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JEE MainChemistryp Block Elements (Group 15, 16, 17 & 18)

At room temperature, dinitrogen ( N₂ ) is chemically inert, whereas white phosphorus ( P₄ ) is highly reactive and spontaneously catches fire in air. The primary reason for this stark difference in reactivity is:

Options

  1. ANitrogen is a gas at room temperature while white phosphorus is a solid.
  2. BNitrogen has a significantly higher electronegativity than phosphorus.
  3. CNitrogen forms a very strong p -p triple bond, whereas phosphorus forms single bonds with significant angle st
  4. DNitrogen lacks vacant d-orbitals in its valence shell, whereas phosphorus has them available for bonding.

Correct answer

C. Nitrogen forms a very strong p -p triple bond, whereas phosphorus forms single bonds with significant angle st

Step-by-step solution

Dinitrogen ( N₂ ) exists as a diatomic molecule with a triple bond ( N N ) formed by p -p multiple bonding. Because of its very high bond dissociation enthalpy, it is highly unreactive at room temperature. On the other hand, phosphorus cannot form stable p -p multiple bonds due to its larger atomic size. It exists as a discrete tetrahedral P₄ molecule with P-P single bonds. The P₄ molecule is highly strained (bond angle 60^ ), making it highly reactive and prone to catching fire in air. Therefore, the primary reaso

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