Naming Inorganic Compounds
yes
yes
Group I or II;
Al, Ag, Zn, NH4?
Metal or NH4?
no
no
yes
yes
O is present,
but not H2O or H2O2?
yes
Type I Ionic Compound
Type II Ionic Compound
Al2O3 (s) aluminum oxide
LiOH (s)
lithium hydroxide
AgNO3(s)
silver nitrate
Na2O2(s)
sodium peroxide
CaCO3(s)
calcium carbonate
NH4NO3(s)
ammonium nitrate
CuCl(s)
copper(I) chloride
CuCl2(s)
copper(II) chloride
Fe2O3(s)
iron(III) oxide
FeO(s)
iron(II) oxide
Cr2(SO4) 3(s)
chromium(III) sulfate
MnS(s)
manganese(II) sulfide
Sn(NO3) 2(s)
tin(II) nitrate
Oxyacid
HClO(aq)
hypochlorous acid
HClO2(aq)
chlorous acid
HClO3(aq)
chloric acid
HClO4(aq) or (l)
perchloric acid
H2SO3(aq)
sulfurous acid
H2SO4(aq) or (l)
sulfuric acid
Nonoxyacid
HCl(aq)
hydrochloric acid
H2S(aq)
hydrosulfuric acid
HCN(aq)
hydrocyanic acid
H in front?
no
no
(aq) is written?
no
Binary Covalent Compound
HCl(g)
hydrogen chloride
H2S(g)
hydrogen sulfide
HCN(g)
hydrogen cyanide
H2O2(l)
hydrogen peroxide
H2O(l)
water
P2O5(s)
diphosphorus pentoxide
NO2(g)
nitrogen dioxide
S2Cl2(l)
disulfur dichloride
CO(g)
carbon monoxide
PF5(g)
phosphorus pentafluoride
XeF4(s)
xenon tetrafluoride
NH3(g)
ammonia
CH4(g)
methane
Intentionally Blank
CHEMICAL SYMBOLS AND FORMULAS
Al
1) Element aluminum
2) Elementary substance (aluminum metal)
3) One atom of aluminum
2Al
Two atoms of Aluminum
2H
Two atoms of hydrogen
H2
1) Molecular hydrogen; substance (hydrogen gas)
2) One molecule of hydrogen
H2O
1) Water as a substance ( a covalent compound)
2) One molecule of water
2H 2 O
Two molecules of water
2Al + 3O 2
Two atoms of aluminum and (mixed with)
three molecules of oxygen
Al 2 (SO 4 ) 3
1) Aluminum sulfate as a substance (an ionic compound)
2) One formula unit of aluminum sulfate:
per each 2 atoms of aluminum there are 3 SO 4 groups
OR
2 atoms of aluminum, 3 atoms of sulfur and 12 atoms of
oxygen per one formula unit of aluminum sulfate
Greek Prefixes for Naming Compounds
Number
Prefix
1
mono-
2
di-
bicycle
3
tri-
tricycle
4
tetra-
5
penta-
6
hexa-
7
hepta-
September
8
octa-
October
9
nona-
10
deca-
11
undeca-
12
dodeca-
13
trideca-
20
icosa-
the Pentagon
(Latin)
November
December
(Latin)
Names and Formulas of Common Ions
Positive Ions (cations)
Negative Ions (anions)
The charges of these ions can be figured out
using the periodic table:
Hydrogen
Lithium
Sodium
Potassium
Rubidium
Cesium
Beryllium
Magnesium
Calcium
Strontium
Barium
Aluminum
H+
Li+
Na+
K+
Rb+
Cs+
Be2+
Mg2+
Ca2+
Sr2+
Ba2+
Al3+
These ions must be memorized:
The charges of these ions can be figured out
using the periodic table:
Hydride
Fluoride
Chloride
Bromide
Iodide
Oxide
Sulfide
Nitride
Phosphide
H
F
Cl 
Br 
I
O 2
S 2
N 3
P 3
These ions must be memorized:
Hydronium
Ammonium
Silver
Cadmium
Zinc
Copper (I) or cuprous
Copper (II) or cupric
Mercury (I) or mercurous
Mercury (II) or mercuric
Lead (II) or plumbus
Lead (IV) or plumbic
Iron (II) or ferrous
Iron (III) or ferric
H 3 O+
NH 4
Ag+
Cd2+
Zn2+
Cu+
Cu2+
Hg 22
Hg2+
Pb2+
Pb4+
Fe2+
Fe3+
Acetate
Hydroxide
Cyanide
Cyanate
Thiocyanate
Hypochlorite
Chlorite
Chlorate
Perchlorate
Nitrate
Nitrite
Permanganate
Carbonate
Manganese (II)
Nickel (II)
Tin (II) or stannous
Tin (IV) or stannic
Chromium (II)
Chromium (III)
Cobalt (II)
Mn2+
Ni2+
Sn2+
Sn4+
Cr2+
Cr3+
Co2+
Hydrogen carbonate or bicarbnate
Chromate
Dichromate
Peroxide
Sulfate
Hydrogen sulfate or bisulfate
Sulfite
Cobalt (III)
Bismuth (III)
Co3+
Bi3+
Hydrogen sulfite or bisulfite
Phosphate
Hydrogen phosphate
Dihydrogen phosphate
Borate
Oxalate
Note: Ions in bold type are very common and must be memorized first!!!
