80 g of substance Bk. both have the same volumel. not enough information to tell

29. The independent variable in the graph ism. volume in mL.n. mass in go. line A.p. line B.

Topic 3: Atomic TheoryWhat is all matter made of?

VocabularyTerm Definition

atom

atomic mass

atomic number

isotope

mass number

neutron

proton

nucleus

atomic orbital

electron

photon

Aufbau principle

Hund’s rule

8

•••••••••••

020406080

100120140160180200

0 1 2 3 4 5 6 7 8 9 10Volume (mL)

•Line A Line B

Name:Pauli exclusion principleatomic emission spectrum

electromagnetic spectrumcontinuous spectrumline spectrum

quanta

Ground state

Excited state

Topic 3: Atomic TheoryWhat is all matter made of?

Objective Practice ProblemsState the position of protons, neutrons and electrons in the atom.

State the relative masses and relative charges of protons, neutrons and electrons.

30. Draw a bohr model of an atom of Sodium-23, labeling the number of protons, neutrons, electrons and their charges.

Determine the number of protons, neutrons and electrons in atoms and ions from the mass number, atomic number and charge.

31. Complete the following table:Symbol

Atomic # Mass # # Protons # Electrons # Neutrons Ionic Charge

34 80 0

Define the term isotope.Write the symbolic notations used to represent isotopes.Calculate the atomic mass for an element given the mass of its isotopes

32. How many neutrons do each of the following isotopes contain?

(a) chlorine-32 ___ (b) gold- 169 _______ c) lead-182 _______

33. Given the following information for element "X",Isotope Mass (amu) Percent Abundance1 34.97 75.77%2 36.97 24.23%(a) Calculate the atomic mass for element “X” (b) Identify element X :

9

Name:and the percent abundance for each.Describe the electromagnetic spectrum.

34. Draw two waves with the wavelengths representing the relative energies of red light and of blue light.Label one “more energetic,” the other “less energetic.”

Describe how the frequencies of light emitted by an atom are a unique characteristic of that atom.Summarize the main features of the Bohr model of the hydrogen atom.

35. Which of the following does the Quantum Mechanical model of the atom propose?a. The atom contains protons and electrons.b. Electrons orbit the nucleus of the atom.c. Electrons orbit the nucleus in specific patterns.d. Electrons emit energy in the form of light.

36. Complete the following table:Principal Energy Level

Total number of sublevels

Total number of orbitals

Total number of electrons

24

25

37. Write labeled orbital diagrams for each of the following elements:Calcium Argon

Apply the Aufbau principle, Hund’s rule and the Pauli Exclusion Principle to write electron configurations for an atom.

Write electron configuration and ion configurations of elements

38. Write the electron configurations for the following elements using noble gas notation.Mn Zn

P Pb

39. Write the full electron configurations for the following ions:P-3 Al 3+

40. Determine which of the following electron configurations represent an atom in theexcited state and identify that element. (Circle choice and name the element)a. 1s22s32p63s23p6 b. 1s22s12p63s23p5 c. 1s23s22s22p63p6

element name_______________________________

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Name:Topic 4: Periodic Trends

What trends are used to identify the properties of elements and compounds?Vocabulary

Term Definition

Diatomic element

Periodicity

Electronegativity

Dimitri Mendeleev

Periodic Law

Group/Family

Period

Valence Shell

Valence Electron(s)

Octet Rule

The shielding effect

Atomic Radius

Ionic Radius

Ionization Energy

Topic 4: Periodic TrendsWhat trends are used to identify the properties of elements and compounds?

Objective Practice ProblemsIdentify the diatomic elements.

41. List the formulas of the diatomic elements: H2 ,

Discuss the relationship between an element's electron configurations its location on the periodic table.

An atom is found to have the electron configuration of [Kr]5s24d105p5

42. Identify this element:

43. How many valence electrons does it have?

44. What family does this element belong to?

45. What charge do all of elements in this family have and why?

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Name:

Compare the periodic trends of atomic and ionic radius, ionization energy, and electronegativity.

Explain how the shielding effect influences atomic radius, ionization energy, and electronegativity.

Classify the phase state of an element as a solid, a liquid, or a gas.

Describe the main features of our modern periodic table.

Locate and name the s, p, d and f- blocks on the periodic table.

Using the periodic table below,46. Circle the only noble gas that does not have a p orbital.47. Number the groups 1A-8A48. Number the periods 1-749. Box and Label the 2-s block, the 3p-block, 5d-block, and the 4-f-block.50. Label the halogens, transition elements, alkaline earth metals, alkali metals, and the noble

gases.51. Label groups 1A, 2A and 7A with their ionic charge52. Put an X through all seven elements that are naturally diatomic.53. Label the arrows to show the trends for electronegativity both along a period and a group54. Label the appropriate arrows to show the trends for atomic radius both along a period and a

group55. Label the appropriate arrows to show the trends for ionization energy both along a period

and a group

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Name:

Topic 5: BondingHow do elements combine to form new matter?

