CHAPTER 5
Nomenclature
CHAPTER ANSWERS
1.
There are millions of known chemical compounds.
2.
A binaiy compound contains only two elements. The major types of binary compounds are ionic
(compounds that contain a metal and a nonmetal) and nonionic (compounds containing two
nonmetals).
3.
cations, anions
4.
cation
5.
positive, negative
6.
Some substances do not contain molecules. For example, the substance sodium chloride consists
of an extended lattice array of sodium ions, Na, and chloride ions, Cl. Each sodium ion is
surrounded by several chloride ions, and each chloride ion is surrounded by several sodium ions.
We write the formula as NaCI to indicate the relative number of each ion in the substance, not to
indicate that there are “molecules” of sodium chloride.
7.
—our, --ic
8.
Roman numeral
9.
a.
sodium iodide
b.
calcium fluoride
c.
aluminum sulfide
d
calcium bromide
e
strontium oxide
f.
silver chloride Isilver(I) chloride]
g.
cesium iodide
h.
lithium oxide
a.
potassium bromide
b.
zinc chloride
c.
cesium oxide
d.
magnesium sulfide
e.
aluminum iodide
10.
magnesium bromide
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56
Chapter 5: Nomenclature
g.
beryllium fluoride
h.
barium hydride
a.
incorrect; Ba
2
li is barium hydride
incorrect; 2
Na is sodium oxide
0
correct
11.
b.
c.
d.
e.
incorrect; Si
2
0 is silicon dioxide
correct
a.
2
A
S
g
b.
2
Ba
li
c.
2
A
3
0
1
d.
2
Mg
F
e.
correct
a.
As the bromide ion has a 1— cha
rge, the tin ion must have a 2+
charge; the name is tin(1I)
bromide.
b.
As the iodide ion has a 1— charge
, the tin ion must have a 4+ charge
; the name is tin(TV)
iodide.
c.
As the oxide ion has a 2— charge
, the chromium ion must have a 2+
charge; the name is
chromium(Il) oxide.
As the oxide ion has a 2— charge,
each chromium ion must have a 3+
charge; the name is
chromium(Ill) oxide.
As, the iodide ion has a 1— charge
, each mercury ion must have a 1+
charge; the name is
mercury(1) iodide.
As the iodide ion has a 1— charge
, the mercury ion must have a 2+
charge; the name is
mercury(jI) iodide.
12.
13.
d.
e.
f.
14.
a.
b.
copper(I1) chloride
copper(I) iodide
c.
manganese(ll) bromide
d.
e.
chromium(1l) iodide
chromiumffl chloride
f.
mercury(11) oxide
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57
Chapter 5: Nomenclature
15.
a.
As each chloride ion has a 1— charge, the cobalt ion must have a 2+ charge; cobaltous
chloride.
b
As each bromide ion has a 1— charge, the chromium ion must have a 3+ charge; the name is
chromic bromide.
c.
As the oxide ion has a 2— charge, the lead ion must have a 2+ charge; the name is plumbous
oxide.
d.
As each oxide ion has a 2— charge, the tin ion must have a 4+ charge;: the name is stannic
oxide.
e.
As each oxide ion has a 2—- charge, the iron ion must have a 3± charge;: the name is ferric
oxide.
f.
As each chloride ion has a 1—. charge, the iron ion must have a 3+ charge; the name is ferric
chloride.
a.
cupric iodide
b.
mercurous bromide
c.
chromous bromide
d.
cobaltous oxide
e.
cobaltic oxide
f.
stannous chloride
16.
17.
Remember that numerical prefixes are used for this type of compound of nonmetals to indicate
how many of each type of atom is present. However, if only one atom of the first element
mentioned in the compound is present in a molecule, the prefix mono— is not needed.
a.
iodine pentafluoride
b.
arsenic trichioride
c.
-selenium monoxide
d.
xenon tetrafluoride
e.
nitrogen triiodide
f.
cliboron trioxide
18.
-
a.
xenon difluoride
b.
diboron trisulfide
c.
dichiorine hept(a)oxide
d.
silicon tetrabromide
e.
nitrogen monoxide
f.
sulfur trioxide
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.
