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Chapter 7 Review

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____ 1. What is the formula for the compound formed by lead(II) ions and chromate ions?

a.

PbCrO4

c.

Pb2(CrO4)3

b.

Pb2CrO4

d.

Pb(CrO4)2

____ 2. What is the formula for tin(IV) chromate?

a.

Sn(CrO4)4

c.

Sn2(CrO4)4

b.

Sn2(CrO4)2

d.

Sn(CrO4)2

____ 3. What is the formula for barium hydroxide?

a.

BaOH

c.

Ba(OH)2

b.

BaOH2

d.

Ba(OH)

____ 4. Name the compound Zn3(PO4)2.

a.

zinc potassium oxide

c.

zinc phosphate

b.

trizinc polyoxide

d.

zinc phosphite

____ 5. Name the compound Hg2(NO3)2.

a.

mercury(II) nitrate

c.

mercury(I) nitrate

b.

dimercury dinitrate

d.

mercuric nitrate

____ 6. Name the compound CuCO3.

a.

copper(I) carbonate

c.

cuprous carbide

b.

cupric trioxycarbide

d.

copper(II) carbonate

____ 7. Name the compound SiO2.

a.

silver oxide

c.

silicon dioxide

b.

silicon oxide

d.

monosilicon dioxide

____ 8. Name the compound N2O4.

a.

sodium tetroxide

c.

nitrous oxide

b.

dinitrogen tetroxide

d.

binitrogen oxide

____ 9. Name the compound SO3.

a.

sulfur trioxide

c.

selenium trioxide

b.

silver trioxide

d.

sodium trioxide

____ 10. Which compound's name includes the Greek numerical prefixes di- and tri-?

a.

Fe2O3

c.

N2O3

b.

Ca3(PO4)2

d.

Al2S3

____ 11. What is the formula for nitrogen trifluoride?

a.

NiF3

c.

N3F

b.

NF3

d.

Ni3F

____ 12. What is the formula for dinitrogen trioxide?

a.

Ni2O3

c.

N2O6

b.

NO3

d.

N2O3

____ 13. What is the formula for diphosphorous pentoxide?

a.

P2PeO5

c.

P2O4

b.

PO5

d.

P2O5

____ 14. What is the formula for carbon disulfide?

a.

CaS2

c.

S2C

b.

CS2

d.

SC2

____ 15. The oxidation number of fluorine is

a.

always 0.

b.

1 in all compounds

c.

+1 in all compounds.

d.

equal to the positive charge of all the metal ions in a compound.

____ 16. What is the oxidation number of oxygen in most compounds?

a.

8

c.

0

b.

2

d.

+1

____ 17. What is the oxidation number of an uncombined element?

a.

1

c.

+1

b.

0

d.

8

____ 18. What is the oxidation number of hydrogen in most compounds?

a.

1

b.

0

c.

+1

d.

It is equal to the algebraic sum of the oxidation numbers of the nonmetals.

____ 19. What is the oxidation number of hydrogen in KH?

a.

1

c.

+1

b.

0

d.

+2

____ 20. What is the oxidation number of hydrogen in H2O?

a.

0

c.

+2

b.

+1

d.

+3

____ 21. What is the oxidation number of sulfur in SO2?

a.

0

c.

+2

b.

+1

d.

+4

____ 22. Name the compound N2O2 using the Stock system.

a.

dinitrogen monoxide

c.

nitrogen(II) oxide

b.

nitrous oxide

d.

nitrogen oxide(II)

____ 23. Name the compound CCl4 using the Stock system.

a.

carbon(IV) chloride

c.

carbon chloride

b.

carbon tetrachloride

d.

carbon hypochlorite

____ 24. Name the compound H2O using the Stock system.

a.

water

c.

hydrogen(I) oxide

b.

hydrogen dioxide

d.

hydrogen(II) oxide

____ 25. Name the compound N2O5 using the Stock system.

a.

nitrogen(II) oxide

c.

nitrogen(VII) oxide

b.

nitrogen(V) oxide

d.

nitrogen pentoxide

____ 26. Name the compound PBr5 using the Stock system.

a.

potassium hexabromide

c.

phosphorus(V) bromide

b.

phosphorus(V) pentabromide

d.

phosphoric acid

____ 27. The molar mass of an element is the mass of one

a.

atom of the element.

c.

gram of the element.

b.

liter of the element.

d.

mole of the element.

