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(A) The order of first ionization enthalpy for elements of the $2nd$ period is: $Li < B < Be < C < O < N < F < Ne$. Generally,ionization enthalpy incr

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$B, F$

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(A) The order of first ionization enthalpy for elements of the $2nd$ period is: $Li Generally,ionization enthalpy increases from left to right across a period. However,there are exceptions due to electronic configuration: $Be$ $(1s^2 2s^2)$ has a higher ionization enthalpy than $B$ $(1s^2 2s^2 2p^1)$ due to a fully-filled $s$-orbital. $N$ $(1s^2 2s^2 2p^3)$ has a higher ionization enthalpy than $O$ $(1s^2 2s^2 2p^4)$ due to a half-filled $p$-subshell. Based on the order $Li The second lowest first ionization enthalpy is $B$. The second highest first ionization enthalpy is $F$. Therefore,$X = B$ and $Y = F$.

In the second period of the long form of the periodic table,an element $X$ has the second lowest first ionization enthalpy and element $Y$ has the second highest first ionization enthalpy values. What are $X$ and $Y$?

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