True or False: (a) Cations are larger than their corresponding neutral atoms. (b) Li^+ is smalle

step 1 here is a statement that is in fact false. The cations are smaller than the neutral atoms in ter

True or False: (a) Cations are larger than their...

Key Concepts

Atomic and Ionic Radii

Atomic radius refers to the size of a neutral atom, while ionic radius refers to the size of an ion. When electrons are removed to form cations, the decrease in electron-electron repulsion and the increased effective nuclear charge lead to a smaller radius compared to the neutral atom. Conversely, adding electrons to form anions generally increases the ionic radius due to additional electron-electron repulsion.

Effective Nuclear Charge

The effective nuclear charge is the net positive charge experienced by electrons in an atom, after accounting for electron shielding. In cations, the loss of electrons results in a higher effective nuclear charge per electron, pulling the remaining electrons closer to the nucleus and reducing the ionic size. In anions, the increased electron-electron repulsion usually results in a larger size despite a similar nuclear charge.

Electron-Electron Repulsion

Electron-electron repulsion is the force that causes electrons to repel each other, impacting the spatial distribution of electrons around the nucleus. In anions, the added electrons increase repulsion, expanding the electron cloud and leading to a larger ionic radius. In cations, the loss of electrons reduces this repulsion, contributing to a contraction of the ionic radius.

Periodic Trends in Atomic and Ionic Sizes

Periodic trends refer to the predictable changes in atomic and ionic sizes across the periodic table. These trends help explain why cations are generally smaller than their neutral atoms, and why anions tend to be larger. Understanding these trends is crucial for predicting and rationalizing the sizes of different ions based on their position and charge in the periodic table.

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