CHAPTER 5
Nomenclature
1.
a.
It was very sweet-tasting.
b.
lead(II) acetate, plumbous acetate
c.
There are millions of known chemical compounds and a system of nomenclature is
essential for communication among scientists.
2.
A binary 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.
positive; negative
4.
anion (negative ion)
5.
cation
6.
Sodium chloride consists of Na+ ions and Cl– ions in an extended crystal lattice array. No discrete
NaCl pairs are present.
7.
–ous, –ic
8.
Roman numeral
9.
a.
sodium bromide
b.
magnesium chloride
c.
aluminum phosphide
d.
strontium bromide
e.
silver iodide [or less frequently as silver(I) iodide]
f.
potassium sulfide
10.
a.
lithium iodide
b.
magnesium fluoride
c.
strontium oxide
d.
aluminum bromide
e.
calcium sulfide
f.
sodium oxide
56
Chapter 5: Nomenclature
11.
a.
correct
b.
incorrect; lead(II) chloride
c.
correct
d.
incorrect; sodium sulfide
e.
correct
12.
a.
incorrect; copper(II) chloride
b.
correct
c.
correct
d.
incorrect; calcium sulfide
e.
correct
13.
a.
As the chloride ion has a 1– charge, the tin ion must have a 4+ charge: the name is
tin(IV) chloride.
b.
As the sulfide ion has a 2– charge, the iron ion must have a 3+ charge: the name is
iron(III) sulfide.
c.
As the oxide ion has a 2– charge, the lead ion must have a 4+ charge: the name is
lead(IV) oxide.
d.
As the sulfide ion has a 2– charge, each chromium ion must have a 3+ charge: the name
is chromium(III) sulfide.
e.
As the oxide ion has a 2– charge, the copper ion must have a 2+ charge: the name is
copper(II) oxide.
f.
As the oxide ion has a 2– charge, each copper ion must have a 1+ charge: the name is
copper(I) oxide.
14.
a.
As the iodide ion has a 1– charge, the iron ion must have a 3+ charge: the name is
iron(III) iodide.
b.
As the chloride ion has a 1– charge, the manganese ion must have a 2+ charge: the name
is manganese(II) chloride.
c.
As the oxide ion has a 2– charge, the mercury ion must have a 2+ charge: the name is
mercury(II) oxide.
d.
As the sulfide ion has a 2– charge, each copper ion must have a 1+ charge: the name is
copper(I) sulfide.
e.
As the oxide ion has a 2– charge, the cobalt ion must have a 2+ charge: the name is
cobalt(II) oxide.
f.
As the bromide ion has a 1– charge, the tin ion must have a 4+ charge: the name is
tin(IV) bromide.
57
Chapter 5: Nomenclature
15.
a.
As each chloride ion has a 1– charge, the copper ion must have a 1+ charge: cuprous
chloride.
b.
As each oxide ion has a 2– charge, the iron ion must have a 3+ charge: the name is ferric
oxide.
c.
As each chloride ion has a 1– charge, each mercury atom must have a 1+ charge: the
name is mercurous chloride.
d.
As each chloride ion has a 1– charge, the manganese ion must have a 2+ charge: the
name is manganous chloride.
e.
As each oxide ion has a 2– charge, the titanium ion must have a 4+ charge: the name is
titanic oxide.
f.
As the oxide ion has a 2– charge, the lead ion must have a 2+ charge: the name is
plumbous oxide.
16.
a.
As each chloride ion has a 1– charge, the cobalt ion must have a 2+ charge: the name is
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 each 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 the oxide ion has a 2– charge, the cobalt ion must have a 3+ charge: the name is
cobaltic oxide.
f.
As the chloride ion has a 1– charge, the iron ion must have a 3+ charge: the name is ferric
chloride.
17.
Remember that for this type of compound of nonmetals, numerical prefixes are used to indicate
how many of each type of atom are 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.
krypton difluoride
b.
diselenium hexasulfide
c.
arsenic trihydride
d.
xenon tetr(a)oxide (the a is usually omitted for easier pronunciation)
e.
bromine trifluoride
f.
diphosphorus pentasulfide
18.
