On the last problem set, we determined that Fe3+ could have three possible confi

Question

On the last problem set, we determined that Fe3+ could have three possible configurations: 4s2-3d3, 4s13d4, or 3d5. Here you will figure out which one is likely the correct ground state. Let's do it one step at a time, starting with the configuration 3d3 since an Fe3+ ion must have at least three 3d electrons. If an electron is added to this d3 ion, will it occupy a 4s orbital or a 3d orbital? Answer this question by calculating the energy of the electron in each case, using Slater's rules, -(Z*)2/(n*)2. The electron will occupy the more stable orbital, the one with the more negative energy. Now add the second electron, to the ion whose configuration you have just determined. Follow the same procedure as in part (a) to determine if this electron occupies a 4s or a 3d orbital.

Explanation / Answer

slater energy rule gives -Z^2/16 for 4th orbit and -z^2/9 for 3rd orbit so Fe3+ is [Ar]3d5

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