Q3 / 150 · MHT CET 2026 (15 April Shift 2) · Chemistry
What type of bond and type of overlapping present in $\text{N}_2$ molecule ?
- ASingle bond and s$-$s overlap
- BDouble bond and s$-$p overlap
- Correct answerCTriple bond and p$-$p overlap
- DDouble bond and p$-$p overlap
Solution
The electronic configuration of a nitrogen atom is $1s^2 2s^2 2p^3$.
Each nitrogen atom has three half-filled $2p$ orbitals ($2p_x, 2p_y, 2p_z$). To achieve a stable octet configuration, two nitrogen atoms share three pairs of electrons, forming a triple bond ($N \equiv N$).
The triple bond consists of one $\sigma$ bond and two $\pi$ bonds. The $\sigma$ bond is formed by the axial overlapping of one set of $p$ orbitals (e.g., $2p_z - 2p_z$), while the two $\pi$ bonds are formed by the lateral overlapping of the remaining two sets of $p$ orbitals (e.g., $2p_x - 2p_x$ and $2p_y - 2p_y$).
Since all the orbitals involved in the bond formation are $p$ orbitals, the overlapping is of the p$-$p type.
Therefore, the $N_2$ molecule contains a triple bond and exhibits p$-$p overlap.
Answer: Triple bond and p$-$p overlap
Each nitrogen atom has three half-filled $2p$ orbitals ($2p_x, 2p_y, 2p_z$). To achieve a stable octet configuration, two nitrogen atoms share three pairs of electrons, forming a triple bond ($N \equiv N$).
The triple bond consists of one $\sigma$ bond and two $\pi$ bonds. The $\sigma$ bond is formed by the axial overlapping of one set of $p$ orbitals (e.g., $2p_z - 2p_z$), while the two $\pi$ bonds are formed by the lateral overlapping of the remaining two sets of $p$ orbitals (e.g., $2p_x - 2p_x$ and $2p_y - 2p_y$).
Since all the orbitals involved in the bond formation are $p$ orbitals, the overlapping is of the p$-$p type.
Therefore, the $N_2$ molecule contains a triple bond and exhibits p$-$p overlap.
Answer: Triple bond and p$-$p overlap
Hence, the correct answer is option: 'C'.