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CHAPTER 6
NOMENCLATURE OF INORGANIC COMPOUNDS
SOLUTIONS TO REVIEW QUESTIONS
1. water (H2O)–dihydrogen monoxide
ammonia (NH3)–nitrogen trihydride
2. An atom must gain one or more electrons to form an anion. An atom must lose one or more electrons to
form a cation.
3. No, if elements combine in a one-to-one ratio the charges on their ions must be equal and opposite in sign.
They could be þ1, 1, or þ2, 2 or þ3, 3 etc.
4. The metal or cation is always named first.
5. (a)
(b)
(c)
K2S
Co(BrO3)2
NH4NO3
(d) H3PO4
(e) Fe2O3
(f) Mg(OH)2
6. The system for naming binary compounds composed of two nonmetals uses the name of the first element
and the stem of the second element plus the suffix –ide. A prefix is attached to each element indicating the
number of atoms of that element in the formula. Thus, N2O5 is dinitrogen pentoxide. Aluminum forms
only one series of compounds in which the cation is always Al3þ. Thus the name for Al2O3, aluminum
oxide, does not need to be distinguished from any other compound.
7. Barium forms only one series of compounds in which the cation is always Ba2þ. Thus the name for BaCl2
(barium chloride) does not need to be distinguished from any other compound. Iron forms two series of
compounds in which the iron ion is Fe2þ or Fe3þ. Thus the name iron chloride does not indicate which
compound is in question. Therefore, FeCl2 is called iron(II) chloride to indicate that the compound
contains the Fe2þ ion. Neither uses prefixes because prefixes are used to name compounds composed of
two nonmetals.
8. The mono prefix is generally not used for the first element.
9. The Stock System clearly indicates cation charges. The classical system works, but requires a chemist to
memorize the common charges on all cations. It is much easier to use the Stock System and much more
error free.
10. Nickel(II) compounds
(a)
(b)
(c)
NiSO4
Ni3P2
NiCrO4
(d) Ni(OH)2
(e) Ni(IO2)2
(f) Ni(C2H3O2)2
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(g)
(h)
(i)
NiCr2O7
NiBr2
Ni(NO3)2
(j)
Ni(ClO)2
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- Chapter 6 11. (a)
HBrO
HBrO2
HBrO3
HBrO4
hypobromous acid
bromous acid
bromic acid
perbromic acid
(b) HIO
HIO2
HIO3
HIO4
hypoiodous acid
iodous acid
iodic acid
periodic acid
12. Include hydrogen or dihydrogen in the name to tell how many hydrogens are left behind.
For example
Phosphate ion PO43
Hydrogen phosphate ion HPO42
Dihydrogen phosphate ion H2PO4
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- Chapter 6 -
SOLUTIONS TO EXERCISES
1. Formulas of compounds:
(a) Ba and S
BaS
(b) Cs and P
Cs3P
(c) Li and Br
LiBr
(d) Mg and N
(e) Ca and I
(f) H and Cl
Mg3N2
CaI2
HCl
2. Formulas of compounds:
(a) Al and S
Al2S3
(b) H and F
HF
(c) K and N
K3 N
(d) Sr and O
(e) Cs and P
(f) Al and Cl
SrO
Cs3P
AlCl3
Ca2þ
Pb2þ
Zn2þ
Agþ
Hþ
Sn2þ
Fe3þ
3. (a) potassium
(b) ammonium
(c) copper(I)
(d) titanium(IV)
(e) nickel(III)
(f) cesium
(g) mercury(II)
Kþ
NHþ
4
Cuþ
Ti4þ
Ni3þ
Csþ
Hg2þ
(h)
(i)
(j)
(k)
(l)
(m)
(n)
calcium
lead(II)
zinc
silver
hydrogen
tin(II)
iron(III)
4. (a) fluoride
(b) acetate
(c) iodide
(d) carbonate
(e) sulfide
(f) nitrate
(g) phosphide
F
C2 H3 O
2
I
CO2
3
S2
NO
3
p3
(h)
(i)
(j)
(k)
(l)
(m)
(n)
oxide
O2
dichromate
Cr2 O2
7
hydrogen carbonate HCO
3
phosphate
PO3
4
sulfate
SO2
4
nitride
N3
chloride
Cl
5. (a)
(b)
(c)
sodium hydrogen carbonate
mercury
calcium oxide
(d) acetic acid
(e) magnesium sulfate heptahydrate
(f) sodium hydroxide
6. (a)
(b)
(c)
sodium thiosulfate
dinitrogen monoxide
aluminum oxide
(d) sodium chloride
(e) magnesium hydroxide
(f) lead(II) sulfide
7.
