Arrange the following as increase in oxidation number (i)${Mn}^{2 +}\$ (ii)${\ MnO}_{2}$ (iii) ${KMnO}_{4}$ (iv) $K_{2}{MnO}_{4}$

Question

Dr. Abubacker · Accepted Answer

(b)
Oxidation state of Mn in ${Mn}^{2 +} = + 2$
Let oxidation state of Mn in ${MnO}_{2} = x$
$\ 	herefore$ $x + (2 	imes - 2) = 0$
$\ 	herefore$ $x =$+4
$(iii)\ \ \ Let\ the\ oxidation\ state\ of\ Mn\ in\ K{MnO}_{4} = x$
$	herefore$ $+ 1 + x + ( - 2 	imes 4) = 0$
$\ \ 	herefore\ \ \ x = + 7$
(iv) Let oxidation state of Mn in $K_{2}{MnO}_{4} = x$
$	herefore\ \ \ \ ( + 1 	imes 2) + x + ( - 2 	imes 4) = 0$
$	herefore\ \ \ x = + 6$
$	herefore\ \ \$Increasing order of oxidation states is
$(i) < (ii) < (iv) < (iii)$

Q. Arrange the following as increase in oxidation number (i)${Mn}^{2 +}\$ (ii)${\ MnO}_{2}$ (iii) ${KMnO}_{4}$ (iv) $K_{2}{MnO}_{4}$

Explanation

Reviewed by Dr. Abubacker

Want more practice?