Get Better Grades- Study AP Chemistry with Dr Uma Sharma

The Learning Process with Dr Uma Sharma

  1. Gain clear understanding of basics of topics so that complete comprehension is achieved.

  2. Highly interactive sessions customized as per your needs

  3. All Sessions recorded for review any time later. Review the recorded sessions from your I-pad or your mobile also.

  4. Practice Quizzes based on AP Chemistry Syllabus to hone your skills after every session.

Take a look at What the parents of students have to say or Check out the Session Reviews- by students.

Grades scored by my students in AP Chemistry Exam 2024 are as follows:

Grade 5 4 3
Students (Total 30) 13 (43%) 15 (50%) 2 (7%)



Session Ratings and Reviews

Student Reviews-5061
Total Sessions-30125

Group Classes

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My Teaching Style

For best comprehension, I like to divide my session into two parts:

Learning Using Specially Created Content. I use my own training content which has been specially prepared keeping the needs of students in mind. I focus upon clearing the basics of the subject first before moving on. Detailed explanations provided in a easy to understand manner forms the key to understanding.

Solving problems based on topics covered. At the end of each session I go over the quizzes on the topic with the student which ensures correct assimilation by the student and any gaps in knowledge are clarified. I also provide Chemistry Quizzes for AP Chemistry Exam which students can attempt in their own time and discuss with me during the sessions.


About AP Chemistry Exam

Advanced Placement Chemistry is a course and examination offered by the College Board as a part of the Advanced Placement Program to give American and Canadian high school students the opportunity to demonstrate their abilities and earn college-level credit.


AP Chemistry Grades

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 Grades Definition
5 Extremely Well Qualified
4 Well Qualified
3 Qualified
2 Possibly Qualified
1 No Recommendation

AP Exam Calculator Policy

Calculators are not permitted in section I and questions based on simple calculators will be the part of section I. Programmable or graphic calculators are permitted for the entire free response exam. Calculators will not be allowed to share and calculators with type writer style (QWERTY) keyboards will not be permitted

The Exam


The AP Chemistry exam has 2 sections

Section I - 90 Minutes Three long free response questions ,two short free response questions. Programmable or graphic calculators are permitted.

Total weightage : 50%

MCQs are either discreet questions or sets of question, Questions are based on the knowledge of Chemistry and Science practices outlined in AP Chemistry course. Question sets are new types of questions in which a stimulus in the form data or series of questions will be provided. No negative marking or no marks deducted for incorrectly answered questions. Score is based on the number of questions correctly answered.


Section II - 90 minutes, 60 Multiple choice questions (MCQs) Calculators are not permitted.

Total weightage : 50%

Questions asked will be based on-

  • Experimental procedures, data, graphs observations and error analysis.
  • Explanation of phenomena based on molecular, atomic level of the matter.
  • Logical and analytical path ways to solve a problem.Commonly used equations sheet will be provided with each exam for use. However in free response exam no marks will be awarded for simply writing the correct equations. No marks will be awarded for ambiguous answers without any reasonable explanations.

    • AP Chemistry Target 2025 Group Classes

    Due to heavy demand for AP Chemistry Online Tutoring with Dr Uma Sharma, NO students for One-on-One tutoring are being accepted.
    However you can join the AP Chemistry Online Classes with Dr Uma Sharma in a small group. Students studying in group classes with Dr Uma Sharma may avail one hour per week One-on-One class (on additional payment) for clearing their doubts from school classes, assignments etc.

    Details of classes are given below

    Free Trial Session:- You can take a Free Trial Session which will help you make your decision. Please click here to Request Free Trial Session

    Highlights -

    1. Highly interactive sessions with active participation by each student.
    2. Additional advantage of peer learning and group motivation. Studies have shown that students tend to learn better in their peer groups
    3. Students learn in small motivational group.
    4. All Sessions recorded for review any time later. Review the recorded sessions from your I-pad or your mobile also.
    5. Practice Quizzes based on up-to-date Syllabus after every session to hone your skills.
    6. Affordable online tutoring with a highly qualified and experienced tutor.

    Click Here to Register for AP Chemistry Group Classes


    AP Chemistry Classes with Dr Uma Sharma

    Teaching Content. I have conducted nearly 26000 hours of live classes and have over 25 years of teaching experience. With this I have a deep understanding of requirements of students. The teaching content for the classes has been specially developed keeping these requirements of students in mind.

