Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Atomic Structure

Organic Chemistry

1. A Review of General Chemistry

Atomic Structure

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Multiple Choice

PRACTICE: Determine which of the three principles of electron configuration is being broken in the electron diagrams below.

Hund's Rule

Aufbau Principle

Pauli Exclusion Principle

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Verified step by step guidance

Examine the electron configuration diagram provided. Notice the distribution of electrons in the 2p orbitals.

Identify the three principles of electron configuration: Hund's Rule, the Aufbau Principle, and the Pauli Exclusion Principle.

Hund's Rule states that every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied. Check if this rule is being followed in the 2p orbitals.

The Aufbau Principle states that electrons fill lower energy orbitals first before moving to higher energy orbitals. Verify if the electrons are filling the orbitals in the correct order of increasing energy.

The Pauli Exclusion Principle states that no two electrons in the same atom can have identical quantum numbers, meaning an orbital can hold a maximum of two electrons with opposite spins. Ensure that this principle is not violated in the diagram.