Name: __________________________ Date: _____________
1. Find the density of gold in kg/m3, if 5.98 g of pure gold occupies a volume of 0.310 cm3.
A)
B)
C)
D)
E)
1.93 x 104
19.3
0.0193
1.93 x 106
1.93 x 103
2. Sulfur and fluorine combine to form two different binary compounds. In the first
compound, 1.87 g of sulfur combines with 4.43 g of fluorine. In the second compound,
1.25 g of sulfur combines with 4.45 g of fluorine. If the formula of the first compound is
SF4, what is the formula of the second compound?
A)
B)
C)
D)
E)
SF6
SF3
SF5
SF2
SF9
3. Magnesium has 3 stable isotopes (Mg-24, Mg-25 and Mg-26) with masses of 23.98504
amu, 24.98584 amu, and 25.98259 amu, respectively. The natural abundance of Mg-25
is 10.1 %. What are the percentages of the other two isotopes?
A)
B)
C)
D)
E)
78.7% and 11.2%
50.0 % and 50.0 %
44.9% and 44.9%
83.6% and 16.4%
78.9% and 21.1%
4. A 200.0 g sample of pure MgCl2 contains:
A)
B)
C)
D)
E)
24
1.265 × 10 molecules of MgCl2
95.211 molecules of MgCl2
2.101 molecules of MgCl2
26
1.204 × 10 molecules of MgCl2
25
5.734 × 10 molecules of MgCl2
Page 1
5. What is the correct name of Co(IO3)2 compound?
A)
B)
C)
D)
E)
Cobalt(II) iodate
Cobalt di-iodate
Cobalt di-iodine hexa-oxide
Mono cobalt di-iodate
Cobalt(IV) iodate
6. The formula of ferrocene is Fe(C5H5)x. What is the value of x in the formula of
ferrocene, if 2.33 g of C5H5 are required for every 1.00 g of Fe?
A)
B)
C)
D)
E)
2
1
3
4
5
7. In which one of the following species does the bromine atom (Br) have an oxidation
number of 5?
A)
B)
C)
D)
E)
HBrO3
HBr
HBrO
HBrO4
BrF3
8. Based on the solubility rules, which one of these compounds should be soluble in water?
A)
B)
C)
D)
E)
K2SO4
Ni(OH)2
FeCO3
PbS
AgCl
Page 2
9. Identify the reducing agent in the following reaction:
2 NO2(g) + 7 H2(g) → 2 NH3(g) + 4 H2O(g)
A)
B)
C)
D)
E)
H2
NO2
NH3
H2O
There is no reducing agent.
10. Calculate the standard enthalpy of formation of liquid methanol, CH3OH(l), using the
following information:
Cgraphite + O2 (g)  CO2 (g)
ΔH° = –393.5 kJ/mol
H2 (g) + (1/2) O2 (g)  H2O (l)
ΔH° = –285.8 kJ/mol
CH3OH (l) + (3/2) O2 (g)  CO2 (g) + 2H2O (l)
ΔH° = –726.4 kJ/mol
A)
B)
C)
D)
E)
–238.7 kJ/mol
–1691.5 kJ/mol
1691.5 kJ/mol
47.1 kJ/mol
–47.1 kJ/mol
11. As a system increases in volume, it absorbs 52.5 J of energy in the form of heat from the
surroundings. The piston is working against pressure of 0.500 atm. The final volume
of the system is 58.0 L. What was the initial volume of the system if the internal
energy of the system is decreased by 102.5 J ? (1L· atm = 101.3 J)
A)
B)
C)
D)
E)
54.9 L
3.06 L
61.1 L
52.5 L
48.8 L
Page 3
12. How much energy (heat) is required to convert 52.0 g of ice at –10.0°C to
steam at 100°C?
specific heat of ice:
2.09 J/g·°C
Hfus = 6.02 kJ/mol
specific heat of water:
4.18 J/g·°C
Hvap = 40.7 kJ/mol
A)
B)
C)
D)
E)
157.8 kJ
40.20 kJ
1.086 x 103 kJ
2.570 x 103 kJ
2.296 x 103 kJ
13. Which one of the following statements about Bohr's model of the hydrogen atom is
correct?
A) The smaller the orbit, the lower the energy of the electron.