Remember that for this type of compound of nonmetals, numerical prefixes are used to indicate
how many of each type of atom are 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.
chlorine pentafluoride
b.
xenon dichloride
58
Chapter 5: Nomenclature
c.
selenium dioxide
d.
dinitrogen trioxide
e.
diiodine hexachloride
f.
carbon disulfide
19.
a.
iron(II) phosphide, ferrous phosphide – ionic
b.
calcium bromide – ionic
c.
dinitrogen pentoxide – nonionic
d.
lead(IV) chloride, plumbic chloride – ionic
e.
disulfur decafluoride – nonionic
f.
copper(I) oxide, cuprous oxide – ionic
20.
Na2O: sodium oxide; N2O: dinitrogen monoxide; For Na2O, the compound contains a metal and a
nonmetal in which the charges must balance. When forming this compound, Na always forms a
1+ charge and oxygen always forms a 2– charge. Therefore, the prefixes are not needed. For N2O,
the compound contains only nonmetals and the charges do not have to balance. Therefore
prefixes are needed to tell us how many of each atom are present.
21.
a.
magnesium sulfide – ionic
b.
aluminum chloride – ionic
c.
phosphorus trihydride (the common name phosphine is always used)
d.
chlorine monobromide – nonionic
e.
lithium oxide – ionic
f.
tetraphosphorus decoxide – nonionic
22.
a.
radium chloride – ionic
b.
selenium dichloride – nonionic
c.
phosphorus trichloride – nonionic
d.
sodium phosphide – ionic
e.
manganese(II) fluoride (or manganous fluoride) – ionic
f.
zinc oxide – ionic
23.
A polyatomic ion is a group of atoms bound together that, as a unit, carries an electrical charge.
Examples will depend on student responses.
24.
oxyanion
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.
59
Chapter 5: Nomenclature
27.
ClO4– perchlorate
ClO–
hypochlorite
ClO3– chlorate
ClO2– chlorite
28.
IO–
hypoiodite
IO2–
iodite
IO3–
iodate
IO4–
periodate
29.
a.
P3–
b.
PO43–
c.
PO33–
d.
HPO42–
30.
a.
CN–
b.
CO32–
c.
HCO3–
d.
C2H3O2–
31.
a.
NaCN
b.
CaCO3
c.
KHCO3
d.
Mg(C2H3O2)2
32.
CN–
cyanide
CO32–
carbonate
HCO3–
hydrogen carbonate (or bicarbonate)
C2H3O2–
acetate
33.
a.
hydrogen carbonate, bicarbonate
b.
acetate
c.
cyanide
d.
hydroxide
e.
nitrite
f.
hydrogen phosphate
34.
a.
ammonium
b.
dihydrogen phosphate
60
Chapter 5: Nomenclature
c.
sulfate
d.
hydrogen sulfite (also called bisulfite)
e.
perchlorate
f.
iodate
35.
a.
ammonium nitrate
b.
calcium hydrogen carbonate, calcium bicarbonate
c.
magnesium sulfate
d.
sodium hydrogen phosphate
e.
potassium perchlorate
f.
barium acetate
36.
a.
sodium permanganate
b.
aluminum phosphate
c.
chromium(II) carbonate, chromous carbonate
d.
calcium hypochlorite
e.
barium carbonate
f.
calcium chromate
37.
An acid is a substance that produces hydrogen ions, H+, when dissolved in water.
38.
oxygen (commonly referred to as oxyacids)
39.
a.
hydrochloric acid
b.
sulfuric acid
c.
nitric acid
d.
hydroiodic acid
e.
nitrous acid
f.
chloric acid
g.
hydrobromic acid
h.
hydrofluoric acid
i.
acetic acid
40.
a.
hypochlorous acid
b.
sulfurous acid
c.
bromic acid
d.
hypoiodous acid
e.
perbromic acid
f.
hydrosulfuric acid
61
Chapter 5: Nomenclature
g.
hydroselenic acid
h.
phosphorous acid
41.
a.
