Examius
🇮🇳 JEE Advanced · subject
JEE Advanced Chemistry Syllabus
The Chemistry syllabus for JEE Advanced in full: 37 chapters, 201 topics and 232 sub-topics, every one listed below, plus 50 Chemistry flashcards with answers.
Chemistry syllabus: all 37 chapters
Expand any chapter to see its topics and sub-topics.
-
General Topics
7 topics- Concept of atoms and molecules
- Dalton’s atomic theory
- Mole concept
- Chemical formulae
- Balanced chemical equations
- Calculations involving common reactions
- Oxidation-reduction reactions
- Neutralisation reactions
- Displacement reactions
- Concentration
- Mole fraction
- Molarity
- Molality
- Normality
-
States of Matter: Gases and Liquids
8 topics- Gas laws and ideal gas equation
- Absolute scale of temperature
- Deviation from ideality
- Van der Waals equation
- Kinetic theory of gases
- Average velocity
- Root mean square velocity
- Most probable velocity
- Relation with temperature
- Law of partial pressures
- Diffusion of gases
- Intermolecular interactions
- Types
- Distance dependence
- Effect on properties
- Liquids
- Vapour pressure
- Surface tension
- Viscosity
-
Atomic Structure
8 topics- Bohr model
- Wave-particle duality
- De Broglie hypothesis
- Uncertainty principle
- Qualitative quantum mechanical picture of hydrogen atom
- Energies
- Quantum numbers
- Wave function and probability density (plots only)
- Shapes of s, p and d orbitals
- Aufbau principle
- Pauli’s exclusion principle
- Hund’s rule
-
Chemical Bonding and Molecular Structure
6 topics- Orbital overlap and covalent bond
- Hybridisation involving s, p and d orbitals only
- Molecular orbital energy diagrams for homonuclear diatomic species (up to Ne2)
- Hydrogen bond
- Polarity in molecules, dipole moment
- VSEPR model and shapes of molecules
- Linear
- Angular
- Triangular
- Square planar
- Pyramidal
- Square pyramidal
- Trigonal bipyramidal
- Tetrahedral
- Octahedral
-
Chemical Thermodynamics
10 topics- Intensive and extensive properties
- State functions
- First law of thermodynamics
- Internal energy, work (pressure-volume only) and heat
- Enthalpy, heat capacity, standard state, Hess’s law
- Enthalpy of reaction, fusion and vaporization, and lattice enthalpy
- Second law of thermodynamics
- Entropy
- Gibbs energy
- Criteria of equilibrium and spontaneity
-
Chemical and Ionic Equilibrium
8 topics- Law of mass action
- Equilibrium constant (Kp and Kc) and reaction quotient
- Le Chatelier’s principle
- Effect of concentration
- Effect of temperature
- Effect of pressure
- Solubility product and its applications
- Common ion effect
- pH and buffer solutions
- Acids and bases (Bronsted and Lewis concepts)
- Hydrolysis of salts
-
Electrochemistry
8 topics- Electrochemical cells and cell reactions
- Standard electrode potentials
- Electrochemical work, Nernst equation
- Electrochemical series, emf of galvanic cells
- Faraday’s laws of electrolysis
- Electrolytic conductance, specific, equivalent and molar conductivity, Kohlrausch’s law
- Batteries: Primary and Secondary, fuel cells
- Corrosion
-
Chemical Kinetics
6 topics- Rates of chemical reactions
- Order and molecularity of reactions
- Rate law, rate constant, half-life
- Differential and integrated rate expressions for zero and first order reactions
- Temperature dependence of rate constant (Arrhenius equation and activation energy)
- Catalysis
- Homogeneous catalysis
- Heterogeneous catalysis
- Enzyme catalysis and its mechanism
-
Solid State
8 topics- Classification of solids
- Crystalline state
- Seven crystal systems
- Cell parameters a, b, c, α, β, γ
- Close packed structure of solids
