Question

The bond energy between carbon and oxygen is 358 for a single bond (C–O) and 745 for a double bond (C=O). Why is the bond energy higher for double-bonded carbon and oxygen (C=O)?
A. Additional bonds require less energy to break, so the bond energy is higher.

B. Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy.

C. Additional electrons repel each other, increasing the distance between atoms, and increasing bond energy.

D. Additional bonds require more energy to break, so the bond energy is higher.

Answer 1

This problem is providing the bond energy for the bonds C-O and C=O which are 358 and 745 respectively, so that a feasible explanation to this behavior is required. At the end, one concludes the correct answer is C. "additional electrons repel each other, increasing the distance between atoms, and increasing bond energy" according to the following:

Bond energy:

In chemistry, we study the bond energy as the energy required to break the bond, binding two elements. In such a way, we can evidence that the more bonds between the atoms, the higher the bond energy such as in the case of C-O and C=O.

In such a way, since bonds are formed between valence electrons, we see that the more of these an atom has available for bonding, the farther away they will be, as they are repelled; thus, causing more distance between atoms and making the bond to be longer.

Hence, the greater the distance between two atoms in a bond, the higher the bond energy; that's why the answer to this question is C. Additional electrons repel each other, increasing the distance between atoms, and increasing bond energy.

Learn more about bond lengths: brainly.com/question/13683866