Arrange Li, Be, B and C in decreasing order o | vedclass

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(C) Across a period,the first ionisation enthalpy generally increases from left to right due to an increase in effective nuclear charge.However,there

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$C > Be > B > Li$

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(C) Across a period,the first ionisation enthalpy generally increases from left to right due to an increase in effective nuclear charge.However,there are exceptions due to stable electronic configurations.$Li$ $(1s^2, 2s^1)$ has the lowest ionisation enthalpy.$Be$ $(1s^2, 2s^2)$ has a fully filled $2s$ subshell,which is more stable than the $2p^1$ configuration of $B$ $(1s^2, 2s^2, 2p^1)$.Therefore,the ionisation enthalpy of $Be$ is higher than that of $B$.$C$ $(1s^2, 2s^2, 2p^2)$ has the highest ionisation enthalpy among these elements.The correct decreasing order is $C > Be > B > Li$.Thus,option $(C)$ is correct.

Arrange $Li, Be, B$ and $C$ in decreasing order of their first ionisation enthalpies.

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