Name: Class: Date: ID: A

ChemA PRACTICE Final Part 2 2013-2014 1. Which of the following did Dalton discuss in his atomic theory?

A. electrons C. isotopes E. protons B. neutrons D. ions F. atoms

2. The law of constant composition applies to A. metals C. heterogeneous mixtures E. compounds B. metalloids D. homogeneous mixtures

3. A substance composed of two or more elements combined chemically in a fixed proportion by mass is A. a compound C. an atom E. None of the above B. a mixture D. a solid

4. The fundamental particle of a chemical element according to Dalton's theory is the A. atom B. compound C. electron D. molecule

5. In chemistry, a formula is used to represent A. a compound C. an element E. None of the above B. a metal D. All of the above

6. The total number of oxygen atoms indicated by the formula Fe2 (804)3 is A. 12 B. 3 C. 7 D. 4 E. 24

7. Which of the following contains the largest number of oxygen atoms? A. H2S04 B. 3C02 C. 4H20 D. A1(N03)3 E. 0 2

8. The chemical formula Ga203 indicates A. two atoms of gallium and three atoms of D. three atoms of gallium and two atoms of

oxygen oxygen B. five atoms of each element E. None of the above C. six atoms of each element

9. Which atomic particle determines the chemical behavior of an atom? A. nucleus C. electron E. None of the above B. neutron D. proton

10. List the three main subatomic particles. 11. Which particle has the smallest mass?

A. helium nucleus B. neutron C. electron D. proton 12. How many protons, electrons, and neutrons, respectively, does 127I have?

A. 74, 53, 127 C. 53, 53, 127 E. 53, 53, 74 B. 53, 74, 53 D. 53, 127, 74

13. An atom with 19 protons and 20 neutrons is an atom of A. Ca B. F C. Sr D. Ne E. K

Identify each of the following: 14. The heaviest noble gas 15. The halogen in the third period 16. The average mass of a calcium atom is 40.08. Assuming you were able to isolate only one boron atom, the

chance that you would randomly get one with a mass of40.08 is A. greater than 50% C. about 60% E. 0% B. 40.08% D. 0.08%

1

Name: ID: A 17. Atoms of the same element having the same atomic number, but different mass numbers, are called

A. isotopes C. neutrons E. nuclei B. orbitals D. isomers

18. The atom with 57 neutrons and 40 protons has a mass number of A. 97 C. cannot be determined E. 17

from information given B. 57 D. 40

19. The mass number of an atom equals A. the atomic number of the element B. the number of neutrons per atom C. the atomic mass of the element D. the number of protons plus the number of neutrons per atom E. None of the above

20. How many neutrons are contained in an Bromine nucleus with a mass number of 80? A. 80 B. 125 C. 53 D. 35 E. 45

21. Which of these are isotopes of helium? A. 3Heand2He C. 2Hand3He E. 12C and 13C B. 42Kand40K D. 2Liand2He

22. How many electrons are present in a germanium atom with a mass number of 73? A. 6.02 xlO23 B. 41 C. 105 D. 32 E. 73

23. How many electrons are present in a bromine atom with a mass number of 87? A. 35 B. 87 C. 6.02 xlO23 D. 122 E. 80

24. The number of protons in the nucleus of an atom is called its A. mass number C. valence E. None of the above B. atomic number D. isotope number

25. Choose the pair in which the components have the same charge. A. a proton and a hydrogen atom C. an electron and a neutron B. a neutron and a hydrogen atom D. a hydrogen atom and an electron Classify the following as a metal, nonmetal, or metalloid. A. metal B. nonmetal C. metalloid

26. arsenic 27. argon 28. calcium 29. plutonium 3 0. Which of the following is a nonmetal?

A. copper B. cesium C. carbon D. calcium 31. An atom with 47 protons has a mass number of 107. The atom is

A. Ag B. Nd C. Bh D. Ir 32. How many electrons are present in a Chlorine, CI, atom?

A. 36 B. 17 C. 7 D. 1 33. How many protons are in the nucleus of a Ca atom?

A. variable B. 40 C. 41 D. 2

E. cerium E. None of the

above E. 35 E. 20

2

Name: ID: A

34. Which of the following elements is an alkali metal? A. Fe B. Sc C. Ca D. Na

E. Cu 35. Which of the following elements is an alkaline earth metal?

A. Cu B. Ca C. Na D. Fe E. Sc

36. Which of the following is a noble gas? A. N2 B. Ar C. H2 D. C02

E. o 2 37. Which of the following elements is most similar to Potassium?

A. H B. N C. Na D. Hg E. Ca

Express the following in scientific notation: 38. 0.00832 39. 178,428 40. 6020 41. 0.00304 42. Convert: 1 cm = mm. 43. Convert: 4.96 kg = mg. 44. Convert: 683 mm = cm. 45. Convert: 25 mL = L-46. The number of cubic centimeters (cm3) in 43.0 mL is

