CHAPTER 6
NOMENCLATURE OF INORGANIC COMPOUNDS
SOLUTIONS TO REVIEW QUESTIONS
1. (a)
(b)
(c)
2.
K2 S
Co(BrO3)2
NH4NO3
(d) H3PO4
(e) Fe2O3
(f) Mg(OH)2
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.
3. (a)
HBrO
HBrO2
HBrO3
HBrO4
(b)
hypobromous acid
bromous acid
bromic acid
perbromic acid
HIO
HIO2
HIO3
HIO4
hypoiodous acid
iodous acid
iodic acid
periodic acid
4.
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.
5.
Nickel(II) compounds
(a) NiSO4
(b) Ni3P2
(c) NiCrO4
6.
(g) NiCr2O7
(h) NiBr2
(i) Ni(NO3)2
(j)
Ni(ClO)2
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.
7. (a)
(b)
(c)
8.
(d) Ni(OH)2
(e) Ni(IO2)2
(f) Ni(C2H3O2)2
Metals are located in groups 1A (except for hydrogen), 2A, 1B–8B and atomic numbers 13, 31, 49,
50, 81, 82, 83, lanthanides and actinides.
The nonmetals include hydrogen, group 7A, the noble gases and atomic numbers 6–9, 15–17, 34,
35, 53 and 85.
The transition metals are located in groups 1B–8B in the center of the periodic table. The lanthanides and actinides are located below the main body of the periodic table.
water (H2O)–dihydrogen monoxide
ammonia (NH3)–nitrogen trihydride
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- Chapter 6 -
SOLUTIONS TO EXERCISES
1. Formulas of compounds:
(a) Ba and S
BaS
(b) Rb and O
Rb2O
(c) Li and Br
LiBr
(d) Mg and N
(e) Al and P
(f) H and Cl
Mg3N2
AlP
HCl
2. Formulas of compounds:
(a) Al and S
Al2S3
(b) H and F
HF
(c) Na and I
NaI
(d) Sr and O
(e) Cs and P
(f) K and Cl
SrO
Cs3P
KCl
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
C 2 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
Mg
2þ
PO3
4
CO2
3
KBr
K2 O
KNO3
K3PO4
K2CO3
MgBr2
MgO
Mg(NO3)2
Mg3(PO4)2
MgCO3
AlBr3
Al2O3
Al(NO3)3
AlPO4
Al2(CO3)3
2þ
ZnBr2
ZnO
Zn(NO3)2
Zn3(PO4)2
ZnCO3
HBr
H2 O
HNO3
H3PO4
H2CO3
Zn
H
NO
3
3þ
Al
8.
O2
þ
- 40 -
- Chapter 6 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
þ
Ag
2þ
Cu
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) dinitrogen pentoxide, N2O5
(b) carbon dioxide, CO2
(c) tribromine octoxide, Br3O8
(d) dinitrogen monoxide, N2O
(e) carbon tetrachloride, CCl4
(f) dichlorine heptoxide, Cl2O7
(g) phosphorus triiodide, PI3
(h) tetranitrogen hexasulfide, N4S6
12. Metal-nonmetal binary compound formulas:
(a) potassium nitride, K3N
(b) aluminum sulfide, Al2S3
(c) iron(II) oxide, FeO
(d) rubidium phosphide, Rb3P
(e) calcium nitride, Ca3N2
(f) cesium bromide, CsBr
(g) copper(II) chloride, CuCl2
(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
14. Naming binary nonmetal compounds:
(a) PBr5, phosphorus pentabromide
(b)
- 41 -
I4O9, tetraiodine nonoxide
- Chapter 6 (c)
(d)
15. (a)
(b)
(c)
N2S5, dinitrogen pentasulfide
S2F10, disulfur decafluoride
CuCl2
CuBr
Fe(NO3)2
copper(II) chloride
copper(I) bromide
iron(II) nitrate
16. Formulas:
(a) tin(IV) bromide
(b) copper(I) sulfate
(c) iron(III) carbonate
17. Add
(a)
(b)
(c)
(e) SiCl4, silicon tetrachloride
(f) ClO2, chlorine dioxide
(g) P4S7, tetraphosphorus heptasulfide
(h) IF6, iodine hexafluoride
(d) FeCl3
(e) SnF2
(f) HgCO3
SnBr4
Cu2SO4
Fe2(CO3)3
iron(III) chloride
tin(II) fluoride
mercury(II) carbonate
(d) mercury(II) nitrite
(e) titanium(IV) sulfide
