25% of the NEET paper

NEET Chemistry flashcards,
built on the NTA syllabus.

Chemistry is a quarter of the NEET paper and three different subjects wearing one name. These are spaced-repetition flashcards for every chapter and subtopic of the NTA NEET Chemistry syllabus, on a schedule that adapts to each of the three separately without you having to plan it.

180
of 720 marks
45
of 180 questions
20
chapters
106
subtopics tracked
Why Chemistry slips

Three subjects.
Three different ways to forget them.

Physical Chemistry behaves like Physics: formulae, the conditions they hold under, units and standard results. Organic behaves like a language. Named reactions, reagents, conditions and selectivity rules are heavily interlinked, so a gap in one place breaks a chain somewhere else. Inorganic is close to pure memory: periodic trends and their exceptions, colours, tests, preparation methods, structures.

Those three decay at completely different rates. Inorganic decays fastest of anything in NEET, and it is also the cheapest to recover, because there is nothing to understand, only something to retrieve on time. Organic decays in chains. Physical mostly behaves.

The mistake is revising Chemistry as one subject on one schedule, which guarantees the Inorganic exceptions are always the stalest thing in your head. A per-card schedule handles this for free: the cards you keep dropping come back tight, the ones you find easy stretch out, and the three halves of Chemistry end up on three different rhythms without you designing any of it.

The syllabus

The NTA NEET Chemistry syllabus,
chapter by chapter.

All 20 chapters and 106 subtopics, in the order the NTA syllabus sets them out. This is the structure NeetFlash organises Chemistry by: cards are tagged to the subtopic, and your progress is tracked at that level, so what you see is which subtopic is slipping, not just which chapter.

01

Some Basic Concepts in Chemistry

  • Matter and its nature; Dalton's atomic theory; concepts of atom, molecule, element and compound
  • Laws of chemical combination
  • Atomic and molecular masses; mole concept; molar mass; percentage composition; empirical and molecular formulae
  • Chemical equations and stoichiometry
02

Atomic Structure

  • Nature of electromagnetic radiation; photoelectric effect; spectrum of the hydrogen atom
  • Bohr model of hydrogen atom: postulates, energy of electron and radii of orbits, limitations
  • Dual nature of matter; de Broglie's relationship; Heisenberg uncertainty principle
  • Quantum mechanical model of the atom; atomic orbitals as one-electron wave functions; variation of Ψ and Ψ² with r for 1s and 2s orbitals
  • Quantum numbers (principal, angular momentum, magnetic) and their significance; shapes of s, p and d orbitals; electron spin and spin quantum number
  • Rules for filling electrons: Aufbau principle, Pauli's exclusion principle, Hund's rule
  • Electronic configuration of elements; extra stability of half-filled and completely filled orbitals
03

Chemical Bonding and Molecular Structure

  • Kossel-Lewis approach to chemical bond formation; concept of ionic and covalent bonds
  • Ionic bonding: formation, factors affecting, calculation of lattice enthalpy
  • Covalent bonding: electronegativity, Fajan's rule, dipole moment
  • VSEPR theory and shapes of simple molecules
  • Valence bond theory; hybridization involving s, p and d orbitals; resonance
  • Molecular orbital theory: LCAO, types of molecular orbitals, sigma and pi bonds, MO electronic configurations of homonuclear diatomic molecules
  • Bond order, bond length and bond energy; metallic bonding; hydrogen bonding and applications
04

Chemical Thermodynamics

  • Fundamentals: system and surroundings, extensive and intensive properties, state functions, types of processes
  • First law of thermodynamics: work, heat, internal energy and enthalpy; heat capacity and molar heat capacity
  • Hess's law of constant heat summation
  • Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution
  • Second law of thermodynamics: spontaneity; ΔS of universe and ΔG of system as criteria; ΔG° and equilibrium constant
05

Solutions

  • Methods of expressing concentration: molality, molarity, mole fraction, percentage by volume and mass
  • Vapour pressure of solutions and Raoult's law: ideal and non-ideal solutions; vapour pressure-composition plots
  • Colligative properties: relative lowering of vapour pressure, depression of freezing point, elevation of boiling point, osmotic pressure
  • Determination of molecular mass using colligative properties; abnormal molar mass; van't Hoff factor and significance
06

Equilibrium

  • Meaning of equilibrium; concept of dynamic equilibrium
  • Equilibria involving physical processes: solid-liquid, liquid-gas and solid-gas equilibria; Henry's law
  • Equilibrium involving chemical processes: law of chemical equilibrium; Kp and Kc; significance of ΔG and ΔG°
  • Factors affecting equilibrium: concentration, pressure, temperature, catalyst; Le Chatelier's principle
  • Ionic equilibrium: weak and strong electrolytes; ionization; concepts of acids and bases (Arrhenius, Bronsted-Lowry, Lewis)
  • Acid-base equilibria including multistage ionization; ionization constants; ionization of water; pH scale
  • Common ion effect; hydrolysis of salts and pH of solutions; solubility of sparingly soluble salts and solubility products; buffer solutions
07