B) The radius of an orbit is inversely proportional to the quantum number n.
C) A photon is emitted when the electron moves from the ground state to an excited
state.
D) An electron can absorbed or emit energy at any quantity.
E) When the electron moves from n=2 to n=1, it emits radiation in the visible region.
14. Arrange the following elements in order of increasing ionization energy: Cs, Sc,
Mn.
A)
B)
C)
D)
E)
Cs < Sc < Mn
Sc < Mn < Cs
Sc < Cs < Mn
Cs < Mn < Sc
Mn < Cs < Sc
15. The ion represented as 48 Ti 4+ has:
22
A)
B)
C)
D)
E)
no 4s electrons
22 total electrons
48 total neutrons
26 total protons
four 3d electrons
Page 4
16. Which one of these molecules would have the greatest percent ionic character?
I.
A)
B)
C)
D)
E)
CO2 ;
II. NaF ;
III SO3 ;
IV HF
V. NF3
II
I
IV
V
III
17. The hybridization of I in ICl2– is expected to be
A)
B)
C)
D)
E)
sp3d
sp3d2
sp3
sp2
sp
18. According to Molecular Orbital Theory, two separate px orbitals (head-to-head) interact
along the x-axis to form what molecular orbitals?
A)
B)
C)
D)
E)
 and *
, *, and 
 and *
, *, , and *
, * and 
19. Which one of the following correctly lists species in order of increasing bond length?
A)
B)
C)
D)
E)
C2– < C2 < C2+
C2 < C2+ < C2–
C2– < C2+ < C2
C2+ < C2 < C2–
C2+ < C2– < C2
Page 5
20. A pure substance A is found to decompose upon heating into two new, pure substances,
B and C.
ABC
Neither B nor C can be decomposed by chemical means. From this we may conclude
that ________.
A)
B)
C)
D)
E)
B and C are elements, A is a compound
A is an element, B and C are compounds
B is a compound, A and C are elements
A, B, and C are all elements
A, B, and C are all compounds
21. Using the following portion of the activity series for oxidation half reactions (Note: ease
of oxidation increases from bottom to top)
Ca(s) → Ca2+(aq) + 2eMg(s) → Mg2+(aq) + 2eZn(s) → Zn2+(aq) + 2eCu(s) → Cu2+(aq) + 2edetermine which reaction(s) will not occur.
I. Ca(s) with Cu2+(aq)
II. Ca(s) with Zn2+(aq)
III. Zn(s) with Cu2+(aq)
IV Zn(s) with Mg2+(aq)
A)
B)
C)
D)
E)
IV only
I, II and III only
II and III only
All of them
III only
22. The intermolecular forces present in CO include which of the following?
I. dipole-dipole
II. ion-dipole
III. dispersion IV. hydrogen bonding
A)
B)
C)
D)
E)
I and III
I, II, III, and IV
I, III, and IV
I and II
II and IV
Page 6
23. Lithium oxide is an effective substance which is being used to remove carbon dioxide
from the environment according to this reaction: Li2O(aq) + CO2(g) → Li2CO3(s)
What volume of carbon dioxide can be absorbed by 1.00 kg of lithium oxide at 25°C
and 1.00 atm?
A)
B)
C)
D)
E)
819 L
687 mL
819 mL
687 L
22.4 L
24. If 250 mL of methane, CH4, effuses through a small hole in 28s, the time required for
the same volume of helium to pass through the hole under the same conditions will be
A)
B)
C)
D)
E)
14 s
7.0 s
1.8 s
56 s
110 s
25. A 19.3-g mixture of oxygen and argon is found to occupy a volume of 16.2 L when
measured at 675.9 mmHg and 43.4oC. What is the partial pressure of oxygen in this
mixture?
A)
B)
C)
D)
E)
436 mmHg
401 mmHg
338 mmHg
274 mmHg
239 mmHg
26. A 0.335-g sample of an unknown gas occupies a volume of 0.107 L at STP. What is the
molecular formula of the gas?
A)
B)
C)
D)
E)
C5H10
C6H12
C7H14
C6H14
C4H8
Page 7
27. PH3 gas is most likely to approach the ideal behavior at
A)
B)
C)
D)
E)
0.10 atm and 100°C.
5.0 atm and 100°C.
