Name:_____________________ Student number:________________________
問答題
1)
Write the Lewis structures (including lone pairs if any) for the following
compounds and predict their geometry. (6 x 2 pts)
(a) ICl3
(b) TeF4
Cl
I
F
Cl
F
F
Cl
T 字型
Te
F
蹺蹺板型
(d) N3-
(c) XeCl4
Cl
-
Cl
Cl
Xe
N
N
N
Cl
square planar
(e) SO2Cl2
linear (isoelectronic to O=C=O)
(f) XeO2Cl2
Cl
O
O
Cl
Xe
S
O
O
Cl
Cl
蹺蹺板型
tetrahedral
2)
Name the following coordination compounds:
(2 x 4 pts)
(a) [Co(NH3)6]Cl2
hexaamminecobalt(II) chloride
(b) [Co(NH3)5Cl]Cl2
pentaamminechlorocobalt(III) chloride
(c) Na3[Co(CN)6]
sodium hexacyanocobaltate(III)
(d) K4[PtCl6]
potassium hexachloroplatinate(II)
1
3) Draw the structures of each of the following. (2 x 2 pts)
(a) cis-dichloroethylenediamineplatinum(II)
Cl
NH2
CH2
Pt
Cl
NH2
CH2
(b) trans-dichlorobis(ethylenediamine)cobalt(II)
Cl
H2C
H2N
NH2
H2C
Co
H2N
CH2
CH2
NH2
Cl
4)
Amino acids can act as ligands toward transition metal ions. The simplest amino
acid is glycine (NH2CH2CO2H). Draw a structure of the glycine anion
(NH2CH2CO2-) acting as a bidentate ligand. Draw the structural isomers of the
square planar complex Cu(NH2CH2CO2)2. (2 + 4 pts)
N
H
N
O
Cu
H N C C
H
O
H
O
O
N
O
N
O
Cu
O
5)
N
Draw the geometrical isomers of the complex ion [Cr(en)(NH3)2I2]+. Are there
any optical isomers? Draw also the structures of optical isomers if they exist.
(6 pts)
(1)
NH
I
3
(2)
I
H3N
N
N
Cr
Cr
I
H3N
N
N
NH3
NH3
H3N
(3)
NH3
N
N
Cr
I
CH2
H2N
I
NH3
N
I
I
mirror
N
Cr
I
I
N
NH3
Cr
N
NH2
CH2
H3N
N
I
2
N
單選題：（每題 2 分）
1. How many of the following molecules possess dipole moments?
BH3, CH4, PCl5, H2O, HF, H2
a) 1
b) 2
c) 3
d)
4
e)
5
2. Which of the following has the smallest radius?
a)
Br– b)
S2-
c)
Xe
d)
Ca2+
e)
Kr
3. Which of these is an isoelectronic series?
a)
d)
Na+, K+, Rb+, Cs+
Li, Be, B, C
b)
e)
K+, Ca2+, Ar, S2c)
none of these (a-d)
Na+, Mg2+, S2-, Cl-
4. Calculate the lattice energy for LiF(s) given the following:
sublimation energy for Li(s)
+166 kJ/mol
a)
d)
Hf for F(g)
+77 kJ/mol
first ionization energy of Li(g)
+520. kJ/mol
electron affinity of F(g)
–
328 kJ/mol
enthalpy of formation of LiF(s)
–
617 kJ/mol
285 kJ/mol
–
1047 kJ/mol
b)
–
650. kJ/mol
c)
e) None of these
800. kJ/mol
5. Which of the following statements concerning lattice energy is false?
a)
b)
c)
d)
e)
It is often defined as the energy released when an ionic solid forms
from its ions.
MgO has a larger lattice energy than NaF.
The lattice energy for a solid with 2+ and 2–ions should be two times
that for a solid with 1+ and 1–ions.
MgO has a larger lattice energy than LiF.
All of these are true.
