SCH 3UI - Nomenclature Methods You Need to Know
Type of
Compound
Examples
Description
Nomenclature Tips
Type of
Bonding
IONIC COMPOUNDS
BINARY
(IONIC)
MgF2
Magnesium Fluoride
POLYATOMIC MgSO4
Magnesium Sulfate
(IONIC)
Only two elements
form the compound:
metal + non-metal
metal + polyatomic
ion
The compound name ends with “ide”
The compound name usually ends with “ate” or
“ite” (Exceptions: hydroxide, bisulfide, cyanide,
etc.)
*see the text to find
the charge of the
polyatomic ion
The polyatomic ion usually ends with “ate” or “ite”
metal + non-metal
or
metal + polyatomic
ion
Apply the same nomenclature rules used above!!
Multivalent
metals
PbO
lead (II) oxide or
plumbous oxide
Using the
Classical
Naming System
Cu3(PO4)2
copper (II) phosphate or
cupric phosphate
Polyatomic
Families
CaSO2 – calcium
hyposulfite
CaSO3 – calcium sulfite
CaSO4 – calcium sulfate
CaSO5 – calcium
persulfite
metal + polyatomic
ion
CuSO4·5H20
Copper (II) Sulphate
Pentahydrate or
Cupric sulphate
pentahydrate
metal + ion (anion
or polyatomic ion)
+ water
ionic
The non-metal ends with “ide”
Ex. Sulfur ---> Sulfide
When writing the names of compounds with
multivalent metals, remember to put the valence in
brackets - Ex. Fe(OH)3 - Iron (III) Hydroxide
When writing the names of compounds with
transition metals (Rows IB to VIIIB) remember to
put the valence in brackets - Ex. Iron (III) Oxide
Mix - Ionic and
Covalent
The atoms within
the polyatomic
ion are bonded
covalently. The
metal is bonded
to the polyatomic
ion ionically
ionic or
mixed
Use the T-chart or box method when trying to name
a compound with multivalent given the formula.
Use page 95 for help with the Classical names
HYDRATES
*see the text to find
the charge of the
polyatomic ion
Same system as polyatomic
compounds
hypo-____-ite = two less O’s than normal
-ite= one less O than normal
-ate = normal number of O’s
per-_____-ate = one more O than normal
The compound is named like any other ionic or
polyatomic compound but the hydrate is added to
the end of the name.
Mix - Ionic and
Covalent
The atoms within
the polyatomic
ion are bonded
covalently. The
metal is bonded
to the polyatomic
ion ionically
Mix - Ionic &
Covalent
Greek prefixes are placed in front of the the term
‘hydrate’ to indicate how many H20 molecules are
incorporated into the structure.
ACIDS
BINARY
ACIDS
OXYACIDS
HCl Hydrochloric Acid
HBr Hydrobromic Acid
or aqueous hydrogen
bromide
HNO3Nitric Acid
H2SO4Sulfuric Acid or
aqueous hydrogen sulfate
hydrogen + nonmetal
usually H + halogen
Hydro + halogen - ending + ic + Acid
Or
Aqueous hydrogen + halogen - ending + ide
Covalent
(polar
covalent)
hydrogen + oxyanion
(polyatomic ion)
polyatomic ion (radical) - ending +” ic” or “ous” +
Acid
Covalent
(polar
covalent)
MOLECULAR COMPOUNDS
MOLECULAR
(Binary)
Hydrocarbons
CO2
Carbon Dioxide
P2O5
Diphosphorus Pentoxride
CH4
C2H6
Methane Ethane
C2H4
Ethene
C2H2
Two non-metals
form the compound
Hydrocarbons
Alkanes (fossil fuels)
with the formula:
CnH2n+2
Compounds are named like binary compounds
except Greek prefixes are placed in front of each
element: (Ex. mono = 1, di = 2, tri = 3, tetra = 4,
penta = 5, hexa = 6, octa = 8, deca = 10). Often
mono is dropped from the first element.
Names end with “ane”, “ene”, and “yne”
covalent
(molecular)
covalent
(molecular)