Assertion :The electron gain enthalpies have large negative values toward the upper right of the periodic table preceding the noble gases. Reason: The effective nuclear charge increases from left to right across a period and consequently, it will be easier to add an electron to a smaller atom since the added electron on an average would be closer to the positively charged nucleus.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
The electron gain enthalpies have large negative values towards the upper right of the periodic table preceding noble gases because as we move from left to right in a period atomic radii decreases due to increase in effective nuclear charge due to which electron attracting tendency increases and consequently the electron gain enthalpy have larger negative values.

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