Redox Reactions and Electrochemistry

  • Electronic concepts of oxidation and reduction; redox reactions; oxidation number; rules for assigning; balancing of redox reactions
  • Electrolytic and metallic conduction; conductance in electrolytic solutions; molar conductivities and variation with concentration; Kohlrausch's law and applications
  • Electrochemical cells: electrolytic and galvanic; types of electrodes; electrode potentials including standard electrode potential
  • Half-cell and cell reactions; EMF of a galvanic cell and measurement; Nernst equation and applications
  • Relationship between cell potential and Gibbs energy change; dry cell and lead accumulator; fuel cells
08

Chemical Kinetics

  • Rate of a chemical reaction; factors affecting rate: concentration, temperature, pressure and catalyst
  • Elementary and complex reactions; order and molecularity; rate law; rate constant and units
  • Differential and integral forms of zero and first-order reactions, characteristics and half-lives
  • Effect of temperature on rate; Arrhenius theory; activation energy and calculation
  • Collision theory of bimolecular gaseous reactions (no derivation)
09

Classification of Elements and Periodicity in Properties

  • Modern periodic law and present form of the periodic table
  • s, p, d and f block elements
  • Periodic trends: atomic and ionic radii, ionization enthalpy, electron gain enthalpy
  • Valence, oxidation states and chemical reactivity
10

p-Block Elements

  • General introduction to Group 13 to Group 18 elements
  • Electronic configuration and general trends in physical and chemical properties across periods and down the groups
  • Unique behaviour of the first element in each group
11

d- and f-Block Elements

  • Transition elements: general introduction, electronic configuration, occurrence and characteristics
  • General trends in properties of first-row transition elements: physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation
  • Preparation, properties and uses of K2Cr2O7 and KMnO4
  • Lanthanoids: electronic configuration, oxidation states and lanthanoid contraction
  • Actinoids: electronic configuration and oxidation states
12

Co-ordination Compounds

  • Introduction to coordination compounds; Werner's theory; ligands, coordination number, denticity, chelation
  • IUPAC nomenclature of mononuclear coordination compounds; isomerism
  • Bonding: valence bond approach and basic ideas of crystal field theory; colour and magnetic properties
  • Importance of coordination compounds: qualitative analysis, extraction of metals, biological systems
13

Purification and Characterisation of Organic Compounds

  • Purification: crystallization, sublimation, distillation, differential extraction and chromatography: principles and applications
  • Qualitative analysis: detection of nitrogen, sulphur, phosphorus and halogens
  • Quantitative analysis (basic principles only): estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus
  • Calculations of empirical and molecular formulae; numerical problems in organic quantitative analysis
14

Some Basic Principles of Organic Chemistry

  • Tetravalency of carbon; shapes of simple molecules; hybridization (s and p)
  • Classification of organic compounds based on functional groups; homologous series
  • Isomerism: structural and stereoisomerism
  • Nomenclature: trivial and IUPAC
  • Covalent bond fission: homolytic and heterolytic; free radicals, carbocations and carbanions; stability; electrophiles and nucleophiles
  • Electronic displacement in a covalent bond: inductive effect, electromeric effect, resonance and hyperconjugation
  • Common types of organic reactions: substitution, addition, elimination and rearrangement
15

Hydrocarbons

  • Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions
  • Alkanes: conformations (Sawhorse and Newman projections of ethane); mechanism of halogenation
  • Alkenes: geometrical isomerism; mechanism of electrophilic addition (hydrogen, halogens, water, hydrogen halides: Markownikoff and peroxide effect); ozonolysis and polymerization
  • Alkynes: acidic character; addition reactions; polymerization
  • Aromatic hydrocarbons: nomenclature; benzene structure and aromaticity; mechanism of electrophilic substitution: halogenation, nitration
  • Friedel-Crafts alkylation and acylation; directive influence of functional group in monosubstituted benzene
16

Organic Compounds Containing Halogens

  • General methods of preparation, properties and reactions; nature of C-X bond
  • Mechanisms of substitution reactions
  • Uses; environmental effects of chloroform, iodoform, freons and DDT
17

Organic Compounds Containing Oxygen

  • General methods of preparation, properties, reactions and uses
  • Alcohols: identification of primary, secondary, tertiary; mechanism of dehydration
  • Phenols: acidic nature, electrophilic substitution (halogenation, nitration, sulphonation); Reimer-Tiemann reaction
  • Ethers: structure
  • Aldehydes and ketones: nature of carbonyl group; nucleophilic addition; relative reactivities
  • Important reactions: nucleophilic addition (HCN, NH3 and derivatives), Grignard reagent; oxidation; reduction (Wolf-Kishner and Clemmensen)
  • Acidity of α-hydrogen; aldol condensation, Cannizzaro reaction, haloform reaction; chemical tests to distinguish aldehydes and ketones
  • Carboxylic acids: acidic strength and factors affecting it
18

