A recently discovered element, 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.