SCH 4C
ELEMENTS
COMPOUNDS
PREFIXES
#
H2
O2
N2
F2
Cl2
Br2
I2
P4
S8
Fe3O4 magnetic iron oxide
CCl4 carbon tetrachloride
CS2 carbon disulphide
CO carbon monoxide
CO2 carbon dioxide
SO2 sulphur dioxide
SO3 sulphur trioxide
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
1
2
3
4
5
6
7
8
9
10
SINGLE VALENCES
+1
+2
+3
±4
H
Li
Na
K
Ag
Be
Mg
Ca
Zn
Ba
B
Al
C
Si
-3
ROMAN
NUMERALS
I
II
III
IV
V
VI
VII
VIII
IX
X
MULTIPLE VALENCES
-2
-1
+1,2
+1,3
+2,3
+2,4
±3,5
O
S
H
F
Cl
Br
I
Cu
Hg
Au
Fe
Cr
Co
Ni
Sn
Mn
Pb
Pt
N
P
As
Sb
RADICALS (POLYATOMIC IONS)
+1
-1
-2
-3
NH4 +, ammonium
ClO3 - , chlorate
BrO3 -, bromate
IO3 -, iodate
NO3 -, nitrate
OH -, hydroxide
C2H3O2 -, acetate
SO4 2-, sulphate
CO3 2-, carbonate
CrO4 2-, chromate
PO4 3-, phosphate
LATIN NAMES
(ous – ic system)
Cu
Fe
Sn
Pb
Au
cuprous
cupric
ferrous
ferric
stannous
stannic
plumbous
plumbic
aurous
auric
SOME COMMON IONS AND THEIR CHARGES
Cations
Aluminum
Ammonium
Antimony (III)/antimonous
Arsenic (III)/arsenious
Barium
Beryllium
Bismuth (III)
Calcium
Cadmium
Cerium (III)/cerous, Cerium (IV)/ceric
Cesium
Chromium (II)/chromous, Chromium (III)/chromic
Cobalt (II)/cobaltous, Cobalt (III)/cobaltic
Copper (I)/cuprous, Copper (II)/cupric
Gallium (III)
Gold (I)/aurous, Gold (III)/auric
Hydrogen, Hydronium
Iron (II)/ferrous, Iron (III)/ferric
Lead (II)/plumbous, Lead (IV)/plumbic
Lithium
Magnesium
Manganese (II), Manganese (IV)
Mercury (I)/mercurous, Mercury (II)/mercuric
Nickel (II), Nickel (III)S
Platinum (II), Platinum (IV)
Potassium
Rubidium
Silver
Sodium
Strontium
Thallium (I)/thallous, Thallium (III)/thallic
Tin (II)/stannous, Tin (IV)/stannic
Titanium (III)/titanous, Titanium (IV)/titanic
Vanadium
Zinc
Symbol
3+
Al
NH4 +
Sb3+
As3+
Ba 2+
Be 2+
Bi 3+
Ca 2+
Cd 2+
Ce2+, Ce3+
Cs +
Cr2+, Cr3+
Co2+, Co3+
Cu+, Cu2+
Ga 3+
Au+, Au3+
H +, H 3O +
Fe2+, Fe3+
Pb2+, Pb4+
Li +
Mg 2+
2+
4+
Mn , Mn
+
2+
Hg , Hg
Ni2+, Ni3+
Pt 2+, Pt 4+
K+
Rb +
Ag +
Na +
Sr 2+
Tl +, Tl 3+
Sn2+, Sn4+
Ti 3+, Ti 4+
V 3+
Zn 2+
Anions
Acetate
Arsenate
Arsenite
Benzoate
Borate
Perbromate
Bromate
Bromite
Hypobromite
Bromide
Carbonate
Hydrogen carbonate or bicarbonate
Chlorate
Chloride
Chromate
Dichromate
Cyanate
Cyanide
Fluorate
Fluoride
Hydride
Hexacyanoferrate (II) or ferrocyanide
Hexacyanoferrate (III) or ferricyanide
Hydrogen phthalate or biphthalate
Hydrogen sulphide or bisulphide
Hydrogen sulphite or bisulphite
Hydroxide
Iodate
Iodide
Nitrate
Orthosilicate
Oxalate
Hydrogen oxalate or bioxalate
Oxide
Permanganate
Peroxide
Phosphate
Monohydrogen phosphate
Dihydrogen phosphate
Pyrophosphate
Silicate
Sulphate
Hydrogen sulphate or bisulphate
Thiocyanate
Thiosulphate
Symbol
C 2H 3O 2 AsO4 3AsO3 3C7H6O2 2BO3 3BrO4 BrO3 BrO2 BrO Br CO3 2HCO3 ClO3 Cl CrO4 2Cr2O7 2CNO CN FO3 FHFe(CN)6 2Fe(CN)6 3HC8H4O4 HS HSO3 OH IO3 INO3 SiO4 4C2O4 2HC2O4 O 2MnO4 O2 2PO4 3HPO4 2H2PO4 P2O7 4SiO3 2SO4 2HSO4 SCN S2O3 2-
SCH 4C
FORMULA WRITING
Write a chemical formula for each of the following compounds showing all the steps. For example.