A. 43.0 cm3 C. 4.30 cm3

B. 0.0430 cm3 D. None of the above 47. Using scientific notation, round 281,472 to three significant figures. 48. Round 0.006781 to two significant figures, and express it in scientific notation. 49. Convert: 801 K = °C. 50. Do significant figures Review worksheet 51. Do Temperature Conversions worksheet ^ ^ ^ - y r a o f r _ e wksk-h 52. Do dimensional analysis/density review worksheet 53. Do writing and balancing equations worksheet

ChemA Practice Final 2013-2014 Part 2 KEY 1. F 10. Electron 17. A 26.C 35.B 43. 4.96 x 106 2. E proton 18. A 27. B 36.B 44. 68.3 3. A neutron 19. D 28.A 37.C 45. 0.025 4. A 11. C 20.E 29.A 38. 8.32 xlO"3 46. A 5. A 12. E 21. A 30.C 39. 1.78248 x 47. 2.81 x 105 6. A 13. E 22.D- 31. A 105 48. 6.8 x lO'3 7. D 14. Rn 23.A 32.B 40. 6.02 xlO3 49. 528 8. A 15. CI 24.B 33.E 41. 3.04 x 10"3 9. C 16. E 25.B 34.D 42. 10

3

Temperature Conversion Review

K = C + 273 C = (F - 32) x 5/9 C = K -273 F = ( C x 9/5) + 32

1) 250 Kelvin to Celsius 7) Convert -200 Celsius to Kelvin

2) 339 Kelvin to Celsius 8) Convert 355 Kelvin to Celsius

3) 17 Celsius to Kelvin 9) Convert 230 Celsius to Fahrenheit

4) 55 Celsius to Kelvin 10) Convert 60 Fahrenheit to Kelvin

5) 89.5 Fahrenheit to Celsius 11) Convert 100 Fahrenheit to Celsius

6) 383 Kelvin to Fahrenheit 12) Convert 150 Celsius to Fahrenheit

KEY

1) -23°C

2) 66 °C

3) 290K

4) 328K

5) 32 °C

6) 230 °F

7) 73K

8) 82 °C

9) 446 °F

10) 290K (289K is acceptable too)

11) 38°C

12) 302°F

4-

Worksheet: Significant Figures Review Directions: Write the number of significant figures in the blank proceeding the number.

1) 10 11) 200. 21) 123,987 2) 3201 12) 102.59 22) 3,180.00

3) 4.00 13) 0.011032 23) 43.60

4) 7.99 14) 932,004.6 24) 1.6000040

5) 0.238 15) 880.00 25) 0.045090

6) 12.010 16) 101 26) 0.095

7) 23,000. 17) 2.808000 27) 100.00

8) 12,800 18) 1.80081 28) 30,022.070

9) 309.009 19) 0.00024900 29) 910 10) 1,000,000 20) 70 30) 0.030300

Significant Figures and Rounding Measurements 1. Round off each of the following numbers to three significant figures a. 15.9994 b. 1.0080 c. 0.6654 d. 4885 e. 87,550 f. 0.027225 2. Put the following numbers into scientific notation and write down the number of significant figures in each: a. 0.225 b. 2.5 c. 44,163 d. 20,190 e. 0.00000000000991 f. 7,000 3. How many significant figures are in each of the following numbers? a. 225.0 b. 1000.0 c. 0.0003210 d. 0.0067 e. 1,000,000. f. 2.00001 4. Express the following fractions in decimal from to 2 significant digits. a. % b. 2/3 c. 5/3 d. 13/5 5. Perform the indicated arithmetic operations, and round the results to the appropriate number of significant digits. REMEMBER - there are two completely different sets of rules for addition/subtraction and multiplication/division!!! a. 77.981 x 2.33 = b. 4x0.0665 =_ c. 17.34 + 4.900 + 23.1 = d. 9.80-4.762 =

5

e. 3 .9X6.05X420 f. 14.1/5 =

g. 1001 + 16.23 h. 424.5 + 2.8461 i. 9 .9-9 .54 =

j . 7.3778-0.000265 = k. (24.358X6.4) =

1. 48.6(0.6959) = m. (6.082-1023)(5.0-10"3)

n. (9.9-104) +(1.273-102)

Worksheet: Significant Figures Review KEY 1) 1 6) 5 11)3 16)3 21)6 26)2 2) 4 7) 5 12)5 17)7 22)6 27)5 3) 3 8) 3 13)5 18)6 23)4 28)8 4) 3 9) 6 14)7 19)5 24)8 29)2 5) 3 10)1 15)5 20)1 25)5 30)5 Significant Figures and Rounding Measurements KEY 1) . 3) . 5) .

