A) \[+\,4;\,1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}\]
B) \[+\,2;\,1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{2}}\]
C) \[+\,3;\,1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{1}}\]
D) \[+\,6;\,1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\]
Correct Answer: D
Solution :
The oxidation number of sulphur in \[{{\text{H}}_{\text{2}}}\text{S}{{\text{O}}_{\text{4}}}\] is \[(2\times 1)+x+(4\times -2)=0\] \[\therefore \] \[2+x+(-8)=0\] \[\therefore \] \[x=8-2=+\,6\] The electronic configuration of sulphur \[16S=1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{4}}\] Electronic configuration of S in \[{{\text{H}}_{\text{2}}}\text{S}{{\text{O}}_{\text{4}}}\] \[16-6=10,\] \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\]
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