We all know that half filled atomic orbitals and fully filled atomic orbitals are more stable and that's why in the electronic configuration of several elements in periodic table violate Aufbau principle for example the electronic configuration of chromium is [Ar]4s 1 3d 5. The electronic configuration of Carbon is 1s 2 2s 2 2p 2 . So why is it not 1s 2 2s 1 2p 3 as both 2s and 2p orbitals will be half filled accounting for greater stability of carbon atom?

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Suraj Prasad · Answer

See, the electronic transition will take place only when it will get oppurtunity to do it. If you see the size of 2S and 4S , 4S is away from nucleus as compared to 2S, hence electronic transition is possible there which do not happens for 2S like you said in carbon.

Pritesh Ramya · Answer

But in chromium atom how is this possible that there is a transition of electron from 4s to 3d orbitals as there will be lots of energy difference

Suraj Prasad · Answer

The difference of energy will obviously be there between 4s and 3d but dear imp thing is that its getting more stabilised by doing so . I hope you know about exchange energy which happens due to transitions. The more the stabilisation energy and more symmetrical it is, more will be the stability .
And always remember evrything not only in chemistry but also in universe will tend towards stability wherever its possible. :)

Pritesh Ramya · Answer

So you are saying that even if the atoms have to lose more energy and get stabilisation in return they will do so so why not carbon does so

Suraj Prasad · Answer

I told dear that in lower atoms like you are saying carbon, 2s shell is very close to nucleus and hence its difficult to do the transition . 4 s is more far as compared to 2s

Pritesh Ramya · Answer

Thank you very much for giving your precious time. Thanks again please answer my other questions as soon as this one was answered.

Suraj Prasad · Answer

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HETAV PATEL

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