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UNIVERSITY OF VICTORIA
FINAL EXAMINATION, DECEMBER 2012
CHEMISTRY 101
Fundamentals of Chemistry I
Time: 3 hours
Hand in only the bubble sheet at the end of the test period (3 hours).
Instructors:
A01 CRN 11868 Dr. N. Burford
A02 CRN 11869 Dr. S. Briggs
A03 CRN 11408 Dr. N. Burford
Before you begin to write your exam you should find three items on your exam desk:
1) An exam placemat bearing your name. Sign this page. It will be collected during the exam when we
check your student ID card. Do not use this page for scrap paper.
2) This exam question paper, containing an unstapled DATA sheet inside the cover page.
3) A bubble sheet (UVic Form A) for recording your answers. PRINT and shade in only your
LAST name, then first name, and the last 7 digits of your student ID number on
the bubble sheet. i.e. Omit the leading V0.
Do NOT include any info about the course, section or date on the bubble sheet.
This exam question paper has 17 pages plus a DATA sheet. Students must count the number of pages in
this examination paper before starting to write the exam. Report any discrepancy immediately to one of the
instructors in the room.
This exam consists entirely of multiple choice questions. There are 65 multiple choice questions worth 2
marks each. TOTAL MARKS AVAILABLE = 130
This question paper contains enough blank space for working out the questions. No other paper is permitted.
The basic Sharp EL510 calculator is the only one approved for use in Chemistry 101.
It is a University Calendar regulation that no student may arrive at the exam after the
first half hour and no student may leave the exam in the first half hour.
If you finish your exam before 2¾ hours have elapsed then you may hand in your
bubble sheet and leave. We ask that students not leave (i.e. that students remain seated)
during the last 15 minutes of the exam so that everyone remaining may finish their
exams without noise or disturbance.
DO NOT BEGIN UNTIL TOLD TO DO SO BY THE INVIGILATOR
The answers must be coded on the optical sense form (bubble sheet) using a SOFT PENCIL.
Chemistry 101 Final Examination
Dec. 10, 2012; Page 2 of 17
Select the BEST response for each question.
Below is the energy level diagram for an electron in a hydrogen atom. Answer questions 1 to 4 with
reference to this diagram.
1. Which of the following statements is INCORRECT?
A. Transition T represents an
absorption of energy.
[Energy levels not exactly to scale]
B. Level C is the second excited
state.
8
C. Transition R corresponds to an
ionization.
S
D
T
C
D. The value of the principal
quantum number n in level C is 2.
W
X
R
B
E. The hydrogen atom loses energy
when it undergoes transition X.
2. What is the frequency of the photon
required to cause the transition
labeled S?
Energy
A. 8.23 × 1014 s−1
B. 2.42 × 10
−19
Y
Z
J
C. 3.29 × 1015 s−1
D. 2.06 × 1014 s−1
E. 3.66 × 1014 s−1
3. What is the energy corresponding to
the transition labeled X?
A. 2.42 × 10−19 J
B. 1.55 × 10−19 J
A
C. 4.84 × 10−19 J
D. 4.30 × 10−19 J
E. 8.72 × 10−20 J
4. Which transition represents the reaction H+ + e–  H (ground state) ?
A. Z
B. Y
C. X
D. R
E. Y & Z
5. In a hydrogen atom, how many unique sets of four quantum numbers, n, ℓ, mℓ and ms can an electron
have when n = 4 and mℓ = −1?
A. 6
B. 1
C. 2
D. 4
E. 3
Chemistry 101 Final Examination
Dec. 10, 2012; Page 3 of 17
6. Which of the following statements about electrons is INCORRECT?
A. Electrons can be diffracted by a crystal.
B. Increasing the speed of an electron increases its wavelength.
C. An electron’s position and momentum cannot be known accurately at the same time.
D. An electron has a smaller mass than a neutron.
E. An electron that is farther from the nucleus of a hydrogen atom is higher in energy than an electron
that is close to the nucleus.
