Chemistry

Problem

In the isoelectronic series Na⁺, Mg²⁺, and Al³⁺, which statement best explains why Al³⁺ has the smallest ionic radius? a)

Al^{3+}

has fewer electron–electron repulsions because it loses three electrons when it forms the ion. b) Atomic radius decreases across a period, and aluminum lies furthest to the right of these three elements, so

Al^{3+}

is the smallest ion. c)

Al^{3+}

possesses the greatest nuclear charge, so the same number of electrons is drawn closer to the nucleus. d)

Al^{3+}

experiences less effective nuclear charge because additional inner-shell shielding occurs.

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