Question

Bond between two nitrogen atoms in Nitrogen molecule is

• A. Single bond
• B. Double bond
• C. Triple bond
• D. Multiple bond % General term

Hint:

- Nitrogen atom (N) has 5 valence electrons. - To achieve a stable octet, it needs 3 more electrons. - In N\(_2\) molecule, the two N atoms share 3 pairs of electrons, forming a N\( \equiv \)N triple bond. - This triple bond consists of one sigma (\(\sigma\)) bond and two pi (\(\pi\)) bonds. - The N\(_2\) molecule is very stable due to the high bond dissociation energy of the triple bond.

Answer 1

The Correct Option is C

Step 1: Consider the electronic configuration of a nitrogen atom.
Nitrogen (N) has an atomic number of 7.
Its electronic configuration is \(1s^2 2s^2 2p^3\).
It has 5 valence electrons (2 in 2s and 3 in 2p).

Step 2: Determine how nitrogen atoms bond to form a nitrogen molecule (N\(_2\)).
To achieve a stable octet (like neon), each nitrogen atom needs to gain 3 more electrons.
In the N\(_2\) molecule, the two nitrogen atoms share three pairs of electrons, forming a triple covalent bond.
N \( \equiv \) N Each nitrogen atom contributes 3 electrons to the bond, and each also has one lone pair of electrons (\( :N \equiv N: \)).

Step 3: Identify the type of bond.
The bond between the two nitrogen atoms in an N\(_2\) molecule is a triple bond.
Option (4) "Multiple bond" is a general term that includes double and triple bonds, but "Triple bond" is more specific and accurate.
This matches option (3).