III
aluminum oxide
II
Al O → Al2O3
1.
magnesium chloride
______________________________
2.
sodium phosphate
______________________________
3.
silver oxide
______________________________
4.
calcium sulphide
______________________________
5.
aluminum hydroxide
______________________________
6.
lead (IV) bromide
______________________________
7.
zinc carbonate
______________________________
8.
lithium nitrate
______________________________
9.
phosphorus (V) sulphate
______________________________
10.
hydrogen bromate
______________________________
11.
mercury (I) oxide
______________________________
12.
iron (II) phosphate
______________________________
13.
manganese dioxide
______________________________
14.
copper (II) sulphide
______________________________
15.
lead (IV) carbonate
______________________________
16.
tin (II) fluoride
______________________________
17.
arsenic (III) acetate
______________________________
18.
magnesium hydroxide
______________________________
19.
antimony (V) iodate
______________________________
20.
barium phosphate
______________________________
CHEMICAL NOMENCLATURE
BINARY COMPOUNDS
Binary compounds contain only 2 elements. Follow the steps in writing formula. The positive
element is written first (the least electronegative element).
A. Monovalent First Element
The name of the first element is written and the name of the second is altered to give an "ide"
i.e.
NaCl
sodium chloride
K2 O
potassium oxide
CaBr2
calcium bromide
Al2S3
aluminum sulphide
RULE I →
element (elem...)ide
EXERCISE 1
Write the correct chemical names for the following binary compounds:
a) CaCl2
b) BaO
c) ZnS
d) H2S
e) AlBr3
f) NaI
g) CaH2
h) AgCl
i) Al2O3
j) SiC
k) MgS
l) HF
m) KBr
n) HgCl2
B. Multivalent First Element
To avoid confusion the valence used must be indicated in the name of the compound. There are 3
ways to do this; the Stock System; the "ous - ic" system and; the Prefix System. Each of these 3
systems are explained below.
i) "ous - ic" System - the oldest system. When an element possessing 2 different valences unites
with another element of constant valence, the compound formed containing the element in its
lower valence attaches the suffix "ous" to the name of that element. The compound containing
the element in its higher valence adds the suffix "ic" to the name of that element.
i.e.
SbI5
HgCl
HgCl2
mercurous chloride
mercuric chloride
CuCl
CuCl2
cuprous chloride
cupric chloride
PBr3
PBr5
phosphorous bromide
phosphoric bromide
FeO
Fe2O3
ferrous oxide
ferric oxide
SbI3
antimonous iodide
antimonic iodide
SnS
SnS2
stannous sulphide
stannic sulphide
AsF3
AsF5
PbBr2
PbBr4
plumbous bromide
plumbic bromide
AuI
AuI3
aurous iodide
auric iodide
arsenious fluoride
arsenic fluoride
***Copper, iron, tin, lead and gold use their Latin names in this system.
RULE II →
1. Lower valence - (elem...)ous (elem...)ide
2. Higher valence - (elem...)ic (elem...)ide
**Memorize
Fe3O4 magnetic iron oxide
EXERCISE 2:
Using Rule II write the chemical name for each binary compound in the first blank following the
formula:
a) FeO
b) Sb2S5
c) SnCl4
d) As2O3
e) SnO
f) Fe2S3
g) P2O3
h) Hg2O
i) CuBr2
j) As2S5
k) Fe2O3
l) CuO
m) SbI3
n) Fe3O4
o) SnS
p) P2O5
q) FeCl3
r) CuF2
s) PbO
t) PbO2
u) AsCl3
v) MnO2
w) AsBr5
x) Sb2O3
y) P2O3
ii) Prefix System - this is generally used for compounds containing 2 non-metals (covalent
compounds). The number of atoms of the first and second element is indicated by a suitable
Greek prefix. ie. mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6), hepta (7), octa (8), nona
(9), & deca (10). If first is mono then it is omitted from the name.