2)

a) 16.0 a) 4 a) 182 b) 1.01 b) 5 b) 0.3 c) 0.665 c) 4 c) 45.3 d) 4890 d) 2 d) 5.04 e) 87,600 e) 7 e) 9900 0 0.0272 f) 6 f) 3

4) • g) 1017 a) 2.25 x 10"1 (3sf) a) 0.25 h) 427.3 b) 2.5 x 10° (2sf) b) 0.67 i) 0.4 c) 4.4163 x 104 (5sf) c) 1.7 j) 7.3775 d) 2.019 xlO 4 (4sf) d) 2.6 k) 160 e) 9.91 x 10"12 (3sf) 1) 33.8 f) 7 x l 0 3 (lsf) m) 3.0 x 1021

n) 9.9 x 10*

Name: Period:

Protons, Neutrons, and Electrons Practice Worksheet

Atomic symbol

Atomic number Protons Neutrons Electrons Mass

Number »* 6

11 24 31 37

39 89 29 35 28 43 100

™Pb2+ 207 102 70

225

—Mo 53

22 19 39

30 16 18 32

Problems 1. Boron has two naturally occurring isotopes: B-10 and B-11. 19.8% is B-10, and the

other 80.2% is B-11. Calculate the average atomic mass of Boron.

2. Nitrogen has two naturally occurring isotopes: N-14 and N-15. The average atomic mass of nitrogen is 14.01. Which isotope is more abundant in nature? Explain.

3. Calculate the average atomic mass of magnesium. The three magnesium isotopes, and their relative abundances are: Mg-24 (79%), Mg-25 (10%), and Mg-26 (11%).

7

Solutions for the Protons, Neutrons, and Electrons Practice Worksheet:

Atomic symbol

Atomic number Protons Neutrons Electrons mass #

5 5 6 5 11

\\Na 11 11 13 11 24

fxGa 31 31 37 31 68 89 y 391

39 39 50 39 89

29 ^-^'^ 29 29 35 29 64

Jc 43 43 57 43 100

82 82 125 80 207

l02Yb 70 70 102 70 172

225 Ac 89 Sit

89 89 136 89 225

HMo 42 42 53 42 95 31 p 3 -1 5 ^ 15 15 16 18 31

19 19 20 19 39

56 Fe 26 26 30 26 56

32 c 2 -1 6 ^

16 16 16 18 32

Problems

1. (0.198)(10) + (0.802)(11) = 10.802

2. N-14 is more abundant. The average atomic mass is much closer to 14, indicating that most nitrogen has a mass number of 14.

3. (0.79)(24) + (0.10)(25) + (0.11)(26) = 24.32

Dimensional Analysis and Density Review Worksheet Conversion Factors: lmile = 1.61km 1 mile = 5280 feet 1 inch = 2.54 cm 454g = lb 1kg = 2.2 lb

(MEMORIZE these, and metric prefixes as well!) 1. Convert 26.4 mi to km

2. Convert 0.0489 g to mg

3.Convert 16 years to days

4. Convert 1067 cm to km

5. How many feet are in 3.2 miles?

6. How many miles is 7,598 feet?

7. How many meters are in 2.7 km?

8. How many inches are in 1.00 mile?

9. How many mm are in 0.001 km?

10. How many km/hr is 30 m/s?

11. How many ft/s is 60 mi/hr?

12. How many miles/hour is 30 km/s?

13. Change 2.6 km/day to m/week

14. Change 60 yds/ hours to inches/ seconds

15. Convert 1.7 Kg to eg

Using density as a conversion factor. Remember, 1 mL = 1 cm3. 1. What is the volume of a liquid with a density of 1.5 g/ml and a mass of 78g? (Hint: make sure your volume units are on the TOP in the setup, so they will be on top in the answer>)

2. What is the density of an object with a mass of 34g and a volume of 13 cm ?

3. What is the mass of an object with a density of 5.7 g/cm3 and a volume of 48 ml? (The density of Al is 2.70 g/cm3.) You will need to convert units too. 4. What is the volume of 0.810 grams of Al?

5. Find the mass in grams of 0.327 liters of Al.

6. Find the volume in liters of 16.2 kg Al.

KEY 1) 42.5 km 4) 0.01067km 7) 2700m 10)110km/hr 13) 18000 m/wk 2) 48.9 g 5) 17,000 ft 8) 63,400 ll)88ft/s 14)0.60 in/s 3) 5800days 6) 1.439 mi 9) 1,000mm 12)67,000 mi/hr 15) 170,000 eg C) Using density as a conversion factor. l . )52ml 2) 2.6 g/cm3 3 )270g 4. ) What is the volume of 0.810 grams of Al?

1 cm3 -x 0.810 g x = 0.300 cm3 (or 0.300 mL) 2.70g J 5. ) Find the mass in grams of 0.327 liters of Al.

