Basic Chemistry Concepts and Reactions

Matter: Anything that has mass and occupies space.
Atoms: Basic units of matter, consisting of protons, neutrons, and electrons.
Elements: Pure substances made of only one type of atom; represented on the periodic table.
Compounds: Substances formed from two or more elements chemically combined in fixed ratios.

Ionic Bonds: Formed when electrons are transferred from one atom to another, creating charged ions.
Covalent Bonds: Formed when atoms share electrons.
Metallic Bonds: Attraction between metal atoms and delocalized electrons, allowing for conductivity.

Solid: Definite shape and volume; particles are tightly packed.
Liquid: Definite volume but no definite shape; particles are close but can move past one another.
Gas: No definite shape or volume; particles are far apart and move freely.

Reactants: Substances that undergo chemical changes.
Products: Substances formed as a result of a chemical reaction.
Types of Reactions:
- Synthesis: Two or more substances combine to form a new compound.
- Decomposition: A single compound breaks down into simpler products.
- Single Replacement: One element replaces another in a compound.
- Double Replacement: Exchange of ions between two compounds.

Mole: A unit that measures the amount of substance (6.022 x 10²³ entities).
Molar Mass: The mass of one mole of a substance, typically in g/mol.
Stoichiometry: The calculation of reactants and products in chemical reactions based on balanced equations.

Acids: Substances that donate protons (H⁺) in solutions; characterized by a sour taste.
Bases: Substances that accept protons; characterized by a bitter taste and slippery feel.
pH Scale: Measures the acidity or basicity of a solution (0-14 scale: <7 = acid, 7 = neutral, >7 = base).

Exothermic Reactions: Release heat to the surroundings (e.g., combustion).
Endothermic Reactions: Absorb heat from the surroundings (e.g., photosynthesis).

Solution: A homogeneous mixture of solute and solvent.
Concentration: Amount of solute in a given volume of solution, often expressed in molarity (M = moles of solute/L of solution).

Atomic Radius: Increases down a group, decreases across a period.
Electronegativity: Tendency of an atom to attract electrons; increases across a period, decreases down a group.
Ionization Energy: Energy required to remove an electron from an atom; increases across a period, decreases down a group.

Titration: Technique to determine concentration of a solution by reacting it with a standard solution.
Filtration: Separation technique to remove solids from liquids.
Distillation: Process of separating mixtures based on boiling points.

Matter: Anything that has mass and takes up space.
Atoms: The basic building blocks of matter, consisting of protons, neutrons, and electrons.
Elements: Pure substances composed of only one type of atom. Represented on the periodic table.
Compounds: Substances formed when two or more elements chemically combine in fixed ratios.

Ionic Bonds: Formed when electrons are transferred from one atom to another, creating positively and negatively charged ions that attract each other.
Covalent Bonds: Formed when atoms share electrons to achieve a stable electron configuration.
Metallic Bonds: Result from the attraction between metal atoms and delocalized electrons, allowing for high conductivity.

Solid: Definite shape and volume, with tightly packed particles that vibrate in fixed positions.
Liquid: Definite volume but no definite shape, with particles close together but able to move past one another.
Gas: No definite shape or volume, with particles widely spaced and moving freely.

Reactants: Substances that undergo chemical changes during a reaction.
Products: Substances formed as a result of a chemical reaction.
Types of Reactions:
- Synthesis: Two or more substances combine to form a new compound (A + B → AB).
- Decomposition: A single compound breaks down into simpler products (AB → A + B).
- Single Replacement: One element replaces another in a compound (A + BC → AC + B).
- Double Replacement: Exchange of ions between two compounds (AB + CD → AD + CB).

Mole: A unit of measurement for the amount of substance, representing 6.022 x 10²³ entities.
Molar Mass: The mass of one mole of a substance, typically expressed in grams per mole (g/mol).
Stoichiometry: The study of quantitative relationships between reactants and products in chemical reactions, allowing for the calculation of amounts involved in a reaction based on balanced chemical equations.

Acids: Substances that can donate protons (H⁺) in solutions, often characterized by a sour taste.
Bases: Substances that can accept protons, typically characterized by a bitter taste and slippery feel.
pH Scale: A measure of acidity or basicity, ranging from 0 to 14, with 7 representing neutral.

Exothermic Reactions: Release heat to the surroundings, resulting in a decrease in the system's temperature.
Endothermic Reactions: Absorb heat from the surroundings, resulting in an increase in the system's temperature.

Solution: A homogeneous mixture of solute and solvent.
Concentration: The amount of solute in a given volume of solution, often expressed as molarity (M = moles of solute/liter of solution).

Atomic Radius: Tends to increase down a group and decrease across a period on the periodic table.
Electronegativity: The tendency of an atom to attract electrons in a chemical bond. Increases across a period and decreases down a group.
Ionization Energy: The energy required to remove an electron from an atom in its gaseous state. Increases across a period and decreases down a group.

Titration: A technique used to determine the concentration of a solution by reacting it with a standard solution of known concentration.
Filtration: A separation technique used to separate solid particles from a liquid mixture.
Distillation: A process used to separate liquids with different boiling points.