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 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 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 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.
Explanation:
The bond energy refers to the amount of energy required to break a chemical bond between two atoms. In the case of carbon and oxygen, a single bond (C–O) has a bond energy of 358 kilojoules per mole, while a double bond (C=O) has a higher bond energy of 745 kilojoules per mole.
When atoms form multiple bonds with each other, such as a double bond, there are more shared electrons between the atoms. These additional shared electrons create stronger electrostatic attractions, making it more difficult to break the bond. Therefore, it requires more energy to break a double bond compared to a single bond.
To determine the bond energy, experiments are typically conducted using spectroscopic techniques or based on thermodynamic principles. These experiments measure the energy changes in chemical reactions involving the breaking or formation of bonds. By comparing the energy changes for different types of bonds, scientists determine the bond energies.