What is a disproportionation reaction? Give an example.
(N/A) disproportionation reaction is a special type of redox reaction in which the same element in a single species is simultaneously oxidized and reduced.
Example: The reaction of white phosphorus $(P_4)$ with sodium hydroxide $(NaOH)$ to form phosphine $(PH_3)$ and sodium hypophosphite $(NaH_2PO_2)$.
$P_4 + 3NaOH + 3H_2O \rightarrow PH_3 + 3NaH_2PO_2$
In this reaction,the oxidation state of phosphorus changes from $0$ in $P_4$ to $-3$ in $PH_3$ (reduction) and to $+1$ in $NaH_2PO_2$ (oxidation).
Example: The reaction of white phosphorus $(P_4)$ with sodium hydroxide $(NaOH)$ to form phosphine $(PH_3)$ and sodium hypophosphite $(NaH_2PO_2)$.
$P_4 + 3NaOH + 3H_2O \rightarrow PH_3 + 3NaH_2PO_2$
In this reaction,the oxidation state of phosphorus changes from $0$ in $P_4$ to $-3$ in $PH_3$ (reduction) and to $+1$ in $NaH_2PO_2$ (oxidation).
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Similar Questions
Manganese $(VI)$ has the ability to disproportionate in an acidic solution. The difference in oxidation states of the two ions it forms in an acidic solution is $...... .$
Which species among the following does not show disproportionation reactions?
Which of the following are disproportionation reactions?
$(A)$ $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$
$(B)$ $2 H_2O_2 \rightarrow 2 H_2O + O_2$
$(C)$ $2 KMnO_4 \rightarrow K_2MnO_4 + MnO_2 + O_2$
$(D)$ $3 MnO_4^{2-} + 4 H^+ \rightarrow 2 MnO_4^- + MnO_2 + 2 H_2O$
$(A)$ $Cl_2 + 2 NaOH \rightarrow NaCl + NaOCl + H_2O$
$(B)$ $2 H_2O_2 \rightarrow 2 H_2O + O_2$
$(C)$ $2 KMnO_4 \rightarrow K_2MnO_4 + MnO_2 + O_2$
$(D)$ $3 MnO_4^{2-} + 4 H^+ \rightarrow 2 MnO_4^- + MnO_2 + 2 H_2O$
Which of the following compounds undergoes disproportionation in the presence of $SO_3$ gas?
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