CoCl2
b.
CoCl3
c.
Na3P
d.
FeO
e.
CaH2
f.
MnO2
g.
MgI2
h.
Cu2S
42.
a.
MgF2
b.
FeI3
c.
HgS
d.
Ba3N2
e.
PbCl2
f.
SnF4
g.
Ag2O
h.
K2Se
43.
a.
CS2
b.
H2O
c.
N2O3
d.
Cl2O7
e.
CO2
f.
NH3
g.
XeF4
44.
a.
P2O
b.
SO2
c.
P2O5
d.
CCl4
e.
NBr3
f.
SiF4
g.
SCl2
62
Chapter 5: Nomenclature
45.
a.
NH4NO3
b.
Mg(C2H3O2)2
c.
CaO2
d.
KHSO4
e.
FeSO4
f.
KHCO3
g.
CoSO4
h.
LiClO4
46.
a.
NH4C2H3O2
b.
Fe(OH)2
c.
Co2(CO3)3
d.
BaCr2O7
e.
PbSO4
f.
KH2PO4
g.
Li2O2
h.
Zn(ClO3)2
47.
a.
H2S
b.
HBrO4
c.
HC2H3O2
d.
HBr
e.
HClO2
f.
H2Se
g.
H2SO3
h.
HClO4
48.
a.
HCN
b.
HNO3
c.
H2SO4
d.
H3PO4
e.
HClO or HOCl
f.
HBr
g.
HBrO2
h.
HF
63
Chapter 5: Nomenclature
49.
a.
Na2O2
b.
Ca(ClO3)2
c.
RbOH
d.
Zn(NO3)2
e.
(NH4)2Cr2O7
f.
H2S(aq)
g.
CaBr2
h.
HOCl(aq)
i.
K2SO4
j.
HNO3(aq)
k.
Ba(C2H3O2)2
l.
Li2SO3
50.
a.
Ca(HSO4)2
b.
Zn3(PO4)2
c.
Fe(ClO4)3
d.
Co(OH)3
e.
K2CrO4
f.
Al(H2PO4)3
g.
LiHCO3
h.
Mn(C2H3O2)2
i.
MgHPO4
j.
CsClO2
k.
BaO2
l.
NiCO3
51.
Formula
Roman Numeral Name
–ous/–ic Name
FeO
iron(II) oxide
ferrous oxide
Fe2O3
iron(III) oxide
ferric oxide
FeS
iron(II) sulfide
ferrous sulfide
Fe2S3
iron(III) sulfide
ferric sulfide
FeCl2
iron(II) chloride
ferrous chloride
FeCl3
iron(III) chloride
ferric chloride
52.
A moist paste of NaCl would contain Na+ and Cl– ions in solution, and would serve as a
conductor of electrical impulses.
53.
NO, nitrogen monoxide; NO2, nitrogen dioxide; N2O4, dinitrogen tetr(a)oxide; N2O5, dinitrogen
pent(a)oxide; N2O, dinitrogen monoxide
64
Chapter 5: Nomenclature
54.
H H+ (hydrogen ion: a cation) + e–
H + e– H– (hydride ion: an anion)
55.
(e); The correct name for (a) is aluminum sulfide. The correct name for (b) is copper(I) nitrate.
The correct name for (c) is iron(II) perchlorate. The correct name for (d) is cesium bromide.
56.
missing oxyanions:
IO3–; ClO2–
missing oxyacids:
HClO4; HClO; HBrO2
57.
a.
calcium acetate
b.
phosphorus trichloride
c.
copper(II) permanganate, cupric permanganate
d.
iron(III) carbonate, ferric carbonate
e.
lithium hydrogen carbonate, lithium bicarbonate
f.
chromium(III) sulfide, chromic sulfide
g.
calcium cyanide
58.
a.
gold(III) bromide, auric bromide
b.
cobalt(III) cyanide, cobaltic cyanide
c.
magnesium hydrogen phosphate
d.
diboron hexahydride (diborane is its common name)
e.
ammonia
f.
silver(I) sulfate (usually called silver sulfate)
g.
beryllium hydroxide
59.
a.
chloric acid
b.
cobalt(III) chloride; cobaltic chloride
c.
diboron trioxide
d.
water
e.
acetic acid
f.
iron(III) nitrate; ferric nitrate
g.
copper(II) sulfate; cupric sulfate
60.
