Which one of the following ions has the ground-state electron configuration [Xe]4f145d10?

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Question restatement: Which one of the following ions has the ground-state electron configuration [Xe]4f145d10?

Option analysis:
- Po3+: Polonium in the +3 oxidation state would involve the loss of electrons from the p-block (6p and possibly 6s or 5d in heavier elements), but its core configuration remains largely based on the heavier p-block electrons. The expected core for a heavy p-block ion does not match the explicit closed 4f/5d shell pattern given here, and Po3+ would not produce a pure [Xe]4f14 5d10 core. This option is not consistent with the specified [Xe]4f145d10 configuration.
- Tl+: Thallium +1 is formed by removing one electron from the neutral Tl, which has a [Xe]4f14 5d10 6s2 6p1 ground-state. Removing a 6p or 6s electron alters the outer shell, but you still would not isolate a clean [Xe]4f14 5d10 core; the 6s and 6p electrons would influence the valence shell. Thus Tl+ does not match the requested core configuration.
- Bi3+: Bismuth in the +3 state is also a p-block ion with electrons removed from p and possibly s orbitals, but like Tl+, the resulting core would not yield a pure [Xe]4f14 5d10 configuration. The 6p/6s electrons would still be involved in the valence, so this option does not align with [Xe]4f145d10.
- Hg+: Mercury +1 would be formed by removing one electron from the neutral Hg atom, whose ground-state is [Xe]4f14 5d10 6s2. If one 6s electron is removed, you would expect a configuration of [Xe]4f14 5d10 6s1, not [Xe]4f14 5d10. If, hypothetically, both 6s electrons were removed, you would have [Xe]4f14 5d10, which corresponds to Hg2+ in most textbook conventions, not Hg+. Therefore Hg+ does not strictly match the given core either, and the pure [Xe]4f145d10 configuration would imply a complete removal of the 6s electrons rather than a +1 charge.
- Pb4+: Lead in the +4 oxidation state is a heavy p-block ion with a configuration derived from ns2 np2 to ns2 np0 in the outer shell after oxidation, but again the core would not reduce to a clean [Xe]4f14 5d10 pattern. This option does not fit the [Xe]4f145d10 core.

Synthesis of reasoning: The explicit core [Xe]4f145d10 represents a closed 4f shell and a filled 5d subshell with the 6s electrons removed entirely. In common electron-counting terms, that pattern corresponds to Hg in a state where both 6s electrons are gone (i.e., Hg2+ in the usual counting, not Hg+). Among the listed ions, none produce exactly [Xe]4f145d10; the configuration points to a mercury species that has lost all 6s electrons, which would be Hg2+ rather than Hg+. The option names here include several heavy ions, but none match the precise core described. The listed correct choice in the provided data is Hg+, yet standard orbital reasoning shows Hg+ would not yield a clean [Xe]4f145d10 core unless the 6s electron counting is interpreted differently, which is uncommon in standard chemistry conventions.

In summary, the stated configuration corresponds to a state in which the 6s electrons are fully removed, yielding a [Xe]4f14 5d10 core; this is not Hg+ under standard electron configurations. The other ions (Po3+, Tl+, Bi3+, Pb4+) do not produce this exact closed-shell core either because their valence electrons originate from different subshells, and removing or not removing those electrons does not generate the [Xe]4f145d10 core.

Note: The provided answer key lists Hg+ as the correct option, but the strict orbital configuration [Xe]4f145d10 corresponds more closely to a form of Hg2+ (no 6s electrons). This highlights that sometimes test keys may reflect convention differences or simplifications, and careful reasoning about core vs. valence electrons is essential.

Which one of the following ions has the ground-state electron configuration [Xe]4f145d10?

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