Basic Concepts of Chemistry

Definition: Chemistry is the scientific study of matter, its properties, composition, structure, and the changes it undergoes during chemical reactions.
Branches:
- Organic Chemistry: Study of carbon-containing compounds.
- Inorganic Chemistry: Study of inorganic compounds, primarily those not containing carbon.
- Physical Chemistry: Study of the physical properties and changes of matter.
- Analytical Chemistry: Techniques and methods to analyze substances.
- Biochemistry: Study of chemical processes in living organisms.

Definition: Anything that has mass and occupies space.
States of Matter:
- Solid: Definite shape and volume.
- Liquid: Definite volume, but takes the shape of its container.
- Gas: No definite shape or volume, expands to fill its container.
Changes of State:
- Melting, freezing, condensation, evaporation, and sublimation.

Atoms: Basic units of matter.
- Composed of protons (+), neutrons (neutral), and electrons (-).
Atomic Number: Number of protons in an atom, defines the element.
Mass Number: Total number of protons and neutrons.
Isotopes: Atoms of the same element with different numbers of neutrons.

Ionic Bonds: Formed through the transfer of electrons from one atom to another.
Covalent Bonds: Formed when two atoms share electrons.
Metallic Bonds: Bonding between metal atoms, involving a 'sea' of delocalized electrons.

Reactants and Products: Substances that undergo change (reactants) and the new substances formed (products).
Types of Reactions:
- Synthesis: Combination of two or more substances to form one compound.
- Decomposition: Breakdown of a compound into simpler products.
- Single Replacement: One element replaces another in a compound.
- Double Replacement: Exchange of ions between two compounds.
- Combustion: Reaction with oxygen, producing heat and light.

Acids: Substances that donate protons (H+) in solutions.
Bases: Substances that accept protons or donate hydroxide ions (OH-) in solutions.
pH Scale: Measures the acidity or basicity of a solution (0-14 scale).

Definition: Study of the quantitative relationships in chemical reactions.
Mole Concept: A mole represents 6.022 x 10²³ particles of a substance.
Balanced Equations: Conservation of mass is vital; the number of atoms must be the same on both sides of a reaction.

Solvent: Substance that dissolves another substance (usually liquid).
Solute: Substance that is dissolved.
Concentration: Amount of solute in a given volume of solvent (often expressed in molarity).

Titration: Method to determine the concentration of a solution by reacting it with a standard solution.
Chromatography: Technique for separating mixtures based on different interactions with a stationary phase.

Personal Protective Equipment (PPE): Use of gloves, goggles, and lab coats.
Safety Data Sheets (SDS): Provide information on handling, hazards, and emergency measures for chemicals.

These notes provide a foundational understanding of key concepts in chemistry and can be expanded upon with more detailed study in specific areas.

Chemistry studies matter, its properties, composition, structure, and changes in chemical reactions.
Five main branches of chemistry:
- Organic Chemistry examines carbon-containing compounds.
- Inorganic Chemistry focuses on inorganic compounds, generally lacking carbon.
- Physical Chemistry looks at the physical properties and changes of matter.
- Analytical Chemistry involves techniques to analyze substances.
- Biochemistry studies chemical processes in living organisms.

Matter is anything with mass that occupies space.
Three states of matter:
- Solids have a definite shape and volume.
- Liquids have a definite volume but take the shape of their container.
- Gases have no definite shape or volume, expanding to fill their container.
Changes of state include melting, freezing, condensation, evaporation, and sublimation.

Atoms are the basic units of matter, consisting of protons (positively charged), neutrons (neutral), and electrons (negatively charged).
Atomic Number indicates the number of protons and determines the element identity.
Mass Number is the sum of protons and neutrons in an atom.
Isotopes are variants of the same element differing in neutron count.

Ionic Bonds form through electron transfer between atoms, creating charged ions.
Covalent Bonds arise when two atoms share electrons.
Metallic Bonds feature delocalized electrons, allowing conductivity and malleability among metal atoms.

Reactants are the starting substances, while products are the new substances produced from a reaction.
Types of reactions include:
- Synthesis: Multiple substances combine to form a single compound.
- Decomposition: A compound breaks down into simpler substances.
- Single Replacement: An element replaces another in a compound.
- Double Replacement: Two compounds exchange ions.
- Combustion: A reaction with oxygen that yields heat and light.

Elements are organized by increasing atomic number.
Groups or families are vertical columns indicating similar chemical behaviors.
Periods are horizontal rows signifying the arrangement of electrons in energy levels.

Stoichiometry explores quantitative relationships in chemical reactions.
The mole concept defines a mole as 6.022 x 10²³ particles of a substance.
Balanced Equations are essential for mass conservation, maintaining equal atom counts on both sides of a reaction.

A Solvent dissolves another substance, typically a liquid.
A Solute is the substance that gets dissolved.
Concentration measures the solute amount in a given solvent volume, often expressed in molarity.

Titration is used to determine solution concentration by reacting it with a standard solution.
Chromatography separates mixtures based on different interactions with a stationary phase.

Personal Protective Equipment (PPE) such as gloves, goggles, and lab coats is crucial for safety.
Safety Data Sheets (SDS) provide essential information on chemical handling, hazards, and emergency protocols.