- Bohr's Theory: Explains the structure of an atom, with electrons orbiting around the nucleus in specific energy levels.
- Quantum Numbers: Describes the energy, position, and orientation of electrons in an atom.
- Pauli's Exclusion Principle: States that no two electrons in an atom can have the same set of quantum numbers.
- Hund's Rule: States that electrons occupy orbitals of equal energy singly before pairing up.


- Valence Bond Theory: Describes the formation of chemical bonds by overlapping atomic orbitals.
- Molecular Orbital Theory: Explains the bonding in molecules using molecular orbitals formed by the combination of atomic orbitals.
- VSEPR Theory: Predicts the molecular geometry based on the repulsion between electron pairs around a central atom.
- Hybridization: Describes the mixing of atomic orbitals to form hybrid orbitals for bonding.


- First Law of Thermodynamics: States that energy can neither be created nor destroyed, only transferred or converted from one form to another.
- Hess's Law: States that the enthalpy change of a reaction is independent of the pathway taken.
- Second Law of Thermodynamics: States that the entropy of an isolated system always increases in a spontaneous process.
- Gibbs Free Energy: Relates the spontaneity of a reaction to its enthalpy and entropy changes.


- Le Chatelier's Principle: States that when a system at equilibrium is subjected to a change, it will shift in a direction that reduces the effect of the change.
- Law of Mass Action: Describes the relationship between the concentrations of reactants and products at equilibrium.
- Equilibrium Constant (K): Represents the ratio of product concentrations to reactant concentrations at equilibrium.


- IUPAC Nomenclature: Provides a systematic way of naming organic compounds.
- Isomerism: Describes the different structural arrangements of molecules with the same molecular formula.
- Functional Groups: Groups of atoms responsible for the characteristic chemical reactions of organic compounds.
- Reaction Mechanisms: Describes the step-by-step pathways by which reactions occur.


- Faraday's Laws of Electrolysis: Relates the amount of substance produced or consumed during an electrolysis reaction to the electric current flowing through the electrolyte.
- Nernst Equation: Relates the potential of an electrochemical cell to the concentrations of reactants and products.
- Galvanic Cells: Devices that convert chemical energy into electrical energy through redox reactions.


- Rate Laws: Describes the relationship between the rate of a reaction and the concentrations of reactants.
- Activation Energy: The energy required for a reaction to occur.
- Collision Theory: States that reactions occur when reactant particles collide with sufficient energy and proper orientation.


- Werner's Theory: Describes