Question

C-C bond length in graphite is shorter than
C-C bond length in diamond - explain.​

Answer 1

Explanation:

Thus, it is found that the carbon-carbon bond diamond has the maximum bond length. However, in graphite, C60 or C70 the carbon is sp2 hybridized. Here, s character is found to be equal to 330/0 , which is greater than the diamond. Thus, for graphite, C60 or C70 the bond length is less than that of the diamond.

Graphite has carbon in sp2 hybrid state (33.3 % s character) but diamond has carbon in sp3 hybrid state (25 % s characrer). More is the percentage of s characters, (by Bent rule) more is the bond multiplicity and hence, shorter the bond is. ... Hence, C-C bond length in graphite is shorter than than in diamond.

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Answer 2

Answer:

Hi there...Here is your answer.

Graphite is sp2 hybridised and C-C bond involves sp2-sp2 hybrid carbons.

Diamond is sp3 hybridised and C-C bond involves sp3-sp3 hybrid carbons. Moreover, greater the s-character in hybridised atom, the smaller is the size of hybridised orbital and greater is the overlapping (hence shorter is the bond length).

Therefore, s-character in sp2 orbital is more than that in sp3 orbital.

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