ionic, covalent and metallic bonding

Ionic Bonding

The electrostatic attraction between oppositely charged ions formed by the full transfer of one or more electrons from a metal atom to a non-metal atom.

Covalent Bonding

A chemical bond that involves the sharing of electron pairs between atoms, typically occurring between non-metal atoms to achieve a stable electron configuration.

Metallic Bonding

The electrostatic attraction between a lattice of positive metal ions and a 'sea' of delocalized valence electrons that are free to move throughout the structure.

Properties of Ionic Compounds

1. High melting and boiling points due to strong electrostatic forces.
2. Conduct electricity when molten or in aqueous solution, but not as solids.
3. Brittle crystalline structures.

Properties of Covalent Compounds

1. Low melting and boiling points (for simple molecular substances) due to weak intermolecular forces.
2. Poor electrical conductivity as they do not have free-moving ions or electrons.
3. Often exist as gases or liquids at room temperature.

Properties of Metallic Substances

1. High electrical and thermal conductivity due to delocalized electrons.
2. Malleable and ductile because layers of ions can slide over each other without breaking the bond.
3. Lustrous appearance.

Electronegativity Difference in Bonding

1. Ionic: Large difference (\Delta\chi > 1.7).
2. Polar Covalent: Moderate difference (0.5 < \Delta\chi < 1.7).
3. Non-polar Covalent: Small to no difference (\Delta\chi < 0.5).