As atomic size increases, electron affinity :

increases

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decreases

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depends on elements

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none of the above

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Solution

The correct option is B decreases
A trend of decreasing electron affinity going down the groups in the periodic table is because the additional electron will be entering in an orbital farther away from the nucleus. Since this electron is far from the nucleus it experiences less attraction towards the nucleus and would release less energy when added.

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Similar questions

Q. The amount of energy released when an atom in the gaseous state accepts an electron to form an anion. factor which affect electron affinity are: atomic size and Nuclear charge. As atomic radii increases, electron affinity increase. As nuclear charge increase, electron affinity increase. it decrease down a group and increases across a period. Explain.

Q. What is electron affinity and how it depends on atomic size, effective nuclear change and screening factor?

Q. Electron affinity is inversely proportional to the size of an atom.

On moving across a period, the atomic size decreases and nuclear charge increases and therefore the force of attraction exerted by the nucleus on the electron in the outermost shell increases.
For the process
$A_{(g)} + e^{-} \to A_{(g)}^{-}; Δ H = x a n d A_{(g)}^{-} \to A_{(g)} + e^{-}; Δ H = y$
Select correct alternate:

Q. The electron affinity increases on moving from left to right along a period. Arrange the reasons in a proper sequence.
(a) The amount of energy released during the addition of an electrons increases from left to right along a period.
(b) Effective nuclear charge of the elements increases from left to right.
(c) The atomic size of the elements decreases from left to right.
(d) The tendency to gain electrons and form anion increases from left to right.

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