How does the type of bond affect the properties of the compound?

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Name:Vocabulary

Term Definition

Ion

Anion

Cation

Ionic bond

Lattice energy

Metallic bond

Oxidation numberCovalent bond

Lewis structure

Resonance structureVSEPR

Polar covalent

Non-polar covalentDispersion force

Dipole-dipole

Hydrogen bond

Pi bond

Orbital hybridizationBond length

Bond strength

Bond energy

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Name:Topic 5: Bonding

How do elements combine to form new matter?How does the type of bond affect the properties of the compound?

Objective Practice ProblemsProperly write the chemical formulas of ionic compounds when given the name

Properly write the chemical formulas of molecular compounds when given the nameProperly write the chemical formulas of acids when given the name

56. Write the correct formula for the following compounds:

sulfur trioxide____________________ calcium sulfate

____________________

phosphoric acid____________________ hydrofluoric

acid____________________

aluminum fluoride ____________________ lead(II)nitrate

____________________

aluminum hydroxide ____________________ ammonium carbonate

______________

gold(III)chloride dinitrogen pentaoxide

Properly name ionic compounds when given the chemical formula

Properly name molecular compounds when given the chemical formula

Properly name acids when given the chemical formula

57. Write one proper name for each of the following compounds.

PbCl4 _____________________________________________

NCl3 _____________________________________________

S2F10 _____________________________________________

Hg(NO3)2 _____________________________________________

HNO3 _____________________________________________

H2S _____________________________________________

Fe(OH)3 _____________________________________________

Sn3(PO4)4 _____________________________________________PREDICT the type of chemical bond formed using electronegativity differences

58. An ionic bond exists when the electronegativity difference is greater than _________

59. A covalent bond exists when the electronegativity difference is _______

60. A polar covalent bond exists when the electronegativity difference is between _______________

15

Name:DESCRIBE the characteristics of ionic and covalent compounds

61. Circle the words that complete the sentence. (Molecular/Ionic) bonds are usually (strong/weak) and (do/ do not) conduct electricity, are volatile and have a low melting point.

16

Name:Topic 5: Bonding(Continued)

DRAW Lewis Diagrams of Ionic and Covalent Bonds based on the Octet Rule

Draw resonance structures

DETERMINE the direction of a dipole moment in a polar molecule

PREDICT the molecular geometry of a molecule using the VSERP Model

Predict the polarity of a molecule

62. Lewis Structure

Electro-negativityDifference

Bond Polarity

Molecular Shape(VSEPR)

Shape Name Molecular Polarity

CBr4

H2O

PH3

SO3

NH4+

Brackets!

BH3

Classify the intermolecular forces that exist between atoms and molecules.

Identify the type of bonding that occurs between the atoms/molecules/ions listed below.(Select: Ionic, polar covalent, nonpolar covalent, dipole-dipole, hydrogen bonding, dispersion forces.)

63. ___________________________Between atoms of hydrogen and oxygen in a water

molecule

64. ___________________________Between molecules of water

65. ___________________________Between atoms of bromine in a bromine molecule

66. ___________________________Between molecules of bromine

67. ___________________________Between ions of sodium and chlorine in sodium chloride

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Name:68. ___________________________Between molecules of fluoromethane

Topic 6: The MoleHow do chemists quantify matter?

VocabularyTerm Definition

Empirical Formula

Molecular Formula

Structural Formula

Formula unit

Mole

Molar mass

Avogadro’s principle

Percent Composition

Objective Practice ProblemsDefine mole, Avogadro's number, and molar mass, and state how all three are related.

Calculate the number of atoms in a sample of any chemical element.

Perform mole-mass conversions.

69. How many atoms are in one mole of sulfur? _______________________________

70. How much volume does one mole of any gas at STP occupy? __________

71. Calculate the molar mass of the following compounds:Ca(OH)2 = Sulfur trioxide =

FeCl3 = Iron(III) sulfide=

72. How many moles are in 10.0g of potassium chlorate?

73. How many grams are in 2.2 moles of hydrosulfuric acid?

74. How many molecules are present in 2.50 moles of sulfur dioxide?

75. How many oxygen atoms are contained in 13.5 grams of carbonic acid?

76. What is the mass of 4.32 x 1025 molecules of ammonia (NH3)?

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Name:

Topic 6: The Mole (continued)Calculate the percent composition of a compound.

