What can be inferred from the magnetic moment values of the following complex species?

Complex	Magnetic Moment $(BM)$
$K_4[Mn(CN)_6]$	$2.2$
$[Fe(H_2O)_6]^{2+}$	$5.3$
$K_2[MnCl_4]$	$5.9$

The spin-only magnetic moment $(\mu)$ is calculated using the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.
$1$. For $K_4[Mn(CN)_6]$: $Mn$ is in the $+2$ oxidation state ($d^5$ configuration). The observed $\mu = 2.2 \ BM$ corresponds to $n \approx 1$. This indicates that $CN^-$ is a strong field ligand causing pairing of electrons.
$2$. For $[Fe(H_2O)_6]^{2+}$: $Fe$ is in the $+2$ oxidation state ($d^6$ configuration). The observed $\mu = 5.3 \ BM$ corresponds to $n \approx 4$. This indicates that $H_2O$ is a weak field ligand and does not cause pairing of electrons.
$3$. For $K_2[MnCl_4]$: $Mn$ is in the $+2$ oxidation state ($d^5$ configuration). The observed $\mu = 5.9 \ BM$ corresponds to $n \approx 5$. This indicates that $Cl^-$ is a weak field ligand and does not cause pairing of electrons.