(b); iron(II) oxide has the formula FeO
61.
a.
K2O
b.
MgO
c.
FeO
d.
Fe2O3
e.
ZnO
65
Chapter 5: Nomenclature
f.
PbO
g.
Al2O3
62.
a.
M(C2H3O2)2
b.
M(MnO4)2
c.
MO
d.
MHPO4
e.
M(OH)2
f.
M(NO2)2
63.
Answers are given, respectively, for the M1+, M2+, and M3+ ions:
a.
M2CrO4, MCrO4, M2(CrO4)3
b.
M2Cr2O7, MCr2O7, M2(Cr2O7)3
c.
M2S, MS, M2S3
d.
MBr, MBr2, MBr3
e.
MHCO3, M(HCO3)2, M(HCO3)3
f.
M2HPO4, MHPO4, M2(HPO4)3
64.
a.
The metal ion is Mn2+. Since the metal ion has 23 electrons and contains a 2+ charge,
this means that it has two less electrons as compared to protons. Therefore the number of
protons is 25. The number of protons is also the atomic number, identifying the metal
ion as manganese.
b.
The halogen ion is Cl– with 18 electrons. The number of protons is 17, identifying the
element as chlorine. Halogens form a 1– charge when bonding with a metal to form an
ionic compound, thus the ion has one more electron as compared to protons.
c.
Since the chloride ion has a 1– charge and the manganese ion has a 2+ charge, the
formula is MnCl2 and is named manganese(II) chloride (or manganous chloride). The
charge on manganese must be specified using the Roman numeral.
65.
Fe2+:
FeCO3
iron(II) carbonate; ferrous carbonate
Fe(BrO3)2
iron(II) bromate; ferrous bromate
Fe(C2H3O2)2
iron(II) acetate; ferrous acetate
Fe(OH)2
iron(II) hydroxide; ferrous hydroxide
Fe(HCO3)2
iron(II) bicarbonate; ferrous bicarbonate
Fe3(PO4)2
iron(II) phosphate; ferrous phosphate
FeSO3
iron(II) sulfite; ferrous sulfite
Fe(ClO4)2
iron(II) perchlorate; ferrous perchlorate
FeSO4
iron(II) sulfate; ferrous sulfate
FeO
iron(II) oxide; ferrous oxide
66
Chapter 5: Nomenclature
FeCl2
iron(II) chloride; ferrous chloride
Al3+:
Al2(CO3)3
aluminum carbonate
Al(BrO3)3
aluminum bromate
Al(C2H3O2)3
aluminum acetate
Al(OH)3
aluminum hydroxide
Al(HCO3)3
aluminum bicarbonate
AlPO4
aluminum phosphate
Al2(SO3)3
aluminum sulfite
Al(ClO4)3
aluminum perchlorate
Al2(SO4)3
aluminum sulfate
Al2O3
aluminum oxide
AlCl3
aluminum chloride
Na+:
Na2CO3
sodium carbonate
NaBrO3
sodium bromate
NaC2H3O2
sodium acetate
NaOH
sodium hydroxide
NaHCO3
sodium bicarbonate
Na3PO4
sodium phosphate
Na2SO3
sodium sulfite
NaClO4
sodium perchlorate
Na2SO4
sodium sulfate
Na2O
sodium oxide
NaCl
sodium chloride
Ca2+:
CaCO3
calcium carbonate
Ca(BrO3)2
calcium bromate
Ca(C2H3O2)2
calcium acetate
Ca(OH)2
calcium hydroxide
Ca(HCO3)2
calcium bicarbonate
Ca3(PO4)2
