Intro-to-Organic-Chemistry

Page 1: Introduction to Organic Compounds

• Topics Covered: Nomenclature, physical properties, and structure representation.

Page 2: What is Organic Chemistry?

• Definition: The chemistry of carbon compounds.

• Carbon (C) Details:

  • Symbol: C

  • Atomic Number: 6

  • Atomic Mass: 12.011

  • Discovered by Lavoisier in 1789.

• Other Elements Related to Carbon:

  • Silicon (Si)

  • Germanium (Ge)

  • Tin (Sn)

  • Lead (Pb)

Page 3: Abundance of Elements in Earth's Crust

• Key Element Percentages:

  • Oxygen (O): 25.7%

  • Silicon (Si): 49.5%

  • Other Elements:

    • Aluminium: 7.4%

    • Iron: 4.7%

    • Calcium: 3.4%

    • Sodium: 2.6%

    • Potassium: 2.4%

    • Magnesium: 1.9%

    • Hydrogen: 0.9%

    • Titanium: 0.6%

    • Others: 0.9%

Page 4: The Chemistry of Carbon

• Carbon Characteristics:

  • Versatile due to having 4 valence electrons.

  • Forms covalent bonds with H, O, P, S, and N.

  • Capable of forming long carbon chains.

Page 5: Types of Bonds in Carbon Compounds

• Carbon Bonding:

  • Typically forms four covalent bonds with no unshared pairs.

  • Other Elements:

    • Nitrogen: 3 covalent bonds, 1 unshared pair.

    • Oxygen: 2 covalent bonds, 2 unshared pairs.

    • Hydrogen: 1 covalent bond, no unshared pairs.

    • Halogens (F, Cl, Br, I): 1 covalent bond, 3 unshared pairs.

Page 6: Carbon Connectivity

• Carbon binds to functional groups:

  • Hydroxyl (-OH) groups in sugars.

  • Amino (-NH2) groups in amino acids.

  • Phosphate (-H2PO4) groups in nucleotides (DNA, RNA, ATP).

Page 7: Sources of Organic Compounds

• A. Isolation from Nature

• B. Synthesis in the Laboratory

• Example: Vitamin C from oranges is chemically identical to synthetic forms.

Page 8: Representing Organic Compounds

• Types of Formulas:

  • Molecular Formula: C4H10

  • Structural Formula: H-CH2-CH2-CH3

  • Condensed Formula: CH3-CH2-CH2-CH3

  • Line Formula: (for graphical representation)

Page 9: Practice on Structural/Formulas

• Examples of drawing different formulas and converting between types.

Page 10: Continued Practice

• More exercises to translate between Structural, Condensed, and Line formulas.

Page 11: Expanded Practice on Formulas

• More complex examples of condensates and structural representation.

Page 12: Families of Organic Compounds

• Hydrochemical Definitions:

  • Hydrocarbon: contains only carbon and hydrogen.

  • Substituted Hydrocarbon: hydrogen atoms are replaced with other atoms/groups.

Page 13: Properties of Hydrocarbons

• Key Characteristics:

  • Non-polar molecules.

  • Weak van der Waals forces leading to low boiling points for smaller hydrocarbons.

  • Non-soluble in polar substances (like water).

Page 14: Aliphatic Hydrocarbons - Alkanes

• All single bonds.

• Saturated with hydrogen.

• General Formula: CnH2n+2.

• Least reactive hydrocarbons, typically used as fuels.

Page 15: Root Names for Hydrocarbons

• Naming conventions based on the number of carbon atoms:

  • 1: Meth-

  • 2: Eth-

  • 3: Prop-

  • (continues through 10).

Page 16: Naming Straight-Chain Alkanes

• Methane as the first type and extending naming conventions for subsequent alkanes.

Page 17: Completing Alkane Nomenclature

• Table completion for the first 10 alkanes and their formulas.

Page 18: Branched-Chain Alkanes

• Definition: Alkanes with one or more alkyl groups attached.

Page 19: Alkyl Groups

• Definition: Hydrocarbon fragments with one less hydrogen than alkane.