6. Using the following bond energies
Bond
CC
C–H
O=O
C=O
O–H
Bond Energy (kJ/mol)
839
413
495
799
467
3
estimate the heat of combustion for one mole of acetylene:
C2H2(g) + (5/2)O2(g)  2CO2(g) + H2O(g)
a) 1228 kJ
b) –1228 kJ
c) –447 kJ
d) +447 kJ
e) +365 kJ
7. As indicated by Lewis structures, which of the following would probably not
exist as a stable molecule?
a)
CH3OH
b)
CH2O
c)
CH3O
d)
C2H2
e)
C3H4
8. Complete the Lewis structure for the molecule:
This molecule has __________ single bonds and __________ multiple bonds.
a)
4, 2
b)
6, 3 c)
11, 5
d)
11, 2
e)
13, 0
9. What type of structure does the XeOF2 molecule have?
a)
d)
pyramidal
b)
trigonal planar
tetrahedral
c)
e) octahedral
T-shaped
10. The hybridization of the phosphorus atom in the cation PH2+ is:
a)
sp2
b)
sp3
c)
dsp
d)
sp
e)
none of these
11. The hybridization of the central atom in XeF5+ is:
a)
sp
b)
sp2
c)
sp3
d)
dsp3
e)
d2sp3
12. What is the bond order of C2+?
a)
0
b)
1/2
c)
1
d)
1 1/2
e)
2
13. Which of the following molecules has a bond order of 1.5?
a)
O2+
b)
N2
c)
O2–
d)
C2
e)
none of these
4
14. Which of the following statements about the species CN–is false?
a)
It is paramagnetic.
b)
c)
It has two bonds. d)
The total number of electrons is 14.
All of these are true.
15. Which of the following has the shortest bond length?
a)
O22–
b)
O2
c)
O2–
d)
O2+
16. The balanced equation for the reaction of bromate ion with bromide in acidic
solution is given by:
–
BrO3
+ 5Br–+ 6H+  3Br2 + 3H2O
At a particular instant in time, the value of –[Br–]/t is 2.0 10–3 mol/L 
s.
What is the value of [Br2]/t in the same units?
a)
d)
1.2 10–3
3.3 10–5
b)
e)
6.0 10–3
2.0 10–3
c)
3.3 10–3
17. The following data were obtained for the reaction of NO with O2.
Concentrations are in molecules/cm3 and rates are in molecules/cm3 s.
[NO]0
1 
1018
2 
1018
3 
1018
1 
1018
1 
1018
[O2]0
Initial Rate
1 
1018
1 
1018
1 
1018
2 
1018
3 
1018
2.0 1016
8.0 1016
18.0 1016
4.0 1016
6.0 1016
Which of the following is the correct rate law?
a)
d)
Rate = k[NO][O2]
Rate = k[NO]2
b)
e)
Rate = k[NO][O2]2 c)
Rate = k[NO]2[O2]2
Rate = k[NO]2[O2]
18–19. The following initial rate data were found for the reaction
2MnO4–+ 5H2C2O4 + 6H+  2Mn2+ + 10CO2 + 8H2O
[MnO4–]0
1 
10–3
2 
10–3
2 
10–3
2 
10–3
[H2C2O4]0
[H+]0
1 
10–3
1 
10–3
2 
10–3
2 
10–3
1.0
1.0
1.0
2.0
Initial Rate (M/s)
2 10–4
8 10–4
1.6 10–3
1.6 10–3
18. Which of the following is the correct rate law?
a)
c)
e)
Rate = k[MnO4–]2[H2C2O4]5[H+]6
Rate = k[MnO4–][H2C2O4][H+]
Rate = k[MnO4–]2[H2C2O4]2
b)
d)
Rate = k[MnO4–]2[H2C2O4][H+]
Rate = k[MnO4–]2[H2C2O4]
5
19. What is the value of the rate constant?
a)
d)
2 105 M s–1
200 M–2 
s–1
b)
e)
2 105 M–2 s–1
2 10–4 M s–1
c)
200 M–1 
s–1
20–21. The reaction
2NOBr  2NO + Br2
exhibits the rate law
[NOBr]
Rate = k[NOBr]2 = –
t
where k = 1.0 10–5 M–1 
s–1 at 25
C. This reaction is run where the initial
concentration of NOBr ([NOBr]0) is 1.00 10–1 M.
