Preparing for AP® Chemistry can be incredibly stressful. From remembering how to balance reactions to keeping entropy and enthalpy straight, AP® Chemistry is one of the densest AP® subjects the College Board offers. Albert.io provides hundreds of AP® Chemistry practice questions to help you prepare smarter for the AP® Chem test. With curriculum-aligned questions, you can rest assured that when you practice on Albert.io, you’re prepping smart for the test.
Sometimes students and teachers want to pinpoint exactly what Essential Understanding or Essential Knowledge concept they need to devote more time towards. As such, we went ahead and tagged every single one of our AP® Chemistry questions to the official College Board curriculum.
So if you’re teaching AP® Chemistry this year, you can turn to this page if you ever need to know which questions to assign your students on Albert.io. If you’re taking AP® Chemistry, you can turn to this page for targeted practice so that you can study more efficiently. Be sure to bookmark this page for quick reference and to share it with friends. Hope you enjoy and best of luck on AP® Chemistry this year!
If you prefer a physical copy, you can download a PDF of this here.
Last updated October 8, 2015
| Big Idea Number | Enduring Understanding | Essential Knowledge | Related Albert.io Questions |
Big Idea 1 |
Enduring understanding 1.A: All matter is made of atoms. There are a limited number of types of atoms; these are the elements. | 1.A.1 | 1. Average Mass 2. Mass Ratio 3. Contamination 4. Purity 5. Composition Variations |
| Enduring understanding 1.A: All matter is made of atoms. There are a limited number of types of atoms; these are the elements. | 1.A.2 | 1. Moles and Empirical Formula 2. Mass Percent Data 3. Mass Data 4. Oxocarbon 5. Combustion Data 6. Hydrate Data 7. Same Mass Percent 8. Mass Percent 9. Empirical and Molecular 10. Molecular Formula of Fructose 11. Acceptable Molecular Mass 12. Simplest Formula 13. Percent by Mass 14. Particulate and Mass Percent 15. Particulate Empirical Formula 16. Valence Electrons and Bonding |
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| Enduring understanding 1.A: All matter is made of atoms. There are a limited number of types of atoms; these are the elements. | 1.A.3 | 1. Mass Percent 2. Atoms in an Element 3. Same Number of Atoms 4. Same Number of Moles 5. Grams of Nitrogen 6. Moles of Oxygen 7. Molecular Formula of Fructose 8. Hydrogen Atoms 9. Comparing Compounds 10. Molar Mass |
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| Enduring understanding 1.B: The atoms of each element have
unique structures arising from interactions between electrons and nuclei. |
1.B.1 | 1. Wavelength 2. Cation 3. Photon Energy 4. Comparing Light 5. Successive Ionization Energy 6. Increasing Ionization 7. Rank Elements 8. Second Ionization Energy 9. Successive Ionization Data 10. Rank Ions 11. Explain Data 12. Orbitals 13. Electron Configuration 14. Identify Element 15. Energy analysis 16. Oxide 17. Successive Ionization Energy 18. Rank Ions 19. Electron Configuration |
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| Enduring understanding 1.B: The atoms of each element have
unique structures arising from interactions between electrons and nuclei. |
1.B.2 | 1. Ground State of an Ion 2. Excited State 3. Effective Nuclear Charge 4. Orbital Diagrams 5. Ion Configuration 6. Successive Ionization Energy 7. Similar Properties 8. Most Reactive Element 9. Different Radii 10. Formula of the Compound 11. Explain Data 12 Exception to Trend |
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| Enduring understanding 1.C: Elements display periodicity in their properties when the elements are organized according to increasing atomic number. This periodicity can be explained by the regular variations that occur in the electronic structures of atoms. Periodicity is a useful principle for understanding properties and predicting trends in properties. Its modern-day uses range from examining the composition of materials to generating ideas for designing new materials. | 1.C.1 | 1. Atomic Radii 2. Smallest Radius 3. Electron Shielding 4. First Ionization Energy 5. Highest Electronegativity 6. Ionization Justification 7. Explain Radii Data 8. Radius and Ionization 9. Similar Atomic Radius 10. Second Ionization Energy 11. Ionization Energy Data 12. Ionization Equations 13. Largest Radius 14. Reactivity 15. Ion Versus Atom 16. Irregular Configuration 17. Same Group 18. Salt 19. Newly Discovered Element 20. Reducing Ability 21. Ionic Radii |