- Cubic and hexagonal
- Packing in fcc, bcc and hcp lattices
- Nearest neighbours
- Ionic radii and radius ratio
- Point defects
-
Solutions
5 topics- Henry’s law
- Raoult’s law
- Ideal solutions
- Colligative properties
- Lowering of vapour pressure
- Elevation of boiling point
- Depression of freezing point
- Osmotic pressure
- Van’t Hoff factor
-
Surface Chemistry
3 topics- Elementary concepts of adsorption
- Physisorption
- Chemisorption
- Colloids
- Types
- Methods of preparation
- General properties
- Elementary ideas of emulsions, surfactants and micelles
- Definitions and examples
- Elementary concepts of adsorption
-
Classification of Elements and Periodicity in Properties
3 topics- Modern periodic law and the present form of periodic table
- Electronic configuration of elements
- Periodic trends
- Atomic radius
- Ionic radius
- Ionization enthalpy
- Electron gain enthalpy
- Valence
- Oxidation states
- Electronegativity
- Chemical reactivity
-
Hydrogen
10 topics- Position of hydrogen in periodic table
- Occurrence
- Isotopes
- Preparation
- Properties and uses of hydrogen
- Hydrides
- Ionic
- Covalent
- Interstitial
- Physical and chemical properties of water
- Heavy water
- Hydrogen peroxide
- Preparation
- Reactions
- Use and structure
- Hydrogen as a fuel
-
s-Block Elements
7 topics- Alkali and alkaline earth metals-reactivity towards air, water, dihydrogen, halogens, acids
- Reducing nature including solutions in liquid ammonia
- Uses of alkali and alkaline earth metals
- General characteristics of oxides, hydroxides, halides, salts of oxoacids
- Anomalous behaviour of lithium and beryllium
- Preparation, properties, and uses of compounds of sodium
- Sodium carbonate
- Sodium chloride
- Sodium hydroxide
- Sodium hydrogen carbonate
- Preparation, properties, and uses of compounds of calcium
- Calcium oxide
- Calcium hydroxide
- Calcium carbonate
- Calcium sulphate
-
p-Block Elements
8 topics- Oxidation state and trends in chemical reactivity of elements of groups 13-17
- Anomalous properties of boron, carbon, nitrogen, oxygen, and fluorine
- Group 13
- Reactivity towards acids, alkalis, and halogens
- Preparation, properties, and uses of borax, orthoboric acid, diborane, boron trifluoride, aluminium chloride, alums
- Uses of boron and aluminium
- Group 14
- Reactivity towards water and halogen
- Allotropes of carbon and uses of carbon
- Preparation, properties, and uses of carbon monoxide, carbon dioxide, silicon dioxide, silicones, silicates, zeolites
- Group 15
- Reactivity towards hydrogen, oxygen, and halogen
- Allotropes of phosphorous
- Preparation, properties, and uses of dinitrogen, ammonia, nitric acid, phosphine, phosphorus trichloride, phosphorus pentachloride
- Oxides of nitrogen and oxoacids of phosphorus
- Group 16
- Reactivity towards hydrogen, oxygen, and halogen
- Allotropes of sulfur
- Preparation, properties, and uses of dioxygen, ozone, sulfur dioxide, sulfuric acid
- Oxoacids of sulfur
- Group 17
- Reactivity towards hydrogen, oxygen, and metals
- Preparation, properties, and uses of chlorine, hydrogen chloride and interhalogen compounds
- Oxoacids of halogens, bleaching powder
- Group 18
- Chemical properties and uses
- Compounds of xenon with fluorine and oxygen
-
d-Block Elements
7 topics- Oxidation states and their stability
- Standard electrode potentials
- Interstitial compounds
- Alloys
- Catalytic properties
- Applications
- Preparation, structure, and reactions of oxoanions of chromium and manganese
-
f-Block Elements
3 topics- Lanthanoid and actinoid contractions
- Oxidation states
- General characteristics
