Chemistry part 40, Julia Burdge,2e (2009) pot

14.81 Since the methanol contains no
oxygen-I
8,
the oxygen atom
must
come
from the phosphate group and not the water.
The
mechanism
must
involve a bond-breaking process like:
o
II
CH-O+P
-
O-H
3 I
O- H
14.83
Most
transition metals have several stable oxidation states. This
allows the metal atoms to act as either a source
or
a receptor
of
electrons
in a broad range
of
reactions. 14.85 (a) Rate = k[CH
3
COCH

3
l[H+l.
(b) 3.8
X 10-
3
M - IS-I. (c) k = k
l
k
2
/L
I
.14.87 (1)
Fe
3+
oxidizes 1- :
2Fe
3+
+
21
- •
2Fe
2+
+ 1
2
; (2) Fe2+ reduces
S
l
O
~-
:

2Fe
l
+ +
S
2
0
~
-
- -

2Fe
3+
+
2S0
~-
;
overall reaction: 2r +
S20
~
-
•. I2 +
2S0
~-
(Fe
3+
undergoes a redox cycle:
Fe
3+
•
Fe

2+
•
Fe
3+
).
The
uncatalyzed reaction is slow because both 1- and
S
2
0
~
-
are negatively
charged which makes their mutual approach unfavorable.
14.89 (a) rate =
k[Al
o
=
k,
[A]
[Al =
-kt
+ [Alo,
slope = k
Time
[Al
o
t
=-"'-
(b) 112

2k.
(c) t =
2t
l/2
' 14.91 There are three gases present and
we
can measure only the total pressure
of
the gases. To measure the partial
pressure
of
azomethane at a particular time,
we
must withdraw a sample
of
the mixture, analyze and determine the mole fractions. Then,
Pa
zo
me
th
ane = Xazome
thane
X P
total
.
14.93
2XG
G
l
+ X l

2EG
Reaction progress
14.95 (a) A catalyst works by changing the reaction mechanism, thus
lowering the activation energy. (b) A catalyst changes the reaction
mechanism. (c) A catalyst does not
change
the enthalpy
of
reaction. (d) A
catalyst increases the forward rate
of
reaction. (e) A catalyst increases the
reverse rate
of
reaction. 14.97
At
very high [Hll, k
l
[H
2
l > > 1 and
,
•
,
ANSWERS
TO
ODD-NUMBERED
PROBLEMS
k
[NOF[H

?l k
rate = I - = 1 [NOF .
At
very low
k
2
[
H
l
l k 2
[H2l, k
l
[H
2
l < < I and
kl[NOF[H
zl
rate =
-'
- -=-
14.99
I
•
:2
2.50,
-

:; ,
:::;;::
Initial Rate vs. Cone.

~
8 2.00
o
-
o
o
- 1.50
x
"
~
'"
1.00
e:::

.,&
0.
50
JL-
r
-
, ,-
-
1
- 0.50 1.00 1.50 2.00 2.50
[Dinitrogen Pentoxide] (M)
AP-
11
rate = k[N
1
0

5
],
k = 1.0 X 10-
5
S - I. 14.101
The
red bromine vapor
absorbs photons
of
blue light and dissociates to form bromine atoms:
Br
l • 2Bf".
The
bromine atoms collide with methane molecules
and abstract hydrogen atoms:
Br·
+
CH
4
•
HBr
+
·CH
3
.
The
methyl radical then reacts with
Br
l, giving the observed product and
regenerating a bromine atom to start the process over again:

·CH
3
+
Br
2 •
CH
3
Br
+ Bf" ,
Bf"
+
CH
4
•
HBr
+
·CH
3
and so on.
14.103 Lowering the temperature would slow all chemical reactions,
which would
be
especially important for those that might
damage
the
brain.
14.105 (a) Rate =
k[X][yf
(
b)

k = 0.019 M -
lS
-
I.
14.107 Second
order,
k = 2.4 X 10
7
M -
I
S - 1 14.109 During the first five minutes
or
so the engine is relatively cold, so the exhaust gases will not fully react
with the components
of
the catalytic converter.
Remember
, for almost all
reactions, the rate
of
reaction increases with temperature. 14.111 (a) Ea
has a large value. (b) Ea =
O.
Orientation factor is not important. 14.113
5.7 X 105
yr.
14.115 (a) Catalys
t:
Mn
2+

; intermediate:
Mn
3+
. First step
is rate-determining. (b) Without the catalyst, the reaction would be a
termolecular
one
involving 3 cations! (Tl+ and two
Ce
4
+)
.
The
reaction
would be slow. (c)
The
catalyst is a homogeneous catalyst because it
has the s
ame
phase
(aqueous) as the reactants. 14.1170.45 atm. 14.119
(a) 6.[Bl/M = kl
[Al
- k2[Bl. (b) [Bl =
(k
l
lk
2
)[Al.
14.121 (a) k =

0.0247 yr-
I
. (b) 9.8 X 10-
4
(c) 186
yr.
14.123 (a) Three steps. (b) Two
intermediates. (c)
The
third step is rate determining. (d)
The
reaction
overall is exothermic.
14.125 1.8 X 10
3
K. 14.127 (a) 2.5 X 10-
5
Mi
s.
(b)
2.5 X 10-
5
Mi
s.
(c) 8.3 X 10-
6
M .
1
14.129
11

= 0,
ti
l?
= C I =
C[Al
o;
-
[Al
o
1
t = C
:-
=
C·
112
[Al
g ,
11
= 1
1
11
= 2, t
ill
=C
[Al
a
14.131 (a) 1.13 X
10-
3
Mlmin.

(b) 6.83 X 10-
4
Mlmin;
8.8 X 10-
3
M.
14.133 Second order,
0.42
I
M·min.
14.135
kl
is 60% larger than k
l
•
Chapter
15
•
15.11 1.08 X
10
7
15.21
(1
) Diagram (a), (2) Diagram (d). Volume
cancels in the
Kc expression.
15.232.40
X 10
33
15.253.5

X 10-
7
15.27 (a) 8.2 X
10-
2
. (b)
0.29.15.29
Kp
= 0.105, Kc = 2.05 X 10-
3
.
15.317.09
X
10-
3
15.33
Kp
= 9.6 X 10-
3
,
Kc = 3.9 X
10
-
4
.15.35
4.0
X 10-
6
15.375.6
X

10
13
15.39
The
equilibrium pressure is less
than the initial
pre
ssure. 15.41 0.173 mol H
2
. 15.43 [H2l = [Brll =
1.80 X
10-
4
M. [HBrl = 0.267 M. 15.45 P
eoCl
, = 0.408
atm
, P
eo
=
AP-12
ANSWERS
TO ODD-NUMBERED PROBLEMS
PC!
, =
0.352
atm. 15.47 P
co
= 1.96 atm, P
co

,
= 2.54 atm. 15.49
The
- -
forward reaction will
not
occur
. 15.55 (a)
The
equilibrium would shift to
the right. (b)
The
equilibrium would
be
unaffected. (c)
The
equilibrium
would
be
unaffected. 15.57 (a) No effect. (b) No effect. (c) Shift to the
left. (d) No effect. (e) Shift to the left. 15.59 (a) Shift to
the
right. (b)
Shift to the left. (c) Shift to
the
right. (d)Shift to
the
left. (e) A catalyst
ha
s no effect on equilibrium position. 15.61

No
change. 15.63 (a) Shift
to right. (b)
No
effect. (c)
No
effect. (d) Shift to left. (e) Shift to the right
[because
NaOH
(
aq
) reacts with
CO
(g) to produce
NaHC0
3
(aq)]. (
f)
Shift
to the left [because
HCl(aq
) reacts
;.'l
ith
CaC0
3
(s) to produce
CO
z(
g)

and other products]. (g)
Shift
to
the
right (the decomposition
of
CaC0
3
is endothermic). 15.65 (a)
20
3
(g) • •
30
2
(g), !:ili0 =
-284.4
kJ.
(b) Equilibrium would shift to the left. 15.67 (a) P 0 = 0.24 atm;
PC!
, = 0.12 atm. (b)
0.017.15.69
(a)
No
effect. (b)
More
CO
2
and H
2
0.

15.71 (a) 8 X 10-
44
. (b) A mixture
of
Hz and Oz can be
kept
at
room
temperature because
of
a v
er
y large activation energy. 15.73 Kp = 1.7,
P
A
= 0.69 atm, P
B
= 0.81 atm. 15.75 1.5 X 10
5
15.77
PH
, = 0.28 atm,
PC!
= 0.051 atm, P
HCI
= 1.67 atm.
15.795.0
X 10
1
atm.

i5.81
0.0384.
,
15.83 328 atm. 15.85 6.3 X 10-
4
15.87 P
N
,
= 0.860 atm.
PH
, = 0.366 atm.
P
NH
=
4.40
X 10-
3
atm. 15.89 (a) 1.16. (b) 53.7%
.15.91
(
it
) 0.49 atm.
3
(b) 0.23 (23%
).
(c) 0.037 (3.7%). (d) Greater than 0.037 mol. 15.93 [H
2
]
= 0.070 M.
[1

2
]
= 0
.1
82 M.
[HI]
= 0.825 M. 15.95 (c) N
2
0 i colorless)
-_.
2N0
2
(brown) is consistent with the observations.
The
reaction is
endothermic so heating darkens
the
color.
Abo
ve 150°C, the O
2
breaks
up into colorless
NO
and O
2
:
2N0
2
(g) •

2NO
(g) + 0
2(
g). An
increase in pressure shifts the equilibrium to the
left
, restoring the color
by producing
N0
2
.
15.97 (a) 4.2 X 10-
4
.
(b) 0.83. (c) 1.1. (d) 2.3 X 10
3
and 2.1
X
lO-
z
.
15.99 (a) Color deepens. (b) Increases. (c) Decreases.
(d) Increases. (e) Unchanged.
15.101
Pota
ss
ium
is
more
volatile than

sodium. Therefore, its removal shifts
the
equilibrium from left to right.
15.1033.6
X 10-
2
15.105 (a) Shifts to the right. (b) Shifts to the right.
(c)
No
change. (d)
No
change. (e)
No
change. (f) Shifts to the left. 15.107
(a) 1.85 X 10-
16
(b) 1.02 X 10-
14
, 1.01 X
10-
7
M.
15.109
P ,
0,
= 0.09
atm, P
NO
,
= 0.100 atm. 15.111 (a) 1.03 atm. (b) 0.39 atm. (c) 1.67 atm.

(d)
0.620- (62.0%
).15.113
(a) Kp = 2.6 X 10-
6
,
Kc =
1.1
X 10-
7
.
(b)
2.2 g, 22
mg/m
3
, yes. 15.115
There
is a temporary dynamic equilibrium
between the melting
ice
cube
s and the freezing
of
water between the
ice
cubes. 15.117 [NH
3
] =
0.042
M, [N

2
]
= 0.086 M,
[H
z] = 0.
26
M .
4
? ?
x-
~
-
15.119 (a)
Kp
= ?
P.
(b)
If
P
incr
ea
ses, the fraction z (and
I-x-
I - x
therefore, x) must decrease. Equilibrium shifts to
the
left to produce less
NO
z
and

more
N
2
0
4
, as predicted. 15.121 P
sop
,
= 3.58 atm, P
so
, = P
C!
,
= 2.71 atm.
15.1234.0.
Chapter
16
16.3 (a) both. (b)
ba
se. (c) acid. (d) base. (e) acid. (
f)
base. (g) neither. (h)
ba
se. (i) acid.
CD
acid. 16.5 (a)
N0
2
.
(b)

HS0
4
.
(c) HS- . (d)
CN
- . (e)
HCOO
-
.16.7
(a)
CH
2
CICOO- .
(b)
10
4
,
(c) H
2
P0
4
. (d)
HPO
~
-
.
(e)
PO
~
-

.
(f) HSO 4' (g)
SO
~
-
.
(h)
10
3
,
(i)
SO
~
-
.
(j)
NH
3
. (k)
HS
- . (1) S2- . (m)
ClO-
.16.17
7. 1 X 10-
12
M. 16.19 (a) 3.00. (b) 13.89. 16.21 (a) 3.8 X
10
-
3
M. (b) 6.2 X 10-

12
M. (c)
1.1
X 10-
7
M. (d) 1.0 X
10-
15
M. 16.23
pH < 7: [H+] > 1.0 X 10-
7
M, acidic;
pH
> 7: [H+] < 1.0 X 10-
7
M,
basic;
pH
= 7: [H+] = 1.0 X 10-
7
M, neutral.
16.252.5
X 10-
5
M. 16.27
0.0022 g. 16.33 (a) - 0.0086. (b) 1.46. (c)
5.82.16.35
(a) 6.17 X 10-
5
M.

(b) 2.82 X
10-
4
M. (c) 0.105 M. 16.37 (a)
pOH
=
-0.093
,
pH
= 14.09.
(b)
pOH
= 0.36,
pH
= 13.64. (c)
pOH
= 1.07,
pH
=
12.93.16.39
(a)
1.1
X 10-
3
M. (b) 5.5 X 10-
4
M. 16.47 (a) Strong. (b) Weak. (c) Weak.
(d) Weak. (e) Strong.
16.492.59.16.515.17.16.534.80
X

10
-
9
.16.55
1.8 X 10-
3
M.
16.576.80.
16.61 6.97 X 10-
7
.
16.63
11.98.16.65
(a) A-
has the smallest
Kb value. (b) B- is the strongest base.
16.692.0
X 10-
5
;
1.4 X 10-
11
; 5.6 X 10-
10
; 2.4 X
10-
8
16.71 (1) c. (2)
band
d.

