What is the electronic configuration of Chromium in $[Cr ({NH}_{3})_{6}]^{3 +}$ ?

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Solution

Electronic configuration:
It is defined as the distribution of electrons of an atom in an atomic orbital.
The general notation of electronic configuration is $s^{a} p^{b} d^{c}$ where $s, p,$ and $d$ represents the subshell and $a, b$ and $c$ represents the number of electrons present in the subshell as superscript.
Atomic number:
The symbol of Chromium is $C r$ .
Atomic number of Chromium is $24$ which is a transition element and it belongs to $4^{t h}$ period and $6^{t h}$ group of periodic table.
As the atomic number is equal to the number of electrons present in a neutral element. So, the number of electrons are $24$ .
The electronic configuration of Chromium should be $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{4}$ .
But as we know that the half-filled and fully filled electronic configuration are more stable. So, one electron is transferred from $4 s$ orbital to $3 d$ orbital.
Thus, the electronic configuration of Chromium is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1} 3 d^{5}$ .
The electronic configuration of Chromium in noble gas notation is represented as $[A r] 3 d^{5} 4 s^{1}$ where $[A r]$ represents the inert core of Argon which is a noble gas and $3 d^{5} 4 s^{1}$ represents the valence shell electronic configuration of Chromium.
Hence, the electronic configuration of Chromium is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1} 3 d^{5}$ or $[A r] 3 d^{5} 4 s^{1}$ .

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The electronic configuration of chromium in [Cr(NH₃)₆]³⁺ is:

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