-
Coordination Compounds
11 topics- Werner’s theory
- Nomenclature
- Cis-trans and Ionization Isomerism
- Hybridization and Geometries
- Linear
- Tetrahedral
- Square Planar
- Octahedral
- Bonding
- VBT
- CFT (Octahedral and Tetrahedral Fields)
- Magnetic Properties
- Spin-only
- Colour of 3d-series Coordination Compounds
- Ligands and Spectrochemical Series
- Stability
- Importance and Applications
- Metal Carbonyls
-
Isolation of Metals
4 topics- Metal Ores and their Concentration
- Extraction of Crude Metal from Concentrated Ores
- Thermodynamic (Iron, Copper, Zinc)
- Electrochemical (Aluminium)
- Cyanide Process
- Silver and Gold
- Refining
-
Principles of Qualitative Analysis
5 topics- Groups I to V (Ag+, Hg2+, Cu2+, Pb2+, Fe3+, Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+, Mg2+)
- Nitrate
- Halides (excluding Fluoride)
- Carbonate and Bicarbonate
- Sulphate and Sulphide
-
Environmental Chemistry
6 topics- Atmospheric Pollution
- Water Pollution
- Soil Pollution
- Industrial Waste
- Strategies to Control Environmental Pollution
- Green Chemistry
-
Basic Principles of Organic Chemistry
13 topics- Hybridisation of carbon
- σ and π-bonds
- Shapes of simple organic molecules
- Aromaticity
- Structural and geometrical isomerism
- Stereoisomers and stereochemical relationship
- Enantiomers
- Diastereomers
- Meso
- Determination of empirical and molecular formulae
- Combustion method
- IUPAC nomenclature of organic molecules
- Hydrocarbons
- Cyclic hydrocarbons
- Mono-functional derivatives
- Bi-functional derivatives
- Hydrogen bonding effects
- Inductive, Resonance and Hyperconjugative effects
- Acidity and basicity of organic compounds
- Reactive intermediates
- Homolytic bond cleavage
- Heterolytic bond cleavage
- Formation, structure and stability
- Carbocations
- Carbanions
- Free radicals
-
Alkanes
6 topics- Homologous series
- Physical properties
- Melting points
- Boiling points
- Density
- Effect of branching
- Conformations of ethane and butane
- Newman projections
- Preparation
- From alkyl halides
- From aliphatic carboxylic acids
- Reactions
- Combustion
- Halogenation
- Allylic halogenation
- Benzylic halogenation
- Oxidation
-
Alkenes and Alkynes
3 topics- Physical properties
- Boiling points
- Density
- Dipole moments
- Preparation
- By elimination reactions
- Reactions
- Acid catalysed hydration
- Metal acetylides
- KMnO4 reactions
- Ozone reactions
- Reduction reactions
- Electrophilic addition reactions
- Effect of peroxide
- Cyclic polymerization reactions
- Physical properties
-
Benzene
3 topics- Structure
- Electrophilic substitution reactions
- Halogenation
- Nitration
- Sulphonation
- Friedel-Crafts alkylation
- Friedel-Crafts acylation
- Effect of directing groups
- Monosubstituted benzene
-
Phenols
4 topics- Physical properties
- Preparation
- Electrophilic substitution reactions
- Halogenation
- Nitration
- Sulphonation
- Reactions
- Reimer-Tiemann reaction
- Kolbe reaction
- Esterification
- Etherification
- Aspirin synthesis
- Oxidation reactions
- Reduction reactions
-
Alkyl Halides
2 topics- Rearrangement reactions
- Alkyl carbocation
- Reactions
- Grignard reactions
- Nucleophilic substitution reactions
- Rearrangement reactions
-
Alcohols
2 topics- Physical properties
- Reactions
- Esterification
- Dehydration
- Reactions with sodium
- Reactions with phosphorus halides
- Reactions with ZnCl2/concentrated HCl
- Reactions with thionyl chloride
- Conversion into aldehydes
- Conversion into ketones
- Conversion into carboxylic acids
-
Ethers
2 topics- Preparation
- Williamson’s synthesis
- Reactions
- C-O bond cleavage reactions