16.73
1.40 (0.040 M HCI), 1.31 (0.
040
M H
2
S0
4
),
16.75 1.0 X
10-
4
M ,
1.0
X 10-
4
M, 4.8 X 10-
11
M. 16.77 1.00. 16.81 (a) H
2
S0
4
> H2
Se0
4' (b)
H
3
P0
4
> H
3

As0
4
.
16.83
The
conjugate
ba
ses are C
6
H
s
O- from phenol
and
CH
3
0 - from methanol.
The
C
6
H
5
0 - is stabilized by resonance:
0-
o
o
o
• •
•
• • •
The

CH
3
0 -
ion has no such resonance stabilization. A
more
stable
conjugate base means an increase in the strength
of
the acid. 16.89 (a)
Neutral. (b)
Ba
sic. (c) Acidic. (d) Acidic. 16.91
HZ
<
HY
< HX. 16.93
pH
> 7
.16.95
4.
82.16.975.39.16
.101 (a)
Al
2
0
3
<
BaO
< K
2

0.
(b)
Cr0
3 <
Cr
Z0 3 < CrO. 16.103 Al(OH)3(s) +
OW(aq)
• Al(OH)4
(aq), Lewis acid-base reaction.
16.107
AICl
3
(AI
3+
) is a Lewis acid,
Cl
-
is a Lewis base.
16.109
CO
2
,
S0
2, and BCI
3
(other answers are possible).
16.111 (a) Acid
= AlBr3, base =
Br
- . (b) Acid = Cr,

ba
se = CO. (c)
Acid
=
Cu
2
+, base =
CN-
. 16.113 (b) represents a strong acid. (c) represents a
weak
acid. (d) represents a very
weak
acid. 16.115
In
theory, the products
will be
CH
3
COO
- (aq) and
HCI
(aq) but this reaction will
not
occur
to any
mea
surable extent. 16.117
pH
= 1.70, % ionization = 2.26%. 16.119 (c).
16.121 (a)

For
the
forward reaction
NH
~
and
NH
3 are the conjugate acid
and
ba
se pair, respectively.
For
the reverse reaction
NH
3 and NH2 are
the
conjugate acid and base pair, respectively. (b) H+ correspo
nd
s to
NH!;
OH
- corresponds to
NH
2
·
Fo
r the neutral solution,
[NH:]
=
[NH

z
].
[W][A-]
_
16.123 K = , [HA]
""
0.1
M,
and [A ]
""
0.1 M. Therefore,
a
[HA]
K K
K =
[W]
= w and
[OW]
= w. 16.125
1.7
X
1010.
a
[OW]
Ka
16.127 (a)
H-
(basel) + H
2
0 (acid

2
)
•
OH-
(basez) + Hz (acid I) '
(b)
H-
is the reducing agent and H
2
0 is the oxidizing agent. 16.129 2.8 X
10-
2
16.131
PH
3
is a weaker base than
NH
3
. 16.133 (a)
HN0
2
.
(b) HF.
(c)
BF
3
. (d)
NH
3
. (e)

H
2
S0
3
.
(f)
HC0
3
and
CO
j

The
reactions for
(
f)
are:
HC0
3
(aq) + H +(aq) •
CO
z(g) + H
2
0(l),
CO
~
-(aq)
+
2H
+(

aq) •
CO
z(g) + HzO(I). 16.135 (a) trigonal pyramidal.
(b)
H
4
0
2+
does
not
exist
be
cause
the positively charged
H30+
ha
s no
affinity to accept the positive H+ ion.
If
H
4
0
2+
existed, it would
ha
ve
a tetrahedral geometry. 16.137
The
equations are:
Cl

z(g) + H
2
0(l)
• •
HCI(aq)
+
HCIO(aq),
HCl(aq)
+
AgN0
3
(aq).
• AgCl(s) +
HN0
3
(aq).
In
the presence
of
OH
- ions, the first equation is shifted to the
right: H+ (from
HCl
) +
OH
- • H
2
0.
Therefore, the concentration
of

HCIO increases. (
The
'bleaching
action' is due to C
IO
- ions.)
16.13911.80.16.141
(a) 0.181 (18.1 %
).
(b) 4.63 X
10
-
3
.16.1434.26.
16.1457.2
X
10
-
3
g. 16.147
1.000. 16.149 (a)
The
pH
of
the solution
ofHA
would
be lower. (b)
The
electrical conductance

of
the
HA
solution would
be
greater. (c)
The
rate
of
hydrogen evolution from the
HA
solution
would
be
greater. 16.151 1.4 X
10
-
4
16.153 2.7 X 10-
3
g. 16.155 (a)
NH
2 (aq) + H
2
0 (
l)
•
NH
3
(aq) +

OW(aq),
and N
3
-(aq)
+
3H
z
O(l)
-_.
NH
3
(aq) +
30
H- (aq). (b) N
3
- .
16.157
In
inhaling the
sme
lling
salt, s
ome
of
the
powder
dissolves in the basic solutio
n.
The
ammonium

ions react with the base as follows:
NH;
(aq) +
OH
-(aq)
•
NH
3(aq)
+ H
2
0.
It is the pungent
odor
of
ammonia that prevents a person from
fainting. 16.159 (c).
16.16121
mL. 16.163 Mg. 16.165
Both
NaF
and
SnF
2
provide F -
ion
s in solution.
The
F - ions replace
OH-
ions during

the remineralization process
5Ca
2+
+
3Pol
- + F - •
Ca
S(P04)3F
(fluorapatite).
Because
F - is a weaker
base
than
OH
- , fluorapatite is
more resistant to attacks by acids compared to hydroxyapatite.
Chapter
17
17.5 (a) 2.57. (b)
4.44.17.9
(c) and (d). 17.11 8.89.
17.130.024.17.15
0.58.17.179.25
and
9.18.17.19
Na
2A1NaHA. 17.21 (1)
a,
b, and
d;

(2) a
(highest concentration
).
17.27202
g!mol.
17.290.25
M. 17.31 (a) 1.10 X
10
2
g/mol. (b) 1.6 X 10-
6
.1
7.335.82.17.35
(a) 2.87. (b) 4.56. (c) 5.34.
(d) 8.78. (e)
12.10. 17.37 (a) Cresol red
or
/phenolphthalein. (b)
Most
of
the indicators in Table 17.3 are suitable for a strong acid-strong base
titration. Exceptions are th
ymo
l blue and. to a les
ser
extent, bromophenol
blue and methyl orange. (c) Bromophenol blue, methyl orange, methyl
red,
or
chlorophenol blue. 17.39 Red. 17.41 (1) Diagram (c), (2) Diagram

(b), (3) Diagram (d), (4) Diagram (a).
17.49
(a) 9.1 X 10-
9
M. (b) 7.4 X
10
-
8
M.
17.511.8
X
lO
- /l.
17.533.3
X
lO
-93
17.559.52.17.57
Yes.
17.63 (a) 1.3 X
lO
- z
M.
(b) 2.2 X
lO
- 4 M. (c) 3.3 X
lO-
3 M. 17.65
(a) 1.0 X lO-
s

M. (b) 1.1 X 10-
10
M. 17.67 (b), (c), (d), and (e) 17.69
(a)
l.6
X
lO
- z M. (b) 1.6 X
lO
- 6 M. 17.71 Fe(OH)z will precipitate.
17.73 [Cd
2+
] =
1.1
X
lO
-
18
M,
[Cd(CN)~
-
]
= 4.2 X
lO
-3 M,
[CW]
= 0.48 M. 17.75 3.5 X
lO
- s
M.

17.77 (a)
The
equations are as follows:
Culz(s),
• Cuz+(aq) +
2I
- (aq), Cu
2+
(aq) +
4NH
3
(aq) • •
[Cu(NH
3
)4
]
2+(
aq). The ammonia combines with the Cu
2+
ions formed
in
the first step to form the complex ion [Cu(NH
3
)4f+,
effectively removing
the Cu
z
+ ions, causing the first equilibrium to shift to the right (resulting
in
more Culz dissolving). (b) Similar to part (a): AgBr(s) • •

Ag
+(aq)
+
Br
- (aq),
Ag
+(aq) +
2CN
- (aq) • •
[Ag(CNhnaq).
(c) Similar
to parts (a) and (b): HgCl
z(
s).
•
Hg
z+(aq) + 2CI- (aq),
Hg
2+
(aq) +
4Cl
-(
aq)'
•
[HgCI
4
]
z-
(aq). 17.81 At pH values between 2.68 and
8.11, Fe(OH)3 will precipitate but

Zn(OH)z will not.
17.830.011
M.
17.85 Chloride ion will precipitate
Ag
+ but not Cu
2+
. So, dissolve some
solid in
H
2
0 and add HCI.
If
a precipitate forms, the salt was
AgN0
3'
A flame test will also work: Cu
2+
gives a green flame test.
17.872.51
to 4.41. 17.89 1.3
M.
17.91 [Na+] = 0.0835
M,
[HCOO-]
= 0.0500 M ,
[OW]
= 0.0335 M, [H+] = 3.0 X
lO
-13

M, [HCOOH] = 8.8 X
10
-
11
M.
17.93
Most
likely the increase
in
solubility is due to complex ion
formation:
Cd(OH)z(s) +
20H
-
(aq)'
•
Cd(OH
)~-
(aq). This is a
Lewis acid-base reaction. 17.95 (d). 17.97 [Ag+]
= 2.0 X
lO
-9 M,
[Cn
=
0.080 M, [Zn
z+
] = 0.070 M,
[N0
3

]
= 0.060 M
.17.990
.035 gIL. 17.101
2.4
X
lO
-
l3.
17.103 1.0 X
lO
- s M.
Ba(N0
3
) is too soluble to be used
for this purpose. 17.105 (a)
AgBr
precipitates first. (b) [Ag+] = 1.8 X
lO
- 7 M. (c) 0.0018%
.17.1073.0
X
lO-
8 17.109 (a) H+ +
OH
- •
HzO:
K =
l.0
X 10

14
. (b) H+ + NH3 •
NH
~
:
1 1
K = = =
l.8
X 10
9
K 5.6 X
10-
10
•
Broken into two equations:
CH
3
C
OOH
•
CH
3
COO
- + H+: Ka
Broken into two equations:
CH
3
COOH
•
CH

3
COO
- + H+: K.
NH
3 + H+
+.
NH~:
11
K
~
K=
Ka _
1.8x10
-
s
=3.2
x
I0
4
K' 5.6 X 10-
10
•
17.111 (a) 500
mL
of
0.40 M
CH
3
COOH
mixed with 500

mL
of
0.40 M
CH
3
COONa. (b) 500
mL
of
0.80 M
CH
3
C
OOH
mixed with 500
mL
of
0.40 M NaOH. (c) 500
mL
of
0.80 M
CH
3
COONa
mixed with 500
mL
of
0.40 M HCl. 17.113 (a) Increase. (b)
No
change. (c) No change. (d)
pK

.
very large. 17.115 (a) Add sulfate.
Na
2
S04
is soluble,
BaS0
4 is not. (b)
Add
sulfide. K
2
S is soluble, PbS is not. (c)
Add
iodide.
ZnI
2
is solubl
e,
HgI2 is not. 17.117
The
amphoteric
ox
ides cannot
be
used to prepare
buffer solutions because they are insoluble in water. 17.119 The ionized
polyphenols have a dark color. In the presence
of
citric acid from lemon
juice

, the anions are converted to the lighter-colored acids. 17.121
Ye
s.
17.123 (c). 17.125
Precipitation would
be
minimized by decreasing pH.
17.127 At
pH
= 1.0, the predominant species is +NH
3
-CH
2
-COOH.
At
pH
= 7.0, the predominant species is +
NH
3
-CH
z
-COO
- . At
pH
= 12.0, the predominant species is NH
2
-
CH
z
-COO

- . 17.129 (a)
pH
= 4.74.
The
pH
of
a buffer does not change upon dilution. (b) Before
dilution, pH
= 2.52; after dilution,
pH
=
3.02.17.1314.75
.17.133
(a)
The
strongest acid group (with the lowest pK.) ionizes first, followed by
the successively weaker acids. They are, in order:
COOH:
pK
. = 1.82,
ANSWERS TO ODD-NUMBERED PROBLEMS
AP-'
3
NH
+:
pK
. = 6.00,
NH
j :
pKa

= 9.17. (b)
The
dipolar ion is the product
of
the
second
ionization. (c)
pi
= 7.59. (d) The pair
shown
in the second
ionization, since the
pK
a for that pair is closest to the required
pH
of
7.4.
Chapter
18
18.9
The
probability that all the molecules will end up in the same flask
(either the flask on the left
or
the flask
on
the right) is (a) 0.125. (b) 1.95
X
10-
3

(c) 1.24 X
lO
-6o.
The
probability that all the molecules will end
up in one
particular
flask is (a) 0.063. (b) 9
.8
X 10-
4
(c) 6.2 X
lO
-61.
18.11 (a) Negative. (b)
Positive. (c) Positive. (d) Negative. 18.15 (c) < (d)
< (e) < (a) < (b). 18.17 (a) 47.5 JI K . mol. (b) - 12.51
JI
K . mol. (c)
-242
.8 JI
K·
mol. 18.23 (a)
-1139
kJ
I K . mol. (b) - 140.0 kJI K . mo!.
(c) - 2935.0
kJ/K . mol. 18.25 (a) Spontaneous at all temperatures.
(b) Spontaneous below
111

K. 18.27 Fusion: 1.00 X 10
2
JI K . mol,
vaporization: 93.6
JI K . mol. 18.29
-226.6
kJ/mol. 18.31 75
.9
kJ
of
Gibbs free energy release
d.
18.350.35.
18.3779
kJ/mo!. 18.39
(a) 39 kJ/mol, 1 X
lO
-7. (b) 48 kJ/mol. 18.41 (a) 1.6 X
lO
-23
atm.
(b) 0.535 atm.
18.4323.6
rrunHg.
18.4793.
18.49 When Humpty broke into
pieces, he became more disordered
(s
pontaneously). Humpty
couldn't

be
put together again because all the King's horses and a
ll
the King's men
could not reverse the spontaneous process. (Too great a negative entropy
change would have been required.) 18.51
E and
H.
18.53
42
°C. 18.55
(a)
t:.H is positive,
t:.S
is positive,
t:.G
is
negative. (b) t:.H is positive,
t:.S
is positive,
t:.G
is zero. (c) t:.H
is
positive,
t:.S
is positive,
t:.G
is positive.
18.57
t:.S

is positive. 18.59 (a) Trouton's rule is a statement about
t:.S
~.P
(See Equation 18.9
).
In
most substances, the molecules are in constant
and random motion in both the liquid and gas phases, so
t:.S
~
ap
=
90
J/mol·K. (b)
But
in ethanol and water, there is less randomness
of
the molecules
due
to the network
of
H -bonds, so
t:.S
~a
p
is greater. 18.61
(a)
2CO(g) +
2NO(g)
• 2CO

z
(g) + Nz(g). (b)
CO
is the reducing
agent.
NO
is the oxidizing agent. (c) 3 X
lO
120.
(d) 1.2 X
lO1
4, reaction
proceeds to the right. (e) No.
18.632.6
X
10
-
9
18.65 703°C.
18.6738
kJ .
18.69174
kJ
/mol. 18.71 (a) Positive. (b) Negative. (c) Positive.
(d) Positive.
18.73625
K. We assume that t:.Ho and
t:.S
o do not depend
on temperature. 18.75

No
. A negative
t:.G
o tells us that a reaction has the
potential to happen, but gives no indication
of
the rate. 18.77 (a)
- lO6.4 kJ/mol, 4 X 10
18
(
b)
- 53.2 kJ/mol, 2 X
lO
9.
18.79 Talking
involves various biological processes (to provide the necessary energy)
that lead to
an
increase in the entropy
of
the universe. Since the
overall process (talking) is spontaneous, the entropy
of
the universe
must increase. 18.81 (a) 86.7
kJ
/mol. (b) 4 X 10-
31
. (c) 3 X
lO

-7
(d)
Lightning supplies the energy neces
sa
ry to drive this reaction, converting
the two most abundant gases in the atmosphere into
NO(g). The NO gas
dissolves
in the rain, which carries it into the soil where it is converted into
nitrate and nitrite by bacterial action. This
"fixed" nitrogen is a necessary
nutrient for plants. 18.83 673.2
K.18.85
(a) 7.6 X
lO
I4
(
b)
K = 4.1 X 10-
12
18.87 (a) Disproportionation redox. (b) 8.2 X
lOI
S.
(c) Less effective.
18.89
1.
8 X
10
7
0. 18.91

t:.S
sys
= 91.1 J/K,
t:.S
surr
=
-9
1.1
J/K,
t:.S
uni
v
= O .
Conclusion: the system is at equilibrium. 18.93
t:.G
= 8.5
kJ
/mol. 18.95
(a)
CH
3
COOH,
t:.G
o = 27 kJ/mol,
CH
2
CICOOH,
t:.G
o = 16 kJ/mo!.
(b) Entropy dominates. (c) Breaking and making

of
specific
0-
H bond
s.
Other contributions include solvent separation and ion solvation.
(d)
The
CH
3
COO
- ion, which is smaller than the
CH
zClCOO- ion,
can participate in hydration to a
greate
~
extent,
leading to more ordered
solutions. 18.97
Xeo
, = 0.55 X
eo
= 0.45.
18.99249
J/K. 18.101 3 X
- 13 -
10
s. 18.103
t:.S

sys
= - 327 JI K . mol,
t:.S
surr
= 1918 JI K . mol,
t:.S
lIni
v
= 1591 JI K . mol. 18.105 q and
ware
not state functions. 18.107
t:.G,
t:.S
, and t:.H are all negative. 18.109 (a) S = 5.76 J/K(mol. (b)
The
fact
that the actual residual entropy is 4.2
J/K(mol means that the orientation
is not totally random. 18.111
t:,.H
0 = 33.89
kJ
/mol,
t:.s
o = 96.4 J/
mol'K
,
t:.G
o = 5.2
kJ