CCl4
CO
SO2
PCl3
P205
carbon tetrachloride
CS2
carbon disulphide
carbon monoxide
CO2
carbon dioxide
sulphur dioxide
SO3
sulphur trioxide
phosphorus trichloride
P2 O3
diphosphorus trioxide
diphosphorus pentoxide
 if an oxide then drop “a” or “o”)
RULE III →
di(element) tri(elem...)ide

 prefixes indicate the # of atoms in each.
Practice
carbon tetrachloride
iodine monochloride
sulfur dioxide
nitrogen triiodide
carbon disulfide
dinitrogen tetroxide
diphosphorus trisulphide
dichlorine monoxide
SF6
N2 O3
OF2
PI5
IF3
As2S3
MnO2
SbCl5
The following formulae have one and only one name. Memorize them:
CCl4
CS2
CO
CO2
SO2
SO3
carbon tetrachloride
carbon disulphide
carbon monoxide
carbon dioxide
sulphur dioxide
sulphur trioxide
iii) Stock System - the most widely used, it is sometimes called the Roman Numeral or the
IUPAC System. The valence of the first element is shown by a Roman Numeral in brackets
following the English name of the element.
HgCl
mercury (I) chloride
HgCl2 mercury (II) chloride
PBr3
phosphorus (III) bromide
PBr5
phosphorus (V) bromide
Fe2O3 iron (III) oxide
SnF2
tin (II) fluoride
CuO
copper (II) oxide
RULE IV →
element (II) (elem...)ide
English name 
 indicates valence of first element
EXERCISE
Using Rule IV write the correct name for the formulae found in Exercise 2 in the blanks provided on the
right hand side of the page.
PEROXIDES
These are binary oxides which contain one extra oxygen. Write the formula as if it is a regular
oxide and then add on one extra oxygen. Do not cancel subscripts to the lowest whole number ratio!
i.e.
hydrogen oxide H2O, hydrogen peroxide H2O2,
RULE V →
element peroxide
Practice;
zinc peroxide
calcium peroxide
_______
_______
potassium peroxide
aluminum peroxide
_______
_______
Na2O2
________________
H2 O2
________________
BaO2
________________
MgO2
________________
FORMULA OF ELEMENTS
Most elements are written as single entities eg: iron-Fe, silver-Ag, etc. The exceptions to this are:
H2, O2, N2, F2, Cl2, Br2, I2, P4, and S8 (for our purposes we will use S not S8).
POLYATOMIC IONS (RADICALS)
A polyatomic ion (or radical) is a group of elements that behaves as a single element in a chemical
reaction. You will find a list of polyatomic ions along with their corresponding valences on the valence
charts.
NH4+
CO32-
CrO42BrO3-
ammonium radical
carbonate radical
chromate radical
bromate radical
When naming compounds containing positively charged polyatomic ions the name of the
polyatomic ion is given followed by the second elements name which is altered to give an "ide" ending.
When naming compounds containing negatively charged polyatomic ions the name of the element is
given followed by the name of the polyatomic ion name. You will notice that naming polyatomic ions
has a similarity to naming monovalent binary compounds. Be sure to use the cross-over rule when
writing formulas.
NH4Cl
Ca(BrO3)2
ammonium chloride
calcium bromate
K2CrO4
H2CO3
potassium chromate
hydrogen carbonate
RULE VI→ 1. positively charged polyatomic ions - radical (elem...)ide
2. negatively charged polyatomic ions - element radical
Practice;
potassium chromate
copper (II) phosphate
copper (II) chromate
FeCO3
(NH4)2SO4
HgSO4
Ag3PO4
_______
_______
_______
_________________
_________________
_________________
_________________
auric bromide
ammonium chloride
HIO3
Cu3(PO4)2
KMnO4
_______
_______
_________________
_________________
_________________
BASES
These compounds contain the hydroxide radical, OH-.
NaOH
Al(OH)3
sodium hydroxide
aluminum hydroxide
Ca(OH)2 calcium hydroxide
NH4OH ammonium hydroxide
If the element has more than one valence, use the "ous - ic" or the Stock System.
