A) \[Li<Be<B<C<N<O<F<Ne\]
B) \[Li<B<Be<C<O<N<F<Ne\]
C) \[Li>Be>B>C>N>O>F>Ne\]
D) .\[Li>B>C>Be>O>N>F>Ne\]
Correct Answer: B
Solution :
The fast lonisation Energy \[(IE)\] increases in a. period. Thus, the first IE of the elements of second period should be as follows: \[Li<Be<B<G<N<O<F<Ne~\] But in practice, the elements do not follow the above order. The first IE of these element is \[Li<B<Be<C<O<N<F<Ne~\] The lower IE of B than that of Be is because in \[B(1{{s}^{2}}2{{s}^{2}}2{{p}^{1}}),\]electron is to be removed from \[2p\]which is easy while in \[Be(1{{s}^{2}},2{{s}^{2}}),\]electron is to be removed from 2s which is difficult. The low IE of O is lower than that of N because of the half-filled \[2p\]orbitals in \[N(1{{s}^{2}},2{{s}^{2}},2{{p}^{3}}).\]
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