Calculate the number of unpaired electrons in the following gaseous ions: $Mn ^{3+}, Cr ^{3+}, V ^{3+}$ and $T i^{3+} .$ Which one of these is the most stable in aqueous solution?
Calculate the number of unpaired electrons in the following gaseous ions: $Mn ^{3+}, Cr ^{3+}, V ^{3+}$ and $T i^{3+} .$ Which one of these is the most stable in aqueous solution?
| Gaseous ions | Number of unpaired electrons | |
| $(i)$ | $Mn ^{3+},[ Ar ] \,3 d^{4}$ | $4$ |
| $(ii)$ | $Cr ^{3+},[ Ar ] \,3 d^{3}$ | $3$ |
| $(iii)$ | $V ^{3+},[ Ar ] \,3 d^{2}$ | $2$ |
| $(iv)$ | $Ti ^{3+},[ Ar ]\, 3 d^{1}$ | $1$ |
$Cr ^{3+}$ is the most stable in aqueous solutions owing owing to a $^{t_{2g}^{3}}$ configuration.
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- [JEE MAIN 2016]
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What can be inferred from the magnetic moment values of the following complex species?
Example
Magnetic Moment $(BM)$
$K _{4}\left[ Mn ( CN )_{6}\right.$
$2.2$
$\left[ Fe \left( H _{2} O \right)_{6}\right]^{2+}$
$5.3$
$K _{2}\left[ MnCl _{4}\right]$
$5.9$
What can be inferred from the magnetic moment values of the following complex species?
| Example | Magnetic Moment $(BM)$ |
| $K _{4}\left[ Mn ( CN )_{6}\right.$ | $2.2$ |
| $\left[ Fe \left( H _{2} O \right)_{6}\right]^{2+}$ | $5.3$ |
| $K _{2}\left[ MnCl _{4}\right]$ | $5.9$ |