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

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

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

Solution:

$\underline{\mathrm{C}} \mathrm{H}_{3} \underline{\mathrm{C}} \mathrm{OOH}$

\mathrm{C}_{2}^{\mathrm{x}}+1_{4} \mathrm{O}_{2}

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

Oxidation no. of $0=-2$

Oxidation no. of $\mathrm{H}=+1$

Then,

$2(x)+4(+1)+2(-2)=0$

$2 x+4-4=0$

$x=0$

Therefore, average oxidation no. of $C$ is 0 . Both the carbon atoms are present in different environments so they

cannot have same oxidation no. Therefore, carbon has oxidation no. of $+2$ and _2 in $\mathrm{CH}_{3} \mathrm{COOH}$ .

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