The electron affinity for sulfur is more exothermic than...

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Key Concepts

Electron Affinity

This concept refers to the energy change that occurs when an electron is added to a neutral atom in the gaseous state. It measures how strongly an atom attracts an extra electron, and is influenced by factors such as atomic size, electron repulsion, and orbital energies.

Atomic Size and Orbital Diffuseness

The size of an atom affects the spatial distribution of its electrons. In larger atoms, the orbitals are more diffuse, which means that an added electron experiences less electron-electron repulsion. This is a key factor in why sulfur, being larger than oxygen, exhibits a more exothermic electron affinity.

Electron-Electron Repulsion

When electrons are added to an atom, repulsion between electrons in the same orbital or region can counteract the energy released from forming a new bond. In smaller atoms like oxygen, this repulsion is stronger due to closer proximity of electrons, leading to a less exothermic electron affinity compared to sulfur, where the effect of repulsion is mitigated by larger, more spread-out orbitals.

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