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)?
Additional electrons repel each other, increasing the distance between atoms, and increasing bond energy
Additional bonds require less energy to break, so the bond energy is higher
Additional bonds require more energy to break, so the bond energy is higher
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy
Additional electrons repel each other, increasing the distance between atoms, and increasing bond energy
Additional bonds require less energy to break, so the bond energy is higher
Additional bonds require more energy to break, so the bond energy is higher
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy
Answers
GPT-4o mini
The correct answer is:
**Additional bonds require more energy to break, so the bond energy is higher.**
Double bonds involve sharing two pairs of electrons between the two atoms, which results in a stronger attraction between the atoms compared to a single bond, where only one pair of electrons is shared. This greater attraction means that it requires more energy to break a double bond than a single bond, resulting in a higher bond energy for C=O compared to C-O.
**Additional bonds require more energy to break, so the bond energy is higher.**
Double bonds involve sharing two pairs of electrons between the two atoms, which results in a stronger attraction between the atoms compared to a single bond, where only one pair of electrons is shared. This greater attraction means that it requires more energy to break a double bond than a single bond, resulting in a higher bond energy for C=O compared to C-O.