Why silicon does not form an analogue of graphite?
Or
Why elemental silicon does not form graphite like structure as carbon does?

In graphite, carbon is sp² hybridised and each carbon is thus linked to three other carbon atoms forming hexagonal rings and also it involves the formation of pi-pi double bonds. On the other hand, the size of a silicon atom is larger than carbon and hence silicon has no tendency to undergo sp² or sp hybridization to form multiple bonds between themselves or with other atoms such as oxygen, nitrogen (for example Si = 0, Si = N). Therefore, silicon always undergoes sp² hybridization and hence all the silicon compounds have tetrahedral geometry. Also, silicon has a lesser tendency for catenation than carbon because Si – Si bonds are much weaker than C – C bonds.