Transition metals have incomplete d-orbitals, allowing electrons to be lost from both the outer s and inner d shells, creating variable states. Manganese, with its particular electron configuration of 3d5 4s2, can sacrifice electrons all the way from +2 to +7 because that half-filled d-subshell offers extra stability at certain points. In my lab, we torture manganese oxides in lithium-ion batteries, watching them shift states with each charge cycle. But frankly, the widest range isn't the most useful; stability is. I’d trade manganese’s showy range for cobalt’s predictable discharge any day, just as I’d trade this frantic Bangalore innovation for my father’s simple, reliable shop ledger.
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