A) \[52.15\]
B) \[911\]
C) \[104\]
D) \[52153\]
Correct Answer: C
Solution :
First ionisation energy increases in a period. Thus, the first IE of the elements of the second period should be as follows \[Be<B<N<O\] But in practice, the elements do not follow the above order. The first IE of these elements is \[B<Be<O<N\] 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 than that of N is because of the half-filled 2p orbitals in \[(1{{s}^{2}},2{{s}^{2}}2{{p}^{3}})\]).
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