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Chapter 7: Problem 1

Which of the following statements is false? (l) According to Lewis theory electrophiles are Lewis acids while nucleophiles are Lewis bases. (2) In Friedel-Crafts reaction, the catalysts used are Lewis acids. (3) In complex compounds, metal ions are Lewis bases while ligands are Lewis acids. (4) Electron-deficient molecules are Lewis acids.

Short Answer

Expert verified
Statement (3) is false.

Step by step solution

01

Understanding Lewis Acids and Bases

Review the definitions: Electrophiles are electron pair acceptors (Lewis acids), while nucleophiles are electron pair donors (Lewis bases).
02

Friedel-Crafts Reaction and Catalysts

Recognize that Friedel-Crafts reactions use catalysts such as AlCl3, which is a Lewis acid.
03

Metal Ions and Ligands in Complex Compounds

In complex compounds, metal ions typically act as Lewis acids because they accept electron pairs from ligands, which act as Lewis bases.
04

Electron-Deficient Molecules

Electron-deficient molecules are Lewis acids because they can accept electron pairs.
05

Identifying the False Statement

Analyze all the statements again. Statements (1), (2), and (4) are true based on the definitions and analyses. However, (3) is incorrect because in complex compounds, metal ions are Lewis acids, not Lewis bases.

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Key Concepts

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

Lewis Acids
Lewis acids are chemical species that can accept an electron pair. This characteristic makes them electrophiles, which seek electrons to achieve a more stable electronic configuration.
Common examples of Lewis acids include:
  • Hydrogen ions (H+)
  • Metal ions such as Fe3+ or Al3+
  • Electron-deficient molecules like BF3 or AlCl3
These species generally have vacant orbitals, enabling them to accept electron pairs from Lewis bases. Understanding Lewis acids is essential when discussing catalytic processes, coordination complexes, and many organic reactions.
Lewis Bases
Lewis bases are compounds that can donate an electron pair. This makes them nucleophiles, meaning they seek positively charged or electron-deficient sites.
Examples of Lewis bases include:
  • Ammonia (NH3)
  • Hydroxide ions (OH-)
  • Water (H2O)
  • Ligands in metal complexes like ethylenediamine
Lewis bases have lone pairs of electrons that they can share with Lewis acids, facilitating the formation of a coordinate bond. This interaction forms the foundation for many reactions, including acid-base interactions and complex formation.
Friedel-Crafts Reaction
The Friedel-Crafts reaction is a type of organic reaction used to attach substituents onto aromatic rings. There are two types: Friedel-Crafts alkylation and Friedel-Crafts acylation.
Key points include:
  • AlCl3 or FeCl3 are common catalysts used in these reactions
  • These catalysts are Lewis acids that accept electron pairs
  • The reaction allows for the formation of new carbon-carbon bonds
During the reaction, the catalyst helps to generate a more reactive electrophile which then reacts with the aromatic compound. Understanding the role of Lewis acids in this reaction is crucial for mastering many synthetic pathways in organic chemistry.
Metal-Ligand Complexes
In coordination chemistry, metal-ligand complexes play a fundamental role in many chemical processes.
Key aspects include:
  • Metal ions are Lewis acids: They accept electron pairs
  • Ligands are Lewis bases: They donate electron pairs
  • The metal-ligand interaction is through a coordinate bond
For example, in a complex like [Fe(CN)6]3-, Fe3+ is the Lewis acid, and the cyanide ions (CN-) are the Lewis bases. The interaction between the metal and the ligands stabilizes the metal ion and modifies its chemical properties.
Understanding these interactions is essential for fields like bioinorganic chemistry, catalysis, and materials science.

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Most popular questions from this chapter

Which onc of the following is not a postulate of Ostwald's theory of indicators? (1) The colour of an indicator in solution is duc to the ions furnished by it (2) The colour of an indicator is duc to the ions furnished by acidic substancc (3) \Lambdall indicators are weak acids or bases (4) \Lambdacidic indicators show decp colour in acidic solutions and vice versa

Oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3}\) by \(\mathrm{O}_{2}\) is an cxothermic reaction. The yicld of \(\mathrm{SO}_{3}\) will be maximum when(1) Temperature is increased and pressure is kept constant. (2) Temperature is reduced and pressure is increased. (3) Both temperature and pressure are increased. (4) Both temperature and pressure are reduced.

At \(1000^{\circ} \mathrm{C}\), the equilibrium constant for the reaction of the system \(2 \mathrm{II}_{2}(\mathrm{~g}) \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) is very largc. This implics that (1) \(\mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) is unstable at \(1000^{\circ} \mathrm{C}\) (2) \(\mathrm{II}_{2}(\mathrm{~g})\) is unstable at \(1000^{\circ} \mathrm{C}\) (3) \(\mathrm{II}_{2}\) and \(\mathrm{O}_{2}\) have very little tendency to combinc at \(1000^{\circ} \mathrm{C}\) (4) \(\mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) has very little tendency to decompose into \(\mathrm{II}_{2}(\mathrm{~g})\) and \(\mathrm{O}_{2}(\mathrm{~g})\) at \(1000^{\circ} \mathrm{C}\)

For the chemical reaction \(3 \mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons \mathrm{X}_{3} \mathrm{Y}(\mathrm{g})\) the amount of \(\mathrm{X}_{3} \mathrm{Y}\) at equilibrium is affected by (1) Tempcrature and pressure (2) Tempcrature only (3) Pressurc only (4) Temperature, pressure and catalyst

Docs Le Chatelier's principle predict a change of equilibrium concentration for the following reaction if the gas mixture is compressed. \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})\) (1) Ycs, backward reaction is favoured. (2) Yes, forward reaction is favoured. (3) No changc. (4) No information.
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