AP Chemistry |
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
www.collegeboard.com
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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
Chemical bonding
- 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
Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications
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States of Matter |
Gases
- 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
- 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
Solutions
- 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)
Reaction types
- 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
Stoichiometry
- 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
Equilibrium
- 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
Kinetics
- 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
Thermodynamics
- 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.
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| 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)
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