Course Outline
Check off chapters as you study them, and take each module's test when you're ready. Everything is saved locally in your browser β nothing is uploaded, no account needed.
A note on these questions
These are practice questions written in NEET-style by the Bryn Flow team, covering the correct syllabus concepts for each chapter β they are not reproduced from official past-year papers. NEET Chemistry leans heavily on direct NCERT-line recall, especially in Inorganic and Organic sections, and these questions are calibrated accordingly rather than mirroring JEE's more calculation-driven Physical Chemistry emphasis.
Module 1 β Foundations
1 Some Basic Concepts in Chemistry
The mole is the SI base unit for amount of substance. One mole of any ideal gas occupies 22.4 litres at STP, regardless of which gas it is. Normality expresses concentration in terms of gram-equivalents of solute per litre of solution β a unit that shows up often in titration calculations.
Percentage composition of a compound is calculated from the mass contribution of each element relative to the compound's total molar mass β the basis for determining empirical formulas from experimental data.
2 States of Matter
Boyle's law relates a gas's pressure and volume at constant temperature; Charles's law relates volume and temperature at constant pressure. Absolute zero is the theoretical temperature at which molecular motion would cease entirely.
A liquid's vapor pressure increases with temperature, since more molecules gain enough energy to escape into the vapor phase β this is directly why liquids boil at higher temperatures under higher external pressure.
3 Atomic Structure
Protons, positively charged, reside in the nucleus alongside neutrally charged neutrons; electrons occupy discrete energy levels surrounding the nucleus, per the Bohr model. Isotopes of an element share the same atomic number (proton count) but differ in mass number (neutron count).
The s-subshell can hold a maximum of 2 electrons, p holds 6, d holds 10, and f holds 14 β a pattern worth memorizing solidly, since it underlies electronic configuration questions throughout the syllabus.
4 Chemical Bonding and Molecular Structure
Ionic bonds form through the complete transfer of electrons between atoms; covalent bonds form through the sharing of electron pairs. Water (HβO) has a bent (angular) molecular geometry, not a straight line, due to the two lone pairs on oxygen.
Hydrogen bonding between water molecules is responsible for water's unusually high boiling point compared to other molecules of similar molar mass.
Module 2 β Physical Chemistry II
5 Chemical Thermodynamics
An exothermic reaction releases heat to the surroundings (negative ΞH); an endothermic reaction absorbs heat from the surroundings (positive ΞH). Enthalpy change is conventionally denoted ΞH.
A reaction is spontaneous when its Gibbs free energy change, ΞG, is negative β this single quantity combines the competing effects of enthalpy and entropy change into one spontaneity criterion.
6 Solutions
A saturated solution contains the maximum amount of solute that can dissolve at a given temperature β adding more solute simply leaves undissolved solid behind. For most solid solutes in water, solubility increases with temperature.
Molarity is technically temperature-dependent (since it's based on solution volume, which can expand slightly with heat), unlike molality. Adding a solute generally lowers the freezing point of the solvent (freezing point depression), one of the classic colligative properties.
7 Equilibrium
At chemical equilibrium, the forward and reverse reaction rates are equal, so concentrations of reactants and products stay constant (though the reactions haven't stopped). A strong acid dissociates essentially completely in water, unlike a weak acid, which only partially ionizes.
pH is calculated as the negative logarithm (base 10) of hydrogen ion concentration. A catalyst speeds up the rate at which equilibrium is reached, but does not shift the equilibrium position itself.
Module 3 β Physical Chemistry III
8 Redox Reactions and Electrochemistry
Reduction involves the gain of electrons (oxidation is the corresponding loss). An electrochemical cell (battery) converts chemical energy into electrical energy through a spontaneous redox reaction.
The rusting of iron is a familiar real-world example of a redox reaction β iron is oxidized in the presence of oxygen and moisture. Electric charge relevant to electrolysis calculations is measured in coulombs.
9 Chemical Kinetics
Reaction rate generally increases with increasing temperature, since more molecules gain enough energy to overcome the activation energy barrier. A catalyst is not consumed in the overall reaction β it's regenerated at the end, even though it participates in intermediate steps.
Reaction rate is expressed as the change in reactant or product concentration per unit time. A higher activation energy generally means a slower reaction rate at a given temperature, since fewer molecular collisions have enough energy to react.
