Indicate which species in each pair has the more favorable (more negative) electron affinity. Ex

step 1 In this question, it says, indicate which species in each part has more favorable or more negati

Indicate which species in each pair has the more favorable...

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Key Concepts

Electron Affinity

Electron affinity is the amount of energy released when an electron is added to an isolated atom in the gaseous state. It reflects how strongly an atom attracts an additional electron, with a more negative value indicating a greater energy release and a more favorable process.

Periodic Trends

Electron affinity generally becomes more negative across a period due to increasing nuclear charge and declining atomic radius, while it becomes less negative down a group as increasing atomic size and electron shielding reduce the nucleus's pull on an added electron.

Atomic Size and Electron Shielding

The size of an atom and the extent of electron shielding influence electron affinity. Smaller atoms with less shielding experience a stronger effective nuclear charge, which more effectively attracts an additional electron, leading to a more favorable (more negative) electron affinity.

Electron-Electron Repulsion

In atoms with closely packed electrons or nearly filled orbitals, added electrons may experience repulsions from existing electrons. This repulsive interaction can reduce the overall energy released when adding an electron, sometimes causing deviations from straightforward periodic trends.

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