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Why an Advanced Placement Chemistry course?
- The AP Chemistry course is designed to be the equivalent of the general chemistry course usually taken during the first college year.
- The AP Chemistry course exposes the student to a universe of knowledge that is unexplored at high school.
- AP Chemistry gives the student a credit for general chemistry during the first college year.
- AP Chemistry helps the student to register for courses in other fields where general chemistry is a prerequisite.
- AP Chemistry fulfills the lab science requirement.
- Outside the U.S., universities in more than 60 countries recognize AP in their admissions processes.
Who can take up an AP chemistry course?
- Students who have successfully completed their first course in high school chemistry.
- It is recommended that students successfully complete a second-year algebra course.
What does a student get from Etutorworld?
- Etutorworld helps students to jump up to Grade 5.
- Students get an in depth understanding of fundamentals and reasonable competence in dealing with chemical problems.
- The tutors at etutorworld help the students to think clearly and express their ideas orally and in writing with clarity and logic.
- Students will develop the required intellectual skills in chemistry.
More on AP chemistry…
- Students in an AP Chemistry course should spend at least five hours a week in individual study outside of the classroom
- Calculators or equation tables are not permitted on the multiple-choice section of the AP Chemistry Exam.
- For the last 40 minutes (Part B) of the exam, students will work without calculators on the free-response section.
- This year the AP chemistry exam will be held on May 11, 2010.
For more on the AP Chemistry course please go to
Structure of Matter
Atomic theory and atomic structure
- Evidence for the atomic theory
- Atomic masses; determination by chemical and physical means
- Atomic number and mass number; isotopes
- Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
- Periodic relationships including, for example, atomic radii, ionization energies,electron affinities, oxidation states
Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications
- Binding forces
- Molecular models
- Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure
States of Matter
Liquids and solids
- Laws of ideal gases
- Equation of state for an ideal gas
- Partial pressures
- Kinetic molecular theory
- Interpretation of ideal gas laws on the basis of this theory
- Avogadro’s hypothesis and the mole concept
- Dependence of kinetic energy of molecules on temperature
- Deviations from ideal gas laws
- Liquids and solids from the kinetic-molecular viewpoint
- Phase diagrams of one-component systems
- Changes of state, including critical points and triple points
- Structure of solids; lattice energies
- Types of solutions and factors affecting solubility
- Methods of expressing concentration (use of normalities is not tested)
- Raoult’s law and colligative properties (nonvolatile solutes); osmosis
- Nonideal behavior (qualitative aspects)
- Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis;coordination complexes; amphoterism
- Precipitation reactions
- Oxidation-reduction reactions
- Oxidation number
- The role of the electron in oxidation-reduction
- Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
- Ionic and molecular species present in chemical systems: net ionic equations
- Balancing of equations, including those for redox reactions
- Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
- Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle; equilibrium constants
- Quantitative treatment
- Equilibrium constants for gaseous reactions: Kp, Kc
- Equilibrium constants for reactions in solution
- Constants for acids and bases; pK; pH
- Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds
- Common ion effect; buffers; hydrolysis
- Concept of rate of reaction
- Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws
- Effect of temperature change on rates
- Energy of activation; the role of catalysts
- The relationship between the rate-determining step and a mechanism
- State functions
- First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of vaporization and fusion; calorimetry
- Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes
- Relationship of change in free energy to equilibrium constants and electrode potential.
| Descriptive Chemistry|
- Chemical reactivity and products of chemical reactions
- Relationships in the periodic table
- Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)