A) \[\text{KMn}{{\text{O}}_{\text{4}}}\]
B) \[{{\text{K}}_{\text{2}}}\text{Mn}{{\text{O}}_{\text{4}}}\]
C) \[\text{M}{{\text{n}}_{\text{2}}}{{\text{O}}_{\text{3}}}\]
D) \[\text{Mn}{{\text{O}}_{\text{2}}}\]
Correct Answer: A
Solution :
Let the oxidation state of Mn is \[x.\] \[KMn{{O}_{4}}\] \[+1+x+(-2)\times 4=0\] \[x-7=0\] \[x=+7\] \[{{K}_{2}}Mn{{O}_{4}}\] \[(+1)\times 2+x+(-2)\times 4=0\] \[x-6=0\] \[x=+\,6\] \[M{{n}_{2}}{{O}_{3}}\] \[x\times 2+(-2)\times 3=0\] \[2x=+\,6\] \[x=+\,3\] \[Mn{{O}_{2}}\] \[x+(-2)\times 2=0\] \[x=+\,4\] Thus, oxidation state of Mn is highest in \[KMn{{O}_{4}}.\]
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