Organic Chemistry Overview

Definition: Study of carbon-containing compounds and their properties.
Key Concepts:
- Functional Groups: Specific groups of atoms that determine the characteristics and reactions of organic molecules (e.g., -OH, -COOH, -NH2).
- Hydrocarbons: Compounds made of hydrogen and carbon; includes alkanes, alkenes, and alkynes.
- Isomerism: Compounds with the same molecular formula but different structures (e.g., structural isomers, stereoisomers).
- Reactions:
  - Substitution Reactions: Replacement of one atom or group in a molecule.
  - Addition Reactions: Atoms are added to a molecule (common in alkenes).
  - Elimination Reactions: Removal of a molecule from a saturated compound to form an unsaturated compound.
Key Types of Compounds:
- Amines: Derivatives of ammonia, important in biology.
- Carboxylic Acids: Contain -COOH, responsible for acidity in organic compounds.
- Esters: Formed from an alcohol and a carboxylic acid, often fruity in smell.

Definition: Study of inorganic compounds, primarily those that do not contain carbon-hydrogen bonds.
Key Concepts:
- Periodic Table: Organization of elements based on atomic structure and properties; groups and periods indicate similar reactivity.
- Coordination Compounds: Consist of a central metal atom bonded to surrounding molecules or ions (ligands).
- Acids and Bases:
  - Arrhenius Definition: Acids produce H+ ions, bases produce OH- ions in water.
  - Brønsted-Lowry Definition: Acids are proton donors, bases are proton acceptors.
- Oxidation States: Indicate the degree of oxidation of an atom in a compound; important for understanding redox reactions.
Important Classes of Compounds:
- Salts: Formed from the neutralization of an acid and a base.
- Metals and Alloys: Conductive materials with specific properties used in various applications.

Definition: Study of how matter behaves on a molecular and atomic level, and how chemical reactions occur.
Key Concepts:
- Thermodynamics: Study of energy, heat, and work; includes laws of thermodynamics governing energy transfer.
- Kinetics: Study of reaction rates; factors influencing rates include concentration, temperature, and catalysts.
- Quantum Chemistry: Application of quantum mechanics to chemical systems; explains the behavior of electrons in atoms and molecules.
- Chemical Equilibrium: The state where the rate of the forward reaction equals the rate of the reverse reaction, characterized by the equilibrium constant (K).
States of Matter:
- Solid: Fixed shape and volume; particles are closely packed.
- Liquid: Fixed volume but takes the shape of the container; particles are less tightly packed.
- Gas: No fixed shape or volume; particles are far apart and move freely.

These summaries provide a foundational overview of the major subfields of chemistry, emphasizing their primary concepts and categories.

Study of carbon-containing compounds, their structure, properties, and reactions.
Functional Groups: Determine the nature and reactions of organic molecules (e.g., hydroxyl -OH, carboxyl -COOH, amino -NH2).
Hydrocarbons: Composed solely of hydrogen and carbon, categorized into alkanes (single bonds), alkenes (double bonds), and alkynes (triple bonds).
Isomerism: Occurrence of compounds with identical molecular formulas but differing structural arrangements including structural isomers and stereoisomers.
Reactions:
- Substitution Reactions: Involve replacing an atom or group in a molecule.
- Addition Reactions: Atoms are added to double or triple bonded structures, common in alkenes.
- Elimination Reactions: Involve removal of a small molecule from a saturated compound, resulting in an unsaturated compound.
Key Types of Compounds:
- Amines: Organic derivatives of ammonia significant in biological processes.
- Carboxylic Acids: Characterized by the carboxyl group -COOH, imparting acidity to organic substances.
- Esters: Formed from the reaction of an alcohol and a carboxylic acid, typically with a fruity aroma.

Study of inorganic compounds, mainly those lacking carbon-hydrogen bonds.
Periodic Table: Arrangement of elements by atomic structure; groups and periods reflect similar chemical properties and reactivity.
Coordination Compounds: Structures featuring a central metal atom surrounded by ligands (molecules or ions).
Acids and Bases:
- Arrhenius Definition: Classifies acids as substances that produce H+ ions and bases as OH- ion producers in aqueous solutions.
- Brønsted-Lowry Definition: Defines acids as proton donors and bases as proton acceptors.
Oxidation States: Indicate how many electrons an atom has gained or lost, crucial for understanding redox (reduction-oxidation) reactions.
Important Classes of Compounds:
- Salts: Result from the neutralization reaction between an acid and a base.
- Metals and Alloys: Materials featuring conductive properties, widely utilized in various fields due to their unique characteristics.

Study of matter's behavior at atomic and molecular levels and the dynamics of chemical reactions.
Thermodynamics: Focuses on energy transformations, heat, and work, guided by laws that dictate energy movement.
Kinetics: Analyzes factors affecting reaction rates such as concentration, temperature, and the presence of catalysts.
Quantum Chemistry: Employs quantum mechanics to elucidate electron behavior within atoms and molecules.
Chemical Equilibrium: Describes a state where the rates of forward and reverse reactions are equal, defined by the equilibrium constant (K).
States of Matter:
- Solid: Possesses a fixed shape and volume, with particles densely packed.
- Liquid: Maintains a constant volume but adopts the shape of its container; particles are less tightly packed.
- Gas: Lacks fixed shape and volume, with particles widely spaced and moving freely.