Which of the following orders is not correct?

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(D) $1$. The $\Delta_0$ order depends on the oxidation state of the metal and the strength of the ligand. $[Co(Cl)_6]^{3-}$ has a weak field ligand,$[

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$C_2H_4 > K[PtCl_3(C_2H_4)]$ ($C-C$ bond length)

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(D) $1$. The $\Delta_0$ order depends on the oxidation state of the metal and the strength of the ligand. $[Co(Cl)_6]^{3-}$ has a weak field ligand,$[Fe(H_2O)_6]^{3+}$ has a moderate field ligand,and $[Fe(CN)_6]^{3-}$ has a strong field ligand,so the order is correct.$2$. The $EAN$ (Effective Atomic Number) for $[Fe(CN)_6]^{4-}$ is $26 - 2 + 12 = 36$ and for $[Fe(CN)_6]^{3-}$ is $26 - 3 + 12 = 35$. Thus,$36 > 35$,so the order is correct.$3$. According to the spectrochemical series,$CO$ is a stronger $\pi$-acid ligand than $CN^-$,so the order $CN^- $4$. In the complex $K[PtCl_3(C_2H_4)]$,the metal $Pt$ donates electron density into the $\pi^*$ antibonding orbital of $C_2H_4$ (synergic bonding). This increases the $C-C$ bond length compared to free $C_2H_4$. Therefore,the bond length in the complex is greater than in free $C_2H_4$. The given order $C_2H_4 > K[PtCl_3(C_2H_4)]$ is incorrect.

List-$I$	List-$II$
$I$. $[Cr(CN)_6]^{4-}$	$P$. $t_{2g}$ orbitals contain $4$ electrons
$II$. $[RuCl_6]^{2-}$	$Q$. $\mu$ (spin-only) $= 4.9 \ BM$
$III$. $[Cr(H_2O)_6]^{2+}$	$R$. low spin complex ion
$IV$. $[Fe(H_2O)_6]^{2+}$	$S$. metal ion in $4+$ oxidation state
	$T$. $d^4$ species

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