-
-
-
-
-
,-
--
-
-
58
Chapter 5: Nomenclature
19.
a.
b.
tm(lV) oxide, stannic oxide
calcium hydride ionic
ionic
—
c.
silicon teirabromide
d.
iron(l1!) sulfide, ferric sulfide
oxygen dichloride nonionic
e.
noruoruc
ionic
—
f.
xenon tetrafluoride
-
nonionic
20.
a.
barium nitride
b.
aluminum sulfide
c.
cl.
diphosphorus trisulfide
calcium phosphide
e.
krypton pentafluoride
f.
copper(I) selenide/cuprous selenid
e
a.
magnesium su1fide
21.
-
I
ionic
b.
akiminum chloride
c,
phosphorus trthydride (the commo
n name phosphine is always used)
chlorine rnonobromidc nonionic
ci.
ionic
—
e.
lithium oxide
f.
tetraphosphorus decoxide
—
tonic
—
nonionic
22.
a.
barium fluoride
b.
radium oxide
c.
dinitrogen oxide
d.
rubidium oxide
e.
diarsenic pent(a)oxide
f.
23.
-•
calcium nitride
ionic
-
ionic
—
-
—
nonionic
ionic
--
nonionic
ionic
A polyatomic ion s a group of atom
s bound together that, as a unit, carr
ies an electrical charge.
Examples will depend on student
responses.
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59
Chapter 5: Nomenclature
24.
An oxyanion is a polyatomic ion containing a given element and one or more oxygen atoms. The
oxyanions of chlorine and bromine are given below:
Oxyanion
Name
Oxyarnon
Name
C10
Cl0
2
3
Cl0
4
C10
hypochiorite
chlorite
chlorate
perchiorate
Br0
BrOj
3
Br0
4
Br0
hypobromite
bromite
bromate
perbromate
25.
one fewer oxygen atom
26.
For a series of oxyanions, the prefix hypo— is used for the anion with the fewest oxygen atoms,
and the prefix per— is used for the anion with the most oxygen atoms.
27.
4
C10
perchiorate
ClO
hypochiorite
3
C10
chlorate
’
2
C10
chlorite
Wi
hypoiodite
102
iodite
103
iodate
104
periodate
28.
29.
a.
’
3
P
b.
3
4
P0
’
3
P0
d.
2
4
HP0
a.
3
N0
b.
N0j
c.
NH
d.
CN
30.
31.
ci
chloride
do
hypochiorite
—
2
do
chlorite
3
C10
chlorate
—
4
do
perchiorate
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ii
60
Chapter 5: Nomendature
32.
CN
cyanide
2
3
c0
carbonate
3
HC
O
hydrogen carbonate
0
3
H
2
C
acetate
33.
a.
permanganate
b.
peroxide
c.
chrornate
d.
dichromate
e.
nitrate
f.
sulfite
a.
ammonium
b.
dihydrogen phosphate
c.
sulfate
d.
e.
hydrogen sulfite (also called bisufflte)
perchiorate
f.
iodate
a.
ammonium nitrite
b.
barium hydroxide
c.
potassium peroxide
d.
aluminum hydrogen sulfate
e.
silver cyanide
f.
calcium hydrogen phosphate
a.
ammonium acetate
b.
lithium perchiorate
c.
sodium hydrogen snifate
d.
gold(ffl) carbonate
e.
calcium chlorate
f.
hydrogen peroxide
34.
‘l
35.
36.
37.
38.
An acid is a substance that produces hydr
ogen ions, H, when dissolved in wate
r.
oxygen (commonly referred to as oxyacids)
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Chapter 5: Nomenclature
61
39.
a.
hydrochloric acid
b.
sulfuric acid
c.
nitric acid
d:
hydroiodic acid
e.
nitrous acid
f.
chioric acid
g.
hydrobromic acid
h.
hydrofluoric acid
i.
acetic acid
a.
hypochiorous acid
b.
sulfurous acid
c.
bromic acid
d.
hypoiodous acid
e.
perbrOrnic acid
f.
hydrosulfuric acid
g.
hydroselenic acid
h.
phosphorous acid
a.
RaO
b.
S
2
Ag
c.