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| Enduring understanding 1.C: Elements display periodicity in their properties when the elements are organized according to increasing atomic number. This periodicity can be explained by the regular variations that occur in the electronic structures of atoms. Periodicity is a useful principle for understanding properties and predicting trends in properties. Its modern-day uses range from examining the composition of materials to generating ideas for designing new materials. | 1.C.2 | 1. Diamagnetic 2. Ionic Radii 3. Semiconductor |
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| Enduring Understanding 1.D: Atoms are so small that they are difficult to study directly; atomic models are constructed to explain experimental data on collections of atoms. | 1.D.1 | 1. Discarding Models 2. Quantum Mechanical Model 3. Atomic Theory |
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| Enduring Understanding 1.D: Atoms are so small that they are difficult to study directly; atomic models are constructed to explain experimental data on collections of atoms. | 1.D.2 | 1. Quantum Mechanical Model 2. Sulfur Isotope 3. Most Abundant Isotope 4. Relative Abundance 5. Identify Element 6. Average Atomic Mass 7. Identify Unknown 8. Largest Peak 9. Evidence of Substance 10. Mass Difference |
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| Enduring Understanding 1.D: Atoms are so small that they are difficult to study directly; atomic models are constructed to explain experimental data on collections of atoms. | 1.D.3 | 1. Bohr Model 2. Electron Transition 3. Carrot Juice 4. Analysis of Unknown 5. Factors of Beer’s Law 6. Types of Spectroscopy 7. Colorimeter Procedure 8. Spectroscopy Error 9. Unknown Concentration 10. Absorbance Data |
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| Enduring Understanding 1.E: Atoms are conserved in physical and chemical processes. | 1.E.1 | 1. Corn | |
| Enduring Understanding 1.E: Atoms are conserved in physical and chemical processes. | 1.E.2 | 1. Balancing 2. Gas Stoichiometry 3. Particilate Stoichiometry 4. Molarity Stoichiometry 5. Concentration of NaOH 6. Volume to Neutralize 7. KHP Titration 8. Titration Error 9. Gravimetric Analysis Procedure 10. Particulate Analysis of Lab 11. Mass Percent 12. Identity of Unknown 13. Gravimetric Analysis Error |
|
Big Idea 2 |
Enduring Understanding 2.A: Matter can be described by its physical properties. The physical properties of a substance generally depend on the spacing between the particles (atoms, molecules, ions) that make up the substance and the forces of attraction among them. | 2.A.1 | 1. Composition Properties 2. IMF and Boiling Point 3. Viscosity and Bonding 4. Complex Ligand Formation |
| Enduring Understanding 2.A: Matter can be described by its physical properties. The physical properties of a substance generally depend on the spacing between the particles (atoms, molecules, ions) that make up the substance and the forces of attraction among them. | 2.A.2 | 1. Ideal Gas Deviation 2. Molar Mass of a Gas 3. Ideal Gas Calculation 4. Ideal Gas Behavior 5. J-tube Calculation 6. Gas Law Calculation 7. Partial Pressure Calculation 8. Density Calculation 9. Density of a Noble Gas 10. Partial Pressure and Moles 11. Gas Stoichiometry 12. Equilibrium System |
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| Enduring Understanding 2.A: Matter can be described by its physical properties. The physical properties of a substance generally depend on the spacing between the particles (atoms, molecules, ions) that make up the substance and the forces of attraction among them. | 2.A.3 | 1. Molarity and Dissolving 2. Mass Fraction 3. Molarity Calculation 4. Unknown Concentration Method 5. Dilution of a Solution 6. Physical Separation 7. Distillation and Properties 8. Laboratory Glassware 9. Solubility Calculation 10. Solvation Thermodynamics 11. Thin Layer Chromatography 12. Percent and Density 13. Solute-solvent Interaction 14. Basic Properties 15. Solubility Thermodynamics 16. Solubility Differences 17. Thermodynamic Solubility 18. Ion Formation in Solution |
