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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

\(\mathrm{CoCl}_{4}^{2-}\) forms a tetrahedral complex ion and \(\mathrm{Co}(\mathrm{CN})_{6}^{3-}\) forms an octahedral complex ion. What is wrong about the following statements concerning each complex ion and the \(d\) orbital splitting diagrams? a. \(\mathrm{CoCl}_{4}^{2-}\) is an example of a strong-field case having two unpaired electrons. b. Because \(\mathrm{CN}^{-}\) is a weak-field ligand, \(\mathrm{Co}(\mathrm{CN})_{6}^{3-}\) will be a low-spin case having four unpaired electrons.

A compound related to acetylacetone is 1,1,1 -trifluoroacetylacetone (abbreviated Htfa): Htfa forms complexes in a manner similar to acetylacetone. (See Exercise \(47 .\) Both \(\mathrm{Be}^{2+}\) and \(\mathrm{Cu}^{2+}\) form complexes with tfa \(^{-}\) having the formula \(\mathrm{M}\) (tfa) \(_{2}\). Two isomers are formed for each metal complex. a. The \(\mathrm{Be}^{2+}\) complexes are tetrahedral. Draw the two isomers of Be(tfa)_2. What type of isomerism is exhibited by \(\mathrm{Be}(\mathrm{tfa})_{2} ?\) b. The \(\mathrm{Cu}^{2+}\) complexes are square planar. Draw the two isomers of \(\mathrm{Cu}(\mathrm{tfa})_{2} .\) What type of isomerism is exhibited by $\mathrm{Cu}(\mathrm{tfa})_{2} ?

The complex ion \(\mathrm{Ru}\) (phen) \(_{3}^{2+}\) has been used as a probe for the structure of DNA. (Phen is a bidentate ligand.) a. What type of isomerism is found in \(\mathrm{Ru}(\text { phen })_{3}^{2+} ?\) b. \(\mathrm{Ru}(\text { phen })_{3}^{2+}\) is diamagnetic (as are all complex ions of \(\mathrm{Ru}^{2+}\) ). Draw the crystal field diagram for the \(d\) orbitals in this complex ion.$

One of the classic methods for the determination of the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.

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.
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