Name: ________________________ Class: ___________________ Date: __________
ID: A
Exam II 2009
Record your name on the top of this exam and on the scantron form.
Record the test ID letter in the top right box of the scantron form.
Record all of your answers on the scantron form.
Turn in your answer sheet at the end of the period. You have 50 minutes. GOOD LUCK !
1. If 50.0 g of ethanol, CH 3CH2OH, at 20.0 °C absorbs 1.45 kJ of heat, what is the final temperature of the ethanol?
The specific heat capacity of ethanol is 2.44 J/g⋅K.
a. 8.1 °C
b. 21.2 °C
c. 31.9 °C
d. 47.7 °C
2. The thermochemical equation for the combustion of benzene is shown below.
ΔrH° = –3909.9 kJ/mol-rxn
2 C6H6(™ ) + 15 O2(g) → 12 CO2(g) + 6 H 2O(g)
What is the enthalpy change for the combustion of 12.5 g C 6H6?
a. –313 kJ
b. –626 kJ
c. –1.22 × 104 kJ
d. –2.44 × 104 kJ
3. If the ground state electron configuration of an element is [Ar]3d104s24p4, what is the typical charge on the
monatomic anion of the element?
a. 4+
b. 2+
c. 1–
d. 2–
4. Which of the following ions have the same ground state electron configuration: Cl –, P3–, Ca2+, and Ga+?
a. Cl– and P3–
b. Cl–, P3–, and Ca2+
c. Ca2+ and Ga+
d. P3– and Ga+
5. Place the following atoms in order of increasing atomic radii: K, Mg, Ca, and Rb?
a. K < Mg < Ca < Rb
b. K < Mg < Rb < Ca
c. Mg < Ca < K < Rb
d. K < Rb < Mg < Ca
6. For which of the following elements is the second ionization energy greatest?
a. Mg
b. Al
c. Na
d. Sc
1
Name: ________________________
ID: A
7. Which of the following statements is INCORRECT?
a. It is not possible to know the exact location of an electron and its exact energy
simultaneously.
b. The energies of an atom's electrons are quantized.
c. Quantum numbers define the energy states and the orbitals available to an electron.
d. The behavior of an atom's electrons can be described by circular orbits around a nucleus.
8. What type of orbital is designated n = 4, ™ = 0, m™ = 0?
a. 4s
b. 4p
c. 4d
d. 4f
9. Which of the following diagrams represent p-orbitals?
a.
b.
c.
d.
1 only
2 only
3 only
4 only
10. Which of the following statements is/are CORRECT for a carbon atom?
1. The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s
electron.
2. The effective nuclear charge felt by a 2p electron is less than that felt by a 2s
electron.
3. The effective nuclear charges felt by 2s and 2p electrons are identical.
a.
b.
c.
d.
1 only
2 only
3 only
1 and 3
11. Which of the following elements is the most electronegative?
a. Li
c. P
b. O
d. K
12. Which of the following electron configurations disobeys Hund’s rule?
a.
c.
b.
d.
2
Name: ________________________
ID: A
13. Which of the following electron configurations violates the Pauli exclusion principal?
a.
c.
b.
d.
14. Which of the following ions is largest?
a. S2b. Br -
c.
d.
K+
Ca2+
15. What is the ground-state electron configuration for Vanadium (V)?
c. [Ar]3d44s1
a. [Ar]3d3
3
2
b. [Ar]3d 4s
d. [Ar]3d5
16. In a certain process 50 J of work is done on the system and 30 J of heat are transferred to the surroundings. The
change in internal energy of the system for this process, in J, is:
a. 80
c. 20
b. -80
d. -20
17. Calculate the ΔH (in kJ) for the reaction:
NO (g) + 1/2O 2 (g) --> NO2 (g)
given the following information:
N2 (g) + O2 (g) --> 2 NO (g) ΔH = +180 kJ
1/2 N 2 (g) + O2 (g) --> NO2 (g) ΔH = +34 kJ
a.
b.
-56
+56
c.
d.
-124
+124
18. Elements in periodic groups IIA and VIA usually react with each other to form compounds that are:
a. covalent
c. insoluble in water
b. ionic
d. metallic
19. From which of the following would it be most difficult to remove an electron?
c. Na+
a. O2b. F
d. Mg2+
20. A line in the emission spectrum of Li has a wavelength of 671 nm. What is the energy, in kJ, of a mole of photons
of this wavelength?
a. 2.96 x 10-19
c. 1.44 x 10-12
b. 178
d. 262
21. What is the oxidation number for sulfur in the sulfate anion, SO 42-?
a. -2
c. +4
b. +2
d. +6
3
Name: ________________________
ID: A
22. In Rutherford’s experiment, particles were shot at a gold foil that was only a few atoms thick. Approximately
what fraction of the particles were deflected by the gold atoms?
a. zero
b. 1/1000
c. 9/10
d. all
23. Which of the following chemical equations does not correspond to a standard molar enthalpy of formation?
a. Ca(s) + C(s) + 3/2 O2(g) → CaCO3(s)
b. C(s) + O2(g) → CO2(g)
c. NO(g) + 1/2 O2(g) → NO2(g)
d. N2(g) + 2 O2(g) → N2O4(g)
24. Which element, E, is described by the following? It forms an oxide of formula EO 3, a hydride of formiula EH2,
and a fluoride of formula EF6.
a. E= N
c. E = P
b. E = O
d. E = S
25. Quantum theory, as applied to atomic properties, tells us that:
a. electrons behave as particles
c. electrons in atoms may have any energy
b. electrons in atoms may have only certain d. light behaves as a wave
energies
26. Which of the following sets of quantum numbers refers to an p-orbital? (it has to be a valid set of quantum
numbers)
a. n = 1, l = 1, ml = 0
c. n = 3, l = 1, ml = 0
d. n = 3, l = 0, ml = 1
b. n = 2, l = 0, ml = 1
4
ID: A
Exam II 2009
Answer Section
MULTIPLE CHOICE
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.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
TOP:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
C
PTS: 1
TOP: 5.2 Specific Heat Capacity: Heating and Cooling
A
PTS: 1
TOP: 5.5 Enthalpy Changes for Chemical Reactions
D
PTS: 1
TOP: 7.4 Electron Configurations of Ions
B
PTS: 1
TOP: 7.4 Electron Configurations of Ions
C
PTS: 1
TOP: 7.5 Atomic Properties and Periodic Trends
C
PTS: 1
TOP: 7.5 Atomic Properties and Periodic Trends
D
PTS: 1
6.5 The Modern View of Electronic Structure: Wave or Quantum Mechanics
A
PTS: 1
TOP: 6.6 The Shapes of Atomic Orbitals
D
PTS: 1
TOP: 6.6 The Shapes of Atomic Orbitals
B
PTS: 1
TOP: 7.2 Atomic Subshell Energies and Electron Assignments
B
PTS: 1
A
PTS: 1
D
PTS: 1
A
PTS: 1
B
PTS: 1
C
PTS: 1
A
PTS: 1
B
PTS: 1
D
PTS: 1
B
PTS: 1
D
PTS: 1
B
PTS: 1
C
PTS: 1
TOP: 5.7 Enthalpy Calculations
D
PTS: 1
B
PTS: 1
C
PTS: 1
1