Section # ______ CH 1010 EXAM 2 Fall 2014

Name ______________________________
ID#_______________________
Section # ________
CH 1010 EXAM 2 Fall 2014 - Form A
Fill in your name, ID#, and section on this test booklet. Fill in and bubble in your name, ID# (use “0” for C),
and section on the scantron form. For question #60 mark A. Mark the best answer after reading all possible
choices. Use a #2 pencil and make clean erasures to insure proper scoring. When finished, turn in your scantron
sheet and show this booklet and your CUID to the proctor. Questions worth four points each unless noted
otherewise.
Questions 1-4 are each worth one point.
5. How many pairs of nonbonding electrons are
missing from the structure below?
1. What is the value of x for the polyatomic ion,
SO4x?
A. 1
B. 2
C. 3
D. +1
E. +2
2. What is the value of x for the polyatomic ion,
NO3x?
A. 1
B. 2
C. 3
D. +1
E. +2
3. What is the value of x for the polyatomic ion,
NH4x?
A. 1
B. 2
C. 3
D. +1
E. +2
4. What is the value of x for the polyatomic ion, OHx?
A. 1
B. 2
C. 3
A. 10
B. 12
C. 18
D. 4
E. 5
6. How many grams of nitrogen are there in 7.5 g of
Ca(NO3)2?
A.
B.
C.
D.
E.
0.64 g
1.3 g
0.15 g
2.6 g
2.3 g
7. Atoms with which of the following electron
configurations are readily able to form cations?
I. ns2 np3
II. ns2
III. ns2 np5
D. +1
E. +2
A.
B.
C.
D.
E.
III only
I and II
II and III
I and III
II only
Page 1 of 4
8. Which of each pair is the more polar bond?
Pair I: F—O versus F—B
Pair II: Si—I versus Si—Br
A.
B.
C.
D.
F—O and Si—I
F—B and Si—I
F—O and Si—Br
F—B and Si—Br
9. What is the empirical formula of a compound that
is 62.1 % C, 10.4 % H and 27.5 % O, by mass?
A.
B.
C.
D.
E.
C3HO
C6HO3
C6H12O2
C3H6O
C5H10O2
13. You perform an experiment in which 0.500 g of
Al(OH)3 (78.0 g/mol) react with HCl, according to
the equation below, to yield AlCl3 (133.3 g/mol).
Your laboratory partner weighs the AlCl3 product
and calculates a 90.0 % yield. What mass of AlCl3
was isolated?
Al(OH)3 + 3 HCl  AlCl3 + 3 H2O
A. 1.02 g
B. 0.769 g
C. 0.500 g
14. Which period three element has these successive
first through seventh ionization energies (kJ/mol)?
Ei1 =
578
Ei2 = 1,817
Ei3 = 2,745
Ei4 = 11,575
Ei5 = 14,830
Ei6 = 18,376
Ei7 = 23,293
10. What is the electron geometry and molecular
geometry of IO2?
A.
B.
C.
D.
E.
tetrahedral, trigonal planar
trigonal planar, bent
trigonal pyramidal, linear
linear, linear
tetrahedral, bent
11. Consider the fourth row metals: Ca, Ni, Cr and Zn.
Which form a 2+ cation that has two unpaired
electrons in its ground state?
A.
B.
C.
D.
E.
A.
B.
C.
D.
E.
Mg
S
Cl
Al
P
15. Rank the following angles by increasing size
(smallest to largest bond angle).
Cr and Zn
Ca only
Cr and Ni
Ca and Zn
Ni only
12. A valid Lewis structure of _______cannot be
drawn without violating the octet rule.
A.
B.
C.
D.
D. 0.00579 g
E. 0.855 g
PCl3
SO3
CCl4
ClF3
A.
B.
C.
D.
E.
III < II < I
I < III < II
II < I < III
I < II < III
II < III < I
16. Which of the following is expected to have the
lowest melting point?
A. Na2O
B. MgO
C. Li2O
D. CaO
Page 2 of 4
17. What is the coefficient of H2O when the following
equation is properly balanced with the smallest
whole number coefficients?
__ Al4C3 + __ H2O → __ Al(OH)3 + __ CH4
A.
