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 bonds require more energy to break, so the bond energy is higher.
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 electrons attract each other, decreasing the distance between atoms, and increasing bond energy.
The correct response is: Additional bonds require more energy to break, so the bond energy is higher.
To explain why this is the case, we need to understand the concept of bond energy. Bond energy refers to the amount of energy required to break a chemical bond, specifically the bond between two atoms.
In a single bond (C–O), there is one shared pair of electrons between the carbon and oxygen atoms. This bond requires a certain amount of energy to be broken.
In a double bond (C=O), there are two shared pairs of electrons between carbon and oxygen. The presence of the additional bond means that there are more electrons holding the carbon and oxygen atoms together. As a result, it requires more energy to break the bond.
Think of it like this: the additional bond provides more strength to hold the atoms together, and more strength means more energy is needed to overcome it and break the bond.
So, when comparing the bond energy between single-bonded carbon and oxygen (C–O) and double-bonded carbon and oxygen (C=O), the bond energy is higher for the double bond because it requires more energy to break.