FSc Pre-Medical 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 FSc Pre-Medical, not a summary of it.

1. 1

   Basic Concepts of Chemistry

   4 topics

   • Atom, Molecule and Ion
   • Relative Atomic Mass and Isotopes
   • The Mole Concept and Avogadro's Number
   • Stoichiometry
2. 2

   Atomic Structure

   4 topics

   • Subatomic Particles and Discovery
   • Bohr's Atomic Model
   • Quantum Numbers and Orbitals
   • Electronic Configuration
3. 3

   Gases

   4 topics

   • Gas Laws
   • Ideal Gas Equation
   • Kinetic Molecular Theory
   • Deviation of Real Gases
4. 4

   Liquids and Solids

   3 topics

   • Intermolecular Forces
   • Properties of Liquids
   • Crystalline and Amorphous Solids
5. 5

   Chemical Bonding

   4 topics

   • Ionic and Covalent Bonds
   • VSEPR Theory and Molecular Geometry
   • Hybridization
   • Bond Energy and Polarity
6. 6

   Thermochemistry

   3 topics

   • System, Surroundings and Enthalpy
   • Hess's Law
   • Born-Haber Cycle
7. 7

   Chemical Equilibrium

   3 topics

   • Reversible Reactions and Equilibrium Constant
   • Le Chatelier's Principle
   • Solubility Product and Ionic Equilibria
8. 8

   Reaction Kinetics

   3 topics

   • Rate of Reaction and Rate Law
   • Order of Reaction
   • Factors Affecting Rate
9. 9

   Electrochemistry

   3 topics

   • Oxidation and Reduction
   • Galvanic and Electrolytic Cells
   • Electrode Potential
10. 10

    Periodic Classification and s/p Block Elements

    3 topics

    • Periodic Table and Periodicity
    • Group IA and IIA Elements
    • Group IVA to VIIA Elements
11. 11

    Fundamentals of Organic Chemistry

    4 topics

    • Classification of Organic Compounds
    • Functional Groups and Nomenclature
    • Isomerism
    • Hydrocarbons
12. 12

    Functional Groups and Biochemistry

    4 topics

    • Alcohols and Phenols
    • Aldehydes and Ketones
    • Carboxylic Acids and Derivatives
    • Carbohydrates, Proteins and Lipids

Chemistry flashcards for FSc Pre-Medical

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

1. What is an atom?

   The smallest particle of an element that can take part in a chemical reaction; it may or may not exist independently.

2. What is a molecule?

   The smallest particle of an element or compound that can exist independently and shows all the properties of that substance.

3. What is an ion?

   An atom or group of atoms carrying a net electrical charge, formed by the loss or gain of electrons. A cation is positive (loss of electrons); an anion is negative (gain of electrons).

4. Differentiate between a molecular ion and a free radical.

   A molecular ion is a charged species produced when a molecule loses or gains electron(s) (e.g. CH4+). A free radical is a neutral species with an unpaired electron (e.g. CH3•), produced by homolytic bond breaking.

5. What is relative atomic mass?

   The average mass of the atoms of an element compared to 1/12th the mass of one atom of carbon-12. It is a ratio and has no units.

6. What are isotopes?

   Atoms of the same element having the same atomic number (same number of protons) but different mass numbers (different numbers of neutrons).

7. Give the three isotopes of hydrogen and their mass numbers.

   Protium (¹H, mass 1), Deuterium (²H, mass 2), and Tritium (³H, mass 3).

8. How is the average atomic mass of an element calculated from isotopic data?

   Average atomic mass = Σ(isotopic mass × fractional abundance), i.e. the weighted mean of the masses of all naturally occurring isotopes by their relative abundances.

9. Which instrument is used to determine relative atomic masses and isotopic abundances?

   The mass spectrometer.

10. Define the mole.

    The amount of a substance that contains as many elementary particles (atoms, molecules, ions) as there are atoms in exactly 12 g of carbon-12; this number is Avogadro's number.

11. What is the value of Avogadro's number?

    6.022 × 10²³ particles per mole.

12. What is molar mass?

    The mass in grams of one mole of a substance, numerically equal to its atomic/molecular/formula mass; its unit is g/mol.

13. How do you calculate the number of moles from a given mass?

    Number of moles = mass of substance (g) ÷ molar mass (g/mol).

14. How do you find the number of particles from the number of moles?

    Number of particles = number of moles × 6.022 × 10²³ (Avogadro's number).

15. What is the molar volume of an ideal gas at STP?

    22.414 dm³ (22.414 litres) per mole at standard temperature and pressure (273.15 K and 1 atm).

16. Define stoichiometry.

    The branch of chemistry that deals with the quantitative relationships between reactants and products in a balanced chemical equation.

17. What is a limiting reactant?

    The reactant that is completely consumed first in a reaction, thereby limiting the amount of product formed; the other reactant(s) are in excess.

18. Define theoretical yield and actual yield.

    Theoretical yield is the maximum amount of product calculated from the balanced equation; actual yield is the amount actually obtained experimentally.

19. How is percentage yield calculated?

    Percentage yield = (actual yield ÷ theoretical yield) × 100.

20. State the assumptions made for stoichiometric (mole) calculations.

    All reactants are completely converted to products, no side reactions occur, and reactants/products are pure; the reaction follows the balanced equation.

21. Who discovered the electron and by what experiment?

    J. J. Thomson discovered the electron through experiments on the discharge of electricity through gases (cathode rays in a discharge tube).

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