Version
B
UNIVERSITY OF VICTORIA
CHEMISTRY 101
Midterm Test 1
October 16, 2015
5-6 pm (60 minutes)
Version
B
DISPLAY YOUR STUDENT ID CARD (ONEcard) ON THE TOP OF YOUR DESK NOW
Answer all multiple choice questions on the bubble sheet provided. Use a pen (or soft
pencil). Complete the identification portion of the bubble sheet according to the
example shown, using your own name and student ID number. Indicate your Test
Version (A or B) in the line labeled ‘Form’.
Hand in only the bubble sheet at the end of the test period (60 minutes).
A DATA sheet is included, unstapled, inside the cover page of this test.
This test has 5 pages (not including the DATA sheet). Count the pages before you begin.
The basic Sharp EL510 calculator and the Sharp EL-510 RNB are the only ones
approved for use in Chemistry 101.
Chemistry 101, Mid-Term Test 1
Version B
Fall 2015
Page 2 of 5
DO NOT BEGIN UNTIL TOLD TO DO SO BY THE INVIGILATOR
This test consists entirely of multiple choice questions and is worth 25 marks. There is one mark per
question. The answers for the 25 questions must be coded on the optical sense form (bubble sheet)
using a PEN or SOFT PENCIL. Select the BEST response for each question below.
Below is the energy level diagram for the possible energy levels of a hydrogen atom (not to scale). Refer to it
when answering questions 1 to 5.
1. Why do none of the transitions into the level marked A
generate a photon in the visible part of the spectrum?
A. Because no transitions in the hydrogen atom produce
visible light
B. Because all of the transitions into A produce longer
wavelength photons in the infrared region of the
spectrum
C. Because all of the transitions into A produce shorter
wavelength photons in the ultraviolet region of the
spectrum
D. Because transitions into A involve the absorption of a
photon, not emission
E. Because electron-electron repulsions make double
occupation of A unfavourable
2. Which of the transition(s) shown result in the hydrogen
electron being in an excited state?
A.
B.
C.
D.
E.
All of F, G, H, I
J only
K only
L and M only
M, L and K
3. What is the energy change (ΔE) corresponding to the transition labeled L
A. −2.04 × 10-18 J
B. 4.58 × 10-19 J
C. −3.03 × 10-19 J
D. 3.03 × 10-19 J
E. −4.58 × 10-19 J
4. What is the wavelength of the photon associated with the transition labelled M?
A. 434 nm
B. 657 nm
C. 487 nm
D. 343 nm
E. 103 nm
5. How many different energy levels (i.e. subshells) does the principal level marked D split into for a multielectron atom?
A. 5
B. 3
C. 4
D. 2
E. 1 (It doesn’t split.)
Chemistry 101, Mid-Term Test 1
Version B
Fall 2015
Page 3 of 5
Questions 6-9 relate to the following set of probability density plots for some orbitals (cross-section through
nucleus).
A
B
C
D
E
6. Which of the above orbitals have no node at the nucleus?
A. A
B. B
C. E
D. B and E
E. A, C and D
7. Which of the orbitals above has an angular momentum quantum number of l = 2?
A. A
B. B
C. E
D. B and E
E. A, C and D
8. Which of the above orbitals have a principal quantum number of n = 2?
A. A
B. B
C. C
D. D and E
E. A, C and D
9. Which of the orbitals above represents a p orbital?
A. A
B. B
C. C
D. D
E. E
10. Which of the following orbitals has the fewest nodes?
A. 3d
B. 4s
C. 5p
D. 4d
E. 4f
11. How many electrons in a tin (Sn) atom have a principal quantum number of n = 3 and a magnetic
quantum number of ml = +1?
A. 2
B. 3
C. 4
D. 6
E. 18
12. The 1s electrons in a gold (Au) atom move at a large fraction of the speed of light, in fact at
approximately 1.74 × 108 m s−1. Assume that the uncertainty in this velocity is 2% . How precisely can their
position be estimated ( in picometers)? ( 1 pm = 10-12 m)
A. 0.19 pm
B. 17 pm
C. 1.7 pm
D. 1.7 × 108 pm
E. 0.33 pm
Chemistry 101, Mid-Term Test 1
Version B
Fall 2015
Page 4 of 5
13. What neutral ground state atom has the electronic structure 1s2 2s2 2p6 3s2 3p6 4s1 3d 5 ?
A. Cu
B. Ni
C. Zn
D. Cr
E. Co
14. If each cell represents an orbital, which of the following is a violation of the Pauli Exclusion Principle?
Answer C
A
B
C
D
E
15. If each cell represents an orbital, which of the above electron configurations violate(s) Hund’s rule?
A. C only
B. A and C only
C. A and C and E
D. A and E only
E. A and C and D
16. Which of the following is NOT a correct ground state electron configuration?
A. Al = [Ne] 3s2 3p1
B. In = [Kr] 5s2 4d10 5p1
C. H = 1s1
D. Ba = [Xe] 6s2
E. Se = [Ar] 4s2 3d10 4p3
17. What is the correct electronic configuration for the Bi3+ ion?
A. [Kr] 5s2 4d 10 5p 2
B. [Kr] 6s2 5d10
C. [Xe] 6s25f145d10
D. [Xe] 6s2 4f 14 5d 10
E. [Xe] 5f 14 5d 10 6p 2
18. If A > B means the atomic radius of A is greater than that of B, which of these pairs of elements is in the
WRONG order with respect to their relative size?
A:
Ar > Si
B:
Mg > S
C:
Bi > S
D:
I > Cl
E:
Zr > Ru
19. Which element from the set below has the largest negative (most favorable) electron affinity?
A. K
B. Ca
C. Ga
D. Ge
E. As
Chemistry 101, Mid-Term Test 1
Version B
Fall 2015
Page 5 of 5
20. Element Z is directly below element X in the periodic table. Which of the following statements are
CORRECT? Students were told to cross out response B and select from the remaining four.
i)
The cation X+ is smaller than the cation Z+
ii)
Z has a larger bonding atomic radius than X
iii)
Z and X have the same number of core electrons
iv)
Z has a greater ionization energy than X
A. ii and iv
B. i and ii
C. i and iii
D. ii and iii
E. i and ii
21. Which of these neutral atoms has an INCORRECT Lewis symbol? Answer E
22. Based on relative electronegativities, which of these is the MOST polar bond?
A. F-F
B. Si-F
C. Cl-Cl
D. Si-I
E. P-F
23. Which of these ionic compounds would have the largest lattice energy?
A. BaS
B. SrSe
C. CaF2
D. MgS
E. MgSe
24. In using a Born-Haber analysis to determine how exothermic is the formation of MgF2 (s) from
magnesium metal and fluorine gas (F2), we need to know the heat of atomization (vaporization) of
magnesium, the heat of atomization of fluorine (i.e. the bond dissociation energy of F2), the first and second
ionization energies of magnesium, the lattice energy of MgF2 (s), and what other quantity?
A.
B.
C.
D.
E.
The electronegativities of both Mg and F
The electrostatic force between M2+ and F–
The Mg-F bond enthalpy (i.e. bond energy)
The electron affinity of fluorine
The dipole moment of the Mg-F bond
25. Which ion is the largest?
A. Se2–
B. Br–
C. Rb+
D. Sr2+
END
E. Y3+