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

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$Be, N$

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(C) The first ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge.However,there are exceptions due to stable electronic configurations.In the second period $(Li, Be, B, C, N, O, F, Ne)$:$1$. $Be$ $(1s^2 2s^2)$ has a higher ionization enthalpy than $B$ $(1s^2 2s^2 2p^1)$ because of the fully filled $2s$ orbital.$2$. $N$ $(1s^2 2s^2 2p^3)$ has a higher ionization enthalpy than $O$ $(1s^2 2s^2 2p^4)$ because of the half-filled $2p$ subshell.Thus,$Be$ and $N$ have higher ionization enthalpies than their immediate neighbors.Therefore,the correct option is $C$.

In the second period of the modern periodic table,two elements $X$ and $Y$ have higher first ionization enthalpy values than the preceding and succeeding elements. $X$ and $Y$ are respectively

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