chem

Metallic Bonding

Occurs between only metals; involves atoms losing valence electrons to form metal cations.

Delocalised Electrons

Valence electrons that are freed to move around in the 3D lattice of metal cations.

Properties of Metals

Includes luster, conductivity (heat and electricity), malleability, ductility, and typically high density.

Ionic Compounds

Compounds formed from positive and negative ions bonded by a strong electrostatic force.

Melting Temperature of Ionic Compounds

Very high melting points due to the strong electrostatic forces in a 3D giant ionic lattice.

Hardness of Ionic Compounds

Hard because ions are held tightly in a rigid, fixed structure.

Brittleness of Ionic Compounds

Brittle due to structure; when force is applied, similar charges repel and cause shattering.

Electrical Conductivity of Ionic Solids

Do not conduct electricity as solids because ions are fixed in place.

Electrical Conductivity of Ionic Solutions

Conduct electricity when dissolved or melted as ions are free to move.

Ionic Bonding

Formed between non-metals and metals when electrons are transferred from one atom to another.

Cations

Atoms that lose electrons and become positively charged.

Anions

Atoms that gain electrons and become negatively charged.

Polyatomic Ion

A charged species composed of two or more atoms bonded together.

Covalent Bonding

A shared pair of electrons between atoms of non-metals.

Diatomic Molecules

Atoms of the same element that share a covalent bond.

Lone Pair

A pair of electrons not involved in bonding.

Giant Covalent Bonding

Very strong bonding that creates substances with high melting and boiling points.