Co-ordination compounds practice · Medium

Which of the following is tetrahedral and paramagnetic complex?

Among the following ions, which one has the highest unpaired electrons?

Assertion: $\left[{Ni}({CN})_4\right]^{-2}$ has zero unpaired electron while that of $\left[{NiCl}_4\right]^{-2}$ has two unpaired ${e}^{-}$

Reason: $\left[{Ni}({CN})_4\right]^{-2}$ has strong crystal field while $\left[{NiCl}_4\right]^{-2}$ has weak crystal field.

Which of the following compounds has same oxidation state of the central metal atom in the cationic and anionic part?

What will be the correct order for the wavelengths of absorption in the visible region of the following:
$\mathop {{{\left[ {{\text{Ni}}{{\left( {{\text{N}}{{\text{H}}_3}} \right)}_6}} \right]}^{2 + }}}\limits_{\text{A}} ,\mathop {{\text{Ni}}{{({\text{CN}})}_6}{]^{ - 4}}}\limits_{\text{B}} ,\mathop {{{\left[ {{\text{Ni}}{{\left( {{{\text{H}}_2}{\text{O}}} \right)}_6}} \right]}^{ + 2}}}\limits_{\text{C}} ,\mathop {{{\left[ {{\text{NiC}}{{\text{l}}_6}} \right]}^{ - 4}}}\limits_{\text{D}}$

According to spectrochemical series strongest field ligand among the following is

Which of the following has least conductivity in aqueous solution

The splitting of the $d$ - orbitals of transition metals by a particular complex geometry gives rise to the pattern,

$\begin{array}{r} \overline{d_{x y}}\,\,\overline{d_{y z}}\,\,\overline{d_{x z}} \\ \text { Energy } \uparrow \overline{d_{x^2-y^2}}\,\,\overline{d_{z^2}} \end{array}$

Which one of the following geometries produces the above splitting pattern?

The correct order of ligands arranged in increasing field strength.

The number of isomers possible for square planar complex ${\mathrm{K}_2}\left[ {\mathrm{PdClB}{\mathrm{r}_2}\mathrm{SCN}} \right]$ is:

The number of ions formed when a molecule of ${\mathrm{K}_4}\mathrm{Fe}{\left( {\mathrm{CN}} \right)_6}$ dissociates is:

Assertion: $\left[{Fe}({CN})_6\right]^{3-}$ is weakly paramagnetic while $\left[{Fe}({CN})_6\right]^{4-}$ is diamagnetic.

Reason: $\left[{Fe}({CN})_6\right]^{3-}$ has +3 oxidation state while $\left[{Fe}({CN})_6\right]^{4-}$ has +2 oxidation state.

$\left[M a_6\right]^{+2},\left[M b_6\right]^{+2},\left[M c_6\right]^{+2}$ and $\left[M d_6\right]^{+2}$ octahydral complex absorbs wavelengths in the region of red, green, blue and yellow respectively. What is the strongest ligand among $a, b, c$ and $\mathrm{d}$.

Which of the following best describes the nature of $\mathrm{FeSO}_4 \cdot\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4 \cdot 6 \mathrm{H}_2 \mathrm{O}$

Statement I: $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ is diamagnetic in nature

Statement II: Nickel atom undergoes $\mathrm{sp}^3$ hybridization

The correct statements from following are:

A. The strength of anionic ligands can be explained by crystal field theory.

B. Valence bond theory does not give a quantitative interpretation of kinetic stability of coordination compounds.

C. The hybridization involved in formation of $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ complex is dsp ${ }^2$.

D. The number of possible isomer(s) of cis- $\left[\mathrm{PtCl}_2(\mathrm{en})_2\right]^{2+}$ is one

Choose the correct answer from the options given below:

Assertion: The geometrical isomers of the complex $\left[{M}\left({NH}_3\right)_4 {Cl}_2\right]$ are optically inactive.

Reason: Both geometrical isomers of the complex $\left[{M}\left({NH}_3\right)_4 {Cl}_2\right]$ posses axis of symmetry.

Which of the following sequence is correct regarding field strength of ligands as per spectrochemical series?

Which of the following statements is not correct?

Statement I: $\left[\mathrm{Co}(\mathrm{en})_2\left(\mathrm{NH}_3\right) \mathrm{Br}\right] \mathrm{SO}_4$ has lower electrical conductivity as compared to $\left[\mathrm{Co}(\mathrm{en})_2\left(\mathrm{NH}_3\right) \mathrm{SO}_4\right] \mathrm{Br}$

Statement II: Both the complexes produce the same number of ions in solution