Hi, this should be relatively simple but I'm struggling to understand the reasoning behind the correct answers for this problem:
Give the ground-state electron configuration expected for each of the following ions:
a) Cu+
b) Bi3+
c) Ga3+
d) Tl3+
I got [Ar] 4s23d8 for both a and c, and [Xe]4f146s25d8. I followed the basic rules of determining configuration because I didn't think there were any exceptions. Can someone please explain why I'm wrong and why the right solutions are correct?
2A5
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Re: 2A5
Postby Ananta3G » Tue Nov 05, 2019 11:54 am
Hi! These ones can be a bit tricky. Cu is an element with an exception where having a fully filled 3d shell is more stable so instead of the original electron configuration being [Ar] 3d9 4s2, it is [Ar] 3d10 4s1. Thus, when you make Cu+ you take away the electron in the 4s1 position leaving us with [Ar] 3d10. For Bi, the electron configuration is [Xe] 6s2 4f14 5d10 6p3 meaning you take away the 3 electrons from 6p3 to get the electron configuration of Bi 3+ is [Xe] 4f14 5d10 6s2. Ga is [Ar] 3d10 4s2 4p1 so for Ga 3+ it would only be [Ar] 3d10 because you take the 3 electrons away from the now highest levels 4s2 and 4p1. I hope this explanation helps! Just try writing the whole configuration out, seeing which one is the highest energy level, and remember that Cr and Cu are exceptions to Hund's rules because it is more stable to have a 1/2 or fully filled d shell than a fully filled s2 shell. :)
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