chem 047 –final review practice problems

1 Chem 047 –Final Review practice problems

Chemistry 047 Final Review Example Problems – (not all types of problems are

covered here!)

1. Scientific notation

a) 6.7

b) 0.0000002

c) 2005000

d) 71 × 103

e) 33 × 10−3

Write in standard notation f) 2.66 × 104

g) 1.5 × 10−2

2. Convert metric to metric

a) 7.2 cm = ____________ mm

b) 400 cm = ___________ m

c) 1.8 m = ______________ cm

d) 306.5 mm = ___________ m

e) 1528.2 g = ____________ kg

f) 3.63 kg = ______________ g

g) 923.6 ml = _____________ L

h) 5.86 L = ________________ ml

i) 5.46m3= ________________L

j) 25.2L = _________________m3

k) 232cm3 = _______________ml


3. Convert between oF, oC, K (use conversion formulas from data sheet)

a) 253 Kelvin to Celsius

b) 17.8 Celsius to Kelvin

c) -89.5 Fahrenheit to Celsius

d) Convert 37.8 Fahrenheit to Kelvin

4. Significant figures

a) What are the rules for sig figs? Include ones for =,-,*, and ÷

How many significant figures in each of the following?

b) 1234 _____

c) 0.023 _____

d) 890 _____

e) 91010 _____

f) 9010.0 _____


g) 1090.0010 _____

h) 0.00120 _____

i) 3.4 x 104 _____

j) 9.0 x 10-3 _____

k) 9.010 x 10-2 _____

l) 0.00030 _____

m) 1020010 _____

n) 780. _____

5. Density

a) Calculate the mass of a liquid with a density of 3.2 g/mL and a volume of 25 mL.

b) An irregular object with a mass of 18 kg displaces 2.5 L of water when placed in a large overflow container. Calculate the density of the object.

c) A graduated cylinder has a mass of 80. g when empty. When 20. mL of water is added, the graduated cylinder has a mass of 100. g. If a stone is added to the graduated cylinder, the water level rises to 45 mL and the total mass is now 156 g. What is the density of the stone?


d) A substance has a density of 5.83 g/cm3. If a piece of this substance weighing 9.2g is

dropped into a graduated cylinder of water containing 62.0ml, what will be the new

volume?

6. Physical states

If a substance has a melting point of 103oC and a boiling point of 152oC. What would

its physical state be at 125oC?

If you know the order of states (solidliquid gas) you can always figure out these

questions!

7. Physical and chem properties and changes

Classify each of the following as a chemical or physical change or chemical or physical

property:

