List of top Chemistry Questions on coordination compounds asked in JEE Main

Given below are two statements:
Statement I: Among [Cu(NH₃)₄]²⁺, [Ni(en)₃]²⁺, [Ni(NH₃)₆]²⁺ and [Mn(H₂O)₆]²⁺, [Mn(H₂O)₆]²⁺ has the maximum number of unpaired electrons.
Statement II: The number of pairs among {[NiCl₄]²⁻, [Ni(CO)₄], {[NiCl₄]²⁻, [Ni(CN)₄]²⁻} and {[Ni(CO)₄], [Ni(CN)₄]²⁻} that contain only diamagnetic species is two.
In the light of the above statements, choose the correct answer from the options given below:}
From the following : (A) $[\text{Co}(\text{NH}_3)_6]^{3+}$ : Inner orbital complex, $d^2sp^3$ hybridization (B) $[\text{MnCl}_4]^{2-}$ : Outer orbital complex, $sp^3d^2$ hybridization (C) $[\text{CoF}_6]^{3-}$ : Outer orbital complex, $d^2sp^3$ hybridization (D) $[\text{FeF}_6]^{3-}$ : Outer orbital complex, $sp^3d^2$ hybridization (E) $[\text{Ni}(\text{CN})_4]^{2-}$ : Inner orbital complex, $sp^3$ hybridization Choose the correct answer from the given options.
Number of unpaired electrons in low spin octahedral complex formed by ions Mn$^{3+}$, Cr$^{3+}$, Fe$^{3+}$, and Co$^{3+}$ follows the order:
Some species are given: \( \text{Ni}^{2+}, \text{Fe}^{2+}, \text{Co}^{2+}, \text{V}^{3+}, \text{Ti}^{2+} \) How many species have a magnetic moment (spin only) less than 3 BM?
Consider the given central metal ions of low spin complex and choose the correct increasing order of unpaired electrons: Mn\(^{+} \), Cr\(^{+} \), Fe\(^{+} \), Co\(^{+} \).
An element from the 1\(^\text{st}\) transition series and another element of the 3\(^\text{rd}\) transition series (same group) do not liberate \( \text{H}_2 \) gas from dilute acids like HCl. Both form halides. The hybridisation state of metal ion halide respectively are:
Which of the following compound is paramagnetic in nature?
Find the ratio of CFSE of [Co(C$_2$O$_4$)$_3$]$^{3-}$ and [Cr(C$_2$O$_4$)$_3$]$^{3-}$, for each complex assume \(\Delta_t>P\):
Given below are two statements: Statement-I: [CoBr$_4$]$^{2-}$ absorbs lesser energy than [CoCl$_4$]$^{2-}$
Statement-II: [CoCl$_4$]$^{2-}$ has higher crystal field splitting energy than [CoBr$_4$]$^{2-}$
How many of the following complexes have unpaired electrons $[\text{Ni}(\text{CO})_4]$, $[\text{NiCl}_4]^{2-}$, $[\text{PtCl}_4]^{2-}$, $[\text{Pt}(\text{CN})_4]^{2-}$, $[\text{Pt}(\text{NH}_3)_2\text{Cl}_2]$
Statement-I Among $\text{V}_2\text{O}_5, [\text{TiF}_6]^{2-}, [\text{Fe}(\text{CN})_6]^{3-}, [\text{CoF}_6]^{3-}$ paramagnetic species are three in number. Statement-II Increasing number of unpaired electrons in the following: $[\text{Fe}(\text{CN})_6]^{4-}<[\text{Fe}(\text{CN})_6]^{3-}<[\text{Fe}(\text{H}_2\text{O})_6]^{2+}$.
Match the List-I and List-II name of species, hybridization and shape.
Statement-I $[\text{Co}(\text{C}_2\text{O}_4)_3]^{3-}$ has magnetic moment of $4.9 \text{ BM}$ & hybridization is $sp^3d^2$. Statement-II $[\text{Ni}(\text{CN})_4]^{2-}, [\text{Cr}(\text{H}_2\text{O})_6]^{2+}$ and $[\text{MnF}_6]^{4-}$ have square planar, octahedral and octahedral geometry respectively and $dsp^2, sp^3d^2, d^2sp^3$ hybridization respectively and $\mu=0, 4.9 \text{ BM}, 5.9 \text{ BM}$ respectively.
Which of the following complexes has unpaired electrons?
A complex Cr(H$_2$O)$_6$Cl$_3$ shows conductance similar to a 1 : 2 electrolyte in aqueous solution. 9.3 g of this complex is passed through a cation exchanger and excess AgNO$_3$ is added. Find the mass of AgCl precipitated in grams.
[Molar mass of Cr = 52 g/mol]

Consider the following complexes: 
(A) [Co(CN)$_6$]$^{3-}$             
(B) [Co(NH$_3$)$_5$H$_2$O]$^{3+}$ 
(C) [Co(H$_2$O)$_6$]$^{3+}$      
(D) [CoF$_6$]$^{3-}$ 
The wavelength absorbed by the above complexes are in the order: 
 

Consider the following conformations: 

Statement-I: I$^{nd}$ is more stable than I$^{st}$. 
Statement-II: As dihedral angle increases, stability decreases. 
 

Select correct option :
Among \(\mathrm{Sc^{3+}},\ \mathrm{Cr^{2+}},\ \mathrm{Mn^{3+}},\ \mathrm{Fe^{3+}},\ \mathrm{Co^{3+}}\), \(n\) is the number of isoelectronic species. \(n\) moles of \(\mathrm{AgNO_3}\) react with \(1\) mole of the complex \([\mathrm{Co(en)_3}]Cl_3\). Find the number of electrons in the \(t_{2g}\) set of the complex.

Arrange the given metal ions in increasing order of number of unpaired electrons in the low spin complexes formed by \( \text{Mn}^{3+}, \text{Cr}^{3+}, \text{Fe}^{3+}, \text{Co}^{3+} \)

An element ‘M’ does not evolve H$_2$ gas on treatment with dilute HCl. MSO$_4$ (1 mol) on treatment with ex. KCN forms a compound ‘P’. The amount of MS formed (in moles) when H$_2$S gas is passed through compound ‘P’ is:
Given below are two statements:
Statement-I: Crystal field stabilisation energy (magnitude) of \( [\text{Co}(H_2O)_6]^{2+} \) is greater than \( [\text{Ni}(H_2O)_6]^{2+} \).
Statement-II: Order of bond energy is \( \text{Cl}_2>\text{Br}_2>\text{F}_2>\text{I}_2 \).
In the light of the above statements, choose the correct option.
An octahedral complex having molecular composition Co.5NH$_3$.Cl.SO$_4$ has two isomers A and B. The solution of A gives a white precipitate with AgNO$_3$ solution and the solution of B gives a white precipitate with BaCl$_2$ solution. The type of isomerism exhibited by the complex is,
The metal ion whose electronic configuration is not affected by the nature of the ligand and which gives a violet color in non-luminous flame under hot condition in borax bead test is:
If \( a_0 \) is denoted as the Bohr radius of the hydrogen atom, then what is the de-Broglie wavelength \( \lambda \) of the electron present in the second orbit of hydrogen atom? (\( n \): any integer)