The first ionisation enthalpies for three ele | vedclass

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Question

(A) The elements $O$,$F$,and $Ne$ belong to the same period,i.e.,the $2nd$ period of the periodic table.As we move from left to right across a period,

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$O, F$ and $Ne$

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(A) The elements $O$,$F$,and $Ne$ belong to the same period,i.e.,the $2nd$ period of the periodic table.As we move from left to right across a period,the atomic radius decreases and the effective nuclear charge increases,which leads to an increase in the first ionisation enthalpy.The order of increasing ionisation enthalpy for these elements is $O Given values are $1314 \, kJ \, mol^{-1}$ for $O$,$1680 \, kJ \, mol^{-1}$ for $F$,and $2080 \, kJ \, mol^{-1}$ for $Ne$.Therefore,the correct sequence is $O, F$ and $Ne$.

The first ionisation enthalpies for three elements are $1314$,$1680$ and $2080 \, kJ \, mol^{-1}$,respectively. The correct sequence of the elements is

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