10 atm and 100°C.
1.0 atm and 0°C.
0.10 atm and –100°C
28. A sample of methane, CH4, occupies a volume of 170.0 mL at 25°C and exerts a
pressure of 965.0 mmHg. If the volume of the gas is allowed to expand to 720.0 mL at
298 K, what will be the pressure of the gas?
A)
B)
C)
D)
E)
227.8 torr
4090. torr
2720. torr
0.008823 torr
550.0 torr
29. How many unpaired electrons does arsenic (As) in its ground state have?
A)
B)
C)
D)
E)
3
4
0
1
2
30. Use the bond enthalpy data given below to estimate the heat released when 50.0 g of
propane gas, C3H8, burns in excess oxygen to yield carbon dioxide and water
vapor at 25°C.
BE(C–C) = 347 kJ/mol
BE(C=O in CO2) = 799 kJ/mol
BE(C–H) = 414 kJ/mol
BE(O–H) = 460 kJ/mol
BE(O=O) = 498.7 kJ/mol
A)
B)
C)
D)
E)
2240 kJ
1360 kJ
1540 kJ
1970 kJ
2370 kJ
Page 8
31. A solution made by dissolving 20.2 mg of sugar in 100 mL of water has an osmotic
pressure of 15.5 mmHg at 25 ºC. Calculate the molar mass of that sugar in g/mol.
A)
B)
C)
D)
E)
242
2.42 x 105
302
318
3.18 x 105
32. Calculate the Henry’s law constant (in mol/L·atm) for O2 in 0.50 L water at 25 ºC, when
3.4 x 10-2 mole of O2 created a pressure of 26 atm over the solution.
A)
B)
C)
D)
E)
2.6 x 10-3
1.3 x 10-3
1.3 x 10-5
8.8 x 10-3
8.8 x 105
33. What is the attractive force between like molecules accounting for capillary actions?
A)
B)
C)
D)
E)
Cohesion
Surface tension
Adhesion
Polarity
Viscosity
34. Determine the molality (m) of an aqueous solution that is 5.5 % NaCl by mass.
A)
B)
C)
D)
E)
1.0 m
9.4 m
0.058 m
5.8 x 10-4 m
0.51 m
Page 9
35. What mass of sodium chloride must be added to 2525 g of water to raise the boiling
point to 105.5 ºC? (Kb = 0.52 ºC/m for water, assume no ion pairing)
A)
B)
C)
D)
E)
780.5 g
390.0 g
1570. g
7800. g
3900. g
36. Which of the following pairs are more likely to form a solution?
A)
B)
C)
D)
E)
chloroform (CHCl3) and acetone (CH3COCH3)
water and octane (C8H18)
methanol (CH3OH) and hexane (C6H14)
water and ethane (C2H6)
ethanol (C2H5OH) and heptane (C7H16)
37. A compound has a vapor pressure of 400. mmHg at 17.9C and a normal boiling point
of 34.6C. What is the heat of vaporization for that compound in kJ/mol?
A)
B)
C)
D)
E)
28.6
67.4
45.3
85.2
122
38. You are given a small bar of an unknown metal, M. You find the density of the metal
to be 10.5 g/cm3. An X-ray diffraction experiment measures the edge of the unit cell
as 409 pm. Assuming that the metal crystallizes in a face-centered cubic lattice, what is
M most likely to be?
A)
B)
C)
D)
E)
Ag
Rh
Pt
Pb
Nb
Page 10
39. Consider the following phase diagram and identify the process occurring as the
substance goes from point C to point D.
A)
B)
C)
D)
E)
Increasing temperature with a phase change from solid to vapour
Increasing temperature with a phase change from liquid to vapour
Increasing temperature with no phase change
Increasing temperature beyond the critical point
Increasing temperature with a phase change from solid to liquid
40. Which one of the following liquids would have the lowest viscosity at 25°C?
H2C
CH2
O
CH2
H2C
CH2
I
A)
B)
C)
D)
E)
H2C
CH2
HN
H2C
CH2
CH2 H2C
H2C
CH2
CH2
III
III
II
I
IV
V
Page 11
CH2
CH2 HN
H2C
II
H2C
PH
H2C
CH2
IV
H2C
C
HN
H2C
C
V
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
Page 12