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| Enduring Understanding 2.B: Forces of attraction between particles (including the noble gases and also different parts of some large molecules) are important in determining many macroscopic properties of a substance, including how the observable physical state changes with temperature. | 2.B.1 | 1. Halogen Intermolecular Forces 2. Molecular Interparticle Forces 3. Pi Bonding |
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| Enduring Understanding 2.B: Forces of attraction between particles (including the noble gases and also different parts of some large molecules) are important in determining many macroscopic properties of a substance, including how the observable physical state changes with temperature. | 2.B.2 | 1. Hydrogen Bonding Structures 2. Molecular Forces and Polarity 3. Dipole-dipole Interactions 4. Structural Properties 5. Dissolution and Forces 6. Polarity and Solubility 7. Solubility of Amino Acids 8. Polar Solubility 9. Non-polar Solubility |
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| Enduring Understanding 2.B: Forces of attraction between particles (including the noble gases and also different parts of some large molecules) are important in determining many macroscopic properties of a substance, including how the observable physical state changes with temperature. | 2.B.3 | 1. Forces and Physical Properties 2. Properties of Gases 3. Solubility of Gases 4. Physical Properties of Gases 5. Melting Point and Forces 6. Structure and Properties 7. Interparticle Forces and MP 8. Bonding and States of Matter 9. Molecular Forces and States 10. Solubility and Pressure 11. Ionic Solubility 12. Solubility and Melting Point 13. Dissolution and Insolubility 14. Molecules and Properties 15. Mixing of Gases 16. P-T Relationship of a Gas 17. Collecting Gas Over Water 18. IMF and Polarity |
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| Enduring Understanding 2.C: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds. | 2.C.1 | 1. Bond Polarity 2. Polar Solubility 3. Non-polar Solubility 4. Multiple Bonds in a Substance 5. Geometry and Polarity 6. Bonds and Pressure Changes |
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| Enduring Understanding 2.C: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds. | 2.C.2 | 1. Ionic Compound Identification 2. Expanded Octets 3. Ionic Formula Unit 4. Metal Oxide Formula 5. Geometry Similarities 6. Valence Electrons and Bonding 7. Valence Electrons and Alloys 8. Ionic Lattice Energy 9. Lattice Structure and BP |
|
| Enduring Understanding 2.C: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds. | 2.C.3 | 1. Metallic Bonding Theories 2. Noble and Base Metals 3. Malleability of Metallic Bonds 4. Valence Electrons and Metals 5. Valence Electrons and Alloys 6. Valence Electrons and Metals |
|
| Enduring Understanding 2.C: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds. | 2.C.4 | 1. Multiple Bonds in a Substance 2. Geometry of a Substance 3. Geometry Similarities 4. Hybrid Orbital Configuration 5. Geometry of Ions 6. Geometry and Polarity 7. RHED Value and Shape 8. Formal Charge and Structure 9. Geometry of Organic Compounds 10. Molecular Geometry 11. Bond Energy of a Substance 12. Resonance Structures 13. Lewis Structure View 14. Geometry of Ions 15. Valence Electrons of Non-metals |
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| Enduring Understanding 2.D: The type of bonding in the solid state can be deduced from the properties of the solid state. | 2.D.1 | 1. Ionic Solids and Metals 2. Ionic Solid Dissolution 3. Ionic Solid Properties 4. Ionic Solid Conduction 5. Coulombic Forces and VP 6. Coulombic Forces in Compounds 7. Coulombic Forces and MP 8. Solvation and Temperature |
