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JEE Main levelSingle correct optionDifficulty 2 of 3pb060

The in-plane C--C bond length in graphite (about 141.5 pm) is shorter than the C--C bond length in diamond (about 154 pm). The best explanation is that

  1. Aeach carbon in graphite uses all four valence electrons in sigma bonds
  2. Bgraphite has weaker van der Waals forces between the layers, which pull the atoms closer within a layer
  3. Cthe in-plane bonds in graphite have partial double-bond character because of the delocalised electrons
  4. Dcarbon in graphite is hybridised and so forms shorter bonds

Answer: C

In graphite the carbons are hybridised and the remaining electrons give a delocalised system. The bond order is therefore about 1.33, which shortens the bond relative to the pure single bond of diamond. The interlayer forces do not affect the in-plane distance.
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