1. principles of chemistry

ionic bonding

electrostatic attraction between two oppositely charged ions

covalent bonding

formed between two non-metal atoms by sharing a pair of electrons to fill in the outer shell

ionic lattices

strong electrostatic forces between oppsitely charged ions, cannot conduct unless molten and in aqueous solution - solid: fixed position, with regular repeating pattern

giant covalent lattices

• do not conduct except graphite

• insoluble

• high melting and boling points

diamond

• each carbon atom joined to 4 other carbon atoms

graphite

giant structure; each carbon is covalently bonded to 3 other carbons, forming layers of hexagonal rings,

• conduct electricity because each carbon atom bonded to 3 other carbon atoms

• weak IMFs between layers

C60

SIMPLE molecular structure (not giant like graphite and diamond)

• weak intermolecular forces of attraction between them which take little energy to overcome. Hence C₆₀ fullerene has a low melting point, and it is soft

• covalently bonded to 3 others and the other electrons are delocalised, these electrons cannot jump between different molecules.

isotope

same proton number, different neutron number