    Question Bank. A exhaustive question bank has been developed through rigorous research on past AP Exam papers. A vast collection of AP-style questions in multiple-choice and free-response formats are available to sharpen skills of the students and also gauge any gaps in knowledge. The progress of students is closely monitored and any gaps in understanding. are covered during class.

    Detailed Notes. Detailed notes are provided to the students which cover every topic and subtopic of AP Chemistry, These are a comprehensive resource for in-depth understanding which can be gone over any time by the students. Also all class sessions are recorded and made available to students ensuring that they never miss a valuable lesson.

    Intensive Review Classes. As part of the package, intensive review classes will be conducted for six weeks prior to the exam. These dynamic sessions expose the students to a wealth of practice opportunities, including multiple-choice questions, free-response questions, and real full-length AP Exam papers setting the stage for success in the final exam.


    Group Name No of Hours Days and Time Class Start Date Status  
    AP Chemistry Target 2025 Group 2 Sat, Sun 100 Hours Sat,Sun
    8.00 PM to 10.00 PM PST     		20-Jul-2024
    		In progress
    Open for Registration     		Register Now
    AP Chemistry Target 2025 Accelerated Classes for Students with Chemistry Background)- Group 5 Tue, Wed 65 Hours Tue,Wed
    8.00 to 9.30 PM EST (5.00 to 6.30 PM PST)     		05-Nov-2024
    		In progress
    Open for Registration     		Register Now
    AP Chemistry Target 2025 Group 3 Sat, Sun 100 Hours Sat,Sun
    8.00 PM to 10.00 PM EST (5.00 to 7.00 PM PST)     		17-Aug-2024
    		In progress
    Registration Closed     		Registration Closed
    AP Chemistry Target 2025 Accelerated Learning Classes- Group 4 Mon, Fri 80 Hours Mon,Fri
    8.00 PM to 10.00 PM EST (5.00 to 7.00 PM PST)     		04-Oct-2024
    		In progress
    Registration Closed     		Registration Closed

    AP Chemistry Exam course content outlined below


    UNIT 1 Mole concept, atomic structure, properties and periodic trends.

    1.1 Meaning and Quantitative Relation in Avogadro’s number, Moles and Molar Mass

    1.2 Average atomic masses and Mass Spectroscopy of Elements

    1.3 Percent composition, empirical and molecular formulas of pure substances.

    1.4 Percent Composition of different substances in hydrates and mixtures

    1.5 Electromagnetic Spectrum photon and Planck’s equation

    1.6 Light and matter-Photoelectric Effect and de-Broglie’s wavelength.

    1.7 Absorption and Emission spectrum in atoms and Bohr’s atomic model of an atom.

    1.8 Modern Atomic Structure and Electron Configuration

    1.9 Valence Electrons and Periodic Trends

    1.10 Periodic trends in Covalent, Ionic character of oxides and predicting their formulas.

    1.11 Photoelectron Spectroscopy, Electron Configuration and Ionization energies .

    1.12 Relation between Absorption of light and concentrations of solution -Beer-Lambert’s Law.


    UNIT 2 Chemical bonding in Molecular and Ionic Compound with their Structures and Properties


    2.1 Different types of Chemical Bonds

    2.2 Ideal gas laws based on relation between P, V ,n and T, Kinetic molecular theory,Maxwell – Boltzmann distribution curve.

    2.3 Real gases deviation from the ideal behavior based on intermolecular interactions.

    2.4 Solutions ,Homogeneous and Heterogeneous solutions, colloids, separation techniques for the components of the solutions based on their chemical and physical properties,dissolution process, molarity, dilution chemistry.

    2.5 Types of intermolecular forces. London Dispersion forces,polar and non polar molecules, Polar forces and hydrogen bonding,Dipole moment.

    2.6 Intermolecular forces and properties of the substance. Boiling point surface tension, capillary action, vapor pressure, viscosity, solubility and deviation from the ideal behavior. Biological reactions affected by the nature and the type of the intermolecular forces like interaction of enzyme with the substrate, Hydrophobic and Hydrophilic regions in proteins.

    2.7 Chemical bonding, valence electrons, inert gas configurations, covalent bonding, Ionic bonding, polar covalent bond. Ionic and covalent character in a compound, Bond energies, metallic bonding and delocalization of electrons.

    2.8 Lewis diagram, use of VSEPR model to determine molecular geometry,shape, bond angles, dipole moment, bond lengths and bond energies. Limitation of Lewis diagrams. Hybridization sp, sp2 and sp3.Use of hybridization in predicting the molecular geometry and bond angles.

