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Topic: Electron configuration question and EXCEPTIONS  (Read 5563 times)

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WESIDA

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Electron configuration question and EXCEPTIONS
« on: November 01, 2005, 11:22:53 AM »
so i have just taken this quiz and i got one of them wrong. i was supposed to write the config for (Cr) and this is wha ti did
1s2 25s 2p6 3s2 3p6 4s2 3d4
technically this is right but what my teacher did was for the last S and D orbitals she took 1 S electron and let it go to the Do orbital making it become
4s1 3d5
My question is why does that happen, are there special atoms that do this like the Cr? is it to make the element more reactive by having electrons unpaired?
thanks alot
MHB
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Offline Winga

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Re:Electron configuration question and EXCEPTIONS
« Reply #1 on: November 01, 2005, 11:45:28 AM »
For maximum multiplicity. (Hund's rule)
Half-filled sub-shells, extra stability.

http://en.wikipedia.org/wiki/Hund's_rule
« Last Edit: November 01, 2005, 11:47:56 AM by Winga »
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Offline jdurg

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Re:Electron configuration question and EXCEPTIONS
« Reply #2 on: November 01, 2005, 12:30:14 PM »
Yes, there are a few 'oddities' like that in the periodic table which you basically just have to remember.  Chromium is one of them, and as you move further down you start finding more and more.
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Offline Albert

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Re:Electron configuration question and EXCEPTIONS
« Reply #3 on: November 01, 2005, 12:41:13 PM »
Quote from: jdurg on November 01, 2005, 12:30:14 PM
Yes, there are a few 'oddities' like that in the periodic table which you basically just have to remember.  
Namely Cr, Cu, Ag and Au.

Cu: [Ar] 4s1 3d10
Ag: [Kr] 5s1 4d10
Au: [Xe] 6s1 5d10 4f14
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Offline jdurg

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Re:Electron configuration question and EXCEPTIONS
« Reply #4 on: November 01, 2005, 01:01:53 PM »
As well as platinum, many of the lanthanides, actinides, etc. etc.
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WESIDA

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Re:Electron configuration question and EXCEPTIONS
« Reply #5 on: November 01, 2005, 04:08:34 PM »
alright thanks guys for the info
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