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Chapter 23: Problem 37

Write the names of the following compounds, using the standard nomenclature rules for coordination complexes: (a) \(\left[\mathrm{Rh}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (b) \(\mathrm{K}_{2}\left[\mathrm{TiCl}_{6}\right]\) (c) \(\mathrm{MoOCl}_{4}\) (d) \(\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\right] \mathrm{Br}_{2}\)

Short Answer

Expert verified
Tetraammine dichloridochromium(III)chloride; Potassium hexachloridotitanate(IV); Oxotetrachloridomolybdenum(VI); Tetraaqua oxalatoplatinum(IV) bromide.

Step by step solution

01

(a) Name the complex \(\left[\mathrm{Rh}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\)

The central metal ion in this complex is Rhodium (Rh), and the ligands are 4 Ammonia (\(\mathrm{NH}_{3}\)) molecules and 2 Chloride ions (\(\mathrm{Cl}\)). The spheration \(\left[\right]\) implies a complex ion, with the Chloride outside the sphere being the counterion. To name the complex, we first list the ligands in alphabetical order, followed by the metal ion's name and oxidation state in Roman numerals in parenthesis. Here, ammonia ligands are named as ammine and have the prefix "tetra-", while chloride ligands are named as "chloro". The complex is thus named: Tetraammine dichloridochromium(III)chloride.
02

(b) Name the complex \(\mathrm{K}_{2}\left[\mathrm{TiCl}_{6}\right]\)

The central metal ion in this complex is Titanium (Ti), and the ligands are 6 Chloride ions (\(\mathrm{Cl}\)). Two potassium (K) ions are the counterions in this complex. To name the complex, we first list the ligands followed by the metal ion's name and oxidation state in Roman numerals in a parenthesis. Since there are 6 chloride ligands, named "hexachloro", the complex is named: Potassium hexachloridotitanate(IV).
03

(c) Name the complex \(\mathrm{MoOCl}_{4}\)

The central metal ion in this complex is Molybdenum (Mo), and the ligands are 1 oxo ligand (\(\mathrm{O}\)) and 4 Chloride ions (\(\mathrm{Cl}\)). To name the complex, we first list the ligands followed by the metal ion's name and oxidation state in Roman numerals in parenthesis. Since there is one oxo ligand, named "oxo", and 4 chloride ligands, named "tetrachlorido", the complex is named: Oxotetrachloridomolybdenum(VI).
04

(d) Name the complex \(\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\right] \mathrm{Br}_{2}\)

The central metal ion in this complex is Platinum (Pt), and the ligands are 4 water molecules (\(\mathrm{H}_{2} \mathrm{O}\)) and 1 oxalate ion (\(\mathrm{C}_{2} \mathrm{O}_{4}\)). The counterions are 2 bromide ions (\(\mathrm{Br}\)). To name the complex, we first list the ligands in alphabetical order, followed by the metal ion's name and oxidation state in Roman numerals in parenthesis. Water ligands are named as aqua and have the prefix "tetra-", while the oxalate ligand is named as "oxalato". The complex is thus named: Tetraaqua oxalatoplatinum(IV) bromide.

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Most popular questions from this chapter

(a) Draw the structure for \(\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2} .\) (b) What is the coordination number for platinum in this complex, and what is the coordination geometry? (c) What is the oxidation state of the platinum? [Section 23.2]

\(\begin{array}{lllll}\text { Sketch all the possible } & \text { stereoisomers } & \text { of }\end{array}\) (a) \(\left[\mathrm{Rh}(\text { bipy })(o \text { -phen })_{2}\right]^{3+}\), (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}(\text { bipy }) \mathrm{Br}\right]^{2+},\) (c) square-planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right]\).

The red color of ruby is due to the presence of Cr(III) ions at octahedral sites in the close-packed oxide lattice of \(\mathrm{Al}_{2} \mathrm{O}_{3} .\) Draw the crystal-field splitting diagram for Cr(III) in this environment. Suppose that the ruby crystal is subjected to high pressure. What do you predict for the variation in the wavelength of absorption of the ruby as a function of pressure? Explain.

The value of \(\Delta\) for the \(\left[\mathrm{CrF}_{6}\right]^{3-}\) complex is \(182 \mathrm{~kJ} / \mathrm{mol}\). Calculate the expected wavelength of the absorption corresponding to promotion of an electron from the lowerenergy to the higher-energy \(d\) -orbital set in this complex. Should the complex absorb in the visible range?

Explain why the \(d_{x y}, d_{x z}\), and \(d_{y z}\) orbitals lie lower in energy than the \(d_{z}^{2}\) and \(d_{x^{2}-y^{2}}\) orbitals in the presence of an octahedral arrangement of ligands about the central metal ion.
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