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Question

For the second period elements the correct increasing order of first ionisation enthalpy is:


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

The correct option is D Li < B < Be < C < O < N < F < Ne
As we go from left to right in a period ionisation energy increases. ′Be′ and ′N′ comparatively more stable valence subshell than 'B' and 'O'. 

Hence, the correct order of first ionisation enthalpy is:
 
$$Li<B<Be<C<O<N<F<Ne$$

Chemistry

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