The Students scores on the free-response questions are combined with the results of the computer-scored multiple-choice questions; the weighted raw scores are summed to give a composite score. The composite score is then converted to a grade on a 5 point scale:
AP Exam Gradings
5
Extremely Well Qualified
4
Well Qualified
3
Qualified
2
Possibly Qualified
1
No Recommendation
The Exam
The AP Chemistry Exam has two main parts,
Section I, Multiple Choice (90 minutes total) consists of 75 multiple-choice questions. Total weightage 50 %. Calculators are not permitted .Points are deducted for incorrect answers. ( Don't guess unless you can eliminate at least two choices! ) You should answer at least sixty (60) questions.
Section II - Contributes 50 percent towards the final grade.It consists of six free response questions: three multipart quantitative questions, one question on writing balanced chemical equations and answering a short question for three different sets of reactants, other two multipart questions that are essentially nonquantitative. . Section II is divided into two parts: for Part A (55 minutes. Students are allowed the use of a calculator, but for Part B (40 minutes), no calculators are permitted.
Study Packages : AP Chemistry
Package
Number of Hours
Pricing
Complete AP Chemistry
40
USD 360
AP Chemistry Review
20
USD 200
AP exam prep
5
USD 60
The study packages for AP Chemistry Exam are customized as per your needs. I emphasise on gaining the complete understanding of the subject so that you can tackle any questions that may come up during the exam. Contact Me or take a Free Demo Session to know how I can help you.
Study Material - I make extensive use of study material prepared by me for tutoring. Some of these presentations are placed at the bottom of this page. If you want any more study material, I can mail them to you free of cost.
1.Atomic masses; determination by chemical and physical means .Atomic number and mass number; isotopes
2. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
3. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
B. Chemical bonding :
1. Binding forces :a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
b. Relationships to states, structure, and properties of matter . Polarity of bonds, electronegativities ,dipole moments of molecules; relation of properties to structure
2. Molecular models :a. Lewis structures and VSEPR : Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes
b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
c. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications
Ii. States of Matter (20%)
A. Gases :
1. Laws of ideal gases , Equation of state for an ideal gas ,. Partial pressures
2. 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
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams of one-component systems, Changes of state, including critical points and triple points
3. Structure of solids; lattice energies
C. Solutions
1. Liquids and solids from the kinetic-molecular viewpoint
2. Methods of expressing concentration (use of normalities is not tested)
3. Raoult's law and colligative properties (nonvolatile solutes); osmosis , Nonideal behavior (qualitative aspects)
III. Reactions (35–40%)
A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism
2. Precipitation reactions
3. Oxidation-reduction reactions:a. Oxidation number , The role of the electron in oxidation-reduction
4. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
B. Stoichiometry
1. Balancing of equations, including those for redox reactions,Ionic and molecular species present in chemical systems: net ionic equations .
2. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constants
2. Quantitative treatment:a. Equilibrium constants for gaseous reactions: K p , K c
3. Equilibrium constants for reactions in solution :(1) Constants for acids and bases; pK; pH ,(2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds ,(3) Common ion effect; buffers; hydrolysis
D. Kinetics
1. Concept of rate of reaction ,. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws
2. Effect of temperature change on rates,Energy of activation; the role of catalysts
3. The relationship between the rate-determining step and a mechanism
E. Thermodynamics
1. First law: State functions ,change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry
2. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes
3. Relationship of change in free energy to equilibrium constants and electrode Potentials
IV. Descriptive Chemistry (10–15%)
1. Chemical reactivity and products of chemical reactions
2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements
3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)
V. Laboratory (5–10%)
• making observations of chemical reactions and substances
• recording data
• calculating and interpreting results based on the quantitative data obtained
• communicating effectively the results of experimental work
Chemical Calculations
1. Percentage composition
2. Empirical and molecular formulas from experimental data
3. Molar masses from gas density, freezing-point, and boiling-point measurements
4. Gas laws, including the ideal gas law, Dalton's law, and Graham's law
5. Stoichiometric relations using the concept of the mole; titration calculations
6. Mole fractions; molar and molal solutions
7. Faraday's laws of electrolysis
8. Equilibrium constants and their applications, including their use for simultaneous equilibria
9. Standard electrode potentials and their use; Nernst equation
10. Thermodynamic and thermochemical calculations
11. Kinetics calculations
Attention should be given to significant figures, precision of measured values, and the use of logarithmic and exponential relationships.
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My exams had gone off so well after my sessions for MCAT exams with you. I have thoroughly understood Aromatic Reactions, Alkenes and Alkynes after studying with you. Thank you so much