(f) iron(II) acetate
formulas:
hydrochloric acid, HCl
chloric acid, HClO3
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) manganese(II) fluoride
(f) ammonium carbonate
(g) chromium(III) oxide
(h) cupric chloride
(i) potassium permanganate
(j) barium nitrite
Ag2SO3
CoBr2
Sn(OH)2
Al2(SO4)3
MnF2
(NH4)2CO3
Cr2O3
CuCl2
KMnO4
Ba(NO2)2
- 42 -
Hg(NO2)2
TiS2
Fe(C2H3O2)2
- Chapter 6 (k)
(l)
(m)
(n)
sodium peroxide
iron(II) sulfate
potassium dichromate
bismuth(III) chromate
Na2O2
FeSO4
K2Cr2O7
Bi2(CrO4)3
22. Formulas for:
(a) sodium chromate
(b) magnesium hydride
(c) nickel(II) acetate
(d) calcium chlorate
(e) lead(II) nitrate
(f) potassium dihydrogen phosphate
(g) manganese(II) hydroxide
(h) cobalt(II) hydrogen carbonate
(i) sodium hypochlorite
(j) arsenic(V) carbonate
(k) chromium(III) sulfite
(l) antimony(III) sulfate
(m) sodium oxalate
(n) potassium thiocyanate
Na2CrO4
MgH2
Ni(C2H3O2)2
Ca(ClO3)2
Pb(NO3)2
KH2PO4
Mn(OH)2
Co(HCO3)2
NaClO
As2(CO3)5
Cr2(SO3)3
Sb2(SO4)3
Na2C2O4
KSCN
23. Names for:
(a) ZnSO4
(b) HgCl2
(c) CuCO3
(d) Cd(NO3)2
(e) Al(C2H3O2)3
(f) CoF2
(g) Cr(ClO3)3
(h) Ag3PO4
(i) NiS
(j) BaCrO4
zinc sulfate
mercury(II) chloride
copper(II) carbonate
cadmium nitrate
aluminum acetate
cobalt(II) fluoride
chromium(III) chlorate
silver phosphate
nickel(II) sulfide
barium chromate
24. Names for:
(a) Ca(HSO4)2
(b) As2(SO3)3
(c) Sn(NO2)2
(d) FeBr3
(e) KHCO3
(f) BiAsO4
(g) Fe(BrO3)2
(h) (NH4)2HPO4
(i) NaClO
(j) KMnO4
calcium hydrogen sulfate
arsenic(III) sulfite
tin(II) nitrite
iron(III) bromide
potassium hydrogen carbonate
bismuth(III) arsenate
iron(II) bromate
ammonium monohydrogen phosphate
sodium hypochlorite
potassium permanganate
- 43 -
- 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)
(f)
(g)
(h)
cane sugar, C12H22O11
borax, Na2 B4 O7 10 H2 O
wood alcohol, CH3OH
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
multivalent metal (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 (eg. HNO3
nitric acid and HNO2 nitrous acid). Also used as a suffix to name the higher ionic charge of a
multivalent metal (e.g. Fe2þ, ferrous and Fe3þ, ferric).
hypo: used as a prefix in naming an acid that has a lower oxygen content that the -ous acid when there
are more than two oxyacids with the same elements (e.g. HClO, hypochlorous acid and HClO2,
chlorous acid).
- 44 -
- Chapter 6 per:
ite:
ate:
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).
the suffix used in naming a salt derived from an -ous acid.
For example, HNO2 (nitrous acid); NaNO2 (sodium nitrite).
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)
AgNO3 þ NaCl ! AgCl þ NaNO3
Fe2 ðSO4 Þ3 þ CaðOHÞ2 ! FeðOHÞ3 þ CaSO4
KOH þ H2 SO4 ! K2 SO4 þ H2 O
35. (a)
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)
N3 nitride
NO2 nitrite
NO2 nitrite
NO3 nitrate
HNO2 nitrous acid
HNO3 nitric acid
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.
39. Let x ¼ molar mass of Y
2.44x þ x ¼ 110.27
x ¼ 32.07, Y ¼ sulfur (from periodic table)
2.44x ¼ (110.27 32.07) ¼ 78.20
The compound formula is X2Y, so the mass of 2X ¼ 78.20
X ¼ 39.11 which is potassium (from the periodic table)
X2Y ¼ K2S
78:20
Ratio ¼
¼ 2:44
32:07
- 45 -