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(B) The first ionisation enthalpy generally increases across a period due to an increase in effective nuclear charge. However,there are deviations due

Vedclass · Accepted Answer

$Li < B < Be < C < O < N < F < Ne$

Vedclass · Answer

(B) The first ionisation enthalpy generally increases across a period due to an increase in effective nuclear charge. However,there are deviations due to stable electronic configurations. The electronic configurations for second period elements are: $Li (2s^1)$,$Be (2s^2)$,$B (2s^2 2p^1)$,$C (2s^2 2p^2)$,$N (2s^2 2p^3)$,$O (2s^2 2p^4)$,$F (2s^2 2p^5)$,$Ne (2s^2 2p^6)$. $Be$ has a fully filled $2s$ orbital,making its ionisation energy higher than $B$. $N$ has a half-filled $2p$ subshell,making its ionisation energy higher than $O$. The correct order is: $Li < B < Be < C < O < N < F < Ne$.

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

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