7. Which of the following statements about a ground state rubidium (Rb) atom is INCORRECT?
A. There are 18 electrons with principal quantum number n = 3.
B. There are 9 electrons with angular momentum quantum number l = 1.
C. There are 2 electrons with magnetic quantum number ml = −2.
D. There are at least 18 electrons with spin quantum number ms = −½.
E. There are 9 s-electrons.
8. The correct condensed electron configuration of mercury (II) (Hg2+) is:
A. [Xe] 6s24f145d10
B. [Xe] 6s24f145d8
C. [Xe] 5d10
D. [Xe] 4f145d10
E. [Xe] 6s24f105d8
9. Which of the following statements in INCORRECT?
A. When a cation is formed from a neutral atom, electrons are removed from the occupied orbital
having the largest principal quantum number.
B. The attraction between opposite electrical charges depends on the magnitudes of the charges and
the distance between them.
C. A valence electron is attracted to the nucleus and repelled by the core electrons.
D. The effective nuclear charge increases from left to right across the first row of the periodic table.
E. Electrons in 4d orbitals strongly shield each other from the charge of the nucleus.
Chemistry 101 Final Examination
Dec. 10, 2012; Page 4 of 17
10. Which of the following pairs of ions are isoelectronic?
A. Ca2+ and Zn2+
B. P3– and N3–
D. Si4– and Sn4+
E. Cl– and Ca2+
C. O2– and Cl–
11. Identify the ion that has the following electron configuration. 1s22s22p63s23p63d8
A. Mn+
B. Co2+
D. Ni+
E. Cu4+
C. Ni2+
12. Which of the following atoms has the ground state electron configuration with the MOST unpaired
electrons?
A. As
B. Au
C. I
D. Li
E. Mn
13. If A > B means that the radius of A is greater than the radius of B then which of the following
is INCORRECT?
A. F > F+
C. Br– > Na+
B. Na– > Na
D. O− > O2−
E. Sr2+ > Ca2+
14. In which one of the following molecules or ions is the octet rule not followed (not counting H)?
B. NH4+
A. NH3
D. BH4−
C. I2
E. NO2
15. Which of the following molecules has the most polar bonds?
A. PF3
B. SF2
C. N2
D. SeBr2
E. CH4
16. Here are two resonance structures for the sulfate ion, SO42–. The formal charges on the sulfur atoms
in structures (i) and (ii) are, respectively?
O
A. +1, −1
S
2-
2-
O
O
O
O
S
O
O
(i)
(ii)
B. −1, +1
O
C. 0, +3
D. −1, −1
E. +1, +1
Chemistry 101 Final Examination
Dec. 10, 2012; Page 5 of 17
17. For which one of the following does the best simple description (i.e. lowest and fewest formal
charges) involve more than one Lewis structure (i.e. two or more resonance structures)?
A. CO32–
B. BF3
D. NH4+
E. OCF2
C. I3–
Consider the following five substances and then answer questions 18 to 20.
A. SCO
B. BaCl2
C. HCCH
D. I2
E. C2F4
18. Which molecule has only ONE pi bond?
19. Which substance exhibits IONIC bonding?
20. Which substance consists of polar molecules?
21. Which of these statements about hybridization is CORRECT?
A. Four atomic orbitals must be mixed to make an sp3d hybridized atom.
B. Water molecules are bent (i.e. V-shaped) because the oxygen atom is sp3 hybridized.
C. All bond angles are 90° in every compound that has an sp3d2 hybridized central atom.
D. The carbon atoms in benzene, C6H6, are all equivalent and sp hybridized.
E. The carbon atoms in hydrocarbons are always sp3 hybridized.
22. Which of the following pairs has the ionic compound with larger (more negative) lattice energy
listed first?
A. CsCl, SrS
B. BaS, CaS
C. BaO, SrO
D. CaO, CaS
E. RbCl, LiCl
Chemistry 101 Final Examination
Dec. 10, 2012; Page 6 of 17
23. The following three diagrams represent the orbital energy bands for three different kinds of solid
materials. These are, from left to right:
A. conductor, semiconductor, insulator
B. semiconductor, conductor, insulator
C. insulator, conductor, semiconductor
D. semiconductor, insulator, conductor
E. insulator, semiconductor, conductor
24. Considering likely intermolecular forces, which of the following should have the highest boiling
point?
