When potassium permanganate (KMnO_4) is heate | vedclass

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(C) The thermal decomposition of potassium permanganate $(KMnO_4)$ at $513 \ K$ is given by the following reaction:$2KMnO_4 \xrightarrow{\Delta} K_2Mn

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Paramagnetic and green

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(C) The thermal decomposition of potassium permanganate $(KMnO_4)$ at $513 \ K$ is given by the following reaction:$2KMnO_4 \xrightarrow{\Delta} K_2MnO_4 + MnO_2 + O_2 \uparrow$In the products,the oxidation states of manganese are:$K_2MnO_4$: $Mn$ is in $+6$ oxidation state.$MnO_2$: $Mn$ is in $+4$ oxidation state.The product with the higher oxidation state is $K_2MnO_4$ $(Mn^{+6})$.The electronic configuration of $Mn^{+6}$ is $[Ar] 3d^1 4s^0$.Since it has one unpaired electron,it is paramagnetic.$K_2MnO_4$ is known to have a characteristic green colour.Therefore,the product with the higher oxidation state $(Mn^{+6})$ is paramagnetic and green.

When potassium permanganate $(KMnO_4)$ is heated at $513 \ K$,it decomposes to form two manganese-based products. The physical properties of the product in which manganese has a higher oxidation state than the other are:

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