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)?(1 point)
Responses
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy.
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy.
Additional bonds require less energy to break, so the bond energy is higher.
Additional bonds require less energy to break, so the bond energy is higher.
Additional electrons repel each other, increasing 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 more energy to break, so the bond energy is higher.
Responses
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy.
Additional electrons attract each other, decreasing the distance between atoms, and increasing bond energy.
Additional bonds require less energy to break, so the bond energy is higher.
Additional bonds require less energy to break, so the bond energy is higher.
Additional electrons repel each other, increasing 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 more energy to break, so the bond energy is higher.
Answers
GPT-4o mini
The correct response is:
**Additional bonds require more energy to break, so the bond energy is higher.**
This explains that double bonds (C=O) involve additional shared electron pairs compared to single bonds (C–O), resulting in a stronger attraction between the nuclei of the bonded atoms and the shared electrons. Consequently, more energy is needed to break the double bond compared to a single bond, which is why the bond energy is higher for double-bonded carbon and oxygen.
**Additional bonds require more energy to break, so the bond energy is higher.**
This explains that double bonds (C=O) involve additional shared electron pairs compared to single bonds (C–O), resulting in a stronger attraction between the nuclei of the bonded atoms and the shared electrons. Consequently, more energy is needed to break the double bond compared to a single bond, which is why the bond energy is higher for double-bonded carbon and oxygen.