C 2 H 3 O 2
OH 
CN 
OCN 
SCN 
ClO 
ClO 2
ClO 3
ClO 4
NO 3
NO 2
MnO 4
CO 32
HCO 3
CrO 42
Cr 2 O 72
O 22
SO 42
HSO 4
SO 32
HSO 3
PO 34
HPO 42
H 2 PO 4
BO 33
C 2 O 24
MONATOMIC IONS
IA
VII A VIII A
-
II A
III A
IV A
VA
VI A
H
C4- N3- O2- F-
III B
IV B
VB
VI B
Cr2+
Cr3+
VII B VIII B VIII B VIII B I B
Mn2+
Fe2+ Co2+
Fe3+ Co3+
Ni2+
II B
Si4- P3- S2- Cl-
Cu+
As3- Se2- Br-
Cu2+
Sn2+
Te2- I-
Sn4+
E
2
Au+ Hg 2
Pb2+
Au3+
Pb4+
Hg2+
Bi3+
metallic elements that form several stable monatomic cations:
Cr3+ is chromium (III) ion, Hg2+ is mercury (II) ion, etc.; Hg 22 is a polyatomic ion called mercury (I) ion
E nonmetallic elements; each forms a single stable monatomic anion:
-
4-
F is fluoride ion, Si 4- is silicide ion, etc.
ions that do not exist in aqueous solutions; they react with water by accepting either H+
or OH- ions (small amounts of H+ and OH- ions are always present in water: H 2 O ⇆ H+ + OH-)
Oxyacids and Oxyanions
SO32─
sulfite ion
minus H+
HSO3─
NO2─
hydrogen
sulfite ion
nitrite ion
minus H+
minus H+
H2SO3
HNO2
sulfurous acid
nitrous acid
minus O
HNO3
nitric acid
minus H+
NO3
─
nitrate ion
minus O
H2CO3
carbonic acid
minus H+
HCO3─
hydrogen
carbonate ion
minus H+
CO32─
carbonate ion
H2SO4
sulfuric acid
minus H+
HSO4─
hydrogen
sulfate ion
minus H+
SO42─
sulfate ion
H3PO4
phosphoric acid
minus H+
H2PO4─
dihydrogen
phosphate ion
minus H+
HPO42─
hydrogen
phosphate ion
minus H+
PO43─
phosphate ion
OXYACIDS
H 2 O (HOH)
*
water
OXYANIONS
OH −
hydroxide ion
HC 2 H 3 O 2 (aq) acetic acid
C 2 H 3 O 2− acetate ion
HClO 4 (aq)
perchloric acid
ClO 4−
perchlorate ion
HClO 3 (aq)
chloric acid
ClO 3−
chlorate ion
HClO 2 (aq)
chlorous acid
ClO 2−
chlorite ion
HClO (aq)
hypochlorous acid
ClO −
hypochlorite ion
HNO 3 (aq)
nitric acid
NO 3−
nitrate ion
HNO 2 (aq)
nitrous acid
NO 2−
nitrite ion
H 2 CO 3 (aq)
carbonic acid CO 32− carbonate ion
HCO 3−
H 2 SO 4 (aq)
sulfuric acid
HSO 4−
H 2 SO 3 (aq)
SO 24−
sulfite ion
hydrogen sulfite ion (bisulfite ion)
phosphoric acid
HPO 24−
sulfate ion
hydrogen sulfate (bisulfate ion)
sulfurous acid SO 32−
HSO 3−
H 3 PO 4 (aq)
hydrogen carbonate ion (bicarbonate ion)
PO 34−
phosphate ion
hydrogen phosphate ion
H 2 PO 4− dihydrogen phosphate ion
*
Pure covalent molecular compounds or their aqueous solutions. Usually, only acids with the highest
number of oxygen atoms (HClO 4 , HNO 3 , H 3 PO 4 , H 2 SO 4 ) can be obtained in pure form. They are also
stable in aqueous solutions. All other acids exist only as aqueous solutions. Organic acids, such as acetic
acid, are stable in pure form and in aqueous solutions.
