Q.Nitrogen molecule is highly stable. Why?

N2 is highly stable because its atoms are held by a very strong triple bond with a bond dissociation enthalpy of about 941 kJ/mol.

Each nitrogen atom has the electron configuration 1s2 2s2 2p3, i.e. three unpaired electrons in the 2p orbitals.

In the dinitrogen molecule these atoms share three electron pairs, forming one sigma bond and two pi bonds - a nitrogen-nitrogen triple bond (N is identical to N).

Consequences of this triple bond:

• The bond dissociation enthalpy is very high (about 941 kJ/mol), one of the highest known for a diatomic molecule.
• The bond length is short (about 110 pm). …

N2 is unreactive because its N≡N triple bond has an exceptionally high bond dissociation energy (~941 kJ/mol), making bond breaking very difficult.

The nitrogen molecule consists of two N atoms bonded by a triple bond:

N≡N (one sigma and two pi bonds)

This triple bond is very short and extremely strong. Its bond dissociation enthalpy is about 941 kJ/mol — one of the highest known for any diatomic molecule.

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The N triple N bond has a very high bond dissociation enthalpy (~941 kJ/mol), so N2 is very stable and unreactive.

A nitrogen molecule (N2) consists of two nitrogen atoms bonded together. Each nitrogen atom has the electronic configuration 1s2 2s2 2p3, i.e. three unpaired electrons in the 2p orbitals. These pair up between the two atoms to form a triple bond (N triple bond N): one sigma bond and two pi bonds.

Because of this triple bond:

• The bond dissociation enthalpy of N2 is extremely high (about 941 kJ mol^-1), one of the highest known for any diatomic molecule.
• The bond length is very short (about 110 pm). …