calcium phosphate
CaSO3
calcium sulfite
Ca(ClO4)2
calcium perchlorate
CaSO4
calcium sulfate
67
Chapter 5: Nomenclature
CaO
calcium oxide
CaCl2
calcium chloride
NH4+:
(NH4)2CO3
ammonium carbonate
NH4BrO3
ammonium bromate
NH4C2H3O2
ammonium acetate
NH4OH
ammonium hydroxide
NH4HCO3
ammonium bicarbonate
(NH4)3PO4
ammonium phosphate
(NH4)2SO3
ammonium sulfite
NH4ClO4
ammonium perchlorate
(NH4)2SO4
ammonium sulfate
(NH4)2O
ammonium oxide
NH4Cl
ammonium chloride
Fe3+:
Fe2(CO3)3
iron(III) carbonate; ferric carbonate
Fe(BrO3)3
iron(III) bromate; ferric bromate
Fe(C2H3O2)3
iron(III) acetate; ferric acetate
Fe(OH)3
iron(III) hydroxide; ferric hydroxide
Fe(HCO3)3
iron(III) bicarbonate; ferric bicarbonate
FePO4
iron(III) phosphate; ferric phosphate
Fe2(SO3)3
iron(III) sulfite; ferric sulfite
Fe(ClO4)3
iron(III) perchlorate; ferric perchlorate
Fe2(SO4)3
iron(III) sulfate; ferric sulfate
Fe2O3
iron(III) oxide; ferric oxide
FeCl3
iron(III) chloride; ferric chloride
Ni2+:
NiCO3
nickel(II) carbonate
Ni(BrO3)2
nickel(II) bromate
Ni(C2H3O2)2
nickel(II) acetate
Ni(OH)2
nickel(II) hydroxide
Ni(HCO3)2
nickel(II) bicarbonate
Ni3(PO4)2
nickel(II) phosphate
NiSO3
nickel(II) sulfite
Ni(ClO4)2
nickel(II) perchlorate
68
Chapter 5: Nomenclature
NiSO4
nickel(II) sulfate
NiO
nickel(II) oxide
NiCl2
nickel(II) chloride
Hg22+:
Hg2CO3
mercury(I) carbonate; mercurous carbonate
Hg2(BrO3)2
mercury(I) bromate; mercurous bromate
Hg2(C2H3O2)2
mercury(I) acetate; mercurous acetate
Hg2(OH)2
mercury(I) hydroxide; mercurous hydroxide
Hg2(HCO3)2
mercury(I) bicarbonate; mercurous bicarbonate
(Hg2)3(PO4)2
mercury(I) phosphate; mercurous phosphate
Hg2SO3
mercury(I) sulfite; mercurous sulfite
Hg2(ClO4)2
mercury(I) perchlorate; mercurous perchlorate
Hg2SO4
mercury(I) sulfate; mercurous sulfate
Hg2O
mercury(I) oxide; mercurous oxide
Hg2Cl2
mercury(I) chloride; mercurous chloride
Hg2+:
HgCO3
mercury(II) carbonate; mercuric carbonate
Hg(BrO3)2
mercury(II) bromate; mercuric bromate
Hg(C2H3O2)2
mercury(II) acetate; mercuric acetate
Hg(OH)2
mercury(II) hydroxide; mercuric hydroxide
Hg(HCO3)2
mercury(II) bicarbonate; mercuric bicarbonate
Hg3(PO4)2
mercury(II) phosphate; mercuric phosphate
HgSO3
mercury(II) sulfite; mercuric sulfite
Hg(ClO4)2
mercury(II) perchlorate; mercuric perchlorate
HgSO4
mercury(II) sulfate; mercuric sulfate
HgO
mercury(II) oxide; mercuric oxide
HgCl2
mercury(II) chloride; mercuric chloride
69
Chapter 5: Nomenclature
66.
