2A #5

Malia Shitabata 1F
Posts: 127
Joined: Sat Aug 17, 2019 12:17 am

2A #5

Give the ground state electron configuration for Cu+ ion. The solutions manual says the answer is [Ar]3d^10 but I wrote out the full electron configuration as $1s^22s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{8}$ which still has the same number of electrons. Am I still right even though they end on two different 3d terms or did I do it wrong? And when are we supposed to use the abbreviated electron configuration using noble gases?

WesleyWu_1C
Posts: 117
Joined: Thu Jul 25, 2019 12:16 am

Re: 2A #5

You unfortunately did it wrong. Always remove electrons in the outermost energy level, which in this case is the 4s orbital. We know the original e- configruation is [Ar] 3d^10 4s^1, so when it become Cu^1+, the one electron in the 4s is removed, leaving behind an e- configuration of [Ar] 3d^10.

I think you just use the abbreviated on to make it easier on everyone.

Malia Shitabata 1F
Posts: 127
Joined: Sat Aug 17, 2019 12:17 am

Re: 2A #5

Thanks! And do we always write the 3 level before the 4 because I thought it was only for chromium and copper?

Justin Sarquiz 2F
Posts: 106
Joined: Fri Aug 30, 2019 12:15 am

Re: 2A #5

Yes always write the 3 before the 4 subshell because the 4th subshell has slightly higher energy than the 3 subshell. The Chromium and Copper exception refers to the fact that these elements grab one electron from the p subshell to make Chromium have all half full d5 subshell. Copper grabs one electron from the p subshell in order to have a full d10 subshell. Therefore, Chromium is [Ar] 3d^5 4s^1 and Copper is [Ar] 3d^10 4s^1.

Justin Sarquiz 2F
Posts: 106
Joined: Fri Aug 30, 2019 12:15 am

Re: 2A #5

Sorry I meant to say that Chromium and Copper takes 1 electron from the s subshell not the p subshell.

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