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Ether

Organic Chemistry Lecture 14

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Chemistry
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Functional groups
Ether
Epoxide
Williamson ether synthesis
Peroxide
Alkoxy group
Diethyl ether
Organolithium reagent
Organic peroxide
Ethylene oxide

Chapter 14 ? 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Ethers, Epoxides, and Sulfides Chapter 14 * Ethers Formula is R?O?R???where R and R? are alkyl or aryl. Symmetrical or unsymmetrical O C H 3 C H 3 O C H 3 Chapter 14 Chapter 14 * Structure and Polarity Oxygen is sp3 hybridized. Bent molecular geometry. C?O?C angles is 110?. Polar C?O bonds. Dipole moment of 1.3 D. Chapter 14 Chapter 14 * Boiling Points Similar to alkanes of comparable molecular weight. Chapter 14 Chapter 14 * Hydrogen Bond Acceptor Ethers cannot hydrogen-bond with other ether molecules. Molecules that cannot hydrogen-bond intermolecularly have a lower boiling point. Ether molecules can hydrogen-bond with water and alcohol molecules. Chapter 14 Chapter 14 *

Organic Chemistry Lecture 11

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Alcohol
Lucas' reagent
Alkene
Ester
Pyridinium chlorochromate
Tosyl
Phosphorus tribromide
Aldehyde
Ether

Chapter 11 Reactions of Alcohols ?2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Chapter 11 * Types of Alcohol Reactions Dehydration to alkene Oxidation to aldehyde, ketone Substitution to form alkyl halide Reduction to alkane Esterification Tosylation Williamson synthesis of ether Chapter 11 Chapter 11 * Summary Table Chapter 11 Chapter 11 * Oxidation States Easy for inorganic salts: CrO42- reduced to Cr2O3. KMnO4 reduced to MnO2. Oxidation: Gain of O, O2, or X2; loss of H2. Reduction: Gain of H2 (or H-); loss of O or O2; and loss of X2. The gain or loss of H+, H2O, HX, etc. is neither an oxidation nor a reduction. Chapter 11 Chapter 11 * Oxidation States of Carbons Chapter 11 Chapter 11 *

Chapter 16 Powerpoint

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Acid-base chemistry
Bases
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Ether
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Chemistry
Acids
Equilibrium chemistry
Bases
Acid-base chemistry
Acid–base reaction
Acid strength
Acid dissociation constant
Acid
Brønsted–Lowry acid–base theory
Carboxylic acid
Lewis acids and bases
education

Acid-Base Equilibria Priyal Patel 0 period 16.1 Acids and Bases: A Brief Review Acids have a sour taste and cause certain dyes to change color Sour taste Linked to H+ ions Bases are bitter and feel slippery Bitter taste Feel slippery Linked to OH- ions When acids and bases are mixed in certain proportions, their characteristics disappear altogether 16.2 Bronsted-Lowry Acids and Bases Danish Chemist Johannes Bronsted and English chemist Thomas Lowry proposed a definition of acids and bases Based on the fact that acid-base reactions involve the transfer of H+ ions from one substance to another. The H+ Ion in Water An H+ is a proton with no surrounding valence electrons This proton bonds interacts with nonbonding electrons of water molecules to form hydrated hydrogen ions.
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