Multiple Choice
In a Lewis dot structure of ethene (C_2H_4), which arrows would point to electrons involved in a pi bond?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Sigma & Pi Bonds
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Which has greater bond strength between the carbon–carbon bond.
C2Cl2 vs. C2Cl6
A
C2Cl2
B
C2Cl6
Verified step by step guidance1
First, understand the types of carbon-carbon bonds present in each molecule. C2Cl2 has a triple bond between the carbon atoms, while C2Cl6 has single bonds between the carbon atoms.
Recall that bond strength is related to the type of bond: triple bonds are stronger than double bonds, which are stronger than single bonds. This is due to the number of shared electron pairs between the atoms.
Consider the molecular structure: C2Cl2, known as dichloroacetylene, has a carbon-carbon triple bond, which involves three shared pairs of electrons, making it very strong.
In contrast, C2Cl6, known as hexachloroethane, has carbon-carbon single bonds, which involve only one shared pair of electrons, making them weaker compared to triple bonds.
Conclude that the bond strength is greater in C2Cl2 due to the presence of the carbon-carbon triple bond, which is inherently stronger than the single bonds found in C2Cl6.
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