PEROXIDES
There are oxides which have oxygen’s united by a simple bond (–O–O–), as the oxygenated
water or hydrogen peroxide H2O2 (H–O–O–H). The ion dioxide (2–) or ion peroxide, O22–,
forms peroxides with elements of the groups 1, 2, 11 and 12.
Peroxide
Na2O2
Stock nomenclature
Sodium peroxide
Systematic nomenclature
Disodium dioxide
K2O2
Potassium peroxide
Dipotassium dioxide
MgO2
Magnesium peroxide
Magnesium dioxide
Cu2O2
Copper (I) peroxide
Dicopper (I) dioxide
ZnO2
Zinc peroxide
Zinc dioxide
BINARY COMPOUNDS
To name a binary (metal non-metal or non meta) compound name each element in the
order they appear in the formula using the appropriate prefix to indicate the
number of atoms of the element in the compound. The second element uses an -ide
ending. If the metal exhibits more than one oxidation state, the oxidation state of
the metal, in the compound of interest, is indicated by a Roman numeral placed in
parentheses following the name of the metal.
Examples:
NaCl is named sodium chloride
CoCl2 is named cobalt (II) chloride cobalt can have oxidation states of +2 and +3
CoCl3 is named cobalt (III) chloride
1) Magnesium sulphide
12) LiBr
2) potassium bromide
13) Sr3P2
3) barium nitride
14) BaCl2
4) aluminium oxide
15) NaBr
5) sodium iodide
16) MgF2
6) strontium fluoride
17) Na2O
7) lithium sulphide
18) SrS
8) radium chloride
19) PCl3
9) calcium oxide
20) AlN
10) aluminium phosphide
21) PCl5
11) K2S
22)FeCl3
1
BASES
Bases are compounds which consist of a metal ion combined with the hydroxide
polyatomic ion (OH)-. To name a base, name the metal (include the oxidation number
in parentheses if the metal is one which has more than one oxidation state) followed by
the word hydroxide.
Examples:
NaOH is named sodium hydroxide
Ba(OH)2 is named barium hydroxide
Fe(OH)2 is named iron(II) hydroxide
Fe(OH)3 is named iron(III) hydroxide
There is no molecular form of ammonium hydroxide, NH4OH. An aqueous solution of
ammonia, NH3, contains ammonium ions, NH4+, and hydroxide ions, OH-.
A. Binary or Non-oxygen Acids
Binary acids consist of hydrogen combined with a non-metal element.
Formula of Gas Name of Gas
Formula of Acid Name of Acid
HF(g)
hydrogen fluoride
HF (aq)
hydrofluoric acid
HCl(g)
hydrogen chloride
HCl (aq)
hydrochloric acid
HBr(g)
hydrogen bromide
HBr(aq)
hydrobromic acid
HI(g)
hydrogen iodide
HI(aq)
hydroiodic acid
H2S(g)
hydrogen sulphide
H2S(aq)
hydrosulphuric acid
B. Oxygen-containing Acids
Oxygen-containing acids consist of three elements: hydrogen, a non-metal, and oxygen.
If there are only two common forms of the acid, suffixes -ous and -ic are used to denote
different oxidation states of the non-metal. Oxygen-containing acids are named by
using the stem name of the non-metal element (the middle element) with an -ous
ending if the element is in its lower oxidation state or an -ic ending if the element is
in its higher oxidation state, followed by the word acid.
Examples:
HClO hypochlorous acid
(oxidation no. of Cl = _________)
HClO2 chlorous acid
(oxidation no. of Cl = _________)
HClO3 chloric acid
(oxidation no. of Cl = _________)
HClO4 perchloric acid
(oxidation no. of Cl = _________)
Salts of Oxygen Acids
A salt of an oxygen containing acid results from the reaction of the acid with a metal
hydroxide or an aqueous ammonia solution. To name these compounds, name the
metal (be sure to include the oxidation number in parentheses when needed) followed
by the name of the acid polyatomic ion. If the polyatomic ion arises from an acid that
has an -ous ending, then the polyatomic ion name will end with -ite. If the polyatomic
ion arises from an acid that has an -ic ending, then the name of the polyatomic ion ends
in -ate. Prefixes such as hypo- and per- remain as part of the polyatomic ion name.
Examples:
KClO potassium hypochlorite
(The ClO- polyatomic ion arises from hypochlorous acid.)
KClO2 potassium chlorite
(The ClO2- polyatomic ion arises from chlorous acid.)
KClO3 potassium chlorate
(The ClO3- polyatomic ion arises from chloric acid.)
2
KClO4 potassium perchlorate
(The ClO4- polyatomic ion arises from perchloric acid.)
FeSO3 iron (II) sulphite
(The iron has an oxidation number of +2. The SO3-2 polyatomic ion comes from H2 SO3,
sulphurous acid.)
Fe2 (SO4)3 iron (III) sulphate
(The iron has an oxidation number of +3. The SO4-2 polyatomic ion comes from H2 SO4,
sulphuric acid.)
Sodium sulphate
K2CO3
Copper (I) oxide
CaSO3
Magnesium chloride
CaSO4
Potassium carbonate
Ca3(PO4)2
Aluminum oxide
NaNO3
Silver sulphide
BaSO4
Ammonium nitrate
NH4Br
Iron (III) sulphide
ZnCl2
Ammonium phosphate
AgNO3
Hydrogen cyanide
MgS
Lead (II) sulphate
CaCO3
Sodium bicarbonate
BaSO4
Ammonia
Na2O2
Hydrazine
C(Cl)4
Arsine
CH4
Phophine
Al(OH)3
Silver hypochlorite
CaO2
Copper(II) nitrate
Na2SO4
Copper(II) hydroxide
CrO3
Sodium peroxide
H3PO4
Tin (IV) sulphide
Ca2C
3