Organic Chemistry Basics

Organic Chemistry

Definition

• Study of carbon-containing compounds and their properties
• Excludes carbonates, cyanides, and oxides

Characteristics of Organic Compounds

• Typically contain hydrogen and carbon atoms
• May contain other elements like oxygen, nitrogen, sulfur, and phosphorus
• Usually have low melting and boiling points
• Often have distinct odors and colors

Functional Groups

• Specific groups of atoms that determine the chemical properties of a molecule
• Examples:
  • Hydroxyl (-OH)
  • Carboxyl (-COOH)
  • Amino (-NH2)
  • Methyl (-CH3)

Types of Organic Compounds

• Alkanes: Saturated hydrocarbons with only single bonds (e.g., methane, ethane)
• Alkenes: Unsaturated hydrocarbons with one or more double bonds (e.g., ethene, propene)
• Alkynes: Unsaturated hydrocarbons with one or more triple bonds (e.g., ethyne, propyne)
• Arenes: Aromatic hydrocarbons with planar, ring-shaped structures (e.g., benzene)
• Alcohols: Compounds with a hydroxyl (-OH) functional group (e.g., methanol, ethanol)
• Ethers: Compounds with an oxygen atom bonded to two alkyl groups (e.g., diethyl ether)
• Carboxylic Acids: Compounds with a carboxyl (-COOH) functional group (e.g., acetic acid, citric acid)
• Amines: Compounds with an amino (-NH2) functional group (e.g., ammonia, methylamine)

Isomerism

• Structural Isomerism: Different arrangements of atoms in a molecule with the same molecular formula
• Stereoisomerism: Different arrangements of atoms in space with the same molecular formula

Reactions

• Substitution Reactions: Replacement of a functional group with another functional group
• Elimination Reactions: Removal of a functional group to form a new bond
• Addition Reactions: Addition of a functional group to a molecule
• Oxidation-Reduction Reactions: Gain or loss of electrons resulting in a change in oxidation state

Organic Chemistry

Definition and Scope

• Organic chemistry studies carbon-containing compounds and their properties, excluding carbonates, cyanides, and oxides

Characteristics of Organic Compounds

• Typically composed of hydrogen and carbon atoms, with possible presence of oxygen, nitrogen, sulfur, and phosphorus
• Low melting and boiling points are common characteristics
• Often exhibit distinct odors and colors

Functional Groups

• Specific groups of atoms that determine a molecule's chemical properties
• Examples:
  • Hydroxyl (-OH) functional group
  • Carboxyl (-COOH) functional group
  • Amino (-NH2) functional group
  • Methyl (-CH3) functional group

Types of Organic Compounds

• Alkanes: Saturated hydrocarbons with single bonds, e.g., methane (CH4) and ethane (C2H6)
• Alkenes: Unsaturated hydrocarbons with one or more double bonds, e.g., ethene (C2H4) and propene (C3H6)
• Alkynes: Unsaturated hydrocarbons with one or more triple bonds, e.g., ethyne (C2H2) and propyne (C3H4)
• Arenes: Aromatic hydrocarbons with planar, ring-shaped structures, e.g., benzene (C6H6)
• Alcohols: Compounds with a hydroxyl (-OH) functional group, e.g., methanol (CH3OH) and ethanol (C2H5OH)
• Ethers: Compounds with an oxygen atom bonded to two alkyl groups, e.g., diethyl ether (C4H10O)
• Carboxylic Acids: Compounds with a carboxyl (-COOH) functional group, e.g., acetic acid (CH3COOH) and citric acid (C6H8O7)
• Amines: Compounds with an amino (-NH2) functional group, e.g., ammonia (NH3) and methylamine (CH3NH2)

Isomerism

• Structural Isomerism: Same molecular formula, different arrangements of atoms, e.g., butane (C4H10) and isobutane (C4H10)
• Stereoisomerism: Same molecular formula, different arrangements of atoms in space, e.g., enantiomers and diastereomers

Reactions

• Substitution Reactions: Replacement of a functional group with another functional group, e.g., chlorination of methane
• Elimination Reactions: Removal of a functional group to form a new bond, e.g., dehydration of ethanol
• Addition Reactions: Addition of a functional group to a molecule, e.g., hydrogenation of ethene
• Oxidation-Reduction Reactions: Gain or loss of electrons resulting in a change in oxidation state, e.g., combustion of methane