Chapter 4
Nomenclature
1.
A binary compound is one that contains only two elements. Examples are sodium chloride, water, and carbon dioxide.
2.
compounds that contain a metal and a nonmetal; compounds containing two nonmetals
3.
cation, anion
4.
cation
5.
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 NaCl to indicate the relative number of each ion in the substance.
6.
a.
sodium iodide
b.
calcium fluoride
c.
aluminum sulfide
d.
calcium bromide
e.
strontium oxide
f.
silver chloride [silver(I) chloride]
g.
cesium iodide
h.
lithium oxide
a.
Incorrect; BaH2 is barium hydride.
b.
Incorrect; Na2O is sodium oxide.
c.
Correct
d.
Incorrect; SiO2 is silicon dioxide.
e.
Correct
a.
Since each iodide ion has a 1– charge, the iron ion must have a 3+ charge: the name is iron(III) iodide.
b.
Since each chloride ion has a 1– charge, the manganese must have a 2+ charge: the name is manganese(II) chloride.
c.
Since the oxide ion has a 2– charge, the mercury ion must have a 2+ charge: the name is mercury(II) oxide.
d.
Since the oxide ion has a 2– charge, the copper atoms must each have a 1+ charge: the name is copper(I) oxide.
e.
Since the oxide ion has a 2– charge, the copper ion must have a 2+ charge: copper(II) oxide.
f.
Since each bromide ion has a 1– charge, the tin ion must have a 4+ charge: tin(IV) bromide.
7.
8.
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9.
10.
11.
12.
13.
Chapter 4
a.
Since each chloride ion has a 1– charge, the cobalt ion must have a 2+ charge: cobaltous chloride.
b.
Since each bromide ion has a 1– charge, the chromium ion must have a 3+ charge: the name is chromic bromide.
c.
Since the oxide ion has a 2– charge, the lead ion must have a 2+ charge: the name is plumbous oxide.
d.
Since each oxide ion has a 2– charge, the tin ion must have a 4+ charge: the name is stannic oxide.
e.
Since each oxide ion has a 2– charge, the iron ion must have a 3+ charge: the name is ferric oxide.
f.
Since each chloride ion has a 1– charge, the iron ion must have a 3+ charge: the name is ferric chloride.
Remember that for this type of compound of nonmetals, numerical prefixes are used 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 trichloride
c.
selenium monoxide
d.
xenon tetrafluoride
e.
nitrogen triiodide
f.
diboron trioxide
a.
germanium tetrahydride
b.
dinitrogen tetrabromide
c.
diphosphorus pentasulfide
d.
selenium dioxide
e.
ammonia (nitrogen trihydride)
f.
silicon dioxide
a.
diboron hexahydride – nonionic (common name: diborane)
b.
calcium nitride – ionic
c.
carbon tetrabromide – nonionic
d.
silver sulfide – ionic
e.
copper(II) chloride, cupric chloride – ionic
f.
chlorine monofluoride – nonionic
a.
radium chloride – ionic
b.
selenium dichloride – nonionic
c.
phosphorus trichloride – nonionic
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Nomenclature
14.
d.
sodium phosphide – ionic
e.
manganese(II) fluoride – ionic
f.
zinc oxide – ionic
An oxyanion is a polyatomic anion containing oxygen combined with another element. The following oxyanions of bromine illustrate the nomenclature: BrO– BrO2– BrO3– BrO4–
hypobromite bromite bromate perbromate
15.
perchlorate, ClO4–
16.
hypobromite IO3– periodate OI– or IO–
17.
18.
19.
20.
a.
NO3–
b.
NO2–
c.
NH4+
d.
CN–
a.
Cl–
b.
ClO–
c.
ClO3–
d.
ClO4–
a.
MgCl2
b.
Ca(ClO)2
c.
KClO3
d.
Ba(ClO4)2
a.
permanganate
b.
peroxide
c.
chromate
d.
dichromate
e.
nitrate
f.
sulfite
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21.
Chapter 4
a.
iron(III) nitrate, ferric nitrate
b.
cobalt(II) phosphate, cobaltous phosphate
c.
chromium(III) cyanide, chromic cyanide
d.
aluminum sulfate
e.
chromium(II) acetate, chromous acetate
f.
ammonium sulfite
22.
An acid is a substance that produces hydrogen ions, H+, when dissolved in water.
23.
oxygen (commonly referred to as oxyacids)
24.
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
a.
Li2O
b.
AlI3
c.
Ag2O
d.
K3 N
e.
Ca3P2
f.
MgF2
g.
Na2S
h.
BaH2
a.
CO2
b.
SO2
c.
N2Cl4
d.
CI4
e.
PF5
f.
P2O5
a.
Ca3(PO4)2
b.
NH4NO3
c.
Al(HSO4)3
25.
26.
27.
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Nomenclature
28.
29.
d.
BaSO4
e.
Fe(NO3)3
f.
CuOH
a.
HCN
b.
HNO3
c.
H2SO4
d.
H3PO4
e.
HClO or HOCl
f.
HBr
g.
HBrO2
h.
