Chemistry, asked by sahilcool5341, 1 year ago

Suggest why chromium prefers d5 configuration

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Answered by Sweetbuddy
3
Hey buddy here is ur answer !!!

Hund's principle states that when electrons start filling up subshells (like the 3d or 4s subshell) they do so in such a way that electrons of the same spin must solely occupy the orbitals within the subshell first. Then electrons of opposite spin will start filling up the remaining space in the orbitals.

It's hard to understand this without diagrams. So see the pictures below-

If you are still confused, watch video in youtube -

Ok! Electron orbitals are most stable when they are fully filled or half filled. So the most stable configuration for the 3d subshell is 3d10 or 3d5.

In the case of Chromium, after the 4s2 3d4 configuration is attained, an electron from the 4s orbital jumps to 3d subshell because 3d5 is a much more stable configuration than 3d4. That's why final configuration for Chromium is 4s1 3d5.

In the case of Vanadium, just the usual Aufbau principle applies.

HOPE U GOT WHAT I AM EXPLAINING !!

^_^

》》》》》》BE BRAINLY《《《《《《
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Answered by HemaMuniyappan
0

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hope it helps !!!✌️✌️✌️

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