Sample Exam 2-2 AF
Dr. V. Williamson
FORM D is EXAM II, VERSION 1 (v1)
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DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO.
These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the
answer sheets.
Completely blacken the answer circle. If you change an answer, erase completely the previous
mark.
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be darkened (B for Blue), if it is not, notify your instructor immediately.
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Fill in your ID number. CAREFULLY, blacken the corresponding numbers below.
Fill in the Dept. Course No. and Section. The Dept. = CHEM, the Course No. = 101, and your
section refers to your lab section.
READ THE TEST CAREFULLY. The time limit on this test is 50 minutes.
Mark your answers in this booklet as well as on the answer sheet so you can check your score
with the key after the test.
There are 17 questions. Each of the 16 multiple-choice questions in the first section counts 6
points (96), and there is one multiple-choice question @ 4 pts for a total of 100 points.
Your score will be calculated from the number of correct answers. There is no penalty for
guessing.
Turn in your scan sheet, show your ID, and have your calculator checked by the TA listed on the
overhead for your last name.
A key will be on the electronic class bulletin board at 11:30PM. This is accessed through the class
homepage ( http://chemed.tamu.edu/bb.htm ). The class average will also be posted when it is
confirmed.
IMPORTANT INFORMATION:
F = 1.8 C + 32
l = h/mv
2
2
7 -1
1/ l = -R [(1/nf ) – (1/ni )] and R = 1.097 X 10 m
2
2
∆E = -RH [(1/nf ) – (1/ni )] and RH = 2.18 X 10
c = 3.00 X 108 m/s
h = 6.63 X 10-34 J•s
© Vickie M. Williamson, All Rights Reserved
-18
J
En = -RH /n2
6.02 E23 = Avogadro’s number
Sample Exam 2-2 AF
Dr. V. Williamson
1. Calculate the formula weight (molar mass) of (NH4)2S4O6.
A. 356
B. 242
C. 260
D. 288
E. 63
2. How many grams of oxygen atoms are in 65 g of C2H2O2
A. 22
B. 36
C. 11
D. 18
E. 72
3. What is the mass percentage of hydrogen in aspirin, C9H8O4?
A. 8.96%
B. 0.555%
C. 80.0%
D. 38.1%
4.
Element G reacts with sodium to form an ionic compound with the formula Na2G. Element
G is a member of group?
A. X
5.
B. S
C. R
D. Y
E. Z
A compound containing only carbon, hydrogen, and oxygen is analyzed and found to be
70.6% carbon, 5.9% hydrogen, and 23.5% oxygen. The molecular weight of the compound
is 136. What is the molecular formula?
A. C8H4O
6.
E. 4.48%
B. C4H4O
C. C9H12O3
D. C8H8O2
E. C3H4O
Which of the following is (are) TRUE?
I. 3.56 Å is equal to 3.56 x 10-13 km
II. 20.0 grams of NaOH represents 0.500 moles of NaOH.
III. The length of the bond in HI would be longer that that in HCl.
IV. A single bond is longer than a double bond between the same atoms.
A. I, IV
B. III, IV
C. II, III
D. I, II
E. all are true
D. sp3d
E. sp3d2
7. The hybridization of iodine in IF3 is
A. sp
B. sp3
C. sp2
8. Which is the correct formula/name combination?
A. H2SO3/ sulfuric acid
B. PNO2/ potassium nitrite
C. (NH4)3PO3 / ammonium phosphate
D. CuC2H3O2/ copper (I) acetate
E. PCl3/ phosphorus trichlorate
© Vickie M. Williamson, All Rights Reserved
Sample Exam 2-2 AF
Dr. V. Williamson
9. (4 pts) Which of the following would be most likely to be bonded with covalent bonds?
A. Ca(OH)2
B. CoClO4
C. AuO3
D. C3H6O2
E. NiCO3
10. The geometry or shape of the molecule about the first carbon (the one connected to 2
oxygen) and the nitrogen respectively, in
A. t-shaped and t-shaped
B. square and square
C. tetrahedral and tetrahedral
D. square planar and tetrahedral
E. triangular planar and triangular pyramid
11. The approximate F—Xe—F bond angle between 2 adjacent F in XeF4 is
A. 180°
B. 120°
C. 109°
D. 90°
E. 160°
12. What is the formal charge on the I atom in the IO3- ion?
A. -3
B. +4
C. 0
D. -l
E. +2
13. Which is FALSE?
A. 67.5 g of CaSO4*2H2O is 0.39 moles
B. CuSO4*5H2O is copper (II) sulfate pentahydrate
C. The reason that P can form a +3 ion is that there is stability with a fully filled
s-sublevel.
D. The bond in Br2 is nonpolar.
E. The Lewis dot diagram for the As atom contains 2 pair of dots and 1 single dot.
© Vickie M. Williamson, All Rights Reserved
Sample Exam 2-2 AF
Dr. V. Williamson
14. Which of the following is INCORRECT?
A. Valence Bond theory assumes that covalent bonds are formed when atomic orbitals on
different atoms overlap.
B. Molecular orbital theory describes bonding orbitals (electrons between the two nuclei)
and antibonding orbitals (electrons on the outside of each nuclei)
C. VSEPR theory describes how the geometry of molecules are formed when valence
electron pairs are arranged around the central atom with maximum separation
D. Molecular orbital theory describes how molecular orbitals are formed from atomic
orbitals
E. Molecular orbital theory is used to explain molecular geometry by hybridization of
orbitals.
15. There are ____ σ and _____ π bonds, respectively, in
A. 11 and 2
B. 13 and 4
C. 13 and 0
D. 11 and 4
E. 13 and 2
16. The molecule ZF4 has 1 lone pair of electrons and sp3d hybridization. What would you
predict about the polarity of the bonds and of the molecule?
A. polar bonds,
nonpolar molecule
B. nonpolar bonds,
nonpolar molecule
D. nonpolar bonds,
polar molecule
E. polar bonds,
partially polar molecule
C. polar bonds,
polar molecule
17. The Lewis dot drawing for the IF4- ion has lone pair(s) of electrons around the central atom.
A. 1
B. 0
C. 3
© Vickie M. Williamson, All Rights Reserved
D. 2
E. 5
Sample Exam 2-2 AF
question
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Dr. V. Williamson
Key
6pts each (unless noted)
C
B
E (B=3pts)
A
D (B=3pts)
E
D
D
D=4pts
E
D
E
E
E
E= 4 pts (B,C = 2pts)
C(A,D,E, = 3pts)
D
© Vickie M. Williamson, All Rights Reserved