Which is the larger species in each pair? a. Sr or S r^2+ b. N or N^3- c. Ni or N

step 1 So now we'll work on problem in chapter 8. Here, they ask us to select the larger species from e

Which is the larger species in each pair? a. Sr or S...

Which is the larger species in each pair?
\begin{equation}
\begin{array} \\ {\text { a. Sr or } S r^{2+} \quad \text { b. } N \text { or } N^{3-} \quad \text { c. Ni or } N i^{2+} \quad \text { d. } S^{2-} \text { or } C a^{2+}}\end{array}
\end{equation}

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Key Concepts

Effective Nuclear Charge

This concept describes the net positive charge experienced by electrons in an atom or ion after accounting for the shielding effect of the inner electrons. In ions, especially in isoelectronic species, a higher effective nuclear charge will pull the electrons closer to the nucleus, resulting in a smaller radius. This is why cations tend to be smaller than their neutral atoms and, conversely, anions are larger.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons but different numbers of protons. Within such a series, the species with more protons (and consequently a higher effective nuclear charge) is typically smaller. This principle helps in comparing the sizes of ions that have been formed by either electron loss or gain across different elements.

Atomic and Ionic Radii

These are measures of the size of atoms and ions, respectively. The atomic radius refers to the size of a neutral atom, while the ionic radius pertains to an ion that has either lost or gained electrons. Changes in electron number during ion formation directly influence the radius: cations (positively charged ions) usually contract because they lose electron-electron repulsion, whereas anions (negatively charged ions) typically expand due to an increase in electron-electron repulsion.

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