Multiple Choice
Identify the
choice that best completes the statement or answers the question.
|
|
|
1.
|
A chemical formula includes the symbols of the elements in the compound and
subscripts that indicate
a. | atomic mass of each element. | b. | number of atoms or ions of each element that
are combined in the compound. | c. | formula mass. | d. | charges on the
elements or ions. |
|
|
|
2.
|
A chemical formula for a molecular compound represents the composition of
a. | a molecule. | c. | the ions that make up the compound. | b. | an
atom. | d. | the crystal
lattice. |
|
|
|
3.
|
How many atoms of fluorine are present in a molecule of carbon tetrafluoride,
CF4?
|
|
|
4.
|
The formula for carbon dioxide, CO2, can represent
a. | one molecule of carbon dioxide. | b. | 1 mol of carbon dioxide
molecules. | c. | the combination of 1 atom of carbon and 2 atoms of oxygen. | d. | all of the
above. |
|
|
|
5.
|
What is the formula for zinc fluoride?
|
|
|
6.
|
What is the formula for the compound formed by calcium ions and chloride
ions?
a. | CaCl | c. | CaCl3 | b. | Ca2Cl | d. | CaCl2 |
|
|
|
7.
|
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 |
|
|
|
8.
|
What is the formula for aluminum sulfate?
a. | AlSO4 | c. | Al2(SO4)3 | b. | Al2SO4 | d. | Al(SO4)3 |
|
|
|
9.
|
What is the formula for barium hydroxide?
a. | BaOH | c. | Ba(OH)2 | b. | BaOH2 | d. | Ba(OH) |
|
|
|
10.
|
Name the compound Ni(ClO3)2.
a. | nickel(II) chlorate | c. | nickel(II) chlorite | b. | nickel(II) chloride | d. | nickel(II)
peroxide |
|
|
|
11.
|
Name the compound Zn3(PO4)2.
a. | zinc potassium oxide | c. | zinc phosphate | b. | trizinc polyoxide | d. | zinc phosphite |
|
|
|
12.
|
Name the compound KClO3.
a. | potassium chloride | c. | potassium chlorate | b. | potassium trioxychlorite | d. | hypochlorite |
|
|
|
13.
|
Name the compound Fe(NO3)2.
a. | iron(II) nitrate | c. | iron(III) nitrate | b. | iron(II) nitrite | d. | iron(III)
nitride |
|
|
|
14.
|
Name the compound Al2S3.
a. | aluminum sulfate | c. | aluminum(II) sulfate | b. | aluminum sulfur | d. | aluminum
sulfide |
|
|
|
15.
|
Name the compound CF4.
a. | calcium fluoride | c. | carbon tetrafluoride | b. | carbon fluoride | d. | monocalcium
quadrafluoride |
|
|
|
16.
|
Name the compound SiO2.
a. | silver oxide | c. | silicon dioxide | b. | silicon oxide | d. | monosilver
dioxide |
|
|
|
17.
|
Name the compound SO3.
a. | sulfur trioxide | c. | selenium trioxide | b. | silver trioxide | d. | sodium trioxide |
|
|
|
18.
|
Name the compound N2O3.
a. | dinitrogen oxide | c. | nitric oxide | b. | nitrogen trioxide | d. | dinitrogen
trioxide |
|
|
|
19.
|
What is the formula for silicon dioxide?
|
|
|
20.
|
What is the formula for dinitrogen trioxide?
|
|
|
21.
|
What is the formula for sulfur dichloride?
|
|
|
22.
|
What is the formula for diphosphorus pentoxide?
a. | P2PeO5 | c. | P2O4 | b. | PO5 | d. | P2O5 |
|
|
|
23.
|
What is the formula for hydrochloric acid?
|
|
|
24.
|
The oxidation number of fluorine is
a. | always 0. | b. | –1 in all compounds. | c. | +1 in all
compounds. | d. | equal to the negative charge of all the metal ions in a
compound. |
|
|
|
25.
|
What is the oxidation number of oxygen in most compounds?
|
|
|
26.
|
What is the oxidation number of a pure element?
|
|
|
27.
|
In a compound, the algebraic sum of the oxidation numbers of all atoms
equals
a. | 0. | c. | 8. | b. | 1. | d. | the charge on the
compound. |
|
|
|
28.
|
What is the oxidation number of hydrogen in compounds containing metals?
a. | –1 | c. | +1 | b. | 0 | d. | the charge on the metal
ion |
|
|
|
29.
|
In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is
equal to
a. | 0. | c. | 10. | b. | the number of atoms in the
ion. | d. | the charge of the
ion. |
|
|
|
30.
|
What is the oxidation number of oxygen in H2O2?
|
|
|
31.
|
What is the oxidation number of hydrogen in KH?
|
|
|
32.
|
What is the oxidation number of hydrogen in H2O?
|
|
|
33.
|
What is the oxidation number of sulfur in SO2?
|
|
|
34.
