Studied by 7 people
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?
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