Physics Overview: Key Concepts and Principles

Definition: The study of matter, energy, and the fundamental forces of nature.
Key Concepts:
- Mechanics: Motion of objects, forces, energy, and momentum.
  - Newton's Laws of Motion:
    1. An object at rest stays at rest; an object in motion stays in motion unless acted on by a force.
    2. Force equals mass times acceleration (F=ma).
    3. For every action, there is an equal and opposite reaction.
- Thermodynamics: Study of heat, work, and energy transfer.
  - Laws of Thermodynamics:
    1. Energy cannot be created or destroyed, only transformed.
    2. Entropy of an isolated system always increases.
- Electromagnetism: Interaction of electric charges and magnetic fields.
  - Maxwell's Equations: Governing equations for electric and magnetic fields.
- Quantum Mechanics: Study of particles at the atomic and subatomic levels.
  - Key Principles: Wave-particle duality, uncertainty principle, quantization of energy.
- Relativity: Einstein's theories about the behavior of objects in high-speed motion.
  - Special Relativity: Time and space are relative; speed of light is constant.
  - General Relativity: Gravity is a curvature of spacetime.

Definition: The study of matter, its properties, composition, structure, and changes during chemical reactions.
Key Concepts:
- Atoms and Molecules:
  - Atoms: Basic units of matter, composed of protons, neutrons, and electrons.
  - Molecules: Groups of atoms bonded together.
- Periodic Table: Organizes elements based on atomic number and properties.
  - Groups: Vertical columns with similar chemical behavior.
  - Periods: Horizontal rows indicating energy levels.
- Chemical Bonds:
  - Ionic Bonds: Transfer of electrons between atoms, resulting in charged ions.
  - Covalent Bonds: Sharing of electrons between atoms.
  - Metallic Bonds: Sea of electrons shared among metal atoms.
- Reactions:
  - Types: Synthesis, decomposition, single replacement, double replacement, combustion.
  - Balancing Equations: Law of conservation of mass requires equal number of atoms on both sides.
- States of Matter:
  - Solid: Fixed shape and volume; particles are closely packed.
  - Liquid: Fixed volume but takes the shape of the container; particles are closely packed but can move.
  - Gas: No fixed shape or volume; particles are far apart and move freely.
- Acids and Bases:
  - Acids: Proton donors, taste sour, turn litmus paper red.
  - Bases: Proton acceptors, taste bitter, turn litmus paper blue.
  - pH Scale: Measures acidity or alkalinity of a solution (0-14 scale).

Physical Chemistry: Intersection of physics and chemistry; studies how matter behaves on a molecular and atomic level.
Thermodynamics in Chemistry: Application of thermodynamics to chemical reactions and processes, including Gibbs free energy and reaction spontaneity.
Quantum Chemistry: Uses quantum mechanics to understand and predict chemical behavior.

Study of matter, energy, and fundamental forces of nature.
Mechanics involves motion, forces, energy, and momentum.
Newton's Laws of Motion outline behavior of objects:
- Objects at rest or in motion stay that way unless acted upon.
- Force is defined as mass multiplied by acceleration (F=ma).
- Actions have equal and opposite reactions.
Thermodynamics examines heat, work, and energy transfer.
Laws of Thermodynamics state:
- Energy cannot be created or destroyed, only transformed.
- Entropy in an isolated system always increases over time.
Electromagnetism focuses on electric charges and magnetic fields.
Maxwell's Equations describe the relationships governing electric and magnetic fields.
Quantum Mechanics studies the behavior of particles at atomic and subatomic levels.
Key principles in Quantum Mechanics include:
- Wave-particle duality: particles can exhibit properties of both waves and particles.
- Uncertainty principle: cannot simultaneously know exact position and momentum.
- Quantization of energy: energy exists in discrete levels.
Relativity, established by Einstein, concerns high-speed motion:
- Special Relativity posits that time and space are relative; speed of light remains constant.
- General Relativity conceptualizes gravity as the curvature of spacetime.

Study of matter, its properties, composition, structure, and chemical reactions.
Atoms are the basic units of matter, consisting of protons, neutrons, and electrons.
Molecules are formed by groups of atoms bonded together.
The Periodic Table organizes elements by atomic number and properties:
- Groups: vertical columns with similar chemical behaviors.
- Periods: horizontal rows indicating levels of energy.
Chemical Bonds include:
- Ionic Bonds: transfer of electrons results in charged ions.
- Covalent Bonds: sharing of electrons among atoms.
- Metallic Bonds: shared electrons form a 'sea' around metal atoms.
Types of Chemical Reactions:
- Synthesis, decomposition, single replacement, double replacement, and combustion.
Balancing Chemical Equations follows the law of conservation of mass, ensuring equal atom numbers on either side.
States of Matter defined as:
- Solid: fixed shape and volume with tightly packed particles.
- Liquid: fixed volume, takes container shape, particles closely packed yet mobile.
- Gas: neither fixed shape nor volume; particles are far apart and move freely.
Acids and Bases:
- Acids act as proton donors, taste sour, and turn litmus paper red.
- Bases act as proton acceptors, taste bitter, and turn litmus paper blue.
The pH Scale measures acidity or alkalinity, ranging from 0 to 14.

Physical Chemistry merges physics with chemistry, analyzing molecular and atomic behavior.
Thermodynamics in Chemistry applies thermodynamic principles to chemical reactions and processes, including Gibbs free energy and spontaneity of reactions.
Quantum Chemistry employs quantum mechanics to forecast and interpret chemical behaviors.