Br
Ion
Kþ
2þ
Mg
NO
3
PO3
4
CO2
3
KBr
K2O
KNO3
K3PO4
K2CO3
MgBr2
MgO
Mg(NO3)2
Mg3(PO4)2
MgCO3
3þ
AlBr3
Al2O3
Al(NO3)3
AlPO4
Al2(CO3)3
2þ
ZnBr2
ZnO
Zn(NO3)2
Zn3(PO4)2
ZnCO3
HBr
H2O
HNO3
H3PO4
H2CO3
Al
Zn
H
O2
þ
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- Chapter 6 8.
Ion
NHþ
4
SO2
4
OH
AsO3
4
C2 H3 O
2
CrO2
4
(NH4)2SO4
NH4OH
(NH4)3AsO4
NH4C2H3O2
(NH4)2CrO4
2þ
CaSO4
Ca(OH)2
Ca3(AsO4)2
Ca(C2H3O2)2
CaCrO4
3þ
Fe2(SO4)3
Fe(OH)3
FeAsO4
Fe(C2H3O2)3
Fe2(CrO4)3
Ag2SO4
AgOH
Ag3AsO4
AgC2H3O2
Ag2CrO4
CuSO4
Cu(OH)2
Cu3(AsO4)2
Cu(C2H3O2)2
CuCrO4
Ca
Fe
Ag
Cu
þ
2þ
9. Kþ compounds: potassium bromide, potassium oxide, potassium nitrate, potassium phosphate,
potassium carbonate.
Mg2þ compounds: magnesium bromide, magnesium oxide, magnesium nitrate, magnesium phosphate,
magnesium carbonate.
Al3þ compounds: aluminum bromide, aluminum oxide, aluminum nitrate, aluminum phosphate,
aluminum carbonate.
Zn2þ compounds: zinc bromide, zinc oxide, zinc nitrate, zinc phosphate, zinc carbonate.
Hþ compounds: hydrogen bromide (or hydrobromic acid), water, nitric acid, phosphoric acid, carbonic
acid.
10. NHþ
4 compounds: ammonium sulfate, ammonium hydroxide, ammonium arsenate, ammonium acetate,
ammonium chromate.
Ca2þ compounds: calcium sulfate, calcium hydroxide, calcium arsenate, calcium acetate, calcium
chromate.
Fe3þ compounds: iron(III) sulfate, iron(III) hydroxide, iron(III) arsenate, iron(III) acetate, iron(III)
chromate.
Agþ compounds: silver sulfate, silver hydroxide, silver arsenate, silver acetate, silver chromate.
Cu2þ compounds: copper(II) sulfate, copper(II) hydroxide, copper(II) arsenate, copper(II) acetate,
copper(II) chromate.
11. Nonmetal binary compound formulas:
(a) diphosphorus pentoxide, P2O5
(b) carbon dioxide, CO2
(c) tribromine octoxide, Br3O8
(d) sulfur hexachloride, SCl6
(e) carbon tetrachloride, CCl4
(f) dichlorine heptoxide, Cl2O7
(g) boron trifluoride, BF3
(h) tetranitrogen hexasulfide, N4S6
12. Metal-nonmetal binary compound formulas:
(a) potassium nitride, K3N
(b) barium oxide, BaO
(c) iron(II) oxide, FeO
(d) strontium phosphide, Sr3P2
(e) calcium nitride, Ca3N2
(f) cesium bromide, CsBr
(g) manganese(III) iodide, MnI3
(h) sodium selenide, Na2Se
13. Naming binary metal-nonmetal compounds:
(a) BaO, barium oxide
(b) K2S, potassium sulfide
(c) CaCl2, calcium chloride
(d) Cs2S, cesium sulfide
(e) Al2O3, aluminum oxide
(f) CaBr2, calcium bromide
(g) SrI2, strontium iodide
(h) Mg3N2, magnesium nitride
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- Chapter 6 14. Naming binary nonmetal compounds:
(a) PBr5, phosphorus pentabromide
(b) I4O9, tetraiodine nonoxide
(c) N2S5, dinitrogen pentasulfide
(d) S2F10, disulfur decafluoride
15. (a)
(b)
(c)
CuCl2
FeCl2
Fe(NO3)2
(e) SiCl4, silicon tetrachloride
(f) ClO2, chlorine dioxide
(g) P4S7, tetraphosphorus heptasulfide
(h) IF6, iodine hexafluoride
copper(II) chloride
iron(II) chloride
iron(II) nitrate
16. Formulas:
(a) tin(IV) bromide
(b) copper(I) sulfate
(c) nickel(II) borate
(d) FeCl3
(e) SnF2
(f) VPO4
iron(III) chloride
tin(II) fluoride
vanadium(III) phosphate
(d) mercury(II) nitrite
(e) cobalt(III) carbonate
(f) iron(II) acetate
SnBr4
Cu2SO4
Ni3(BO3)2
17. Formulas of acids:
(a) hydrochloric acid, HCl
(b) chloric acid, HClO3
(c) nitric acid, HNO3
(d) carbonic acid, H2CO3
(e) sulfurous acid, H2SO3
(f) phosphoric acid, H3PO4
18. Formulas of acids:
(a) acetic acid, HC2H3O2
(b) hydrofluoric acid, HF
