CHEMISTRY 110 EXAM 1
Sept 23, 2013
FORM A
--------------------------------------------------------------------------------1. A graduated cylinder is filled with 50.0 g of ethylene glycol,
which has a density of 1.11 g/cm3. What is the volumetric
reading on the graduated cylinder when it is filled?
--------------------------------------------------------------------------------3. A compound containing 10.4% of C, 27.8% of S, and 61.7% of
Cl (by weight) has a molecular weight of 115 g/mol. What is its
molecular formula?
A. CSCl2
B. C2SCl
C. CS2Cl
A. 40.6 mL
D. C2S2Cl
B. 45.0 mL
E. CS2Cl2
C. 50.0 mL
D. 55.5 mL
E. 61.6 mL
--------------------------------------------------------------------------------2. Which one of the following has an equal number of electrons
and neutrons?
A.
13
B.
19 !
C.
32 2!
D.
35
Cl
E.
56
Fe3+
C
F
S
--------------------------------------------------------------------------------4. What is the maximum number of electrons in the ground state
of As that could have a quantum number ms = !1/2?
A. 16
B. 18
C. 32
D. 34
E. 36
--------------------------------------------------------------------------------5. Which one of the following is a possible electron configuration
for Xe in an excited state?
A. [Ne] 3s23p6
B. [Ar] 3s23p6
---------------------------------------------------------------------------------
C. [Ar] 3d104s24p6
D. [Kr] 4d105s25p5
E. [Kr] 4d105s25p56s1
--------------------------------------------------------------------------------
--------------------------------------------------------------------------------6. Which one of the following is the ground state electron
configuration of a sulfide ion?
--------------------------------------------------------------------------------9. Which of the following best describes the shape of a 3d atomic
orbital?
A
A. 1s22s22p4
B
C
D
E
B. 1s22s22p6
C. 1s22s22p63s2
D. 1s22s22p63s23p4
n
!
m!
ms
A. 4
0
0
0
B. 3
0
"
0
C. 4
1
0
+"
D. 4
0
0
+"
E. 3
2
!2
!"
--------------------------------------------------------------------------------8. How many possible values are there for the magnetic quantum
number (m!) for an electron in the 6f subshell?
x
x
x
y
y
y
x
x
y
y
--------------------------------------------------------------------------------10. Assuming that a one-electron atom has only 4 possible energy
levels as shown, how many lines will there be in the emission
spectrum?
A.
B.
C.
D.
E.
3
4
6
8
10
n=4
n=3
n=2
Energy
E. 1s22s22p63s23p6
--------------------------------------------------------------------------------7. Which series of quantum numbers can describe the highest
energy electron in the ground state of calcium?
A. 3
B. 4
C. 6
n=1
D. 7
E. 14
---------------------------------------------------------------------------------
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------!"
11. An isotope of gallium can be represented using this symbol: !"
!" .
Given that the average atomic mass of gallium is 69.72 amu,
which of the following statements must be true?
i.
There is more than one isotope of gallium found in
nature.
ii. Most gallium atoms have more neutrons than protons.
iii. The most common isotope of gallium has fewer than 38
neutrons.
A. i only
--------------------------------------------------------------------------------13. Consider the process of walking from your home to this class.
Which one of the following observables is a state function?
A. The time it takes to travel to class.
B. The distance you walk to class.
C. The number of people that you pass on the way to class.
D. The gain or loss in elevation.
E. The number of steps that you take.
--------------------------------------------------------------------------------14. Which one of the atoms or ions below requires the most
energy to remove its highest- energy electron?
B. ii only
C. iii only
D. i and ii only
A. Mg+2
E. all three must be true
B. Na+
--------------------------------------------------------------------------------12. Which of the following samples has the greatest number of O
atoms?
A. 0.2 moles of sucrose
C12H22O11
B. 0.3 moles of glucose
C6H12O6
C. 0.6 moles of copper sulfate CuSO4
C. Ne
D. Li+
E. Be+2
--------------------------------------------------------------------------------15. Which one of the following rankings of atomic sizes (from
largest to smallest) is correct?
D. 1.0 moles of dioxygen
O2
A. Cl > Al > Ba > Cs
E. 2.0 moles of methanol
CH3OH
B. Al > Cl > Ba > Cs
C. Ba > Cl > Al > Cs
---------------------------------------------------------------------------------
D. Ba > Cs > Al > Cl
E. Cs > Ba > Al > Cl
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------16. A scientist has two identical pistons filled with argon gas (Ar).
The Ar gas in both pistons begins with the same internal energy of
10 kJ. She makes the following changes to the pistons:
--------------------------------------------------------------------------------18. Which of the following electron configurations violate Hund's
rule and/or the Pauli exclusion principle?
