Name: ____________________
Mock Exam 3A
Multiple choice (5 percent each, no partial credit)
1. It takes 233.5 J of energy to raise the
temperature of 13.00 g of an unknown
metal by 40.00 °C. What is the identity of
the metal?
a. Cobalt
b. Copper
c. Iron
d. Nickel
e. Titanium
Metal
Specific heat
capacity (J/g·°C)
Aluminum
Iron
Copper
Gold
Titanium
Nickel
Cobalt
0.897
0.449
0.385
0.128
0.527
0.443
0.421
2. A 27.0 g sample of solid aluminum at 100 °C is placed in a container of 100 g of water that is initially
at 30.0 °C. Assuming that no heat is transferred to the container, calculate the final temperature of
the aluminum and water. The specific heat capacity of aluminum is 0.897 J/g·°C.
a. 33.8 °C
b. 25.7 °C
c. 44.9 °C
d. 65.0 °C
e. None of the others
3. The balanced reaction below is performed in a coffee-cup calorimeter containing 450 mL of solution.
The temperature rises 15.5 °C. Assume that the calorimeter doesn’t absorb any heat and that the
specific heat capacity of the solution is 4.184 J/g·°C. Also assume that the density of the solution is
0.998 g/mL. Find the ΔH of the reaction.
LiOH(aq) + HCl(aq) → LiCl(aq) + H2O(l)
a. -6.98 kJ
b. -29.1 kJ
c. -1.88 kJ
d. -3.92 kJ
e. None of the others
4. A substance is burned in a bomb calorimeter causing the temperature to rise by 35.0 °C. The heat
capacity of the bomb is 289 J/°C. The calorimeter contains 500 g of water. What is the amount of
heat transferred in this process?
a. None of the others
b. -10.1 kJ
c. -73.2 kJ
d. -83.3 kJ
e. -41.7 kJ
5. Which of the following statements are true?
A. Heat transferred (q) is a state function
B. The change in internal energy (ΔE) is the sum of heat transferred (q) and work done (w)
C. The heat transferred (q) to a system during a process at constant pressure is the change in
enthalpy (ΔH)
a. A only
b. A and B
c. B only
d. A and C
e. B and C
6. Use thermochemical expressions (1) and (2) below to find the ΔH for reaction (3).
(1) S8(s) + 4 Cl2(g) → 4 S2Cl2(g)
(2) S8(s) + 8 Cl2(g) → 8 SCl2(g)
(3) S2Cl2(g) + Cl2(g) → 2 SCl2(g)
ΔH = -66.8 kJ
ΔH = -141 kJ
ΔH = ?
a. -208 kJ
b. -74.2 kJ
c. -18.6 kJ
d. -124 kJ
e. -102 kJ
7. Which of the following is an invalid set of quantum numbers?
a. (3, 2, -2, ½)
b. n = 4, l = 0, ml = 0, ms = -½
c. (2, 2, 1, ½)
d. n = 5, l = 3, ml = -1, ms = -½
e. (4, 2, 0, -½)
8. Which of the following statements is false?
A. The ionic radius of a cation is always larger than the atomic radius of the neutral atom
B. Isoelectronic ions have the same electron configuration
C. The atomic radii of transition metal atoms continuously decrease as you go from left-to-right
along a row.
a. A only
b. B only
c. C only
d. A and B
e. A and C
9. Predict the order from smallest to largest for the following set of atoms
Bi
P
Se S
As
a. Bi, P, Se, S, As
b. None of the others
c. Bi, Se, As, S, P
d. P, Se, S, As, Bi
e. P, S, As, Se, Bi
10. Predict the order from largest to smallest for the following set of ions
Br-
Ca2+ K+
As3-
Se2-
a. Ca2+, K+, Br-, Se2-, As3b. K+, Ca2+, As3-, Se2-, Brc. Br-, Se2-, As3-, Ca2+, K+
d. None of the others
e. As3-, Se2-, Br-, K+, Ca2+
11. Which of the following is the correct electron configuration for Al using noble-gas notation?
a. [He]2s22p63s23p1
b. [Ne]3s23p1
c. [Mg]3p1
d. None of the others
e. 1s22s22p63s23p1
12. Which is the correct electron configuration for Cu2+ using noble-gas notation?
a. [Ar]4s13d10
b. [Ar]4s23d7
c. None of the others
d. [Ar]3d9
e. [Ar]4s13d8
13. Use the table below to find the ΔH for the following balanced reaction.
I2(s) + 2 H2O(l) + SO2(g) → 2 HI(aq) + H2SO4(aq)
Compound
H2O(l)
SO2(g)
HI(aq)
H2SO4(aq)
a.
b.
c.
d.
e.
Not enough information to answer
-381.6 kJ
-151.2 kJ
-95.97 kJ
-437.0 kJ
ΔHf° (kJ/mol)
-285.83
-296.83
-55.19
-909.27
14. How much heat is required to convert 80.0 g of ice at -15.0 °C to water at 25.0 °C. The specific heat
capacity for ice is 2.06 J/g·°C. The ΔHfusion is 333 J/g.
a. 26.6 kJ
b. 33.2 kJ
c. 40.0 kJ
d. 37.5 kJ
e. 9.99 kJ
15. Calculate the wavelength of light required to excite an electron in a hydrogen atom from the n = 2
state to the n = 5 state.
a. 4.34 × 10-7 m
b. 6.56 × 10-7 m
c. 4.86 × 10-7 m
d. 4.10 × 10-7 m
e. 1.22 × 10-7 m
16. Calculate the de Broglie wavelength of a neutron moving at 50 m/s. The mass of a neutron is 1.6749
× 10-24 g.
a. None of the others
b. 1.26 × 108 m
c. 7.91 × 10-9 m
d. 1.26 × 1011 m
e. 7.91 × 10-12 m
Short answer 2 (5 points each, no partial credit)
Sketch the orbitals and label your axes. You’ll be graded on the shape, orientation, shading and relative
size.
17. 2px
18. 3dz2
x
z
y
y
19. Draw the energy level diagram for nitrogen and indicate whether it is paramagnetic or diamagnetic.
Paramagnetic
20. Draw the orbital box diagram for S2- and indicate whether it is paramagnetic or diamagnetic.
Diamagnetic
Useful information
Speed of light: c = 2.998 × 108 m/s
Planck’s constant: h = 6.626 × 10-34 J·s