    2.9 Molecular orbital theory and understanding of sigma and pi bonds.

    2.10 Types of solids, Ionic solids, covalent solids, metallic solids ,and molecular solids.

    UNIT 3 Intermolecular Forces and States of matter.-~14–15 Class Periods 18–22% AP Chemistry Exam Weighting


    3.1 Intermolecular Attractive Forces (IMF) in molecules 4 SAP.

    3.2Kinetic Molecular Theory, IMF and Changes of State in Solids, Liquids, and Gases 3 SAP.

    3.3 Types of Solids and their Properties. 4 SAP.

    3.4 Properties of Liquids and the Kinetic-Molecular Theory 4 SAP.

    3.5 Ideal Gas Law and the Kinetic-Molecular Theory 5 SAP.

    3.6 Real Gases and Deviation from Ideal Gas Behavior 6 SPQ.

    3.7 Solutions as Homogeneous Mixtures and Concentrations of the Solutions 5 SPQ .

    3.8 Representations of Solutions on Microscopic level as weak Electrolyte and strong Electrolyte 3 SPQ.

    3.9Separation Techniques for Solutions and Mixtures using Distillation and Chromatography 2SPQ.


    3.10 Solubility and Intermolecular forces of Attraction -Like Dissolves like Rule 4 SAP.


    UNIT 4 Chemical Reactions-~14–15 Class Periods 7–9% AP Chemistry Exam Weighting


    4.1 Meaning of Chemical Reaction and Balancing of Equations 2 TRA.

    4.2 Solubility rules and Balanced Net Ionic Equations 5 TRA.

    4.3 Representations of Chemical Reactions on Microscopic level 3 TRA.

    4.4 Energy Changes Curing Chysical and Chemical Changes 6 SPQ.

    4.5 Stoichiometry of Reaction, Limiting Reactants and % Rield.5 .

    4.6 Different Types of Chemical Reactions 1 TRA.

    4.7 Acid-Base Reactions and their net Ronic Rquations.3TRA.

    4.8 Meaning of Titrations and Retermination of Roncentrations of solutions using titrations..

    4.9 Meaning of Oxidation-Reduction and Ralancing of Redox Reactions.


    UNIT 5 Kinetics ~13–14 Class Periods 7–9% AP Chemistry Exam Weighting TRA


    5.1 Collision Theory, Reaction Energy Profile and Activation Energy.

    5.2 Meaning of Rates of Reactions and Rate-Influencing Factors.

    5.3 Rate Laws for Reactions, Order and rate Constant.

    5.4 Concentration Changes Over Time -Integrated Rate Laws and Half-Lives.

    5.5 Elementary steps, Intermediate, Catalyst and Reaction Mechanisms.

    5.6 Rate Law of Elementary step, Reaction Pathway and Rate Determining Step.

    5.7 Steady-State Approximation for Determining Rate Law in Multiple Step Reaction with Intermediates.

    5.8Energy Profile for Multiple Step Reaction Mechanism.

    5.9 Activation Energy and Factors Affecting Activation Energy.

    5.10Catalysis.