- Preparation
-
Aldehydes and Ketones
2 topics- Preparation
- From acid chlorides
- From nitriles
- From esters
- From toluene
- From benzene
- Reactions
- Oxidation reactions
- Reduction reactions
- Oxime formation
- Hydrazone formation
- Aldol condensation
- Cannizzaro reaction
- Haloform reaction
- Nucleophilic addition reactions
- Preparation
-
Carboxylic Acids
3 topics- Physical properties
- Preparation
- From nitriles
- From Grignard reagents
- From esters
- From amides
- From alkylbenzenes
- Reactions
- Reduction reactions
- Halogenation reactions
- Ester formation
- Acid chloride formation
- Amide formation
-
Amines
2 topics- Preparation
- From nitro compounds
- From nitriles
- From amides
- Reactions
- Hoffmann bromamide degradation
- Gabriel phthalimide synthesis
- Reaction with nitrous acid
- Azo coupling reaction
- Sandmeyer reactions
- Carbylamine reaction
- Hinsberg test
- Alkylation reactions
- Acylation reactions
- Preparation
-
Haloarenes
1 topic- Reactions
- Fittig reaction
- Wurtz-Fittig reaction
- Nucleophilic aromatic substitution
- Substituted haloarenes
- Reactions
-
Biomolecules
3 topics- Carbohydrates
- Classification
- Mono- and di-saccharides (glucose and sucrose)
- Oxidation
- Reduction
- Glycoside formation
- Hydrolysis of disaccharides (sucrose, maltose, lactose)
- Anomers
- Proteins
- Amino acids
- Peptide linkage
- Structure of peptides (primary and secondary)
- Types of proteins (fibrous and globular)
- Nucleic acids
- Chemical composition and structure of DNA and RNA
- Carbohydrates
-
Polymers
9 topics- Types of polymerization (addition, condensation)
- Homo and copolymers
- Natural rubber
- Cellulose
- Nylon
- Teflon
- Bakelite
- PVC
- Bio-degradable polymers
- Applications of polymers
- Types of polymerization (addition, condensation)
-
Chemistry in Everyday Life
3 topics- Therapeutic action
- Antacids
- Antihistamines
- Tranquilizers
- Analgesics
- Antimicrobials
- Antifertility drugs
- Artificial sweeteners names only
- Soaps, detergents, and cleansing action
- Therapeutic action
-
Practical Organic Chemistry
2 topics- Detection of elements
- N
- S
- Halogens
- Detection and identification of functional groups
- Hydroxyl (alcoholic and phenolic)
- Carbonyl (aldehyde and ketone)
- Carboxyl
- Amino
- Nitro
- Detection of elements
JEE Advanced Chemistry flashcards — 50 questions with answers
State the main postulates of Dalton's atomic theory.
(1) Matter is made of tiny indivisible particles called atoms. (2) Atoms of a given element are identical in mass and properties; atoms of different elements differ. (3) Atoms combine in small whole-number ratios to form compounds. (4) Atoms can neither be created nor destroyed in a chemical reaction (only rearranged).
Distinguish between an atom and a molecule.
An atom is the smallest particle of an element that takes part in a chemical reaction. A molecule is the smallest particle of an element or compound that can exist independently, formed by two or more atoms chemically bonded (e.g. $\ce{O2}$, $\ce{H2O}$).
Which two laws of chemical combination did Dalton's atomic theory explain?
The law of conservation of mass and the law of constant (definite) proportions. It also predicted the law of multiple proportions.
State the law of multiple proportions and give an example.
When two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in small whole-number ratios. Example: in $\ce{CO}$ and $\ce{CO2}$, the masses of oxygen combining with $12\ \text{g}$ of carbon are $16\ \text{g}$ and $32\ \text{g}$, a ratio of $1:2$.
Define one mole and give the value of Avogadro's number.