RbI
d.
AgI
e.
2
CaR
f.
2
P
3
Mg
g.
CsBr
.h.
2
N
3
Ba
40.
VV.
.
41.
42.
a.
lithium nitrate
b.
chromium(ffl) carbonate/chromic carbonate
c.
copper(ll) carbonate/cupric carbonate
d.
copper(l) selenide/cuprous selenide
e.
manganese(IV) sulfate
f.
magnesium nitrite
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>.
4
j
62
Chapter 5: Nomer,cature
43.
a.
3
P1
b.
4
SCJ
c.
5
0
2
N
d.
IBr
e.
13203
f.
3
NCI
g.
CO
a.
0
2
N
b.
2
NO
c.
4
0
2
N
d.
6
SF
e.
3
P13r
f.
4
Cl
g.
2
0C1
a.
NO
4
NH
3
b.
)
0
3
H
2
Mg(C
c.
2
Ca0
d,
4
KHSO
e.
4
FeSO
f.
3
KHCO
g.
4
CoSO
h.
4
LiC1O
a.
3
BaSO
b.
P0
Ca(B
2
)
4
c.
4
NHC1O
d.
4
NaMnO
e.
(50
2
Fe
3
)
4
f.
3
CoCO
g.
2
Ni(OH)
h.
4
ZnCrO
44.
45.
46.
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Chapter 5: Nomenclature
a.
S
2
H
b.
4
HBrO
C.
0
3
H
2
HC
4.
HBr
e.
2
HC1O
f.
e
H
S
2
g.
0
3
S
2
H
h.
4
HC1O
a.
HCN
b.
3
HNO
C.
HS0
d.
0
4
P
3
H
e.
HCZO or HOC1
f.
HBr
g.
2
HBrO
h.
HF
a.
0
2
Na
b.
0
3
Ca(C1
2
)
C.
RbOH
d.
2
)
3
Zn(N0
e.
Cr
2
)
1
(Na
7
0
f.
HS(aq)
g.
2
CaBr
h.
HOC1(aq)
i.
KS0
j.
aq)
HNO
(
3
k.
3 02)2
H
2
Ba(C
1.
3
LiS0
a.
O
4
Mg(HS
2
)
b.
4
CsC1O
48.
49.
so.
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63
64
Chapter 5: Nomenclature
C.
FeO
d.
H
T
2
e
e.
3
Sr
2
)
(N0
f.
Sn(C
4
)
2
0
3
H
g.
4
Mn
SO
h.
4
0
2
N
I.
4
N
H
2
PO
a
J.
Li
2
0
k.
2
HN
O
1.
Co(N0
3
)
51.
.
Formula Roman Numeral Name
—nuil-ic Name
FeO
ironQl) oxide
ferrous oxide
Fe
3
0
2
iron(ffl) oxide
ferric oxide
FeS
iron(Ji) sulfide
ferrous sulfide
3
S
2
Fe
iron(ffl) sulfide
ferric suffide
FeC1
2
iron(]I). chloride
ferrous chloride V
FeC1
3
iron(ffl) chloride
ferric chloride
52.
A moist paste of NaC1 would contain
Na and CP ions in solution and wou
ld serve as a conductor
of electrical impulses.
53.
NO, nitrogen monoxide; NO
, nitrogen dioxide; N
2
, dinitrogen tetr(a)oxide; N
4
0
2
, dinitrogen
5
0
2
pent(a)oxide; N
O, dinitrogen monoxide
2
54.
H —> H (hydrogen ion: a cation) + e
H’+ e — BE (hydride ion: an anion)
55.
Answer depends on student choices.
missing oxyanions: IO; Cl0
2
56.
missing oxyacids: ;
4
HC
1O HC1O; HB
2
rO
57,
a.
calcium acetate,
b.
phosphorus trichioride
c.
copper(ll) permanganate, cuprie perman
ganate
iron(ffl) carbonate, ferric carbonate
d.
e.
f.
g.