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| Enduring Understanding 2.D: The type of bonding in the solid state can be deduced from the properties of the solid state. | 2.D.2 | 1. Ionic Solids and Metals 2. Solvation and Temperature 3. Solvation and Free Energy 4. Alloy Substances 5. Alloy Applications 6. Specific Heat of Metals 7. Malleability of Metallic Bonds 8. Metallic Mixture Benefits 9. Large Molecule Application |
|
| Enduring Understanding 2.D: The type of bonding in the solid state can be deduced from the properties of the solid state. | 2.D.3 | 1. Allotropes of Carbon 2. Covalent Compound Properties 3. Covalent Network Solids 4. Silicon as a Network Solid 5. 3D Covalent Network Solids |
|
| Enduring Understanding 2.D: The type of bonding in the solid state can be deduced from the properties of the solid state. | 2.D.4 | 1. Molecular Solid Compounds 2. Weak IMF in a Solid 3. Solid Melting Points 4. Spontaneity of a Reaction |
|
Big Idea 3 |
Enduring Understanding 3.A: Chemical changes are represented by a balanced chemical equation that identifies the ratios with which reactants react and products form. | 3.A.1 | 1. Chemical Equation 2. Spectator Ion 3. Most Product 4. Aqueous Solutions 5. Maximum Mass 6. Identify Spectator Ions 7. Ions and Solids 8. Acid-base Reaction 9. Net Ionic Equation 10. Moles of Ions 11. Equation Type |
| Enduring Understanding 3.A: Chemical changes are represented by a balanced chemical equation that identifies the ratios with which reactants react and products form. | 3.A.2 | 1. Neutralization 2. Gas Stoichiometry 3. Mole Stoichiometry 4. Volume of Hydrogen Gas 5. Laboratory Observations 6. Excess Reactant 7. Ion Concentration 8. Unknown Element 9. Equilibrium System 10. Mass Produced 11. Percent Yield of a Gas 12. Ostwald Process 13. Percentage by Weight 14. Mass of Ore Sample |
|
| Enduring Understanding 3.B: Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change from one into the other. Classes of chemical reactions include synthesis, decomposition, acid-base, and oxidation-reduction reactions. | 3.B.1 | 1. Change in Mass 2. Silver Oxide Procedure 3. Hydrate Lab Procedure 4. Empirical Formula Data 5. Unknown Copper Oxide 6. Unknown Oxide of Titanium 7. Alum Lab Data 8. Hydrate Errors 9. Non-redox |
|
| Enduring Understanding 3.B: Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change from one into the other. Classes of chemical reactions include synthesis, decomposition, acid-base, and oxidation-reduction reactions. | 3.B.2 | 1. Conjugate Base 2. Amphoteric 3. Amphoteric Hydroxides 4. Conjugate Acid 5. Strongest Conjugate Base 6. Strongest Acid 7. Strongest Base 8. Percentage by Weight |
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| Enduring Understanding 3.B: Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change from one into the other. Classes of chemical reactions include synthesis, decomposition, acid-base, and oxidation-reduction reactions. | 3.B.3 | 1. Non-redox 2. Highest Oxidation Number 3. Oxidation Half Reaction 4. Oxidation and Reduction 5. Balancing Redox in Basic 6. Balancing Redox in Acidic 7. Final Concentration 8. Electron Transfer 9. Hydrogen Peroxide |
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| Enduring Understanding 3.C: Chemical and physical transformations may be observed in several ways and typically involve a change in energy. | 3.C.1 | 1. Classify Chemical Equation 2. Classify Copper Reaction 3. Ambiguous Change 4. Particulate Diagram 5. Classify the Diagram |
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| Enduring Understanding 3.C: Chemical and physical transformations may be observed in several ways and typically involve a change in energy. | 3.C.2 | 1. Laboratory Observation 2. Effect of Enthalpy 3. Overall Reaction 4. Energy Calculation 5. Endothermic |
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| Enduring Understanding 3.C: Chemical and physical transformations may be observed in several ways and typically involve a change in energy. | 3.C.3 | 1. Cathode 2. Ecell 3. Oxidation or Reduction 4. Electroplating 5. Salt Bridge 6. Gibbs Free Energy 7. Ease of Oxidation 8. Electrochemical Cell 9. Diagram 10. Adding NaOH 11. Anode 12. Unknown Chloride 13. Increasing Voltage 14. Unknown Metal |
|
Big Idea 4 |
