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AP Chemistry (NCAA Approved)

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Open to: Grades 9 - 12

Eligibility: CTY-level or Advanced CTY-level math score required

Prerequisites: Completion of Algebra I

Course Format: Session Based. See calendar for session dates and application deadlines.

Course Length: 30 weeks (Academic Year)

Recommended School Credit: One academic year

Student Expectations: Students are strongly encouraged to work an average of 6-8 hours per week for the 30-week session with breaks for holidays.

Course Code: APCH
 

green arrow Available Start Dates: 10/12/20

Course Description

Description

The AP Chemistry course covers topics typically found in a first-year introductory college chemistry course and advances students' understanding of concepts normally covered in high school chemistry. It provides a solid preparation for the AP Chemistry exam and draws on curriculum provided by FlinnPrep.

Major course themes include:

  • Nomenclature
  • Atomic structure and the periodic table
  • Chemical reactions
  • Bonding basics
  • Structure and properties
  • Stoichiometry
  • Gases
  • Solutions
  • Acids and bases
  • Aqueous equilibria
  • Thermochemistry
  • Equilibrium
  • Kinetics
  • Electrochemistry
  • Photoelectron spectroscopy and mass spectrometry

Highly qualified instructors guide students through online lectures, readings, animations, laboratory exercises, and other resources. Student knowledge is assessed through problem set assignments, tests, and exams. Unit tests, midterm and final exams are modeled after the AP exam format including multiple choice and free response questions. This course includes a laboratory component designed to meet College Board standards and has been reviewed and approved by the College Board. Hands-on labs require a materials kit that must be purchased separately by the student. This course does not have any synchronous class meetings, but students may schedule one-on-one virtual meetings directly with the instructor to answer questions or concerns.

Videos from YouTube or other web providers may be present in this course. Video recommendations or links provided at end of videos are generated by the video host provider and are not CTY recommendations. 

Materials Needed

The following lab kit is required for this course:

Quality Science Labs: Micro Chem Kit, Advanced Placement Kit

An individual license from FlinnPrep is required to access the course curriculum.

Detailed Course Information

Course Details

Unit 1 – Nomenclature

  • Ionic Compounds
  • Cations and Anions
  • Cations with One Charge
  • Cations with Multiple Charges
  • Polyatomic Ions
  • Naming Ionic Compounds and Writing Formulas
  • More Examples of Ionic Compound Names and Formulas
  • Common Mistakes
  • Naming Covalent (Molecular) Compounds
  • Examples of Covalent Compounds with Chemical Names and Formulas
  • Naming Binary Acids and Oxyacids

Unit 2 – Atomic Structure and Periodic Trends

  • Protons, Neutrons and Electrons
  • Ions
  • Isotopes
  • Average Atomic Mass
  • Electron Configuration and Valence Electrons
  • Periodic Trends
  • Atomic Radius
  • Ionic Radius
  • Ionization Energy
  • Electron Affinity
  • Electronegativity

Unit 3 – Chemical Reactions

  • Writing Chemical Reactions
  • Balancing Chemical Equations
  • Evidence of a Chemical Reaction
  • Precipitation Reactions
  • Oxidation–Reduction (Redox) Reactions
  • Acid–Base Reactions
  • Synthesis and Decomposition Reactions

Unit 4 – Bonding Basics

  • The Chemical Bond
  • Octet Rule
  • Electronegativity
  • Ionic Bonds
  • Covalent Bonds
  • Polar and Nonpolar Covalent Bonds
  • Lewis Structures
  • Rules for Drawing Lewis Structures
  • Incomplete and Expanded Octets
  • Lewis Structures and Polyatomic Ions
  • Resonance
  • Determining Electron and Molecular Geometries
  • Metallic Bonds

Unit 5 – Structures and Properties

  • Molecular Compounds
  • Intermolecular Forces and States of Matter
  • Dispersion Forces
  • Dipole–Dipole Forces
  • Hydrogen Bonds
  • Ion–Dipole Forces
  • Polarity
  • Ionic and Atomic Solids
  • Ionic Solids
  • Nonbonding Atomic Solids
  • Metallic Solids
  • Network Covalent Solids
  • Alloys

Unit 6 – Stoichiometry

  • The Mole
  • Molar Mass
  • Conversion Calculations
  • Percent Composition
  • Empirical and Molecular Formulas
  • Stoichiometry Calculations
  • Limiting and Excess Reactants

Unit 7 – Gases

  • Pressure
  • The Simple Gas Laws
  • Charles’s Law (Volume and Temperature)
  • Boyle’s Law (Volume and Pressure)
  • Avogadro’s Law (Volume and Amount)
  • The Ideal Gas Law
  • Gaseous Mixtures and Partial Pressures (Dalton’s Law)
  • Gas Stoichiometry
  • Kinetic Molecular Theory

