Chemistry: Gas Laws and Atomic Reactions

Unit 1: Gas Laws

• 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

Unit 2: Atoms

• 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

Unit 3: Electrons and Bonding

• 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

Unit 4: Bonds

• 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⁻)

Unit 5: Molecules

• 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

Unit 6: Reactions

• 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

Unit 7: Energy in Reactions

• 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

Unit 8: Solutions

• 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)