General Chemistry: Chapter 2 (Naming Ionic Compounds)

H⁺

Hydrogen

Li⁺

Lithium

Na⁺

Sodium

K⁺

Potassium

Cs⁺

Cesium

Ag⁺

Silver

Mg²⁺

Magnesium

Ca²⁺

Calcium

Sr²⁺

Strontium

Ba²⁺

Barium

Zn²⁺

Zinc

Cd²⁺

Cadmium

Al³⁺

Aluminum

H⁻

Hydride

F⁻

Fluoride

Cl⁻

Chloride

Br⁻

Bromide

I⁻

Iodide

O²⁻

Oxide

S²⁻

Sulfide

N³⁻

Nitride

NH₄⁺

Ammonium

H₃O⁺

Hydronium

CH₃COO⁻ or C₂H₃O₂⁻

Acetate

CN⁻

Cyanide

OH⁻

Hydroxide

ClO⁻

Hypochlorite

ClO₂⁻

Chlorite

ClO₃⁻

Chlorate

ClO₄⁻

Perchlorate

NO₂⁻

Nitrite

NO₃⁻

Nitrate

MnO₄⁻

Permanganate

CO₃²⁻

Carbonate

HCO₃⁻

Hydrogen Carbonate or Bicarbonate

CrO₄²⁻

Chromate

Cr₂O₇²⁻

Dichromate

O₂²⁻

Peroxide

PO₄³⁻

Phosphate

HPO₄²⁻

Hydrogen Phosphate

H₂PO₄⁻

Dihydrogen Phosphate

SO₃²⁻

Sulfite

SO₄²⁻

Sulfate

HSO₄⁻

Hydrogen Sulfate or Bisulfate

mono-

1

di-

2

tri-

3

tetra-

4

penta-

5

hexa-

6

hepta-

7

octa-

8

nona-

9

deca-

10

TRANSITION METAL Ionic Compounds

Must specify the charges.

(indicate by Roman Numerals)

Example: Iron (II) Chloride