A. CH3CH2—O—CH2CH3
B. CH3CH2CH2CH3
D. CH3CH2SH
E. CF4
25. Argon condenses to a liquid at 87 K because of:
A. the fact that it is a noble gas.
B. London dispersion forces.
C. covalent bonding.
D. ion-dipole forces.
E. dipole-dipole forces.
C. CH3CH2OH
Chemistry 101 Final Examination
Dec. 10, 2012; Page 7 of 17
26. The ellipsoidal rods in the picture below best represent molecules in a
A. normal liquid
B. nematic liquid crystalline phase
C. smectic liquid crystalline phase
D. cholesteric liquid crystalline phase
E. crystalline solid
27. The structure shown is a representation of which molecule?
A. GaBr3
B. ClF3
C. BF3
D. SbH3
E. PCl3
28. A plot of change in potential energy versus distance for two H atoms combining to form H2 is
shown below. At what point (A, B, C, D or E) is this two-atom system the most stable?
Chemistry 101 Final Examination
Dec. 10, 2012; Page 8 of 17
29. Which of these compounds is NOT sp3d hybridized?
A. [SiF4]2–
B. SF4
C. BrF5
D. PF5
E. XeF2
30. Which of the following oxides of nitrogen (A, B, C, D or E) is NON-polar?
N
N
N
N
N
N
N
A. NO
C. N2O3
B. N2O
D. NO2
N
E. N2O4
31. Diethyl ether ( CH3CH2OCH2CH3 ) can be involved in hydrogen bonding with:
A. ethane
B) itself
C) bromine
D) water
E) polypropylene
32. The structure below is Naproxen, a non-steroidal anti-inflammatory drug. How many sp2 hybridized
CARBON atoms are present in this molecule?
H
H
CH3 O
C
C
C
H
H
C
C
C
C
C
C
C
O
H
CH3
O
C
C
H
H
H
Naproxen
A. 1
B. 2
C. 3
D. 10
E. 11
Chemistry 101 Final Examination
Dec. 10, 2012; Page 9 of 17
33. Consider the molecule Naproxen, whose structure is shown above in question 32.
The oxygen-containing functional groups on the left and on the right of this molecule are, respectively:
A. ether, carboxylic acid
B. ester, alcohol
D. ester, carboxylic acid
E. ketone, ester
C. ether, carboxylic ester
34. Which of the following molecules has only single bonds?
A.
B.
C.
D.
E.
1-pentene
ethyne
Naproxen (shown above in question 32)
2,2-dimethylbutane
benzene
35. The correct name for the compound below is:
CH3
CH3
CH2
CH
CH
CH3
CH3
A. 3,4-dimethylpentane
B. 3-methylisohexane
C. 2-ethyl-3-methylbutane
D. 2,3-methylpentane
E. 2,3-dimethylpentane
36. Which one of the following compounds forms an ester on reaction with ethanol?
OH
O
O
CH3CH2CH2CH2OH
CH3COH
CH3CH2CH
A
B
C
CH3CH2
O
D
CH2CH3
E
Chemistry 101 Final Examination
Dec. 10, 2012; Page 10 of 17
37. Which of the following molecules is/are chiral?
H
Cl
OH
Cl
OH
Cl
H
(i)
H
Br
Br
all are chiral
B.
none are chiral
C.
(ii) and (iv)
D.
(i), (ii) and (iv)
E.
(ii), (iii) and (iv)
Cl
H
I
(iii)
(ii)
A.
CH3
CH3
F
(iv)
38. Which of the following molecules could best form a liquid crystal?
O
A.
O
OH
O
B.
NH
C.
Boron-doped germanium
n
HO
CH3
O
E.
D.
O
OH
H2C
CH
Chemistry 101 Final Examination
Dec. 10, 2012; Page 11 of 17
39. The correct name for the compound below is:
CH3
H
C
C
H
CH
CH3
CH3
A)
B)
C)
D)
E)
cis-2-methyl-3-pentene
trans-2-methyl-3-pentene
trans-isohexene
cis-4-methyl-2-pentene
trans-4-methyl-2-pentene
40. Consider the hydrogenation of ethane (reaction shown).
H2
+
H2C
nickel catalyst
CH2
CH3CH3
Using data from the DATA sheet, calculate (estimate) the enthalpy change (heat change) for this
reaction. The answer is: (in kJ mol−1)
A. 432
B. 1044
D. −130
C. 130
E. −1174
41. To a close approximation, the ideal bond angles marked a, b, c in the molecule below are _______,
________, and ________ respectively.
a
H
H
O
H
O
N
C
C
C
b
H
A. 90°, 180°, 90°
D. 120°, 120°, 90°
O
H
c
B. 109.5°, 120°, 109.5°
E. 109.5°, 90°, 120°
C. 120°, 120°, 109.5°
42. The molecule in question 41 above has _______ sigma ( ) and ________ pi ( ) bonds,
respectively.