|
What is the oxidation number of sulfur in H2SO4?
|
|
|
35.
|
What is the oxidation number of oxygen in CO2?
|
|
|
36.
|
Name the compound N2O2 using the Stock system.
a. | dinitrogen monoxide | c. | nitrogen(II) oxide | b. | nitrogen dioxide | d. | nitrogen
oxide(II) |
|
|
|
37.
|
Name the compound SO2 using the Stock system.
a. | sulfur(II) oxide | c. | sulfur dioxide | b. | sulfur(IV) oxide | d. | sulfur oxide |
|
|
|
38.
|
Name the compound CCl4 using the Stock system.
a. | carbon(IV) chloride | c. | carbon chloride | b. | carbon tetrachloride | d. | carbon
hypochlorite |
|
|
|
39.
|
Name the compound H2O using the Stock system.
a. | water | c. | hydrogen(I) oxide | b. | hydrogen dioxide | d. | hydrogen(II)
oxide |
|
|
|
40.
|
Name the compound CO2 using the Stock system.
a. | carbon(IV) oxide | c. | monocarbon dioxide | b. | carbon dioxide | d. | carbon oxide |
|
|
|
41.
|
Name the compound PBr5 using the Stock system.
a. | potassium hexabromide | c. | phosphorus(V) bromide | b. | phosphorus(V)
pentabromide | d. | phosphoric
acid |
|
|
|
42.
|
The molar mass of an element is the mass of one
a. | atom of the element. | c. | gram of the element. | b. | crystal of the element. | d. | mole of the
element. |
|
|
|
43.
|
What is the sum of the atomic masses of all the atoms in a formula for a
compound?
a. | molecular mass | c. | atomic mass | b. | formula mass | d. | actual mass |
|
|
|
44.
|
What is the formula mass of magnesium chloride, MgCl2?
a. | 46 amu | c. | 95.21 amu | b. | 59.76 amu | d. | 106.35 amu |
|
|
|
45.
|
What is the formula mass of ethyl alcohol, C2H5OH?
a. | 30.33 amu | c. | 45.06 amu | b. | 33.27 amu | d. | 46.08 amu |
|
|
|
46.
|
What is the formula mass of (NH4)2SO4?
a. | 114.09 amu | c. | 128.06 amu | b. | 118.34 amu | d. | 132.16 amu |
|
|
|
47.
|
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 1 atom of Mg and 2
atoms of I. | d. | the sum of the masses of 1 atom of Mg and 1 atom of
I. |
|
|
|
48.
|
The molar mass of NO2 is 46.01 g/mol. How many moles of
NO2 are present in 114.95 g?
a. | 0.4003 mol | c. | 2.498 mol | b. | 1.000 mol | d. | 114.95 mol |
|
|
|
49.
|
The molar mass of CCl4 is 153.81 g/mol. How many grams of
CCl4 are needed to have 5.000 mol?
a. | 5 g | c. | 769.0 g | b. | 30.76 g | d. | 796.05 g |
|
|
|
50.
|
The molar mass of H2O is 18.02 g/mol. How many grams of
H2O are present in 0.20 mol?
a. | 0.2 g | c. | 35.9 g | b. | 3.6 g | d. | 89.9 g |
|
|
|
51.
|
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 |
|
|
|
52.
|
The molar mass of CS2 is 76.15 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. | 761.5 g |
|
|
|
53.
|
The molar mass of NH3 is 17.03 g/mol. How many moles of
NH3 are present in 107.1 g?
a. | 0.1623 mol | c. | 6.289 mol | b. | 3.614 mol | d. | 107.1 mol |
|
|
|
54.
|
What is the mass of 0.240 mol glucose,
C6H12O6?
a. | 24.0 g | c. | 180.16 g | b. | 43.2 g | d. | 750. g |
|
|
|
55.
|
How many Cl– ions are present in 2.00 mol of KCl?
a. | 1.20  1024 | c. | 2.00 | b. | 6.02 
1024 | d. | 0.5 |
|
|
|
56.
|
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 |
|
|
|
57.
|
How many oxygen atoms are there in 0.500 mol of CO2?
a. | 6.02 
1023 | c. | 15.9994 | b. | 3.01 
1023 | d. | 11.0 |
|
|
|
58.
|
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 |
|
|
|
59.
|
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 |
|
|
|
60.
|
How many molecules are there in 5.0 g of methyl alcohol,
CH3OH?
a. | 9.4  1022 | c. | 3.6 
1024 | b. | 3.0  1024 | d. | 3.8 
1024 |
|
|
|
61.
|
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 |
|
|
|
62.
|
What is the percentage composition of CO?
a. | 50% C, 50% O | c. | 25% C, 75% O | b. | 12% C, 88% O | d. | 43% C, 57% O |
|
|
|
63.
|
What is the percentage composition of CuCl2?
a. | 33% Cu, 66% Cl | c. | 65.50% Cu, 34.50% Cl | b. | 50% Cu, 50% Cl | d. | 47.27% Cu, 52.73%
Cl |
|
|
|
64.
