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Single N-N bond is weaker than the singl...

Single `N-N` bond is weaker than the single `P-P` bond. This is because of `:`

A

larger `N-N` bodn length in comparison to `P-P` bond length.

B

high interelectronic repulsion of the non`-` bondioni electrons, owing to the small `N-N` bond length in comparison to that in that in `P-P` single bond.

C

Higher electronegativity of N in comparison to P.

D

smaller atomic size of N as compared to that of P.

Text Solution

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The correct Answer is:
2
Statement is correct.
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Read the passage given below and answer the questions that follows: Nitrogen differs from the rest of the members of this group due to its small size, high electronegativity, high ionisation enthalpy and non-availability of d-orbitals. Nitrogen has unique ability to form p pi- p pi multiple bonds with itself and with other elements having small size and high electronegativity (For example, C, O). Heavier elements of this group do not form p pi - p pi bonds as their atomic orbitals are so large and diffuse that they cannot have effective overlapping. Thus, nitrogen exists as a diatomic molecule with a triple bond (one s and two p) between the two atoms. Consequently, its bond enthalpy (941.4 kJ "mol"^(-1) ) is very high. On the contrary, phosphorus, arsenic and antimony form single bonds as P-P, As-As and Sb-Sb while bismuth forms metallic bonds in elemental state, However, the single N-N bond is weaker than the single P-P bond because of high interelectronic repulsion of the non-bonding electrons, owing to the small bond length. Why is the single N- N bond weaker than the single P - P bond ?

Read the passage given below and answer the questions that follows: Nitrogen differs from the rest of the members of this group due to its small size, high electronegativity, high ionisation enthalpy and non-availability of d-orbitals. Nitrogen has unique ability to form p pi- p pi multiple bonds with itself and with other elements having small size and high electronegativity (For example, C, O). Heavier elements of this group do not form p pi - p pi bonds as their atomic orbitals are so large and diffuse that they cannot have effective overlapping. Thus, nitrogen exists as a diatomic molecule with a triple bond (one s and two p) between the two atoms. Consequently, its bond enthalpy (941.4 kJ "mol"^(-1) ) is very high. On the contrary, phosphorus, arsenic and antimony form single bonds as P-P, As-As and Sb-Sb while bismuth forms metallic bonds in elemental state, However, the single N-N bond is weaker than the single P-P bond because of high interelectronic repulsion of the non-bonding electrons, owing to the small bond length. Heavier elements of Group 15 do not form p pi - p pi bonds.

Knowledge Check

  • The number of P-O-P bonds in cyclic trimeter of N is:

    A
    Three
    B
    Two
    C
    Zero
    D
    Four

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