Given below are two statements: Statement I : Hybridisation, shape...

In Statement I, for $K_3[Co(CO_3)_3]$, Cobalt is in $+3$ oxidation state ($Co^{3+}: 3d^6$). Carbonate ($CO_3^{2-}$) is a weak field ligand. Thus, no pairing occurs, resulting in 4 unpaired electrons. Hybridisation is $sp^3d^2$, shape is octahedral, and $\mu = \sqrt{4(4+2)} = \sqrt{24} \approx 4.9$ BM. Statement I is true.
In Statement II:
For $[Ni(CN)_4]^{2-}$, $Ni^{2+}$ is $3d^8$. $CN^-$ is a strong field ligand, causing pairing. Hybridisation is $dsp^2$, geometry is square planar, and $\mu = 0$ BM.
For $[MnBr_4]^{2-}$, $Mn^{2+}$ is $3d^5$. $Br^-$ is a weak field ligand. Hybridisation is $sp^3$, geometry is tetrahedral, and $\mu = \sqrt{5(5+2)} = \sqrt{35} \approx 5.9$ BM.
For $[CoF_6]^{3-}$, $Co^{3+}$ is $3d^6$. $F^-$ is a weak field ligand. Hybridisation is $sp^3d^2$, geometry is octahedral, and $\mu = \sqrt{4(4+2)} = \sqrt{24} \approx 4.9$ BM.
Statement II is true.
Both statements are true.