1s
Piston 1: She increases the internal energy of the gas in
the first piston to a final value of 20 kJ by
heating it while keeping the volume constant.
Piston 2: She does 20 kJ of work to the gas in the
second piston by compressing it while the gas
loses 10 kJ of heat to the surroundings.
A.
Which statement is true of the gas in the pistons?
2s
2p
3s
i.
(!) (!)
(!) ("") (")
ii.
(!) (!)
(!) (!)
(")
iii. (!) (!)
(!) (!)
( )
(!)
Violates Hund's rule Violates Pauli
i
iii
B.
i and ii
iii
C.
ii and iii
i
A. The gas in both pistons has the same final internal energy.
D.
ii
i and iii
B. The gas in Piston 1 has a higher final internal energy.
E.
iii
i
C. The gas in both pistons does the same amount of work.
D. The gas in Piston 1 undergoes an exothermic change.
E. The gas in Piston 2 undergoes an endothermic change.
--------------------------------------------------------------------------------19. Which of the following orbitals are degenerate in the hydrogen
atom with n = 3?
--------------------------------------------------------------------------------17. Which one of these solids has the highest melting point?
A. CaS
B. BaO
A. II and III only
C. NaI
B. I and IV only
D. LiBr
C. I, II, and IV only
E. MgO
D. II, III, and IV only
---------------------------------------------------------------------------------
E. all
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------20. Which of the following ions are isoelectronic?
Cu+
Cu+2
Zn+2
A. Cu
+
and Sr
B. Cu
+2
and Zn+2
Ni+2
Sr+2
+2
C. 0.0225
D. 0.315
D. Ni+2 and Cu+2
E. Zn
and Sr
A. 1.89 # 1023
B. 0.02245
C. Zn+2 and Cu+
+2
--------------------------------------------------------------------------------22. How many oxygen atoms are present in 10.3 g of
Cd(MnO4)2!6H2O?
E. 1.35 # 1022
+2
--------------------------------------------------------------------------------21. Consider a neutral substance where the two atoms form an
ionic bond. Given this figure depicting the sizes of the ions,
which of the following atomic assignments could be correct?
--------------------------------------------------------------------------------23. Rank the three waves shown below in order of decreasing
energy, assuming they are all electromagnetic radiation.
1
Ion 1
Ion 2
3
A. 1 > 2 > 3
B. 1 > 3 > 2
A.
Ion 1
Mg
Ion 2
Cl
B.
Br
Ca
D. 2 > 1 > 3
C.
I
K
E. 3 > 1 > 2
D.
Li
Cl
E.
S
Mg
---------------------------------------------------------------------------------
2
C. 2 > 3 > 1
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------24. The energy of a pulse of green light (" = 532 nm) is 1.92 # 10!3 J.
How many photons are in the pulse?
A. 3.63 # 103
B. 5.21 # 103
--------------------------------------------------------------------------------26. In a photochemical process a hydrogen atom absorbs a 410 nm
photon and shortly thereafter it emits a 2628 nm photon. What
is $E for the combination of these processes?
A. 3.02 # 10$19 J
C. 5.14 # 1015
B. 4.09 # 10$19 J
D. 1.16 # 1021
C. –2.46 # 10$19 J
E. 1.57 # 1024
D. –4.09 # 10$19 J
E. –3.02 # 10$19 J
--------------------------------------------------------------------------------25. A line in the hydrogen emission spectrum has a wavelength of
434.5 nm. If this line results from the transition of an electron
into the n = 2 level, what was the initial energy state of the
electron?
A. n = 1 level
B. n = 3 level
C. n = 4 level
D. n = 5 level
E. n = 6 level
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------27. A student synthesizes a compound composed of carbon,
hydrogen, and nitrogen and submits 0.1156 g of it to
combustion analysis. The student recovers 0.1638 g of carbon
dioxide and 0.1676 g of water. What is the mass percent of
carbon in the compound?
A. 38.67%
B. 4.470%
C. 16.23%
D. 45.10%
E. 77.34%
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------28. The diagram below depicts two cases of interacting charged
particles separated by the same distance. Which of the
following statements are true, regarding this diagram?
i.
The electrostatic potential energy for A is lower than B.
ii.
The electrostatic potential energy for B is lower than A.
iii.
The electrostatic potential energy for A and B is the same.
iv.
The electrostatic potential energies for A and B have the same
magnitude, but opposite signs.
A. i only
B. ii only
C. iii only
D. iv only
E. ii and iv only
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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.
B
B
A
B
E
E
D
D
D
C
D
C
D
E
E
A
E
E
E
C
D
A
D
C
D
B
A
E
CHEM 110
Fall 2013
Exam 1 Form A
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