`N_(2)` is less reactive than `CN^(-)` due to

Options

A. Presence of more electrons in orbitals
B. Absence of dipole moment
C. Difference in spin quantum no
D. A trpile bond between nitrogen atoms

Answer

To determine why \( N_2 \) is less reactive than \( CN^- \), we can analyze the molecular structure and properties of both species step by step.

### Step 1: Analyze the molecular structure of \( N_2 \)
- \( N_2 \) consists of two nitrogen atoms connected by a triple bond, represented as \( N \equiv N \).
- This molecule is non-polar because the two nitrogen atoms have the same electronegativity, resulting in no charge separation.

### Step 2: Analyze the molecular structure of \( CN^- \)
- \( CN^- \) (cyanide ion) also has a triple bond between carbon and nitrogen, represented as \( C \equiv N \).
- However, the cyanide ion carries a negative charge, which introduces a dipole moment due to the difference in electronegativity between carbon and nitrogen.

### Step 3: Compare the dipole moments
- The dipole moment of \( N_2 \) is zero because it is non-polar.
- The dipole moment of \( CN^- \) is non-zero due to the presence of the negative charge, making it a polar molecule.

### Step 4: Relate polarity to reactivity
- Reactivity in chemical species is often influenced by polarity. Polar molecules tend to be more reactive because they can interact with other charged or polar species.
- Since \( N_2 \) is non-polar and has a dipole moment of zero, it is less reactive compared to the polar \( CN^- \).

### Step 5: Conclusion
- The primary reason \( N_2 \) is less reactive than \( CN^- \) is the absence of a dipole moment in \( N_2 \). The lack of polarity means \( N_2 \) does not readily engage in chemical reactions, while the polar \( CN^- \) can react due to its charge.

### Final Answer
\( N_2 \) is less reactive than \( CN^- \) due to the absence of a dipole moment in \( N_2 \).

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