/mo!.
Chapter
19
19.1 (a) 2H+ + HzO
z
+ 2Fe
2+
• 2Fe
3
+ + 2H
2
0.
(b
) 6H+ +
2HN0
3
+
3Cu • 3Cu
2+
+
2NO
+
4H
2
0.
(c) H
2
0 +
2Mn0
4

+
3CN
- •
AP-14
ANSWERS
TO ODD-NUMBERED PROBLEMS
2Mn0
2 +
3CNO
- +
20
H- . (d)
60
H- + 3
Br
2 •
Br0
3
+
3H
2
0 +
5Br- . (e)
2SzO
~
-
+ 12 •
S
4
0

~-
+
21
- . 19.11
3Ag
+(
l.0
M)
+ Al(s)
-_.
3Ag(s) + AlH (
l.O
M),
E
~ell
= 2.46
V.
19.13 CI
2
(g) and
Mn0
4
(aq).
19.15 (a) Spontaneous. (b)
Not
spontaneous. (c)
Not
spontaneous. (d)
Spontaneous. 19.17 (a) Li. (b) H
2

. (c)
Fe
2+
. (d)
Br
- .
19.213
X 10
54
19.23 (a) 2 X 10
18
(b) 3 X 10
8
.
(c) 3 X 10
62
. 19.25 -
81
kJ, 2 X 10
14
19.29 1.09
V.
19.31
E
~ell
= 0.76
V;
E
eel!
= 0.78

V.
19.33 6.9 X 10-
38
19.39
l.09
V.
19.43 12.2 g Mg. 19.45 It is less expensive to prepare 1 ton
of
sodium by electrolysis.
19.470.012
F.
19.495.33
g Cu, 13.4 g
Br
2'
19.517.70
X 10
3
C. 19.53
l.
84 kg/h.
19.5563.3
g/mol.
19.5727.0
g/
mol.
19.63 (a) (i) H
2
(g) •
2H

+(aq) +
2e
- ;
Ni
2+(aq) +
2e-
• Ni(s);
(ii)
Hz(g) + Ni
2+
(aq) •
2H
+(aq) + Ni(s); (iii)
Re
action will proceed
to the left. (b) (i)
2Cqaq
) • Clz(g) +
2e-;
5
e-
+ 8H +(aq) +
Mn0
4
(aq) •
Mn
2+(aq) +
4H
2
0(l);

(ii)
l6H
+(a
q) +
2Mn0
4
(a
q) +
lOC
qaq)
•
2Mn2+(aq)
+ 8H
2
0
(l)
+ 5CI
2
(g); (iii)
Re
action will
proceed to the right. (c) (i) Cr(s)
•
Cr
H(
aq) +
3e
- ;
Zn
2+

(aq) +
2e
- •
Zn
(s); (ii)
2C
r(s) +
3Z
n2+(aq) •
2Cr
3+(aq) + 3Zn(s),
(iii)
2Cr
H (aq) + 3Zn(s) • 2Cr(s) +
3Zn
2+(
aq
). Reaction will
proceed to the left.
19.650.00
944 g
S0
2'
19.67 (a)
2Mn0
4
+ 6H+ +
5H
2
0

2
•
2Mn
2+
+
8H
2
0
+
50
2
,
(b) 0.0602
M.
19.690.232
mg
Ca/mL
blood.
19.715
X 10-
13
. 19.73 (a) 3.14
V.
(b) 3.13
V.
19.75 E
eeu
=
0.035
V.

19.77 Mercury(I) is Hg
;+
. 19.79 [Mg2+] = 0.0500 M, and
Mg
(s)
+ -
=
l.44
g.
[Ag ] = 7 X 10-» M. 19.81 (a) Hydrogen gas, 0.206 L.
(b) 6.09 X 10
23
e- /
mol
e- . 19.83 (a)
-1356.8
kJ/mol. (b)
1.1
7
V.
19.85
+3
.19.876.8
kJ
/mo
l ,
0.064.19.891.4
A. 19.91
+4.19
.93

l.60
X
10-
19
C
le
- . 19.95 Cells
of
high
er
volta
ge
require very reacti
ve
oxidizing
and reducing agents, which are difficult to handle. Batteries ma
de
up
of
several cells in series are easier to us
e.
19.972
X 10
20
19.99 (a)
E
~ed
for
X is negative (- 0.25 V),
E

~ed
for Y is
po
sitive
(+0
.
34
V). (b)
E
~ll
=
0.59
V.
19.101 (a) Gold does not tarnish in air becau
se
the reduction
potential for oxygen is not sufficiently
po
sitive to result in the oxidation
of
gold. (b) Yes,
E
~ell
= 0.19
V.
(c) 2Au(s) +
3F
2
(g)
•

2A
uF
3(
aq).
19.103 [Fe
2
+] = 0.0920 M, [Fe
H
] = 0.0680 M. 19.105
The
t
wo
h
alf
reactions are: H
2
0
2
(aq) +
2H
+(aq) +
2e
- •
2H
2
0(l),
1.77
V;
H
2

0
2
(aq) • Oz(g) +
2H
+(aq) +
2e
- ,
-0
.68
V.
Overall:
2H
2
0z(aq)
•
2H
2
0
(l)
+ 0
2(g
), EO = 1.09 V
(s
pontaneous). 19.107
(a) Unchanged. (b) Unchanged. (c) Squared. (d) Doubled. (e) Doubled.
19.109 As [H+] increases, F
2
(g)
doe
s beco

me
a stronger oxidizing
age
n
t.
19.111 4.4 X 10
2
atm. 19.113 (a) Half-reaction
s:
1120
2
(g) + 2e - •
0
2
-
(aq), Zn(s) •
Zn
2+(aq) +
2e
- . O
ve
rall:
Zn
(s) +
1I20
z(g) •
ZnO
(s),
E
~ell

= 1.65
V.
(b) 1.63
V.
(c) 4.87 X 10
3
kJ/kg Zn. (d) 64 L
of
air. 19.115
-3.05
V.
19.117 1 X 10-
14
19.119 (a)
3600
C. (b) 105 A·h.
(c)
E
~ell
= 2.01
V,
t1G
o =
-388
kJ/
mol.
19.121 $217
.19.123
-0.03
7

V.
19.125 2 X 10
37
Chapter
20
20.5 (a)
~~
Na.
(b) :
H.
(c) 6 n. (d)
~~
Fe.
(e) __
~
f3.
20.13 2.72 X 10
14
glc
m
3
.
20.15 (a) Nl. (b) Se. (c) Cd. 20.174.85 X 10 L kg. 20.19 (a) 6.30 X
10-
12
J,
9.00 X 10-
13
J/nucleon. (b) 4.78 X 10-
11

J,
1.
37 X 10-
12
J/nucleon.
20.23 (a)
2~~
Th
" )
2~~
Ra
~)
2~~
Ac
~)
2~g
Th.
(b)
2~~U
" )
23
1
Th
90
~
)
231
Pa
91
" )

2~~
Ac.
(
c)
237
Np
")
233
Pa
~)
233
U " )
229
Th
93
91
92
90'
20.254.89
X 10
19
atoms.
20.273.09
X 10
3
y
r.
20.29 A = 0
mol
, B =

0.25
mol
, C = 0, D = 0.75 mol. 20.31 5.5 dpm. 20.33 Mass ratio
UlP
b =
43.3:1. 20.37 (a)
14N(ex,
p)
17
0.
(b) 9
Be
(ex
,n)
12
c.
(c)
238U(
d,2n
)238N
p.
20.39 (a)
4o
Ca(d,p)4ICa. (b)
32
S(n,p
i2
p' (c) 239
Pu
(ex,

n)
242
Cm.
20.41
1§~
Hg
+ 6n ) 1
§6
Hg )
I
j~
Au
+
:p.
20.53
Thef
act that
the radioisotope appears only
in
the 12 shows that the
10
3
is formed only
from the
10
4' 20.55 Add iron-59 to the person's diet, and allow a few days
for the iron-59 isoto
pe
to
be

incorporated into the perso
n's
body. Isolate
red blood cells from a blood sample and monit
or
radioactivity from the
hemoglobin molecules present in the red blood cells.
20.61 3.96 X 10
15
20.63 65.3 y
r.
20.65 70.5 dpm.
2067
(a)
235
U + In
-7
1
4°
Ba
+ 3 In + 93
Kr
•
92
0560
36 '
(b)
235
U + In
-7

144CS
+
90
Rb
+ 2 In
92
0
55
37
0 .
(
c)
235
U + In
-7
8
7
Br
+
146
La + 3 In
92
0
35
57
0 .
(
d)
235
U + In

-7
160
S
m
+
72
Zn + 4 In
92 0
62
30
0 .
20.69 (a)
~
H
-7
_
~
f3
+
~
He
(b)
2~~
Pu
-7
i
ex
+
2~~U
(

c)
13
1
1-7
0
(.)
+
I~I
Xe
53
-1
1-'
)4
(
d)
251
Cf
-7
4
ex
+
247
Cm
98
2
96
.
20.71 Because both Ca and
Sr
belong to Group 2A, radioactive strontium

that has been ingested into the
human
body becomes concentrated in
bone
s (replacing
Ca
) and can damage blood cell production. 20.73
Normally the human body concentrates iodine in the thyroid gland.
The
purpose
of
the lar
ge
doses
of
KI
is to
di
splace radioactive iodine from the
thyroid and allow its excretion from the body.
20.75 (a)
2~~
Bi
+ i
ex
)
2~~
At
+ 2 6n.
(

b)
209
Bi
(ex
2n) 211 At
83'
85
'
20.77 2.77 X 10
3
yr.
20.790.069
%
.20.81
(a) 5.59 X 10-
15
J and 2.84 X
10-
13
J. (b) 0.024 mol. (c) 4.26 X 10
6
kJ. 20.83 2.8 X 10
14
.20.856.1
X
10
23
atoms/mol. 20.87 (a) 1.73 X 10-
12
J.

(b)
The
a particle will move
away fast
er
because it is smaller. 20.89 U-238, t
1/2
= 4.5 X 10
9
yr and
Th-232,
t
ll2
= 1.4 X 10
10
yr.
Th
ey are still present
be
cause
of
their long
half
lives. 20.91 8
.3
X 10-
4
nm. 20.93 3H. 20.95 A small scale chain
reaction (
fi

ssion
of
235
U
).
20.97 2.1 X 10
2
g/mol.
20.99 (a) r = roA
11
3
(ro is a proportionality constant). (b)
1.
7 X 10-
42
m
3
20.101 0.49 rem.
Chapter
21
21.5 X = 3.30 X 10-
4
,
ppm
=
330.21.7
In the stratosphere, the air
temperature
ri
ses with altitude. This warming effect is the result

of
exothermic reactions triggered by
UV
radiation from the sun. 21.11
260 nm. 21.21 3.2 X 10
12
kg 0
3
, 4.0 X 10
37
molecules 0
3
, 21.23
CC4
+
HF • HCl + CFCl
3
(
Freon-II),
CFCl
3
+
HF
•
HCl
+
CF
2
Cl
2

(Freon-12).
21.25479
kJ/
mol
, this is sufficient to break the
C-Cl
bond,
but not enough to break the
C-
F bond.
o.
••
+
:Cl-O-N-O:

II

•
••
••
4
21.27
:0:,
.<;:)
- Q'. 21.39 2.6 X 10 ton
S0
2' 21.41 4.8 X
10
16
kg ic

e.
21.49 5.2 X 10
8
L
S0
2' 21.57 (a) rate = k
[NOf[0
2]' (
b)
rate =
k[NO]
2 (c)
tl
l2 = 1.3 X 10
3
min.
21.594.1
X
10
-
7
atm
, 1 X
10
16
moleculeslL. 21.65 378 g CO. 21.67 Of green house
ga
s, toxic to
humans, attacks rubber;
S0

2: toxic to humans, forms acid rain;
N0
2
:
forms acid rain, destroys ozone; CO: toxic to human
s;
PAN: a powerful
lachrymator, causes breathing difficulties;
Rn: causes lung cancer. 21.69
(a)
Ke =
[0
2
][HbCO]
/
[CO][Hb0
2
]
(b) 4.7 X 10-
2
.21.71
(a)
2N
2
0
+ O
2
+.
4NO and
NO

+ 0
3
•
N0
2
+ O
2
. (b) N
2
0 is a
more
effective
greenhouse
ga
s than
CO
2
because it has a permanent dipole. (c) 3.0 X
10
10
mol.
21.731.
8 X 10
19
,6.4
X 10
16
.21.75
(a) High reactivity
of

the
OH
radical. (b)
OH
has an unpaired electron; free radicals are always
good oxidizing agents.(c)
OH
+
N0
2
•
HN0
3
.
(d) Two reactions:
OH
+
S0
2 •
HS0
3
and
HS0
3
+ O
2
+ H
2
0 • H
2

S0
4
+
H0
2
.
21.77
The
blackened bucket has a large deposit
of
elemental carbon.
When
heated over the burner, it forms poisonous carbon monoxide:
C +
CO
2
• 2CO.
A smaller amount
of
CO
is also formed as follows:
2C
+ O
2
•
2CO. 21.79
The
use
of
the aerosol can liberate CFCs

that
de
stroy the ozone layer. 21.81
C-Cl
=
340
kJ/mol, so the photons
that photolyze
C-Cl
bonds could easily photolyze the
C-
Br
bonds as
well. Light
of
wavelength 409
nm
(visible)
or
shorter will break the
C-Br
bond. 21.83 (
a)
6.2 X 10
8
(b) The
CO
2
liberated from limestone
contributes to global warming. 21.85

Mo
st water molecules contain
oxygen-16, but a small percentage
of
water molecules contain oxygen-
18.
The
ratio
of
the two isotopes in the ocean is essentially constant, but
the ratio in the water va
por
evaporated from the oceans is temperature-
dependent, with the vapor becoming slightly enriched with oxygen-18
as temperature increases.
The
water locked up in ice cores provides a
historical record
of
this oxygen-l8 enrichment, and thus ice cores contain
information about past global temperatures.
Chapter
22
22.11 (a)
+3.
(b)
6.
(c) Oxalate ion. 22.13 (a) Na = +
1,
Mo =

+6
(0
=
-2).
(b) Mg =
+2,
W =
+6
(0
=
-2).
(c)
Fe = 0 (CO
is
a
neutral ligand). 22.15 (a) Cis-dichlorobis(ethylenediamine)cobalt(III).
(
b)
Pentamminechloroplatinum(IV) chloride. (c) Pentamminechlorocobalt
(III) chloride. 22.17 (a)
[Cr(enhClzt
. (b) Fe(CO)s. (c)
Kz[Cu(CNM
(d)
[Co(NH
3
MH
z
O)CI]Cl
z

