Road to a 5 : AP Chemistry : Accelerated Program
SAT Score Range
•
7 sessions
•
AA
BZ
CR
+2
About
Think of this as your express train to AP Chemistry mastery! We're diving deep into the foundational concepts of Atomic Structure (Unit 1), Molecular and Ionic Compounds (Unit 2), and Intermolecular Forces & Properties (Unit 3) and uptil Electrochemistry (Unit 9). Because we're moving quickly, staying on track is key. We'll build concepts layer by layer, so each session is crucial. Dedicate time to practice problems after each session—that's how we ensure you "stick the landing" on every topic!
✋ ATTENDANCE POLICY
Attendance is optional , but absence will be detrimental to the understanding of this course.
SESSION 1
21
Jul
SESSION 1
AP Chemistry
AP Chemistry
Mon 11:00 AM - 2:00 PM UTCJul 21, 11:00 AM - 2:00 PM UTC
Unit 1: Atomic Structure and Properties (Accelerated Dive)
We'll jump right into the essentials:
1.1 Moles and Molar Mass (though we'll cover its core elements first for foundational understanding before full mole calculations).
Essential measurement techniques, precision, accuracy, and Significant Figures.
1.2 Mass Spectrometry of Elements (conceptual introduction).
1.3 Atomic Structure and Electron Configuration: Bohr model (limitations), Quantum mechanical model; Electron shells, subshells, orbitals; Aufbau principle, Hund's rule, Pauli exclusion principle.
1.4 Photoelectron Spectroscopy (PES): Interpreting spectra for electron energy levels and confirming configurations.
1.5 Periodic Trends: Atomic radius, ionization energy, electron affinity, electronegativity; Introduction to Coulomb's Law.
1.6 Valence Electrons and Ionic Compounds: Basic distinction, formation of simple ions, common polyatomic ions, basic nomenclature.
1.7 Molecular and Covalent Compounds: Basic distinction, introduction to shared electrons.
(Note: Topics 1.1 and 1.2 from the original plan were re-sequenced and integrated for flow in this condensed format)
Your Mission After This Session: This unit is the bedrock! Dedicate serious time to practice problems immediately to solidify your understanding. No falling behind on day one!
SESSION 2
22
Jul
SESSION 2
AP Chemistry
AP Chemistry
Tue 11:00 AM - 2:00 PM UTCJul 22, 11:00 AM - 2:00 PM UTC
Unit 2: Molecular and Ionic Compound Structure and Properties (Building Bonds!)
We'll start with 2.1 Types of Chemical Bonds (Ionic, Covalent, and Metallic bonds – formation, characteristics, electron behavior).
Explore 2.2 Intramolecular Forces and Potential Energy (relationship between bond formation, energy changes, and ideal bond length).
Dive into 2.3 Structure of Ionic Solids (crystal lattices, lattice energy factors, properties) and 2.4 Structure of Metals and Alloys (electron sea model, properties, types of alloys).
A crucial skill: mastering 2.5 Lewis Diagrams for molecules and polyatomic ions, including the octet rule and its exceptions, assigning valence electrons, and drawing multiple bonds.
We'll then tackle 2.6 Resonance and Formal Charge (when a single Lewis structure is insufficient, criteria for valid resonance structures, delocalization, formal charge calculation and its use in determining plausible structures).
Finally, we'll use 2.7 VSEPR and Bond Hybridization to predict molecular shapes and bond angles (electron domain vs. molecular geometry, common geometries), discuss the impact of lone pairs, determine molecular polarity, and introduce hybridization (sp, sp$^2$, sp$^3$, sp$^3d, sp^3d^2$).
Your Mission After This Session: Practice, practice, practice! Lewis structures, VSEPR, and formal charge are hands-on skills. The more you draw, the better you'll "see" these molecules.
SESSION 3
23
Jul
SESSION 3
AP Chemistry
AP Chemistry
Wed 11:00 AM - 2:00 PM UTCJul 23, 11:00 AM - 2:00 PM UTC
Unit 3: Intermolecular Forces and Properties (Part 1 - The World Between Molecules)
We'll shift our focus to 3.1 Intermolecular Forces (IMFs): Distinction between intra- and intermolecular forces. Types: London Dispersion Forces (LDFs), Dipole-Dipole Forces, Hydrogen Bonding.
Understand 3.2 Properties of Liquids and Solids and how they correlate with IMF strength: Vapor pressure, boiling point, melting point, surface tension, viscosity, capillary action, and solubility ("Like dissolves like").
Then, we'll transition to 3.3 Solids, Liquids, and Gases: Kinetic Molecular Theory (KMT) for ideal gases. Properties of Gases (Volume, Pressure, Temperature, Moles).
