Question

why copper and chromium have exceptional electronic configuration and give reasons in support your answer abd show expected configuration as well as actual configuration and then explain​

Answer 1

Answer:

To explain :

Why Copper and Chromium have exceptional electronic configurations ?

Explaination:

First let's see the expected and actual electronic configurations of both Chromium and Copper :

Chromium:

$Cr(24) \: : {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {4s}^{2} {3d}^{4}$

But the actual configurations goes as follows :

$\boxed{ Cr(24) \: : {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {4s}^{1} {3d}^{5} }$

The sole reason why Chromium takes up this kind of configurations is because of the very good stability of 3d(5) orbital. Stability arises due to half filled orbital.

Copper :

$Cu(29) \: : {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {4s}^{2} {3d}^{9}$

But the actual configurations goes as follows :

$\boxed{ Cu(29) \: : {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {4s}^{1} {3d}^{10} }$

Similar to the Chromium, copper attains stability due to 3d(10) configuration. Stability arises due to full-fulled d orbital.

Answer 2

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Question :

Why copper and chromium have exceptional electronic configuration .

Solution :

Supposed Electronic Configuration :

$\tt{\purple{ \leadsto{Cu \: = \: [Ar] 4 {s}^{2} 3 {d}^{4}}}}$

$\tt{\red{ \leadsto{Cr \: = \: [Ar] 4 {s}^{2} 3 {d}^{9}}}}$

Actual Configuration :

$\tt{\orange{ \leadsto{Cu \: = \: [Ar] 4 {s}^{1} 3 {d}^{5}}}}$

$\tt{\green{ \leadsto{Cr \: = \: [Ar] 4 {s}^{1} 3 {d}^{10}}}}$

This is because :

Consider the stability of the atom.

3d^5 and 3d^10 are more stable.

Every element prefers to have a stable configuration, so in this case, one electron will shift from S shell to D shell.

...This is called exceptional Configuration...

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