·
22.23 (a) 2,
. (b) 2,
22.25 (a) 2 geometric isomers (trans- and cis-):
(b)Twoopli'']i'o~,,,
~ ~
22.31 When a substance appears to be yellow, it
is
absorbing light
from the blue-violet, high energy end
of
the visible spectrum. Often
this absorption is
ju
st the tail
of
a strong absorption in the ultraviolet.
Substances that appear green or blue to the eye are absorbing light from
the lower energy red or orange part
of
the spectrum. Cyanide ion is a
very strong field ligand. It causes a larger crystal field splitting than
water, resulting in the absorption
of
higher energy (shorter wavelength)
radiation when a
d electron
is
excited to a higher energy d orbita!.
22.33 (a)

Orange. (b) 255 kJ/mo!. 22.35 2.0 mol, [Co(NH3
)4C
l
z]CI.
22.37
!:J.
would be greater for the higher oxidation state. 22.41 Use a radioactive
label such
as
14CN
- (in NaCN). Add NaCN to a solution
of
K3
Fe(CNk
Isolate some
of
the K3Fe(CN)6 and check its radioactivity.
If
the complex
shows radioactivity, then it must mean that the
CN-
ion has participated
in the exchange reaction. 22.43
CU(CN)2
is
the white precipitate.
It
is
soluble in KCN(aq), due to formation
of

[CU(CN)4]2- , so [Cu
2
+] is
too small for Cu
2
+ ions to precipitate with sulfide.
22.451.4
X
lO
z
.
22.47 The purple color is caused by the build-up
of
deoxyhemoglobin.
When either oxyhemoglobin or deoxyhemoglobin takes up
CO, the
carbonylhemoglobin takes on a red color, the same
as
oxyhemoglobin.
22.49 Mn
3+
. 22.51
Ti
3+
lFe3+. 22.53 1.6 X
10
4
g/mo!. There are
four iron atoms per hemoglobin molecule. 22.55
(a)

[Cr(H
z
O)6]CI
3
,
number
of
ions:
4.
(b) [Cr(HzO)5CI]CI2' H
zO
, number
of
ions:
3.
(c)
[Cr(HzO)4ClzlC
I'2H
zO,
number
of
ions: 2. Compare the compounds
with equal molar amounts
of
NaCI, MgCl
z,
and FeCl
3
in
an electrical

conductance experiment. 22.57
-1.8
X
10
2
kJ/mol, 6 X
10
3
0.
22.59 Iron
is much more abundant that cobalt. 22.61 Oxyhemoglobin absorbs higher
energy light than deoxyhemoglobin. Oxyhemoglobin
is
diamagnetic
(low spin), while deoxyhemoglobin
is
paramagnetic (high spin). These
differences occur because oxygen
(Oz) is a strong-field ligand. 22.63
Zn
z
+, Cu +, Pb
z
+ are
iO
ions; V
5+,
Ca
z
+,

Sc
3
+ are
dO
ions. 22.65 Dipole
moment measurement.
Only the cis isomer h
as
a dipole moment. 22.67
EDTA sequesters metal ions (like
Ca2+
and Mg
2+
) which are essential for
growth and function, thereby depriving the bacteria to grow and multiply.
a"
/b
b"
/a
a"
/c
22.69 Three isomers: Pt
P\
/P\
d/
"c
d/
c d b
22.712.2
X

lO-
zo
M. 22.73 (a) 2.7 X 10
6
(b) A soluble copper(I)
salt could not be isolated from an aqueous solution because it would
disproportionate before it could be crystallized.
Chapter
23
23.13 4.5 X 10
5
.23.15
Ag, Pt, and
Au
will not be oxidized, but the other
meta
ls
will. 23.17 (a) 8.9 X
10
IZ
cm
3
.
(b) 4.0 X 10
8
kg S02' 23.19
AI,
Na,
ANSWERS TO ODD-NUMBERED PROBLEMS AP-15
and Ca would require electrolysis. 23.33 (a) 2Na(s) + 2H

2
0(l)
-
2NaOH(aq)
+ H2(g). (b) 2NaOH(aq) + COz(g) - Na2C03(aq) +
HzO(l). (c) Na
Z
C0
3
(s)
+ 2HCI(aq) - 2NaCI(aq) + CO
2
(g) +
H
2
0(l).
(d)
NaHC0
3
(aq)
+ HCI(aq) - NaCI(aq) + COz(g) +
HzO(l). (e)
2NaHC0
3
(s) -
Na
Z
C0
3
(s)

+ COz(g) + HzO(g).
(f) Na2C03
(S)
- no reaction. Unlike
CaC0
3
(s), Na2C03
(S)
is not
decomposed
by
moderate heating. 23.35 5.59
L.
23.39 First magnesium
is
treated with concentrated nitric acid (redox reaction)
to
obtain magnesium
nitrate: 3Mg(s) +
8HN0
3
(aq) -
3Mg(N0
3
)z(aq)
+ 4H
z
O(l)
+
2NO(g). The magnesium nitrate is recovered from solution

by
evaporation,
dried, and heated in air
to
obtain magnesium
ox
id
e:
2Mg(N0
3
)z(s)
-
2MgO(s) +
4NO
z
(g)
+ 0 2(g). 23.41 The electron configuration
of
magnesium
is
[Ne]3s2 The 3s electrons are outside the neon core
(shielded), so they ha
ve
relatively low ionization energies. Removing the
third electron means separating
an
electron from the neon (closed shell)
core, which requires a great deal more energy. 23.43 Even though helium
and the Group 2A metals have
ns

2
outer electron configurations, helium
has a closed shell noble gas configuration and the Group 2A metals do
not. The electrons in He are much closer to and more strongly attracted
by the nucleus. Hence, the electrons in He are not easily removed. Helium
is
inert. 23.45 (a) CaO. (b) Ca(OH)z. 23.49 60.7
h.
23.51 (a) 1.03
V.
(b)
3.32 X
10
4
kllmo!.
23.53
4AI(N0
3
Ms)
-
2AI
2
0
3
(s) +
12NO
z
(g) +
30
z

(g). 23.55 The "bridge" bonds
in
Al
z
CI
6
break at high temperature:
Al
z
CI
6
(g)
~
2AICI
3
(g
).
This increases the number
of
molecules
in
the gas phase and causes the pressure
to
be higher than expected for pure
A1
z
CI
6
.
23.57

A1
2
CI
6
: each aluminum atom
is
Sp
3 hybridized;
A1CI
3
: the
aluminum atom is
Sp
2 hybridized. 23.59 65.4 glmol (Zn). 23.61 Water
should not be affected by the copper purification process under standard
conditions. 23.63 (a) 1482
kJ. (b) 3152.8
kJ.
23.65 Mg(s) reacts with
Nz(g) to produce
Mg
3N
z(
S)
at high temperatures. 23.67 (a) In water the
aluminum(III) ion causes an increase in the concentration
of
hydrogen ion
(lower pH). This results from the effect
of

the small diameter and high
charge
(3
+ )
of
the aluminum ion on surrounding water molecules. The
aluminum ion draws electrons in the
0-
H bonds to itself, thus allowing
easy formation
of
H+ ions. (b) A1(OH)3 is an amphoteric hydroxide.
It
will dissolve in strong base with the formation
of
a complex ion.
AI(OHMs) +
OW(aq)
- A1(OH)4(aq). 23.69 CaO(s) + 2HCI(aq)
- CaClz(aq)
+ HzO(l). 23.71 Metals have closely spaced energy
levels and a very small energy gap between filled and empty levels. 23.73
NaF: cavity prevention.
(F
- )
LiC0
3
: antidepressant (Li+
).
Mg(OHh:

laxative (Milk
of
Magnesia®
).
CaC0
3
: calcium supplement; antacid.
BaS04: radiocontrast agent. 23.75 Both Li and Mg form oxides (LizO
and MgO). Other Group 1A metals (Na,
K,
etc.) also form peroxides
and superoxides. In Group
lA
, only Li forms nitride (Li3
N)
, like Mg
(Mg
3
N
2
). Li
re
sembles Mg
in
that its carbonate, fluoride, and phosphate
have low solubilities. 23.77 Zn. 23.79 87.66%
Na20 and 12.34% Na202'
23.81 727 atm.
Chapter
24

24.11 Element number
17
is the halogen, chlorine. Since
it
is
a nonmetal,
chlorine will form the molecular compound
HCI. Element 20 is the
alkaline earth metal calcium which will form an ionic hydride,
CaHz. A
water solution
of
HCI is called hydrochloric acid. Calcium hydride will
react according to the equation CaHz(s), +
2H
z
O(I) - Ca(OH)z(aq)
+ 2H
2
(g). 24.13 NaR: ionic compound, reacts with water
as
follows:
NaR(s) + HzO(l) - NaOH(aq) + Hz(g) ; CaR
2
: ionic compound, reacts
with water
as
follows: CaR
2
(s)

+ 2H
2
0(l)
- Ca(OH)z(s) +
2H
z
(g);
CH
4
: covalent compound, umeactive, bums in air or oxygen:
CHig)
+
20
z
(g)
- COz(g) + 2H
z
O(l); NH3: covalent compound, weak
base in water:
NH
3
(aq)
+ HzO(I)
~
NH
; (aq) +
OH
- (aq);
HzO: covalent compound, forms strong intermolecular hydrogen bonds,
good solvent for both ionic compounds and substances capable

of
forming hydrogen bonds; HCI: covalent compound (polar), acts as a
strong acid
in water: HCI(g) + Hz
O(l)
- H30 +(aq) +
CC(aq).
24.15 CaHz(s) + HzO(l) -
Ca(OHMaq)
+
2Hig)
, 22.7 g CaHz.
24.17 CuO(s) + Hz(g) - Cu(
s)
+ HzO(g
).
24.25
~C
=Cp

AP-16
ANSWERS
TO ODD-NUMBERED PROBLEMS
24.27 (a)
2NaHC0
3
(s)
•
Na
2

C0
3
(S)
+ H
2
0(
g)
+
CO
2
(g). (b)
Ca(
OHMaq)
+
CO
2
(g) •
CaC0
3
(s) +
H
2
0(l
).
The
visual
proof
is
the formation
of

a white precipitate
of
CaC0
3
.
24.29 Heat causes
bicarbonates to decompo
se
according to the reaction:
2HCO~
+.
o
COj- + H
2
0 + CO
2
, Generation
of
carbonate ion causes precipitation
of
the insoluble
MgC0
3
. 24.31 The wet sodium hydroxide is first converted
to sodium carbonate,
2NaOH
(a
q) +
CO
2

(g) •
Na2C0
3(aq) +
H
2
0(
I), and then to sodium hydrogen carbonate:
Na
2
C0
3(aq) + H
2
0(l)
+
cO
2
(g) •
2NaHC0
3
(aq). Eventually, the sodium hydrogen
carbonate precipitates (the water
solvr
nt
evaporates since N
aHC0
3
is
not hygroscopic). Thu
s,
most

of
the white solid is
NaHC0
3
plus some
Na2C03' 24.33
Ye
s. 24.39 (a)
2NaN0
3
(s)
•
2NaN0
2
(s) +
0 2(g) . (b)
NaN0
3
(s) + C(s)
•
NaN0
2
(s) +
CO
(g). 24.41
NH
3(g) +
CO
2
(g)

>.
(NH
2
hCO(s)
+ H
2
0 (I) . The reaction should be run at high
pressure. 24.43 The oxidation state
of
N in nitric acid is + 5, the highest
oxidation state for
N.
N can be easily reduced to ox
id
ation state + 3.
24.45 (a) NH
4
N0
3
(s) •
N
2
0(g)
+
2H
2
0(I
). (b)
2KN0
3

(s)
•
2KN0
2
(s) +
02(g)
. (c)
Pb(N0
3
Ms) • PbO(s)
+
2N0
2
(g) + O
zCg)
. 24.47
KN0
3
(s) +
C(s)
•
KN0
2
(s) +
CO
(g), 48.0 g
KN0
2
. 24.49 (a)
D.G

~
=
86.7 kJ/
mol.
(b) K = Kp = Kc = 4 X 10-
31
. 24.51 125 g/
mol,
P
4
.
24.53
4HN0
3
+ P
4
0
lO
•
2N
2
0
S
+
4HP0
3
, 60.4
g. 24.55
Sp
3 24.63

- 198.3
kJ/mol
, K =
Kp
= Kc = 6 X 10
34
24.65 (a) To exclude light. (b)
0.371
L.
24.67 F = - 1,
0=
0.24.69
(a)
HCOOH
(l) . • CO (g) +
H
2
0(I).
(b)
4H
3
PO
il)
. • P
4
0
IO
(S) +
6H
2

0
(l
). (c)
2HN0
3
(l)
+.
=='
N
2
0
S
(g) + H
2
0 (I). (d)
2HCl0
3
(l) • •
CI
2
0
s
(l
) + H
2
0
(l)
. 24.71 To
form
OF

6 there would have to be six bonds (twelve electrons) around the
oxygen atom. This would violate the octet rule. 24.73 35 g
C1
2
.
24.75
9H
2
SOiaq)
+
8Nal(aq)
•
41
2
(s)
+ H
2
S(g) +
8Na
HS0
4
(aq) +
4H
2
0(l).
24.79 (a)
H-
f.: H-
f.: (b) W H-
:f.f

24.81 (a) Linear.
(b) Tetrahedral. (c) Trigonal bipyramidal. (d) See-saw. 24.83
25
.3 L
C1
2
.
24.852.81
L.
24.87 1
2
0
5
(s) +
5CO
(g) •
5C0
2
(g) + 12(s), iodine is
reduced and carbon is oxidized. 24.89 (a)
2H
3
P0
3
(aq) • H
3
PO
iaq)
+
PH

3
(g)
+ 0 2(g) . (b) Li
4
C(s) +
4HCI(aq)
• 4LiCl(aq) +
CH
4
(g).
(c) 2HI(g) +
2HN0
2
(aq) , 1
2
(s)
+
2NO
(g) +
2H
2
0 (I). (
d)
H
2
S(g)
+
2CI
2
(g) •

2HCI(g)
+ SCI
2
(1)
. 24.91 (a)
SiC1
4
.
(b)
F
(c)
F.
(d)
CO
2
, 24.93
O.
24.95 PC!; , tetrahedral,
Sp
3 hybrid
s;
PC1
6
,
octahedra!,
sp
3
d
2
hybrids. 24.97 K

298
= 9.61 X 10-
22
, Km = 1.2 X
10-
15
24.99
The
glass is etched (dissolved) uniformly by the reac
ti
on 6
HF
(aq) +
Si0
2
(s)
+. H
2
SiF
6
(aq) + 2H
2
0 (l). 24.101
1.18.24.1030.
833 gIL. The molar
mass derived from the observed density is 74.41, which suggests that the
molecules are associated to some extent in the gas phase. This makes
sense due to strong hydrogen bonding in HF.
Chapter
25

25.3 The monomer must have a triple bond. 25.5 There are two possible
polymers, but
if
they are long enough, the difference would be negligible:
°
II
H?
N-CH
-C-O
- I
CH?
I -
SH
°
II
HN-CH-C-O
2 I
CH-OH
I
CH
3
° °
H
II
H
II
N-CH-C-O-N
-C
H-C-O
I I

CH-OH
CH
2
I I
CH
3
SH
II
° °
H
II
H
II
N-CH-C
-O
-N
-CH-C-O
I I
CH?
CH-O
H
I - I
SH
CH
3
II
°
H
II
N-CH-C-OH

I
CH-OH
I
CH
3
°
H II
N
-CH-C-OH
I
CH
2
I
SH
25.9 (1)
Sc
(s)
+
2C
2
H
s
OH(l) • Sc(OC
2
H
s
)(alc) + 2H+(alc)
("alc" indicates a solution
in
alcohol); (2) Sc(OC2Hs)(alc) + 2H

