Refer to the periodic table and answer the following questions:
$(a)$ Select the possible non-metals that can show disproportionation reaction.
$(b)$ Select three metals that can show disproportionation reaction.
$(a)$ Select the possible non-metals that can show disproportionation reaction.
$(b)$ Select three metals that can show disproportionation reaction.
(N/A) In disproportionation reactions,one of the reacting substances always contains an element that can exist in at least three oxidation states.
$(a)$ $P, Cl$,and $S$ can show disproportionation reactions as these elements can exist in three or more oxidation states.
$(b)$ $Mn, Cu$,and $Ga$ can show disproportionation reactions as these elements can exist in three or more oxidation states.
$(a)$ $P, Cl$,and $S$ can show disproportionation reactions as these elements can exist in three or more oxidation states.
$(b)$ $Mn, Cu$,and $Ga$ can show disproportionation reactions as these elements can exist in three or more oxidation states.
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Similar Questions
Which of the following does not show a disproportionation reaction?
The $Mn^{3+}$ ion is unstable in solution and undergoes disproportionation to give $Mn^{2+}$,$MnO_2$,and $H^{+}$ ion. Write a balanced ionic equation for the reaction.
Difficult
View SolutionAssign $A, B, C, D$ from the given type of reaction.
$2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$
$2Se_2Cl_2 \xrightarrow{\Delta} SeCl_4 + 3Se$
Medium
View SolutionWhen $Cl_2$ gas is passed through a hot and concentrated solution of $KOH$,which of the following compounds is formed?
Medium
View SolutionObserve the following reaction:
$Cl_{2(g)} + 2OH^{-}_{(aq)} \rightarrow ClO^{-}_{(aq)} + Cl^{-}_{(aq)} + H_2O_{(l)}$
Identify the correct statements about this reaction:
$I$. $Cl_{2(g)}$ is oxidized to $ClO^{-}_{(aq)}$
$II$. $Cl_{2(g)}$ is oxidized to $Cl^{-}_{(aq)}$
$III$. $Cl_{2(g)}$ is reduced to $ClO^{-}_{(aq)}$
$IV$. $Cl_{2(g)}$ is reduced to $Cl^{-}_{(aq)}$
The correct answer is:
$Cl_{2(g)} + 2OH^{-}_{(aq)} \rightarrow ClO^{-}_{(aq)} + Cl^{-}_{(aq)} + H_2O_{(l)}$
Identify the correct statements about this reaction:
$I$. $Cl_{2(g)}$ is oxidized to $ClO^{-}_{(aq)}$
$II$. $Cl_{2(g)}$ is oxidized to $Cl^{-}_{(aq)}$
$III$. $Cl_{2(g)}$ is reduced to $ClO^{-}_{(aq)}$
$IV$. $Cl_{2(g)}$ is reduced to $Cl^{-}_{(aq)}$
The correct answer is:
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