2.43 6th Edition

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Edward Suarez 1I
Posts: 75
Joined: Fri Sep 28, 2018 12:27 am

2.43 6th Edition

Postby Edward Suarez 1I » Sat Nov 03, 2018 1:29 pm

Hi, so I had a few questions about this problem:
What is the ground-state electron con guration expected for each of the following elements: (a) silver; (b) beryllium;
(c) antimony; (d) gallium; (e) tungsten; (f) iodine?

so particularly, a) the ground state is [Kr] 3d^10 4s^1 instead of [Kr] 3d^9 4s^2, and to my understanding its because it's more stable to have the d orbital filled/half filled. However, how come for e) tungsten, the configuration is not [Xe] 4f^14 5d^5 6s^1? (if half/full filled is a more stable configuration)

thank u!

Hannah Morales 1D
Posts: 31
Joined: Fri Sep 29, 2017 7:06 am

Re: 2.43 6th Edition

Postby Hannah Morales 1D » Sun Nov 04, 2018 11:57 am

a) it would actually be [Kr} 4d^10 5s^1 because it is in the second row of the transition metals ( d orbital section)
your understanding of this concept however is correct in that it is more stable when it is half filled/ filled.

e) it is because the pairing energy is less than the energy required to put the 6th electron into a higher energy level.

I don't think that a question on the midterm will ask for tungsten though or any element beyond the 3rd row though!

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