Select the smaller member of each pair.
(a) $\mathrm{P}$ or $\mathrm{P}^{3-}$
$P$
$\mathrm{P}^{3-}$
(b) $\mathrm{Mn}^{4+}$ or $\mathrm{Mn}^{2+}$
$\mathrm{Mn}^{4+}$
$\mathrm{Mn}^{2+}$

C $\mathrm{Rb}$ or $\mathrm{Rb}^{+}$
$\mathrm{Rb}$
$\mathrm{Rb}^{+}$
d) $\mathrm{Ce}$ or $\mathrm{Ce}^{3+}$
$\mathrm{Ce}$
$\mathrm{Ce}^{3+}$

Question

Select the smaller member of each pair.
(a) $\mathrm{P}$ or $\mathrm{P}^{3-}$
$P$
$\mathrm{P}^{3-}$
(b) $\mathrm{Mn}^{4+}$ or $\mathrm{Mn}^{2+}$
$\mathrm{Mn}^{4+}$
$\mathrm{Mn}^{2+}$

C $\mathrm{Rb}$ or $\mathrm{Rb}^{+}$
$\mathrm{Rb}$
$\mathrm{Rb}^{+}$
d) $\mathrm{Ce}$ or $\mathrm{Ce}^{3+}$
$\mathrm{Ce}$
$\mathrm{Ce}^{3+}$

Accepted Answer

***A*** ∻Key Concept∻ ⚹Atomic size and ionic charge⚹ ∻Explanation∻ ⚹The phosphorus atom ($\mathrm{P}$) is smaller than its anion ($\mathrm{P}^{3-}$) because adding electrons increases the electron-electron repulsion and causes the atomic radius to expand.⚹ ***A*** ∻Key Concept∻ ⚹Ionic size and nuclear charge⚹ ∻Explanation∻ ⚹$\mathrm{Mn}^{4+}$ is smaller than $\mathrm{Mn}^{2+}$ because a higher positive charge pulls the electrons closer to the nucleus, reducing the ionic radius.⚹ ***B*** ∻Key Concept∻ ⚹Cation size compared to its neutral atom⚹ ∻Explanation∻ ⚹$\mathrm{Rb}^{+}$ is smaller than $\mathrm{Rb}$ because the loss of an electron reduces electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus.⚹ ***B*** ∻Key Concept∻ ⚹Cation size and electron removal⚹ ∻Explanation∻ ⚹$\mathrm{Ce}^{3+}$ is smaller than $\mathrm{Ce}$ because removing electrons reduces the size of the electron cloud and the effective nuclear charge per electron increases, pulling the electrons closer to the nucleus.⚹◊Which ion would have a smaller size: $\mathrm{Rb}$ or $\mathrm{Rb}^{+}$?⍭ Generate me a similar question◊

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