Compute the oxidation state of every central metal atom of the coordination compounds below:

i. [Pt(en)₂Cl₂]

ii. [Co(dien)(NH₃)₂]Cl₃

iii. [Cr(EDTA)(H₂O)₂]Br₂

Identify the oxidation number of each metal center in the following coordination compounds.

i. [Cr(en)₂(CO)Cl]²⁺

ii. Co(H₂O)₃(CN)₃

iii. [Ni(C₂O₄)₂(NH₃)₂]^2–

iv. [Fe(OH)₅]^3–

v. Cr(CO)₆

Is the given ligand monodentate? If not, what is its denticity? Is it capable of forming chelate rings?

Draw the structure of [V(H₂O)₂(cat)₂]Cl. Identify the coordination geometry, oxidation number, and coordination number of V.

Consider the reaction of glycinate ion (H₂NCH₂COO^–) with Co³⁺ to produce [Co(gly)₃]³⁺.

(i) Which is the Lewis acid and the Lewis base in the reaction?

(ii) Which are the ligands and donor atoms in the complex?

(iii) Determine the coordination number and the geometry of the central metal ion.

Identify the charge, denticity, and number of electrons donated by the ligand shown below:

Tris(2-(di-tert-butylphosphino)-1-phenylindole)rhodium(II), [Rh(dtbpi)₃]²⁺, is an octahedral complex with three bidentate ligands surrounding the central metal atom.

Note: dtbpi is represented as:

What are the structures of all the diastereoisomers of the complex? Which isomers are enantiomers?

Using crystal field theory, provide the splitting energy diagram of Cr³⁺ in [CrCl₆]^3– and rationalize why [CrCl₆]^3– is colored.

For an ML₂ complex, what is its crystal field energy-level diagram if its two ligands are aligned along the ± z-axis and it has a linear geometry?

The nickel complex ions [NiCl₄]^2– and [Ni(NH₃)₆]²⁺ have different colors. [NiCl₄]^2– is blue, while [Ni(NH₃)₆]²⁺ is violet. Explain this color difference and identify the complex that will absorb at longer wavelengths.