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Chapter 23: Problem 109

The coordination compound \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{SCN})_{2}\right]\) displays two types of isomerism. Name the types, and give names and structures for the six possible isomers.

Short Answer

Expert verified
The coordination compound displays cis/trans geometrical isomerism and linkage isomerism. There are six isomers: three cis and three trans forms with each form involving different linkage (\(\mathrm{SCN}\) and \(\mathrm{NCS}\)).

Step by step solution

01

Identify Types of Isomerism

The coordination compound \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{SCN})_{2}\right]\)displays both geometrical (cis/trans) and linkage isomerism. Geometrical isomerism arises due to different spatial arrangements, and linkage isomerism occurs when the ligand can bind through different atoms.
02

Understand Geometrical Isomerism

Geometrical isomers are due to different positions of ligands around the central metal ion. For this compound, there are two geometrical isomers:1. Cis-isomer: Both \(\mathrm{SCN}\) ligands are adjacent to each other.2. Trans-isomer: \(\mathrm{SCN}\) ligands are opposite to each other.
03

Understand Linkage Isomerism

Linkage isomerism is seen when a ligand can coordinate through different atoms. In \(\mathrm{SCN}\), the thiocyanate ligand can bind to the central metal through either the sulfur (\(\mathrm{S}\)) or the nitrogen (\(\mathrm{N}\)) atom. This results in two linkage forms for each geometrical isomer.
04

Combine Both Isomerism Types

Combining geometrical and linkage isomerism leads to six possible isomers:1. Cis form with both \(\mathrm{SCN}\) via \(\mathrm{S}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)_2\right]_{\text{cis}}\)2. Cis form with one \(\mathrm{SCN}\) via \(\mathrm{S}\) and one via \(\mathrm{N}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)(\mathrm{NCS}\right]_{\text{cis}}\)3. Cis form with both \(\mathrm{SCN}\) via \(\mathrm{N}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{NCS}\right)_2\right]_{\text{cis}}\)4. Trans form with both \(\mathrm{SCN}\) via \(\mathrm{S}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)_2\right]_{\text{trans}}\)5. Trans form with one \(\mathrm{SCN}\) via \(\mathrm{S}\) and one via \(\mathrm{N}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)(\mathrm{NCS}\right]_{\text{trans}}\)6. Trans form with both \(\mathrm{SCN}\) via \(\mathrm{N}\): \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{NCS}\right)_2\right]_{\text{trans}}\)
05

List and Name the Isomers

1. **Cis-isomer with\(\mathrm{SCN}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)_2\right]_{cis}\)2. **Cis-isomer with \(\mathrm{SNC}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)(\mathrm{NCS}\right]_{cis}\)3. **Cis-isomer with \(\mathrm{NCS}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{NCS}\right)_2\right]_{cis}\)4. **Trans-isomer with \(\mathrm{SCN}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)_2\right]_{trans}\)5. **Trans-isomer with \(\mathrm{SNC}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{SCN}\right)(\mathrm{NCS}\right]_{trans}\)6. **Trans-isomer with \(\mathrm{NCS}\)** - \(\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2\left(\mathrm{NCS}\right)_2\right]_{trans}\)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Geometrical Isomerism
Geometrical isomerism occurs in coordination compounds due to different spatial arrangements of ligands around the central metal ion. It is also known as cis-trans isomerism. In the given compound, \(\text{[Pt(NH}_3\text{)_2(SCN}_2\text{)]}\), there are two geometrical isomers:
  • Cis-isomer: Both \(\text{SCN}\) ligands are adjacent to each other.
  • Trans-isomer: The \(\text{SCN}\) ligands are opposite to each other.
The relative positioning of the ligands around the central platinum ion differentiates the isomers. The distinction between cis and trans isomers significantly impacts the physical and chemical properties of the coordination compounds.
Linkage Isomerism
Linkage isomerism arises when a ligand can coordinate to the central metal atom through different atoms. For example, thiocyanate (SCN) can bind through either the sulfur (\(\text{S}\)) or the nitrogen (\(\text{N}\)) atom. This leads to two distinct isomeric forms for each geometrical isomer:
  • \
Coordination Compounds
Coordination compounds, also known as complex compounds, consist of a central metal atom or ion bonded to surrounding molecules or ions called ligands. These compounds exhibit various types of isomerism, including geometrical and linkage isomerism as seen in the compound \(\text{[Pt(NH}_3\text{)_2(SCN}_2\text{)]}\). Understanding coordination compounds involve studying the roles of:
  • Central Metal Ion: The atom or ion which is surrounded by ligands. In the example, it is platinum (\(\text{Pt}\)).
  • Ligands: Molecules or ions that bond to the central metal. Each ligand can donate at least one pair of electrons to form a coordinate bond. In the example, the ligands are ammonia (\(\text{NH}_3\)) and thiocyanate (\(\text{SCN}\)).
  • Coordination Number: The total number of ligand bonds to the central atom. For example, in \(\text{[Pt(NH}_3\text{)_2(SCN}_2\text{)]}\), the coordination number of platinum is 4.
  • Types of Isomerism: Coordination compounds can exhibit various isomerism types as seen in the distinction between geometrical isomerism and linkage isomerism shown for \(\text{[Pt(NH}_3\text{)_2(SCN}_2\text{)]}\).
Coordination compounds have significant roles in biological, industrial, and chemical applications.

