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The correct order of increasing bond length of C–H, C–O, C–C and C=C is
A
C–H < C–O < C–C < C=C
B
C–H < C=C < C–O < C–C
C
C–C < C=C < C–O < C–H
D
C–O < C–H < C–C < C=C
Detailed Solution
Typical bond lengths: C–H = 107 pm, C=C = 133 pm, C–O = 143 pm, C–C = 154 pm.
C–H is the shortest because hydrogen is the smallest atom.
A double bond is shorter than a single bond, so C=C is shorter than both C–O and C–C.
Oxygen is smaller than carbon, so C–O is shorter than C–C.
Increasing order of bond length: C–H < C=C < C–O < C–C
C–H is the shortest because hydrogen is the smallest atom.
A double bond is shorter than a single bond, so C=C is shorter than both C–O and C–C.
Oxygen is smaller than carbon, so C–O is shorter than C–C.
Increasing order of bond length: C–H < C=C < C–O < C–C