Which one of the following ion has the highest value of ionic radius? (a) F^- (b) O^2- (c) B^3+

Which one of the following ion has the highest value of...

Key Concepts

Ionic Radius

Ionic radius is a measure of the size of an ion, typically defined as the distance from the nucleus to the outermost electron cloud. It is influenced by factors such as the number of electron shells and the effective nuclear charge acting on the electrons. This concept is important because it helps explain trends in periodic properties and reactivity among different ions.

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by electrons in an atom or ion after accounting for shielding effects. A higher effective nuclear charge tends to pull electrons closer to the nucleus, resulting in a smaller ionic radius, whereas a lower effective nuclear charge allows electrons to be less tightly bound and results in a larger radius. This concept is key to understanding variations in ionic sizes among isoelectronic species.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons, meaning they share a similar electron configuration. However, differences in the number of protons (and thus the effective nuclear charge) among these species lead to differences in ionic radii. Typically, among isoelectronic ions, those with fewer protons have larger ionic radii because the lower effective nuclear charge cannot pull the electron cloud as tightly toward the nucleus.

Periodic Trends in Ion Size

Periodic trends in ion size are determined by the interplay between electron configuration, nuclear charge, and electron shielding. In a group of ions, negatively charged ions (anions) usually have larger radii compared to their neutral atoms, while positively charged ions (cations) are smaller. These trends help in predicting and comparing the ionic radii across different elements or ionic species.

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