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:
Count carbons in the longest chain.
Number for minimal side chain positions.
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.