What are the oxidation number of the underlined elements and how do you rationalise your results?$\mathrm{Fe}_{3} \mathrm{O}_{4}$

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What are the oxidation number of the underlined elements and how do you rationalise your results? $\mathrm{Fe}_{3} \mathrm{O}_{4}$

What are the oxidation number of the underlined elements and how do you rationalise your results? $\mathrm{Fe}_{3} \mathrm{O}_{4}$

Solution:

$\mathrm{Fe}_{3} \mathrm{O}_{4}$

Let $x$ be the oxidation no. of Fe.

Oxidation no. of $0=-2$

Then, at that point,

$3(x)+4(- 2)=0$

$3 x-8=0$

$x=\frac{8}{3}$

Oxidation no. can’t be partial.

One of the three particles of Fe has oxidation no. $+2$ and other two particles of Fe has oxidation no. $+3$ .

$\mathrm{F}^{+2} \mathrm{C}_{2} \mathrm{O}, \mathrm{F} \mathrm{F}_{2} \mathrm{O}_{3}$

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