One mole is the amount of substance containing as many elementary entities as there are atoms in $12\ \text{g}$ of $\ce{^{12}C}$. This number is Avogadro's number, $N_A = 6.022 \times 10^{23}\ \text{mol}^{-1}$.
How is the number of moles related to mass and molar mass?
$$n = \frac{m}{M}$$ where $n$ is moles, $m$ is the given mass, and $M$ is the molar mass in $\text{g mol}^{-1}$.
How do you find the number of particles from the number of moles?
$$N = n \times N_A$$ where $N$ is the number of particles, $n$ is moles, and $N_A = 6.022 \times 10^{23}\ \text{mol}^{-1}$.
What is the molar volume of an ideal gas at STP?
$22.4\ \text{L mol}^{-1}$ (i.e. $22400\ \text{cm}^3$) at $273.15\ \text{K}$ and $1\ \text{atm}$. Number of moles of a gas at STP $= \dfrac{V}{22.4\ \text{L}}$.
Define molar mass and how it relates to relative molecular mass.
Molar mass is the mass of one mole of a substance, expressed in $\text{g mol}^{-1}$. It is numerically equal to the relative atomic/molecular mass (which is dimensionless, defined relative to $\frac{1}{12}$ the mass of a $\ce{^{12}C}$ atom).
What is the difference between an empirical formula and a molecular formula?
The empirical formula gives the simplest whole-number ratio of atoms (e.g. $\ce{CH2O}$). The molecular formula gives the actual number of atoms in a molecule (e.g. $\ce{C6H12O6}$). Molecular formula $= n \times$ empirical formula.
How is the molecular formula obtained from the empirical formula?
Compute $n = \dfrac{\text{molar mass}}{\text{empirical formula mass}}$, then multiply each subscript of the empirical formula by $n$.
Outline the steps to determine an empirical formula from percentage composition.
(1) Divide each element's percentage by its atomic mass to get relative moles. (2) Divide all results by the smallest value. (3) Round to the nearest whole number (multiply if needed) to get the simplest atom ratio.
What is the mole fraction of a component in a mixture?
$$x_A = \frac{n_A}{n_A + n_B + \dots}$$ The sum of all mole fractions equals 1: $x_A + x_B + \dots = 1$. Mole fraction is dimensionless.
Define molarity and give its formula and units.
Molarity is the number of moles of solute per litre of solution: $$M = \frac{n_{\text{solute}}}{V_{\text{solution (L)}}}$$ Units: $\text{mol L}^{-1}$ (M). It is temperature dependent.
Define molality and give its formula and units.
Molality is the number of moles of solute per kilogram of solvent: $$m = \frac{n_{\text{solute}}}{w_{\text{solvent (kg)}}}$$ Units: $\text{mol kg}^{-1}$. It is independent of temperature.
Why is molality preferred over molarity for studies involving temperature change?
Molality is based on the mass of solvent, which does not change with temperature, whereas molarity is based on volume of solution, which expands or contracts with temperature.
Define normality and how it relates to molarity.
Normality is the number of gram-equivalents of solute per litre of solution: $$N = \frac{\text{gram equivalents}}{V_{\text{(L)}}}$$ It relates to molarity by $N = M \times n$, where $n$ is the n-factor (valency factor).
What is the n-factor (equivalent factor) for acids, bases, and redox species?
For an acid: number of replaceable $\ce{H+}$ ions. For a base: number of replaceable $\ce{OH-}$ ions. For a redox species: number of electrons gained or lost per formula unit.
What is the equivalent mass of a substance?
$$\text{Equivalent mass} = \frac{\text{molar mass}}{n\text{-factor}}$$ For example, equivalent mass of $\ce{H2SO4} = \frac{98}{2} = 49\ \text{g eq}^{-1}$.
State the relationship between molarity, mass percentage, and density of a solution.
$$M = \frac{10 \times \%\text{(w/w)} \times d}{M_{\text{solute}}}$$ where $d$ is the density in $\text{g mL}^{-1}$ and $M_{\text{solute}}$ is the molar mass in $\text{g mol}^{-1}$.