Fe(OH)2
CuOH
ferrous hydroxide
copper (I) hydroxide
Fe(OH)3 ferric hydroxide
Cu(OH)2 copper (II) hydroxide
RULE VII→ element hydroxide
(include valence indicator if necessary)
Practice;
potassium hydroxide
zinc hydroxide
barium hydroxide
Pb(OH)2
Cu(OH)2
Ca(OH)2
________
________
________
____________________
____________________
____________________
ferrous hydroxide
aluminum hydroxide
tin (IV) hydroxide
AuOH
NaOH
Sn(OH)2
________
________
________
____________________
____________________
____________________
HYDRATES
The compound is named following the necessary rule and is followed by a Greek prefix with
"hydrate" to indicate how many water molecules are associated with the crystal.
CuSO4 • 5 H2O
Cl2 • 8 H2O
RULE VIII→
copper (II) sulphate pentahydrate
chlorine octahydrate
compound dihydrate
 Greek prefix
Practice;
calcium sulfate dihydrate
barium chloride dihydrate
sodium carbonate decahydrate
aluminum nitrate monohydrate
aluminum oxide monohydrate
bromine decahydrate
ferric chloride hexahydrate
iodine tetrahydrate
Ca(NO3)2 • 3 H2O
Cu(BrO3)2 • 6 H2O
Cu(NO3)2 • 5 H2O
FeI2 • 4 H2O
LiCl • H2O
Ba(OH)2 • 8 H2O
___________________
___________________
___________________
___________________
___________________
___________________
___________________
___________________
_________________________________________
_________________________________________
_________________________________________
_________________________________________
_________________________________________
_________________________________________
ACIDS
Acids contain hydrogen atoms (H) which give them their acidity. There are a number of different
kinds of acids.
A. Binary Acids
These are two element acids containing hydrogen and a non-metal. They are formed when binary
gases react with water therefore, all are dissolved in water and must have (aq) following the formula.
Binary acids must contain H as the first element. Normal cross-over rule determines the formula. The
names of these acids have the prefix "hydro" and the suffix "ic".
Gases
HCl(g) hydrogen chloride
HF(g)
hydrogen fluoride
HBr(g) hydrogen bromide
RULE IX→
Practice;
hydrobromic acid
hydroiodic acid
hydrofluoric acid
HBr(aq)
HI(aq)
Acids
HCl(aq)
HF(aq)
HBr(aq)
hydrochloric acid
hydrofluoric acid
hydrobromic acid
hydro (elem...)ic acid
_______
_______
_______
______________________
______________________
hydrochloric acid
hydronitric acid
hydrosulphuric acid
_______
_______
_______
HF(aq)
______________________
HCl(aq) ______________________
B. Oxyacids and Their Derivatives
Also known as oxoacids, all acids of this type contain H, O and one other element. The H gives
these compounds their acidity. The element and the O are contained within a polyatomic ion or radical.
All these radicals have 3 oxygens in them except SO42-, PO43- and C2H3O2-. The last of these you will
notice also has hydrogen locked up within the radical. Study the following example to see how these
acids are named. You will notice that the name of the radical is at the root of the acid name and that
various suffixes and prefixes are added depending on the number of oxygen atoms the acid has. The
parent oxy acid contains the radical in its natural state as shown on your valence sheets. The derivatives
of the parent contain more or fewer oxygen atoms than the radical.
OXYACID NAME
hypochlorous acid
chlorous acid
chloric acid
perchloric acid
RULE X→
HClO
HClO2
HClO3
HClO4
Acids;
hypo(rad...)ous acid
(rad...)ous acid
(rad...)ic acid
per(rad...)ic acid
Radicals;
hypo(rad...)ite
(rad...)ite
(rad...)ate
per(rad...)ate
Number of "O" atoms
2 less
1 less
parent
1 more
-
ClO
ClO2ClO3ClO4-
RADICAL NAME
hypochlorite
chlorite
chlorate
perchlorate
No. of "O" atoms
2 less
1 less
parent
1 more
No. of "O" atoms
2 less
1 less
parent
1 more
Practice;
phosphoric acid
hypophosphorous acid
nitrous acid
HBrO
HIO
HNO3
___________
___________
___________
_________________________
_________________________
_________________________
phosphorous acid
sulfuric acid
perbromic acid
HIO4
HClO4
H2SO4
___________
___________
___________
_________________________
_________________________
_________________________
Complete the chart on the next page by following the example. Do not put anything where the block is
"X"ed out as those compounds do not exist!
