The correct order of ionization energy in the following second-period elements is:

Question

The correct order of ionization energy in the following second-period elements is: (A) B < Be < C < N < O (B) B < Be < N < C < O (C) Be>B>C>N>O (D) B < Be < C < O < N

Tardigrade Admin · Accepted Answer

Ionization energy increases along the period. But Be(2 s2) and N(2 s2 2 p3) have higher ionization energy than boron and oxygen respectively due to stable electronic configuration (half-filled and full-filled subshells are exceptionally stable).

Q. The correct order of ionization energy in the following second-period elements is:

$B < B e < C < N < O$

$B < B e < N < C < O$

$B e > B > C > N > O$

$B < B e < C < O < N$

Ionization energy increases along the period. But $B e (2 s^{2})$ and $N (2 s^{2} 2 p^{3})$ have higher ionization energy than boron and oxygen respectively due to stable electronic configuration (half-filled and full-filled subshells are exceptionally stable).

Q. The correct order of ionization energy in the following second-period elements is:

B<Be<C<N<O

B<Be<N<C<O

Be>B>C>N>O

B<Be<C<O<N

Ionization energy increases along the period. But Be(2s2) and N(2s22p3) have higher ionization energy than boron and oxygen respectively due to stable electronic configuration (half-filled and full-filled subshells are exceptionally stable).

$B < B e < C < N < O$

$B < B e < N < C < O$

$B e > B > C > N > O$

$B < B e < C < O < N$

Ionization energy increases along the period. But $B e (2 s^{2})$ and $N (2 s^{2} 2 p^{3})$ have higher ionization energy than boron and oxygen respectively due to stable electronic configuration (half-filled and full-filled subshells are exceptionally stable).