A. 11, 3
B. 13, 0
C. 11, 2
D. 9, 2
E. 4, 2
Chemistry 101 Final Examination
Dec. 10, 2012; Page 12 of 17
43. Consider the following reaction:
OH
CH3
CH
CH3 +
CH
?
H2SO4
CH3
CH2
CH
CH3
The missing reactant represented by the question mark in this reaction is?
A. H2
B. H2O
C. O2
D. HOOH
E. Nickel catalyst
44. Consider the following reaction:
+
H2SO4
?
+ H2O
NO2
The missing reactant represented by the question mark in this reaction is?
A. NH3
B. Nickel catalyst
C. O2
D. HNO3
E. NO
45. Consider the following reaction:
CH3CH2CH2CH3
+
ignition or spark
O2(g)
?
The missing product or products represented by the question mark in this reaction is/are?
A. CH4 & H2O
B. CH3CH2CH2CH2OH
D. HNO3
E. CO2 & H2O
C. CH3CH2OOCH2CH3
46. Consider the following reaction:
O
O
CH3C
OH
+
?
CH3C
OCH3
The missing reactant represented by the question mark in this reaction is?
A. CH4
B. CH3CH2CH2CH2OH
D. H2O
E. OCH2
C. CH3OH
+ H2O
Chemistry 101 Final Examination
Dec. 10, 2012; Page 13 of 17
47. The covalent molecules PF3 and ClF3 have different bond angles. The predicted (i.e. estimated)
sizes of the F-P-F bond angles in PF3 and the F-Cl-F bond angles in ClF3 are, respectively,
___degrees and _____degrees.
A. 109.5, 90
B. 109.5, 120
C. 120, 120
D. 90, 90
E. 109.5, 109.5
48. Which of the following compounds is capable of geometrical (cis-trans) isomerism?
III
II
I
CH3
CH3CHCH
CH
CHCH3
CH2
CH3CH2CHCH3
Cl
Cl
A. I and II
B. II and III
C. I only
D. II only
E. III only
49. Which of the following statements concerning modern materials is INCORRECT?
A. Vulcanization of natural rubber involves cross-linking the chains with sulfur.
B. Doping a semiconductor makes it more conducting.
C. Plasticizers decrease the interaction between polymer chains.
D. A polymer formed from two different monomers is called a copolymer.
E. Semiconductors have a larger band gap than insulators.
50. The following is the molecular orbital energy diagram for MOs obtained from combining the 1s
orbitals of two atoms such as H or He. To correctly represent the electron energies for the ground
state of helium hydride ion HeH+ the orbitals labeled A and B will contain ___ electron(s) and
___ electron(s) respectively.
A. 2, 1
B. 2, 2
C. 1, 0
D. 1, 1
E. 2, 0
Chemistry 101 Final Examination
Dec. 10, 2012; Page 14 of 17
51. Band theory is the best way to account for the physical properties of transition metals. Which of the
following sets of transition metals would you expect to have filled bonding molecular orbitals and empty
antibonding orbitals, therefore the highest melting points?
A. Ti, Zr, Hf
B. Cu, Ag, Au
C. Co, Rh, Ir
D. Cr, Mo, W
E. Zn, Cd, Hg
52. If you want to dope germanium (Ge) to make an n-type semiconductor, an appropriate element to
select as a dopant is ___.
A. Ga
B. As
C. Al
D. Sn
E. Si
53. The structure of the styrene molecule is shown.
From the selection of polymer structures given below, pick the one
that correctly represents the molecular structure of polystyrene.
