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Question

The  correct increasing order for second ionization energy of  $$ He, Li, Be, B, C, N, O, F, Ne$$  is :


A
Be<C<B<N<O<F<Ne<Li<He
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B
Be<B<C<N<O<F<Ne<He<Li
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C
Be<C<B<N<F<O<Ne<He<Li
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D
Be<C<B<O<N<F<Ne<He<Li
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Solution

The correct option is B $$Be\, <\, C\, <\, B\, <\, N\, <\, F\, <\, O\, <\, Ne\,<\, He\,<\,Li$$
$$He^+- 1s^1$$
$$Li^+- [He]$$
$$Be^+- [He]2s^1$$
$$B^+- [He]2s^2$$
$$C^+- [He]2s^22p^1$$
$$N^+- [He]2s^22p^2$$
$$O^+- [He]2s^22p^3$$
$$F^+- [He]2s^22p^4$$
$$Ne^+- [He]2s^22p^5$$
$$Li^+$$ is most stable and then comes $$He^+$$. Half filled orbitals are more stable than partially filled.
Hence the correct order will be $$Be\, <\, C\, <\, B\, <\, N\, <\, F\, <\, O\, <\, Ne\,<\, He\,<\,Li$$

Chemistry

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