_ T 1000 mL I cm3 2.70 g 0.327 L x x x —f - = 8 8 3 g 1 L ImL l cm 6. ) Find the volume in liters of 16.2 kg Al.

1000 g I cm3 ImL \L 16.2 g x x x x = 6.00 L

I kg 2.70 g \cm3 1000 mL

10

Balancing Chemical Equations (do on a separate paper)

1) N 2 + H 2 ^ NH 3

2) K C I O 3 •> KCI + 0 2

3) NaCI + F 2 NaF + Cl 2

4) H 2 + 0 2 -» H 2 0

5) Pb(OH)2 + HCI ^ H 2 0 + PbCI2

6) AIBr3 + K 2 S0 4 -> KBr + AI 2(S0 4) 3

7) CH 4 + 0 2 C0 2 + H 2 0

8) C 3 H 8 + 0 2 -> C0 2 + H 2 0

9) C 8 H i 8 + 0 2 -> C0 2 + H 2 0 10) FeCI3 + NaOH Fe(OH)3 + NaCI

11) P + 0 2 - » P 2 0 5

12) Na + H 2 0 - * NaOH + H 2

13) A g 2 0 ^ Ag+ 0 2

14) S 8 + 0 2 ^ S 0 3

15) C 0 2 + H 2 0 -» C 6 H 1 2 0 6 + 0 2

16) K + MgBr^ KBr + Mg

17) HCI + CaC0 3 -> CaCI2 + H 2 0 + C0 2

18) H 2 0 + 0 2 H 2 0 2

19) NaBr + CaF2 -» NaF + CaBr2

20) H2SO4 + NaN0 2 -» HN0 2 + Na 2S0 4

Baiancinq Chemical Equations - Answer Key 1) 1 N 2 + 3 H 2 ^ 2 N H 3

2) 2 KCI0 3 -> 2 KCI + 3 0 2

3) 2 NaCI + 1 F 2 -» 2 NaF + 1 Cl 2

4) 2 H 2 + 1 02 -> 2 H 2 0 5) 1 Pb(OH)2 + 2 HCI -» 2 H 2 0 + 1 PbCI2

6) 2 AIBr3 + 3 K 2 S0 4 6 KBr + 1 AI 2(S0 4) 3

7) 1 CH 4 + 2 0 2 -> 1 C0 2 + 2 H 2 0 8) 1 C 3H 8 + 5 0 2 -» 3 C0 2 + 4 H 2 0 9) 2 C 8 H 1 8 + 25 0 2 -> 1 6 C 0 2 + 18 H 2 0 10) 1 FeCI3 + 3 NaOH 1 Fe(OH)3 + 3 NaCI 11) 4 P + 5 0 2 ^ 2 P 2 0 5

12) 2Na + 2 H 2 0 ^ 2 N a O H + 1 H 2

13) 2 Ag 2 0 •» 4Ag + 1 0 2

14) 1 S 8 + 12 0 2 ^ 8 S 0 3

15) 6 C 0 2 + 6 H 2 0 -» 1 C 6 H 1 2 0 6 + 6 0 2

16) 1 K + 1 MgBr -> 1 KBr + 1 Mg 17) 2 HCI + 1 CaC0 3 -> 1 CaCI2 + 1 H 2 0 + 1 C0 2

18) 2 H 2 0 + 1 0 2 ^ 2 H 2 0 2

19) 2 NaBr + 1 CaF2 -> 2 NaF + 1 CaBr2

20) 1 H 2 S0 4 + 2 NaN0 2 ^ 2 HN0 2 + 1 Na 2 S0 4

Word Equations Write the word equations below as chemical equations and balance: 1) Zinc and lead (II) nitrate react to form zinc nitrate and lead.

2) Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas.

3) Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride.

4) Potassium metal and chlorine gas combine to form potassium chloride.

5) Aluminum and hydrochloric acid react to form aluminum chloride and hydrogen gas.

6) Calcium hydroxide and phosphoric acid react to form calcium phosphate and water.

7) Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide

8) Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.

Word Equations - Answer Kev

1) 1 Zn + 1 Pb(N0 3) 2 -» 1 Zn(N0 3) 2 + 1 Pb 2) 2 AIBr3 + 3 Cl 2 -> 2 AICI3 + 3 Br2

3) 2 Na 3P0 4 + 3 CaCI2 6 NaCI + 1 Ca 3(P0 4) 2

4) 2 K + 1 Cl 2 -> 2 KCI 5) 2 Al + 6 HCI -» 3 H 2 + 2 AICI3

6) 3 Ca(OH)2 + 2 H 3 P0 4 -> Ca 3(P0 4) 2 + 6 H 20 7) 1 Cu + 2 H 2 S0 4 -» 1 CuS0 4 + 2 H 20 + 1 S0 2

8) 2 H 2 + 2 NO -> 2 H 20 + 1 N 2

R