77. Calculate the percentage composition by mass of C12H22O11.

Determine the empirical formula and molecular formula of a compound.

78. An unknown compound is composed of 71.0% silver, 7.9% carbon, and 21.1% oxygen.Determine the empirical formula for this compound.

79. What is the molecular formula and name of this compound if it has been determined to have the molar mass of 303.8 grams?

Determine the chemical formula of a hydrate.

Experimentally determine the chemical formula of a hydrate.

80. Use the data below to determine the formula and name for the aluminum bromide hydrate, AlBr3•XH2O.

Mass of empty crucible and lid: 4.26 gMass of crucible, lid, and hydrate: 8.60 gMass of crucible, lid, and anhydrate (i.e., after heating): 7.35 g

19

Name:

Topic 7: Chemical ReactionsHow do chemists quantify matter?

VocabularyTerm Definition

decomposition (analysis)

combination (synthesis)

single-replacement

double-replacement

combustion of a hydrocarbonneutralization reaction

Precipitate

Activity Series

Topic 7: Chemical ReactionsObjective Practice Problems

STATE the reasons why a chemical reaction must be balanced.

81. A balanced equation verifies the law of conservation of matter becausea. the molar masses of all substances are the sameb. the coefficients on both sides of equation are the samec. the moles of reactants equals the moles of productsd. the mass of reactants equals the mass of products

READ a chemical reaction properly and identify the major parts, such as products, reactants, yields, and phase states.

82. The equation that correctly describes the reaction at right isa. Al2 + 3 Cl2 --> Al2Cl6b. 2 Al + 3 Cl --> 2 AlCl3c. 2 Al + Cl2 --> 2 AlCld. 2 Al + 3 Cl2 --> 2AlCl3

83. Identify the products above:

84. Identify the reactants above:

85. Aqueous solutions of magnesium chloride and sodium hydroxide are mixed together to produce solid magnesium hydroxide. Write a complete balanced equation for this reaction (include phases).

20

Cl

ClAl

Al

Al

Al

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Name:86. What type of reaction is this? ________________________________

APPLY the rules for balancing chemical reactions to a given list of chemical reactions.

87. Balance the following equations:a. N2 + H2 NH3

b. Cs + H3PO4 Cs3PO4 + H2

c. MnO2 + HCl MnCl2 + H2O + Cl2

d. C4H10 + O2 CO2 + H2O

IDENTIFY and NAME the major types of chemical reactions- synthesis, single replacement, double replacement, combustion or decomposition.

PREDICT the products or reactants of a chemical reaction when given one or the other.

88. Properly predict the products, balance and name each of the reactions below. Assume all reactions occur (phases not needed)

Reactants Products Reaction Type

Ca(OH) 2 + H2SO4

Mg(ClO3) 2 + O2

K + O2

C7H16 + O2

Li + I2

Al + HCl

CaO

Zn + FeCl3

Al2 SO4)3 + MgCl2

Determine an activity series and predict whether or not a reaction will occur

89. Predict whether a reaction will occur for each of the following. If a reaction takes place, write a balanced chemical equation (including phases). If a reaction does not take place, write No RXN.

a. Cl2 (g) + KBr (aq)

b. NaOH (aq) + AlCl3 (aq)

c. Fe(NO3)2 (aq) + MgCl2 (aq)

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Name:

d. H2CO3 (aq) + Ba(OH)2 (aq) Topic 8: Stoichiometry

How do chemists predict the amount of products that can be produced by a chemical reaction?Vocabulary

Term Definitionstoichiometry

Limiting reactant

Excess reactant

Theoretical yield

Percent Yield

Precipitate

Topic 8: StoichiometryHow do chemists predict the amount of products that can be produced by a chemical reaction?

Objective Practice ProblemsPREDICT the amount of a substance being used or produced by a reaction using the method of stoichiometry

90. Determine the moles of hydrogen gas produced when 50 grams of aluminum are reacted with sulfuric acid.

91. Calculate the volume of hydrogen gas that must be burned with oxygen gas to form 4.0 moles of water at STP.

92. When 234 grams of HgO is heated until decomposition, what mass of mercury will be formed?

22

Name:Topic 8: Stoichiometry (continued)

How do chemists predict the amount of products that can be produced by a chemical reaction?DETERMINE the limiting reactant in a chemical reaction

CALCULATE percent yield of a reaction.

93. 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)According to the above balanced chemical equation, if you place 5.00 grams of aluminum into 5.00 grams of sulfuric acid….

a. How many grams of aluminum sulfate can be produced?

b. What is the limiting reactant? ___________________

c. Which reactant is in excess and by how much?

d. If the actual yield of the aluminum sulfate is 5.35 grams, what is the percent yield?