NONOXYACIDS AND NONOXYANIONS
COMPOUNDS
ACIDS
ANIONS
pure substances:
only HX molecules
aqueous solutions:
HX dissolved in H 2 O
exist in ionic crystals
or as X−(aq) in aqueous
solutions
HF(g)
hydrogen fluoride
HF(aq)
hydrofluoric acid
F−
fluoride ion
HCl(g)
hydrogen chloride
HCl(aq)
hydrochloric acid
Cl −
chloride ion
HBr(g)
hydrogen bromide
HBr(aq) hydrobromic acid
Br −
bromide ion
HI(g)
hydrogen iodide
HI(aq)
hydroiodic acid
I−
iodide ion
H 2 S(g)
hydrogen sulfide
H 2 S(aq)
hydrosulfuric acid
S 2− sulfide ion
HS − hydrogen sulfide ion
HCN(g)
hydrogen cyanide
HCN(aq) hydrocyanic acid
CN − cyanide ion
PREFIXES AND SUFFIXES IN THE NAMES OF ACIDS
AND CORRESPONDING ANIONS
Number of
Oxygen Atoms
Acid
Anion
Greatest
per– ...... –ic acid
per– ...... –ate ion
Greater
....... –ic acid
....... –ate ion
Smaller
....... –ous acid
....... –ite ion
Smallest
None
hypo– ..... –ous
acid
hypo– ..... –ite ion
hydro– ....... –ic acid
....... –ide ion
EXAMPLE:
−
perchlorate ion
−
chlorate ion
ClO2
−
chlorite ion
hypochlorous acid
ClO
−
hypochlorite ion
hydrochloric acid
Cl
HClO 4 (aq)
perchloric acid
ClO4
HClO 3 (aq)
chloric acid
ClO3
HClO 2 (aq)
chlorous acid
HClO(aq)
HCl(aq)
−
chloride ion
Formulas and Names of Binary Ionic Compounds
(1) Write the formula for each ion below the ion’s name.
(2) Fill in the blanks with the correct formula and name of the compound formed by the combination of ions.
Chloride ion
Cl
Sodium ion
+
Na
Copper (I) ion
Calcium ion
Iron (II) ion
Iron (III) ion
Aluminum ion
─
NaCl
sodium chloride
Oxide ion
Bromide ion
Sulfide ion
Nitride ion
Formulas and Names of Binary Covalent Compounds
Fill the blanks in the following table.
Formula
Name
Formula
CO
tetraphosphorus decaoxide
carbon disulfide
NH 3
SO 2
sulfur hexafluoride
SiC
N2O3
dinitrogen monoxide
OF 2
P4S3
silicon tetrachloride
IF 7
CH 4
H2O
sulfur trioxide
dihydrogen disulfide
Cl 2 O 7
Name
KrF 2
dinitrogen pentaoxide
Formula Writing Exercise A
For each box write the chemical formula of the compound formed by the cation at the head of the column
and the anion at the left of the row.
