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Chapter 20: Problem 78

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

Short Answer

Expert verified
The short answer for the given coordination compounds is: a. Tetrasodium trioxalatonickel(II) b. Dipotassium tetrachloridocobalt(II) c. Tetraamminecopper(II) sulfate d. Diethylenediamine thiocyanato chloridocobalt(III) chloride

Step by step solution

01

Identify the central metal atom/ion and ligands

In this compound, Ni is the central metal ion and three oxalate ligands (\(\mathrm{C}_{2}\mathrm{O}_{4}^{-2}\)) are surrounding it. There are 4 sodium ions (\(\mathrm{Na}^{+}\)) as counterions.
02

Name the compound following IUPAC conventions

The name of the compound should follow the order: cation - anion - ligand - metal - oxidation state. We have: 1. Cation: tetrasodium 2. Ligand: trioxalato (since there are three oxalate ligands) 3. Metal: nickel 4. Oxidation state: (3 x (-2)) + (4 x 1) = 0; hence, oxidation state = 2. The full name is: Tetrasodium trioxalatonickel(II) #(b) \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\):#
03

Identify the central metal atom/ion and ligands

In this compound, Co is the central metal ion and there are 4 chloride ions (\(\mathrm{Cl}^{-}\)) surrounding it. There are 2 potassium ions (\(\mathrm{K}^+\)) as counterions.
04

Name the compound following IUPAC conventions

The name of the compound should follow the order: cation - anion - ligand - metal - oxidation state. We have: 1. Cation: dipotassium 2. Ligand: tetrachlorido (since there are 4 chloride ligands) 3. Metal: cobalt 4. Oxidation state: (4 x (-1)) + (2 x 1) = 0; hence, oxidation state = 2. The full name is: Dipotassium tetrachloridocobalt(II) #(c) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\):#
05

Identify the central metal atom/ion and ligands

In this compound, Cu is the central metal ion and there are 4 ammonia ligands (\(\mathrm{NH}_{3}\)) surrounding it. The counterion is sulfate (\(\mathrm{SO}_{4}^{-2}\)).
06

Name the compound following IUPAC conventions

The name of the compound should follow the order: cation - anion - ligand - metal - oxidation state. We have: 1. Cation: tetraammine (since there are 4 ammonia ligands) 2. Anion: sulfate 3. Metal: copper 4. Oxidation state: 0; hence, oxidation state = 2. The full name is: Tetraamminecopper(II) sulfate #(d) \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\):#
07

Identify the central metal atom/ion and ligands

In this compound, Co is the central metal ion, and its ligands are 2 ethylenediamine ligands (en), one thiocyanate ligand (\(\mathrm{SCN}^{-}\)), and one chloride ion (\(\mathrm{Cl}^{-}\)). The counterion is one chloride ion.
08

Name the compound following IUPAC conventions

The name of the compound should follow the order: cation - anion - ligand - metal - oxidation state. We have: 1. Cation: diethylenediamine (since there are 2 en ligands), thiochanato (follow alphabetical order) 2. Anion: chlorido 3. Metal: cobalt 4. Oxidation state: (1 x (-1)) + (1 x 1) = 0; hence, oxidation state = 3. The full name is: Diethylenediamine thiocyanato chloridocobalt(III) chloride

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Most popular questions from this chapter

Compounds of copper(II) are generally colored, but compounds of copper(I) are not. Explain. Would you expect \(\mathrm{Cd}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\) to be colored? Explain.

The \(\operatorname{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) ion is diamagnetic, but \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) is para-magnetic. Explain.

Draw all geometrical and linkage isomers of square planar \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{SCN})_{2}\)

The complex ion \(\mathrm{PdCl}_{4}^{2-}\) is diamagnetic. Propose a structure for \(\mathrm{PdCl}_{4}^{2-}\)

Consider the complex ions \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}, \mathrm{Co}(\mathrm{CN})_{6}^{3-},\) and \(\mathrm{CoF}_{6}^{3-} .\) The wavelengths of absorbed electromagnetic radiation for these compounds (in no specific order) are \(770 \mathrm{nm}\) \(440 \mathrm{nm},\) and \(290 \mathrm{nm} .\) Match the complex ion to the wavelength of absorbed electromagnetic radiation.
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