Mark the correct statement(s)about graphite and diamond.

see full answer

Your Exam Success, Personally Taken Care Of

1:1 expert mentors customize learning to your strength and weaknesses – so you score higher in school , IIT JEE and NEET entrance exams.

An Intiative by Sri Chaitanya

Graphite uses $s p^{2}$ hybrid orbitals and diamond uses $s p^{3}$ hybrid orbitals in bonding

Both are insulators

Graphite is thermodynamically more stable

The graphite hexagonal layers can slide over one another and thus used as lubricant while diamond is hard as it has 3-dimensional structure.

answer is A, B, D.

(Unlock A.I Detailed Solution for FREE)

Best Courses for You

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

(a) Graphite uses three electrons in bonding with ${sp}^{2}$ hybrid orbitals and fourth electron is delocalized in $π -$ bonding. Thus, graphite is conducting.

Diamond uses four electrons in bonding with $s p^{3}$ hybrid orbitals and thus non-conducting. Thus, correct

(b) Graphite consists of planer hexagonal layers of C-atoms held together by weak van der waals’ forces. Layers can slide over one another. This makes graphite a lubricant and slippery. Thus correct.

(d) Diamond 0 $\overset{Δ}{\to}$ Graphite. Thus, graphite is thermodynamically more stable than diamond.

Watch 3-min video & get full concept clarity