• General Formula: CnH2n+1.

• Naming approach for alkyl groups, e.g., heptyl (C7H15).

Page 20: Common Alkyl Groups

• Examples: Methyl, Ethyl, Propyl, and their structures represented.

Page 21: Naming Branched-Chain Alkanes

• Steps in naming:

  1. Count carbons in the longest chain.

  2. Number for minimal side chain positions.

  3. Name and number side chains alphabetically.

Page 22: Practice Naming Alkanes

• Example: 4-ethyl-3-methylheptane.

Page 23: Advanced Naming Problems

• Practice problems presented requiring naming and structural understanding.

Page 24: More Advanced Naming Problems

• Continuation of naming exercises.

Page 25: Cycloalkanes

• Definition: Alkanes with carbon forming a ring structure.

• Naming: Add prefix "cyclo" to the base alkane name.

Page 26: Examples of Cycloalkanes

• Different named cycloalkanes with structural representations.

Page 27: More Practice

• Exercises to practice naming and identifying cycloalkanes.

Page 28: Alkenes and Alkynes

• Alkenes: Hydrocarbon with at least one double bond (General Formula: CnH2n).

• Alkynes: Hydrocarbon with at least one triple bond (General Formula: CnH2n-2).

Page 29: Naming Alkenes

• Examples of alkenes and their naming conventions.

Page 30: Continued Practice Naming Alkenes

• Provided molecular structure examples to practice naming.

Page 31: Advanced Alkenes Naming

• Practice on determining alkene structures for proper naming.

Page 32: Further Number Assignments

• Continuing systematic number assignments for branched alkenes.

Page 33: Assigning Numbers for Alkene Names

• Explanation of how to assign numbers based on double bond positions.

Page 34: Continued Number Assignments for Alkenes

• Continued practice of number assignments with examples.

Page 35: Name for Side Chains in Alkenes

• Stylized format for naming side branches in alkene formulas.

Page 36: Final Name for Alkenes and Side Chains

• Name resulting from assignments and conventions outlined.

Page 37: Group Similar Branches in Alkenes

• Methods for simplifying and grouping names for branched alkenes.

Page 38: Similar Branches in Alkene Naming

• Techniques used for finalizing alkene names.

Page 39: Representation of Alkene Names

• Examples showing the final representation of both structures and names.

Page 40: Naming Practice for Similar Structures

• Analytical practice with solutions showing correct nomenclature.

Page 41: Visual Examples of Hydrocarbons

• Visual representation of molecules for clarity in understanding.

Page 42: Examples of Alkynes

• Examples associated with naming and structural representations (C2H2, C3H4, etc.).

Page 43: Review of Hydrocarbon Types

• Summary of alkanes, cycloalkanes, alkenes, and alkynes; molecular formulas included.

Page 44: Hydrocarbon Isomerism

• Isomerism defined with examples and boiling points.

Page 45: Types of Isomers

• Definitions:

  • Isomers: Same formula, different structures.

  • Constitutional Isomers: Different arrangements of the same atoms.

Page 46: Examples of Isomers

• Illustrated examples demonstrating positional variances in hydrocarbons.

Page 47: Aromatic Compounds

• Aromatic hydrocarbons with benzene rings (C6H6).

• Foundational discoveries by Faraday and Kekulé.

Page 48: Examples of Aromatic Compounds

• Compounds like Naphthalene and their applications as moth repellents, etc.

Page 49: Further Classifications of Aromatic Compounds

• Naming and representations for several aromatic structures.

Page 50: Common Nomenclature Pitfalls

• Common errors to avoid in naming conventions e.g., incorrect carbon chain identification, improper enumeration.

Page 51: Functional Groups

• Definition: Atoms/groups exhibiting specific properties in molecular structures.

Page 52: Biomolecules and Functional Groups

• Functional groups give specific properties to biomolecules (e.g., hydroxyl group).

Page 53: Importance of Functional Groups

• Role in predictable chemical behavior, physical properties, classification of organic compounds, and their naming.