Branches and Concepts of Chemistry

Organic Chemistry: Study of carbon-containing compounds, their properties, structures, and reactions.
Inorganic Chemistry: Focuses on inorganic compounds, often metals and their minerals.
Physical Chemistry: Examines the physical properties and behaviors of chemical systems using principles of physics.
Analytical Chemistry: Involves the qualitative and quantitative analysis of substances.
Biochemistry: Study of chemical processes within and related to living organisms.

Atoms and Molecules:
- Atoms: Basic units of matter, consisting of protons, neutrons, and electrons.
- Molecules: Groups of two or more atoms bonded together.
Elements and Compounds:
- Elements: Pure substances that cannot be broken down (e.g., hydrogen, oxygen).
- Compounds: Substances formed from two or more elements chemically bonded (e.g., water, NaCl).
Chemical Reactions:
- Reactants: Substances consumed in a reaction.
- Products: Substances formed as a result of a chemical reaction.
- Types of reactions: Synthesis, decomposition, single replacement, double replacement, combustion.

Organized by increasing atomic number and groups elements with similar properties.
Groups: Vertical columns, indicating similar chemical behaviors.
Periods: Horizontal rows that show trends in properties and atomic structure.

Atomic Theory: Matter is made up of atoms, which are indivisible and form compounds in whole-number ratios.
Law of Conservation of Mass: Mass is neither created nor destroyed in a chemical reaction.
Chemical Bonds:
- Ionic Bonds: Transfer of electrons from one atom to another, creating charged ions.
- Covalent Bonds: Sharing of electrons between atoms.
- Metallic Bonds: Attraction between metal ions and delocalized electrons.

Solids: Definite shape and volume; particles are tightly packed.
Liquids: Definite volume but no definite shape; particles are close but can move freely.
Gases: No definite shape or volume; particles are far apart and move independently.

Titration: Method to determine concentration of a solution by reacting it with a standard solution.
Filtration: Separating solids from liquids or gases using a barrier that allows only the fluid to pass.
Chromatography: Technique for separating mixtures based on the distribution of components between phases.

Ideal Gas Law: PV = nRT; relates pressure (P), volume (V), temperature (T), and number of moles (n) of a gas.
Le Chatelier's Principle: If a system at equilibrium is disturbed, it will adjust to counteract the disturbance.
Avogadro’s Law: Equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules.

Measures acidity or basicity of a solution:
- Acidic: pH < 7
- Neutral: pH = 7
- Basic/Alkaline: pH > 7

Always wear appropriate personal protective equipment (PPE) such as gloves, goggles, and lab coats.
Familiarize with emergency procedures and the location of safety equipment (e.g., eyewash stations, fire extinguishers).

Organic Chemistry focuses on carbon-containing compounds, including their properties, structures, and reactions
Inorganic Chemistry concentrates on compounds without carbon, often metals and their associated minerals
Physical Chemistry uses physics principles to investigate the physical characteristics and behaviors of chemical systems
Analytical Chemistry determines the qualitative and quantitative composition of substances
Biochemistry studies chemical processes in living organisms

Atoms are the basic building blocks of matter, made of protons, neutrons, and electrons
Molecules are groups of two or more atoms bonded together
Elements are pure substances that can't be further broken down, like hydrogen and oxygen
Compounds are formed when two or more elements combine chemically, examples include water and sodium chloride (NaCl)
Chemical Reactions involve reactants being consumed and products being formed
- Synthesis combines substances to form a new compound
- Decomposition breaks down a compound into simpler substances
- Single replacement involves one element replacing another in a compound
- Double Replacement involves the exchange of ions between two reactants
- Combustion involves a substance reacting with oxygen, releasing heat and light

Organized according to increasing atomic number, with elements having similar properties grouped together
Groups (vertical columns) indicate similar chemical behavior within elements
Periods (horizontal rows) showcase trends in properties and atomic structure

Atomic Theory states that matter is composed of indivisible atoms that combine in whole-number ratios to form compounds
Law of Conservation of Mass states that mass remains constant during a chemical reaction
Chemical Bonds are the forces that hold atoms together
- Ionic Bonds involve the transfer of electrons, creating charged ions
- Covalent Bonds involve the sharing of electrons between atoms
- Metallic Bonds occur between metal ions and delocalized electrons

Solids have a fixed shape and volume, with particles tightly packed together
Liquids have a definite volume but not a fixed shape, particles are in close proximity but can move freely
Gases have no fixed shape or volume, particles are far apart and move independently

Titration quantifies a solution's concentration by reacting it with a known solution
Filtration separates solids from liquids or gases using a barrier that allows only the fluid to pass
Chromatography separates mixtures based on the distribution of components between phases

Ideal Gas Law (PV = nRT) describes the relationship between pressure, volume, temperature, and the number of moles of a gas
Le Chatelier's Principle states that a system at equilibrium will shift to counteract any disturbance
Avogadro’s Law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules

Measures the acidity or alkalinity of a solution:
- Acidic: pH < 7
- Neutral: pH = 7
- Basic/Alkaline: pH > 7

Always wear appropriate personal protective equipment (PPE) like gloves, goggles, and lab coats
Be familiar with emergency procedures and safety equipment locations (eyewash stations, fire extinguishers)