4
V
lithium hydrogen carbonate, lithium
bicarbonate
chromium(ffl) suffide, chromic sulf
ide
calcium cyanide
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65
Chapter 5: Nomenclature
58.
a.
gold(IU) bromide, auric bromide
b.
cobalt(fll) cyanide, cobaltic cyanide
c.
magnesium hydrogen phosphate
d.
diboron hexahydride (diborane is its common name)
e.
ammonia
f.
silver(1) sulfate (usually called silver sulfate)
g.
beryllium hydroxide
a
chionc acid
b.
cobalt(lll) chloride; cobaltic chloride
c.
diboron trioxide
d.
water
e.
acetic acid
f.
iron(JL1) nitrate; fenic nitrate
g.
copper(1I) sulfate; cupric sulfate
a.
ammonium carbonate
b.
ammonium hydrogen carbonate, ammonium bicarbonate
c.
calcium phosphate
d.
sulfurous acid
e.
manganese(IV) oxide
f.
iodic acid
g.
potassium hydride
a.
0
2
K
b.
MgO
c.
FeO
d.
3
0
2
Fe
e.
ZnO
59.
V
V
60.
V
V
61.
f
V
g.
PbO
3
0
2
A1
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66
Chapter 5: Nomenclature
:1
62.
63.
a.
3
M
F
4
)
2
0
(C
1
b.
M(Mn0
4
)
c.
2
MO
d.
4
M(I
2
)
-1P0
e.
4
M(O
H)
f.
M(NO
Answers are given, respectively, for the M’
a.
CrO 4
2
M
,
4
MCrO 4
,
(Cr0
2
M
3
)
b.
c.
d.
e.
f.
64.
65.
,
, and M
2
M
3 ions:
Cr O
2
M
,
7
O
2
M
,
7
Cr 0
(Cr
2
M
3
)
7
S, MS, M
2
M
3
S
2
MBr, ,
2r MB
MB
3r
MHCO 3
,
3
M(HCO )
,
2
)
M(HCO
3
[1PO, 4
2
M
MHPO 4
,
(HPO
2
M
3
)
M compounds: MD, 2
M
E
,3
M
F
2 compounds: MD
M
, ME, M
2
2
F
3
3 compounds: MD
M
,M
3
, MF
3
E
2
t:
2
Fe
3
FeC
O
iron(ll) carbonate; ferrous carbonate
iron(1J) bromate; ferrous bromate
3
Fe(
2
)
Br0
Fe(C
)
2
0
3
H
.)r
.,
iron(ll) acetate; ferrous acetate
iron(Il) hydroxide; ferrous hydroxide
2
Fe(
OI{)
3
Fe(
2
)
HCO
iron(ll) bicarbonate; ferrous bicarbonate
iron(l [) phosphate; ferrous phosphate
4
F
(
3
2
)
Pe
0
3
FeS
O
iron(U) sulfite; ferrous sulfite
iron(ll) perchiorate; ferrous perchiorate
4
Fe(
2
)
C10
4
FeS
O
FeO
iron(ll) sulfate; ferrous sulfate
iron(il) oxide; ferrous oxide
2I
FeC
iron(ll) chloride; ferrous chloride
A
(
2
3
)
C0
l
aluminum carbonate
A1(Br0
3
)
aluminum bromate
Al(C
)
2
0
3
H
aluminum acetate
3
Al(
OH)
aluminum hydroxide
3
A
:
l
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-
.-—-
---..
