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

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Aicharya · Accepted Answer

The order of ionization enthalpy of elements of 2nd period in long form of periodic table is $\mathrm{Li} < \mathrm{B} < \mathrm{Be} < \mathrm{C} < \mathrm{O} < \mathrm{N} < \mathrm{F} < \mathrm{Ne}$. Generally, on going left to right in a period, ionization energy increases, but there are some exceptions to this. For example, Be has more ionization energy than $\mathrm{B}$, due to fulfilled s-orbital. And $\mathrm{N}$ has more ionization energy than $\mathrm{O}$ due to half filled p-subshell. So,In second period of the long form of the periodic table, the element B has second lowest first ionization enthalpy and element F has second highest first ionization enthalpy values. ^

In second period of the long form of the periodic table, an element X has second lowest first ionization…

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