Get Through Medical College - Study NEET 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 NEET Chemistry Syllabus to hone your skills after every session.

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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 NEET Chemistry Exam which students can attempt in their own time and discuss with me during the sessions.


About IIT-JEE Main Chemistry Exam

IIT-JEE Mains Chesmistry is part of the IIT-JEE entrance exam which is used to measure a student's capability in Sciences, mathematics and/or architecture. Students are granted admission into the prestigous IIT-JEE instutioons and other institutions in fields related to science and arrchitecture on the basis of their senior secondary scores and IIT-JEE advanced exam scores.


IIT-JEE Main Chemistry marking scheme

The exam is now conducted on computers. The stuudents have to answer a mix of multiple choice questions and numerical answer questions in each of the three sections (physics, chemistry and mathematics). 4 marks will be awarded for each correct answer. Every incorrect answer wil incur a penalty of -1 mark.

Marks subject
100 Chemistry
100 Physics
100 Maths

The Exam


The IIT-JEE Main Chemistry exam has 2 sections

Section I - 20 questions.

MCQs are either discreet questions or sets of question, Questions are based on the knowledge of Chemistry and Science practices outlined in IIT-JEE Main Chemistry course. These questions are a mix of theoretical and numerical questions ranging from eassy to moderate difficulty. The MCQs also form the bulk of the total questions in each subject, thereby being the quickest source of marks for each student.


Section II - 10 questions

The student has to answer 5 questions out of these 10 questions

This section contains questions with numerical answers that the student must input. Usually these questions are time consuming and difficult to solve. Answering nomenclature (such as number of decimal places, rounding of numbers allowed) is often provided with these questions.

IIT-JEE Exam Calculator Policy

Calculators are not permitted in in the IIT-JEE Chemistry exam. Any attempt to use calculator will be considered as cheating and the student's exam will be terminated immediately. Thus, we highly recommend memorizing formulas, values and basic calculations beforehand.



NEET Chemistry Exam Course Content Outlined Below


UNIT I: Some Basic Concepts of Chemistry

1.1 General Introduction: Important and scope of chemistry.

1.2 Laws of Chemical Combination.

1.3 Dalton’s Atomic Theory.

1.4 Concept of elements,Atoms and molecules.

1.5 Atomic and molecular masses.

1.6 Mole concept and molar mass.

1.7 Percentage composition.

1.8 Empirical and molecular formula.

1.9 Types of Chemical reactions.

1.10 Concentrations -Molarity ,molality ,ppm ,ppb, mass percent, volume percent.

1.11 Stoichiometry and Calculations based on Stoichiometry.


UNIT II: Structure of Atom

2.1- Atomic number, Isotopes and Isobars.

2.2- Electromagnetic Spectrum.

2.3- Dual Nature of Matter and Light.

2.4- De Broglie’s Relationship.

2.5- Heisenberg Uncertainty Principle.

2.6- Concept of orbital, Quantum numbers, Concept of Shells and Subshells, Shapes of s,p and d orbitals.

2.7- Rules for filling electrons in orbitals- Aufbau principle, Pauli exclusion principles and Hund’s rule.

2.8- Electronic configuration of atoms.

2.9- Stability of half filled and completely filled orbitals.

UNIT III: Classification of Elements and Periodicity in Properties


3.1 Modern periodic law and long form of periodic table.

3.2 Periodic trends in Properties of Elements-
(a) General electronic configuration.
(b) Valence shell and valence electrons.
(c) Atomic radii.
(d) Ionic radii.
(e) Ionization enthalpy.
(f) Electron gain enthalpy.
(g) Electronegativity.
(h) Metals and non-metals.
(i) Acidic oxides and basic oxides.


UNIT IV: Chemical Bonding and Molecular Structure


4.1- Valence electrons ,rule of octet ,expanded octet and less than 8 electrons species.

4.2- Ionic bond

4.3- Covalent bond

4.4- Bond parameter like bond length and bond angle.

4.5- Formal charge and Lewis structure.

