bondings revised
simple covalent
giant lattice covalent
ionic bonding
they have strong intra molecular forces
they have weak intermolecular forces
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Low melting and boiling point, so often liquid or gas at room temp (usually gas)
can be presented using a dot cross diagram
graphite (carbon)
has 3 bondings, with 1 free delocalised electron, which therefore allows it to conduct electricity. Has a layered hexagonal structure, and the weak intermolecular forces between the layers allow layers to slide over others with ease. Hence why graphite is used in pencils, leaving a layer of graphite on the paper
Diamond (carbon)
has 4 bondings, therefore making it rather strong, with a high bonding point
silica - silicon has six bondings with oxygen, and oxygen has two bondings with silicon.
bondings between metal and non-metal
in aqueous solution or molten, they can conduct electricity, due to free moving ions
is a strong forces of electrostatic attraction between oppositely charged ions
e.g. sodium chloride
Due to this they have strong intermolecular bondings
this makes it harder to break the bonds, giving them a high melting and boiling point
allowing them to be separated through the process of electrolysis