$_{24} C r - [A r] 3 d^{5} 4 s^{1}$
$_{29} C u - [A r] 3 d^{10} 4 s^{1}$
Why chromium and copper exhibits such electronic configuration ?

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Solution

$Electron orbitals are most stable when they are fully filled or half-filled.$ In the case of Chromium, and Copper after the $4 s^{2}, 3 d^{4} a n d 4 s^{2}, 3 d^{9}$ respectively configuration is attained, an electron from the $4 s$ orbital jumps to $3 d$ subshell because $3 d^{5} a n d 3 d^{10}$ is a much more stable configuration than $3 d^{4} a n d 3 d^{9}$ . That's why chromium and copper exhibits such electronic configuration

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3 d^{5} 4 s^{1}

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