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Ch.1 - Intro to General Chemistry

The Scientific Method Mixtures Scientific Notation Accuracy & Precision Standard Deviation, Mean, Median & Mode Metric Prefixes Significant Figures Energy, Heat and Temperature Physical & Chemical Changes Physical & Chemical Properties Types of Energy Dimensional Analysis Density

Ch.2 - Atoms & Elements

Periodic Table Periodic Table Charges Mole Concept Calculating Molar Mass Isotopes Subatomic Particles Atomic Theory Oil Drop Experiment

Ch.3 - Chemical Reactions

Ionic and Covalent Bonds Molecular Models Polyatomic Ions Naming Covalent Compounds Naming Ionic Compounds Naming Acids Empirical Formula Molecular Formula Combustion Analysis Mass Percent Formula Balancing Chemical Equations Functional Groups in Chemistry Stoichiometry Theoretical Yield Limiting Reagent Limiting Reactant Percent Yield

BONUS: Lab Techniques and Procedures

Distillation & Floatation Test for Ions and Gases

BONUS: Mathematical Operations and Functions

Multiplication and Division Operations

Ch.4 - Chemical Quantities & Aqueous Reactions

Molarity Normality & Equivalent Weight Solution Stoichiometry Dilution Solubility Rules Net Ionic Equations Net Ionic Equation Electrolytes Redox Reaction Balancing Redox Reactions Redox Reactions Oxidation Reduction (Redox) Reactions Calculate Oxidation Number Oxidation Number Types of Chemical Reactions Activity Series

Ch.5 - Gases

Pressure Units Manometer Partial Pressure The Ideal Gas Law Chemistry Gas Laws Ideal Gas Law Boyle's Law Ideal Gas Law Density Ideal Gas Law Molar Mass Standard Temperature and Pressure Gas Stoichiometry Collecting Gas Over Water Effusion Root Mean Square Speed Kinetic Molecular Theory Van der Waals Equation Kinetic Energy of Gases Velocity Distribution Charles Law Combined Gas Law

Ch.6 - Thermochemistry

Units of Energy Internal Energy Endothermic & Exothermic Reactions Calorimetry Thermochemical Equation Hess's Law Enthalpy of Formation Enthalpy

Ch.7 - Quantum Mechanics

Electromagnetic Spectrum Wavelength and Frequency Diffraction vs Refraction The Particle Nature of Light Photoelectric Effect De Broglie Wavelength Heisenberg Uncertainty Principle Bohr Model Bohr and Balmer Equations Wave Function Introduction to Quantum Mechanics

Ch.8 - Periodic Properties of the Elements

Electron Configuration Orbital Diagrams Paramagnetic and Diamagnetic Coulomb's Law Effective Nuclear Charge Quantum Numbers The Spin Quantum Number Orbital Shapes Periodic Trends Atomic Radius Periodic Trends: Atomic Radius Periodic Trends: Ionic Radius Periodic Trends: Ionization Energy Ionization Energy Periodic Trends: Electron Affinity Periodic Trends: Metallic Character Periodic Trend: Noble Gases

Ch.9 - Bonding & Molecular Structure

Chemical Bonds Lattice Energy Lattice Energy Application Born Haber Cycle Dipole Moment Lewis Dot Structure Octet Rule Formal Charge Resonance Structures Bond Energy

Ch.10 - Molecular Shapes & Valence Bond Theory

Molecular vs Electron Geometry Molecular Geometry VSEPR Theory Bond Angles Electronegativity Hybridization Benzene Orbital Overlap Molecular Orbital Theory Bond Order Delocalized Electrons Homonuclear Diatomic Molecules Heteronuclear Diatomic Molecules

Ch.11 - Liquids, Solids & Intermolecular Forces

Molecular Polarity Intermolecular Forces Intermolecular Forces and Physical Properties Phase Diagram Heating and Cooling Curves Unit Cell Atomic, Ionic, and Molecular Solids Clausius-Clapeyron Equation

Ch.12 - Solutions

Solutions, Molarity and Intermolecular Forces Making Solutions Henry's Law Calculate Molarity Mass Percent Molality Mole Fraction ppm Boiling Point Elevation Freezing Point Depression The Colligative Properties

