Question

Consider the elements in the second period and p-block. The first
lonization energy (of these elements)
Increases steadily from B to Ne
Decreases steadily from B to Ne
Increases from B to O, decreases for F and then increases for Ne
Increases steadily from B to N, decreases for O and increases from O to Ne​

Answer 1

Answer:

Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'.

Hence, the correct order of first ionisation enthalpy is:

$\large\rm {Li<B<Be<C<O<N<F<Ne}$

Answer 2

Answer:

Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'.

Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'. Hence, the correct order of first ionisation enthalpy is:

Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'. Hence, the correct order of first ionisation enthalpy is:

Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'. Hence, the correct order of first ionisation enthalpy is: Li<B<Be<C<O<N<F<Ne