Which of the following bonds has the highest bond energy (is the strongest)?

• A. N≡N (nitrogen triple bond)
• B. O=O (oxygen double bond)
• C. H–H (hydrogen single bond)
• D. Cl–Cl (chlorine single bond)

Answer: (A)

Verified step by step guidance

1. Understand that bond energy refers to the amount of energy required to break one mole of a particular bond in the gas phase. Generally, the more bonds between two atoms, the stronger and higher the bond energy.
2. Recall the types of bonds in the options: N≡N is a triple bond, O=O is a double bond, and H–H and Cl–Cl are single bonds. Multiple bonds (double and triple) involve more shared electrons and stronger attractions.
3. Recognize that a triple bond (N≡N) involves three shared pairs of electrons, making it stronger and requiring more energy to break compared to double or single bonds.
4. Consider the bond energies trend: triple bonds > double bonds > single bonds, and also take into account the atoms involved, as smaller atoms with multiple bonds tend to have stronger bonds due to shorter bond lengths.
5. Conclude that among the given options, the nitrogen triple bond (N≡N) has the highest bond energy because it is a strong triple bond between small atoms, making it the strongest bond listed.