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NEET CHEMISTRYMedium

The correct order of increasing bond length of C-H\text{C-H}, C-O\text{C-O}, C-C\text{C-C} and C=C\text{C=C} is:

A

C-C<C=C<C-O<C-H\text{C-C} < \text{C=C} < \text{C-O} < \text{C-H}

B

C-O<C-H<C-C<C=C\text{C-O} < \text{C-H} < \text{C-C} < \text{C=C}

C

C-H<C-O<C-C<C=C\text{C-H} < \text{C-O} < \text{C-C} < \text{C=C}

D

C-H<C=C<C-O<C-C\text{C-H} < \text{C=C} < \text{C-O} < \text{C-C}

Step-by-Step Solution

Bond length is determined by the size of the bonded atoms and the multiplicity of the bond.

  1. C-H\text{C-H}: Hydrogen is the smallest atom, resulting in the shortest bond length (107 pm107\text{ pm}).
  2. C=C\text{C=C}: A double bond is shorter than a single bond due to greater orbital overlap and stronger attraction pulling the nuclei closer together (133 pm133\text{ pm}).
  3. C-O\text{C-O}: Oxygen has a smaller atomic radius than carbon, making the C-O\text{C-O} single bond (143 pm143\text{ pm}) shorter than a C-C\text{C-C} single bond.
  4. C-C\text{C-C}: A single bond between two carbon atoms has the longest bond length among these choices (154 pm154\text{ pm}). Therefore, the correct increasing order of bond lengths is C-H<C=C<C-O<C-C\text{C-H} < \text{C=C} < \text{C-O} < \text{C-C}.
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