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Chapter 1: Problem 10

The six carbon atoms in a benzene molecule are shown in different resonance forms as three single bonds and three double bonds. If the length of a single carbon-carbon bond is 154 pm and the length of a double of a single carbon bond is \(133 \mathrm{pm},\) what length would be expected for the carbon-carbon bonds in benzene? (A) 126 \(\mathrm{pm}\) (B) 133 \(\mathrm{pm}\) (C) 140 \(\mathrm{pm}\) (D) 154 \(\mathrm{pm}\)

Short Answer

Expert verified
The expected length for the carbon-carbon bonds in benzene would be closest to 140pm (Option C).

Step by step solution

01

Understand the resonance in benzene

Benzene has a resonance structure, meaning it exists in two forms interchangeably which have three single and three double bonds each. These do not exist independently rather they hybridize and form the actual structure of benzene. The bond length in benzene will thus be an average of that in single and double bond.
02

Calculate the average bond length

As benzene exists in two resonance structures, we take a simple average of the lengths of single and double bond. The formula for average is (sum of quantities)/number of quantities. \(Average bond length = \frac{(154pm + 133pm)}{2} = 143.5pm\)
03

Compare with given options

The calculated average bond length does not match exactly with any of the given options. However, we should choose the value closest to our calculated value. In this case, the closest given value is 140pm (C)

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Most popular questions from this chapter

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