For each of the following groups, place the atoms and/or...

For each of the following groups, place the atoms and/or ions in order of decreasing size. a. $\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}, \mathrm{V}^{5+}$ b. $\mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Cs}^{+}$ c. $\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}$ d. $\mathrm{P}, \mathrm{P}^{-}, \mathrm{P}^{2-}, \mathrm{P}^{3-}$ e. $\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}, \mathrm{Te}^{2-}$

For each of the following groups, place the atoms and/or ions in order of decreasing size.
a. $\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}, \mathrm{V}^{5+}$
b. $\mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Cs}^{+}$
c. $\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}$
d. $\mathrm{P}, \mathrm{P}^{-}, \mathrm{P}^{2-}, \mathrm{P}^{3-}$
e. $\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}, \mathrm{Te}^{2-}$

Key Concepts

Electron-Electron Repulsion and Nuclear Attraction

The overall size of atoms and ions is determined by the balance between the attractive force of the nucleus on the electrons and the repulsive forces between electrons. Variations in electron count and the net positive charge of the nucleus alter this balance, leading to differences in atomic and ionic radii.

Isoelectronic Comparisons

Isoelectronic species are atoms or ions that have the same number of electrons. When comparing isoelectronic species, differences in the nuclear charge dictate their sizes: species with a higher nuclear charge tend to have smaller radii, as the electrons are more strongly attracted to the nucleus.

Ionic Charge Effects

Ionic charge effects refer to how the gain or loss of electrons influences an ion's size. Cations, which form by losing electrons, are typically smaller than their neutral atoms due to reduced electron-electron repulsion, while anions, which gain electrons, are larger because the additional electrons increase repulsive forces and spread out the electron cloud.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom or ion after accounting for shielding by other electrons. A higher effective nuclear charge generally pulls the electrons closer to the nucleus, resulting in a smaller atomic or ionic radius.

Periodic Trends

Periodic trends describe how atomic and ionic sizes change in a predictable way across periods and down groups in the periodic table. Generally, atomic radii decrease across a period due to increasing effective nuclear charge, and increase down a group as additional electron shells are added.

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