The increasing order of the first ionisation enthalpies of the elements B, P, S and F (lowest first) is

  • Option 1)

    F<S<P<B\;

  • Option 2)

    \; P<S<B<F\;

  • Option 3)

    \; B<P<S<F\;

  • Option 4)

    \; B<S<P<F

 

Answers (1)

As we learnt in

Ionization enthalpy -

It is defined as the minimum amount of energy required to remove the outer most shell electron from an isolated gaseous atom (X) to form the gaseous ion.

- wherein

X_{(g)}\rightarrow X^{+}_{(g)}  +e^{-}

 

 Along a period from left to right, I.E increases with increasing atomic number, and ionization enthalpy decreases down the group. But P has a half filled stable configuration as compared to S and because of that ionization enthalpy of P is higher than S.


Option 1)

F<S<P<B\;

This option is incorrect.

Option 2)

\; P<S<B<F\;

This option is incorrect.

Option 3)

\; B<P<S<F\;

This option is incorrect.

Option 4)

\; B<S<P<F

This option is correct.

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