Oxidation no. of $P$ in ${{\rm{H}}_4}{{\rm{P}}_2}{{\rm{O}}_5},{{\rm{H}}_4}{{\rm{P}}_2}{{\rm{O}}_6},{{\rm{H}}_4}{{\rm{P}}_2}{{\rm{O}}_7}$ are respectively :

$ + 3,{\rm{ }} + 4,{\rm{ }} + 5$

$ + 3,{\rm{ }} + 5,{\rm{ }} + 4$

$ + 4,{\rm{ }} + 3,{\rm{ }} + 5$

$ + 5,{\rm{ }} + 3,{\rm{ }} + 4$

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JEE CHEMISTRY MCQ: REDOX REACTIONS

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Application +4 | -1

Oxidation no. of

P

{\mathrm{H}_4}{\mathrm{P}_2}{\mathrm{O}_5},{\mathrm{H}_4}{\mathrm{P}_2}{\mathrm{O}_6},{\mathrm{H}_4}{\mathrm{P}_2}{\mathrm{O}_7}

are respectively :

View answer and explanation

Correct option: C

+ 3,\mathrm{ } + 4,\mathrm{ } + 5

Option C (+3, +4, +5) is correct because it accurately calculates the oxidation number of P in each compound based on the standard rules for assigning oxidation numbers.

More Questions from REDOX REACTIONS

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The oxidation number of

\mathrm{H}

in sodium hydride is A reagent, which can decrease the oxidation number of an element, is called Consider the following decomposition reaction

2 \mathrm{KClO}_3 \longrightarrow 2 \mathrm{KCl}+3 \mathrm{O}_2

In the above reaction, Assertion (A):

\mathrm{HNO}_3

acts as oxidizing agent.

Reason (R): Oxidation no. of nitrogen is +5, no increase in oxidation no. beyond +5 can occur. The oxidation no. of

\mathrm{HNO}_3

can only decrease. Assertion :- Bromide ion is serving as a reducing agent in the reaction.

\mathrm{MnO}_4^{-}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{MnO}_2(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+2 \mathrm{OH}^{-}(\mathrm{aq})

Reason :- Oxidation number of

\mathrm{Br}

increases from

-1

+5.

A substance, that by its sharp colour change indicates the completion of reaction is known as :