Consider the following statements regarding allotropes of carbon: 1. Graphite is a good conductor of electricity due to the presence of delocalized free electrons in its layered planar structure. 2. Diamond is an exceptional thermal conductor and electrical insulator due to its rigid three-dimensional tetrahedral sp3 hybridized covalent network. Which of the statements given above is/are correct?

💡 Solution & Explanation

Carbon exhibits allotropy with graphite and diamond being the most prominent crystalline forms. Graphite features sp2 hybridized carbon atoms arranged in hexagonal sheets held by weak van der Waals forces, allowing one unbonded electron per atom to move freely and conduct electricity. Diamond features sp3 hybridized carbon atoms bonded tetrahedrally, making it extremely hard and an electrical insulator while conducting heat exceptionally well through lattice vibrations.