Allotropes of Carbon - Diamond and Graphite

allotrope

different structural forms of the same element in the same physical state

giant covalent structures

diamond & graphite - made of a regular lattice of covalently bonded atoms - very strong

each carbon atom in diamond

each carbon atom is covalently bonded to 4 other carbon atoms (maximum covalent bonds a carbon atom can make) - regular 3D pattern

diamond properties

each of its covalent bonds is very strong, it would take loads of energy to break them -> diamond is very strong + has a very high melting point

diamond electricity

doesn't conduct electricity as it has no free electrons or ions that can move around

each carbon atom in graphite

each carbon atom is bonded to 3 other carbon atoms

atoms arrangement in graphite

atoms arranged into hexagons that together form large flat sheets - then arranged on top of another to form lots of layers

graphite properties

the layers on top of one another are held together weakly as there are no covalent bonds between them - free to slide over one another - soft

graphite properties

very high melting point - individual layers are strongly held together by covalent bonds

graphite electricity

because in graphite each carbon atom makes 3 covalent bonds, each carbon atom has one spare electron that is not used in bonding (delocalised - free to move around) - allow graphite to conduct electricity + heat