The correct order of first ionisation enthalp | vedclass

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Question

(A) The first ionisation enthalpy generally increases as we move from left to right across a period due to an increase in effective nuclear charge. Ho

Vedclass · Accepted Answer

$Li < B < Be < C$

Vedclass · Answer

(A) The first ionisation enthalpy generally increases as we move from left to right across a period due to an increase in effective nuclear charge. However,$Be$ $(1s^2 2s^2)$ has a fully-filled $2s$ subshell,which is more stable than the $2p^1$ configuration of $B$ $(1s^2 2s^2 2p^1)$. Therefore,$Be$ has a higher first ionisation enthalpy than $B$. The correct order is $Li < B < Be < C$.

The correct order of first ionisation enthalpy of the given elements is:

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