Chapter 5: Nomenclature
)
3
Al(HCO
aluminum bicarbonate
4
AIPO
aluminum phosphate
(S0
2
A1
3
)
aluminum sulfite
3
)
4
Al(C10
aluminum perchiorate
S0
4
(
2
A1
3
)
aluminum sulfate
3
0
2
A1
aluminum oxide
3
A1CI
aluminum chloride
CO
2
Na
3
sodium carbonate
3
NaBrO
sodium bromate
O
3
H
2
NaC
sodium acetate
NaOH
sodium hydroxide
3
NaHCO
sodium bicarbonate
O
4
P
3
Na
sodium phosphate
O
3
S
2
Na
sodium sulfite
4
NaCIO
sodium perchiorate
O
4
S
2
Na
sodium sulfate
0
2
Na
sodium oxide
NaCI
sodium chloride
3
CaCO
calcium carbonate
2
)
3
Ca(Br0
calcium bromate
)
0
3
H
2
Ca(C
calcium acetate
Ca(OH)z
calcium hydroxide
2
)
3
Ca(11C0
calcium bicarbonate
P0
4
(
3
Ca
2
)
calcium phosphate
3
CaSO
calcium sulfite
2
)
4
Ca(C10
calcium perchlorate
4
CaSO
calcium sulfate
CaO
calcium oxide
2
CaCI
calcium chloride
0
3
C
2
)
4
(N}1
ammonium carbonate
BrO
4
NH
3
ammonium bromate
0
3
H
2
C
4
NH
ammonium acetate
+
Na:
:
2
Ca
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67
68
Chapter 5: Nomenclature
4
N
O
H
ammonium hydroxide
3
N
H
4
CO
H
ammonium bicarbonate
(N0
P
3
)
4
H
ammonium phosphate
3
(N
S
2
)
4
11
0
ammonium sulfite
NIO
C
4
H
airunonium perchiorate
(N0
S
3
)
4
H
ammonium sulfate
(NH0
ammonium oxide
NH
C
4
1
ammonium chloride
F
(
2
3
)
Ce
0
iron(III) carbonate
Fe(Br0
3
)
iron(lIl) bromate
Fe(
1
3
)
2
0
1
C
iron(l1 I) acetate
Fe(OH )
iron(lII) hydroxide
Fe(HCO
3
)
iron( III) bicarbonate
4
FeP
O
iron(ffl) phosphate
F
(
2
3
)
Se
0
iron(Ill) sulfite
Fe(C 104)3
iron(Jll) perchiorate
4
F
(
2
3
)
Se
0
iron(1Il) sulfate
3
0
2
Fe
iron(lll) oxide
FeCis
iron(1I1) chloride
3
NiC
O
mckel(Il) carbonate
3
Ni(
2
)
Br0
nickel(IT) bromate
Ni(C
)
2
0
3
H
nickel(11) acetate
2
Ni(
OH)
nickel(lI) hydroxide
3
Ni(
2
)
HCO
nickel(1I) bicarbonate
4
N
(
3
2
)
P0
i
nickel(U) phosphate
3
NiS
O
nickel(I1) sulfite
4
Ni(
2
)
C10
nickel(Il) perchiorate
4
NiS
O
nickel(ll) sulfate
NiO
nickel(I1) oxide
2
NiC
1
nickel(ll) chloride
3
H
C
2
O
g
mercury(l) carbonate
3
H
(
2
)
Br0
g
mercury(T) bromate
:
3
Fe
4’
2
N
:
i
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t.
69
Chapter 5: Nomenclature
1
C
3
(
Hg
1
)
2
0
mercury(1) acetate
(OH)
Hg
2
mercury(I) hydroxide
(HCO
Hg
2
)
3
mercury(l) bicarbonate
(P0
3
(Hg
2
)
4
mercury(I) phosphate
SO
2
Hg
3
mercury(1) sulfite
(C10
Hg
2
)
4
mercury(1) perchiorate
SO
2
Hg
4
mercury(1) sulfate
‘S
‘V
0
2
Hg
mercury(1) oxide
C1
Hg
2
mercury(I) chloride
3
HgCO
mercury(I1) carbonate
2
)
3
Hg(Br0
mercury(II) bromate
1
3
1
Hg(C
)
2
0
mercury(ll) acetate
2
Hg(OH)
mercury(I]) hydroxide
2
)
3
Hg(HCO
mercury(ll) bicarbonate
(P0
3
Hg
2
)
4
mercury(ll) phosphate
3
HgSO
mercury(11) sulfite
2
)
4
Hg(C10
mercury(II) perchiorate
4
HgSO
mercury(I1) sulfate
HgO
mercury(lI) oxide
2
HgCI
mercury(11) chloride
.
.-“.:‘
‘V.’
:
24
Hg
;‘•
“V
•c
66.