____ 28. What is the formula mass of ethyl alcohol, C2H5OH?

a.

30.328 amu

c.

45.061 amu

b.

33.271 amu

d.

46.069 amu

____ 29. What is the formula mass of (NH4)2SO4?

a.

114.09 amu

c.

128.06 amu

b.

118.34 amu

d.

132.13 amu

____ 30. The molar mass of MgI2 is

a.

the sum of the masses of 1 mol of Mg and 2 mol of I.

b.

the sum of the masses of 1 mol of Mg and 1 mol of I.

c.

the sum of the masses of 2 mol of Mg and 2 mol of I.

d.

impossible to calculate.

____ 31. The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37 g?

a.

0.3998 mol

c.

2.500 mol

b.

1.333 mol

d.

36.32 mol

____ 32. The molar mass of CS2 is 76.14 g/mol. How many grams of CS2 are present in 10.00 mol?

a.

0.13 g

c.

10.00 g

b.

7.614 g

d.

761.4 g

____ 33. How many OH ions are present in 3.00 mol of Ca(OH)2?

a.

3.00

c.

3.61 1024

b.

6.00

d.

2.06 1023

____ 34. How many Mg2+ ions are found in 1.00 mol of MgO?

a.

3.01 1023

c.

12.04 1023

b.

6.02 1023

d.

6.02 1025

____ 35. If 0.500 mol of Na+ combines with 0.500 mol of Cl to form NaCl, how many formula units of NaCl are present?

a.

3.01 1023

c.

6.02 1024

b.

6.02 1023

d.

1

____ 36. What is the percentage composition of CF4?

a.

20% C, 80% F

c.

16.8% C, 83.2% F

b.

13.6% C, 86.4% F

d.

81% C, 19% F

____ 37. The percentage composition of sulfur in SO2 is about 50%. What is the percentage of oxygen in this compound?

a.

25%

c.

75%

b.

50%

d.

90%

____ 38. What is the percentage composition of chlorine in NaCl?

a.

35.45%

c.

60.7%

b.

50%

d.

64.5%

____ 39. A formula that shows the simplest whole-number ratio of the atoms in a compound is the

a.

molecular formula.

c.

structural formula.

b.

ideal formula.

d.

empirical formula.

____ 40. What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen?

a.

P3O7

c.

P2O3

b.

PO3

d.

P2O5

____ 41. What is the empirical formula for a compound that is 7.9% Li and 92.1% Br?

a.

LiBr

c.

LiBr3

b.

LiBr2

d.

LiBr4

____ 42. A compound contains 64 g of O and 4 g of H. What is the empirical formula for this compound?

a.

H2O

c.

HO2

b.

H2O2

d.

HO

____ 43. What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl?

a.

CaCl

c.

CaCl2

b.

Ca2Cl

d.

Ca2Cl2

____ 44. To find the molecular formula from the empirical formula, one must determine the compound's

a.

density.

c.

structural formula.

b.

formula mass.

d.

crystal lattice.

____ 45. The empirical formula and the formula mass of a compound are needed to determine the compound's

a.

molecular formula.

c.

lattice structure.

b.

bond energy.

d.

toxicity.

____ 46. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?

a.

CHO

c.

C3H4O3

b.

CH2O

d.

C2H4O2

____ 47. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?

a.

N2O5

c.

NO3

b.

N4O10

d.

N2O4

____ 48. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?

a.

NO

c.

NO4

b.

N2O2

d.

N2O4

____ 49. A compound's empirical formula is HO. If the formula mass is 34 amu, what is the molecular formula?

a.

H2O

c.

HO3

b.

H2O2

d.

H2O3

Short Answer

50. Explain the term empirical formula. What is the empirical formula of strontium bromide, SrBr2?

Problem

51. The molar mass of aluminum is 26.98 g/mol and the molar mass of fluorine is 19.00 g/mol. Calculate the molar mass of aluminum trifluoride, AlF3.

52. The molar mass of copper is 63.55 g/mol, the molar mass of sulfur is 32.07 g/mol, and the molar mass of oxygen is 16.00 g/mol. Calculate the molar mass of copper(II) sulfate, CuSO4.

53. The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.09 g/mol, and the molar mass of oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate, Fe2SiO4.

54. The molar mass of aluminum is 26.98 g/mol and the molar mass of oxygen is 16.00 g/mol. Determine the molar mass of Al2O3.


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