4.6- VSEPR theory, geometry of molecules and shapes of some simple molecules.

4.7- Polar character of covalent bond and polarity of molecules.

4.8- Concept of hybridization involving s, p and d orbitals and valence bond theory.

4.9- Resonance.

4.10- Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only).

4.11- Hydrogen bond.


UNITV: States of Matter:


5.1 Gases and Liquids
5.1.1- Three states of matter.

5.1.2- Intermolecular interactions.

5.1.3- Types of solids and comparison of their melting and boiling points.

5.1.4- Empirical derivation of gas law -
(a) Boyle’s law.
(b) Charle’s law.
(c) Gay Lussac’s law.
(d) Avogadro’s law.
(e) Ideal gas equation.

5.1.5- Kinetic energy and molecular speeds (elementary idea),
(a) Ideal behaviour of gases.
(b) Deviation from idealbehaviour.
(c) Liquefaction of gases.
(d) Critical temperature.


5.2 Liquid State- (qualitative idea only, no mathematical derivations).

5.2.1- Vapour pressure.

5.2.2- Boiling point.

5.2.3- Viscosity.

5.2.4- Surface tension.


UNITVI : Thermodynamics


6.1 First law of thermodynamics-internal energy and enthalpy.

6.2 Heat capacity and specific heat.

6.3 Measurement of U and H.

6.4 Hess’s law of constant heat summation.

6.5 Enthalpy of :
(a) Bond dissociation.
(b) Combustion.
(c) Formation.
(d) Atomization.
(e) Sublimation.
(f) Phase transition.
(g) Ionization.
(h) Solution and.
(i) Dilution.

6.6 Introduction of entropy as state function,

6.7 Second law of thermodynamics.

6.8 Gibbs energy change for spontaneous and non-spontaneous process.

6.9 Criteria for equilibrium and spontaneity.

6.10 Third law of thermodynamics- Brief introduction.


UNIT VII: Equilibrium


7.1 Equilibrium in physical and chemical processes,

7.2 Dynamic nature of equilibrium.

7.3- Law of chemical equilibrium.

7.4- Equilibrium constant.

7.5- Factors affecting equilibrium-Le Chatelier’s principle.

7.6- Ionic equilibrium- ionization of acids and bases.

7.7- Strong and weak electrolytes.

7.8- Degree of ionization.

7.9- Ionization of polybasic acids.

7.10- Acid strength.

7.11- Concept of pH.

7.12- Hydrolysis of salts (elementary idea).

7.13- Buffer solutions.

7.14- Henderson equation.

7.15- Solubility product.

7.16- Common ion effect (with illustrative examples).


UNIT VIII: Redox Reactions


8.1 Concept of oxidation and oxidation and reduction.

8.2 Redox reactions.

8.3 Oxidation number.

8.4 Balancing redox reactions in terms of loss and gain of electron and change in oxidation numbers.


UNIT IX: Hydrogen


9.1 Occurrence, isotopes, preparation, properties and uses of hydrogen.

9.2 Hydrides ionic,covalent and interstitial.

9.3 Physical and chemical properties of water.

9.4 Heavy water.

9.5 Hydrogen peroxide-
(a) Structure.
(b) Preparation.
(c) Reactions.
(d) Uses.


UNIT X: s-Block Elements (Alkali and Alkaline earth metals) Group I and group 2 elements:



10.1 General introduction and occurrence.

10.2 Electronic configuration.

10.3 Anomalous properties of the first element of each group.

10.4 Diagonal relationship.

10.5 Trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii).

10.6 Trends in chemical reactivity with
(a) Oxygen.
(b) Water.
(c) Hydrogen.
(d) Halogens.

10.7 Uses and preparation and properties of Some important Compounds:
(a) Sodium Carbonate.
(b) Sodium Chloride.
(c) Sodium Hydroxide and.
(d) Sodium Hydrogen Carbonate.
(e) Biological Importance of Sodium and Potassium.
(f) Industrial Use of Lime and Limestone.
(g) Biological Iimportance of Mg and Ca.