Ca(N0
2
)
3
2
)
3
Sr(N0
NO
4
NH
3
)
3
A1(N0
)
3
Fe(N0
2
)
3
Ni(N0
3
•AgNO
)
3
Au(N0
3
KNO
2
)
3
Hg(N0
2
)
3
Ba(N0
CaSO
4
4
SrSO
SO
2
(NH)
4
(S0
2
A1
3
)
4
(S0
2
Fe
3
)
4
4
NiSO
SO
2
Ag
4
(S0
2
Au
3
)
4
S0
2
K
4
4
HgSO
4
BaSO
Ca(HSO
2
)
4
2
)
4
Sr(HSO
HSO
NH
4
5
)
4
AlHSO
)s
4
J?e(J1S0
2
Ni(HSO4)
4
AgHSO
3
)
4
Au(HSO
4
KHSO
2
)
4
Hg(11S0
2
)
4
Ba(HSO
4
P
CaH
2
)
O
P0
Sr(H
2
)
4
PO
2
H
NI1
4
P0
2
AJ(H
3
)
4
P0
2
Fe(H
3
)
4
P0
Ni(H
2
)
4
PO
2
AgH
4
P0
2
Au(11
3
)
4
PO
2
KH
4
P0
Hg(H
2
)
4
P0
Ba(H
2
)
4
67.
unreactive
68.
helium
69.
two
70.
iodine (solid), bromine (liquid), fluorine and chlorine (gases)
CaO
SrO
O
2
(N}L)
A1
3
0
2
3
0
2
Fe
NiO
0
2
Ag
3
0
2
Au
0
2
K
HgO
BaO
‘
CaC1
2
2
SrCI
C1
4
NH
3
Aid
3
FeC1
2
Nicl
AgC1
3
AuCI
KC1
2
HgC1
2
BaCI
-
Copyright © Houghton MIfflin Company. AU rights reserved.
4
ç;4’:’
70
I
Chapter 5: Nomenclature
71.
2—
72.
73.
3+
74.
1—
75.
[1]
e
[2]
a
[3]
a
[4]
g
[5]
g
[6]
f
[1
g
[8]
a
[91
e
[10]
j
:
:
.‘
76.
a.
A1(13e)
b.
c.
S(I6e)+2e — S(18e)
Cu(29e)
Cu(28e) + e
d.
F(9e)
e.
Zn(30e”)
f.
P(15e)+3e
a.
none likely (Element 36, Kr, is a noble
gas.)
3
Ga
(Element 31, Ga, is in Group 3.)
2
Te
(Element 52, Te, is in Group 6.)
3
A
(
l0e)
[ + 3e
-4
-
+
e
-4
-4
F(10e)
I
2
Z
(
28n
e) + 2e
—*
P
(
3
18e)
77.
b.
c.
d.
e.
Bf
(Element 81, Ti, is in Group 3.)
(Element 35, Br, is in Group 7.)
f.
Fr
(Element 87, Fr, is in Group 1.)
-
.
‘
I
78.
a.
Two 1+ ions are needed to balance a 2—
ion, so the formula must have two Na ions
for each
S ion; 2
2
Na
S
.
b.
One 1+ ion exactly balances a 1— ion, so
the formula should have an equal number
of K and
C1 ions; KC1.
c.
One 2+ ion exactly balances a 2— ion,
so the fonnula musthave an equalnumb of
er Ba
” and
2
ions; BaO.
02
Copyright © Houghton Mifflin Company. All rights
reserved.
Chapter 5: Nomenclature
71
d.
2
One 2+ ion exactly balances a 2— ion, so the formula must have an equal number of Mg
and Se
2 ions; MgSe.
e.
One 2-f ion requires two 1— ions to balance charge, so the formula must have twice as many
.
2
2 ions; CuBr
Br ions as Cu
f,
One 3± ion requires three 1— ions to balance charge, so the formula must have three times as
.
3
3 ions; All
many 1 ions as Al
g.
Two 3± ions give a total of 6+, whereas three 2— ions will give a total of 6--. The formula
.
3
0
2
3 ions and three 02_ ions; A1
then should contain two Al
2
Three 2-f ions are required to balance two 3— ions, so the formula must contain three Ca
.
2
N
3
Ca
ions;
two
3
N
ions for every
h.