Enduring Understanding 4.A: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time. | 4.A.1 | 1. Acid-base Reaction Rate 2. Reaction Rate and Orientation 3. Titration Rate Indicator 4. Change in Reactants 5. Beer’s Law Application 6. Catalyst Definition 7. Chlorofluorocarbons 8. Rates of the Opposing Reaction |
| Enduring Understanding 4.A: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time. | 4.A.2 | 1. Half-life Reaction Rate 2. Thermodynamic and Rates 3. Change in Reactants and Rates 4. Change in Reactant Calculation 5. Boltzmann’s Equation 6. Reaction Order Calculation 7. Reaction Order Determination 8. Multi-step Reaction Basics 9. Reaction Order Changes 10. Rate Law Application 11. Rate Law Determination 12. Rate Law Calculation 13. Increase of a Reaction Rate 14. Radioactive Rate Law 15. Rate Law Based on Data 16. Rate Law and Rate Order 17. Catalysts and Rate Laws 18. Rate Law Order Calculation |
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| Enduring Understanding 4.A: Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time. | 4.A.3 | 1. Half-life Reaction Rate 2. Rate Constant and Ea 3. Unit for a Rate Constant |
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| Enduring Understanding 4.B: Elementary reactions are mediated by collisions between molecules. Only collisions having sufficient energy and proper relative orientation of reactants lead to products. | 4.B.1 | 1. Reaction Order and Rate Laws 2. Reaction Order and Half-life 3. Collisions and Rate Laws 4. Effect of Collisions on Rates 5. Frequency and Collisions 6. Elementary Reactions 7. Elementary Reaction Graph 8. Elementary Reaction Order |
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| Enduring Understanding 4.B: Elementary reactions are mediated by collisions between molecules. Only collisions having sufficient energy and proper relative orientation of reactants lead to products. | 4.B.2 | 1. Temperature Dependence of Ea 2. Activation Energy of Reactions 3. Ea of a Reversible Reaction 4. Activation Energy Definition 5. Collisions and Orientation 6. Collisions and Rate Laws 7. Boltzmann Graph Interpretation 8. Maxwell Boltzmann Graph 9. Maxwell Boltzmann & Collisions 10. Rates of Non-elementary Rxns 11. Rates and Product Formation 12. Rates and Chemical Kinetics |
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| Enduring Understanding 4.B: Elementary reactions are mediated by collisions between molecules. Only collisions having sufficient energy and proper relative orientation of reactants lead to products. | 4.B.3 | 1. Energy Diagram Interpretation 2. Energy Graph Designation 3. Energy Diagram and Reactions 4. Arrhenius Equation 5. Energy Graph and Temperature 6. Energy Profile Analysis 7. Energy Profile Graphs |
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| Enduring understanding 4.C: Many reactions proceed via a series of elementary reactions. | 4.C.1 | 1. Reaction Mechanism Properties 2. Components of a Multi-step Rxn 3. Interpretation of a Reaction 4. Overall Reaction and Mechanism 5. Gas Phase Rate Law 6. Overall Reaction Information 7. Elementary Reaction Steps 8. Rate Law Mechanisms 9. Rate Laws and Catalysts 10. Thermolecular Rate Law 11. Reaction Order and Rate Laws |
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| Enduring understanding 4.C: Many reactions proceed via a series of elementary reactions. | 4.C.2 | 1. Multi-step Reaction Rate Law 2. Rate Determining Step 3. Mechanisms and Rates 4. Rate Law and Mechanism 5. Gas Phase Rate Law 6. Individual Mechanism Steps 7. Overall Reaction Thermodynamic |
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| Enduring understanding 4.C: Many reactions proceed via a series of elementary reactions. | 4.C.3 | 1. Components of a Mechanism 2. Intermediate of a Reaction 3. Intermediate Properties 4. Intermediate Identification 5. Overall Reaction and Mechanism 6. Gas Phase Rate Law 7. Multi-step and Related Rate 8. Overall Reaction Intermediate 9. Temperature and Mechanisms |
