Question

Graphite is a much better conductor of heat and electricity than diamond. This is due to the fact that each carbon atom in graphite:

• A. undergoes $s{p}^2$ hybridization and forms three sigma bonds with three neighbouring carbon atoms
• B. undergoes $sp$ hybridization
• C. is tetrahedrally bonded
• D. is free from van der Waals force

Answer 1

The correct option is A undergoes $s{p}^2$ hybridization and forms three sigma bonds with three neighbouring carbon atoms

A carbon atom can bind up to 4 other atoms around it. However, in graphite each carbon atom only bonds to 3 others around it- this means there is an electron spare which becomes 'delocalized'.

This means that it is donated to form a common pool of electrons which can flow through the molecule carrying a charge and so conduct electricity.