Question

Which choice has the bonds listed in the order of increasing bond energy?

a) HF < HCl < HBr
b) C-O < C=O < C≡O
c) F₂ < Cl₂ < Br₂
d) N₂ < C-C bond in C₂H₄ < C-C bond in C_2H_6
e) All the same

Answer 1

The bonds listed in the order of increasing bond energy is (b) C-O < C=O < C≡O, reflecting the increasing bond strengths from single to triple bonds.

Step-by-step explanation:

The choice that has the bonds listed in the order of increasing bond energy is (b) C-O < C=O < C≡O. Bond energy generally increases with the number of bonds between two atoms, which means a single bond has less energy than a double bond, which in turn has less energy than a triple bond. This trend is due to the increasing overlap of atomic orbitals and the greater electron density between the two bonded atoms.

In this scenario, a single C-O bond is weaker than the double C=O bond, which is weaker than the triple C≡O bond. This pattern is consistent with the known strengths of covalent bonds and can also be associated with the lengths of these bonds, where shorter bonds are typically stronger due to better orbital overlap.

Answer 2

The choice with bonds listed in order of increasing bond energy is (b) C-O < C=O < C≡O, as bonds with more shared electrons (double, triple bonds) have higher bond energy than single bonds.

The right answer is d) N₂ < C-C bond in C₂H₄ < C-C bond in C₂H₆

Step-by-step explanation:

The question asks about the order of bond energy for various bonds. The correct choice that has bonds listed in order of increasing bond energy is (b) C-O < C=O < C≡O, since single, double, and triple carbon-oxygen bonds have increasing bond energy respectively.

The bond energy increases with the number of shared electrons in the bond, meaning that a single bond (C-O) has fewer shared electrons and thus less bond energy compared to a double bond (C=O), which in turn has less bond energy than a triple bond (C≡O).

The right answer is d) N₂ < C-C bond in C₂H₄ < C-C bond in C₂H₆