7.Organic_Chemistry-Modules_27-32

Organic Chemistry Study Guide

Page 1: Resources

  • Practice Questions: Complete questions on pages 6, 21, 29, 54.

  • Lecture Notes: Print and review as usual.

  • Textbook Chapters:

    • Nomenclature & Isomers: Chapters 23, Sections 23.1-23.7.

      • Questions: 23.1, 23.3, 23.10, 23.14-23.18, 23.25, 23.29, 23.35, 23.39, 23.41, 23.53, 23.55, 23.65

    • Physical Properties: Chapter 11, Section 11.5.

      • Questions: 11.63, 11.65, 11.71, 24.25

    • Condensation Polymers: Chapter 24, Section 24.1.

      • Questions: 24.29, 24.31, 24.53, 24.55

Page 2: Chemistry of Carbon Compounds

  • Carbon Compounds: Approximately 20 times more known compounds containing carbon than those without.

  • Isomers: Same molecular formula but different structures and properties.

  • Reasons for Variety in Organic Compounds:

    1. Carbon's ability to form strong covalent bonds with itself.

    2. Carbon can form four covalent bonds.

Page 3: Classification Based on Functional Groups

  • Functional Groups and Examples:

    • Alkanes: None (e.g., Ethane)

    • Alkenes: >C=C< (e.g., Ethene)

    • Aromatics: (e.g., Toluene)

    • Alkynes: -C≡C- (e.g., Ethyne)

    • Halides: -C-X (e.g., Chloromethane)

    • Ethers: -C-O-C- (e.g., Dimethyl ether)

    • Alcohols: -C-OH (e.g., Methanol)

    • Amines: -C-N- (e.g., Methylamine)

    • Aldehydes: O=C-H (e.g., Ethanal)

    • Ketones: O=C-C (e.g., Propanone)

    • Carboxylic Acids: O=C-OH (e.g., Ethanoic acid)

    • Esters: O=C-O-(e.g., Methyl ethanoate)

    • Acid Chlorides: O=C-Cl (e.g., Ethoyl chloride)

    • Amides: O=C-N (e.g., Acetamide)

Page 4: Hydrocarbons

  • Definition: Simplest organic compounds made only of C and H.

  • Saturated Hydrocarbons: Only C-C bonds and maximum H for each carbon.

  • Classes of Saturated Hydrocarbons:

    1. Alkanes: Formula - CnH2n+2.

    2. Cycloalkanes: Ring structures, formula - CnH2n.

  • Common Alkanes:

    • CH4 (Methane)

    • C2H6 (Ethane)

    • C3H8 (Propane)

    • C4H10 (Butane)

    • C5H12 (Pentane)

    • C6H14 (Hexane)

    • C7H16 (Heptane)

    • C8H18 (Octane)

    • C9H20 (Nonane)

    • C10H22 (Decane)

Page 5: Substituents and IUPAC Rules

  • Alkyl Substituents Derived from Alkanes:

    • CH3- (Methyl)

    • C2H5- (Ethyl)

    • C3H7- (Propyl)

    • etc.

  • IUPAC Naming Rules:

    1. Identify the longest C chain.

    2. Number chains from the end closest to substituents.

    3. Name the chain.

    4. Use prefixes for multiple substituents (di, tri, tetra, etc.).

    5. List substituents in alphabetical order.

    6. Punctuation rules for naming.

Page 6: Nomenclature of Unsaturated Hydrocarbons

  • Alkenes and Alkynes:

    • Alkenes: CnH2n.

    • Alkynes: CnH2n-2.

    • Naming: Identify longest chain; use 'ene' or 'yne' based on functional groups.

Page 7: Functional Groups

  • 1. Organic Halogen Compounds:

    • Classification as alkyl halides or aryl halides; strong electrophiles.

  • 2. Ethers: R-O-R, commonly used as solvents.

  • 3. Alcohols and Phenols:

    • Alcohols are hydrocarbons with -OH groups (RH).

  • 4. Amines: Derived from ammonia; basic nature.

Page 8: Aldehydes, Ketones, Carboxylic Acids

  • Aldehydes: Contain a carbonyl (C=O) group at the end; named with '-anal'.

  • Ketones: Carbonyl (C=O) group in the middle; ending '-anone'.

  • Carboxylic Acids: Contain -COOH group, ending '-anoic acid'.

Page 9: Classifying Carbons and Hydrogens

  • Types of Carbons:

    • Primary (1), Secondary (2), and Tertiary (3).

    • Electrons attached to carbon atoms are classified similarly.

Page 10: Stereochemistry and Isomers

  • Structural or Constitutional Isomers: Different connectivity.

    • Types include skeletal, positional, functional, etc.

    • Example Molecular Formula: C4H8O2 can yield various structures.

  • Geometric Isomers: Different spatial arrangements due to double bonds or rings.

Page 17: Properties of Organic Compounds

  • Physical Properties: Influenced by intermolecular forces such as:

    • Ion-Ion, Hydrogen Bonding, Dipole-Dipole, and London Dispersion Forces.

  • Impact of Intermolecular Forces: Affects boiling points and solubility. Higher forces = higher boiling point.

Page 32: Reactions of Alcohols

  • Oxidation: Primary alcohol to aldehyde, can further oxidize to carboxylic acid.

  • Secondary Alcohol: Converts to ketone.

  • Tertiary Alcohol: Does not oxidize due to a lack of hydrogen.

Page 39: Preparation of Carboxylic Acids

  • Oxidation: 1º alcohols or aldehydes.

  • Esters Formation: Via acid + alcohol.

  • Amides Formation: Less effective via direct reaction; often via esterization.

Page 44: Organic Acids and Bases

  • Acids: Weak acids include carboxylic acids, while alcohols are very weak acids.

  • Bases: Can donate lone pair electrons.

  • Salt Formation: Between organic acid/base and strong base/acid.

Important Notes

  • Refer to practice question answers for further review.

  • Ensure understanding of nomenclature, functional groups, and reaction mechanisms to prepare effectively for the exam.