This page delves into the unique structure of benzene, explaining why it differs from what one might expect based on its molecular formula.

The stability of benzene is discussed through three key points:

1. Lack of reactivity: Benzene does not undergo typical alkene reactions like decolorizing bromine water, indicating its unique structure.
2. Intermediate bond lengths: X-ray diffraction studies show that all bonds in benzene are of equal length, falling between single and double bond lengths.
3. Hydrogenation enthalpies: The actual hydrogenation enthalpy of benzene is 152 kJ/mol less than expected, demonstrating its enhanced stability.

Vocabulary: Kekulé's model refers to the cyclic structure of benzene proposed by August Kekulé, representing it as a six-membered ring with alternating single and double bonds.

Highlight: Benzene's stability is 152 kJ/mol greater than what would be expected for a cycloalkene structure, indicating its unique aromatic character.

This page explains the delocalized electronic structure of benzene, which is fundamental to understanding its stability and reactivity.

The formation of the delocalized structure is described as follows:

Each carbon atom in benzene uses three of its four electrons to form sigma bonds with two other carbons and one hydrogen. The remaining electron occupies a p-orbital perpendicular to the plane of the ring. These p-orbitals overlap above and below the ring plane, creating a region of electron density.

Definition: Delocalization refers to the spread of electron density over multiple atoms in a molecule, rather than being confined to specific bonds.

Highlight: The overlapping p-orbitals in benzene create a delocalized π-system that spreads over all six carbon atoms, contributing to its unique stability and reactivity.

This page details the benzene electrophilic substitution mechanism for nitration, a classic example of aromatic electrophilic substitution.

The nitration reaction occurs under the following conditions:

• Temperature: 50°C
• Catalyst: Concentrated H₂SO₄

The mechanism proceeds in three steps:

1. Formation of the electrophile $NO₂⁺$: HNO₃ + H₂SO₄ → H₂O + NO₂⁺ + HSO₄⁻
2. Attack of the electrophile on the benzene ring
3. Loss of a proton to restore aromaticity: H⁺ + HSO₄⁻ → H₂SO₄

Example: The nitration of benzene mechanism is a prime illustration of electrophilic aromatic substitution, where the nitro group $NO₂$ replaces a hydrogen atom on the benzene ring.

Highlight: The use of concentrated sulfuric acid as a catalyst is crucial for generating the electrophilic nitronium ion $NO₂⁺$.

This page discusses the halogenation of benzene, another important benzene electrophilic substitution mechanism.

The key points about benzene halogenation are:

1. Benzene's stability makes it unreactive towards direct halogenation due to insufficient electron density to polarize a halogen molecule.
2. A halogen carrier $catalyst$ such as iron or iron$III$ bromide is required for the reaction to proceed.

The mechanism involves three steps:

1. Formation of the electrophile: Br₂ + FeBr₃ → FeBr₄⁻ + Br⁺
2. Attack of the electrophile on the benzene ring
3. Loss of a proton and regeneration of the catalyst: H⁺ + FeBr₄⁻ → FeBr₃ + HBr

Vocabulary: A halogen carrier is a Lewis acid catalyst that facilitates the formation of the electrophilic halogen species in aromatic halogenation reactions.

Highlight: The use of a halogen carrier distinguishes the halogenation of benzene from the halogenation of alkenes, which occurs readily without a catalyst.

This page covers the Friedel-Crafts alkylation and acylation steps, which are important carbon-carbon bond-forming reactions in aromatic chemistry.

Friedel-Crafts Alkylation:

1. Formation of the carbocation electrophile: R-Cl + AlCl₃ → R⁺ + AlCl₄⁻
2. Attack of the electrophile on the benzene ring
3. Loss of a proton: H⁺ + AlCl₄⁻ → AlCl₃ + HCl

Friedel-Crafts Acylation:

1. Formation of the acylium ion: RCOCl + AlCl₃ → RCO⁺ + AlCl₄⁻
2. Attack of the electrophile on the benzene ring
3. Loss of a proton: H⁺ + AlCl₄⁻ → AlCl₃ + HCl

Example: The Friedel-Crafts acylation of benzene using acetyl chloride $CH₃COCl$ and AlCl₃ produces acetophenone.

Highlight: Friedel-Crafts reactions are versatile methods for introducing alkyl or acyl groups onto aromatic rings, but they have limitations such as rearrangements in alkylations and the requirement for at least equimolar amounts of AlCl₃.

This page provides a comparison between the reactivity of alkenes and arenes $aromatic compounds like benzene$, highlighting their differences in electronic structure and chemical behavior.

Key differences:

1. Electron distribution: Alkenes have localized electrons in π-bonds, while arenes have delocalized electrons in a π-system.
2. Reactivity towards electrophiles: Alkenes have sufficient electron density to polarize molecules like bromine, whereas arenes require a halogen carrier.
3. Reaction types: Alkenes undergo electrophilic addition, while arenes undergo electrophilic substitution.

Definition: Arenes are aromatic hydrocarbons characterized by a planar ring structure with delocalized π-electrons, exemplified by benzene and its derivatives.

Highlight: The delocalized nature of electrons in arenes contributes to their stability and unique reactivity, distinguishing them from alkenes in electrophilic reactions.

This page introduces phenol, discussing its acidity and reactivity in electrophilic substitution reactions.

Key points about phenol:

1. It is a weak acid, more acidic than alcohols.
2. Phenol undergoes electrophilic substitution reactions more readily than benzene.

Bromination of phenol:

• Reacts with bromine water without a catalyst
• Produces 2,4,6-tribromophenol as a white precipitate

Example: The reaction of phenol with sodium hydroxide demonstrates its acidic nature, forming sodium phenoxide.

Highlight: Phenol's enhanced reactivity in electrophilic substitutions is due to the electron-donating effect of the -OH group, which increases electron density in the aromatic ring.

This page covers the nitration of phenol and compares the reactivities of benzene and phenol.

Nitration of phenol:

• Occurs with dilute nitric acid, unlike benzene which requires concentrated acid and a catalyst
• Produces a mixture of 2-nitrophenol and 4-nitrophenol

Reactivity comparison:

1. Benzene requires harsh conditions $concentrated acids, catalysts$ for electrophilic substitution.
2. Phenol reacts under milder conditions without catalysts.

Vocabulary: Ortho and para directors are substituents that direct incoming electrophiles to positions 2 and 4 on the benzene ring, respectively.

Highlight: The lone pair of electrons on the oxygen atom in phenol's -OH group is partially donated into the π-system, increasing the electron density and reactivity of the aromatic ring.

This page introduces the topic of benzene and phenols, setting the stage for a detailed exploration of their chemical properties and reactions. The title suggests that the document will cover the structure, reactivity, and various aspects of these aromatic compounds.