10 Classification of Elements and Periodicity
Elements in the same group (column) of the periodic table share similar chemical properties, since they have the same number of valence electrons. Metallic character generally decreases moving across a period from left to right.
Noble gases show very low reactivity due to their stable, complete outer electron shells. The modern periodic table arranges elements in order of increasing atomic number, not atomic mass.
Module 4 β Inorganic Chemistry
11 p-Block Elements
Group 17 elements (the halogens) are highly reactive nonmetals, readily forming compounds with most other elements. Carbon is distinctively known for catenation β its ability to form long chains and rings by bonding to itself, which underlies the entire field of organic chemistry.
Nitrogen makes up about 78% of Earth's atmosphere by volume. Group 18 elements are called noble gases precisely because their filled outer electron shells make them chemically inert under most conditions.
12 d- and f-Block Elements
Transition elements are found in the d-block of the periodic table β familiar examples include iron, copper, and zinc. Transition metals typically have relatively high melting and boiling points, due to strong metallic bonding involving both s and d electrons.
The lanthanides and actinides, sometimes shown as a separate row below the main table, belong to the f-block.
13 Coordination Compounds
A ligand donates a lone pair of electrons to a central metal atom or ion, forming a coordinate (dative) bond. Werner's theory laid the historical foundation for modern coordination chemistry.
Two biologically vital coordination compounds worth remembering: hemoglobin has iron as its central coordinated metal ion (essential for oxygen transport in blood), while chlorophyll has magnesium as its central metal ion (essential for photosynthesis).
14 General Principles of Extraction of Metals
An ore is a naturally occurring mineral from which a metal can be extracted profitably; the unwanted impurities present alongside it are called gangue. Blast furnaces are the standard industrial method used to extract iron from its ore.
Electrolytic refining is used to obtain very high-purity metals, passing an electric current through a solution to selectively deposit pure metal at one electrode.
Module 5 β Organic Chemistry I
15 Basic Principles of Organic Chemistry
Organic chemistry is fundamentally the study of carbon compounds. Isomers share the same molecular formula but differ in structural arrangement, often giving them quite different physical and chemical properties.
A molecule's functional group β like a hydroxyl or carbonyl group β largely determines its characteristic chemical behavior, regardless of the rest of the carbon skeleton. Distillation separates mixtures of compounds based on differences in boiling point.
16 Hydrocarbons
Alkanes are saturated hydrocarbons containing only single carbon-carbon bonds; alkenes contain at least one carbon-carbon double bond. Benzene is a well-known aromatic hydrocarbon, its structure a ring of six carbon atoms with delocalized electrons.
Complete combustion of any hydrocarbon in excess oxygen produces carbon dioxide and water as the only products, releasing energy β the basis of using hydrocarbons as fuels.
17 Organic Compounds Containing Halogens
Haloalkanes contain a halogen atom (F, Cl, Br, or I) bonded to an alkyl group. Chloroform (CHClβ) was historically used as an anesthetic before safer alternatives were developed.
DDT, a chlorinated organic compound, was once widely used as an insecticide before its environmental persistence and toxicity led to bans in many countries. Freons (CFCs) were historically used as refrigerants, though their role in ozone depletion has led to their phase-out.
Module 6 β Organic Chemistry II
18 Organic Compounds Containing Oxygen
Alcohols contain a hydroxyl (βOH) functional group. Acetic acid (ethanoic acid) is the main component responsible for vinegar's characteristic sourness and smell.
Both aldehydes and ketones contain a carbonyl (C=O) group, differing in what's attached on either side. Esters are commonly responsible for the pleasant, fruity smell characteristic of many fruits.
19 Organic Compounds Containing Nitrogen
Amines can be thought of as organic derivatives of ammonia, with one or more hydrogens replaced by alkyl or aryl groups. Aniline is a well-known aromatic amine, derived from benzene.
Proteins are built from amino acids, each containing both an amine group and a carboxylic acid group. Urea, a nitrogen-containing waste compound, is excreted by the human body as a way of safely removing excess nitrogen.
20 Biomolecules, Polymers & Chemistry in Everyday Life
The four major classes of biomolecules are carbohydrates, proteins, lipids, and nucleic acids. Both starch and cellulose are polysaccharides built from repeating glucose units, despite having very different properties due to different bonding patterns between those units.
Enzymes are biological catalysts, mostly made of protein. Polymers in general are large molecules built from many repeating smaller units called monomers.