Bond enthalpy in H 2 molecule is 435.8 KJ mole –1 where as bond enthalpy in N 2 molecule is 946.0 KJ mole –1 , because

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Bond Type: Hydrogen (H₂) contains a single covalent bond (H–H) formed by sharing one electron pair.

Multiple Bonding: Nitrogen (N₂) contains a triple covalent bond (N≡N) formed by sharing three electron pairs.

Bond Strength: A triple bond is much stronger than a single bond due to greater electron density between the nuclei.

Enthalpy Difference: Because breaking a triple bond requires significantly more energy, N₂ has a much higher bond enthalpy ( $946.0 k J / m o l$ ) than H₂ ( $435.8 k J / m o l$ ).

Chemistry - CHEMICAL BONDING Question with Solution | TestHub

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