79.
a.
beryllium oxide
b.
magnesium iodide
c.
sodium sulfide
d.
aluminum oxide
e.
hydrogen chloride (gaseous); hydrochloric acid (aqueous)
f.
lithium fluoride
g.
silver(I) sulfide; usually called silver sulfide
h.
calcium hydride
a.
silver(I) oxide or just silver oxide
b.
correct
C,
iron(IT1) oxide
d.
plumbic oxide
e.
correct
-
.
-
-
-
-
-
80.
-
81.
-
a.
As the bromide ion must have a 1— charge, the iron ion must be in the 2+ state; the name is
iron(ll) bromide.
As the sulfide ion always has a 2— charge, the cobalt ion must be in the 2+ state; the name is
cobalt(ll) suffide.
As the sulfide ion always has a 2— charge, and as there are three sulfide ions present, each
cobaltion must be in the 3± state; the name is cobalt(ffl) sulfide.
-
b.
c.
d.
e.
1’.
-
As the oxide ion always has a 2— charge, the tin ion must be in the 4+ state; the name is
tin(IV) oxide.
As chloride ion always has a 1— charge, each mercury ion must be in the 1+ state; thç name
is mercury(1) chloride.
As chloride ion always has a 1— charge, the mercury ion must be in the 2+ state; the name is
mercury(ll) chloride.
Copyright © Houghton Muffin Company. All rights reserved.
72
Chapter 5: Nomenclature
82.
a.
As bromide ions always have
a 1— charge, the cobalt ion mu
st have a 3+ charge; the name
cobaltic bromide.
is
As iodide ions always have a
1— charge, the lead ion must
have a 4+ charge; the name is
plumbic iodide.
b.
c.
As oxide ions always have a 2—
charge, and as there are three
oxide ions, each iron ion must
have a 3+ charge; the name is
ferric oxide.
As sulfide ions always have a
2— charge, the iron ion must hav
e a 2+ charge; the name is
ferrous sulfide.
As chloride ions always hav
e a 1— charge, the tin ion must hav
e a 4+ charge; the name is
stannic chloride.
d.
e.
f.
As oxide ions always have a
2— charge, the tin ion must have
a 2+ charge; the name is
stannous oxide.
a.
xenon hexafluoride
b.
oxygen difluoride
c.
arsenic triiodide
d.
dinitrogen tetraoxide (tetroxid
e.
dichiorine monoxide
f.
sulfur hexafluoride
a.
b
iron(ffl) acetate, ferric acetate
bromine monofluonde
c
potassium peroxide
d.
silicon teträbromide
83.
e)
84.
e.
85.
86.
copper([E) permanganate, cup
ric permanganate
f.
calcium chromate
nitrate (The ending —ate alw
ays implies the larger number
of oxygen atoms.)
a.
3
C
2
0
b
3
HC
O
c.
O
3
H
2
C
d.
CN
i.
Copyright © Houghton Mifflin Com
pany. All rights reserved.
A,
-
Chapter 5 Nomenclature
87.
a.
Cr2+
b.
2
4
Cr0
c.
3
Cr
d.
7
0
2
Cr
a.
carbonate
b.
chlorate
c.
sulfate
d.
phosphate
e.
perchiorate
f.
permanganate
a.
lithium dihydrogen phosphate
b.
copper(ll) cyanide
c.
lead(II) nitrate
d.
sodium hydrogen phosphate
e.
sodium chlorite
f.
cobalt(lll) sulfate
88.
89.
90. Answer depends on student choices.
91.
a.
.
2
SO
b.
0
2
N
c.
4
XeF
d.
10
0
4
P
e.
5
PCi
f.
6
SF
g.
2
NO
a.
PO
2
NaH
4
b.
4
LiC1O
c.
2
)
3
Cu(HCO
d.
0
3
H
2
KC
92.
Copyright © Houghton Mifflin Company. All rights reserved.
73
74
Chapter 5: Nomenclature
e.
2
Ba0
f.
3
CsSO
a.
4
AgCIO
b.
3
Co(OH)
c.
NaCIO or NaOCI
d.
Cr
K
7
O
2
e.
N0
4
NH
2
f.
Fe(OH)
g.
HCO
4
NH
3
h.
4
KBrO
93.
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rights reserved.