UNIT XI: Some p-Block Elements

11.1 Group 13 elements:
(a) General introduction, occurrence.
(b) Electronic configuration.
(c) Variation of properties.
(d) Oxidation states.
(e) Trends in chemical reactivity.
(f) Anomalousproperties of first element of the group.
(g) Boron and some important compounds.
i Borax.
ii Boric acids.
iii Boron hydrides.
(h) Aluminium.
i Uses.
ii Reactions with acids and alkalies.

11.2 General 14 elements:
(a) General introduction, occurrence.
(b) Electronic configuration.
(c) Variation of properties.
(d) Oxidation states.
(e) Trends in chemical reactivity.
(f) Anomalous behaviour of first element.
(g) Carbon, allotropic forms.
i Physical and chemical properties.
ii Uses of some important compounds: oxides.
(h) Important compounds of silicon and a few uses.
i Silicon tetrachloride.
ii Silicones.
iii Silicates and zeolites, their uses.


UNIT XII: Organic Chemistry- Some Basic Principles and Techniques


12.1 General introduction.

12.2 Methods of Purification Qualitative and Quantitative Analysis.

12.3 Classification and IUPAC Nomenclature of Organic Compounds.

12.4 Electronic Displacements in a Covalent bond:
(a) Inductive effect.
(b) Electromeric effect.
(c) Resonance.
(d) Hyperconjugation.
(e) Molytic and heterolytic fission of a covalent bond.

12.5 Free Radials, Carbocations,Carbanions.

12.6 Electrophiles and Nucleophiles.

12.7 Types of Organic Reactions.


UNIT XIII: Hydrocarbons


13.1 Alkanes-
(a) Nomenclature.
(b) Isomerism.
(c) Conformations (ethane only).
(d) Physical Properties.
(e) Chemical Reactions Including.
i Free Radical Mechanism of Halogenation.
ii Combustion and.
iii Pyrolysis.

13.2 Alkenes.
(a) Nomenclatur.
(b) Structure of Double Bond (Ethene).
(c) Geometrical Isomerism..
(d) Physical Properties.
(e) Methods of Preparation.
(f) Chemical Reactions: Addition of.
i Hydrogen.
ii Halogen.
iii Water.
iv Hydrogen Halides (Markovnikov’s Addition and Peroxide Effect).
v Ozonolysis.
vi Oxidation.
vii Mechanism of Electrophilic Addition.

13.3 Alkynes.

13.4 Nomenclatur.

13.5 Structure of Triple Bond (Ethyne).

13.6 Physical Properties.

13.7 Methods of Preparation.

13.8- Acidic Character of Alkynes.

13.9- Chemical Reactions: Addition Reaction of- (a) Hydrogen. (b) Halogens. (c) Hydrogen halides. (d) Water.

13.10- Aromatic Hydrocarbons.

13.11- Introduction.

13.12- IUPAC Nomenclature-Benzene.

13.13- Resonance.

13.14 Aromaticity.

13.15 Chemical Properties.
(a) Mechanism of Electrophilic Substitution.
(b) Nitration.
(c) Sulphonation.
(d) Halogenation.
(e) Friedel Craft’s Alkylation and Acylation.

13.16 Directive Influence of Functional group in mono-substituted Benzene.

13.17 Carcinogenicity and Toxicity.


UNIT XIV: Environmental Chemistry


14.1 Environmental Pollution.
(a) Air.
(b) Water and.
(c) Soil.

14.2 Chemical Reactions in Atmosphere.

14.3 Smogs.

14.4 Major Atmospheric Pollutants.

14.5 Acid Rain Ozone and its Reactions.

14.6 Effects of depletion of ozone layer.

14.7 Greenhouse Effect.

14.8 Global Qarming-Pollution Due to Industrial Wastes.

14.9 Green Chemistry as an Alternative Tool for Reducing Pollution.

14.10 Strategy for Control of Environmental Pollution.



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