Determine the activity series of a set of reactions.

From the data below, determine the activity series of these six elements:X, Y, Z, H, Ba, and Hg, placing the most active one first in the box provided below.

Reactants Observations

X + HCl Bubbles formY + HCl No ReactionZ + BaCl2 No Reaction

Y + HgCl2 A liquid metal begins to appear

Z + HCl Bubbles formZ + XCl3 A dark substance begins to form on the Z metal

Work space: (if needed)

94. Activity Series:

most active ------------------------------------------------------------------> least active23

Name:

Topic 9: Acids/ Bases/ MolarityHow do acids and bases react in solution?

VocabularyTerm Definition

Solute

Solvent

Saturated Solution

Solution

Solubility

Molarity

Bronsted-Lowry Acid:

Bronsted-Lowry Base:

Titration:

Salt:

Buffer:

pH

Objective Practice ProblemsGiven two of the following values (molarity, mass, and volume), CALCULATE the third value.

95. How many grams of K2SO4 will be required to prepare 250mL of 0.5 M potassium sulfate?

96. How many grams of NaOH will be required to prepare 500mL of 0.25 M sodium hydroxide?

CALCULATE and DESCRIBE how to prepare a solution and perform a dilution

97. Describe how you would prepare 100mL of 0.1 M HCl from 1M HCl?

24

Name:DIFFERENTIATE between an Arrhenius acid/base and a Bronsted-Lowry acid/base.

98. Label and connect the conjugate acid-base pairs in the following reactions:

NH4+ + OH- NH3 + H2O_________ _________ _________ _________

C2H3O2- + H2O HC2H3O2 + OH-_________ _________ _________ _________

99. Which reaction(s) above don’t fit Arrhenhius’s definition of an acid/base and WHY?

Topic 9: Acids/ Bases/ Molarity (continued)EXPLAIN the differences among an acid, a base, and a salt, and write balanced chemical equations for neutralization reactions.

100. Complete and balance the neutralization reactions shown below. Include the intermediate acid-base ions. Your completed reactions must be balanced..

HCl + Mg(OH)2

H3PO4 + Ga(OH)3

HNO3 + Ba(OH)2

RELATE the ideas of Ka, pH, and conductivity to acid-base chemistry, and describe the relationship among, Ka, pH and conductivity, and acid-base strength.

Given that HNO3, is a strong acid,

101. Would you expect the Ka value for nitric acid, HNO3, to be large or small?

_______102. Would the equilibrium mixture for nitric acid, HNO3, contain mainly products

or mainly reactants? _______103. When 4 moles of nitric acid dissolve in 1 liter of water, what will be the

approximate concentration of H3O+ ion formed? ________

104. Would HNO3 have a high or a low conductivity? __________

105. Would HNO3 have a high or a low pH value? __________

106. Below you are given three values for the concentration of H+ ions of three

different acids. Based on your knowledge of the relationship between [H+], pH, and conductivity, determine which of the three given pH values and relative

conductivities best matches each of the concentrations of H+.

[H+] pH (9.2, 6.9, or 1.4) Conductivity (high, medium, or low)

5.7 X 10-10M _______________ ___________

1.3 X 10-7M _______________ ___________

25

Name:

4.4 X 10-2M _______________ ___________107. A solution has a hydrogen ion concentration of 3.42 x 10-10 M.

What is [OH-] of the solution?

What is the pH of the solution?

Is the solution acidic or basic? __________________EXPLAIN the principles involved in the titration of acids and bases, and use unit analysis to calculate concentrations or volumes in titration problems.

108. What is the molarity of a nitric acid solution if 43.3 mL of 0.100 M KOH solution is needed to neutralize 20.0 mL of the acid?

109. Based on the data gathered below after titrating an solution of sodium hydroxide of unknown concentration, calculate the average concentration of the unknown sodium hydroxide solution. Show all of your work.

Calculation Trial 1:

Calculation Trial 2:

Calculation Trial 3:

Average concentration of unknown NaOH solution:

Concluding questions If you were graded on the overall effort you put into this class, what grade do you think you would deserve? (Please answer this as honestly as possible!)

26

Trial 1 Trial 2 Trial 3Initial burette HCl reading 0 15.0 29.2Final burette HCl reading 15.0 29.2 45.5

mL of acid addedVolume of NaOH solution 10.0 mL 10.0 mL 10.0 mL

Concentration of HCl 1.00 1.00 1.00Concentration of Unknown NaOH

Name:That’s it... You’re Done! Good Luck on the Final!!!

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