Arrange the following species into groups of isoelectronic...

Arrange the following species into groups of isoelectronic species: $\begin{array}{llllll}\mathrm{F}^{-} & \mathrm{Sc}^{3+} & \mathrm{Be}^{2+} & \mathrm{Rb}^{+} & \mathrm{O}^{2-} & \mathrm{Na}^{+} & \mathrm{Ti}^{4}\end{array}$ $\begin{array}{lllll}\mathrm{Ar} & \mathrm{B}^{\mathrm{s} *} & \mathrm{He} & \mathrm{Se}^{2-} & \mathrm{Y}^{\mathrm{s}}\end{array}$

Arrange the following species into groups of isoelectronic species:
$\begin{array}{llllll}\mathrm{F}^{-} & \mathrm{Sc}^{3+} & \mathrm{Be}^{2+} & \mathrm{Rb}^{+} & \mathrm{O}^{2-} & \mathrm{Na}^{+} & \mathrm{Ti}^{4}\end{array}$
$\begin{array}{lllll}\mathrm{Ar} & \mathrm{B}^{\mathrm{s} *} & \mathrm{He} & \mathrm{Se}^{2-} & \mathrm{Y}^{\mathrm{s}}\end{array}$

Key Concepts

Isoelectronic Species

Isoelectronic species are atoms, ions, or molecules that have the same number of electrons and thus share an identical electron configuration. This concept is important because, despite having different nuclear charges, these species exhibit similar electron distributions, which can lead to analogous chemical behaviors and properties.

Electron Configuration

Electron configuration defines the arrangement of electrons in the orbitals of an atom or ion. It plays a crucial role in determining the chemical and physical properties of a species. When comparing different species, having an identical electron configuration indicates that they are isoelectronic, regardless of differences in atomic number or ionic charge.

Ionization and Ionic Charges

Ionization involves the loss or gain of electrons, resulting in the formation of ions with positive or negative charges. Understanding how atoms achieve a particular electron count through ionization is fundamental when grouping species into isoelectronic sets, as ions can still be isoelectronic with neutral atoms even though their overall charge differs.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by electrons in an atom or ion, taking into account both the actual nuclear charge and the shielding effect of inner electrons. In isoelectronic species, variations in effective nuclear charge, due to differences in the number of protons, can influence the size, ionization energy, and other properties, even though the species share the same electron configuration.

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