CHEMISTRY 110 EXAM 1
Feb. 4, 2013
FORM A
--------------------------------------------------------------------------------1. What is the mass of calcium that contains 8.075 ! 1012 Ca
atoms?
A. 1.341 ! 10!11 g
B. 3.353 ! 10!13 g
C. 5.376 ! 10!10 g
--------------------------------------------------------------------------------3. How many protons, neutrons, and electrons does 108Ag+ have?
p
n
e!
A.
47
61
62
B.
108
47
48
C.
62
46
61
D.
47
61
46
E.
None of the answers listed here are correct
D. 1.860 ! 109 g
E. 3.234 ! 1014 g
--------------------------------------------------------------------------------2. A graduated cylinder contains 15.5 mL of water. After a metal
ball with a mass of 7.95 g is dropped into the graduated
cylinder the volume changes to 95.2 mL. What is the density of
this metal?
--------------------------------------------------------------------------------4. For the following arrangement, what is the internal energy
change for System A if q1 = 10 kJ, q2 = 5 kJ, w1 = 8 kJ and w2
= 10 kJ?
A. 9.97 ! 10!2 g/mL
B. 0.0718 g/mL
A. !2 kJ
C. 0.0835 g/mL
B. !7 kJ
D. 0.513 g/mL
C. !33 kJ
E. 10.0 g/mL
D. +10 kJ
E. +3 kJ
---------------------------------------------------------------------------------
---------------------------------------------------------------------------------
--------------------------------------------------------------------------------5. A modern cell phone uses 1900 MHz electromagnetic waves
to communicate. What is the wavelength of this radiation in
cm?
--------------------------------------------------------------------------------7. What is the percent sodium in sodium carbonate?
A. 43.4%
B. 11.3%
A. 29.48 cm.
C. 45.3%
B. 294.8 cm
D. 27.7%
C. 15.78 cm
E. 23.0%
D. 19.01 cm
E. 1900 cm
--------------------------------------------------------------------------------6. Which of the following are an incorrect set of quantum
numbers for an atom?
A. n = 3, ! = 2, m! =
0, ms = +1/2
B. n = 4, ! = 3, m! = !2, ms = !1/2
C. n = 2, ! = 2, m! =
2, ms = !1/2
D. n = 1, ! = 0, m! =
0, ms = +1/2
E. n = 3, ! = 1, m! = !1, ms = !1/2
--------------------------------------------------------------------------------8. Which of these choices is the electron configuration for the
aluminum ion?
A. 1s22s22p63s2
B. 1s22s22p63s23p2
C. 1s22s22p63s23p1
D. 1s22s22p6
E. 1s22s22p63s23p4
--------------------------------------------------------------------------------9. Which of the elements listed below has the largest atomic
radius?
A. B
---------------------------------------------------------------------------------
B. Al
C. S
D. P
E. Si
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--------------------------------------------------------------------------------10. Which one of the following equations correctly represents the
process associated with the ionization energy of X?
A. X(g) " X2+(g) +2 e–
--------------------------------------------------------------------------------13. A compound is 53.3% C, 11.2 % H and 35.5 % O by mass.
What is the molecular formula of the compound if the molar
mass is 90 g/mol?
A. CH2O
B. X2(g) " X+(g) + X–(g)
B. C2H5O
C. X(g) + e– " X–(g)
C. C4H10O2
D. X–(g) " X(g) + e–
D. C3H6O3
E. X(g) " X+(g) + e–
E. C5H14O
--------------------------------------------------------------------------------11. Which orbital has an unpaired electron in the ground state of
bromine?
--------------------------------------------------------------------------------14. Which one of these ions has the smallest radius?
A. K+
B. Cl!
C. Na+
E. None of these: there are no unpaired electrons in the
ground state of bromine.
--------------------------------------------------------------------------------12. Which bond in the molecule below is the most polar?
H
C. C#Br
D. C#O
E. C#F
E. O2!
--------------------------------------------------------------------------------15. Which one of these has the greatest number of moles of
atoms?
