JIPMER Entrance 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 JIPMER Entrance, not a summary of it.

1. 1

   Physical Chemistry

   7 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and stoichiometry
     • Empirical and molecular formulae
   • Atomic Structure
     • Quantum numbers and orbitals
     • Electronic configuration and Aufbau principle
   • States of Matter: Gases and Liquids
   • Chemical and Ionic Equilibrium
     • Le Chatelier's principle and Kc/Kp
     • pH, buffers and solubility product
   • Thermodynamics and Thermochemistry
   • Electrochemistry
     • Galvanic cells and Nernst equation
     • Electrolysis and conductance
   • Chemical Kinetics and Solutions
2. 2

   Inorganic Chemistry

   6 topics

   • Periodic Table and Periodicity
     • Periodic trends in properties
     • Modern periodic law
   • Chemical Bonding and Molecular Structure
     • Ionic, covalent and coordinate bonding
     • VSEPR theory, hybridization and MO theory
   • s-Block and p-Block Elements
   • d- and f-Block Elements and Coordination Compounds
   • Metallurgy and Principles of Isolation of Elements
   • Hydrogen, Water and Environmental Chemistry
3. 3

   Organic Chemistry

   7 topics

   • Basic Concepts and Isomerism
     • IUPAC nomenclature
     • Structural and stereoisomerism
   • General Organic Chemistry
     • Inductive, resonance and hyperconjugation effects
     • Reaction mechanisms and intermediates
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Haloalkanes, Alcohols, Phenols and Ethers
   • Aldehydes, Ketones and Carboxylic Acids
   • Amines and Nitrogen Compounds
   • Biomolecules and Polymers
     • Carbohydrates, proteins and nucleic acids
     • Synthetic and natural polymers

Chemistry flashcards for JIPMER Entrance

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

1. State Avogadro's number and what one mole represents.

   Avogadro's number is 6.022 x 10^23. One mole is the amount of a substance that contains exactly 6.022 x 10^23 elementary entities (atoms, molecules, ions, etc.) and equals the substance's molar mass in grams.

2. What is the difference between empirical formula and molecular formula?

   The empirical formula gives the simplest whole-number ratio of atoms of each element in a compound (e.g. CH for benzene). The molecular formula gives the actual number of atoms of each element in a molecule (e.g. C6H6 for benzene). Molecular formula = n x empirical formula.

3. 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 simple whole-number ratio. Example: in CO and CO2, masses of oxygen combining with 12 g carbon are 16 g and 32 g, a ratio of 1:2.

4. How is molarity defined and what is its formula?

   Molarity (M) is the number of moles of solute dissolved per litre of solution. M = moles of solute / volume of solution in litres. It is temperature-dependent because volume changes with temperature.

5. What are the four quantum numbers and what does each describe?

   Principal (n) gives shell/energy and size; Azimuthal (l) gives subshell/shape (0=s,1=p,2=d,3=f); Magnetic (m) gives orbital orientation (ranges -l to +l); Spin (s) gives the electron's spin direction (+1/2 or -1/2).

6. State the Heisenberg uncertainty principle.

   It is impossible to determine simultaneously, with absolute accuracy, both the position and the momentum of a microscopic particle such as an electron. Mathematically, delta-x . delta-p >= h/4pi.

7. State Aufbau principle, Pauli exclusion principle, and Hund's rule.

   Aufbau: electrons fill orbitals in order of increasing energy. Pauli exclusion: no two electrons in an atom can have all four quantum numbers identical (an orbital holds max 2 electrons of opposite spin). Hund's rule: electrons occupy degenerate orbitals singly with parallel spins before pairing.

8. What is the de Broglie equation relating wavelength to momentum?

   lambda = h / (mv) = h / p, where lambda is the wavelength, h is Planck's constant, m is mass and v is velocity. It expresses the dual wave-particle nature of matter.

9. State the ideal gas equation and identify each term.

   PV = nRT, where P = pressure, V = volume, n = number of moles, R = universal gas constant (8.314 J/mol K), and T = absolute temperature in kelvin.

10. State Boyle's law and Charles's law.

    Boyle's law: at constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure (PV = constant). Charles's law: at constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature (V/T = constant).

11. What are the key postulates of the kinetic theory of gases?

    Gas molecules are tiny particles in constant random motion with negligible volume; there are no intermolecular forces; collisions are perfectly elastic; average kinetic energy is directly proportional to absolute temperature.

12. Define vapour pressure and how it relates to boiling point.

    Vapour pressure is the pressure exerted by a vapour in equilibrium with its liquid at a given temperature. A liquid boils when its vapour pressure equals the external (atmospheric) pressure; lower external pressure means a lower boiling point.

13. State Le Chatelier's principle.

    If a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the equilibrium shifts in the direction that tends to counteract (oppose) the imposed change.

14. What is the relationship between Kp and Kc?

    Kp = Kc (RT)^(delta-n), where delta-n is the change in the number of moles of gas (moles of gaseous products minus moles of gaseous reactants), R is the gas constant and T is the absolute temperature.

15. Define pH and pOH and state their relationship at 25 degrees C.

    pH = -log[H+] and pOH = -log[OH-]. At 25 degrees C, pH + pOH = 14, since Kw = [H+][OH-] = 1.0 x 10^-14.

16. What is the common ion effect?

    The suppression of the ionisation of a weak electrolyte by adding a strong electrolyte that has an ion in common with it. For example, adding NaCl decreases the solubility/ionisation of a sparingly soluble chloride or a weak acid sharing that ion.

17. State the first law of thermodynamics and its equation.

    Energy can neither be created nor destroyed, only converted from one form to another. delta-U = q + w, where delta-U is the change in internal energy, q is heat added to the system, and w is work done on the system.

18. What is Hess's law of constant heat summation?

    The total enthalpy change for a reaction is the same whether it occurs in one step or several steps, depending only on the initial and final states and not on the path taken.

19. Define enthalpy of formation and enthalpy of combustion.

    Enthalpy of formation is the heat change when one mole of a compound forms from its elements in their standard states. Enthalpy of combustion is the heat released when one mole of a substance is completely burned in excess oxygen.

20. How do the signs of delta-G predict reaction spontaneity?

    delta-G < 0: reaction is spontaneous; delta-G = 0: system is at equilibrium; delta-G > 0: reaction is non-spontaneous. delta-G = delta-H - T delta-S.

21. What is the difference between oxidation and reduction in terms of electrons?

    Oxidation is the loss of electrons (increase in oxidation number); reduction is the gain of electrons (decrease in oxidation number). Remember OIL RIG: Oxidation Is Loss, Reduction Is Gain.

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