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Most popular questions from this chapter

For any of the following that can exist as isomers, state the type of isomerism and draw the structures: (a) \(\left[\mathrm{Zn}(\mathrm{en}) \mathrm{F}_{2}\right]\) (b) \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)\left(\mathrm{NH}_{3}\right) \mathrm{FCl}\right]\) (c) \(\left[\mathrm{Pd}(\mathrm{CN})_{2}(\mathrm{OH})_{2}\right]^{2-}\)

Only a few lanthanides show an oxidation state other than \(+3 .\) Two of these, europium (Eu) and terbium (Tb), are found near the middle of the series, and their unusual oxidation states can be associated with a half-filled \(f\) subshell. (a) Write the electron configurations of \(\mathrm{Eu}^{2+}, \mathrm{Eu}^{3+},\) and \(\mathrm{Eu}^{4+} . \mathrm{Why}\) is \(\mathrm{Eu}^{2+}\) a common ion, whereas \(\mathrm{Eu}^{4+}\) is unknown? (b) Write the electron configurations of \(\mathrm{Tb}^{2+}, \mathrm{Tb}^{3+},\) and \(\mathrm{Tb}^{4+} .\) Would you expect \(\mathrm{Tb}\) to show \(\mathrm{a}+2\) or a +4 oxidation state? Explain.

Using the periodic table to locate each element, write the electron configuration of (a) Os; (b) \(\mathrm{Co} ;\) (c) Ag.

Ionic liquids have many applications in engineering and materials science. The dissolution of the metavanadate ion in chloroaluminate ionic liquids has been studied: $$\mathrm{VO}_{3}^{-}+\mathrm{AlCl}_{4}^{-} \longrightarrow \mathrm{VO}_{2}\mathrm{Cl}_{2}^{-}+\mathrm{AlOCl}_{2}^{-}$$ (a) What is the oxidation number of \(\mathrm{V}\) and \(\mathrm{Al}\) in each ion? (b) In reactions of \(\mathrm{V}_{2} \mathrm{O}_{5}\) with \(\mathrm{HCl}\), acid concentration affects the product. At low acid concentration, \(\mathrm{VO}_{2} \mathrm{Cl}_{2}^{-}\) and \(\mathrm{VO}_{3}^{-}\) form: $$\mathrm{V}_{2} \mathrm{O}_{5}+\mathrm{HCl} \longrightarrow \mathrm{VO}_{2}\mathrm{Cl}_{2}^{-}+\mathrm{VO}_{3}^{-}+\mathrm{H}^{+}$$ At high acid concentration, \(\mathrm{VOCl}_{3}\) forms: $$\mathrm{V}_{2} \mathrm{O}_{5}+\mathrm{HCl} \longrightarrow \mathrm{VOCl}_{3}+\mathrm{H}_{2} \mathrm{O}$$ Balance each equation, and state which, if either, is a redox process. (c) What mass of \(\mathrm{VO}_{2} \mathrm{Cl}_{2}^{-}\) or \(\mathrm{VOCl}_{3}\) can form from \(12.5 \mathrm{~g}\) of \(\mathrm{V}_{2} \mathrm{O}_{5}\) and the appropriate concentration of acid?

Give formulas corresponding to the following names: (a) Tetraamminezinc sulfate (b) Pentaamminechlorochromium(III) chloride (c) Sodium bis(thiosulfato)argentate(I)
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