In a period,the first ionisation enthalpy of | vedclass

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(C) In a period,the first ionization enthalpy increases from left to right due to an increase in the effective nuclear charge and a decrease in atomic

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lowest and highest

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(C) In a period,the first ionization enthalpy increases from left to right due to an increase in the effective nuclear charge and a decrease in atomic size.Therefore,the element at the extreme left of a period has the lowest first ionization enthalpy.Conversely,the electron gain enthalpy becomes more negative (higher magnitude) as we move from left to right across a period (excluding noble gases,which have positive values due to stable configurations).Thus,the element at the extreme right (halogens) has the highest negative electron gain enthalpy.

In a period,the first ionisation enthalpy of the element at the extreme left and the negative electron gain enthalpy of the extreme right element,except noble gases,are respectively.

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