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| Enduring Understanding 4.D: Reaction rates may be increased by the presence of a catalyst. | 4.D.1 | 1. Reaction Rate Reduction 2. Pollution & Reaction Rate 3. Reaction Rate & Catalysts 4. Reaction Rate Thermodynamics 5. Catalyzed vs Uncatalyzed Graph 6. Catalyst 7. Catalyst Application 8. Reaction Energy Profile 9. Basic Rate Law Information 10. Energy Diagram Interpretation 11. Catalyst and Energy Profile |
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| Enduring Understanding 4.D: Reaction rates may be increased by the presence of a catalyst. | 4.D.2 | 1. Acid-base Catalyst 2. Surface Catalyst 3. Biological Catalyst 4. Metal Heterogeneous Catalyst 5. Commercial Surface Catalyst 6. Ionic Compound as a Catalyst 7. Catalyst Identification 8. Lock and Key Enzyme 9. Biological Systems & Enzymes 10. Heterogeneous Catalyst 11. Multi-step Homogeneous Catalyst 12. Acid-base Catalyst Application |
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Big Idea 5 |
Enduring Understanding 5.A: Two systems with different temperatures that are in thermal contact will exchange energy. The quantity of thermal energy transferred from one system to another is called heat. | 5.A.1 | 1. Kinetic Energy Changes 2. Temperature Changes Graphic 3. Effect on Temperature 4. Absolute Zero 5. Average Kinetic Energy 6. Heat of a Substance 7. Boltzmann Graph |
| Enduring Understanding 5.A: Two systems with different temperatures that are in thermal contact will exchange energy. The quantity of thermal energy transferred from one system to another is called heat. | 5.A.2 | 1. Kinetic Energy 2. Particle Velocity 3. Change in Energy 4. Energy Transfer 5. KE of Gases 6. Kinetic Energy Comparison 7. Energy Transfer Values 8. Heat Definition 9. Thermal Equilibrium 10. Thermal Equilibrium Graph 11. Energy Change of a System 12. Specific Heat Comparison 13. Heat Transfer 14. Heat of Formation 15. Potential Energy Source 16. Lattice Energy 17. Bond Order 18. Bond Length 19. Potential Energy 20. Bond Breaking Energy 21. Internal Energy |
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| Enduring Understanding 5.B: Energy is neither created nor destroyed, but only transformed from one form to another. | 5.B.1 | 1. Law of Conservation of Energy 2. Energy at a Particulate Level 3. Energy Transfer for a System 4. Pure Thermal Transfer Energy 5. Work and Heat Energy View 6. Energy Applied to a Battery 7. Work & Internal Energy Change 8. Work and Change in Energy |
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| Enduring Understanding 5.B: Energy is neither created nor destroyed, but only transformed from one form to another. | 5.B.2 | 1. Energy Transfer for a System 2. Energy Released from a System 3. Systems & Transfer of Energy |
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| Enduring Understanding 5.B: Energy is neither created nor destroyed, but only transformed from one form to another. | 5.B.3 | 1. Enthalpy Change of a Reaction 2. Energy Change for a System 3. Heat of Formation 4. Chemical Systems & Energy 5. Energy Transfer and Phases 6. System Energy Description 7. Thermal Processes and Energy 8. Temperature Change 9. Condensation of Water 10. Heat Diagram of Water 11. Enthalpy Changes for a System |
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| Enduring Understanding 5.B: Energy is neither created nor destroyed, but only transformed from one form to another. | 5.B.4 | 1. Enthalpy and Electrolysis 2. Calorimetry Measurements 3. Calorimetry Calculation 4. Calorimetry & Heat Capacity 5. Calorimetry and Molar Enthalpy 6. Calorimetry Application 7. Final Temperature Calculation 8. Lab Errors 9. Density and Calorimetry 10. Specific Heat Definition 11. Heat Capacity Ordering |
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| Enduring Understanding 5.C: Breaking bonds requires energy, and making bonds releases energy. | 5.C.1 | 1. Applied Bond Breaking Energy 2. Geometric Energy Forces 3. Geometric Energy of Foods 4. Geometric Bond Dissociation 5. Geometric Energy of Fuels 6. Geometric Bond Enthalpy 7. Geometric Energy & BP 8. Potential Energy Determination |
