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ap_chemistry [2024/04/20 05:37] – external edit 127.0.0.1ap_chemistry [2024/04/30 00:07] (current) – mrdough
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 ●**Trust in your preparation and knowledge!** AP Chemistry is a difficult class, but you have worked hard the entire year. Show what you know and how hard you have worked on the exam. ●**Trust in your preparation and knowledge!** AP Chemistry is a difficult class, but you have worked hard the entire year. Show what you know and how hard you have worked on the exam.
  
-**Unit 1 - Atomic Structures and Properties** **Photoelectron Spectroscopy**+======Unit 1 - Atomic Structures and Properties Photoelectron Spectroscopy======
  
 {{AP_Chem_Study_Guide_f1860aefc7694aeeaeba53de03d04968:image2.png}} {{AP_Chem_Study_Guide_f1860aefc7694aeeaeba53de03d04968:image2.png}}
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 **Pauli Exclusion Principle** states that no two electrons in the same atom can have identical values for all four of their quantum numbers. **Pauli Exclusion Principle** states that no two electrons in the same atom can have identical values for all four of their quantum numbers.
  
-**Unit 2 - Molecular and Ionic Compound Structures and** +======Unit 2 - Molecular and Ionic Compound Structures and Properties======
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-**Properties** +
 **Coulomb’s law** - Ions have stronger attractive force if they have larger charge and smaller ionic radius(smaller distance between ions) **Coulomb’s law** - Ions have stronger attractive force if they have larger charge and smaller ionic radius(smaller distance between ions)
  
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 **Sigma and pi bonding** - each single bond is a sigma bond, any other bonds are pi bonds(triple bond has a sigma and two pi bonds) **Sigma and pi bonding** - each single bond is a sigma bond, any other bonds are pi bonds(triple bond has a sigma and two pi bonds)
  
-**Unit 3 - Intermolecular Forces and Properties**+======Unit 3 - Intermolecular Forces and Properties======
  
 **Nonpolar molecule** - bond dipoles cancel out due to symmetry **Nonpolar molecule** - bond dipoles cancel out due to symmetry
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 ●To predict possible experimental error, decide how the error affects the equation and use ratio reasoning, i.e. if water is left in a cuvette, concentration of the solution would be less, so absorbance would be less ●To predict possible experimental error, decide how the error affects the equation and use ratio reasoning, i.e. if water is left in a cuvette, concentration of the solution would be less, so absorbance would be less
  
-**Unit 4 - Chemical Reactions**+======Unit 4 - Chemical Reactions======
  
 How to write Net ionic equations: How to write Net ionic equations:
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 ○Multiply reactions so the number of electrons matches and combine half reactions **Precipitation reactions** - two ionic compounds combine to form a solid in an aqueous solution ○Multiply reactions so the number of electrons matches and combine half reactions **Precipitation reactions** - two ionic compounds combine to form a solid in an aqueous solution
- +======Unit 5 - Kinetics======
-**Unit 5 - Kinetics**+
  
 Concentration of reactants, presence of catalysts, temperature, pressure and surface area affect reaction rate by changing the rate of collisions. Concentration of reactants, presence of catalysts, temperature, pressure and surface area affect reaction rate by changing the rate of collisions.
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 Catalysts provide a reaction mechanism with lower activation energy, so it has a shorter hump and reaches the potential energy of products faster. Catalysts provide a reaction mechanism with lower activation energy, so it has a shorter hump and reaches the potential energy of products faster.
  
-**Unit 6 - Thermodynamics**+======Unit 6 - Thermodynamics======
  
 **Potential Energy** - energy associated with position **Potential Energy** - energy associated with position
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 w=-PΔV w=-PΔV
  
-**Unit 7 - Equilibrium**+======Unit 7 - Equilibrium======
  
 At **equilibrium**, concentration of reactants and products remain constant. The concentrations do not have to be in equal amounts. The forward and reverse reactions occur at equal rates, so there is no observable change in concentration. At **equilibrium**, concentration of reactants and products remain constant. The concentrations do not have to be in equal amounts. The forward and reverse reactions occur at equal rates, so there is no observable change in concentration.
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 A precipitate will form in a reaction is Q>𝐾𝑠𝑝. Calculate the concentrations of each ion and plug them into a Q expression to see if Q is larger than the given K. A precipitate will form in a reaction is Q>𝐾𝑠𝑝. Calculate the concentrations of each ion and plug them into a Q expression to see if Q is larger than the given K.
  
-**Unit 8 - Acids and Bases**+======Unit 8 - Acids and Bases======
  
 **Amphoteric** - can act as acid or base i.e. water **Amphoteric** - can act as acid or base i.e. water
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 pH can be greater than 14 or less than 0. pH can be greater than 14 or less than 0.
  
-**See these Quizlets to learn more(in no particular order):** 
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-**Unit 9 - Applications of Thermodynamics**+======Unit 9 - Applications of Thermodynamics======
  
 **Entropy** ⊗**S**: A driving force for a spontaneous process is an increase in the entropy of the universe. Entropy represents the disorder of a reaction. **Entropy** ⊗**S**: A driving force for a spontaneous process is an increase in the entropy of the universe. Entropy represents the disorder of a reaction.
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