Organic Compounds Containing Nitrogen

  • General methods of preparation, properties, reactions and uses
  • Amines: nomenclature, classification, structure; identification of primary, secondary, tertiary amines and their basic character
  • Diazonium salts: importance in synthetic organic chemistry
19

Biomolecules

  • General introduction and importance of biomolecules
  • Carbohydrates: classification; aldoses and ketoses; monosaccharides (glucose, fructose); constituent monosaccharides of oligosaccharides (sucrose, lactose, maltose)
  • Proteins: α-amino acids, peptide bond, polypeptides; primary, secondary, tertiary, quaternary structure (qualitative); denaturation; enzymes
  • Vitamins: classification and functions
  • Nucleic acids: chemical constitution of DNA and RNA; biological functions
  • Hormones (general introduction)
20

Principles Related to Practical Chemistry

  • Detection of extra elements (nitrogen, sulphur, halogens) in organic compounds
  • Detection of functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones), carboxyl and amino groups
  • Preparation of inorganic compounds: Mohr's salt, potash alum
  • Preparation of organic compounds: acetanilide, p-nitroacetanilide, aniline yellow, iodoform
  • Titrimetric exercises: acids, bases and use of indicators; oxalic acid vs KMnO4; Mohr's salt vs KMnO4
  • Qualitative salt analysis: cations (Pb²⁺, Cu²⁺, Al³⁺, Fe³⁺, Zn²⁺, Ni²⁺, Ca²⁺, Ba²⁺, Mg²⁺, NH₄⁺) and anions (CO₃²⁻, S²⁻, SO₄²⁻, NO₃⁻, NO₂⁻, Cl⁻, Br⁻, I⁻)
  • Enthalpy of solution of CuSO4; enthalpy of neutralization of strong acid and strong base
  • Preparation of lyophilic and lyophobic sols
  • Kinetic study of the reaction of iodide ions with hydrogen peroxide at room temperature
The schedule

How FSRS-5 handles Chemistry.

Because FSRS-5 holds a difficulty figure per card and not per chapter, the Inorganic exception you keep losing is scheduled tightly while the Physical formula you find obvious stretches out to months, inside the same subject and in the same daily session. That is the part a hand-written revision plan cannot do: it would need one rhythm per fact, and you have thousands of facts.

The interval is not a setting you pick. It is computed from your own ratings, per card, and it is the day your recall of that fact is predicted to fall to 90%: your own forgetting curve for that one fact, rather than a weekly rotation everybody shares. How the engine works ›

Past papers

NEET previous year questions,
sorted by Chemistry topic.

Inorganic in particular is drawn from a well NTA returns to, and the fastest way to find out whether a trend has actually stuck is to meet it in the form it was asked. NeetFlash serves NEET previous year questions sorted by topic, so you can follow a chapter’s cards straight into that chapter’s past questions, and send the misses to your mistake bank tagged by subtopic.

Questions

NEET Chemistry flashcards: common questions

Are these aligned with the latest NTA NEET Chemistry syllabus?
Yes. The list on this page is the structure the cards are organised by: 20 chapters and 106 subtopics from the NTA NEET syllabus, spanning Physical, Organic and Inorganic. Cards are tagged to the subtopic and progress is tracked at that level.
My Inorganic Chemistry keeps slipping. Does this actually help?
This is the exact case spaced repetition was designed for. Inorganic is a large body of facts with very little internal structure to hang them on, so it decays quickly and predictably. Predictable decay is something an algorithm can stay ahead of. FSRS-5 schedules each trend, exception, colour and test on its own interval, based on how you have actually performed on that specific card.
Does it cover Organic reaction mechanisms?
Named reactions, reagents, conditions and products are cards, because those are the things you lose. The mechanism itself is something you understand once, in class or from NCERT. What NeetFlash does is stop that understanding from fading into “I have definitely seen this” by the time you sit the paper.
Do I still need to practise numericals?
Yes, and NeetFlash includes that: chapter tests plus full-length mock tests marked +4 / −1, with everything you get wrong collected in a mistake bank tagged by topic. Cards handle recall; tests handle applying it against the clock.
Do I have to pay to use it?
No. Every new account opens with 7 days of Premium, free, no card needed. After that the free plan gives you 10 flashcard reviews and 50 searches a day, and progress tracking, weak-spot analysis, streaks and the mistake bank stay free with no daily cap.
The other two

Stop re-reading.
Start remembering.

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