Assertion: Ionisation enthalpy of group $16$ elements is lower than that of group $15$ elements.
Reason: On moving left to right in a period, effective nuclear charge increases.

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

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Both Assertion and Reason are correct and Reason is NOT the correct explanation of the Assertion

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Assertion is correct and Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is B Both Assertion and Reason are correct and Reason is NOT the correct explanation of the Assertion
On moving left to right in a period, effective nuclear charge increases due to which the ionisation enthalpy decreases from left to right. But because of the extra stable half-filled $p$ -orbital in group $15$ elements, its ionisation enthalpy is higher than that of group $16$ elements.

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Similar questions

Explain the following
(i) Electronegativity of elements increase on moving from left to right in the periodic table.

(ii) Ionisation enthalpy decreases in a group from top to bottom.

Assertion: The atomic radius decreases as we move from left to right in a period.

Reason: Effective nuclear charge increases across the period from left to right.

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