Why does the first ionisation enthalpy increase as we go from left to right through a given period of the periodic table?

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Solution

This is due to the gradual increase in nuclear charge and with the simultaneous decrease in atomic size the electrons are more and more tightly bound to the nucleus. This results in the gradual increase in ionization energy across the period.

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Ionisation energy increases as we move down the group of a periodic table whereas it decreases as we move from left to right of the periodic table.

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 ionisation energy decreases as we go from left to right in a period.

Reason: The nuclear charge increases as we go from left to right in a period but the number of shells remain the same in a period.

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