B.
C.
D.
E.
1
3
4
6
12
18. Which is larger in size of each pair:
Br+ or Br–
A.
B.
C.
D.
Br+
Br+
Br–
Br–
and
and
and
and
21. Which of the following has the strongest C—O
bond?
A.
B.
C.
D.
CO
CO2
CO32
All three have approximately the same C—O
bond dissociation energy.
22. What are the hybridizations of the carbon atoms
labeled C1 and C2, respectively, in the amino acid,
glycine?
; Cs+ or I –
Cs+
I–
Cs+
I–
19. Multiple bonds have been omitted from the
structure below. Add them where appropriate and
determine the number of sigma (σ) and pi (π)
bonds in the molecule.
A.
B.
C.
D.
E.
C1
sp2
sp2
sp3
sp3
sp
C2
sp2
sp3
sp3
sp2
sp
23. For a given arrangement of ions, the lattice energy
increases as ionic radius______ and as ionic
charge _______.
A.
B.
C.
D.
E.
14  & 3 
14  & 5 
12  & 2 
13  & 2 
16  & 3 
20. What mass, in grams, of hydrogen is produced
from the reaction of 4.73 g of Mg with 1.83 g of
H2O?
Mg(s) + 2H2O(l) → Mg(OH)2(s) + H2(g)
A.
B.
C.
D.
E.
0.102 g
0.0162 g
0.0485 g
0.219 g
0.393 g
A.
B.
C.
D.
E.
increases, decreases
increases, increases
decreases, increases
decreases, decreases
this cannot be predicted
24. What is the concentration of a solution made by
dissolving 12.0 g of oxalic acid, H2C2O4
(90.035 gmol–1), in enough water to give
500.0 mL of solution?
A. 0.0666 M
B. 0.133M
C. 0.267 M
D. 0.750 M
E. 1.080 M
25. Which of the compounds listed is best represented
as a resonance hybrid?
A. NO2+
B. H2O
C. HCN
D. SeO2
Page 3 of 4
26. Based on formal charges, which of the following
structures contributes the most to the resonance
hybrid and which contributes the least for N2O?
I
II
III
A. Structure I contributes the most and structure II
contributes the least.
B. Structure II contributes the most and structure
III contributes the least.
C. Structure II contributes the most and structure I
contributes the least.
D. Structure III contributes the most and structure
II contributes the least.
E. Structure III contributes the most and structure
I contributes the least.
27. Based on molecular orbital theory, what is the
bond order of the H-H bond in H2, H2+, and H2
_____ respectively?
For the next two questions, worth 2 points each,
consider the following Lewis Structure.
29. The nitrogen/nitrogen double bond includes a
sigma bond made from the overlap of…
A.
B.
C.
D.
E.
hybridized sp orbitals from both nitrogens.
hybridized sp2 orbitals from both nitrogens.
hybridized sp3 orbitals from both nitrogens.
atomic s orbitals from both nitrogens.
atomic p orbitals from both nitrogens.
30. The nitrogen/nitrogen double bond includes a pi
bond made from the overlap of…
A.
B.
C.
D.
E.
hybridized sp orbitals from both nitrogens.
hybridized sp2 orbitals from both nitrogens.
hybridized sp3 orbitals from both nitrogens.
atomic s orbitals from both nitrogens.
atomic p orbitals from both nitrogens.
60. Mark A on your scantron.
A.
B.
C.
D.
E.
1, 0, 0
1, ½, 0
1, 0, ½
1, ½, ½
1, 2, 0
28. What volume of 0.0183 M barium hydroxide,
Ba(OH)2, is needed to exactly react with 27.8 mL
of 0.0217 M pyrophosphoric acid, H4P2O7?
H4P2O7(aq) + 2Ba(OH)2(aq) → 4H2O(l) + Ba2P2O7(s)
A. 65.9 mL
B. 23.4 mL
C. 132 mL
D. 33.0 mL
E. 46.9 mL
Page 4 of 4
______________________________________________________________________________________________
USEFUL INFORMATION:
NA = 6.0221 x 1023
1 amu = 1.66054 × 1024 g
_______________________________________________________________________________________

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