A recently discovered element, $\mathrm{T}$, with an atomic number of 135 , forms a complex ion, T3+. This ion demonstrates an exceptional degree of stability, contrary to expectations for such a high atomic number. Advanced spectroscopic analysis suggests the presence of a half-filled subshell with a unique electron configuration. Given the known principles of quantum chemistry and electron configuration, which of the following best explains the stability of the T3+ ion? Options: a) T3+ achieves a pseudo-noble gas configuration with a completely filled f-subshell. b) The ion exhibits a special stability due to a half-filled g-subshell. c) T3+ stabilizes through a symmetrical distribution of electrons in d-orbitals, resembling a transition metal ion. d) The ion achieves stability by a rare configuration involving a half-filled p-subshell and partially filled $d$ and $f$ subshells.

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***B*** ∻Key Concept∻ ⚹Half-filled subshells and stability⚹ ∻Explanation∻ ⚹Atoms and ions with half-filled subshells often exhibit enhanced stability due to the symmetrical distribution of electrons and exchange energy, which is also applicable to the hypothetical g-subshell for element T with an atomic number of 135.⚹◊What is the electron configuration of the T3+ ion?⍭ Generate me a similar question◊

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