Lecture Notes: Introduction to Organic Chemistry

Experiment with Reverse Psychology

• Presenter initiated an experiment by telling viewers not to watch the video to see if they'd still watch it.
• Asked viewers to comment why they chose to watch the video despite the warning.
• Possible reasons: curiosity or interest in learning organic chemistry.

Introduction to Organic Chemistry (Orgo Chem)

• Designed for beginners or those about to take an organic chemistry course.

Lewis Structures

Periodic Table Groups and Valence Electrons

• Group 1 (e.g., Hydrogen, Lithium, Sodium): 1 valence electron, typically form 1 bond.
• Group 2 (e.g., Beryllium): 2 valence electrons, typically form 2 bonds.
• Group 3A (e.g., Boron): 3 valence electrons, typically form 3 bonds.
• Group 4 (e.g., Carbon): 4 valence electrons, typically form 4 bonds.
• Group 5 (e.g., Nitrogen): 5 valence electrons, typically form 3 bonds to achieve octet rule.
• Group 6 (e.g., Oxygen): 6 valence electrons, typically form 2 bonds.
• Group 7 (e.g., Fluorine): 7 valence electrons, typically forms 1 bond, true for other halogens (Chlorine, Bromine, Iodine).

Examples of Drawing Lewis Structures

• Methane (CH4): Carbon forms 4 bonds with Hydrogen.
• Ethane (CH3CH3): Two Carbon atoms each form 3 bonds with Hydrogen and 1 bond with another Carbon.
• Propane (CH3CH2CH3): Three Carbon atoms, 8 Hydrogen atoms; all Carbons form 4 bonds in total.
• Ethylene (C2H4): Two Carbon atoms each with 2 Hydrogen atoms and a double bond between Carbons.
• Acetylene (C2H2): Two Carbon atoms each with 1 Hydrogen atom and a triple bond between Carbons.

Saturation of Hydrocarbons

• Alkanes: Saturated hydrocarbons with single bonds.
• Alkenes: Unsaturated hydrocarbons with at least one double bond.
• Alkynes: Unsaturated hydrocarbons with at least one triple bond.

Naming Alkanes, Alkenes, and Alkynes

• Methane (CH4): 1 Carbon, alkane.
• Ethane (C2H6): 2 Carbons, alkane.
• Ethylene (Ethene, C2H4): 2 Carbons, alkene.
• Acetylene (Ethyne, C2H2): 2 Carbons, alkyne.
• Propanol, Butanol, Hexane, etc.: Naming follows similar structure with varying carbon chains.

Functional Groups

• Alcohol (e.g., Methanol): -OH group.
• Ether (e.g., Dimethyl ether): R-O-R' structure.
• Ketone (e.g., Butanone): Carbonyl group (C=O) within a carbon chain.
• Aldehyde (e.g., Ethanal): Carbonyl group (C=O) at the end of a carbon chain.
• Carboxylic Acid (e.g., Propanoic acid): -COOH group.
• Esters, Amines, Amides, Nitriles, Acid Chlorides, Benzene Ring: Other functional groups important in organic chemistry.

Formal Charge Calculation

• Formula: Valence electrons - (number of bonds + number of lone pair electrons).
• Examples with Oxygen, Nitrogen, etc., showing how to determine charges in different structures.

Resonance Structures

• Definition: Different ways of drawing the same molecule using electron movement without changing atom positions.
• Examples: Resonance in ions like acetate, amides, and carbocations.

IUPAC Naming of Alkanes

• Rules: Choose the longest carbon chain, number it for the lowest set of locants for substituents, alphabetize substituents.
• Examples: Hexane, heptane, methyl, and ethyl substituents.

Additional Resources

• Mention of additional videos and resources on Lewis structures, resonance, naming conventions, etc. available on the presenter's YouTube channel.