Show the other 30 Chemistry flashcards
What does it mean to balance a chemical equation, and on what law is it based?
Balancing means making the number of atoms of each element equal on both sides by adjusting stoichiometric coefficients. It is based on the law of conservation of mass.
Balance the combustion of methane.
$$\ce{CH4 + 2O2 -> CO2 + 2H2O}$$
Balance the formation of ammonia from its elements.
$$\ce{N2 + 3H2 -> 2NH3}$$
Define the limiting reagent.
The limiting reagent is the reactant that is completely consumed first in a reaction; it determines (limits) the maximum amount of product formed. Other reactants are present in excess.
How is percentage yield calculated?
$$\%\text{ yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$$
In $\ce{N2 + 3H2 -> 2NH3}$, how many moles of $\ce{NH3}$ form from 2 mol $\ce{N2}$ and 3 mol $\ce{H2}$?
$\ce{H2}$ is limiting: $3\ \text{mol}\ \ce{H2}$ produces $2\ \text{mol}\ \ce{NH3}$ (from the $3:2$ ratio). The $\ce{N2}$ is in excess.
Define oxidation and reduction in terms of electron transfer.
Oxidation is the loss of electrons; reduction is the gain of electrons. Mnemonic: OIL RIG — Oxidation Is Loss, Reduction Is Gain.
Define oxidising agent and reducing agent.
An oxidising agent accepts electrons (and is itself reduced). A reducing agent donates electrons (and is itself oxidised).
Define oxidation and reduction in terms of oxidation number.
Oxidation is an increase in oxidation number; reduction is a decrease in oxidation number.
What is a redox (oxidation-reduction) reaction?
A reaction in which oxidation and reduction occur simultaneously, involving transfer of electrons and changes in oxidation numbers. Example: $\ce{Zn + Cu^{2+} -> Zn^{2+} + Cu}$.
State the main rules for assigning oxidation numbers.
Free element $= 0$; monatomic ion $=$ its charge; $\ce{O} = -2$ (except peroxides $-1$, $\ce{OF2}$ $+2$); $\ce{H} = +1$ (except metal hydrides $-1$); sum in a neutral molecule $= 0$; sum in a polyatomic ion $=$ its charge.
What is a disproportionation reaction? Give an example.
A redox reaction in which the same element is simultaneously oxidised and reduced. Example: $$\ce{Cl2 + 2OH- -> Cl- + ClO- + H2O}$$ where $\ce{Cl}$ goes from $0$ to both $-1$ and $+1$.
Define a neutralisation reaction and write its net ionic equation.
A reaction between an acid and a base producing salt and water. Net ionic equation for strong acid + strong base: $$\ce{H+ + OH- -> H2O}$$
What is the enthalpy of neutralisation for a strong acid and strong base, and why is it constant?
It is approximately $-57.1\ \text{kJ mol}^{-1}$. It is constant because the only reaction occurring is $\ce{H+ + OH- -> H2O}$, regardless of the specific strong acid or base used.
Define a displacement reaction and give the two main types.
A reaction in which a more reactive element displaces a less reactive one from its compound. Types: single displacement (e.g. $\ce{Fe + CuSO4 -> FeSO4 + Cu}$) and double displacement (e.g. $\ce{AgNO3 + NaCl -> AgCl + NaNO3}$).
Write an example of a metal displacing hydrogen from an acid.
$$\ce{Zn + 2HCl -> ZnCl2 + H2 ^}$$ Zinc, being more reactive than hydrogen, displaces it.
What does the reactivity series predict about displacement reactions?
A metal higher in the reactivity series can displace a metal lower in the series from its salt solution. For example, $\ce{Zn}$ displaces $\ce{Cu}$ but $\ce{Cu}$ cannot displace $\ce{Zn}$.
State Boyle's law with its mathematical expression.
