Question

Why are ni2+ compounds more stable than fe2+

Answer 1

Answer:

Since Mn2+ has stable half filled electronic configuration, therefore Mn2+ compounds are more stable than Fe2+ towards oxidation to their +3 state. Fe2+(3d6) can lose one electron easily to give Fe3+(3d5, stable configuration).

Answer 2

$Ni^{2+}$ compounds more stable than $Fe^{2+}$because of the number of half filled electrons.

Explanation:

Ni2+ compounds more stable than Fe2+

• The electronic configuration Nickel=$[Ar] 3d5.$
• Its half-filled subshells are more stable, Thus we can see that Fe ion will be more stable than $Ni+2$, because of more number of electrons in half-filled subshells are found.

• In  $Mn2+$ has a stable half-filled electronic configuration, therefore $Mn2+$compounds are more stable than $Fe2+$towards oxidation to their +3 state
• $Fe2+$=$3d6$ can lose one electron easily to give  $Fe3+$ = $3d5$, stable configuration.

• Electronic configuration of $Ni+2 = [Ar] 3d8$
• Electronic configuration of $Fe+3 = [Ar] 3d5.$
• So, half-filled subshells are more stable, Thus, $Fe+3 ion$ will be more stable than $Ni+2$ because of more number of exchanges in half filled subshells.