|
The percentage composition of sulfur in SO2 is about 50%. What is the
percentage of oxygen in this compound?
|
|
|
65.
|
What is the mass percentage of OH– in
Ca(OH)2?
a. | 45.9% | c. | 75% | b. | 66.6% | d. | 90.1% |
|
|
|
66.
|
What is the mass percentage of chlorine in NaCl?
a. | 35.45% | c. | 60.7% | b. | 50% | d. | 64.5% |
|
|
|
67.
|
A formula that shows the simplest whole-number ratio of the atoms in a compound
is the
a. | molecular formula. | c. | experimental formula. | b. | ideal
formula. | d. | empirical
formula. |
|
|
|
68.
|
The empirical formula is always the accepted formula for a(n)
a. | atom. | c. | molecular compound. | b. | molecule. | d. | ionic compound. |
|
|
|
69.
|
The empirical formula for a compound shows the symbols of the elements with
subscripts indicating the
a. | actual numbers of atoms in a molecule. | b. | number of moles of the compound in 100
g. | c. | smallest whole-number ratio of the atoms. | d. | atomic masses of
each element. |
|
|
|
70.
|
The empirical formula may not represent the actual composition of a unit of
a(n)
a. | ionic compound. | c. | salt. | b. | molecular compound. | d. | crystal. |
|
|
|
71.
|
What is the empirical formula for a compound that is 31.9% potassium, 28.9%
chlorine, and 39.2% oxygen?
a. | KClO2 | c. | K2Cl2O3 | b. | KClO3 | d. | K2Cl2O5 |
|
|
|
72.
|
What is the empirical formula for a compound that is 43.6% phosphorus and 56.4%
oxygen?
|
|
|
73.
|
What is the empirical formula for a compound that is 53.3% O and 46.7%
Si?
|
|
|
74.
|
A compound contains 259.2 g of F and 40.8 g of C. What is the empirical formula
for this compound?
|
|
|
75.
|
A compound contains 64 g of O and 8 g of H. What is the empirical formula for
this compound?
|
|
|
76.
|
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 |
|
|
|
77.
|
A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula
for this compound?
|
|
|
78.
|
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. |
|
|
|
79.
|
A molecular compound has the empirical formula XY3. Which of the
following is a possible molecular formula?
|
|
|
80.
|
The molecular formula for vitamin C is C6H8O6.
What is the empirical formula?
a. | CHO | c. | C3H4O3 | b. | CH2O | d. | C2H4O2 |
|
|
|
81.
|
Of the following molecular formulas for hydrocarbons, which is an empirical
formula?
|
|
|
82.
|
Which of the following molecular formulas does not have the corresponding
empirical formula XY2Z?
a. | X2Y4Z2 | c. | X6Y12Z6 | b. | XYZ | d. | X3Y6Z3 |
|
|
|
83.
|
A compound's empirical formula is C2H5. If the
formula mass is 58 amu, what is the molecular formula?
a. | C3H6 | c. | C5H8 | b. | C4H10 | d. | C5H15 |
|
|
|
84.
|
A compound's empirical formula is N2O5. If the
formula mass is 108 amu, what is the molecular formula?
|
|
|
85.
|
A compound's empirical formula is CH. If the formula mass is 26 amu, what
is the molecular formula?
|
|
|
86.
|
A compound's empirical formula is NO2. If the formula mass is 92
amu, what is the molecular formula?
|
|
|
87.
|
A compound's empirical formula is CH3. If the formula mass is 30
amu, what is the molecular formula?
|
|
|
88.
|
A compound's empirical formula is HO. If the formula mass is 34 amu, what
is the molecular formula?
|
|
|
89.
|
What is the molecular formula of a compound that has a formula mass of 50.48 amu
and an empirical formula of CH3Cl?
a. | CHCl | c. | CH3Cl | b. | CH2Cl | d. | CH2Cl2 |
|
Short Answer
|
|
|
90.
|
What type of compound cannot be represented by a molecular formula? Explain your
answer.
|
Problem
|
|
|
91.
|
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.
|
|
|
92.
|
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.
|
|
|
93.
|
The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.08 g/mol,
and the molar mass of oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate,
Fe2SiO4.
|
|
|
94.
|
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.
|
Completion
Complete each
statement.
|
|
|
95.
|
The name and formula for the compound formed by strontium ions and sulfite ions
are ____________________.
|
|
|
96.
|
The Stock name for the compound P2O5 is
____________________.
|
|
|
97.
|
The name for the  ion is ____________________.
|
|
|
98.
|
The oxidation numbers for each atom in  are
____________________.
|
|
|
99.
|
The oxidation numbers for each atom in H2CO3 are
____________________.
|
Essay
|
|
|
100.
|
HO and H2O2 are examples of the empirical and molecular
formula of a compound, respectively. Explain the relationship between these two types of
formulas.
|