Naming Ionic Compounds

Cation

A positively charged ion that results from losing one or more electrons.

Anion

A negatively charged ion that forms when an atom gains one or more electrons.

Ionic compound

A compound formed by the electrostatic attraction between cations and anions.

Group 1 elements

Elements that lose one electron to form cations with a charge of 1+.

Halogens

Elements in group 17 that tend to gain one electron to become anions with a charge of 1-.

Copper (I) ion

Also known as cuprous ion; a copper ion with a charge of 1+.

Copper (II) ion

Also known as cupric ion; a copper ion with a charge of 2+.

Oxidation state

The charge of an ion that indicates its loss or gain of electrons.

Polyatomic ion

An ion composed of two or more atoms that can be positively or negatively charged.

Sulfate ion

A polyatomic ion with the formula SO4^2-.

Nitrate ion

A polyatomic ion with the formula NO3^-.

Chlorate ion

A polyatomic ion with the formula ClO3^-.

Chlorite ion

A polyatomic ion with the formula ClO2^-.

Hypochlorite ion

A polyatomic ion with the formula ClO^-.

Perchlorate ion

A polyatomic ion with the formula ClO4^-.

Binary covalent compound

A compound composed of two different nonmetal elements.

Prefix 'mono-'

Used in naming covalent compounds to denote one atom of an element.

Suffix '-ide'

Used for monatomic anions, indicating that they are derived from a single element.

Roman numerals in chemical naming

Used to indicate the oxidation state of transition metals in compounds.

Ratios of ions in ionic compounds

Determined by the need for the total charge to equal zero.

Magnesium chloride

An ionic compound formed from magnesium ions (2+) and chloride ions (1-).