SRMJEEE Chemistry Syllabus

Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry in SRMJEEE, not a summary of it.

1. 1

   Physical Chemistry I

   4 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and stoichiometry
     • Empirical and molecular formulae
     • Concentration terms and limiting reagent
   • Atomic Structure
     • Bohr model and quantum numbers
     • Dual nature and de Broglie equation
     • Aufbau, Pauli and Hund's rules
   • States of Matter
     • Gas laws and ideal gas equation
     • Kinetic theory and real gases
     • Liquid state properties
   • Chemical Bonding and Molecular Structure
     • Ionic and covalent bonding
     • VSEPR theory and hybridisation
     • Molecular orbital theory
2. 2

   Physical Chemistry II

   5 topics

   • Thermodynamics
     • First law, enthalpy and Hess's law
     • Entropy, free energy and spontaneity
   • Chemical and Ionic Equilibrium
     • Law of mass action and Kc, Kp
     • Le Chatelier's principle
     • pH, buffers and solubility product
   • Chemical Kinetics
     • Rate laws and order of reaction
     • Arrhenius equation and activation energy
   • Electrochemistry
     • Electrochemical cells and EMF
     • Nernst equation and conductance
     • Electrolysis and Faraday's laws
   • Solutions and Surface Chemistry
     • Colligative properties
     • Adsorption and catalysis
     • Colloids and emulsions
3. 3

   Inorganic Chemistry

   5 topics

   • Periodic Classification
     • Periodic trends in properties
     • Ionisation enthalpy and electronegativity
   • s-Block and p-Block Elements
     • Alkali and alkaline earth metals
     • Group 13 to 18 trends and compounds
   • d- and f-Block Elements
     • Transition metals and properties
     • Lanthanides and actinides
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in complexes
     • Valence bond and crystal field theory
   • Metallurgy and Hydrogen
     • Principles of metallurgy
     • Hydrogen and its compounds
4. 4

   Organic Chemistry I

   4 topics

   • Basic Concepts of Organic Chemistry
     • IUPAC nomenclature
     • Inductive, resonance and hyperconjugation
     • Reaction intermediates and mechanisms
   • Isomerism
     • Structural isomerism
     • Stereoisomerism and chirality
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Haloalkanes and Haloarenes
     • SN1 and SN2 mechanisms
     • Elimination reactions
5. 5

   Organic Chemistry II

   4 topics

   • Alcohols, Phenols and Ethers
     • Preparation and reactions of alcohols
     • Acidity of phenols
   • Aldehydes, Ketones and Carboxylic Acids
     • Nucleophilic addition reactions
     • Aldol and Cannizzaro reactions
     • Acidity and derivatives of acids
   • Nitrogen Compounds
     • Amines and their basicity
     • Diazonium salts
   • Biomolecules and Polymers
     • Carbohydrates, proteins and nucleic acids
     • Classification of polymers
     • Chemistry in everyday life

Chemistry flashcards for SRMJEEE

21 of 51 cards from the Chemistry deck — real questions with worked answers.

1. State the law of conservation of mass and name the scientist who proposed it.

   Mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products. It was proposed by Antoine Lavoisier.

2. State the law of multiple proportions with 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 a ratio of small whole numbers. Example: in $\ce{CO}$ and $\ce{CO2}$, the masses of oxygen combining with a fixed 12 g of carbon are in the ratio $16:32 = 1:2$.

3. Define the mole and give the value of Avogadro's number.

   A mole is the amount of substance containing as many elementary entities as there are atoms in 12 g of $\ce{^{12}C}$. Avogadro's number is $N_A = 6.022 \times 10^{23}\ \text{mol}^{-1}$.

4. What is the molar volume of an ideal gas at STP, and what conditions does STP define?

   At STP ($273.15\ \text{K}$ and $1\ \text{bar}$) the molar volume is approximately $22.7\ \text{L mol}^{-1}$ (about $22.4\ \text{L mol}^{-1}$ at $1\ \text{atm}$).

5. Give the formula relating number of moles to mass and to number of particles.

   $$n = \frac{m}{M} = \frac{N}{N_A}$$ where $m$ is mass, $M$ is molar mass, $N$ is number of particles and $N_A$ is Avogadro's number.

