Common Cations, Anions, Acids, Salts and Hydrate Nomenclature
Cations (positive ions)
Anions (negative ions)
Acids (H+ and anion)
H+
Hydrogen ion (proton)
NH4+ Ammonium ion
Main Group Ions
Li+ Lithium ion
Na+ Sodium ion
K+
Potassium ion
Rb+ Rubidium ion
Cs+ Cesium ion
Be2+ Beryllium ion
Mg2 Magnesium ion
Ca2+ Calcium ion
Sr2+ Strontium ion
Ba2+ Barium ion
AI3+ Aluminum ion
Sn2+ Tin(II) (stannous) ion
Sn4+ Tin(IV) (stannic) ion
Pb2+ Lead(II) (plumbous) ion
Pb4+ Lead(IV) (plumbic) ion
Sb3+ Antimony(III) (antimonous) ion
Sb5+ Antimony(V) (antimonic) ion
Bi3+ Bismuth(III) (bismuthous) ion
Bi5+ Bismuth(V) (bismuthic) ion
Transition metal ions
Cr2+ Chromium(II) (chromous) ion
Cr3+ Chromium(III) (chromic) ion
Mn2+ Manganese(II) (manganous) ion
Mn3+ Manganese(III) (manganic) ion
Fe2+ Iron(II) (ferrous) ion
Fe3+ Iron(III) (ferric) ion
Co2+ Cobalt(II) (cobaltous) ion
Co3+ Cobalt(III) (cobaltic) ion
Ni2+ Nickel(II) (nickelous) ion
Ni3+ Nickel(III) (nickelic) ion
Cu+ Copper(l) (cuprous) ion
Cu2+ Copper(II) (cupric) ion
Ag+ Silver(I) ion
Au+ Gold(I) (aurous) ion
Au3+ Gold(III) (auric) ion
Zn2+ Zinc ion
Cd2+ Cadmium ion
Hg22+ Mercury(I) (mercurous) ion
Hg2+ Mercury(II) (mercuric) ion
H–
Hydride ion
F–
Fluoride ion…………………………………… …
Cl –
Chloride ion…………………………………… …
Br –
Bromide ion…………………………………… …
I–
Iodide ion …………………………………… …
2–
O
Oxide ion
OH–
Hydroxide ion
O22–
Peroxide ion
S2–
Sulfide ion ………………………………………
HS–
Hydrogen sulfide ion
Se2–
Selenide Ion
N3–
Nitride ion
–
N3
Azide ion
P3–
Phosphide ion
As3Arsinide ion
C4–
Carbide ion
CN–
Cyanide ion…………………………………… …
Oxoanions
CIO1– Hypochlorite ion……………………………… …
CIO2– Chlorite ion…………………………………… …
CIO3– Chlorate ion…………………………………… …
ClO4– Perchlorate ion ……………………………… …
SO32– Sulfite ion……………………………………… …
SO42– Sulfate ion ………………………………………
HSO4– Hydrogen sulfate ion (bisulfate ion)
S2O32- Thiosulfate ion …………………………………
NO2– Nitrite ion …………………………………………
NO3– Nitrate ion…………………………………………
PO33– Phosphite ion………………………………… …
PO43– Phosphate ion………………………………… …
HPO42– (Mono)hydrogen phosphate ion
H2PO4– Dihydrogen phosphate ion
CO32– Carbonate ion………………………………… …
HCO3– Hydrogen carbonate ion (bicarbonate ion)
C2O42– Oxalate ion ………………………………………
NCO– Cyanate ion…………………………………… …
OCN– Isocyanate ion……………………………………
SCN– Thiocyanate ion……………………………… …
CrO42– Chromate ion ………………………………… …
Cr2O72– Dichromate ion ……………………………… …
MnO4– Permanganate ion
Salts (Made of ions, neutral in charge)
Name: (Cation)(anion) (prefix)hydrate (If # = 0 hydrate is omitted)
Formula: (Cation)m(Anion)n·(#)H2O (If # = 0 H2O is omitted)
Examples
Cations on the left, anions on the right, charge must cancel
Strontium Chloride = Strontium ions and Chloride ions = Sr+2 and Cl‐ = SrCl2
Multiples of polyatomic ions require parenthesis
Ammonium Sulfate = Ammonium ions and Sulfate ions = NH4+ and SO42‐ = (NH4)2SO4
Calcium Phosphate = Calcium ions and Phosphate ions = Ca2+ and PO43‐ = Ca3(PO4)2
Waters of hydration (use table to left)
copper(II) sulfate pentahydrate = CuSO4∙5H2O
HF
HCl
HBr
HI
Hydrofluoric acid
Hydrochloric acid
