C2 Summary 

Ionic Bonding

Atoms gain or lose electrons to form ions

Happens between a metal and non-metal

Metal loses electron as non-metal gains them

Reactions with water very vigorous hydrogen produced fizzing

Reactions with chlorine from white metal chloride salts

Reactions with oxygen form metal oxide

Ionic Compounds

Giant ionic structure

Regular lattice structure

High melting and boiling points

Strong forces of electrostatic attraction between oppositely charged ions in all directions

Can’t conduct electricity

If in liquid form can carry and electrical current

Covalent Bonding

Between two non-metals

Sharing of electrons

Simple Molecular Substances

Oxygen, Water, Methane, Hydrogen, Chlorine, Hydrogen Chloride

Strong covalent bonds between atoms

High melting and boiling points as molecules increase in size

Weak intermolecular forces between molecules

Don’t conduct electricity

Polymers

Repeating long chains of monomers

Allotropes off Carbon

Diamond is hard as has 4 covalent bonds

High melting and boiling point

Strong covalent bonds

Can’t conduct electricity as no delocalised electrons

Graphite is covalently bonded 3 times in hexagon shapes

Each layer isn’t bonded to the other

Soft and slippery lubricant

Delocalised electron so can carry an electrical charge

High melting point

Graphene is one layer of graphite

Very strong and lightweight

Strong covalent bonds so lots of energy needed to overcome them

Delocalised electrons

Metallic Bonding

Between 2 metals

Different sized ions distort the layers making them harder and stronger