H
A. C#H
B. C#Cl
D. S2!
F
C
Cl
C
C
C
C
C
A. 5.00 g of H2
B. 25.00 g of C
C. 82.00 g of Pb
Br
OH
---------------------------------------------------------------------------------
D. 127.00 g of Cu
E. 384.00 g of Au
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--------------------------------------------------------------------------------16. What is the wavelength of a photon emitted by a hydrogen
atom when its electron drops from n=4 to n=2?
--------------------------------------------------------------------------------19. Which one of the following orbital diagrams is an excited
state electron configuration of nitrogen?
A. None of the answers listed here.
B. 364 "m
C. 486 "m
1s
2s
2p
3s
A
D. 486 nm
E. 364 nm
--------------------------------------------------------------------------------17. Which of the following set of quantum numbers has the
greatest number of degenerate orbitals?
A. n = 3, ! = 2
B
C
D
B. n = 4, ! = 3
C. n = 2, ! = 1
E
D. n = 6, ! = 0
E. n = 1, ! = 0
--------------------------------------------------------------------------------18. How many unpaired electrons are in the ground state of
Co3+?
A. 2
B. 3
C. 4
D. 5
--------------------------------------------------------------------------------20. Which of the following compounds is an ionic compound?
A. KF
B. CCl4
C. CS2
D. CO2
E. ICl
E. 6
---------------------------------------------------------------------------------
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--------------------------------------------------------------------------------21. The first four ionization energies (I) for an atom are given
below. What is the identity of this atom?
I1 = 738 kJ/mol
I2 = 1451 kJ/mol
I3 = 7733 kJ/mol
I4 =10,542 kJ/mol.
--------------------------------------------------------------------------------23. Boron has two naturally occurring isotopes, 10B and 11B. The
average atomic mass of boron is 10.811. What is the percent
abundance these isotopes?
A. 20% 10B
80%11B
B. 80% 10B
20%11B
A. Na
C. 50%
B
50%11B
B. Al
D. 60% 10B
40%11B
C. Cl
E. 40% 10B
60%11B
10
D. Si
E. Mg
--------------------------------------------------------------------------------24. Rank the following electrostatic interactions in order of
increasing electrostatic potential energy.
--------------------------------------------------------------------------------22. Select the compound with the highest lattice energy.
A. CaS
0.5 d
0.5 d
+1
#1
4d
+2
#1
+2
#2
B. BaS
C. NaI
1
2
3
D. MgO
E. LiBr
A. 1 < 2 < 3
B. 1 < 3 < 2
---------------------------------------------------------------------------------
C. 3 < 2 < 1
D. 2 < 3 < 1
E. 2 < 1 < 3
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--------------------------------------------------------------------------------25. 90.1 g of FeCl3 $ x H2O is heated to drive off all of the water of
hydration. The mass of the remaining salt is 54.1 g. What is
the value of x in the formula for the hydrate?
--------------------------------------------------------------------------------27. Assuming the pictures below schematically represent visible,
microwave and X-ray radiation, what is the correct
assignment?
A. 2
B. 3
C. 4
D. 5
E. 6
--------------------------------------------------------------------------------26. Which of the following could have the quantum numbers n =
2, m! = !1?
A. 1 only
B. 2 only
C. 2, 4 and 5
D. 1, 2,4, and 5
E. all of these are possibilities
---------------------------------------------------------------------------------
1000 nm
107 nm
0.1 nm
1
2
3
A
B
C
D
E
1
visible
microwave
X-ray
X-ray
visible
2
X-ray
visible
microwave
visible
microwave
3
microwave
X-ray
visible
microwave
X-ray
--------------------------------------------------------------------------------28. How many moles of ultra-violet light with a wavelength of 400
nm does it take to equal the energy in 1.0 mole of infrared
radiation of 1000 nm?
A. 0.080 moles
B. 2.5 moles
C. 0.40 moles
D. 1.0 moles
E. None of the answers listed here are correct
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END OF EXAM
CHEMISTRY 110 EXAM 1
February 4, 2013
Answer Key
FORM A
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