Question 16

Nitrogen gas is an extremely stable molecule due to its triple covalent bonds.

Nitrogen gas (N₂) consists of two nitrogen atoms connected by a triple covalent bond, which involves sharing three pairs of electrons. This strong bond contributes significantly to the stability of the nitrogen molecule, making it less reactive under standard conditions.

A) resonance bonds

Resonance bonds involve the delocalization of electrons across multiple structures, which is not applicable to nitrogen gas. Therefore, this option is incorrect as it does not explain the stability of N₂.

B) ionic bonds

Ionic bonds are formed through the transfer of electrons between atoms, resulting in charged ions. Nitrogen gas does not form ionic bonds; instead, it is characterized by covalent bonding. Thus, this option is incorrect in the context of nitrogen's stability.

C) triple covalent bonds

The triple covalent bonds in nitrogen gas are formed by sharing three pairs of electrons between the two nitrogen atoms. This strong bond results in a very stable molecule, making nitrogen gas inert under many conditions. This option correctly explains why nitrogen gas is stable.

D) hydrogen bonds

Hydrogen bonds are weak attractions between molecules that involve hydrogen atoms. They are not relevant to the stability of nitrogen gas, which does not involve hydrogen bonding. Therefore, this option is incorrect.

Conclusion

The reason nitrogen gas is extremely stable is due to the presence of triple covalent bonds, which provide significant strength and stability to the molecule. Other options fail to accurately represent the bonding characteristics of nitrogen gas, reinforcing that triple covalent bonding is the key factor in its stability.