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| Enduring Understanding 5.C: Breaking bonds requires energy, and making bonds releases energy. | 5.C.2 | 1. Net Energy Change Calculation 2. New Energy Change Diagram 3. Net Energy Change Description 4. Metabolism and Net Energy 5. Net Energy Change ID 6. Net Energy Change of a Rxn 7. Net Energy Change Graph 8. Efficient Net Energy Change 9. Enthalpy of Atomization 10. Overall Enthalpy of Formation 11. Commercial Use of Enthalpy 12. Standard Enthalpy of Formation 13. Metals & Enthalpy of Reaction 14. Ionic Enthalpy of Formation 15. Non-zero Standard Enthalpy 16. Potential Energy Determination |
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| Enduring Understanding 5.D: Electrostatic forces exist between molecules as well as between atoms or ions, and breaking the resultant intermolecular interactions requires energy. | 5.D.1 | 1. Intermolecular Force Strength 2. Weak Intermolecular Force 3. IMF and Calorimetry |
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| Enduring Understanding 5.D: Electrostatic forces exist between molecules as well as between atoms or ions, and breaking the resultant intermolecular interactions requires energy. | 5.D.2 | 1. Physical State of a Molecule 2. Energy Transfer 3. Strong Intermolecular Energy 4. Inter vs Intra Changes 5. IMF and Properties 6. Forces and Dissolution 7. Inter vs Intra Polarizability 8. Inter vs Intra Identification |
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| Enduring Understanding 5.D: Electrostatic forces exist between molecules as well as between atoms or ions, and breaking the resultant intermolecular interactions requires energy. | 5.D.3 | 1. Intermolecular Energy 2. Large Biological Molecules 3. Biological Molecule Properties 4. Dissolving Biological Molecule 5. Biological Molecule pH 6. Biological Hydrogen Bonding 7. Ligand Properties |
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| Enduring Understanding 5.E: Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy, or both. | 5.E.1 | 1. 2nd Law and Entropy 2. Entropy Changes in a System 3. Entropy and Phase Diagrams 4. Entropy of Gases 5. Entropy 6. Entropy Change Calculation 7. Endothermic Dissolution 8. Change in Entropy Calculation |
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| Enduring Understanding 5.E: Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy, or both. | 5.E.2 | 1. Spontaneous Definition 2. Enthalpy for Forming a Base 3. Thermodynamic Favorability 4. Endothermic & Low Entropy 5. Cellular Respiration 6. Change in Enthalpy Calculation 7. Free Energy Change Calculation 8. Overall Energy Calculation |
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| Enduring Understanding 5.E: Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy, or both. | 5.E.3 | 1. Gibbs and Work Energy 2. Gibbs and Thermodynamics 3. Gibbs and Temperature 4. Gibbs and Spontaneity 5. Slow Reaction in Biological 6. Change in Enthalpy Calculation 7. Free Energy Value Change 8. Free Energy Change Calculation 9. Gibbs & Equilibrium Constant |
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| Enduring Understanding 5.E: Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy, or both. | 5.E.4 | 1. Endothermic Dissolution 2. Coupled Reactions 3. Coupled Reaction Intermediate 4. Coupled Reaction & Favorable 5. Le Chatelier’s Applied 6. Coupled Rxn Interpretation |
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| Enduring Understanding 5.E: Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy, or both. | 5.E.5 | 1. Thermodynamic Properties 2. Exothermic and High Entropy 3. Kinetic vs Thermodynamics 4. Thermodynamically Unfavored 5. Interpreting Thermodynamics |
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Big Idea 6 |
Enduring Understanding 6.A: Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal. | 6.A.1 | 1. Not a Reversible Reaction 2. Reversible Reaction 3. Rusting of Iron 4. Hemoglobin |
| Enduring Understanding 6.A: Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal. | 6.A.2 | 1. Reactant Quotient Expression 2. Kp 3. Kp and Kc 4. Equilibrium Trials 5. Kc from Reactions 6. Graph of Q and K 7. Changes in Ratio 8. Moles at Equilibrium |
