JEE Advanced 2025 Paper 1 Online

MCQ (Single Correct Answer)

-1

The correct order of the wavelength maxima of the absorption band in the ultraviolet-visible region for the given complexes is

[Co(CN)₆] ³⁻ < [Co(NH₃)₆]³⁺ < [Co(NH₃)₅(H₂O)]³⁺ < [Co(NH₃)₅(Cl)]²⁺

[Co(NH₃)₅(Cl)]²⁺ < [Co(NH₃)₅(H₂O)]³⁺ < [Co(NH₃)₆]³⁺ < [Co(CN)₆]³⁻

[Co(CN)₆]³⁻ < [Co(NH₃)₅(Cl)]²⁺ < [Co(NH₃)₅(H₂O)]³⁺ < [Co(NH₃)₆]³⁺

[Co(NH₃)₆]³⁺ < [Co(CN)₆]³⁻ < [Co(NH₃)₅(Cl)]²⁺ < [Co(NH₃)₅(H₂O)]³⁺

JEE Advanced 2024 Paper 1 Online

MCQ (Single Correct Answer)

-1

Among the following options, select the option in which each complex in Set-I shows geometrical isomerism and the two complexes in Set-II are ionization isomers of each other.

$$ \text { [en }=\mathrm{H}_2 \mathrm{NCH}_2 \mathrm{CH}_2 \mathrm{NH}_2 \text { ] } $$

Set-I: $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ and $\left[\mathrm{PdCl}_2\left(\mathrm{PPh}_3\right)_2\right]$

Set-II: $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{SO}_4$ and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5\left(\mathrm{SO}_4\right)\right] \mathrm{Cl}$

Set-I: $\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_3\right)_2 \mathrm{Cl}_2\right]$ and $\left[\mathrm{PdCl}_2\left(\mathrm{PPh}_3\right)_2\right]$

Set-II: $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]\left[\mathrm{Cr}(\mathrm{CN})_6\right]$ and $\left[\mathrm{Cr}\left(\mathrm{NH}_3\right)_6\right]\left[\mathrm{Co}(\mathrm{CN})_6\right]$

Set-I: $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_3\left(\mathrm{NO}_2\right)_3\right]$ and $\left[\mathrm{Co}(\mathrm{en})_2 \mathrm{Cl}_2\right]$

Set-II: $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{SO}_4$ and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5\left(\mathrm{SO}_4\right)\right] \mathrm{Cl}$

Set-I: $\left[\mathrm{Cr}\left(\mathrm{NH}_3\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_2$ and $\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_3\right)_2 \mathrm{Cl}_2\right]$

Set-II: $\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_3$ and $\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_5 \mathrm{Cl}\right] \mathrm{Cl}_2 \cdot \mathrm{H}_2 \mathrm{O}$

JEE Advanced 2023 Paper 1 Online

MCQ (Single Correct Answer)

-1

Match the electronic configurations in List-I with appropriate metal complex ions in List-II and choose the correct option.

[Atomic Number: $\mathrm{Fe}=26, \mathrm{Mn}=25, \mathrm{Co}=27$ ]

List - I	List - II
(P) $t_{2 g}^6 e_g^0$	(1) $\left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$
(Q) $t_{2 g}^3 e_g^2$	(2) $\left[\mathrm{Mn}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$
(R) $\mathrm{e}^2 \mathrm{t}_2^3$	(3) $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$
(S) $t_{2 g}^4 e_g^2$	(4) $\left[\mathrm{FeCl}_4\right]^{-}$
	(5) $\left[\mathrm{CoCl}_4\right]^{2-}$

$\mathrm{P} \rightarrow 1 ; \mathrm{Q} \rightarrow 4 ; \mathrm{R} \rightarrow 2 ; \mathrm{S} \rightarrow 3$

$P \rightarrow 1 ; \mathrm{Q} \rightarrow 2 ; \mathrm{R} \rightarrow 4 ; \mathrm{S} \rightarrow 5$

$\mathrm{P} \rightarrow 3 ; \mathrm{Q} \rightarrow 2 ; \mathrm{R} \rightarrow 5 ; \mathrm{S} \rightarrow 1$

$\mathrm{P} \rightarrow 3 ; \mathrm{Q} \rightarrow 2 ; \mathrm{R} \rightarrow 4 ; \mathrm{S} \rightarrow 1$

JEE Advanced 2022 Paper 1 Online

MCQ (Single Correct Answer)

-1

LIST-I contains metal species and LIST-II contains their properties.

List-I	List-II
(I) $\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4-}$	(P) $t_{2 \mathrm{g}}$ orbitals contain 4 electrons
(II) $\left[\mathrm{RuCl}_{6}\right]^{2-}$	(Q) $\mu$ (spin-only $)=4.9 \mathrm{BM}$
(III) $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$	(R) low spin complex ion
(IV) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$	(S) metal ion in $4+$ oxidation state
	(T) $d^{4}$ species

[Given: Atomic number of $\mathrm{Cr}=24, \mathrm{Ru}=44, \mathrm{Fe}=26$ ]

Match each metal species in LIST-I with their properties in LIST-II, and choose the correct option

I $\rightarrow$ R, T; II $\rightarrow$ P, S; III $\rightarrow$ Q, T; IV $\rightarrow$ P, Q

I $\rightarrow$ R, S; II $\rightarrow$ P, T; III $\rightarrow$ P, Q; IV $\rightarrow$ Q, T

I $\rightarrow$ P, R; II $\rightarrow$ R, S; III $\rightarrow$ R, T; IV $\rightarrow$ P, T

I $\rightarrow$ Q, T; II $\rightarrow$ S, T; III $\rightarrow$ P, T; IV $\rightarrow$ Q, R

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