Ca(NO3)2
CaSO4
Ca(HSO4)2
Ca(H2PO4)2
CaO
CaCl2
Sr(NO3)2
SrSO4
Sr(HSO4)2
Sr(H2PO4)2
SrO
SrCl2
NH4NO3
(NH4)2SO4
NH4HSO4
NH4H2PO4
(NH4)2O
NH4Cl
Al(NO3)3
Al2(SO4)3
Al(HSO4)3
Al(H2PO4)3
Al2O3
AlCl3
Fe(NO3)3
Fe2(SO4)3
Fe(HSO4)3
Fe(H2PO4)3
Fe2O3
FeCl3
Ni(NO3)2
NiSO4
Ni(HSO4)2
Ni(H2PO4)2
NiO
NiCl2
AgNO3
Ag2SO4
AgHSO4
AgH2PO4
Ag2O
AgCl
Au(NO3)3
Au2(SO4)3
Au(HSO4)3
Au(H2PO4)3
Au2O3
AuCl3
KNO3
K2SO4
KHSO4
KH2PO4
K2O
KCl
Hg(NO3)2
HgSO4
Hg(HSO4)2
Hg(H2PO4)2
HgO
HgCl2
Ba(NO3)2
BaSO4
Ba(HSO4)2
Ba(H2PO4)2
BaO
BaCl2
67.
unreactive
68.
(NH4)3PO4
69.
two
70.
iodine (solid), bromine (liquid), fluorine and chlorine (gases)
71.
2–
72.
1+
73.
3+
74.
2–
75.
[ 1]
e
[ 2]
a
[ 3]
a
[ 4]
g
[ 5]
g
[ 6]
f
[ 7]
g
[ 8]
a
[ 9]
e
[10]
j
76.
a.
Al(13e–) Al3+(10e–) + 3e–
b.
S(16e–) + 2e– S2–(18e–)
c.
Cu(29e–) Cu+(28e–) + e–
d.
F(9e–) + e– F–(10e–)
e.
Zn(30e–) Zn2+(28e–) + 2e–
f.
P(15e–) + 3e– P3–(18e–)
70
Chapter 5: Nomenclature
77.
a.
none likely
(element 36, Kr, is a noble gas)
b.
Ga3+
(element 31, Ga, is in Group 3)
c.
Te2–
(element 52, Te, is in Group 6)
d.
Tl3+
(element 81, Tl, is in Group 3)
e.
Br–
(element 35, Br, is in Group 7)
f.
Fr+
(element 87, Fr, is in Group 1)
78.
a.
Two 1+ ions are needed to balance a 2– ion, so the formula must have two Na+ ions for
each S2– ion: Na2S.
b.
One 1+ ion exactly balances a 1– ion, so the formula should have an equal number of K+
and Cl– ions: KCl.
c.
One 2+ ion exactly balances a 2– ion, so the formula must have an equal number of Ba2+
and O2– ions: BaO.
d.
One 2+ ion exactly balances a 2– ion, so the formula must have an equal number of Mg2+
and Se2– ions: MgSe.
e.
One 2+ ion requires two 1– ions to balance charge, so the formula must have twice as
many Br– ions as Cu2+ ions: CuBr2.
f.
One 3+ ion requires three 1– ions to balance charge, so the formula must have three times
as many I– ions as Al3+ ions: AlI3.
g.
Two 3+ ions give a total of 6+, whereas three 2– ions will give a total of 6–. The formula
then should contain two Al3+ ions and three O2– ions: Al2O3.
h.
Three 2+ ions are required to balance two 3– ions, so the formula must contain three Ca2+
ions for every two N3– ions: Ca3N2.
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
80.
a.
silver(I) oxide or just silver oxide
b.
correct
c.
iron(III) oxide or ferric oxide
d.
lead(IV) oxide or plumbic oxide
e.
correct
71
Chapter 5: Nomenclature
81.
a.
As the bromide ion must have a 1– charge, the iron ion must be in the 2+ state: the name
is iron(II) bromide.
b.