We'll cover the Ideal Gas Law (PV = nRT) and its foundational derivations (Combined Gas Law, Boyle's Law, Charles's Law, Avogadro's Law).
Your Mission After This Session: Practice those gas law calculations and train your eye to identify the different types of IMFs in various compounds. Understanding these forces is key to explaining physical properties!
SESSION 4
24
Jul
SESSION 4
AP Chemistry
AP Chemistry
Thu 11:00 AM - 2:00 PM UTCJul 24, 11:00 AM - 2:00 PM UTC
Unit 3: Intermolecular Forces and Properties (Part 2 - Realities and Solutions)
We'll explore 3.4 Deviations from the Ideal Gas Law: Real Gases vs. Ideal Gases; Conditions for ideal behavior; Intermolecular attractions and molecular volume (conceptual understanding of Van der Waals equation).
Dive into 3.5 Solutions and Mixtures: Types of Solutions; Concentration Units (Molarity, Mass Percent, Mole Fraction); Dilution calculations; Factors Affecting Solubility (Temperature for gases/solids, Pressure for gases - Henry's Law).
A brief introduction to 3.6 Chromatography: Principles of separation (differential attractions to stationary and mobile phases); Brief overview of types (Paper, Thin-Layer, Column); Conceptual understanding of Retention Factor (Rf).
Introduce 3.7 Spectroscopy (Introduction to Beer-Lambert Law): Principles of Spectrophotometry; Beer-Lambert Law (A = εbc - conceptual understanding and simple calculations); Using spectroscopy to determine concentration.
(Conceptual connection/brief review): Photoelectric Effect (how light energy interacts with electrons, relevant to electron energy levels and light).
Your Mission After This Session: Work on solution stoichiometry and concentration problems. The Beer-Lambert Law is a straightforward application, but practice makes it perfect!
SESSION 5
25
Jul
SESSION 5
AP Chemistry
AP Chemistry
Fri 11:00 AM - 2:00 PM UTCJul 25, 11:00 AM - 2:00 PM UTC
Unit 4: Chemical Reactions
4.1 Introduction for Reactions: This topic generally covers:
Identifying physical vs. chemical changes. (Briefly touched on in the context of net ionic equations, but important to distinguish.)
Basic concepts of reactants and products.
Conservation of mass in chemical reactions (which underpins balancing equations).
4.2 Net Ionic Equations: (Covered)
Writing complete ionic equations.
Identifying spectator ions.
Writing net ionic equations.
4.3 Representations of Reactions: This involves:
Using particulate diagrams (molecular, ionic) to represent what happens at the atomic/molecular level during a reaction, including changes in bonding and phases. This is a common AP question format.
4.4 Physical and Chemical Changes: (As mentioned in 4.1, a distinct topic focusing on the differences and how to identify them.)
4.5 Stoichiometry: (Covered extensively)
Balancing equations.
Mole-to-mole, mass-to-mass conversions.
Limiting reactants, theoretical yield, percent yield.
4.6 Introduction to Titration: (Covered)
Concepts and calculations for acid-base titrations.
4.7 Types of Chemical Reactions: (Covered)
Precipitation (with solubility rules).
Acid-base (Arrhenius, Brønsted-Lowry, neutralization).
Redox (identifying oxidation states, oxidizing/reducing agents).
Implicitly within types of reactions, you also generally cover synthesis, decomposition, single replacement, and double replacement as broader categories.
4.8 Introduction to Acid-Base Reactions: (Covered within 4.7, but sometimes listed separately to emphasize the details of acid-base definitions and neutralization.)
4.9 Oxidation-Reduction (Redox) Reactions: (Covered within 4.7, with focus on identifying species involved.)
SESSION 6
26
Jul
SESSION 6
AP Chemistry
AP Chemistry
Sat 11:00 AM - 2:00 PM UTCJul 26, 11:00 AM - 2:00 PM UTC
AP Chemistry Unit 5: Kinetics
Fri 7:00 AM - 10:00 AM EDT
5.1 Reaction Rates:
Definition of reaction rate (change in concentration over time).
Factors affecting reaction rate:
Concentration of reactants.
Temperature.
Surface area.
Presence of a catalyst.
Calculating average and instantaneous rates from concentration vs. time data.
Relating rates of disappearance of reactants and appearance of products using stoichiometry.
5.2 Introduction to Rate Law:
Defining the rate law expression (Rate = k[A]m[B]n).
Understanding the rate constant (k) and its temperature dependence.
Determining reaction orders (m, n) from experimental data (initial rates method).
Calculating the overall reaction order.
Units of the rate constant for different overall reaction orders.
5.3 Concentration Changes Over Time (Integrated Rate Laws):
Integrated rate laws for:
Zero-order reactions ([A]t = -kt + [A]0).
First-order reactions (ln[A]t = -kt + ln[A]0).
