[ 3 / biz / cgl / ck / diy / fa / ic / jp / lit / sci / vr / vt ] [ index / top / reports ] [ become a patron ] [ status ]
2023-11: Warosu is now out of extended maintenance.

/sci/ - Science & Math

View post   
File: 7 KB, 400x300, 1325124313492.png [View same] [iqdb] [saucenao] [google]
4240402 No.4240402 [Reply] [Original]

Hello /sci/ i wonder if you can help me.

I'm not in school or anything so this is not homework. Anyways i have always been fascinated with the thought of atoms and such so i decided to educate myself a wee bit. I know its very basic chemistry but i'm a little confused.

1s2 2s2 2p6 3s2 3p6 3d5 4s1 is the electronic structure of Chromium. I know that usually the 4s orbital would get filled before the 3d orbitals but not in this case.

At this point '1s2 2s2 2p6 3s2 3p6' there a six electrons yet to find their homes.

My question is, has one of the electrons been taken from the 4s orbital and shared with the 3d orbitals, as to fill them up with one each?

I apologize if this is a stupid question.

>> No.4240590

special relativity (and chemistry is not a true science yet)
http://en.wikipedia.org/wiki/Electron_configuration#Other_exceptions_to_Madelung.27s_rule

>> No.4240594

>>4240590
Chemistry is the new Biology.

>> No.4240601

>>4240594

> Chemistry is the new Biology.
Fuck, thyself.

>> No.4240610

Yes, there are exceptions! Chromium does that in order to be stabilized.

>> No.4240613

>>4240601
I'm majoring in Chemistry myself and I think that's funny.

>> No.4240673

OP here. Thanks for the replies fellas.

>> No.4240706

It's a good question.

Half filled orbitals are more stable than not and filled orbitals more stable (lower in energy) still.
The reason a 4s shell electron and a 3d electron can swap places is because they're very close together (energy wise).

>> No.4240721

>>4240706
Cheers chap. Also copper is another exception, am i right? But this time maxing up those d orbitals, 3d10 4s1?

>> No.4240800
File: 1.58 MB, 2200x2000, wave function orbitals.png [View same] [iqdb] [saucenao] [google]
4240800

>>4240721

Bingo.

Take a look at this though (we haven't properly looked at the 2nd row transition metals in Uni yet) but:

Y: 4d1 5S2
Zr: 4d2 5S2
Nb: 4d4 5S1

Apparently for a Niobium atom, it's more stable to have 4 electrons in the d subshell, and a half filled s shell, than to have all 5 in a half filled d subshell.

The d orbitals are quite complex though - as you're teching yourself, you should look at the mathematical models from the Schrodinger equation etc which show the spaces where electrons occupy (giving us a 3d model of the orbital.)

S orbitals are spheres; P orbitals are like dumbbells and there are 5 d orbitals shaped like 3 Xs, a + and a crazy thing lol (dZ^2).
Also to learn: Atomic orbitals vs Molecular orbitals (s,p,d and f orbitals are 'atomic' and they overlap to form 'molecular' orbitals (bonds) called sigma, pi etc

If it gets a bit complicated, back up a step. As a chemfag, i'm afraid i have nothing but love for this kind of stuff.

>> No.4240824

>>4240800
Also, check out that Technetium to Ruthenium jump:

Tc: 4d5 5s2
Ru: 4d7 5s1

Obviously we can conclude that the 4d shell is more stable than the 5s shell, so electrons being in the lower energy shell makes the atom altogether more stable.

>> No.4240917

>>4240800
>>4240824
Sorry i was away making food.

Thanks for all this info. This is great.

I grew up in Salford, nicknamed little beirut and only came away with a C in Gcse, science. I'm an idiot for not trying harder, i hate myself for it.

But its never too late i suppose. This stuff does look a little too strong at the moment though. Still i'm completed fascinated by it. Thanks again mate.