As sulfide ion always has a 2– charge, the cobalt ion must be in the 2+ state: the name is
cobalt(II) sulfide.
c.
As sulfide ion always has a 2– charge, and as there are three sulfide ions present, each
cobalt ion must be in the 3+ state: the name is cobalt(III) sulfide.
d.
As oxide ion always has a 2– charge, the tin ion must be in the 4+ state: the name is
tin(IV) oxide.
e.
As chloride ion always has a 1– charge, each mercury ion must be in the 1+ state: the
name is mercury(I) chloride.
f.
As chloride ion always has a 1– charge, the mercury ion must be in the 2+ state: the name
is mercury(II) chloride.
82.
a.
stannous chloride
b.
ferrous oxide
c.
stannic oxide
d.
plumbous sulfide
e.
cobaltic sulfide
f.
chromous chloride
83.
a.
xenon hexafluoride
b.
oxygen difluoride
c.
arsenic triiodide
d.
dinitrogen tetraoxide (tetroxide)
e.
dichlorine monoxide
f.
sulfur hexafluoride
84.
a.
iron(III) acetate, ferric acetate
b.
bromine monofluoride
c.
potassium peroxide
d.
silicon tetrabromide
e.
copper(II) permanganate, cupric permanganate
f.
calcium chromate
85.
nitrate (the ending –ate always implies the larger number of oxygen atoms)
86.
(a); The correct name is aluminum sulfide.
87.
a.
Cr2+
b.
CrO42–
c.
Cr3+
72
Chapter 5: Nomenclature
d.
Cr2O72–
88.
a.
carbonate
b.
chlorate
c.
sulfate
d.
phosphate
e.
perchlorate
f.
permanganate
89.
a.
lithium dihydrogen phosphate
b.
copper(II) cyanide or cupric cyanide
c.
lead(II) nitrate or plumbous nitrate
d.
sodium hydrogen phosphate
e.
sodium chlorite
f.
cobalt(III) sulfate
90.
RbCl; Alkali metals form a 1+ charge when bonding with a nonmetal to form an ionic compound.
Since the ion contains 36 electrons and has a 1+ charge, this means it has one more proton as
compared to electrons. The number of protons is therefore 37, identifying the ion as rubidium.
91.
a.
SO2
b.
N2O
c.
XeF4
d.
P4O10
e.
PCl5
f.
SF6
g.
NO2
92.
a.
NaH2PO4
b.
LiClO4
c.
Cu(HCO3)2
d.
KC2H3O2
e.
BaO2
f.
Cs2SO3
93.
a.
AgClO4
b.
Co(OH)3
c.
NaClO or NaOCl
d.
K2Cr2O7
73
Chapter 5: Nomenclature
e.
NH4NO2
f.
Fe(OH)3
g.
NH4HCO3
h.
KBrO4
94.
Atom
G or L
Ion
K
L
K+
Cs
L
Cs+
Br
G
Br–
S
G
S2–
Se
G
Se2–
95.
Compound Name
Formula
Carbon tetrabromide
CBr4
Cobalt(II) phosphate
Co3(PO4)2
Magnesium chloride
MgCl2
Nickel(II) acetate
Ni(C2H3O2)2
Calcium nitrate
Ca(NO3)2
96.
Formula
Compound Name
Co(NO2)2
cobalt(II) nitrite or cobaltous nitrite
AsF5
arsenic pentafluoride
LiCN
lithium cyanide
K2SO3
potassium sulfite
Li3N
lithium nitride
PbCrO4
lead(II) chromate or plumbous chromate
97.
Formula
Compound Name
H2SO3
sulfurous acid
HC2H3O2
acetic acid
HClO4
perchloric acid
HOCl
hypochlorous acid
HCN
hydrocyanic acid
98.
(b) and (d); The symbols for the elements magnesium, aluminum, and xenon are Mg, Al, and Xe,
respectively. Ga is expected to lose electrons to form ions in ionic compounds. The correct name
for TiO2 is titanium(IV) oxide.
74