At constant temperature and amount of gas, the volume of a gas is inversely proportional to its pressure: $$P \propto \frac{1}{V} \quad \Rightarrow \quad PV = \text{constant}, \quad P_1V_1 = P_2V_2$$
State Charles's law with its mathematical expression.
At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature: $$V \propto T \quad \Rightarrow \quad \frac{V}{T} = \text{constant}, \quad \frac{V_1}{T_1} = \frac{V_2}{T_2}$$
State Gay-Lussac's (pressure-temperature) law.
At constant volume, the pressure of a fixed mass of gas is directly proportional to its absolute temperature: $$\frac{P}{T} = \text{constant}, \quad \frac{P_1}{T_1} = \frac{P_2}{T_2}$$
State Avogadro's law.
Equal volumes of all gases at the same temperature and pressure contain equal numbers of molecules. Hence $V \propto n$ at constant $T$ and $P$.
Write the ideal gas equation and name each term.
$$PV = nRT$$ where $P$ = pressure, $V$ = volume, $n$ = moles, $R$ = universal gas constant, $T$ = absolute temperature.
Give the value of the universal gas constant $R$ in common units.
$R = 8.314\ \text{J K}^{-1}\text{mol}^{-1} = 0.0821\ \text{L atm K}^{-1}\text{mol}^{-1} = 2\ \text{cal K}^{-1}\text{mol}^{-1}$.
Express the ideal gas equation in terms of density and molar mass.
Since $n = \frac{m}{M}$, $$PM = \frac{m}{V}RT = dRT \quad \Rightarrow \quad d = \frac{PM}{RT}$$
State the combined gas law.
$$\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$$ combining Boyle's, Charles's, and Gay-Lussac's laws for a fixed amount of gas.
What is the absolute (Kelvin) scale of temperature and absolute zero?
The absolute scale measures temperature from absolute zero ($0\ \text{K} = -273.15\,^{\circ}\text{C}$), the temperature at which the volume/pressure of an ideal gas extrapolates to zero. Conversion: $T(\text{K}) = t(^{\circ}\text{C}) + 273.15$.
What is the compressibility factor $Z$ and its value for an ideal gas?
$$Z = \frac{PV}{nRT}$$ For an ideal gas $Z = 1$ at all conditions. Deviations ($Z \neq 1$) indicate real (non-ideal) gas behaviour.
What do $Z > 1$ and $Z < 1$ indicate about a real gas?
$Z < 1$: gas is more compressible than ideal (attractive forces dominate, common at moderate pressures). $Z > 1$: gas is less compressible than ideal (repulsive forces/molecular volume dominate, common at high pressures).
Under what conditions do real gases behave most ideally?
At low pressure and high temperature, where molecules are far apart, intermolecular forces are negligible, and molecular volume is small compared with the container volume.
Write the van der Waals equation for $n$ moles of a real gas and explain the correction terms.
$$\left(P + \frac{an^2}{V^2}\right)(V - nb) = nRT$$ The term $\frac{an^2}{V^2}$ corrects pressure for intermolecular attraction; $nb$ corrects volume for the finite size of molecules. $a$ and $b$ are van der Waals constants.
JEE Advanced Chemistry FAQ
What is in the JEE Advanced Chemistry syllabus?
JEE Advanced Chemistry is split into 37 chapters: General Topics, States of Matter: Gases and Liquids, Atomic Structure, Chemical Bonding and Molecular Structure, Chemical Thermodynamics, Chemical and Ionic Equilibrium, Electrochemistry, Chemical Kinetics, Solid State, Solutions, Surface Chemistry and Classification of Elements and Periodicity in Properties, and 25 more. Together they contain 201 topics and 232 sub-topics.
How many chapters are in JEE Advanced Chemistry?
37 chapters, containing 201 topics and 232 sub-topics. The largest chapter is Basic Principles of Organic Chemistry, with 13 topics.
Are there flashcards for JEE Advanced Chemistry?
Yes — a 50-card Chemistry deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.