Chapter 5 - Ionic Bonding

Also known as a ‘salt’; a compound made up of a metal and a non-metal.

A rule which states that atoms are most stable with 8 electrons in their outer shell, and try to lose/gain electrons to achieve this.

A substance created from a regular lattice. Example: salt crystals.

Hard, but breaks easily under stress.

The measure of how easily something evaporates. Low volatility = doesn’t evaporate.

Brittle, low volatility, high melting/boiling points, don’t conduct as solids, do conduct as liquids.

An ion made up of more than one type of element. For example: ammonium (NH4+)

A set of chemically identical atoms or molecules. For example: H H H H H.

A state of matter in which a substance is dissolved in water.

A hard and brittle ionic compound made of clay, used in pots or bowls.

The process of a solid or liquid solute being distributed evenly throughout a solvent, forming a solution.

An ionic substance that can be dissolved, such as sodium chloride (NaCl).

The overall electric charge on an atom. E.g. an atom that has gained 1 electron has a valency of 1-.

Chemical bonding between a metal and a non-metal, such as sodium and chloride. Involves the metal atom donating an electron to the non-metal, forming ions with an electrostatic attraction between them; results in an ionic lattice.

A regular arrangement of cations and anions, joined together by electrostatic attraction.

An insoluble compound formed from two soluble compounds.

A chemical reaction in which two soluble aqueous compounds react to form an insoluble precipitate.

The measure of how readily or easily a substance dissolves in water.

Ions that do not undergo a chemical change in a reaction. For example, potassium or sodium.

A rule stating that sodium, nitrate, ammonium, potassium and ethanoate ions are always soluble in water.