Question

question 8
1 pts
which of the following statements is true about single, double, and triple covalent bonds?
a. triple bonds have the longest bond length and highest bond energy.
b. double bonds have higher bond energy but shorter bond length than single bonds.
c. single bonds have the shortest bond length and highest bond energy.
d. bond energy decreases as the number of shared electron pairs increases.

Explanation:

• Bond length: As the number of shared electron pairs (i.e., bond order) increases, the bond length decreases. So, triple bonds (bond order = 3) are shorter than double bonds (bond order = 2), which are shorter than single bonds (bond order = 1).
• Bond energy: As the number of shared electron pairs increases, more energy is required to break the bond. So, triple bonds have higher bond energy than double bonds, which have higher bond energy than single bonds.
• Option A: Triple bonds have the shortest bond length (not the longest) and highest bond energy. So, this option is incorrect.
• Option B: Double bonds (bond order = 2) have higher bond energy (more energy to break) and shorter bond length (compared to single bonds, bond order = 1). This option is correct.
• Option C: Single bonds have the longest bond length (not the shortest) and lowest bond energy (not the highest). So, this option is incorrect.
• Option D: Bond energy increases as the number of shared electron pairs increases. So, this option is incorrect.

Answer:

B. Double bonds have higher bond energy but shorter bond length than single bonds.