HF
a.
LiCl
b.
Cu2CO3
c.
HBr
d.
Ca(NO3)2
e.
NaClO4
f.
Al(OH)3
g.
Ba(HCO3)2
h.
FeSO4
i.
B2Cl6
j.
PBr5
k.
K2SO3
l.
Ba(C2H3O2)2
30.
A moist paste of NaCl would contain Na+ and Cl– ions in solution, and would serve as a conductor of electrical impulses.
31.
A binary compound is a compound containing two and only two elements. A polyatomic anion is several atoms bonded together which, as a whole, carries a negative electrical charge. An oxyanion is a negative ion containing a particular element and one or more oxygen atoms.
32.
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
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33.
34.
35.
Chapter 4
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.
K2 O
b.
MgO
c.
FeO
d.
Fe2O3
e.
ZnO
f.
PbO
g.
Al2O3
M+ compounds: MD, M2E, M3F M2+ compounds: MD2, ME, M3F2 M3+ compounds: MD3, M2E3, MF
36.
Fe2+:
FeCO3 Fe(BrO3)2 Fe(C2H3O2)2 Fe(OH)2 Fe(HCO3)2 Fe3(PO4)2 FeSO3 Fe(ClO4)2 FeSO4 FeO FeCl2
iron(II) carbonate; ferrous carbonate iron(II) bromate; ferrous bromate iron(II) acetate; ferrous acetate iron(II) hydroxide; ferrous hydroxide iron(II) bicarbonate; ferrous bicarbonate iron(II) phosphate; ferrous phosphate iron(II) sulfite; ferrous sulfite iron(II) perchlorate; ferrous perchlorate iron(II) sulfate; ferrous sulfate iron(II) oxide; ferrous oxide iron(II) chloride; ferrous chloride
Al3+:
Al2(CO3)3 Al(BrO3)3 Al(C2H3O2)3 Al(OH)3 Al(HCO3)3 AlPO4 Al2(SO3)3 Al(ClO4)3 Al2(SO4)3 Al2O3 AlCl3
aluminum carbonate aluminum bromate aluminum acetate aluminum hydroxide aluminum bicarbonate aluminum phosphate aluminum sulfite aluminum perchlorate aluminum sulfate aluminum oxide aluminum chloride
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Nomenclature
Na+:
Na2CO3 NaBrO3 NaC2H3O2 NaOH NaHCO3 Na3PO4 Na2SO3 NaClO4 Na2SO4 Na2O NaCl
sodium carbonate sodium bromate sodium acetate sodium hydroxide sodium bicarbonate sodium phosphate sodium sulfite sodium perchlorate sodium sulfate sodium oxide sodium chloride
Ca2+:
CaCO3 Ca(BrO3)2 Ca(C2H3O2)2 Ca(OH)2 Ca(HCO3)2 Ca3(PO4)2 CaSO3 Ca(ClO4)2 CaSO4 CaO CaCl2
calcium carbonate calcium bromate calcium acetate calcium hydroxide calcium bicarbonate calcium phosphate calcium sulfite calcium perchlorate calcium sulfate calcium oxide calcium chloride
NH4+: (NH4)2CO3 NH4BrO3 NH4C2H3O2 NH4OH NH4HCO3 (NH4)3PO4 (NH4)2SO3 NH4ClO4 (NH4)2SO4 (NH4)2O NH4Cl
ammonium carbonate ammonium bromate ammonium acetate ammonium hydroxide ammonium bicarbonate ammonium phosphate ammonium sulfite ammonium perchlorate ammonium sulfate ammonium oxide ammonium chloride
Fe3+:
iron(III) carbonate iron(III) bromate iron(III) acetate iron(III) hydroxide iron(III) bicarbonate iron(III) phosphate iron(III) sulfite iron(III) perchlorate
Fe2(CO3)3 Fe(BrO3)3 Fe(C2H3O2)3 Fe(OH)3 Fe(HCO3)3 FePO4 Fe2(SO3)3 Fe(ClO4)3
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Chapter 4
Ni2+:
37.