20. What is one half-life for this experiment?
a)
d)
5.0 10–1 s
1.0 106 s
b)
e)
6.9 104 s
c)
none of these
1.0 10–5 s
21. The [NO] after 1.00 hour has passed is
a)
d)
3.5 
10–4 M
1.0 
10–3 M
b)
e)
9.9 
10–3 M c)
none of these
9.7 
10–3 M
22. In 6 M HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products.
The reaction is first order in Ru(NH3)63+ and has a half-life of 14 hours at
25
C. Under these conditions, how long will it take for the [Ru(NH3)63+] to
decrease to 12.5% of its initial value?
a)
d)
28 hours
14 hours
b)
e)
35 hours
42 hours
c)
2.7 hours
23. The decomposition of ozone may occur through the two-step mechanism
shown:
step 1
O3  O2 + O
step 2
O3 + O  2O2
The oxygen atom is considered to be a(n)
a)
d)
reactant b) product c)
reaction intermediate
e)
catalyst
activated complex
6
24. Using the following information determine the activation energy for the
reaction shown here:
2NO  N2 + O2
a)
d)
Temperature (K)
Rate Constant
(L/mol 
s)
1400
1500
0.143
0.659
3.2 104 J/mol
6.8 105 J/mol
b)
e)
9.5 106 J/mol
2.7 105 J/mol
c)
2.8 104 J/mol
25. If the concentration of the product were to double, what would happen to the
equilibrium constant?
a)
b)
c)
d)
e)
It would double its value.
It would become half its current value.
It would quadruple its value.
It would not change its value.
It would depend on the initial conditions of the product.
26. Determine the equilibrium constant for the system N2O4
2NO2 at
25
C. The concentrations are shown here: [N2O4] = 4.27 10–2 M, [NO2] = 1.41
10–2 M
a)
0.33
b)
3.0
c)
0.66
d)
0.05
e)
0.0047
27. At 500.0 K, one mole of gaseous ONCl is placed in a one-liter container. At
equilibrium it is 9.0% dissociated according to the equation shown here:
2ONCl
2NO + Cl2
Determine the equilibrium constant.
a)
d)
4.4 10–4
2.2 10–4
b) 2.2 102
e) 9.1 10–1
c)
1.1 102
28. Initially 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter
container and the following reaction then occurred:
3H2(g) + N2(g)
2NH3(g)
The equilibrium concentration of NH3(g) = 0.68 moles/liter at 700
C. The
value for K at 700
C for the formation of ammonia is:
a)
d)
3.6 10–3
5.0 10–2
b)
e)
1.4 10–1
c)
none of these
1.1 10–2
7
29. Ammonia is prepared industrially by the reaction:
N2(g) + 3H2(g)
2NH3(g)
For the reaction, H= –
92.2 kJ and K (at 25
C) = 4.0 108. When the
temperature of the reaction is increased to 500
C, which of the following is
true?
a)
b)
c)
d)
e)
K for the reaction will be larger at 500
C than at 25
C.
At equilibrium, more NH3 is present at 500
C than at 25
C.
Product formation (at equilibrium) is not favored as the temperature is
raised.
The reaction of N2 with H2 to form ammonia is endothermic.
None of these is true.
30. Which of the following ligands might give linkage isomers?
a)
d)
NO2–
a and b
b)
e)
SCN–
c)
a, b, and c
H2NHC2CH2NH2
31. Which of the following statements concerning the complex ion Co(en)2Cl2+ is
true?
(en = ethylenediamine, NH2CH2CH2NH2)?
a)
b)
c)
d)
e)
The complex ion contains Co(I).
The complex ion exhibits cis and trans geometric isomers, but no optical
isomers.
The complex ion exhibits two geometric isomers (cis and trans) and two
optical isomers.
Since en is a strong field ligand (large ), the complex ion is
paramagnetic.
The geometric isomers of the complex ion have identical chemical
properties.
32. Which of the following complexes can exhibit optical isomerism?
(en = H2NCH2 CH2 NH2 and is bidentate)
a)
b)
c)
d)
e)
cis–Co(NH3)4Cl2
trans–Co(en)2Br2
cis–Co(en)2Cl2
Co(NH3)3Cl3
none of these
8
33. Which of the following coordination compounds will form a precipitate when
treated with an aqueous solution of AgNO3?
a)
b)
c)
d)
e)
[Cr(NH3)3Cl3]
[Cr(NH3)6]Cl3
[Cr(NH3)Cl]SO4
Na3[Cr(CN)6]
Na3[CrCl6]
34. The coordination theory was proposed by:
a)
b)
c)
d)
e)
Bailar
Jorgensen
Blomstrand
Werner
none of these
35. Ethylenediamine (en) is a bidentate ligand. What is the coordination number
of cobalt in [Co(en)2Cl2]Cl?
a)
b)
c)
d)
e)
four
five
seven
eight
six
9