Hydrobromic acid
Hydroiodic acid
H 2S
Hydrosulfuric acid
HCN
Hydrocyanic Acid
Oxoacids
HCIO
Hypochlorous acid
HCIO2 Chlorous acid
HCIO3 Chloric acid
HClO4 Perchloric acid
H2SO3 Sulfurous acid
H2SO4 Sulfuric acid
H 2S 2O 3
HNO2
HNO3
H3PO3
H3PO4
Thiosulfuric acid
Nitrous acid
Nitric acid
Phosphorous acid
Phosphoric acid
H2CO3
Carbonic Acid
H 2C 2O 4
HOCN
HNCO
HNCS
H2CrO4
H2Cr2O7
Oxalic acid
Cyanic Acid
Isocyanic acid
Thiocyanic Acid
Chromic acid
(Di)Chromic acid
# of Water Prefix
1
Mono
2
Di
3
Tri
4
Tetra
5
Penta
6
Hexa
7
Hepta
8
Octa
9
Nona
10
Deca
11
Undeca
Common Covalent Binary Inorganic Compounds
# of atoms Prefix
1
2
3
4
5
6
7
8
9
10
Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Common Examples (element closest to fluorine goes on right)
H2
O2
O3
H 2O
F2
HF
Cl2
HCl
Br2
I2
Hydrogen
Oxygen
Ozone
Water (Dihydrogen Monoxide)
Fluorine
Hydrogen fluoride
Chlorine
Hydrogen chloride
Bromine
Iodine
N2
NH3
NO
NO2
N 2O
N 2O 2
N 2O 4
CO
CO2
CCl4
Nitrogen
Ammonia
Nitrogen monoxide (Nitric Oxide)
Nitrogen dioxide
Dinitrogen monoxide (Nitrous oxide)
Dinitrogen dioxide
Dinitrogen tetroxide
Carbon monoxide
Carbon dioxide
Carbon tetrachloride
Organic Nomenclature and Symbolism
(Other group prefixes)(longest chain prefix)(highest bond root)(most important group suffix)
Bond Order Name Drawn Root Formula
Carbon
Chain Prefix
Carbon has 4 bonds
1
Single C-C
ane
CnH2n+2
In formula:
#
Systematic
Common**
Groups -1 H
2
Double C=C
ene
CnH2n
1
Methyl
Formyl
Other C-C bonds -2 H
3
Triple C≡C
yne
CnH2n-2
2
Ethyl
Acetyl
3
Propyl
Propionyl
Group Name
Drawn
Prefix
Suffix
4
Butyl
Butyryl
Amine
-NH2
Amino
amine
5
Pentyl
Valeryl
Ammonium ion
-NH3+
ammonium ion
6
Hexyl
Caproyl
7
Heptyl
Enanthyl
Carboxylic acid*
Carboxyl
oic acid
or -COOH or -CO2H
8
Octyl
Caprylyl
9
Nonyl
Pelargonyl
Carboxylate ion*
oate ion
or -COO- or -CO210
Decyl
Capryl
Alcohol
-OH
Hydroxy
ol
Drop ‘yl’ from prefix for longest chain
-F
Fluoro
*Include carbon in chain prefix
-Cl
Chloro
Halogen
-Br
Bromo
**Don’t use bond root (names only ane)
-I
Iodo
Drop ‘o’ from carboxyl groups
Aromatic
Phenyl
(‘ic’ and ‘ate’)
or C6H5 or -Ф or -Ph
Examples
Name Formula
Methane
CH4
Ethane
C 2H 6
Propane
C 3H 8
Butane
C4H10
Pentane
C5H12
Methanol CH3OH
Ethanol C2H5OH
Propanol C3H7OH
Butanol C4H9OH
Pentanol C5H11OH
Systematic Name
Methanoic acid
Ethanoic acid
Propanoic acid
Butanoic acid
Pentanoic acid
Methanoate ion
Ethanoate ion
Propanoate ion
Butanoate ion
Pentanoate ion
Common Name
Formic acid
Acetic acid
Propionic acid
Butyric acid
Valeric acid
Formate ion
Acetate ion
Propionate ion
Butyrate ion
Valerate ion
Formula
HCO2H
CH3CO2H
C2H5CO2H
C3H7CO2H
C4H9CO2H
HCO2CH3CO2C2H5CO2C3H7CO2C4H9CO2-
Name
1,2-Dichloroethane
Methylamine
Methylammonium ion
1,3-butadiene
Hydroxyethanoic acid
Phenol
Formula
C2H4Cl2
CH3NH2
CH3NH3+
C 4H 6
HOCH2CO2H
C6H5OH
Special Names
Benzene
Toluene
Formula
C 6H 6
C6H5CH3
Most Common Formula Representations (All represent ethanol)
Example
C 2H 6O
CH3CH2OH
Name
Molecular Formula
Condensed Molecular
Formula
Structural Formula
Line Formula
0
