Mn^{2+} compounds are more stable than Fe^{2+ | vedclass

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Question

(A) The electronic configuration of $Mn^{2+}$ is $[Ar] 3d^5$. This configuration is half-filled,which provides extra stability.The electronic configur

Vedclass · Accepted Answer

$Mn^{2+}$ is more stable with high $3rd$ ionization energy.

Vedclass · Answer

(A) The electronic configuration of $Mn^{2+}$ is $[Ar] 3d^5$. This configuration is half-filled,which provides extra stability.The electronic configuration of $Fe^{2+}$ is $[Ar] 3d^6$.Oxidation to the $+3$ state involves the removal of an electron from the $d$-subshell. For $Mn^{2+}$,removing an electron disrupts the stable half-filled $d^5$ configuration,requiring a very high third ionization energy.For $Fe^{2+}$,removing an electron from the $3d^6$ configuration results in a stable $3d^5$ configuration,which requires less energy.Therefore,$Mn^{2+}$ is more resistant to oxidation to the $+3$ state compared to $Fe^{2+}$.

List-$I$ (Elements)	List-$II$ (Group)
$A$. $Mn, Tc, Re$	$IV$. $7$
$B$. $Zn, Cd, Hg$	$I$. $12$
$C$. $Ti, Zr, Hf$	$II$. $4$
$D$. $Ga, In, Tl$	$V$. $13$

$Mn^{2+}$ compounds are more stable than $Fe^{2+}$ compounds towards oxidation to their $+3$ state,because

Similar Questions

Which of the following sets correctly represents the increase in the paramagnetic property of the ions?

Identify the element for which the electronic configuration in the $+3$ oxidation state is $[Ar] 3d^5$:

Match the following elements in List-$I$ with their respective groups in List-$II$.
List-$I$ (Elements) List-$II$ (Group)
$A$. $Mn, Tc, Re$ $IV$. $7$
$B$. $Zn, Cd, Hg$ $I$. $12$
$C$. $Ti, Zr, Hf$ $II$. $4$
$D$. $Ga, In, Tl$ $V$. $13$

The correct answer is:

To which block does the element with atomic number $106$ belong?

Which of the following metal ions are colorless?

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