Question
Explain Catalytic property of transition element.
✓
Answer
$\rightarrow$ The transition metals and their compounds are known for their catalytic activity.
$\rightarrow$ This activity is ascribed to their ability to adopt multiple oxidation states and to form complexes.
$\rightarrow$ Vanadium $(V)$ oxide $($in Contact Process$),$ finely divided iron $($in Haber's Process$),$ and nickel $($in Catalytic Hydrogenation$)$ are some of the examples.
$\rightarrow$ Catalysts at a solid surface involve the formation of bonds between reactant molecules and atoms of the surface of the catalyst $($first row transition metals utilise $3d$ and $4s$ electrons for bonding$)$.
$\rightarrow$ This has the effect of increasing the concentration of the reactants at the catalyst surface and also weakening of the bonds in the reacting molecules $($the activation energy is lowering$)$.
$\rightarrow$ The Transition metal ions can change their oxidation states, they become more effective as catalysts.
$\rightarrow$ For example, iron $(III)$ catalyses the reaction between iodide and persulphate ions. $
\ce{2I^{-}+ S_2O_8^{2-}\rightarrow I _2+2SO_4^{2-}}$
$\rightarrow$ An explanation of this catalytic action can be given as :
$ \begin{array}{l} \ce{2Fe^{3+}+2 I^{-} \rightarrow 2Fe^{2+}+ I_2} \\ 2\ce{Fe^{2+}+ S_2 O_8^{2-} \rightarrow 2Fe^{3+}+2SO_4^{2-}} \end{array}$
$\rightarrow$ This activity is ascribed to their ability to adopt multiple oxidation states and to form complexes.
$\rightarrow$ Vanadium $(V)$ oxide $($in Contact Process$),$ finely divided iron $($in Haber's Process$),$ and nickel $($in Catalytic Hydrogenation$)$ are some of the examples.
$\rightarrow$ Catalysts at a solid surface involve the formation of bonds between reactant molecules and atoms of the surface of the catalyst $($first row transition metals utilise $3d$ and $4s$ electrons for bonding$)$.
$\rightarrow$ This has the effect of increasing the concentration of the reactants at the catalyst surface and also weakening of the bonds in the reacting molecules $($the activation energy is lowering$)$.
$\rightarrow$ The Transition metal ions can change their oxidation states, they become more effective as catalysts.
$\rightarrow$ For example, iron $(III)$ catalyses the reaction between iodide and persulphate ions. $
\ce{2I^{-}+ S_2O_8^{2-}\rightarrow I _2+2SO_4^{2-}}$
$\rightarrow$ An explanation of this catalytic action can be given as :
$ \begin{array}{l} \ce{2Fe^{3+}+2 I^{-} \rightarrow 2Fe^{2+}+ I_2} \\ 2\ce{Fe^{2+}+ S_2 O_8^{2-} \rightarrow 2Fe^{3+}+2SO_4^{2-}} \end{array}$
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