1. _____ Heat conductivity 8. _____ Combustible

2. _____ Silver tarnishing 9. _____ Water freezing

3. _____ baking bread 10. _____ Wood burning

4. _____ magnetizing steel 11. _____ Milk souring

5. _____ length of metal object 12. _____ Brittleness

6. _____ shortening melting

7. _____ exploding dynamite

8. Classify between elements, molecules, compounds, mixtures

1. Sand 2. Salt 3. Pure Water

4. Soil 5. Sugar Water 6. Air

7. Carbon Dioxide 8. Gold 9. Brass

10. Oxygen 11. Italian Salad Dressing 12. Salt Water


13. Raisin Bran 14. Silver 15. Lithium Iodide


9. Nomenclature

1. Potassium dichromate

2. Lithium sulfide

3. Potassium bromide

4. Cesium iodide

5. Calcium phosphide

6. Sodium fluoride

7. Strontium oxide

8. Beryllium sulfide

9. Magnesium bromide

10. Lithium oxide

11. Strontium chloride

12. Barium bromide

13. Magnesium sulfide

14. Magnesium iodide

15. Hydrofluoric acid

16. Barium phosphide

17. Sodium phosphate

18. Potassium chloride

19. Lithium nitride

20. Calcium sulfide

21. Rubidium oxide

22. Strontium nitride

23. Cesium phosphide

24. Magnesium carbonate

25. Beryllium sulfate

26. Dinitrogen Tetroxide

27. Carbon dioxide

29. Hydroiodic acid

30. Iodic acid

33. Phosphorus pentachloride

34. Iodine monochloride

35. Antimony (III) fluoride

36. Bromine monofluoride

37. Bromine dioxide

38. Dinitrogen pentoxide

39. Carbon monosulfide

40. Tellurium dioxide

41. Phosphorus tribromide

42. Carbon tetraiodide

43. Vanadium (V) chromate

44. Zinc carbonate

45. Silver hydroxide

46. Vanadium (III) chromate

47. Mercury (II) iodide

48. Uranium (V) nitrate

49. Nickel (III) nitride

50. Sulfuric acid

51. ScCl3

52. HCl(aq)

53. PtO2

54. Sb(ClO3)5

55. GeS2

56. ZnO

57. VSO4


58. CuCl2

59. TiO2

60. NiN

61. Ni3(PO4)2

62. CoF3

63. Au2O3

64. Zn3P2

65. Cr(NO3)6

67. NaIO3

68. NaI

69. H2SO3 (aq)

70. H2CO3 (aq)

71. AlN

72. AlH3

73. Li3AsO4

74. NaCN

75. Na2O2

76. Li3PO3

77. KHCO3

78. HF(aq)

79. AuI2

80. KMnO4

81. Na2Cr2O7

82. Ag2CrO4

83. AgCl

85. RaF2

86. KSCN

87. FeS

88. Fe2(SO3)3

89. FeSO4

90. MgS

92. RbCl

93. Cu(OH)2

94. Mg3N2

95. Cu3N

96. LiH

97. K2O

98. K2O2

99. Li3N

100. CBr4

101. N2O5

102. NCl3

103. PCl3


10. Calculate Molar Mass

BF3

CCl2F2

Mg(OH)2

11. To 18. On Final Review List

Refer to previous practice worksheets…

19. Info on Atoms

Name Symbol Atomic # Mass # # Protons # Neutrons # Electrons

Al+3 14

Iron

ion

56 24

15 16 18

F-1 19

Name Symbol Atomic # Mass # # Protons # Neutrons # Electrons

Selenium 45

222 86

118 79

11

12


20. What is an isotope?

21. Electron configurations –do some of the shorter ones as full configurations for

practice, and the rest as abbreviated.

a. Boron

b. Silicon

c. Sulfur

d. Calcium

e. Rubidium

f. Chromium

g. Gallium

h. Neon

i. Vanadium

j. Copper

22. Periodic Table Trends

For each of the following sets of atoms, rank the atoms from smallest to largest atomic radius.

a. C, Li, F b. Na, Li, K c. O, Ge, P d. Si, C, N e. Ar, Cl, Br

For each of the following sets of atoms, rank them from lowest to highest ionization energy.

a. Mg, Si, S b. Mg, Ba, Ca c. F, Br, Cl d. Ne, Cu, Ba e. N, Si, P


For each of the following sets of atoms, rank them from lowest to highest electronegativity.

a. N, C, Li b. Ne, O, C c. O, P, Si d. Mg, K, P e. F, S, He

23. Valence electrons and unpaired electrons

For each of the following how many valence electrons and unpaired electrons available

for bonding:

a. Si

b. Mg

c. Se

d. Pb2+

24. Lewis Dot Diagrams

a. Magnesium sulfide

b. Calcium fluoride

c. Potassium oxide

d. Na3N


e. Ca3P2

f. H2S

g. NH4+

h. PO43-

i. SiO2

25. Conjugate acid/base pairs

Find the reactant that is the conjugate pair of each product:

a) HClO4(aq) + H2O(l) ⇄ H3O+(aq) + ClO4–(aq)

b) H2SO3(aq) + H2O(l) ⇄ H3O+(aq) + HSO3–(aq)

c) HC2H3O2(aq) + H2O(l) ⇄ H3O+(aq) + C2H3O2–(aq)

d) H2S(g) + H2O(l) ⇄ H3O+(aq) + HS–(aq)


e) HSO3–(aq) + H2O(l) ⇄ H3O+(aq) + SO32–(aq)

f) NH3(g) + H2O(l) ⇄ NH4+(aq) + OH–(aq)

g) HF(aq) + HSO3–(aq) ⇄ F–(aq) + H2SO3(aq)

h) HNO2(aq) + HS–(aq) ⇄ NO2–(aq) + H2S(aq)

How many Hydrogen ions are accepted or donated in each case? Can you accept or donate more than this number and still be considered a conjugate acid/base pair?

26. Solution stoichiometry and molarity questions

Refer to past practice worksheets and problems.

27. Calculate concentration of ions in solution

Refer to past practice worksheets and problems.

chem 047 –final review practice problems

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