6. Distinguish between empirical formula and molecular formula.

   The empirical formula gives the simplest whole-number ratio of atoms of each element in a compound; the molecular formula gives the actual number of atoms of each element in a molecule. They are related by $\text{Molecular formula} = n \times \text{Empirical formula}$ where $n = \frac{\text{molar mass}}{\text{empirical formula mass}}$.

7. How is the empirical formula of a compound determined from percentage composition?

   Divide each element's percentage by its atomic mass to get the mole ratio, then divide all values by the smallest to obtain the simplest whole-number ratio, multiplying up if needed to clear fractions.

8. Define molarity and write its formula.

   Molarity is the number of moles of solute per litre of solution: $$M = \frac{n_{\text{solute}}}{V_{\text{solution (L)}}}$$ Its unit is $\text{mol L}^{-1}$.

9. Define molality and state why it is temperature-independent.

   Molality is the number of moles of solute per kilogram of solvent: $$m = \frac{n_{\text{solute}}}{\text{mass of solvent (kg)}}$$ It is temperature-independent because it depends on mass, not volume, and mass does not change with temperature.

10. What is the limiting reagent in a reaction?

    The limiting reagent is the reactant that is completely consumed first, thereby limiting the amount of product formed; the other reactants are present in excess.

11. Define mole fraction and state the sum of mole fractions in a mixture.

    The mole fraction of a component is $x_i = \frac{n_i}{n_{\text{total}}}$. For any mixture, $\sum_i x_i = 1$.

12. State the postulates of Dalton's atomic theory (key points).

    Matter consists of indivisible atoms; atoms of a given element are identical in mass and properties; compounds form when atoms combine in fixed whole-number ratios; and atoms are neither created nor destroyed in chemical reactions, only rearranged.

13. Give the relationship between wavelength, frequency and speed of electromagnetic radiation, and the energy of a photon.

    $c = \nu\lambda$ and the photon energy is $E = h\nu = \frac{hc}{\lambda}$, where $h = 6.626 \times 10^{-34}\ \text{J s}$ is Planck's constant.

14. Write the expression for the energy of the nth orbit of a hydrogen atom in the Bohr model.

    $$E_n = -\frac{2.18 \times 10^{-18}}{n^{2}}\ \text{J} = -\frac{13.6}{n^{2}}\ \text{eV}$$ where $n$ is the principal quantum number.

15. Write the Rydberg formula for the wavenumber of spectral lines in the hydrogen spectrum.

    $$\bar{\nu} = \frac{1}{\lambda} = R_H\left(\frac{1}{n_1^{2}} - \frac{1}{n_2^{2}}\right)$$ where $R_H = 1.097 \times 10^{7}\ \text{m}^{-1}$ and $n_2 > n_1$.

16. State the radius of the nth Bohr orbit of hydrogen.

    $$r_n = 0.529 \times n^{2}\ \text{Å} = 52.9 \times n^{2}\ \text{pm}$$ The first orbit ($n=1$) radius is $0.529\ \text{Å}$, the Bohr radius.

17. Name the four quantum numbers and what each describes.

    Principal quantum number $n$ (energy/shell size); azimuthal quantum number $l$ (subshell/orbital shape, $0$ to $n-1$); magnetic quantum number $m_l$ (orbital orientation, $-l$ to $+l$); and spin quantum number $m_s$ (electron spin, $+\tfrac{1}{2}$ or $-\tfrac{1}{2}$).

18. State the de Broglie equation and its significance.

    $$\lambda = \frac{h}{p} = \frac{h}{mv}$$ It expresses the dual (wave-particle) nature of matter, associating a wavelength $\lambda$ with any moving particle of momentum $p$.

19. State Heisenberg's uncertainty principle.

    It is impossible to determine simultaneously, with arbitrary precision, the exact position and momentum of a particle: $$\Delta x \cdot \Delta p \geq \frac{h}{4\pi}$$

20. State the Aufbau principle.

    In the ground state, electrons fill atomic orbitals in order of increasing energy, occupying the lowest-energy available orbital first. The order follows the $(n+l)$ rule.

21. State Pauli's exclusion principle.

    No two electrons in an atom can have the same set of all four quantum numbers; an orbital can hold at most two electrons with opposite spins.

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