Isomerism In Coordination Compounds

Indicate the type of isomerism exhibited by the complex $\left[\mathrm{Pt}\right({\mathrm{NH}}_3\left)\right({\mathrm{H}}_2\mathrm{O}\left){\mathrm{Cl}}_2\right]$ and draw the structures for its isomers.

Indicate the types of isomerism exhibited by the following complex and draw the structures for these isomers

$\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_5\left({\mathrm{NO}}_2\right)\right]{\left({\mathrm{NO}}_3\right)}_2$.

Indicate the types of isomerism exhibited by the following complex and draw the structures for these isomers.

$\left[\mathrm{Co}{\left(\mathrm{en}\right)}_3\right]{\mathrm{Cl}}_3$

Explain the violet colour of the complex ${\left[\mathrm{Ti}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{3+}$on the basis of crystal field theory.

Discuss the nature of bonding in the following coordination entity based on valence bond theory ${\left[{\mathrm{CoF}}_6\right]}^{3-}$.

Discuss the nature of bonding in the following coordination entity based on valence bond theory ${\left[\mathrm{Co}{\left({\mathrm{C}}_2{\mathrm{O}}_4\right)}_3\right]}^{3-}$.

Discuss the nature of bonding in the following coordination entity based on valence bond theory ${\left[{\mathrm{FeF}}_6\right]}^{3-}$.

Aqueous copper sulphate solution (blue in colour) gives a bright green solution with aqueous potassium chloride. Explain these experimental results.

Draw all the isomers (geometrical and optical) of:

${\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_2{\mathrm{Cl}}_2\left(\mathrm{en}\right)\right]}^{+}$

Draw all the isomers (geometrical and optical) of:

${\left[\mathrm{Co}\left({\mathrm{NH}}_3\right)\mathrm{Cl}{\left(\mathrm{en}\right)}_2\right]}^{2+}$

Draw the structures of optical isomers of ${\left[\mathrm{Cr}{\left({\mathrm{NH}}_3\right)}_2{\mathrm{Cl}}_2\left(\mathrm{en}\right)\right]}^{+}$.

Draw the structures of optical isomers of ${\left[{\mathrm{PtCl}}_2{\left(\mathrm{en}\right)}_2\right]}^{2+}$.

How many geometrical isomers are possible in the following coordination entity?

$\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_3{\mathrm{Cl}}_3\right]$

${\left[\mathrm{F}\mathrm{e}{\left(\mathrm{C}\mathrm{N}\right)}_6\right]}^{4-}$ and ${\left[\mathrm{F}\mathrm{e}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+}$ are of different colours in dilute solutions. Why?

A solution of ${\left[\mathrm{N}\mathrm{i}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+}$ is green but a solution of ${\left[\mathrm{N}\mathrm{i}{\left(\mathrm{C}\mathrm{N}\right)}_4\right]}^{2-}$ is colourless. Explain.

${\left[\mathrm{C}\mathrm{r}{\left(\mathrm{N}{\mathrm{H}}_3\right)}_6\right]}^{3+}$ is paramagnetic while ${\left[\mathrm{N}\mathrm{i}{\left(\mathrm{C}\mathrm{N}\right)}_4\right]}^{2-}$ is diamagnetic. Explain why?

What is crystal field splitting energy? How does the magnitude of ${∆}_{\mathrm{o}}$ decide the actual configuration of $\mathrm{d}$-orbitals in a coordination entity?

What is the spectrochemical series? Explain the difference between a weak field ligand and a strong field ligand.

Draw figure to show the splitting of $\mathrm{d}$ orbitals in an octahedral crystal field.

Discuss the nature of bonding in the following coordination entity based on valence bond theory: ${\left[\mathrm{F}\mathrm{e}{\left(\mathrm{C}\mathrm{N}\right)}_6\right]}^{4-}$