Name: ________________________________
IONS – MONATOMIC CATIONS
Main Group Elements
1A
I & II
II & III
II & IV
Charge
1+
2A
2+
3A
3+
Examples:
d –block elements
Name
Ag+
Silver
Cd2+
Cadmium
Mn2+
Manganese (II)
Ni2+
Nickel (II)
Zn2+
Zinc
Stock
Latin
Cu+
Copper (I)
Cuprous
Cu2+
Copper (II)
Cupric
Hg2 2+
Mercury (I)
Mercurous
Hg2+
Mercury (II)
Mercuric
Fe2+
Iron (II)
Ferrous
Fe3+
Iron (III)
Ferric
Co2+
Cobalt (II)
Cobaltous
Co3+
Cobalt (III)
Cobaltic
Cr2+
Chromium (II)
Chromous
Cr3+
Chromium (III)
Chromic
Pb2+
Lead (II)
Plumbous
Pb4+
Lead (IV)
Plumbic
Sn2+
Tin (II)
Stannous
Sn4+
Tin (IV)
Stannic
IONS – POLYATOMIC
Polyatomic Ions
Name
NH4 +
Ammonium
C2H3O2 -
Acetate
BrO4 -
Perbromate
BrO2 -
Bromate
BrO3 -
Bromite
BrO -
Hypobromite
ClO4 -
Perchlorate
ClO3 -
Chlorate
ClO2 -
Chlorite
ClO -
Hypochlorite
IO4 -
Periodate
IO3 -
Iodate
IO2 -
Iodite
IO -
Hypoiodite
CN –
Cyanide
HCO3 -
Bicarbonate (Hydrogen carbonate)
HSO4 -
Bisulfate (Hydrogen sulfate)
MnO4 -
Permanganate
NO3 -
Nitrate
NO2 -
Nitrite
OH -
Hydroxide
CO3 2-
Carbonate
SO4 2-
Sulfate
SO3 2-
Sulfite
CrO42-
Chromate
Cr2O72-
Dichromate
PO4 3-
Phosphate
IONS – ANIONS
The anions are determined by the group number they are located in on the periodic table. This can
be easily completed by subtracting the group number the element is located in from the number
eight.
When naming the anion, the ending portion of the name (such as –ine) is removed and –ide is
added.
Nonmetal
Anion
Name of Anion
Fluorine
F-
Fluoride
Chlorine
Cl-
Chloride
Bromine
Br-
Bromide
Iodine
I-
Iodide
Oxygen
O2-
Oxide
Sulfur
S2-
Sulfide
Nitrogen
N3-
Nitride
Phosphorus
P3-
Phosphide
Prefixes
1
mono
2
di
3
tri
4
tetra
5
penta
6
hexa
7
hepta
8
octa
9
nona
10
deca
3 Naming systems:
1. Ionic Naming – Used when a metal or polyatomic cation and a nonmetal or polyatomic anion
bond. This system uses the charge of the ions to determine the name and/or formula.
2. Molecular Naming – Used when two nonmetals bond. This system uses prefixes to determine
the name and/or formula.
3. Acid Naming – Always starts formula with H and always has Acid in the name. Uses the
anion’s name to determine the name and/or formula.
Ionic Naming:
Used when a metal or polyatomic cation and a nonmetal or polyatomic anion bond. This system uses the
charge of the ions to determine the name and/or formula.
When given a formula: Say or write the cation’s name followed by a space and then the anion’s name.
When given a name: Write down each ion’s symbol including its charge. Use the numeric part of the cation’s
charge to tell how many anions you need (Cross charges). Use the numeric part of the anion’s charge to tell
how many cations you need. Reduce if possible to the lowest whole number ratio.
When a hydrate is present: Name or write the formula for the ionic compound just the same as you would
otherwise. Use the prefixes to determine the correct number of hydrates (waters) and write H2O if writing the
formula or prefix - “hydrate” if naming the compound.
Practice problems:
1) Ferrous oxide -FeO
6) CuO Cupric Oxide
2) Calcium fluoride CaF2
7)
3) Aluminum sulfide Al2S3
8) Hg2I2 Mercurous Iodide
13) CoO Cobaltous Oxide
4) Cobalt (II) bromide CoBr2
9) Sr3N2 Strontium Nitride
14) NiF2 Nickel (II) Fluoride
5) Chromic nitride CrN
10) PbS2 Plumbous Sulfide
15) CdO Cadmium Oxide
MgCl2 Magnesium Chloride
11) Sn3P2 Stannous Phosphide
12) Cr2S3 Chromic Sulfide
Polyatomic Ionic Compounds Practice Problems:
1) Zinc Nitrite Zn(NO3)2
4) Sn(BrO2)2 Stannous Bromite
2) Calcium Permanganate Ca(MnO4)2
5) Ag2CO3 Silver Carbonate
3) Iron (III) Carbonate Fe2(CO3)3
6) Al(NO3)3 Aluminum Nitrate
Hydrate Practice:
1) MgSO4· 7H2O Magnesium Sulfate
heptahydrate
5) Sodium carbonate monohydrate Na2CO3 ∙H2O
2) CuSO4 · 5H2O Cupric Sulfate pentahydrate
3) Pb(C2H3O2)2 · 3H2O Plumbous Acetate
Trihydrate
6) Potassium carbonate decahydrate K2CO3
∙10H2O
7) Ferric chloride hexahydrate FeCl3∙ 6H2O
4) MgCl2 · 6H2O Magnesium Chloride
hexahydrate
8) Barium chloride dihydrate
BaCl2∙ 2H2O
∙
Molecular Naming:
Used when two nonmetals bond. This system uses prefixes to determine the name and/or formula.
When given a formula: Say or write the prefix for the number of the first element present (if more than
one) followed by the first element’s name. Next write the prefix for the number of the second element
represented in the formula followed by the name of the second element as if it were an anion (see the chart
on page 3).
When given a name: Write down each ion’s symbol. Use the prefixes of each to tell how many you need.
Practice problems:
1) NO Nitrogen Monoxide
2) BI3 Boron triiodide
5) PCl4 Phosphorous
tetrachloride
9) Carbon monoxide CO
10) Diphosphorus pentaoxide
3) NO2
6) SeCl4
11) Carbon tetrafluoride
4) AsCl5
7) SBr6
12) Tetraphosphorus decaoxide
8) Dinitrogen monoxide
Acid Naming:
Always starts formula with H and always has Acid in the name. Use the anion’s name to determine the
name and/or formula.
1. Binary Acid – Starts with “H” and has no “O”
When given a formula: Always start with “hydro” then the name of the name of the element
minus its ending and add “ic”. Always add the word acid to the end.
When given a name: Write the symbol of the element referenced between “hydro” and “ic”.
Determine the charge it would have as an anion. Then write H and the number from the charge
before the symbol from the first step.
2. Oxy-Acid – Starts with “H” and has at least one “O”
When given a formula: Write the name of the anion (after the H). If it ends with “ate” replace
with “ic”. If it ends with “ite” replace with “ous”. End with the word Acid. Be careful with
sulfur and phosphorus anions because they gain a syllable.
When given a name: Write the formula of the anion referenced before acid. Remember if it
ends with “ic” replace with “ate”. If it ends with “ous” replace with “ite” Determine the
charge, then write H and the number from the charge before the symbol from the first step.
Practice problems:
1) HI
8) H3PO4
2) H2S
9) Hypochlorous Acid
3) HBr
10) Perchloric Acid
4) Hydrochloric Acid
11) Carbonic Acid
5) Hydrofluoric Acid
12) Nitrous Acid
6) H2SO4
7) HNO3