2
0(I)
• Sc(OH
Ms)
+ 2C
2
H
s
OH(alc); (3) Sc(
OH
Ms) • ScO(s) +
2H
2
0(g
). 25.11 Bakelite is best described as a thermosetting composite
polymer. 25.15 No. These polymers are too flexible, and liquid crystals
require long, relatively rigid molecules. 25.19 Alternating condensation
copolymer
of
the polyester class. 25.21 Metal amalgams expand with
age; composite fillings tend to shrink. 25.25
sp2 25.27 Dispersion forces.
25.31 (a)
4+
5: n-type. (b)
4+
3:
p-type. 25.35 Bi2Sr2
Cu0
6' 25.37 Two

are
+2
([Ar
]3£),
one is + 3 (
[Ar]3d
8
) .
The
+3
oxidation state is unusual
° °
II
II
for
co
pper. 25.39 H
2N
-fCH
2)8
NH
2
HO-C-fCH:m C-OH
25.41 In a plastic (organic) polymer: covalent, disulfide (covalent),
H-bonds and dispersion forces; in ceramics, mostly ionic and network
covalent. 25.43 Fluoroapatite is less soluble than hydroxyapatite,
particularly
in
acidic solutions. Dental fillings must also be insoluble.
25.45 The molecule is long, flat, and rigid, so it should form a liquid

crystal.
Answers
To
PRE-PROFESSIONAL PRACTICE
EXAM
PROBLEMS
Chapter
1
Chapter
8
Chapter
15
Chapter
22
I.b
I.e
I.b
I.e
2.d
2.a 2.a
2.
a
3.e
3.
a
3.b
3.
b
4.a
4.

b
4.d
4.
b
Chapter
2
Chapter
9
Chapter
16
Chapter
23
I.e
I.e
I.d
1.
e
2.d
2.
b
2.
b
2.d
3.
a
3.
b
3.
a
3.

b
4.
b
4.
d
4.
b
4.a
Chapter
3
Chapter
10
Chapter
17
Chapter
24
l.d
I.e I.e
La
2.b
2.d
2.
e
2.
b
3.b
3.a
3.
a
3.e

4.e
4.e
4.d
4.
b
Chapter
4
Chapter
11
Chapter
18
Chapter
25
La
Lb Ld Lb
2.
b
2.a
2.
b
2.d
3.a
3.
b
3.a
3.
b
4.e
4.d
4.e

4.d
Chapter
5
Chapter
12
Chapter
19
Ld
I.e
Lb
2.a
2.
b
2.e
3.e
3.d
3.d
4.
b
4.a
4.d
Chapter
6
Chapter
13
Chapter
20
I.b
Lb
La

2.a
2.d
2.e
3.e
3.e
3.d
4.e 4.e
4.a
Chapter
7
Chapter
14
Chapter
21
I.b
La
Lb
2.a
2.
b
2.d
3.
b
3.e
3.e
4.d
4.
b
4.a
AP-17

A
absolute entropies, 735, 736
absolute temperature scale, 424
absolute zero,
10,
424
absorbed, 531
acceptor impurities,
890
accuracy, 18-19
acid-base indicators,
698-700
acid-base reactions, 121-122, 125-126
acid-base neutralization, 124
Br¢nsted acids and bases, 122-124
strong acids and bases, 122
acid-base titrations, 144-146, 690-691
acid-base indicators,
698-700
strong acid-strong base titrations, 691-692
strong acid-weak base titrations, 696-698
weak acid-strong base titrations, 693-696
acid ionization constant, 648
acid rain, 838, 843-845
acids
in
molecular compounds, 50,
51
oxoacids, 59
strong, 112, 113, 122

acids and bases, 634-635
acid-base properties
of
oxides and
hydroxides, 667- 668
acid-base properties
of
salt solutions, 662-667
acid-base properties
of
water, 637-639
Br¢nsted, 636-637
conjugate acid-base pairs, 654-657
diprotic and polyprotic acids, 657-659
Lewis acids and bases, 668-670
molecular structure and acid strength,
660-662
pH scale, 639- 644
strong, 644-647
weak acids and acid ionization constants,
647-652
weak bases and base ionization constants,
652-654
actinide series, 225
action potential, 776
activated complex, 564
activation energy, 563
active metals,
130, 258
active site, 575

active transport, 643
activity series,
130,
131
actual yield, 96
addition polymerization, 936
addition polymers, 395-396, 397, 936-941
addition reactions, 386-388
adenosine diphosphate
(ADP), 389
adenosine triphosphate
(ATP), 389
adhesion, 468
adsorbed, 531
aerosol, 845
Agriculture,
U.S. Department
of
, 159
airbag,433
alcohols, 367,
370, 372
aldehydes, 367,
370, 373
aliphatic compound
s,
365
alkali metals, 45,
891
- 893

alkaline batteries, 777
alkaline earth metals, 45, 893-895
alkanes, 51, 52, 365, 368
alkyl group, 366, 367, 368
alkynes, 943
allotropes, 48, 910
alloys, 883
alpha
(a)
particles,
38
alpha
(a)
rays, 38
altitude sickness, 448
aluminum, 895-897
alums, 897
amalgam
defined, 883
dental, 759,
950
amide group, 367, 370
amide ions, 912
amide linkages, 464
amides, 367,
370, 373
amines, 367,
370, 373
amino acid residue, 464
amino acids,

370, 397-399
amino group, 367,
370
ammonia, 912
amorphous solids, 484
amount-volume relationship, 425-426
amphoteric, 266, 637
amplitude, 194
analogues, 363
angular momentum quantum number, 213, 214
anions, 55
anisotropic, 947
Annan, Kofi, 829
anode, 36, 763, 766
antacids, 642- 643
antibonding molecular orbital, 343
aqueous solutions,
506
acid-base reactions, 121-126
Index
aqueous defined, 77
aqueous reactions and chemical analysis,
142-147
concentration of solutions, 136-142
general properties
of
, 112-116
oxidation-reduction reactions, 126-
13
6

precipitation reactions, 117-121
Aristotle, 34
Armstrong, Lance,
73
aromatic compounds, 365
Arrhenius acid, 123
Arrhenius base, 123
Arrhenius equation, 564-565
Arrhenius, Svante, 122
arsenic,
905
artificial joints, 951- 952
ascorbic acid, 33, 635,
671
Aston,
F.
w.,
43
atactic,
941
atmosphere
Earth's, 830-833
phenomena in the outer layers,
83
3- 834
atmospheres (atm), 418
atmospheric pressure, 417
atomic bomb, 812
atomic ions,
55-56

atomic line spectra, 201-202
atomic mass, 46
atomic ma
ss
unit (amu), 46
atomic number
(Z), 40, 239
atomic orbitals, 212, 216, 219
d orbitals and other higher-energy or
bi
tals.
217-218
energies
of
orbitals, 218, 219-220
forbitals,218
hybridization of, 327-334,
351
P orbitals, 217
s orbitals, 216-217
atomic radiu
s,
246-247, 255
atomic
theory,
34-36
atomic weight, 46
atoms, 4
atomic mass scale and average atomic
mass

46-47
atomic number, mass number,
an
d
isOl
ope5_
40-43
atomic theory,
34-36
defined, 36
hydrogen atom,
200- 208, 212
structure of,
36-40
attracti on, 160
1-2
INDEX
attractive forces, 245, 457
Aufbau principle, 221
aurora australis, 833
aurora borealis, 833
autoionization
of
water, 638
average reaction rate
s,
544-546
Avogadro, Amedeo, 425
Avogadro's law,
425-426,

440
Avogadro's number, 82
Axel, Richard, 313
axial, 316
B
•
balanced equations,
77-78
ball-and-stick models (molecular art), 5
Balmer, Johann, 202
band theory, 888
band theory
of
conductivity, 888
conductors,
888-889
semiconductors,
889-890
barometer, 418, 419
base
Br0nsted acids and bases,
122-124
defined, 112
strong acids and bases, 122
base ionization constants, 652
basic oxygen process,
885-886
batteries
defined, 777
dry cells and alkaline, 777

fuel cells,
778-779
lead storage,
777-778
lithium-ion, 778
Becquerel, Antoine, 38
belt
of
stability, 800
bends, the, 438
beta-particle emission,
800-801
beta
(f3)
particles, 39
beta
(f3)
rays, 39
bidentate ligands,
861
bimolecular, 569
binary hydrides,
907-908
binary molecular compounds, 49,
51
biological catalysts,
575-577
biological concentration cells, 776
biological polymer
s,

397-401
biomedical material
s,
949-952
bioterrorism agents, 3, 23
bipolar disorder, 267
birth defects, 363
blackbody radiation, 197
blast furnace, 884, 885
blood, maintaining pH of,
689-690
blood alcohol concentration (BAC), 111
blood doping, 591
blood plasma, 689, 690
body-centered cubic cell, 474
Bohr, Niels, 202
.
Bohr's theory
of
the hydrogen atom,
200-201,
208,212
atomic line spectra,
201-202
line spectrum
of
hydrogen,
202-207
boiling point, 485
boiling-point elevation,

519-520
Boltzmann constant, 729
bomb calorimetry, 175
bond angle, 316, 319
bond dipoles, 321, 322
bond enthalp
y,
286,
300-303,
324
bond length, 285
bond order,
343-344
bonding molecular orbital, 342
bonding theories,
351-353
bone, radioactive, ?65
Born-Haber cycle,
282-283
boron neutron capture therapy (BNCT), 797
Boyle, Robert, 421
Boyle's law,
421-423,
440
Bragg equation, 476
Breathalyzer test,
Ill,
148
breeder reactors, 814
bromine, 927

Br0nsted acids and bases, 123,
636-637
Br
0nsted base, 123
Br0nsted, Johannes, 123
Buck, Linda, 313
buckyballs, 953
buffer, 683
buffer solutions, 683
with a specific pH,
688-689
calculating the pH
of
a buffer,
684-688
buret, 8, 9
bums, 489
burst lung, 415
c
Cade, John, 267
Cade, Mary, 115
Cade, Robert, 114-115
caffeine, 653
calcium,
894-895
calcium ascorbate, 671
calories
caloric content
of
food, 159

calorie (cal) defined, 162
Calorie (Cal) defined, 163
calorimeter,
l7
5
calorimetry
bomb (constant-volume
),
l75-177
constant-pressure,
l72-l74
defined,
171
specific heat and heat capacity,
171
- 172
cancer
drugs, 73
nuclear chemistry in treating, 797
smoking and,
819-820
capillary action, 468
carbides, 910
carbocation, 387
carbohydrates,
80
carbon,
364-365,
910-911
carbon-14, 563, 806

carbon dating, 806
carbon dioxide,
838-842,
848, 911
carbon disulfide, 921
carbon monoxide,
348-349,
848, 911
carbon nanotubes, 953
carbonyl group, 367, 370
carborundum, 910
carboxy group, 367, 370
carboxylic acids, 367, 370, 372, 662
Carothers, Wallace, 397
cast iron, 885
catalysi
s,
573-577
,
616-617
catalyst, 573
Category A agent
s,
3, 23, 298
catenation,
365,910
cathode, 36, 763, 766
cathode ray tube,
36-37
cathodic protection, 785

cations, 55, 56, 714
cell potential, 764
Celsius scale,
10-11, 424
cementite, 886
Centers for Disease Control and Prevention
(CDC), 3, 23
central science, 4
ceramic matrix composites, 946
ceramics,
945-946
Chadwick, James, 40
chain reactions, 396
chalco gens, 45
Charles, Jacque
s,
423
Charles's and Guy-Lussac
's
law,
423-425
Charles's law, 424, 440, 441
Chauvin, Yves, 935
chelating agents, 861
chelation therap
y,
857, 873
chemical analysis, 873
chemical bonding, basic concept
s,

276-277
bond enthalpy,
300-303
Born-Haber cycle,
282-284
comparison
of
ionic and covalent
compounds, 286
covalent bonding,
284-286
drawing Lewis structures, 291
-2
92
e1ectronegativity and polarity,
286-290
exceptions to the octet rule,
296-300
ionic bonding,
279-284
lattice energy, 280-281
Lewis dot symbol
s,
278-279
Lewis structures,
284-285
Lewis structures and formal charge,
292-295
multiple bond
s,

285-286
resonance,
295-296
chemical bonds, 47
chemical change,
15
chemical energy, 160
chemical equation
s,
76
balancing,
77-81
calculations with balanced, 89-91
interpreting and writing,
76-77
chemical equilibrium, 113,
590-591
concept
of
equilibrium,
592-594
equilibrium constant,
594-598
equilibrium expressions,
599-605
equilibrium expressions in problem solving,
606-611
factors that affect,
611-6l7
free energy and,

742-746
chemical formulas, 48
chemical kinetics,
542-543
catalysis,
573-577
dependence
of
reactant concentration on
time,
555-562
dependence
of
reaction rate on reactant
concentration,
551-555
dependence
of
reaction rate on temperature,
562- 568
reaction mechanisms, 568
-573
reaction rates,
544-550
chemical properties,
15
chemical reaction
s,
4, 7
comparison

of
nuclear reactions and, 798
energy changes in, 160-161
chemical reduction, 884
chemistry
defined, 4
study of,
4-6
chemotherapy, 73, 873
chiral, 383
chiral switching, 385
chloralkali process, 923
chlorine,
926-927
chlorofluorocarbons (CFCs), 829, 835, 837-838,
841 , 842
cholesteric, 947
cidofovir, 23
cis isomers, 337, 382, 865
-8
66
cisplatin, 73
Clausius-Clapeyron equation,
470
closed system, 163, 164
closest packing, 475,
478-479
coal, 910
cohesion, 468
coinage metals, 265

colligative properties, 517
collision theory,
562-564
colloids, 530- 532
color,
868-869
combination reaction
s,
98, 133, 134
combustion analysis
of
compounds,
87-88
determination
of
empirical formula, 87
determination
of
molecular formula, 88
combustion reaction
s,
98, 134
common ion effect,
682-683,
705-7l0
complex ion, 710
complex ion formation,
710-712
composite materials, 946
compounds,

6-7.
See also inorganic
compounds; organic compounds
insoluble, 118
ionic, 55,
57-61
, 116,
117-119
molecular, 47,
49
-
51
, 116
,417
percent composition of,
75-76
soluble, 118
compressibility, gas,
440
concentration cells,
775-776
concentration
of
solutions
concentration defined, 136
dilution, 137, 140
molarity,
136-137,
138-139
preparing a solution from a solid,

