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 \[{{H}_{2}}S{{O}_{4}}\] is \[(2\times 1)+x+(4\times -2)=0\] \[\therefore \] \[2+x+(-8)=0\] \[\therefore \] \[x=8-2=+6\] The electronic configuration of sulphur \[_{16}S=1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{4}}\] Electronic configuration of S in \[{{H}_{2}}S{{O}_{4}}\] \[16-6=10,\] \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\]
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