Bonding chemistry

Ionic bonding

Metals + non metals

Attractive forces between oppositely charged ions

Covalent bonding

Non metals

Atoms share pairs of electrons

Metallic bonding

Metals

Attractive forces between positive ions and delocalised electrons

What are polymers?

Large molecules

Atoms linked together with strong covalent bonds

Giant covalent compounds/structures

Diamond

Graphite

Graphene

Silicon dioxide

Diamond

4 bonds per carbon atom

Covalent bonds (hard to break, requires a lot of energy)

Covalent bonds means that diamond is very hard, high melting point, does not conduct electricity (no free electrons cannot conduct)

Graphite

3 bonds per carbon atom

Weak intermolecular forces between layers (broken easy)

Delocalised electrons move + conduct electricity

Layers of hexagons can slide over each other which makes graphite soft - used as a lubricant

Graphene

A single layer of graphite

Conducts electricity

Very strong

What is fullernes?

Hollow tubes or spheres of graphene

Used for nanotechnology, electronics and materials

State symbols

s = Solid

l = Liquid

g = Gas

aq = aqueous (solution forms when a substance dissolves in water)

What is a lattice?

Repeated pattern of either negative or positive ions

Giant ionic structure properties

Non metals + metals

High melting and boiling points

What bonding is present in silicon dioxide?

Giant covalent

What bonding is present in magnesium chloride?

Simple ionic

What bonding is present in h20?

Simple covalent

Simple molecules

Small and can be separated into individual units without breaking bonds.

Giant ionic + covalent structures

Form huge continuous networks of atoms that are bonded together, which cannot be seperated into individual units unless the bonds are broken.

Hi lol sam

w flashcards?