I feel so stupid!

[topdent1]

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I can't believe i got this question wrong. I still don't understand it.

What is the correct electron configuration for Zn2+? Seems easy right? My answer was [Ar] 4s2, 3d8.

However, the correct answer is [Ar] 4s0, 3d8. Why does Zn lose electrons from the s subshell first? I feel so stupid!

 

[Mamona]

You need to remember that 4s subshell comes first than 3d....

 

[TeamGuo]

You need to remember that 4s subshell comes first than 3d....

That's not the reason for this problem.

OP's answer is wrong I believe, maybe it's a typo. You mean the answer should be 4s03d10. not = 4s03d8

you are missing 2 electrons for Zn2+.

Anyways, the reason is because it's more likely to loose 2 electrons from the s orbtial then d orbitals, since you can keep the d orbitals full if you just take 2 electrons away from the s orbital. Hence, it's more favorable.

 

[doc3232]

Reminds me of a question:
Can someone please list out the Elements that will take electrons from s and put in d to make a half filled or filled d subshell??

Thanks in advance
Please do list them all.

 

[topdent1]

That's not the reason for this problem.

OP's answer is wrong I believe, maybe it's a typo. You mean the answer should be 4s03d10. not = 4s03d8

you are missing 2 electrons for Zn2+.

Anyways, the reason is because it's more likely to loose 2 electrons from the s orbtial then d orbitals, since you can keep the d orbitals full if you just take 2 electrons away from the s orbital. Hence, it's more favorable.

Alright...but why is it more favorable to have a full d orbital vs. a full s orbital? And you are right, that was a typo its supposed to be 4s03d10.

 

[Optimism Smiles]

Reminds me of a question:
Can someone please list out the Elements that will take electrons from s and put in d to make a half filled or filled d subshell??

Thanks in advance
Please do list them all.

I'm not sure about them ALL...but I do know Cr and Cu are two!

 

[tuthluver]

I'm not sure about them ALL...but I do know Cr and Cu are two!

It's all of the transition metals. This is known as Hund's Rule:
http://upload.wikimedia.org/wikipedia/commons/d/dd/Electron_configuration_order.gif

 

[TeamGuo]

Alright...but why is it more favorable to have a full d orbital vs. a full s orbital? And you are right, that was a typo its supposed to be 4s03d10.

actually, you are not comparing the full d orbital vs. s orbital. Take a look at

4s2 3d8. You have 2 of the d-orbitals half-filled, Vs. if you let the 2 electrons to be taken away from s orbital, all of the d-orbitals are filled.

This is a general rule, orbitals likes to be either filled or half-filled, this is energetically more favorable.

For electron configuration, just watch out for Cr and Cu, they always give you an ionic form of these metals, where you have to take the 4s electrons first before taking the 3d electrons.

 

[klutzy1987]

Reminds me of a question:
Can someone please list out the Elements that will take electrons from s and put in d to make a half filled or filled d subshell??

Thanks in advance
Please do list them all.

Im am not typing them all, but all elements that are in group 4B and 9B will shift up one and fill their 3D5 and 3d10 orbitals and have a 4s1. That the rule you need to know. Also 4s orbitals gie up their electrons more easily than the 3d subshell. Therfore ions first will lose their 4s electrons and then their 3d electrons.