(c) hydrosulfuric acid, H2S
(d) boric acid, H3BO3
(e) nitrous acid, HNO2
(f) hypochlorous acid, HClO
19. Naming acids:
(a) HNO2, nitrous acid
(b) H2SO4, sulfuric acid
(c) H2C2O4, oxalic acid
(d) HBr, hydrobromic acid
(e) H3PO3, phosphorous acid
(f)
(g)
(h)
(i)
HC2H3O2, acetic acid
HF, hydrofluoric acid
HBrO3, bromic acid
HIO4, periodic acid
20. Naming acids:
(a) H3PO4, phosphoric acid
(b) H2CO3 carbonic acid
(c) HIO3, iodic acid
(d) HCl, hydrochloric acid
(e) HClO, hypochlorous acid
(f)
(g)
(h)
(i)
HNO3, nitric acid
HI, hydroiodic acid
HClO4 perchloric acid
H2SO3, sulfurous acid
21. Formulas for:
(a) silver sulfite
(b) cobalt(II) bromide
(c) tin(II) hydroxide
(d) aluminum sulfate
(e) lead(II) chloride
(f) ammonium carbonate
(g) chromium(III) oxide
(h) cupric chloride
(i) potassium permanganate
Ag2SO3
CoBr2
Sn(OH)2
Al2(SO4)3
PbCl2
(NH4)2CO3
Cr2O3
CuCl2
KMnO4
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Hg(NO2)2
Co2(CO3)3
Fe(C2H3O2)2
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- Chapter 6 (j)
(k)
(l)
(m)
(n)
arsenic(V) sulfite
sodium peroxide
iron(II) sulfate
potassium dichromate
bismuth(III) chromate
As2(SO3)5
Na2O2
FeSO4
K2Cr2O7
Bi2(CrO4)3
22. Formulas for:
(a) sodium chromate
(b) magnesium hydride
(c) nickel(II) acetate
(d) calcium chlorate
(e) magnesium bromate
(f) potassium dihydrogen phosphate
(g) manganese(II) hydroxide
(h) cobalt(II) hydrogen carbonate
(i) sodium hypochlorite
(j) barium perchlorate
(k) chromium(III) sulfite
(l) antimony(III) sulfate
(m) sodium oxalate
(n) potassium thiocyanate
Na2CrO4
MgH2
Ni(C2H3O2)2
Ca(ClO3)2
Mg(BrO3)2
KH2PO4
Mn(OH)2
Co(HCO3)2
NaClO
Ba(ClO4)2
Cr2(SO3)3
Sb2(SO4)3
Na2C2O4
KSCN
23. Names for:
(a) ZnSO4
(b) Hg2S
(c) CuCO3
(d) Cd(NO3)2
(e) Al(C2H3O2)3
(f) CoF2
(g) Cr(ClO3)3
(h) Ag3PO4
(i) MnS
(j) BaCrO4
zinc sulfate
mercury(I) sulfide
copper(II) carbonate
cadmium nitrate
aluminum acetate
cobalt(II) fluoride
chromium(III) chlorate
silver phosphate
manganese(II) sulfide
barium chromate
24. Names for:
(a) Ca(HSO4)2
(b) As2(SO3)3
(c) Sn(NO2)2
(d) CuI
(e) KHCO3
(f) BiAsO4
(g) (NH4)2CO3
(h) (NH4)2HPO4
(i) NaClO
(j) KMnO4
calcium hydrogen sulfate
arsenic(III) sulfite
tin(II) nitrite
copper(I) iodide
potassium hydrogen carbonate
bismuth(III) arsenate
ammonium carbonate
ammonium monohydrogen phosphate
sodium hypochlorite
potassium permanganate
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- Chapter 6 25. Formulas for:
(a) slaked lime, Ca(OH)2
(b) fool’s gold, FeS2
(c) washing soda, Na2 CO3 10 H2 O
(d) calcite, CaCO3
(e) cane sugar, C12H22O11
(f) borax, Na2 B4 O7 10 H2 O
(g) wood alcohol, CH3OH
(h) acetylene, C2H2
26. Formulas for:
(a) grain alcohol, C2H5OH
(b) cream of tartar, KHC4H4O6
(c) gypsum, CaSO4 2 H2 O
(d) brimstone, S
(e)
(f)
(g)
(h)
muriatic acid, HCl
plaster of paris, CaSO4 1=2 H2 O
lye, NaOH
laughing gas, N2O
27. (a)
(b)
(c)
K ! Kþ þ e
I þ e ! I
Br þ e ! Br
(d) Fe ! Fe2þ þ 2e
(e) Ca ! Ca2þ þ 2e
(f) O þ 2e ! O2
28. (a)
(b)
(c)
sulfate
phosphate
nitrate
(d) chlorate
(e) hydroxide
(f) carbonate
29. (a)
(b)
(c)
CaSO4
Ca3(PO4)2
Ca(NO3)2
(d) Ca(ClO3)2
(e) Ca(OH)2
(f) CaCO3
30. (a)
(b)
(c)
K2SO4
K3PO4
KNO3
(d) KClO3
(e) KOH
(f) K2CO3
31. (a)
(b)
CBr4 carbon tetrabromide
BF3 boron trifluoride
(c)
PCl5 phosphorus pentachloride
32. Formula: KCl Name: potassium chloride
33. ide:
suffix is used to indicate a binary compound except for hydroxides, cyanides, and ammonium
compounds.
