Answer
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Work Step by Step
The bond energy in CO (1072 kJ/mol) is higher than the bond energy in $N_{2}$ (945 kJ/mol), indicating that the CO bond is stronger.
However, CO is considerably more reactive than $N_{2}$. This can be explained by the polarity of the CO molecule.
The difference in electronegativity between carbon (2.55) and oxygen (3.44) results in a significant polarity in the CO molecule, with the oxygen atom bearing a partial negative charge and the carbon atom bearing a partial positive charge. This polarity makes the CO molecule more reactive, as the partial charges can interact with other molecules or ions, facilitating various chemical reactions.
In contrast, the $N_{2}$ molecule is non-polar, as the electronegativity difference between the two nitrogen atoms is negligible. The lack of polarity in the $N_{2}$ molecule makes it less reactive compared to the polar CO molecule, despite the $N_{2}$ bond being weaker.
The polarity of the CO molecule allows it to participate in a wider range of chemical reactions, such as acid-base reactions, coordination reactions, and redox reactions, making it more reactive than the non-polar $N_{2}$ molecule.