138-139
solution stoichiometry,
141-142
condensation, 470
condensation polymers,
396-397,
941-944
condensation reactions, 396
condensed structural formulas, 376
condensed structures, 376
conducting polymers,
943-944
conduction band, 954
conductivity,
113-114
conductors,
888-889
conjugate acid, 636
conjugate acid-base pairs,
654-657
conjugate base, 636
conjugate pair, 636
constant-pressure calorimetry, 172- 174
constant-volume (bomb) calorimetry,
175-177
constant-volume calorimetry, 175
-177
constituent elements, 7
constitutional isomerism, 382
constructive interference, 195, 196

conversion factors,
20
coordinate covalent bonds, 297, 858
coordination chemistry,
856-857
applications
of
coordination compounds,
873-874
coordination compounds,
858-864
coordination compounds, defined, 858
crystal field theory,
867-872
naming coordination compounds,
862-864
reactions
of
coordination compounds,
872-873
structure
of
coordination compounds,
864-867
coordination number
s,
473, 861
copolymers, 396, 939
copper, 898
core electrons, 244

con'osion,
784-785
coulomb (C), 289
Coulomb's law, 245, 386,
800
covalent bond,
284
types
of
covalent bonds,
285-286
covalent bonding, 284
covalent compounds, 286, 925
covalent crystals, 482, 483
covalent hydride
s,
908
covalent radiu
s,
246
cowpox, 3
crenation,
524-525
critical
ma
ss, 812
critical pressure, 486, 487
critical temperature, 486, 487
cross-links, 937
Crutzen, Paul, 829

crystal field splitting, 867, 868
crystal field theo
ry
, 867
color,
868-869
crystal field splitting in octahedral
complexes,
867-868
magnetic properties,
869-871
tetrahedral and square-planar complexes,
871
crystal structure, 472
closest packing, 475,
478-479
packing spheres,
473-475
structures
of
crystals,
476-477
types
of
crystals,
480-484
unit cells,
472-473
crystalline solid, 472, 507
cubic cells,

474-475
cubic close-packed (ccp) structure, 478
Cunningham, Orville, 438
curie (Ci
),
818, 847
Curie, Marie, 38
cyanides, 911
INDEX
D
d-block elements, ions of,
253-254
d orbital
s,
330- 334
Dalton, John,
34-36
Dalton's law
of
partial pressures,
434-435,
440,442
dative bond, 297
Davisson, Clinton Joseph, 210
de Broglie hypothesis, 208- 210
de Broglie wavelength,
209
Debye
(D), 289
decomposition reactions, 98, 133- 134

decompression sickness (DCS), 438
definite proportions, law of, 35
degenerate, 221
delocalized bonding,
351-353
delocalized bonds, 352
delocalized electrons, 944
demineralization, 681
Democritu
s,
34, 35
density, 12- 13, 15
dental implant
s,
950
dental pain, electrochemistry of, 759
deoxyribonucleic acid (DNA),
400, 401
deposition, 488
derived units,
12-13
destructive interference, 195,
196,208
detergents, 874
dextrorotatory isomer, 384, 866
dialysis,
505
diamagnetic, 342
diatomic molecule
s,

48
diffraction, electron,
210
diffusion, 444
dilution, 137,
140
dimensional analysis, 20
diodes, 955
dipole-dipole interactions,
462-463
dipole moment,
289-290
dipoles, bond, 321, 322
diprotic acids,
123,657-659
directionality, chemical bonds and, 325
dispersion forces,
465-467
displacement reactions, 130
disproportionation reaction, 134, 917
dissociation, 112, 523, 529
distillation, 887
distribution, 729
diving, 415, 438, 448
donor atoms,
860
donor impurities, 890
doping, 889, 955
double bonds, 285, 336, 338
double-sli experiment, nature

of
light and,
195-196
Douglas, Dwayne, 114-115
drugs
chiral switching in,
385-386
organic chemistry and, 363
single-isomer versions, 385- 386
drunk driving,
III
dry cells, 777
dynamic chemical equilibrium, 113
dynamic equilibrium,
470
1-3
1-4
INDEX
E
Earth
alkaline earth metals, 45, 893-895
atmosphere,
830-833
elements on, 45
eff
ective collision, 562
effective nuclear charge
(Zeff)' 244
effusion, 444, 445
•

Einstein, Albert, 193, 198, 199
,802,8
10
elastomers, 937
electrocardiogram (E
eG
),
776
electrochemistry,
758-759
balancing redox reactions, 760- 762
batterie
s,
777-779
corrosion,
784-785
electrolysis,
780-784
galvanic cells,
763-764
spontaneity
of
redox reactions under
conditions other than standard state,
773-777
spontaneity
of
redox reactions under
standard-state conditions, 77
0-

773
standard reduction potential
s,
7
64-770
electrodes, 763
electrolysis
of
an aqueous sodium chloride solution,
781-782
defined, 780
in metals purification,
887-888
of
molten sodium chloride, 780
quantitative applications of,
782-783
of
water,
780-781
electrolyte solutions,
523-524
electrolytes
in aqueous solutions,
112-114
compounds as, 116
defined, 112
electrolytic cells,
780
electrolytic reduction, 884

electromagnetic spectrum, 194
electromagnetic wave, 195
electromotive force (emf), 764
electron affinity
(EA), 250-251
electron capture, 801
electron configuration
Aufbau principle, 221
defined, 219
energies
of
atomic orbitals in many-electron
systems,
219
-22
0
general rules for writing, 222
Hund's rule,
221-222
Pauli exclusion principle, 220-221
and the periodic table,
223-226
electron density, 212
electron-domain geometr
y,
316-319
defined, 316
electron domains,
314-315
electron spin quantum number,

214-215
electronegativity,
287-290
electronic structure
of
atoms, 193
electrons, 39,
40,
41
diffraction
of
, 210
discovery of,
36-38
free, 203
odd number of,
297-298
in orbitals, 324
electrophile addition, 387
electrophiles, 386
electrospinning, 951
electrostatic energy,
160
elemental iron, 33
elementary reactions,
568-569
elements. See also periodic table
defined, 5, 6
elimination reactions, 394
emission spectra,

200, 20 I, 202
emission spectrum
of
hydrogen, 203,
204-205
empirical formula mass, 75, 87
empirical formulas,
51-52,
53,
54-55
determination
of
, 87
from percent composition,
85
-86
emulsifier/emulsifying agent,
532
enantiomer
s,
383
-3
84, 385-386, 866
end point, 698
endothermic process, 161, 169
entropy changes, 734
ionic bonds, 279
in solution-formation,
507
endpoints, 144

energy
defined,
160
energy changes in chemical reaction
s,
160 161
forms of, 160
ionization energy, 247
-249
nuclear binding energ
y,
801-803
quantization
of
, 197
-198
in solution formation,
508-509
units
of
, 161-163
English unit
s,
8
enthalpy
bond, 286,
300-303,324
defined, 168
and enthalpy changes, 168
-169

reac
ti
ons under constant-volume or
constant-pressure conditions, 167-168
thermochemical equations,
169-1
71
enthalpy
of
reaction
s,
169
entropy,
508,
724-726
defined, 726
entropy changes in a system,
730 733
entropy changes in the surroundings,
734-73
5
living systems in, 725
microstates,
727-729
probabilit
y,
726-727
standard,
729-730
third law

of
thermodynamic
s,
735-736
environmental chemistry,
828-829
acid rain,
843-845
depletion
of
ozone in the stratosphere,
835-838
Earth's atmosphere,
830-833
greenhouse effect,
838-843
indoor pollution,
846-848
phenomena in the outer layers
of
the
atmosphere,
833-834
photochemical smog,
845-846
volcanoe
s,
838
Environmental
Protection Agency (EPA

),
847
enzymes, biological catalysts,
575-577
equatorial, 316
equilibrium.
See also chemical equilibrium
concepto~
592-594
defined, 592
and tooth decay, 681
equilibrium constants
calculating,
595-597
defined,
594-595
magnitude
of
the, 598
units in, 622
equilibrium expressions, 594, 599
calculating equilibrium concentrations,
607-611
containing gases,
603-604
heterogeneous equilibria,
599-600
manipulating,
600-602
predicting the direction

of
a reaction, 606- 607
in problem solving,
606-6ll
equilibrium process, 733
equilibrium va
por
pressure, 470
equivalence point
s,
144
erythrocytes,
689-690
esters, 367, 370, 372
ethyl group,
370
ethylene, 749
evaporation,
469-470
exact number
s,
15
excess reactants, 92
excited state,
203
exothermic process, 161
entropy changes, 734
ionic bonds, 279
in solution-formation,
507

expanded octets,
298-300
extensive propertie
s,
15
F
f orbital
s,
218
face-centered cubic cell, 474
factor-label method,
20
Fahrenheit, Daniel Gabriel,
11
Fahrenheit temperature scale,
11
families, in periodic table, 44
Faraday constant, 771
Faraday, Michael, 782
fat soluble vitamins,
509-5ll
ferromagnetic metals, 883
ferrous sulfate, 33
. .
first law
of
thermodynamics,
164-165,725
first-order reactions,
555-556

fi
ssion, 811
flotation, 883
fluoresce, 38
fluoride, 533, 716
fluorine,
921-922
fluoroapatite, 716
Food and Drug Administration (FDA),
U.S.,
23,63,159,267,363,402
food labels, 159
formal charge,
292-295
.
formaldehyde, 848
formation constants
(Kf), 710-
711
formic acid, 49
formula mass,
74
formula weight, 74
fossil fuels,
843-844
fractional precipitation, 712-713
Frasch process, 919
free electrons,
203
free energy

and chemical equilibrium,
742-746
defined, 737, 771
Gibbs free energy,
736-742
free radicals, 297, 819
freezing, 486
freezing point,
486-487
freezing-point depression,
521-522
Freon, 835
frequency, 194
fuel cells,
778-779
Fuller, R. Buckminster, 953
fullerenes, 953
functional groups, 51, 53
fusion, 486
G
galvanic cells,
763-764
galvanization, 785
gamma
(y) rays, 194
Gamow Bag, 448
Gamow, Igor, 448
gangue, 883
gas, 6, 7
gas constant

(R), 427
gas embolism, 415
gas laws,
421-426
application
to
the,
440-445
defined, 421
gases
characteristics of, 417
deviation from ideal behavior,
445-447
diving and the property of, 415
equilibrium expressions containing,
603-604
gas laws,
421-426,
440-445
gas mixtures, 434 439
gas pressure,
417-420
ideal gas equation,
427-430
kinetic molecular theory
of
gases,
439-445
properties
of

, 416-421
reactions with gaseous reactants and
products,
430-433
Gatorade, 114-115
geiger counter, 818
Geiger, Hans, 39
General Conference on Weights and
Measures, 8
geodesic dome, 953
geometric isomers, 865
geometrical isomers, 382
Gerlach, Walther, 215
Germer, Lester Halbert,
210
Gibbs free energy, 737
glass, 484, 485
glassware, volumetric, 9
Goodyear, Charles, 937
graduated cylinder, 8, 9
Graham's law, 444
graphene, 953
graphite,
952-953
Graves, Ray, 115
gravimetric analysis, 142-143
gravitational constant, 418
Greek prefixes, 49
greenhouse effect, 838-843
ground state,

203, 223, 224
Group
lA
elements, 258,
264-265
Group
1B
elements, 264-265
Group 2A elements, 259
Group 3A elements,
260
Group 4A elements, 261
Group 5A elements,
261-262
Group 6A elements, 262, 263
Group 7 A elements, 262, 263
Group 8A elements, 264
group number, 291
groups, in periodic table,
44
Grubbs, Robert H., 935
Guldberg, Cato, 595, 596
Guy-Lussac, Joseph,
423-425
H
Haber process, 611, 612
half-cell potentials, 764
half-cell reactions, 766-768
half-cells, 763
half-life, 558-559,

806-807
half-reaction method, 131-132, 760
half-reactions,
127,760-761
halides, 262
Hall process,
895-896
halogens, 45, 906,
921-922
compounds of, 925-926
properties of, 922, 923-925
uses of,
926-927
heart medication, explosives and, 277
heat
specific heat and heat capacity,
171-172
thermal energy and, 161
and work, 165-167
heat capacity, 171- 172
heavy water,
814,908
Heisenberg uncertainty principle, 211
Heisenberg, Werner, 211
hemochromatosis,
63
hemodialysis, 527
hemoglobin, 617, 848
hemolysi
s,

525
Henderson-Hasselbalch equation, 685,
688,694
Henry's law, 516
Henry's law constant, 516
Hertz (Hz), 194
Hess's law, 177-178
heteroatom
s,
377
heterogeneous catalysis,
574-575
heterogeneous equilibria,
599-600
heterogeneous mixtures, 7
heteronuclear diatomic molecules, 48
hexagonal close-packed (hcp) structure, 478
high-density polyethylene
(HDPE),
936-937
high-spin complex, 870
high-temperature superconductor, 956
homogeneous catalysis, 575
INDEX
homogeneous mixtures, 7
homonuclear diatomic molecules, 4
Hund
's
rule,
221-222,

869-870
hybridization
defined,327
in molecules containing multiple
bon

335-341
hybridization
of
atomic orbitals, 327. 3 - 1
sand p orbitals,
328-330
s,
p,
and d orbitals,
330-334
hydrated ions, 120
hydrates,
61
hydration, 117,
118,391,508
hydrazine, 912-913
hydride ions, 257
hydrocarbons,
51
hydrocyanic acid, 911
hydrofluoric acid, 922
hydrogen,
906-907
binary hydrides, 907

-908
hydrogen economy,
909-910
hydrogenation, 909
isotopes of,
908-909
in the periodic table, 257
hydrogen atom
Bohr's theory
of
the,
200-208
-

-
quantum mechanical description
of
the. _: :
hydrogen bomb, 816
hydrogen bonding,
463-464
hydrogen displacement, 133
hydrogen fluoride, 922
hydrogen peroxide, 917
-9
18
hydrogen sulfide,
919-920
hydrohalic acids, 660
hydrolysis, 389

hydronium ion, 123
hydrophilic,
530,
531-532
hydrophobic, 530, 531- 532
hydroxide ion, 123
hydroxy group, 367,
370
hyperbaric oxygen therapy, 438
hypertonic, 525
hypothermia
heat capacity and, 174
phase changes and, 489
hypothesis,S
hypotonic, 525
hypoxic tents, 591, 623
I
ideal behavior (gas), 445
factors that cause deviation from,
4-+
-
van der Waals equation, 445 447
ideal gas, 427
ideal gas equation, 427
ideal solution, 519
implosion, 816
in phase, 195
incomplete octet
s,
297

indicator
s,
144
indoor pollution, 846-848
inert complex, 872
inert gases, 264
inexact numbers,
15
initial
rate,S
51
1-6
INDEX
inorganic compound
s,
51,
61-62
defined, 364
insoluble compo
un
ds, 118
instantaneous dipole, 466
instantaneous rate
s,
546- 548
ins
ul
ators, 889
integrated rate law, 556
intensive propertie

s,
15
interatomic, 5
interference, 195
interference pattern, 195, 196
intermediate
s,
568
intermolecular bonding, 286
intermolecular forces
defined, 462
•
dipole-dipole interaction
s,
462-463
dispersion force
s,
465-467
hydrogen bonding,
463-464
ion-dipole interaction
s,
467
solutions and,
507-508
internal energy (U),
165
International System
of
Unit

s,
9
International
Union
of
Pur
e and Applied
Chemistry, 242
internuclear axis, 335
interstitial h
yd
rides, 908
intramolecular bonding, 286
intravenous fluid
s,
524-526
iodine, 927
ion-dipole interaction
s,
467
ion pair
s,
523
ion-product constant
(Kw),
638
ionic bonding, 279
io
ni
c bond

s,
286, 288
ionic compounds
defined, 55,
11
6
formulas of, 57- 58
halides as, 925
lattice energy of, 280-281
naming,
58-
61
solubility
pr
oducts of, 702
in water, solubility guidelines, 117- 119
ionic crystals,
480-482,
483
ionic equations,
120
net, 120
ionic hydrides,
907-908
ionic radiu
s,
254-256
ionizable hydrogen atoms,
51
ionization, electrolytes and, 112

ionization, percent, 529,
649-650
ionization constants
acid, 647- 652
base,
652-654
ionization energy (fE), 247-249
ionosphere, 833
ion-product constant
(K,.), 638
•
Ions
atomic,
55-5
6
common ion effect,
682-683,
705- 710
com
plex ion formation, 710- 712
defined, 43, 55
electron configuration of,
252-254
formulas
of
ionic
com
pound
s,
57-58

ionic and covalent compounds, 286
ionic bonding, 279
ionic compound
s,
55,
57-61
, 116,
117-119
naming ionic
com
pound
s,
58-61
polyatomic,
56-57
solubility and
se
paration of, 712- 715
iron, 63,
884-885
iron deficiency, 33
iron deficiency anemia (IDA), 33
isoelectronic, 253
isoelectronic series,
255-256
isolated system, 163,
l75
isomerism, 382- 386
isomerization reaction
s,