ous:
used as a suffix to name an acid that has a lower oxygen content than the -ic acid (e.g., HNO2,
nitrous acid, and HNO3, nitric acid). Also used as a suffix to name the lower ionic charge of a
metal with more than one possible charge (e.g., Fe2þ, ferrous, and Fe3þ, ferric).
ic:
used as a suffix to name an acid that has a higher oxygen content than the -ous acid (e.g., HNO3
nitric acid, and HNO2 nitrous acid). Also used as a suffix to name the higher ionic charge of a
metal with more than one possible charge (e.g., Fe2þ, ferrous, and Fe3þ, ferric).
hypo: used as a prefix in naming an acid that has a lower oxygen content than the -ous acid when there
are more than two oxyacids with the same elements (e.g., HClO, hypochlorous acid, and HClO2,
chlorous acid).
per:
used as a prefix in naming an acid that has a higher oxygen content than the -ic acid when there
are more than two oxyacids with the same elements (e.g., HClO4, perchloric acid, and HClO3,
chloric acid).
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- Chapter 6 ite:
the suffix used in naming a salt derived from an -ous acid.
For example, HNO2 (nitrous acid); NaNO2 (sodium nitrite).
ate:
the suffix used in naming a salt derived from an -ic acid.
For example, H2SO4 (sulfuric acid); CaSO4 (calcium sulfate).
Roman numerals: In the Stock System Roman numerals are used in naming compounds that contain metals
that may exist as more than one type of cation. The charge of a metal is indicated by a Roman numeral
written in parenthesis immediately after the name of the metal. For example, FeCl2 [iron (II) chloride].
34. (a)
(b)
(c)
35. (a)
Calcium carbonate or CaCO3 is the principal ingredient in lime, chalk, and marble. It is harmless,
though it does leave a residue on plumbing. There should be no concern regarding this spill.
Acetic acid or HC2H3O2 is found in vinegar. This is not a particularly hazardous spill, though it
will be widely apparent due to the characteristic odor of vinegar. (Perhaps it could be cleaned up
with lots of lettuce?)
Dihydrogen oxide or H2O is commonly known as water and it may be safely dumped into the
sewer.
50 e, 50 p
(b)
48e, 50 p
(c)
46 e, 50 p
36. The formula for a compound must be electrically neutral. Therefore X ¼ þ3 and Y ¼ 2 since in X2Y3
this would give 2(þ3) þ 3(2) ¼ 0.
37. Li3Fe(CN)6
AlFe(CN)6
Zn3[Fe(CN)6]2
38. (a)
(b)
(c)
39. (a)
(b)
(c)
(d)
(e)
(f)
N3 nitride
NO2 nitrite
NO2 nitrite
NO3 nitrate
HNO2 nitrous acid
HNO3 nitric acid
Potassium chloride
Calcium carbonate
Ferrous sulfate
Zinc oxide
Manganese sulfate
Copper sulfate
(g) Manganous oxide
(h) Potassium iodide
(i) Cobalt carbonate
(j)
Sodium chloride
One has oxygen the other does not, charges on the ions differ.
The number of oxygens differ, but the charge is the same.
The number of oxygens in the compounds differ but they both have only
one hydrogen and one nitrogen atom.
KCl
CaCO3
FeSO4
ZnO
MnSO4 and Mn2(SO4)3 would both be described by this name. Better
names would be Manganese(II) sulfate for MnSO4 and Manganese(III)
sulfate for Mn2(SO4)3
CuSO4 and Cu2SO4 would both be described by this name. Better names
would be Copper(II) sulfate and cupric sulfate for CuSO4 or Copper(I)
sulfate or cuprous sulfate for Cu2SO4
MnO
KI
CoCO3 and Co2(CO3)3 would both be described by this name. Better
names would be Cobalt(II) carbonate for CoCO3 and Cobalt(III) carbonate for Co2(CO3)3
NaCl
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