Basic Concepts in Chemistry

Matter: Anything that has mass and occupies space; exists in three states: solid, liquid, gas.
Elements: Pure substances that cannot be broken down into simpler substances; represented on the periodic table.
Compounds: Substances formed when two or more elements chemically combine; can be broken down into simpler substances.

Atoms: Basic units of matter; consist of protons, neutrons, and electrons.
- Protons: Positive charge, found in the nucleus.
- Neutrons: No charge, found in the nucleus.
- Electrons: Negative charge, orbit around the nucleus.
Atomic Number: Number of protons in an atom; defines the element.
Mass Number: Total number of protons and neutrons in the nucleus.

Ionic Bonds: Formed when electrons are transferred from one atom to another, resulting in charged ions.
Covalent Bonds: Formed when atoms share electrons.
Metallic Bonds: Formed by the attraction between metal atoms and the surrounding sea of electrons.

Reactants: Substances that undergo chemical change.
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 compound breaks down into simpler substances.
- 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; one mole contains Avogadro's number of particles (6.022 x 10²³).
Balancing Equations: Ensuring the number of atoms for each element is equal on both sides of a chemical equation.

Acids: Substances that release hydrogen ions (H⁺) in solution; pH less than 7.
Bases: Substances that release hydroxide ions (OH⁻) in solution; pH greater than 7.
pH Scale: Measures acidity or alkalinity on a scale of 0 to 14.

Hydrocarbons: Compounds made up of hydrogen and carbon; include alkanes, alkenes, and alkynes.
Functional Groups: Specific groups of atoms that determine the characteristics and reactions of organic compounds.

Salts: Ionic compounds formed from the reaction of acids and bases.
Coordination Compounds: Complexes formed from a central metal atom bonded to surrounding ligands.

Safety Equipment: Use goggles, gloves, and lab coats.
Proper Handling: Follow guidelines for the storage and disposal of chemicals.
Emergency Procedures: Know the steps for chemical spills and exposure.

Matter includes any substance with mass and volume, existing as solids, liquids, or gases.
Elements are the simplest form of matter, represented on the periodic table and cannot be decomposed chemically.
Compounds are formed from two or more elements chemically combined, and can be broken down into their constituent elements.

Atoms are the fundamental units of matter, comprised of protons, neutrons, and electrons.
Protons possess a positive charge and are located in the atom's nucleus.
Neutrons are neutral particles also found in the nucleus.
Electrons carry a negative charge and orbit the nucleus at various energy levels.
The atomic number signifies the number of protons in an atom, distinguishing different elements.
The mass number is the sum of an atom's protons and neutrons, reflecting its overall mass.

Ionic bonds arise from the transfer of electrons between atoms, creating positively and negatively charged ions.
Covalent bonds involve the sharing of electrons between atoms, forming molecular compounds.
Metallic bonds are characterized by an aggregation of metal atoms and a 'sea' of delocalized electrons, responsible for metallic properties.

Reactants are the starting substances in a chemical reaction that undergo transformation.
Products are the new substances formed as a result of a chemical reaction.
Key types of chemical reactions include:
- Synthesis: Two or more reactants combine to form one product.
- Decomposition: A single compound breaks down into simpler products.
- Single Replacement: An element displaces another in a compound.
- Double Replacement: The ions of two compounds exchange places.

The mole is a fundamental unit representing 6.022 x 10²³ particles, known as Avogadro's number.
Balancing chemical equations ensures conservation of mass, maintaining equal numbers of atoms for each element on both sides of the equation.

Acids yield hydrogen ions (H⁺) in solution, typically associated with a pH below 7.
Bases release hydroxide ions (OH⁻) in solution and usually have a pH above 7.
The pH scale ranges from 0 (most acidic) to 14 (most basic), indicating the acidity or alkalinity of solutions.

Exothermic reactions release energy, often manifested as heat, causing a temperature increase in the surroundings.
Endothermic reactions absorb energy from the environment, leading to a temperature decrease.

Hydrocarbons consist of hydrogen and carbon; they include alkanes (single bonds), alkenes (double bonds), and alkynes (triple bonds).
Functional groups are specific clusters of atoms in organic molecules that define their chemical properties and reactions.

Salts are ionic compounds formed from the neutralization reaction between acids and bases.
Coordination compounds involve a central metal atom surrounded by molecules or ions known as ligands, forming complex structures.

Essential safety equipment includes goggles, gloves, and lab coats to protect against chemical exposure.
Proper handling of chemicals entails strict adherence to storage and disposal protocols.
Familiarity with emergency procedures is crucial for managing chemical spills and exposure incidents.