    UNIT 6 Thermodynamics ~10–11 Class Periods 7–9% AP Chemistry Exam Weighting


    6.1 Meaning of Endothermic and Exothermic Processes.

    6.2 Energy profile for a Reaction and Enthalpy of a Reaction.

    6.3 Law of Conservation of Energy, Flow of Heat and meaning of Thermal Equilibrium.

    6.4 Meaning of Heat Capacity and use of Calorimeter for Experimental determination of Heat Changes during a Reaction..

    6.5 Energy changes during Change in Phases -Heating and Cooling Curves.

    6.6 Meaning of Enthalpy of Reaction.

    6.7 Meaning of Bond Enthalpy and Use of Bond Enthalpies to Calculate Enthalpy of Reaction.

    6.8 Meaning of Enthalpy of Formation and its use to Calculate Enthalpy of Reaction.

    6.9 Hess’s Law and its use to Calculate Enthalpy of Reaction.


    UNIT 7 Equilibrium ~14–16 Class Periods 7–9% AP Exam Weighting


    7.1 Meaning of Reversible Reactions, Equilibrium and Dynamic Equilibrium.

    7.2 Equilibrium Constant expression, Magnitude of the Equilibrium Constant and Direction of Equilibrium.

    7.3 Mathematical Properties of the Equilibrium Constant.

    7.4 Comparison of Magnitude of Reaction Quotient and Equilibrium Constant to Predict Shifting of Equilibrium.

    7.5 From Equilibrium Concentrations, Calculate the Equilibrium Constant.

    7.6 Use of ICE Table to Calculate Equilibrium Concentrations.

    7.7 Representations of Equilibrium using Particulate Diagrams.

    7.8 Shifting of Equilibrium and Le Châtelier’s Principle.

    7.9 Solubility, Solubility Equilibria and Ksp.

    7.10 Effect of Common Ion and pH on the Solubility of a compound.

    7.11 Meaning of Free Energy -Driving Force of Reactions.

    7.12 Gibb’s Free Energy of dissolution.


    UNIT 8 Acids and Bases ~14–15 Class Periods 11–15% AP Exam Weighting SAP


    8.1 Introduction to Acids and Bases and Conjugate Acid and Conjugate Bases.

    8.2 Meaning and Relation between Kw ,[H+] ,[OH-] ,Ka ,Kb ,pKw, pH ,pOH pKa and pKb.

    8.3 Calculation of pH and pOH of Strong Acids and Bases.

    8.4 Weak Acid and Base Equilibria Calculation of pH and pOH of Weak Acids and Bases.

    8.5 Acidic, basic and neutral salts and their pH values.

    8.6 Meaning of Buffers and Buffer Action.

    8.7 Buffer solutions and Properties of Buffers.

    8.8 Henderson-Hasselbalch Equation to Calculate pH of a Buffer Solution.

    8.9 Meaning of Buffer Capacity.

    8.10 Change in pH during Acid -Base Titrations and pH Titration Curves.

    8.11 Effect of Molecular Structure on Strength of Acids and Bases.


    UNIT 9 Applications of Thermodynamics ~10–13 Class Periods 7–9% AP Exam Weighting


    9.1 Meaning of Spontaneity and Entropy 6 ENE.

    9.2 Entropy Change during a Chemical Reaction and Absolute Entropy.5 ENE.

    9.3 Meaning of Thermodynamic Favorable Reactions and Sign of Gibbs Free Energy and ENE.

    9.4 Thermodynamically Controlled and Kinetically Controlled Chemical Reactions.6 ENE.

    9.5 Calculation of Free Energy change for a Reaction.

    9.6 Non – Spontaneous Reactions and Coupled Reactions.4 ENE.

    9.7 Spontaneous Reaction, Cell Potential and Galvanic (Voltaic) Cell. 2 ENE.

    9.8 Relation in Cell Potential, Free Energy and Equilibrium Constant.5 ENE.

    9.9Nernst Equation-Cell Potential Under Nonstandard Conditions ENE.

    9.10 Non – Spontaneous Reactions, Electrolysis and Electrolytic Cell.

    9.11 Quantitative Application of Electrolysis -Relation between Charge ,Moles of Electrons ,Moles of Substance and Grams of Substance.


    7.1 Exceptions to the Aufbau Principle.

    7.2 Assignment of quantum numbers to the electron.

    7.3 Phase diagram.

    7.4 Calculations of molality, percent by mass and percent by volume.

    7.5 Colligative properties.

    7.6 Weaker hydrogen bonding: Hydrogen bonding due to high electronegative elements N, O, F will be tested.

    7.7 Crystal shapes or structures.

    7.8 Use of Formal change to explain why certain molecules do not obey the octet rule.

    7.9 Limitations of Lewis dot model.

    7.10 Molecules orbital diagrams, and filling of orbital diagrams.

    7.11 Varieties of crystal lattices for ionic compounds.

    7.12 Lewis- acid- Base concepts.

    7.13 Language of reducing agent and oxidizing agent.

    7.14 Labeling electrodes as positive or negative.

    7.15 Nernst Equation Calculations. Qualitative reasoning based on the Nernst Equation is the part of the exam.

    7.16 Calculations based on Arrhenius equation. Conceptual aspects and interpretation of graphs is the part of the course.

    7.17 Calculations of the concentration of each species present in the titration curve for polyprotic acids.

    7.18 Calculations of the change in pH due to addition of an acid or a base to a buffer.

    7.19 The derivation of the Henderson – Hasselbalch equation.

    7.20 Memorization of solubility rules’ other than that all salts of first group ions, ammonium and nitrates are soluble in water.


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