Chemistry: Chemical Bonding and Structure - Day 2

Ionic Bonding

The electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions).

Key Points on Ionic Bonding

• Formed when metals lose electrons (cations) and non-metals gain electrons (anions).

• Example: Sodium (Na) loses one electron to become Na⁺; Chlorine (Cl) gains one electron to become Cl⁻.

• Properties: High melting and boiling points, conduct electricity when molten or dissolved in water.

Covalent Bonding

A bond formed by the sharing of pairs of electrons between atoms.

Key Points on Covalent Bonding

• Each shared pair of electrons constitutes one covalent bond.

• Example: In water (H₂O), oxygen shares electrons with two hydrogen atoms.

• Properties: Lower melting and boiling points compared to ionic compounds; do not conduct electricity.

Metallic Bonding

The electrostatic attraction between positively charged metal ions and a sea of delocalised electrons.

Key Points on Metallic Bonding

• Metals are good conductors of electricity and heat due to the movement of delocalised electrons.

• Properties: Malleable and ductile; high melting and boiling points.