Electron Configuration

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Electron Configuration

Postby WUng_1D » Sun Oct 20, 2019 9:32 pm

Can someone explain to me why an element such as Scandium ([Ar]3d14s2) has the 3d orbital come before the 4s orbital?

Harry Zhang 1B
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Re: Electron Configuration

Postby Harry Zhang 1B » Sun Oct 20, 2019 9:39 pm

Normally, the order of electron-filling takes the following sequence: 1s 2s 2p 3s 3p 4s 3d.... However, when the electrons contain more than 20 electrons, that is, after potassium starting with scandium, the 4s orbital is complete and electrons start going into the 3d orbital but once there is electron in the 3d orbital, for some reason in the quantum world, the 3d electron becomes lower energy and therefore is placed before the 4s electron. This rule is true for all atoms having more than 20 electrons in the subsequent period.

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Re: Electron Configuration

Postby ABombino_2J » Sun Oct 20, 2019 9:41 pm

The 3d orbital has less energy than the 4s orbital so it must come before because electron configurations are written in order based on amounts of energy.

Chris Tai 1B
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Re: Electron Configuration

Postby Chris Tai 1B » Sun Oct 20, 2019 10:12 pm

You can also think of this in terms of valence electrons. The 4s shells will contain electrons that are more likely to be lost, thus ionizing a particular atom. Since it's more probable for a 4s electron to be given up by an atom than a 3d electron, the 3d shell should come first in the sequence. This makes it easier to write ions too, so for instance

Zn: [Ar] 3d^10 4s^2
Zn^2+: [Ar] 3d^10

Michelle N - 2C
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Re: Electron Configuration

Postby Michelle N - 2C » Tue Oct 22, 2019 9:46 pm

When the d-orbital is not full, they are generally lower in energy. Plus, it would then follow the trend and order of the numbers.

Sorry this is vague, but that's how I was able to get it..

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