Chemistry Unit 1: Gas Laws and Unit 2: Atoms

Study Notes

Relationship between Pressure (P), Volume (V), Temperature (T), and Moles (n) is described by the Ideal Gas Law: PV=nRT
Boyle's Law states that P1V1=P2V2
Charles' Law and Avogadro's Law are also important gas laws
Kinetic Molecular Theory describes the behavior of gas particles, assuming particles are in constant random motion, collisions are elastic, and no intermolecular forces

Nuclear Reactions: Fission, Fusion, Alpha Decay, Beta Decay, and Gamma Decay
The Nucleus of an Atom contains protons and neutrons
Isotopes: Atoms with the same number of protons but different numbers of neutrons
Radioactive Decay: Alpha (α) decay, Beta (β) decay, Gamma (γ) decay, and Half-Life: Time it takes for half of a radioactive sample to decay

Electron Configurations: Arrangement of electrons in an atom, noted by notation (e.g., 1s² 2s² 2p⁶)
Spectra: Emission and Absorption Spectra, used to identify elements
Electron Shielding: Inner electrons shield outer electrons from the full charge of the nucleus
Electronegativity: Measure of an atom's ability to attract electrons in a bond

Types of Bonds: Ionic (Transfer of electrons), Covalent (Sharing of electrons), and Metallic (Free-flowing electrons in metals)
Ionic Compounds: Formed from positive and negative ions, with properties like high melting points and conductivity when molten or dissolved in water
Polyatomic Ions: Ions composed of two or more atoms covalently bonded (e.g., NH₄⁺, SO₄²⁻)

Periodic Table Trends: Atomic radius, Ionization Energy, Electron Affinity, Electronegativity
Lewis Structures and Structural Formulas: Representation of molecules showing how atoms are bonded
Molecule Shapes and Isomers: VSEPR theory for predicting shapes, Isomers: Compounds with the same formula but different structures
Polar/Non-polar: Polar molecules have uneven distribution of charge, Non-polar molecules have even distribution of charge
Intermolecular Forces (IMFs): Dipole-dipole, Hydrogen Bonding, London Dispersion Forces

Balancing Reactions: Ensuring the same number of each type of atom on both sides of the equation
Types of Reactions: Synthesis, Decomposition, Single Replacement, Double Replacement, Combustion
Stoichiometry: Calculations based on balanced chemical equations
Limiting Reactants: The reactant that is completely consumed first, limiting the amount of product formed

Exothermic/Endothermic Reactions: Exothermic releases heat, Endothermic absorbs heat
Energy Diagrams: Graphical representation of energy changes during a reaction
Heat of Reaction: The change in enthalpy (ΔH) during a reaction
Bond Energy: Energy required to break a bond

Mixtures and Solutions: Mixture is a combination of two or more substances, Solution is a homogeneous mixture of solute dissolved in solvent
Calculating Concentrations and Dilutions: Concentration is amount of solute per unit volume of solution (e.g., molarity M = moles/L), Dilution: C1V1=C2V2 (Concentration and volume before and after dilution)