394
isopropy
I group, 370
isotactic, 941
isotonic, 523
isotopes,
41-42
chemical analysi
s,
817
hydrogen,
908- 909
in medicine,
817-818
parent and daughter, 805
isotropic, 947
J
Jenner, Edward, 3
joule
(J),
161-162
Joule, Jame
s,
161
K
Kekule structures, 376
Kelvin, Lord (William Thomason
),
424
Kelv

in
temperatu
re
scale, 10-
11
, 424
ketones, 367,
370, 373
kilojoule (kJ), 162
kinetic energy,
160
kinetic isotope effect, 909
kinetic lability, 872
kinetic molecular theory, 439
kinetic molecular theory
of
gases,
439-445
L
labile complexes, 872
lanthanide (rare earth) series,
224-225
lasers,
207-208
laser pointer
s,
199
in medicine, 193
LASIK
surgery, 193

lattice, 57
lattice energy, 279, 280-281
lattice points, 472
lattice structure, 472
laughing gas, 913
law
of
conservation
of
energy, 160
law
of
conservation
of
mass, 36
law
of
definite proportions, 35
law
of
mass action, 595
law
of
multiple proportion
s,
35
law
of
octaves, 238
law, scientific, 5

Le
Chiltelier's principle,
611-612
lead poisoning, 857
lead storage batterie
s,
777- 778
levorotatory isomer, 384, 866
Lewis acids and bases,
668-670
Lewis dot symbols,
278-279
Lewis, Gilbert, 278, 284
Lewis structures,
284-285
drawing, 291- 292
and formal charge,
292-295
Lewis theory
of
bonding, 284, 324, 351
Libby, Willard
F.,
563
ligand exchange, 872
Ligand
s, 860-861
light, nature of, 194, 197
double-slit experiment,
195-196

electromagnetic spectrum, 195
propel1ies
of
waves, 194-195
light water reactor
s,
812-8
13
liming, 845
limiting reactant,
92
determining the, 93
-95
reaction yield,
96-97
Lind, James, 635
line spectra,
201
liquid crystal
s,
947-949
liquids,
6,
7
gases as, 417
liquid-vapor phase transition,
485-486
properties of,
468-472
solid-liquid phase transition,

486-488
surface tension, 468
vapor pressure,
469-472
viscos
it
y,
468-469
liter, 12
lithium, 267
lithium-ion ba
tt
eries, 778
Ii
ving systems
ent
ropy in, 725
thermodynamics in,
746-748
localized bonds, 352, 378
London's dispersion forces, 466
lone pairs, 284, 285
low-density polyethylene
(LDPE
),
936-937
low-spin complex, 870
M
macroscopic level, 5
magic number

s,
800
magma, 838
magnesium, 894
magnetic confinement, 816
magnetic quantum number, 213- 214
main group elements, 241
manometer, 419
Mars Climate Orbiter, 14
Marsden, Ernest, 39
mass,
9-10
atomic, 46
law
of
conservation
of
ma
ss, 36
molecular and formula,
74
percent composition by mass, 75
of
reactants and products, 90-91
mass defect, 802
mass-energy equivalence relationship,
Einstein's,
802
mass number (A),
40-41

mass spectrometer, 43
matter
classification of,
6-8
defined, 4
•
properties
of
, 14 15
states of, 6, 7
Maxwell, James Clerk,
195,442
measured numbers, 16-
18
measurement, uncertainty in,
15
-
19
medicine
lasers in, 193
nuclear,
817-818
Meissner effect, 956
melting, 486
melting point, 486
membrane potential, 776
Mendeleev, Dimitri,
238-239
meniscus, 468
Menkes disease, 881

mercury,
418-420,
422
mesosphere, 833
metabolic acidosis, 543
metabolism, stoichiometry of,
80
metal matrix composites, 946
metallic character, 252
metallic crystals, 483
metallic radius, 246
metalloids, 44, 244, 252, 905,
906
metallurgy, 873, 880-881
alkali metals,
891-893
alkaline earth metals, 893- 895
aluminum,
895-897
band theory
of
conductivity, 888- 890
defined,883
of
iron,
884-885
metallurgical processes,
883-888
metals in human biology, 881
occurrence

of
metals, 882
periodic trends in metallic properties,
890-891
preparation
of
the ore, 883
production
of
metals,
883-884
purification
of
metals,
887-888
steelmaking,
885-887
metals,
44
, 45, 56
in chemical equations, 243- 244
oxidation
of
metals in aqueous solutions, 130
oxides of,
667-668
qualitative analysis
of
metal ions in solution,
714-715

metathesis method, 935
meterstick, 8
methanol, 578
methanol poisoning, 543
methyl group, 367,
370
metric system, 8, 12
Meyer, Lothar, 238
microstates, 728- 729
millicurie (mCi), 818
Millikan, R. A., 37
milliliter
(mL),
12
millimeters mercury (mmHg), 418
minerals, 882
miscible,
508
mixtures,
7-8
gas, 434 439
moderators, 813
modern materials,
934-935
biomedical materials,
949-952
ceramics and composite material
s,
945-946
.

liquid crystal
s,
947- 949
nanotechnology,
952-953
polymers,
936-945
semiconductors, 95
4
956
superconductors, 956- 957
molal boiling-point elevation constant,
520
molal freezing-point depression constant, 521
molality, 512
molar concentration, 136
molar heat
of
fusion, 488
molar heat
of
sublimation, 488
molar heat
of
vaporization,
485-486
molar mass, 84
molar solubility,
701
molarity (

M),
136, 138- 139
mole and molar masses
determining molar mass, 84
empirical formula from percent composition,
85-86
interconverting mass, moles, and numbers
of
particles, 84 85
the mole, 82- 84
mole defined, 82
moles
of
reactants and products, 89- 90
mole fractions,
435-436
, 513, 518
molecular art, 5
molecular compounds, 47,
49-51
,
116,417
molecular crystals, 483
molecular equations, 119
molecular formula, determination
of
, 88
molecular geometry, 314
defined, 316
deviation from ideal bond angles, 319

electron-domain geometry and, 316- 319
geometry
of
molecules with more than one
central atom, 319- 320
and polarity,
321-323
VSEPR model, 314 315
molecular level, 5
molecular mass, 74
molecular orbital theory,
342
, 351- 353
bond order, 343- 344
bonding and antibonding molecular orbital
s,
342- 343
defined,342
molecular orbital diagram
s,
346-347
, 349
molecular orbitals,
342-345
molecular parity, 321
molecular speed,
442-444
molecular weight, 74
molecularity,
568-569

molecule
s,
4, 5,
47-48
with delocaliz
ed
bonding,
351-35
3
empirical formulas, 51, 53, 54 55
hybridization and multiple bond
s,
335-341
molecular formulas, 48
naming molecular compounds, 49-
51
,
52
,
53
, 374
representation
of
organic molecule
s,
375- 381
Molina, Mario, 829
molybdenum, 883
momentum (p), 211
monatomic cation

s,
55
monatomic ion
s,
55, 56
monatomic molecules, 47
Mond
process, 887
INDEX
1-7
monodentate ligands, 861
monomers, 395, 936
monoprotic acids, 123
Montreal
Protocol, 829, 837
Moseley, Henry, 239
mUltiple bond
s,
285-286
multiple proportion
s,
law of, 35
musk,354
N
n-type semiconductors, 890, 955
nanofibers, 951
nanotechnology,
952-953
nanotubes, 953
NASA,14

natural rubber,
936-937
Nelmes, Sarah, 3
nematic, 947
Nernst equation,
773-775
net ionic equations, 120
neutralization reactions, 124
neutron-to-proton ratio (nip),
800
neutrons,
40
,
41
Newlands, John, 238
Newton's laws
of
motion, 212
newtons (N),
14,418
nitric acid,
913-9
14
nitric oxide,
304, 845-846, 913
nitrogen, 911- 914
nitrogen dioxide, 913
nitrogen fixation, 831, 913
nitroglycerin, 277
nitrous oxide, 913

Nobel, Alfred, 277
Nobel
Prize, 277, 313, 563, 829, 935
noble gas core, 223
noble gases, 45, 241, 244
noble metals,
130
nodes, 208
nomenclature, chemical, 49
nonconductor
s,
954
nonelectrolyte
s,
112
nonmetals, 44
carbon, 910- 911
in chemical equation
s,
244
general properties
of
, 906
halogens,
921-92
7
hydrogen,
906-910
nitrogen, 911- 914
oxides of,

667-668
oxyg
en,9l6
- 918
phosphorus, 914 916
sulfur, 918- 921
nonpolar,,288, 321
nonpolar covalent bonds, 288
nonspontaneous processes, 726
nonvolatile, 517
normal boiling point, 485
northem lights, 833
nuclear binding energy,
801- 803
nuclear chain reaction, 812
nuclear chemistry,
796-797
•
biological effects
of
radiation,
818-
819
natural radioactivity,
804-808
nuclear
fi
ss
ion, 811- 815
1-8

INDEX
nuclear
chemistry-continued
nuclear fusion,
815-817
nuclear stability,
799-804
nuclear transmutation, 808-811
nuclei and nuclear reactions, 798
-799
uses
of
isotopes,
817-818
nuclear fission, 811-815
nuclear fusion,
815-817
nuclear medicine, 817- 818
nuclear reactors,
812-815
nuclear transmutation, 798, 808-811
nucleic acids, 397,
400, 401
nucleons,
41
nucleophile addition, 388
nucleophiles, 386, 387
nucleotides,
400, 401
nucleus, 40

utrition Facts label
s,
159
nylon,
396-397
o
octet rule, 284, 285
exceptions to,
296
-3
00
oil-drop experiment, Millikan, 38
old quantum theory, 212
olefin metathesis, 935
olfactory receptors, 313
open system, 163, 164
optical isomers, 383, 865, 866
orbitals
electrons in, 324
•
hybridization
of
atomic,
327-334,
351
molecular orbital theory, 342-351
ore, 882
organic chemistry
carbon,
364-365

classes
of
organic compounds,
365-375
and drugs, 363
isomerism,
382-386
organic polymers, 395-401
organic reactions,
386-395
representation
of
organic molecule
s,
375-381
organic compounds, 50-
51
classes of, 365
-37
5
defined, 364
naming,
368-369
osmosis, 522, 527
osmotic pressure, 522- 523
out
of
phase, 195
overvoltage,
782

oxidation, 127
oxidation number, 127
oxidation-reduction reactions,
126-127
, 394
balancing simple redox equation
s,
130-133
oxidation number
s,
127-130
oxidation
of
metals in aqueous solutions, 130
oxidation state, 127
oxides
acid-base properties
of
hydroxides and,
667-668
basic and amphoteric hydroxide
s,
668
of
metals and nonmetals,
667-668
variation
of
third-period element
s,

265-266
oxidizing agent, 127
oxoacids, 59, 660
-66
1
oxoanions, 59
oxygen,
916-918
oxygen transport, 874
ozone, 918
CFCs and, 829, 835
depletion
of
stratospheric,
835-836
polar ozone holes,
836-838
p
p orbitals, 217,
328-334
p-type semiconductor
s,
890, 955
packing sphere
s,
473-475
paramagnetic,
342
partial charges, 289
partial pressure, 434

particle accelerator, 810
particles (N), 84
pascal
(Pa), 418
passivation, 785
patina, 785
Pauli exclusion principle,
220-221,
870
Pauling,
Linus, 287
peptide bonds, 398, 399
per
mole
of
the reactio
n,
169
percent by mass, 512
percent composition by mass, 75,
85-86
percent dissociation, 529
percent ionic character, 288
percent yield, 96
periodic table, 44
46, 135
atomic radius,
246-247,
255
classification

of
elements,
241-243
comparing ionic radius with atomic
radius, 255
comparison
of
Group
lA
and
Gr
oup
IE
elements,
264-265
development of,
238-240
effective nuclear charge,
244-245
electron affinity (EA), 250-251
electron configuration
of
ion
s,
252-254
electron configurations and the,
223-226
elements essential for life,
239-240
gaseous elements in, 416

general trends in chemical propertie
s,
257
Group
lA
element
s,
258
Group
lB
elements,
264-265
Group
2A
elements, 259
Group
3A
elements, 260
Group
4A
elements, 261
Group 5A elements,
261-262
Group 6A element
s,
262, 263
Group 7 A elements, 262, 263
Group 8A elements, 264
ionic radius,
254-256

ionization energy (IE), 247-249
ions
of
d-block element
s,
253-254
ions
of
main group elements, 253
isoelectronic
se
rie
s,
255-256
main group elements,
256-266
metallic character, 252
modern,
240-244
numbers at top of, 242
periodic trends in metallic propertie
s,
890 891
periodic trends in properties, 245,
246-252,
256-266
properties
of
other main group elements,
260-264

properties
of
the active metal
s,
258-259
properties
of
transition metal
s,
858-859
representing free elements in chemical
equations,
243-244
salt and salt s
ub
stitutes, 237
variation in properties
of
oxides within a
period,
265-266
periodicity, 238
period
s,
in periodic table, 44
peroxide,
917-918
pH, 639
of
acid-base titrations, 691

acid ionization constants and,
648-651
base ionization constants and,
653-654
buffer solutions and,
684-689
mean precipitation
pH
in the U.S., 843
pH scale, 639
-6
44
phase boundary line, 491
phase changes,
484
485,486
dangers of,
489-491
liquid-vapor phase transition,
485-486
solid-liquid phase transition,
486-488
solid-vapor phase transition, 488
phase diagrams,
491-493
Phipps, James, 3
phosphine,
914-915
phosphorus,
914-916

photochemical smog,
845-846
photodecomposition, 830
photodissociation, 835
photoelectric effect,
198-199
photons,
198-199
photosynthesis, 830, 832
physical change,
15
physical properties,
14-15
pi bonds, 336, 340-341
pig iron, 885
pipet, 8, 9
Planck, Max, 193, 197, 198
plasma, 816
Platinol, 73
Plato,
34
pOH
scale, 641
polar, 286
polar covalent bond
s,
286, 288
polar molecules, 117,
321,462
polar ozone hole

s,
836-838
polar stratospheric clouds (PSCs), 836, 837
polar vortex, 836
polarimeter, 866
polarity, molecular geometry and,
321-323
polarized light, 384, 385, 866, 867
polarized molecules, 466
pollution
acid rain,
843-845
greenhouse effect,
838-843
indoor,
846-848
photochemical smog,
845-846
polyamides, 942
polyatomic ion
s,
56-57
poly atomic molecules, 48, 840
polyesters, 942
polyisoprene,
936-937
polymer matrix composites, 946
polymers
addition,
395-396,