Li 
Br 
SO 24
OH 
F
O 2
NO 3
PO 34
Cl 
S 2
I
CO 32
LiBr
Mg 2
NH 4
Al 3
Na 
Ba 2
K
Ca 2
FORMULA WRITING – EXERCISE 1
Give a correct chemical name for each of the following compounds:
1.
MgO
____magnesium oxide____________________
2.
PbI 2
______________________________________
3.
FeS
______________________________________
4.
ZnSO 4
______________________________________
5.
Li 2 CO 3
______________________________________
6.
Ba(NO 3 ) 2
______________________________________
7.
NH 4 NO 2
______________________________________
8.
K 2 SO 3
______________________________________
9.
CrCl 3
______________________________________
10.
Sr(C 2 H 3 O 2 ) 2 ______________________________________
11.
Mg 3 N 2
______________________________________
12. Ca 3 (PO 4 ) 2
______________________________________
13. SnO 2
______________________________________
14. KMnO 4
______________________________________
15. Hg 2 Cl 2
______________________________________
16. NaHCO 3
______________________________________
17. CCl 4
______________________________________
18. NO 2
______________________________________
19.
______________________________________
N2O5
20. PBr 5
______________________________________
21. CaO 2
______________________________________
22. HCl(aq)
______________________________________
23. HNO 3 (aq)
______________________________________
24.
H 2 SO 3 (aq)
______________________________________
25.
H 3 PO 4 (aq)
______________________________________
FORMULA WRITING – EXERCISE 2
Write chemical formulas for the following compounds:
1.
Potassium iodide
______________________________________
2.
Barium sulfate
______________________________________
3.
Aluminum nitrate
______________________________________
4.
Copper (II) carbonate
______________________________________
5.
Gold (III) chloride
______________________________________
6.
Ferric hydroxide
______________________________________
7.
Lead (II) chromate
______________________________________
8.
Nickel (II) hydroxide
______________________________________
9.
Mercury (II) bromide
______________________________________
10.
Silver acetate
______________________________________
11.
Magnesium chlorate
______________________________________
12.
Sodium peroxide
______________________________________
13.
Manganese (II) phosphate
______________________________________
14.
Ammonium sulfide
______________________________________
15.
Platinum (IV) fluoride
______________________________________
16.
Chromium (III) hydroxide
______________________________________
17.
Calcium oxalate
______________________________________
18.
Antimony trichloride
______________________________________
19.
Ammonia
______________________________________
20.
Silicon dioxide
______________________________________
21.
Carbon monoxide
______________________________________
22. Hydrobromic acid
______________________________________
23.
Nitrous acid
______________________________________
24.
Acetic acid
______________________________________
25.
Sulfuric acid
______________________________________
FORMULA AND NAME EXERCISES
Indicate the covalent compounds below with *. Write the complete chemical formulas for
each of the compounds (ionic or covalent).
1. Barium sulfate
___________
2.
Calcium chloride
___________
3. Potassium oxide
___________
4.
Lithium hydroxide
___________
5. Aluminum iodide
___________
6.
Carbon disulfide
___________
7. Tin (IV) fluoride
___________
8.
Manganese (II) phosphide
___________
9. Iron (III) sulfite
___________
10.
Beryllium acetate
___________
11. Mercury (II) nitrite
___________
12.
Copper (I) phosphate
___________
13. Dinitrogen pentoxide
___________
14.
Hydrogen peroxide
___________
15. Boron tribromide
___________
16.
Nickel (II) chromate
___________
17. Sodium hydrogen carbonate ___________
(sodium bicarbonate)
18.
Hydrocyanic acid
___________
19. Nitrous acid
20.
Silver hypochlorite
___________
___________
Indicate covalent compounds below with *. Write the complete name formulas for each of the
compounds (ionic or covalent).
1. Mg(CN)2
____________________
2.
Li3PO4
____________________
3. P4O10
____________________
4.
KMnO4
____________________
5. (NH4)2CO3
____________________
6.
Hg(OH)2
____________________
7. CdSe
____________________
10.
OF2
____________________
11. N2(g)
____________________
12.
HBrO3(aq)
____________________
13. CsHS
____________________
14.
SiCl4
____________________
15. KH2PO4
____________________
16.
HBr(aq)
____________________
17. Cd(NO3)2·7H2O ____________________
17.
AsH3
____________________