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

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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