SALTS
The word salt, is a general name given to a class of compounds which can be formed when an acid
and a base neutralize each other. There are different types of salts just as there are different types of
acids.
A. Binary Salts
Most of the compounds we dealt with in the section on binary compounds could be considered to
be salts formed from a base and a binary acid. We name these salts exactly like binary compounds, they
are, in fact, the same thing.
MgCl2
NaI
magnesium chloride
sodium iodide
CuCl2
KBr
cupric chloride
potassium bromide
B. Salts from Oxy Acids or Their Derivatives
The salts of an oxy acid or its derivative may have lost all or only some of its hydrogen. This
results in two distinct types of salts in this category.
i) Normal Salt
These salts have no remaining acidic hydrogen. They are named with the element
replacing the hydrogen followed by their analogous oxy acid radical name.
sodium hypochlorite
sodium chlorite
sodium chlorate
sodium perchlorate
NaClO
NaClO2
NaClO3
NaClO4
Number of "O" atoms
2 less
1 less
parent
1 more
RULE XI→
element hypo(rad...)ite
element (rad...)ite
element (rad...)ate
element per(rad...)ate
No. of "O" atoms
2 less
1 less
parent
1 more
Practice;
potassium chlorate
iron (III) acetate
magnesium phosphate
tin (IV) hypochlorite
________
________
________
________
sodium nitrate
aluminum chlorite
aurous sulfate
sodium phosphite
________
________
________
________
Au3PO4
NH4NO3
______________________
______________________
Mg(ClO3)2
K2CO3
______________________
______________________
CuMnO4
Hg(ClO4)2
______________________
______________________
(NH4)3PO2
MgSO3
______________________
______________________
PAINLESS PRACTICE
Enter formulae for the 80 compounds
potassium
ammonium
calcium
aluminum
hypochlorite
chlorite
chlorate
perchlorate
hypobromite
bromite
bromate
perbromate
hypoiodite
iodite
iodate
periodate
nitrite
nitrate
sulphite
sulphate
carbonate
hypophosphite
phosphite
phosphate
SUMMARY OF NOMENCLATURE RULES
1. BINARY COMPOUNDS (two elements)
Basic Rule: element (elem...)ide
If the first element has more than one valence, use one of the the following:
a) ous-ic System: lower valence → (elem...)ous (elem...)ide
higher valence → (elem...)ic (elem...)ide
b) Greek Prefix System: element tri(elem...)ide
 # of atoms of 2nd element
c) Roman Numeral System (IUPAC): element (III) (elem...)ide
English name 
 valence of 1st element
Peroxide = oxide + one more oxygen atom
2. BASES (OH)
Basic Rule: element hydroxide
If the element has more than one valence, use ous-ic system or Stock System as indicated above in
binary compounds.
3. ACIDS (H)
1) Binary Acids: hydro(elem...)ic acid
2) Oxygen Acids:
acid rule
# "O" atoms
hypo(rad...)ous acid
2 less
(rad...)ous acid
1 less
(rad...)ic acid
parent radical
per (rad...)ic acid
1 more
4. SALTS
1) Binary: use rules for binary compounds.
1) Polyatomic: use compound rule for oxy acids.
5. HYDRATES
Basic Rule: compound dihydrate
Use appropriate rule   # of water molecules attached.
compound rule
hydrogen hypo(rad...)ite
hydrogen (rad...)ite
hydrogen (rad...)ate
hydrogen per(rad...)ate
SCH 4C
Nomenclature Practice #1
Name__________________________
I. Write the formulae for the following substances whether they exist or not.
1.
magnesium bromide
1.
2.
cupric oxide
2.
3.
ferrous hypophosphite
3.
4.
lead (II) nitrate
4.
5.
iodous acid
5.
6.
calcium peroxide
6.
7.
aluminum hydroxide
7.
8.
antimonic chlorite
8.
9.
barium pernitrate
9.
10. nitrogen
10.
11. manganese (IV) oxide
11.
12. hydrosulphuric acid
12.
13. silver carbonate
13.
14. diarsenic pentoxide
14.
15. magnetic iron oxide
15.
16. ammonium perchlorate
16.
17. sodium sulphite
17.
18. zinc acetate
18.
19. phosphorous fluoride
19.
20. silicon dioxide
20.
21. potassium phosphate
21.
22. aluminum hypocarbonite
22.
23. stannic sulphide
23.
24. calcium sulphate dihydrate
24.
25. iron (II) bromite
25.