Second-order reactions (1/[A]t = kt + 1/[A]0).
Graphical determination of reaction order (linear plots of [A] vs. t, ln[A] vs. t, 1/[A] vs. t).
Calculating the rate constant (k) from the slope of linear plots.
Definition and calculation of half-life (t1/2) for each order, with emphasis on the constant half-life for first-order reactions.
5.4 Elementary Reactions:
Understanding elementary steps (unimolecular, bimolecular, termolecular).
Relating molecularity to reaction order for elementary steps.
5.5 Collision Model:
Key principles of collision theory:
Molecules must collide.
Collisions must have sufficient energy (activation energy, Ea).
Collisions must have the correct orientation.
Understanding activation energy and the transition state (activated complex).
Interpreting reaction energy profiles (potential energy diagrams).
5.6 Reaction Energy Profile:
Drawing and labeling potential energy diagrams for exothermic and endothermic reactions.
Identifying reactants, products, activation energy, and enthalpy change (delta H).
5.7 Introduction to Reaction Mechanisms:
Defining a reaction mechanism as a sequence of elementary steps.
Identifying intermediates (formed and consumed within the mechanism).
Identifying catalysts (consumed in an early step and regenerated in a later step).
5.8 Reaction Mechanism and Rate Law:
Determining the overall rate law from a multi-step mechanism by identifying the rate-determining step (the slowest step).
Approaches for deriving rate laws when the slow step involves an intermediate.
5.9 Steady-State Approximation: (This is a more advanced topic sometimes covered, but less frequently tested in detail on the AP exam compared to the rate-determining step).
5.10 Multistep Reaction Energy Profile:
Drawing and interpreting energy profiles for multi-step reactions, showing multiple transition states and intermediates.
Relating the highest energy transition state to the rate-determining step.
5.11 Catalysis:
How catalysts increase reaction rates by providing an alternate reaction pathway with a lower activation energy.
Distinguishing between homogeneous and heterogeneous catalysis.
Understanding the role of enzymes as biological catalysts.
SESSION 7
27
Jul
SESSION 7
AP Chemistry
AP Chemistry
Sun 11:00 AM - 2:00 PM UTCJul 27, 11:00 AM - 2:00 PM UTC
AP Chemistry Unit 6: Thermochemistry
7:00 AM - 10:00 AM EDT
6.1 Endothermic and Exothermic Processes:
Definition of enthalpy (H) and enthalpy change (delta H).
Distinguishing between endothermic processes (absorb heat, delta H > 0) and exothermic processes (release heat, delta H < 0).
Understanding the transfer of energy between system and surroundings.
6.2 Energy Diagrams:
Interpreting potential energy diagrams for chemical reactions.
Identifying reactants, products, activation energy (Ea), and delta H on a diagram.
Relating the position of reactants and products to endothermic and exothermic reactions.
6.3 Heat Transfer and Thermal Equilibrium:
Understanding heat (q) as energy transferred due to temperature difference.
Concepts of specific heat capacity (c) and heat transfer calculations (q = mc delta T).
Defining thermal equilibrium (no net heat transfer).
6.4 Heat Capacity and Calorimetry:
Principles of calorimetry as a method for measuring heat changes.
Using constant-pressure calorimetry (coffee-cup calorimeter) to determine heat changes (q) and enthalpy changes (delta H) for reactions.
Understanding heat capacity of a calorimeter (Ccal) and calculations involving it.
6.5 Energy of Phase Changes:
Understanding phase changes (melting, freezing, boiling, condensation, sublimation, deposition) and associated energy changes.
Calculating heat involved in phase changes using heats of fusion (delta Hfus) and heats of vaporization (delta Hvap).
Interpreting heating curves and identifying energy changes at plateaus.
6.6 Introduction to Enthalpy of Reaction:
Calculating enthalpy of reaction (delta Hrxn) for various chemical reactions.
Understanding that delta H is a state function (path independent).
6.7 Bond Enthalpies:
Using bond energies (bond enthalpies) to estimate delta Hrxn.
Understanding that breaking bonds requires energy (endothermic) and forming bonds releases energy (exothermic).
Applying the formula: delta Hrxn = (Sum of bond energies broken) - (Sum of bond energies formed).
6.8 Enthalpy of Formation:
Definition of standard enthalpy of formation (delta Hf degrees).
Calculating delta Hrxn using standard enthalpies of formation.
Applying the formula: delta Hrxn = Sum(n * delta Hf degrees (products)) - Sum(m * delta Hf degrees (reactants)), where n and m are stoichiometric coefficients.
6.9 Hess's Law:
Using Hess's Law to calculate delta Hrxn from a series of known reactions.
Manipulating thermochemical equations (reversing, multiplying) and applying corresponding changes to delta H.