What is the systematic name for each of the following coordination compounds? 
(a) Cs[FeCl₄]
(b) [V(H₂O)₆](NO₃)₃

What is the name of the compound [Fe(H2O)5(SCN)]Cl2? 

(a) pentaaquathiocyanatoiron(III) chloride 

(b) pentaaquachlorothiocyanato iron(III) 

(c) pentaaquathiocyanatoiron(III) dichloride

(d) pentaaquathiocyanatoiron(II) chloride

Two first-series transition metals have three unpaired electrons in complex ions of the type [MCl4]2-.

(a) What are the oxidation state and the identity of M in these complexes?

(b) Draw valence bond orbital diagrams for the two possible ions.

(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which ion is more likely to exist?

<QUESTION REFERENCES FIGURE 21.6>

Constitutional isomers of a ruthenium(II) coordination compound are shown below.

(a) Give the formula and name for structures 1-3.

(b) Which structures are linkage isomers? 

(c) Which structures are ionization isomers?

Nickel(II) complexes with the formula NiX₂L₂, where X⁻ is Cl⁻ or N-bonded NCS⁻ and L is the monodentate triphenylphosphine ligand P(C₆H₅)₃, can be square planar or tetrahedral.

(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.

There are two possible [M(OH)4]- complexes of first-series transition metals that have three unpaired electrons.

(a) What are the oxidation state and the identity of M in these complexes?

(b) Using orbital diagrams, give a valence bond description of the bonding in each complex.

(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which [M(OH)4]- complex is more likely to exist? 

<QUESTION REFERENCES FIGURE 21.6>-

Classify the following ligands as monodentate, bidentate, tri-dentate, or tetradentate. Which can form chelate rings?

(a)  

(b) 

(c) 

(d)