SCH 4C
Nomenclature Practice #1
Name__________________________
II. Write one suitable chemical name for each of the following substances whether they exist or not.
1.
Hg2SO4
1.
2.
Ca3N2
2.
3.
K2CO3
3.
4.
SbI3
4.
5.
(NH4)3PO3
5.
6.
Fe(OH)3
6.
7.
Na2CO3 • 10 H2O
7.
8.
HNO2
8.
9.
CuClO
9.
10. CCl4
10.
11. H3PO5
11.
12. AgNO3
12.
13. SO3
13.
14. Mg(C2H3O2)2
14.
15. H2O2
15.
16. K3PO2
16.
17. HBr
17.
18. SnS
18.
19. NH4BrO4
19.
20. Zn(IO)2
20.
21. BaSO3
21.
22. Al4C3
22.
23. SiI4
23.
24. MnSO4
24.
25. CO
25.
SCH 4C
Nomenclature Practice #2
Name__________________________
I. Write the formulae for the following substances whether they exist or not.
1.
sodium sulphite
1.
2.
iodous acid
2.
3.
zinc oxide
3.
4.
aluminum hydroxide
4.
5.
potassium persulphate
5.
6.
diphosphorus tetraoxide
6.
7.
ammonium hypophosphite
7.
8.
mercurous sulphate
8.
9.
iodine tribromide
9.
10. antimonous chloride
10.
11. calcium bromite
11.
12. magnetic iron oxide
12.
13. copper (II) sulphate pentahydrate
13.
14. tin (II) carbonate
14.
15. barium peroxide
15.
16. hydrogen
16.
17. ferric sulphide
17.
18. hydrosulphuric acid
18.
19. diphosphorus trioxide
19.
20. acetic acid
20.
21. ferrous nitrite
21.
22. silver perchlorate
22.
23. monopotassium hydrogen phosphite
23.
24. stannic fluoride
24.
25. hypophosphorous acid
25.
SCH 4C
Nomenclature Practice #2
Name__________________________
II. Write one suitable chemical name for each of the following substances whether they exist or not.
1.
Hg(BrO)2
1.
2.
AsCl3
2.
3.
KNO2
3.
4.
SO3
4.
5.
H3PO2
5.
6.
(NH4)3PO3
6.
7.
Ag2S
7.
8.
Mg(OH)2
8.
9.
HClO4
9.
10. SnCl4
10.
11. HOH
11.
12. CaSO4 • 2 H2O
12.
13. HNO3
13.
14. HI (g)
14.
15. Cu(IO2)2
15.
16. NH3
16.
17. H2S
17.
18. Al2(SO3)3
18.
19. Zn(ClO4)2
19.
20. CS2
20.
21. Sn(BrO3)2
21.
22. Pb(C2H3O2)2
22.
23. FeCO3
23.
24. MnO2
24.
25. Ca3(PO4)2
25.
SCH 4C
1.
2.
ASSIGNMENT
Write a formula for each of the following;
sodium sulphite
aluminum chlorate
mercuric perphosphate
stannic bromate
antimony (v) oxide
plumbous chloride
lead (ii) nitrate
acetic acid
sulphur dioxide
manganese (iv) sulphide
cupric bromite
calcium phosphate
mercury (ii) hyposulphite
zinc perchlorate
phosphorous acid
hydrogen iodide
ferrous nitrite
silver sulphide
calcium hypochlorite
ammonium phosphate
hydrofluoric acid
calcium hydroxide
mercury (ii) oxide
perbromic acid
magnesium hyposulphite
sodium iodite
silver phosphate
iodic acid
chlorine
sodium peroxide
nitrogen (iii) sulphide
barium nitrate
carbon disulphide
magnetic iron oxide
Write one suitable name for each of the following;
AsCl3
Ca(Br)2
NH4Br
H3PO5 (aq)
Hg2O
Al(NO2)3
NH3
Na2SO3
AgOH
K2CO3
Al2(SO3)3
Sb2S5
HgClO
HIO2
Ca(C2H3O2)2
FeS
Pb(NO3)2
NH4BrO4
HgS
MgO
Zn(OH)2
Al4C3
HClO2
Fe3O4
SO2
Fe2(CO3)3
KNO3
Ca(ClO4)2
(NH4)3PO3
Na3PO3
HI (g)
HClO4 (aq)
Mn(NO3)2
CS2
As2(SO4)3
Fe(OH)2
O2
H 2O 2