Bonding

So that the atoms can achieve a more stable electron arrangement, often a full outer energy level, like noble gases.

A chemical bond in which electron(s) are transferred from one atom to another, resulting in the formation of oppositely charge ions with electrostatic forces of attraction between them.

A chemical bond in which outer electrons are delocalised within the lattice of metal ions.

A chemical bond in which a pair of electrons are shared between two atoms.

Always solid at room temperature, have giant structures so high melting points, conduct electricity when molten or dissolved in water, are brittle.

When they receive a sharp blow, the ions may move and contact with another ion of a like charge which repels it and the structure shatters.

At room temperature they are gases, liquids or solids with low melting points. Poor conductors of electricity.

Good conductors of electricity. Good conductors of heat. Malleable and ductile. High melting point.

Where both the electron in the covalent bond come from one of the atoms in the bond.

Each pair of electrons will repel all other electron pairs and will therefore take up positions as far apart as possible to minimise repulsion

Linear, 180

Trigonal planar, 120

Bent (still planar), 118

Tetrahedral, 109.5

Trigonal pyramid (lone pair at top), 107

V-shaped (on plane), 104.5

Trigonal bipyramid (trigonal planar with one atom above and below), 90 and 120

Trigonal planar (with one lone pair above and below), 120. Or t-shape (lone pairs on same plane), 89

Octahedral, 90

Square pyramid (with one lone pair below), 89

Square planar (with one lone pair above and below), 90

The power of an atom to attract the electron density in a covalent bond towards itself.

The nuclear charge, the atomic radius, the shielding

It decreases as the atoms get bigger and there are more electron shells for shielding.