397,
936-941
biological,397-401
condensation,
396-397,
941-944
defined,395,936,941
electrically conducting,
943-944
organic, 395-401
polypeptides, 399
polyprotic acids, 59, 123-
124,657-659
polysaccharides, 397, 400
polystyrene, 938
polyvinyl chloride
(PVC), 938
positron, 798
potass
ium
hydroxide, 893
potassium nitrate, 893
potential energy,
160
pounds, 14
precipitate, 117
precipitation, fractional,
712-713
precipitation reactions
in aqueous solutions, 117-121

defined,117
solubility and,
704-705
precision,
18-19
prefixes, Greek, 49
pressure
calculation of, 418
Dalton's law
of
partial pressures, 434 435
defined,418
equilibrium and,
614-615
measurement of,
418-420
pressure-volume relationship,
421-423
solubility and,
515-517
using partial pressure to solve problems,
436-438
primary ami des, 373
primary amines, 373
primary pollutants, 845
primary structure, protein, 465
principal quantum number, 213, 214
probability,
726-727
probability density, 216-

2l7
problem solving, using units and,
20-22
products, in chemical reactions, 77
proteins, 397,
399-400
protein structure, 464 465
proton acceptor, 123
proton donor, 123
protons,
40,
41
Proust, Joseph, 35
pure covalent bonds, 286, 288
pyrometallurgy,
883-884
qualitative analysis,
714-715
qualitative properties, 14
quantitative properties,
8,
14
quantum mechanics,
210-211
beginning of, 212
quantum mechanical description
of
the
hydrogen atom, 212
Schrodinger equation, 212

uncertainty principle, 211
quantum numbers, 212,
213-214
electron spin quantum number,
214-215
quantum theory, 193, 197
developments in, 212
photons and the photoelectric effect,
198-200
quantization
of
energy, 197- 198
quantum defined, 197
quaternary structure, protein, 465
quicklime,
844-845
R
racemic mixture, 384, 866
racemization, 391
radial probability distribution,
216-2l7
radiation, 36
biological effects of,
818-819
ultraviolet (UV), 830
radiation absorbed dose (rad), 818
radicals, 297, 298, 819
radio waves, 194, 195- 196
radioactive bone, 265
radioactive decay

dating based on,
806-808
defined, 798
kinetics of,
805-806
radioactive decay series,
804-805
radioacti
vi
ty,
38-39,798
radiocarbon dating, 563,
806-808
radon, 820,
846-847
randomness, 508
Raoult's law, 517
rate constant, 547
rate-determining step, 569-571
rate law, 551
rate
of
reaction, 548
reactant
s.
See also limiting reactant
defined, 77
gaseous,
430-433
mass

of
reactants and product
s,
90-91
moles
of
reactants and product
s,
89
-90
reversible, 592
reaction mechanism, 568
reaction order, 551
reaction quotient, 595
reaction rate
s,
544
Arrhenius equation,
564-·565
average,
544-546
catalysis,
573-577
collision theory,
562-564
elementary reactions,
568-569
experimental determination
of
the rate law,

551-555
first-order reactions,
555-559
instantaneous rate,
546-548
rate-determining step, 569- 572
rate law, 551
reaction mechanisms, 568- 573
second-order reactions,
560-561
stoichiometry and,
548-550
reactions
organic,
386-395
types of, 98
red phosphorus, 914
redox reactions, 126
balancing,
760-762
balancing simple redox equations,
130-133
INDEX 1-9
spontaneity under conditions other than
standard state,
773-777
spontaneity under standard-state conditions.
770-773
types of,
133-134

reduced iron, 33
reducing agent, 127
reduction, 127
Reinitzer, Frederick, 947
relative biological effectiveness
(REE
),
81
8
remineralization, 681
representative elements, 241
repulsion,
160
repulsive force, 245
resonance
,29
5-296,378-381
resonance stabilized, 378
resonance structures, 295, 378
reversible process, 592
revised metric system
(SI) units, 8, 9
rhombic sulfur, 919
ribonucleic acid (RNA),
400, 401
roentgen equivalent for man (rem),
81
Roman numerals, cations with, 56
Rontgen, Wilhelm, 38
root-mean-square (rms) speed,

442
Ro
senberg, Barnett, 73
Rowland,
F.
Sherwood, 829
rubber,
936-938
Rutherford, Ernest, 39, 40, 193
Rydberg equation,
202
Rydberg, Johan, 202
5
s orbitals,
216-217,
328-334
salt
in acid-base reactions, 124
and salt substitutes, 237
salt bridge,
763-764
salt hydrolysis, 662
salt solutions
acid-base properties of,
662-66
7
acidic,
664-665
basic,
662-663

cations and anions, 666
neutral,
665-666
saturated solutions, 506
scanning tunneling microscope (
STM
. 9':::
Schrock, Richard R., 935
Schrodinger equation, 212
Schrodinger, Erwin, 212
scientific measurement, 8-
13
scientific method, 3,
5-6
scurvy, 635
second law
of
thermodynamic
s,
725. ,
'}-
-
~:
second-order reactions, 560
secondary pollutants, 845
secondary structure, protein, 465
semiconductors,
889-890,
954-
9-6

semipermeable membrane, 522
sequestrants, 874
shell, 213
shielding, 244
shielding constant, 245
SI base units, 9, 10, 12
sickle cell disease, 461
1-10
INDEX
sigma
bond
s, 335, 338
sigma molecular orbitals, 343
significant figures,
15
- 16
sil ver fluoride, 922
simple cubic cell, 4
73-474
single
bond
s, 285
sintering, 945- 946
skeletal structures,
376-378
slag, 885
smallpox, 3, 23
smectic, 947
smell, olfactory receptors, 313
smog, photochemical,

845-846
smoking, radioactivity in tobacco,
8
19-
820
SNI reactions,
390-391
soda ash, 893
sodium carbonate, 893
sodium chloride
•
electrolysis
of
an aqueous sodium chloride
solution, 78
1-
782
el
ec
trolysis
of
molten, 780
sodium hydroxide, 893
sodium nitrate, 893
sof
t
ti
ssue materials, 9
50-951
sol-gel process, 946

solar flares, 833
solids, 6, 7.
See also crystal
st
ructure
amorphous, 484
gases as, 417
preparing a solution from, 1
38-139
solid-liquid phase transition, 486
-4
88
solid-vapor phase transition, 488
solubility
defined,
117,50
6,7
01
factors that affect, 515- 517, 705
-7
12
guidelines f
or
ionic co
mp
ounds,
117-119
separation
of
ions in,

712
- 715
vitamin, 509- 511
solubility equilibria,
700-705
solubility product constant, 701
soluble compounds, 118
solutes,
112,
50
6
solution stoichiometr
y,
141-142
solutions, 112
colligative properties,
51
7
-52
9
colloids,
530
-
532
concentration units,
511-514
energy and entropy in solution formation,
508-509
factors that affect solubilit
y,

515- 517
intermolecular forces,
507-
50
8
types of,
506-507
solvation,
50
7
solvents, 112
,506
solving problems, using units and,
20-22
space-filling models (molecular art), 5
space shuttles,
my
stery glow of, 834
specific heat,
171-172
spectator ions, 120
spectrochemical se
ri
es, 869
speed
of
light (c), 194
splitting,
of
energy levels, 219

spontaneous processes,
72
6
stability constant,
7l
0
standard atmospheric pressure, 419
standard enthalpies
offo
rmation, 179
-1
81
standard enthalpy
of
reaction, 179
standard entropy,
729-730,
736
standard free-energy
of
formation, 739
standard free-energy
of
reaction, 738
standard hydrogen electrode (
SHE
), 765
standard reduction potential, 765
standard solution, 144
standard states, 622

standard temperature and pressure
(S
TP
), 428
standing/stationary waves,
208, 209
state functions, 163
state
of
a system, 163
s
team
burns, 489
steelmaking,
885-887
stereoisomerism,
382-384
stereoiso
mer
s, 382, 865
Stern,
Otto, 215
Stock
system,
56
stoichiometric amount, 90
stoichiometric coefficients, 77
stoichiometry
and reaction rates,
548-550

solution, 1
41-
1
42
stoichiometry, ratios
of
combination, 72- 73
calculations with balanced chemical
equations,
89-91
chemical equations, 76- 81
combustion analysis,
86-89
limiting reactants,
92-97
mole and molar masses,
82-86
molecular and formula
masse
s,
74
percent composition
of
compounds,
75-76
reaction types, 98
stomach,
pH
balance,
642-643

stratosphere
defined,833
depletion
of
ozone in,
835-838
strong acid-strong base titrations,
691-692
strong acid-weak base titrations, 696- 698
strong acids,
644-645
strong bases,
645-647
strong conjugate acid, 655
strong conjugate base, 655
strong electrolytes
in aqueous solutions,
112-116
, 120
defined, 112
strong-field ligands, 869
structural formulas, 48
structural isomers,
32
1, 382
subatomic particles,
36
, 798
sub
cr

itical mass, 812
sublimation, 488
subshell,2
13
substances
defined,6
equilibrium and addition/removal of,
612-614
substituents, 368, 374
substitution reactions,
388-390
substrate, 575
sulfur,
918-921
s
ul
fur dioxide, 843- 845,
920-921
sulfur hexafluoride, 9? I
sulfur trioxide, 921
su lfuric acid, 921
supercondu
ct
ing transition temperature, 956
superconductors, 956- 957
supercooling, 488
supercritical fluids,
486
supersaturated solutions, 506,
50

7
surface tension, 468
su
tT
oundings, 160
sutures, 951
symbols, el
eme
nt, 41
symbols,
Le
wis dot, 278
syndiotactic, 941
systems,
160
T
tacticit
y,
941
Te
fl
on, 939
temperature, 10-
11
,
15
absolute, 10
equilibrium and,
61
5

-6
16, 618- 619
solubility and, 515
temperature-volume relationship,
423-425
tempering, 886
termolecular, 569
tertiary stru
ct
ure, prote
in
, 465
testicular can
ce
r, 73
thalidomide, 363,
390,
402
theoretical yield, 96
theory, scien ti
fi
c, 5
thermal energy,
160
thermal pollution, 515
thermite reaction, 897
thermochemical equations, 169- 171
thermochemistry,
158-159,
182- 183

calorimetry, 171- 177
defined, 161
energy and energy changes, 1
60-
163
enthalp
y,
167
-1
7 1
He
ss's
la
w,
177
-178
standard enthalpies
of
formation, 179-181
thermodynamics, 163- 167
thermodynamics
defined, 163
first law
of
thermodynamics, 1
64-
165
,72
5
in

living systems,
74
6-74
8
second law
of
thermodynamics, 725,
733-73
5
states and state functions, 163- 164
third law
of
thermodynamics, 735- 736
work and heat, 1
65-
167
thermonuclear bomb, 816
thermonuclear reactions, 815
thermoplastic, 936
thermosetting, 936
thermosphere, 833
third law
of
thermodynamics,
735-736
Thomson, George Paget, 210
Thomson
,
J.
1.

, 37, 39
three-dimensional (3D)
mo
vies, 385
threshold frequency, 198
titrations, 1
44
. See also acid-base titrations
tobacco, radioac
ti
vity
in
,
819-820
tooth deca
y,
681
to
tT
,4
18
trace elements,
240
tracers, 817
trans isomers, 337, 382,
865-866
transition elements, 45
transition metal
s,
45, 56, 223, 241,

858-859
transition rate, 564
transition state, 564
transmutation elements,
809
transmutation, nuclear, 798, 808- 811
triple bonds, 285, 338
triple point, 491 , 492
triprotic acids, 123
troposphere, 832- 833
Tyndall effect, 530, 531
u
ultraviolet (UV) radiation, 830
uncertain digits,
15
uncertainty in measurement, 15-19
uncertainty principle, 211
unimolecular, 569
unit cells, 472-473
units, 8
unsaturated solutions,
506
uranium decay series, 804-805
v
vaccination,
3,
23
vaccinia immune globulin (VIG), 23
valence band, 888, 954
valence bond theory, 324-326, 351

valence electrons, 243
valence-shell electron-pair repulsion (VS
EPR
)
model, 314- 315, 351
van der Waals equation,
445-447
van der Waals forces, 362
van der Waals,
J,
D., 445
vanadium oxide, 921
van't
Hoff
factor, 523
vapor, solid-vapor phase transition,
488
vapor pressure, 437,
469-472
vapor-pressure lowering,
517-519
vaporization, 470
visible light, 194
vision, 394-395
vitamin C, 635, 671
vitamin solubility, 509-511
volatile, 469, 519
volcanoe
s,
838

voltaic cells, 763
volume
amount-volume relationship,
425-426
constant-volume calorimetry,
l75-177
equilibrium and, 614-615, 620-621
pressure-volume relationship, 421-423
reactions under constant-volume!
constant-pressure conditions,
167-168
temperature-volume relationship, 423-425
volumetric flask,
8,
9
von
Laue
, Max Theodor Felix, 476
VSEPR
model, 314-315, 351
vulcanization, 937
Waage, Peter, 595, 596
water
acid-base properties of,
637-639
electrolysis of, 780-781
molecule, 48
physical states of, 6, 7
water gas,
907

water-soluble, 112
water-insoluble compounds,
11
8
water-soluble compounds,
11
8
wave function, 212
wave mechanics, 212
wave properties
of
matter, 208
de Broglie hypothesis,
208-210
diffraction
of
electrons, 210
INDEX
wavelength, 194
waves, properties of, 194-
195
weak acid-strong base titration
s,
693 696
weak acids, 647
weak bases, 652
weak conjugate acid, 655
weak conjugate base, 654
weak electrolytes
in aqueous solutions,

11
2- 116
defined, 112
weak-field ligands, 869
weight, 9
Werner, Alfred,
858
Werner's coordination theory. 858
white phosphoru
s,
914 ·
Wilson disease, 881
Wohler, Friedrich, 364
work, and heat,
165-167
• •
World Anti-Doping Agency (WADA '.
'::
91. '
':'::
World Health Organization
(WHO
).
"'.
"':
x
X-ray diffraction, 210, 476, 477
X-rays, 38, 194
,239
y

yield
actual,
96
percent, 96
theoretical, 96
z
zeroth-order reaction, 561
zone refining, 888
Avogadro's number
Electron charge
(e)
Electron mass
Paraday constant
Gas constant (R)
Planck's constant (h)
Proton mass
Neutron mass
Speed
of
light in a vacuum
tera (T)
10
12
giga (G)
10
9
mega (M)
10
6
kilo (k)

10
3
deci (d)
10-
1
lIb
= 453.6 g
1 in = 2.54
cm
(exactly)
1
mi
= 1.609
km
1
km
= 0.6215 mi
,
1pm
= 1 X
1O
-
12
m=
1 X
lO-
lO
cm
6.0221367 X 10
23

1.6022 X 10-
19
C
9.109387 X
10-
28
g
96,485.3 Clmo1
e-
0.08206 L . atrnlK . mol
8.314
J/K·
mol
62.36 L .
torr/K . mol
1.987 cal/K . mol
6.6256 X 10-
34
J . s
1.672623 X 10-
24
g
1.674928 X 10-
24
g
2.99792458 X 10
8
rnIs
centi (c)
10-

2
milli (m)
10-
3
micro
(IL)
10-
6
nano (n)
10-
9
pico (p)
10-
12
1 atm = 760 rnmHg = 760 torr = 101,325 N/m2 = 101,325 Pa
1 cal = 4.184 J (exactly)
1 L . atm = 101.325
J
IJ=1CX1V
?OC
=
(OP
_ 32
0
P) X 5°C
. 9°P
?OP
= 9°P X
(OC)
+ 32°P

5°C
?K =
(OC
+ 273.1 5°C)
(
1\~
•
,