Ch.13 - Chemical Kinetics

Rate of Reaction Average Rate of Reaction Instantaneous Rate of Change Arrhenius Equation Energy Diagram Catalyst Reaction Mechanism Rate Law Integrated Rate Law Identifying Reaction Order Collision Theory

Ch.14 - Chemical Equilibrium

Chemical Equilibrium Equilibrium Expressions ICE Chart Le Chatelier's Principle The Reaction Quotient

Ch.15 - Acid and Base Equilibrium

Identifying Acids and Bases Strong Acids and Strong Bases Arrhenius Acid and Base Bronsted Lowry Acid and Base Conjugate Acids and Bases Amphoteric Lewis Acid and Base pH and pOH Strong Acid-Base Calculations Weak Acids Weak Bases Ka and Kb Ionic Salts Diprotic Acid Polyprotic Acid

Ch.16 - Aqueous Equilibrium

Buffer Henderson Hasselbalch Equation Acid and Base Titration Curves Weak Acid Strong Base Titrations Weak Base Strong Acid Titrations Equivalence Point Strong Acid Strong Base Titrations Titrations of Diprotic and Polyprotic Acids Acid Base Indicators Ksp Selective Precipitation Formation Constant

Ch. 17 - Chemical Thermodynamics

Spontaneous Reaction First Law of Thermodynamics Second and Third Laws of Thermodynamics Entropy Boltzmann Equation Gibbs Free Energy

Ch.18 - Electrochemistry

Redox Reaction Balancing Redox Reaction The Nernst Equation Faraday's Constant Galvanic Cell Cell Notation Standard Hydrogen Electrode Cell Potential Nernst Equation Batteries and Electricity Electroplating Electrolysis of Water & Mixture of Ions

Ch.19 - Nuclear Chemistry

Radioactive Decay Alpha Decay Beta Decay Gamma Emission Electron Capture Positron Emission Band of Stability First Order Half Life Nuclear Fission Mass Defect Nuclear Fusion Nuclear Transmutation

Ch.20 - Organic Chemistry

Introduction to Organic Chemistry Structural Formula Stereoisomers Chirality Optical Isomers The Alkyl Group Naming Alkanes Naming Alkenes Naming Alkynes Organic Chemistry Nomenclature Alkane Reactions Alkenes and Alkynes Functional Groups Alcohol Reactions Carboxylic Acid Derivative Reactions Polymer

Ch.22 - Chemistry of the Nonmetals

Alkali Metals

Ch.23 - Transition Metals and Coordination Compounds

Transition Metals Transition Metals Electron Configuration Oxidation States of Transition Metals Coordination Complexes Naming Coordination Compounds Coordination Isomers Crystal Field Theory Colors of Complex Ions

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Q. How will you increase the solubility of oxygen in water? The partial pressure of oxygen (PO2) is 0.21 atm in air at 1 atm (Pext).

Q. The solubility of carbon dioxide in water is very low in air (1.05x10^-5 M at 25°C) because the partial pressure of carbon dioxide in air is only 0.00030 atm. What partial pressure of carbon dioxide is needed to dissolve 100.0 mg of carbon dioxide in 1.00 L of water.

Q. Select the statement that is the most accurate description of gas solubility in a liquid.

Q. The concentration of carbon dioxide gas in water is 1.0x10^-5 M at 25 degree Celsius when the partial pressure of CO2 over water is 0.228 torr. Calculate the concentration of CO2 gas in water at 25 degree Celsius when the partial pressure of CO2 over water is 1.00 atm.

Q. How many moles of carbon dioxide are dissolved in a 500. ml of an unopened coke bottle if the soda manufacturer pressurized the bottle with a partial pressure of 2.0 atm of Carbon dioxide at 25 degree Celsius? KH for CO2 is 0.0301 M/atm at 25 degree Celsius.

Q. How many grams of carbon dioxide gas is dissolved in a 1.00 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25 degree Celsius? Given: KH of CO2 in water = 0.0301 M/atm at 25 degree Celsius. A. 3.52 g B. 3.18 g C. 5.55 g D. 4.67 E. 0.0755 g

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