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Question
Chemistry
Posted 6 months ago
Select the smaller member of each pair.
(a) P\mathrm{P} or P3\mathrm{P}^{3-}
PP
P3\mathrm{P}^{3-}
(b) Mn4+\mathrm{Mn}^{4+} or Mn2+\mathrm{Mn}^{2+}
Mn4+\mathrm{Mn}^{4+}
Mn2+\mathrm{Mn}^{2+}

C Rb\mathrm{Rb} or Rb+\mathrm{Rb}^{+}
Rb\mathrm{Rb}
Rb+\mathrm{Rb}^{+}
d) Ce\mathrm{Ce} or Ce3+\mathrm{Ce}^{3+}
Ce\mathrm{Ce}
Ce3+\mathrm{Ce}^{3+}
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Answer from Sia
Posted 6 months ago
A
Key Concept
Atomic size and ionic charge
Explanation
The phosphorus atom (P\mathrm{P}) is smaller than its anion (P3\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
Mn4+\mathrm{Mn}^{4+} is smaller than Mn2+\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
Rb+\mathrm{Rb}^{+} is smaller than Rb\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
Ce3+\mathrm{Ce}^{3+} is smaller than Ce\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.

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