Fe2(SO4)3 Fe2O3 FeCl3
iron(III) sulfate iron(III) oxide iron(III) chloride
NiCO3 Ni(BrO3)2 Ni(C2H3O2)2 Ni(OH)2 Ni(HCO3)2 Ni3(PO4)2 NiSO3 Ni(ClO4)2 NiSO4 NiO NiCl2
nickel(II) carbonate nickel(II) bromate nickel(II) acetate nickel(II) hydroxide nickel(II) bicarbonate nickel(II) phosphate nickel(II) sulfite nickel(II) perchlorate nickel(II) sulfate nickel(II) oxide nickel(II) chloride
Hg22+: Hg2CO3 Hg2(BrO3)2 Hg2(C2H3O2)2 Hg2(OH)2 Hg2(HCO3)2 (Hg2)3(PO4)2 Hg2SO3 Hg2(ClO4)2 Hg2SO4 Hg2O Hg2Cl2
mercury(I) carbonate mercury(I) bromate mercury(I) acetate mercury(I) hydroxide mercury(I) bicarbonate mercury(I) phosphate mercury(I) sulfite mercury(I) perchlorate mercury(I) sulfate mercury(I) oxide mercury(I) chloride
Hg2+:
mercury(II) carbonate mercury(II) bromate mercury(II) acetate mercury(II) hydroxide mercury(II) bicarbonate mercury(II) phosphate mercury(II) sulfite mercury(II) perchlorate mercury(II) sulfate mercury(II) oxide mercury(II) chloride
HgCO3 Hg(BrO3)2 Hg(C2H3O2)2 Hg(OH)2 Hg(HCO3)2 Hg3(PO4)2 HgSO3 Hg(ClO4)2 HgSO4 HgO HgCl2
Ca(NO3)2 Sr(NO3)2 NH4NO3 Al(NO3)3
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CaSO4 SrSO4 (NH4)2SO4 Al2(SO4)3
Ca(HSO4)2 Sr(HSO4)2 NH4HSO4 Al(HSO4)3
Ca(H2PO4)2 Sr(H2PO4)2 NH4H2PO4 Al(H2PO4)3
CaO SrO (NH4)2O Al2O3
CaCl2 SrCl2 NH4Cl AlCl3
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23
Nomenclature
Fe(NO3)3 Ni(NO3)2 AgNO3 Au(NO3)3 KNO3 Hg(NO3)2 Ba(NO3)2 38.
39.
40.
Fe(HSO4)3 Ni(HSO4)2 AgHSO4 Au(HSO4)3 KHSO4 Hg(HSO4)2 Ba(HSO4)2
Fe(H2PO4)3 Ni(H2PO4)2 AgH2PO4 Au(H2PO4)3 KH2PO4 Hg(H2PO4)2 Ba(H2PO4)2
Se2
36e–
I
54e
S2
18e–
F
10e
P3
18e
Cl
18e
O2
10e
Br
36e
N3–
10e
At
86e
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–)
a.
none likely (element 36, Kr, is a noble gas)
b.
Ga3+
(element 31, Ga, is in Group 3)
c.
2–
(element 52, Te, is in Group 6)
3+
(element 81, Tl, is in Group 3)
–
(element 35, Br, is in Group 7)
+
(element 87, Fr, is in Group 1)
d. e.
41.
Fe2(SO4)3 NiSO4 Ag2SO4 Au2(SO4)3 K2SO4 HgSO4 BaSO4
Te Tl
Br
Fe2O3 NiO Ag2O Au2O3 K2 O HgO BaO
FeCl3 NiCl2 AgCl AuCl3 KCl HgCl2 BaCl2
f.
Fr
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.
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42.
43.
44.
45.
46.
Chapter 4
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.
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.
incorrect. Si is the element silicon, not silver.
b.
incorrect. Co is the symbol for cobalt, not copper.
c.
incorrect. Hydrogen exists as the hydride ion in this compound.
d.
correct
e.
incorrect. P is just “phosphorus” not “phosphoric.”
a.
Since the bromide ion must have a 1– charge, the iron ion must be in the 2+ state: the name is iron(II) bromide.
b.
Since sulfide ion always has a 2– charge, the cobalt ion must be in the 2+ state: the name is cobalt(II) sulfide.
c.
Since sulfide ion always has a 2– charge, and since there are three sulfide ions present, each cobalt ion must be in the 3+ state: the name is cobalt(III) sulfide.
d.
Since oxide ion always has a 2– charge, the tin ion must be in the 4+ state: the name is tin(IV) oxide.
e.
Since chloride ion always has a 1– charge, each mercury ion must be in the 1+ state: the name is mercury(I) chloride.
f.
Since chloride ion always has a 1– charge, the mercury ion must be in the 2+ state: the name is mercury(II) chloride.
a.
xenon hexafluoride
b.
oxygen difluoride
c.
arsenic triiodide
d.
dinitrogen tetraoxide (tetroxide)
e.
dichlorine monoxide
f.
sulfur hexafluoride
a.
iron(III) acetate, ferric acetate
b.
bromine monofluoride
c.
potassium peroxide
d.
silicon tetrabromide
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Nomenclature
e. f.
copper(II) permanganate, cupric permanganate calcium chromate
47.
a. b. c. d. e. f.
lithium dihydrogen phosphate copper(II) cyanide lead(II) nitrate sodium hydrogen phosphate sodium chlorite cobalt(III) sulfate
48.
a. b. c. d. e. f. g. h.
CaCl2 Ag2O Al2S3 BeBr2 H2 S KH MgI2 CsF
49.
a.
SO2
b.
N2 O
c.
XeF4
d.
P4O10
e.
PCl5
f.
SF6
g.
NO2
50.
a. b. c. d. e. f.
NaH2PO4 LiClO4 Cu(HCO3)2 KC2H3O2 BaO2 Cs2SO3
51.
a. b. c. d. e. f. g. h.
AgClO4 Co(OH)3 NaClO or NaOCl K2Cr2O7 NH4NO2 Fe(OH)3 NH4HCO3 KBrO4
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