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The electronic configuration of sulphur is:(A)- ${\text{K}}\left( {\text{2}} \right){\text{,L}}\left( {\text{8}} \right){\text{,M}}\left( {\text{6}} \right)$(B)- ${\text{K}}\left( {\text{2}} \right){\text{,L}}\left( {\text{8}} \right){\text{,M}}\left( 8 \right)$(C)- ${\text{K}}\left( {\text{2}} \right){\text{,L}}\left( 6 \right)$(D)- ${\text{K}}\left( {\text{2}} \right){\text{,L}}\left( {\text{8}} \right)$

Last updated date: 13th Jun 2024
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Hint: For showing the electronic configuration of any atom, first of all we should know about the total number of electrons present in that atom. And the number of electrons in an atom is always equal to the Atomic Number of that atom.

In the periodic table Sulphur is denoted as ${}_{{\text{16}}}^{{\text{32}}}{\text{S}}$, where upper quantity displays the atomic mass (${\text{A}}$) of the sulphur and lower quantity displays the atomic number (${\text{Z}}$).
i.e. Atomic Number (${\text{Z}}$) = No. of electrons = No. of protons
-From ${}_{{\text{16}}}^{{\text{32}}}{\text{S}}$ it is clear that, atomic number of sulphur is 16 and total number of electrons present in sulphur is also 16.
${\text{1}}{{\text{s}}^{\text{2}}}{\text{,2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{,3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{4}}}$
-From above configuration it is clear that total two electrons are present in innermost or 1st shell, eight electrons are present in the 2nd shell ($2 + 6$) and six electrons ($2 + 4$) are present in the 3rd shell after nucleus of the sulphur atom.