Question

Which carbon compound is soft, slippery, a decent electricity conductor, and bonded in a way that forms planes?

coal
petroleum
graphite

Answer 1

The correct answer is option C, Graphite

Step-by-step explanation:

The structure of graphite is a covalent structure in which one carbon atom is bonded to three other carbon atoms and that too through a covalent bond. Due to this arrangement there is one non bonded electron with each carbon atom which makes graphite a good conductor. The overall structure of graphite consists of several bonded set of carbon molecules (hexagonal structure) to form sheets of carbon which lie over each other. The layer of graphite slip over each other as they are bonded by weak forces and thus it is soft and slippery.

Answer 2

Graphite is correct answer. Graphite is allotrop of carbon and has sp2 hybridization. Carbon in graphite form single bonds, angles between bond are 120°.