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| Enduring Understanding 6.A: Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal. | 6.A.3 | 1. System at Equilibrium 2. Equilibrium Has Been Reached 3. Data at Equilibrium 4. Equilibrium Concentrations 5. Equilibrium Constant 6. Moles and Equilibrium 7. Gaseous Equilibrium 8. Concentration at Equilibrium 9. Graph Analysis 10. Match Lines 11. Describing K 12. Adding a Catalyst 13. Concentration-time Graph 14. Match K to Moles 15. Kc 16. Possible K |
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| Enduring Understanding 6.A: Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal. | 6.A.4 | 1. STP 2. Instant of Mixing 3. Different Concentrations 4. K from Diagram 5. Concentrations from K 6. K and Hemoglobin |
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| Enduring Understanding 6.B: Systems at equilibrium are responsive to external perturbations, with the response leading to a change in the composition of the system. | 6.B.1 | 1. Increasing Water Vapor 2. Temperature Stress 3. Increase Concentration 4. Adding Reactant 5. Graphs and Stress 6. Temperature and K 7. Decrease in Mass 8. Adding Gas 9. Catalyst 10. Maximum Conversion 11. Temperature Change 12. Density and Allotropes 13. Lunar Lander 14. Ostwald Process |
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| Enduring Understanding 6.B: Systems at equilibrium are responsive to external perturbations, with the response leading to a change in the composition of the system. | 6.B.2 | 1. Endothermic 2. Increased pH 3. Equalities 4. Qp 5. Initial Moles |
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| Enduring Understanding 6.C: Chemical equilibrium plays an important role in acid-base chemistry and in solubility. | 6.C.1 | 1. Unknown Acid 2. Predicting Ka 3. Predicting pOH 4. Predominate Ions 5. Predicting Ions Present 6. Weak Acids 7. Concentration of Hydronium 8. Strength of Conjugate Base 9. Antacids 10. pOH of Solutions 11. Ka and Ionization 12. Equivalence Point 13. pKa from Titration Graph 14. Comparing Graphs 15. Choosing an Indicator 16. Comparing Concentrations 17. Titration Technique 18. Hydroxide Ion Concentration 19. Acidity Rank 20. Temperature and Kw 21. pKa and Concentration 22. pH to Hydronium 23. Stomach Ulcers 24. Hydroxide to pH 25. Pyridine 26. Dilution and pH 27. pH and Molarity 28. pH of Salt Solutions 29. Hydronium and Molarity 30. Saturated Base 31. Dissociation and Ka 32. Changing Ionization 33. Estimating pH of a Solution 34. Dilution and Hydronium 35. Half-equivalence Point 36. Mixture pH 37. Comparing Titrations 38. Comparing Two Acidic Solutions 39. Titration of a Mixture 40. pH at the Equivalence Point 41. Titration of a Metal Hydroxide 42. Buffering Action 43. Making a Buffer 44. Concentrations in a Buffer |
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| Enduring Understanding 6.C: Chemical equilibrium plays an important role in acid-base chemistry and in solubility. | 6.C.2 | 1. Finding the pH of a Buffer 2. pH of a Mixture 3. Blood 4. Malonic Acid 5. Labile Protons and Graphs 6. Conjugate Base in Solution 7. Thymolphthalein 8. Making Buffers 9. Strong Acids and Buffers 10. Effective Buffers 11. Identifying Buffers 12. pKa and pH 13. Ksp Ranking 14. Ksp and Relative Solubility 15. Molar Solubility |
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| Enduring Understanding 6.C: Chemical equilibrium plays an important role in acid-base chemistry and in solubility. | 6.C.3 | 1. Molar Solubility with a Salt 2. Ion Concentration 3. Factors Changing Ksp 4. Mixing Salts 5. Sea Water 6. Ksp from Data 7. Ksp and Ecell 8. Least Soluble 9. Factors Affecting Solubility 10. Solubility in Acidic Solutions 11. Water Softeners 12. Ions and Solubility 13. Precipitation and Solubility 14. Increasing Solubility 15. Salts and Solubility 16. Salting Out 17. Identify Unknown Metal 18. Entropy Versus Enthalpy 19. Enthalpy of a Solution 20. Comparing Dissolution Steps |
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| Enduring Understanding 6.D: The equilibrium constant is related to temperature and the difference in Gibbs free energy between reactants and products. | 6.D.1 | 1. Value of Zero 2. Free Energy and Q 3. Standard State Conditions 4. K and Free Energy 5. Thermodynamic Data and K 6. Endergonic and Exergonic |
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Hi,
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