CH
Styrene
A
B
C
D
CH
CH2
CH
CH2
CH
CH
CH2
CH
CH2
CH
CH2
C
CH
C
CH
C
CH
CH
CH2
CH
CH2
CH
CH2
CH2
E
CH2
CH2
CH2
CH2
CH2
CH2
CH2
Chemistry 101 Final Examination
Dec. 10, 2012; Page 15 of 17
54. The compound C3H6Cl2 has how many structural (constitutional) isomers?
A. 1
B. 2
C. 3
D. 4
E. 5
55. Polyacrylonitrile is an addition polymer used in making furniture and clothing as well as many
other items. Its molecular structure is given below.
CH2
CH
CH2
CH
CN
CH2
CH
Polyacrylonitrile
CN
CN
Which of the following structures is the monomer from which polyacrylonitrile is made?
A
B
CH
CH2
D
C
CH3
CH2
CH2
CN
E
CH2
CN
CH
CH3
CH
NH2
CN
N
56. The structural formula for the natural polymer cellulose is shown below. This polymer is familiar
to us as cotton, from which many clothing items are made.
HO
H
HO
H
H
HO
H
H
O
H
HO
H
H
H
OH
H
O
H
O
O
HO
HO
H
O
H
OH
O
O
HO
H
H
H
OH
O
HO
H
OH
H
H
H
The reason that wet cotton clothing takes so long to dry is?
A. The cellulose polymer molecules are mostly cross-linked.
B. Water reacts with the cellulose to produce carboxylic esters.
C. Cotton contains plasticizers that attract water molecules by ion-dipole forces.
D. Water is attracted to cellulose by London dispersion forces.
E. Water molecules are attracted strongly to the cellulose by hydrogen bonding.
Chemistry 101 Final Examination
Dec. 10, 2012; Page 16 of 17
Questions 57–61 refer to the figure below. All of these structures have five (5) electron domains.
57. Which of these molecular shapes is NOT found for an sp3d hybridized central atom?
58.Which of these molecular shapes can be achieved by a central atom with a hybridization that
is sp3d and also by a central atom with another type of hybridization?
59. Which of the shapes can lead to a molecule with an overall dipole moment vector of 0 (i.e. a
non-polar molecule)?
A.
A and E
B.
B, C and D
C.
A only
D.
E only
E.
none of them
60. Which element M will lead to an MF5 molecule with shape A above?
A. Al
B. Si
C. S
D. P
E. Cl
61. Which element M will lead to an MF3 molecule with shape D above?
A. Al
B. Si
C. P
D. S
E. Cl
Chemistry 101 Final Examination
Dec. 10, 2012; Page 17 of 17
62. If part of a Liquid Crystal Display (LCD) (such as on a cell phone) is heated, that part of
the screen will go black. Why?
A.
The molecules become locked in position, and can no longer affect polarized light.
B.
The liquid crystal phase becomes a normal liquid phase, which is unable to affect
polarized light
C.
The nematic liquid crystal phase transforms into a smectic liquid crystal phase, which
unable to affect polarized light.
D.
The liquid crystal molecules react with each other to form a polymer, which is unable
to affect polarized light.
E.
Light is efficiently absorbed by hot molecules.
63. A certain solid is moderately hard and has a high melting point. The solid does not
conduct electricity but the liquid formed when it is melted does conduct electricity. What
class of solid is this substance?
A. polymer
B. ionic
C. metallic
D. molecular
E. covalent network
64. Which identification is INCORRECT for the following substances as solids?
A.
B.
C.
D.
E.
SiC is a covalent-network solid
Li2CO3 is an ionic solid
Table sugar is a molecular solid
SiO2 is a covalent-network solid
Diamond is a molecular solid
65. The 2010 Nobel Prize in Physics was awarded to Andre Geim and Konstantin Novoselov
at the University of Manchester for their work on graphene, essentially single layers of
graphite sometimes characterized as atomic-scale chickenwire. This exciting allotrope of
carbon behaves as an excellent electrical conductor because...
A. Carbon p-orbitals overlap side-to-side throughout the entire sheet of graphene.
B. The carbon network consists of only sigma bonds.
C. Graphene has a valence shell MO band that is exactly half filled and the band gap is zero.
D. Both A and C above.
E. Both B and C above.
END OF EXAM