Unit 8 – Solutions

  • Solutions
  • Aqueous Solutions
  • Solubility
  • Solution Concentration
  • Solution PreparationDilutions
  • Solution Stoichiometry

Unit 9 – Acids and Bases

  • Arrhenius Acids and Bases
  • BrØnsted-Lowry Acids and Bases
  • Strong and Weak Acids
  • The Acid Dissociation Constant, Ka
  • What Does “Small” Mean When it Comes to Ka Values?
  • The pH Scale
  • Autoionization of Water
  • Strong Acid Calculations
  • Diprotic Acids
  • Strong and Weak Bases
  • Strong Base Calculations
  • Acid–Base Reactions
  • Counting H+ and OH– Ions
  • Titrations
  • Indicators

Unit 10 – Aqueous Equilibrium

  • Weak Acids
  • Calculations Involving Weak Acids
  • Weak Bases
  • Calculations Involving Weak Bases
  • Buffers
  • Calculating the pH of a Buffer Solution
  • Buffer Capacity
  • Buffer Problems and Calculations
  • The Soulbility Product Constant, K sp
  • Q and K sp
  • The Common Ion Effect
  • Thermodynamics of Solubility

Unit 11 – Thermochemistry

  • Average Kinetic Energy
  • Maxwell-Boltzmann Distributions
  • Temperature
  • Kinetic Energy and Potential Energy
  • Heat and Work
  • State Functions or State Properties
  • Enthalpy
  • Enthalpy of Reaction
  • Hess’s Law
  • Calorimetry

Unit 12 – Equilibrium

  • What is Equilibrium?
  • Equilibrium and Concentration
  • Equilibrium and Pressure
  • Relating Kc and Kp
  • Calculating Kc with Known Equilibrium Concentrations
  • Calculating Kc with Initial Concentrations and a Known Equilibrium Concentration
  • Calculating Equilibrium Concentration from Kc and Remaining Equilibrium Concentrations
  • Calculating Equilibrium Concentration from Kc and Initial Concentrations
  • Heterogeneous Equilibrium
  • LeChâtelier’s Principle
  • Changing Concentration in the Equilibrium Reaction
  • Adding New Substances to the Equilibrium Reaction
  • Changing Temperature in an Equilibrium Reaction
  • Changing Pressure in an Equilibrium Reaction
  • Reaction Quotient

Unit 13 – Kinetics

  • Chemical Kinetics
  • Reaction Rates
  • Reaction Rates and Stoichiometry
  • Rate Laws
  • Determining Reaction Orders
  • Half-Life
  • Integrated Rate Law
  • Reaction Mechanisms
  • The Collision Model
  • Catalysis

Unit 14 – Electrochemistry

  • Oxidation–Reduction Reactions and Balancing Equations
  • Balancing Redox Equations in Acidic Solution
  • Balancing Redox Equations in Basic Solution
  • Galvanic Cells (Voltaic Cells)
  • Standard Reduction Potentials
  • Line Notation
  • Gibbs Free Energy, ∆G
  • Corrosion
  • Electrolysis

Unit 15 – Photoelectron Spectroscopy & Mass Spectrometry

  • Ionization Energy and Electronic Structures of Atoms
  • Coulomb’s Law
  • Principles of Photoelectron Spectroscopy
  • Interpreting Photoelectron Spectra
  • Number of Peaks
  • Peak Position
  • Peak Size
  • More Examples of Photoelectron Spectra
  • Mass Spectrometry
  • Electronic and Vibrational Spectroscopy
  • UV Spectroscopy
  • Infrared Spectroscopy
  • Visible Spectroscopy, Beer’s Law

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Technical Requirements

This course requires a properly maintained computer with high-speed internet access and an up-to-date web browser (such as Chrome or Firefox). The student must be able to communicate with the instructor via email. Visit the Technical Requirements and Support page for more details.

This course requires that the student use a web browser with the Adobe Flash plugin. Note that many tablets and handhelds (particularly the iPad) do not support Flash and cannot view the lessons.

The student will need the Java Runtime Environment.

Zoom online virtual classroom
This course uses an online virtual classroom which can be used for instructor-student communication if the student has any questions about the course or curriculum. The classroom works on standard computers with the Zoom desktop client and also tablets or handhelds that support the Zoom Mobile app. Students will need a computer with the Zoom desktop client installed to watch any recorded meetings. The Zoom desktop client and Zoom Mobile App are both available for free download.

This course uses Respondus LockDown Browser proctoring software for designated assessments. LockDown Browser is a client application that is installed to a local computer. Visit the Respondus website for system requirements.

While Chromebook can be used to progress through the course, all exams must be completed on a PC or Mac.