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Electron Configuration for 1st row transition metals

Posted: Wed Jul 10, 2019 5:08 pm
by Karina Vasquez 1D
Are the only special cases when completing ground state electron configuration Cu and Cr or is it all of the first row of transition metals?

Re: Electron Configuration for 1st row transition metals

Posted: Wed Jul 10, 2019 7:37 pm
by Chem_Mod
The special cases when completing ground state electron configurations are Cu and Cr. Its not all of the first row of transition metals.

Re: Electron Configuration for 1st row transition metals

Posted: Thu Jul 11, 2019 9:26 am
by Leah farhadi 1F
In addition, those metals below Cu and Cr follow the same pattern, where the row beginning with Cu is nd^5ns^1 and the row beginning with Cr is nd^10ns^1.

Re: Electron Configuration for 1st row transition metals

Posted: Thu Jul 11, 2019 4:29 pm
by Brian Kwak 1D
For the purposes of this course you only need to know Cu and Cr, but all the elements in those rows show the same pattern because it is more stable for the elements to be either have all the d orbital filled with electrons or half filled.

Re: Electron Configuration for 1st row transition metals

Posted: Fri Jul 12, 2019 2:40 pm
by Karina Vasquez 1D
Ok thank you! Also, should we know/memorize the exceptions of ionic charges for transitional metals?

Re: Electron Configuration for 1st row transition metals

Posted: Fri Jul 12, 2019 7:30 pm
by Karolina herrera1F
The only cases are just Cu and Cr because in these cases, a completely full or half full d sub-level is more stable than a partially filled d sub- level, so an electron from the 4s orbital is excited and rises to a 3d orbital.

Re: Electron Configuration for 1st row transition metals

Posted: Sun Jul 14, 2019 4:38 pm
by simmoneokamoto3K
Cu and Cr are both special cases and the only special cases in that row. Basically, because Cu's configuration is 3d^9 and 4s^2, the 3d^9 steals an electron from 4s^2 turning it into 4d^10 and the same thing with Cr.