Hi Nayi, your electron configuration is correct. This ion will be diamagnetic because it has no unpaired electrons. In some cases this can depend on the enviroment the ion is in; for example, the type of "ligands" bound to certain transition metal ions can give "high spin" vs. "low spin" d-electron configurations, a topic of transition metal coordination compounds. But here all of the atomic orbitals have two electrons paired in them, including the seven 4f and five 5d orbitals, so there are no "odd" electrons without a "partner". A neutral thallium atom, [Xe] 4f14 5d10 6s2 6p1, would be paramagnetic because it has an odd electron in one of the 6p orbitals.
>> type of electronic configuation... how do I do that? <<
I'm not sure what they're asking for there, possibly that this is a ground state configuration, not an excited state configuration.
Steve
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