FBISE Examinations Chemistry (HSSC) Syllabus

Chemistry (HSSC) syllabus — full chapter and topic list

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

1. 1

   Basic Concepts

   3 topics

   • Atomic Mass and Mole Concept
   • Empirical and Molecular Formula
   • Stoichiometry
2. 2

   States of Matter

   3 topics

   • Gas Laws
   • Kinetic Molecular Theory
   • Liquids and Solids
3. 3

   Atomic Structure

   3 topics

   • Discharge Tube Experiments
   • Bohr's Model and Spectra
   • Quantum Numbers and Orbitals
4. 4

   Chemical Bonding

   3 topics

   • Ionic and Covalent Bonds
   • VSEPR Theory and Molecular Geometry
   • Hybridization
5. 5

   Thermochemistry

   3 topics

   • Enthalpy and Internal Energy
   • Hess's Law
   • Born-Haber Cycle
6. 6

   Chemical Equilibrium

   3 topics

   • Law of Mass Action
   • Le Chatelier's Principle
   • Ionic Product and pH
7. 7

   Reaction Kinetics

   3 topics

   • Rate of Reaction
   • Order of Reaction
   • Catalysis
8. 8

   Electrochemistry

   3 topics

   • Oxidation and Reduction
   • Galvanic and Electrolytic Cells
   • Electrode Potential
9. 9

   Organic Chemistry Fundamentals

   3 topics

   • Hydrocarbons
   • Functional Groups
   • Isomerism
10. 10

    Macromolecules and Industrial Chemistry

    3 topics

    • Polymers
    • Carbohydrates and Proteins
    • Environmental Chemistry

Chemistry (HSSC) flashcards for FBISE Examinations

25 of 52 cards from the Chemistry (HSSC) deck — real questions with worked answers.

1. Define one mole and state the value of Avogadro's number.

   One mole is the amount of a substance containing as many particles as there are atoms in 12 g of carbon-12. Avogadro's number = 6.022 x 10^23 particles per mole.

2. What is the relationship between number of moles, mass, and molar mass?

   Number of moles (n) = mass (m) / molar mass (M).

3. How do you calculate the number of particles from the number of moles?

   Number of particles = number of moles x Avogadro's number (6.022 x 10^23).

4. Define relative atomic mass.

   The relative atomic mass is the average mass of one atom of an element compared to 1/12 of the mass of one carbon-12 atom. It is a dimensionless quantity.

5. What volume does one mole of any ideal gas occupy at STP?

   22.414 dm^3 (22.4 litres) at standard temperature and pressure (0 degrees Celsius and 1 atm).

6. How is the molar mass of a gas determined from its density at STP?

   Molar mass = density (g/dm^3) x 22.4 dm^3/mol, using the molar volume of a gas at STP.

7. Define empirical formula.

   The empirical formula is the simplest whole-number ratio of atoms of each element present in a compound.

8. Define molecular formula.

   The molecular formula gives the actual number of atoms of each element present in one molecule of a compound.

9. What is the relationship between molecular formula and empirical formula?

   Molecular formula = n x (empirical formula), where n = molar mass / empirical formula mass.

10. List the steps to determine an empirical formula from percentage composition.

    1) Take the percentage as grams. 2) Divide each by its atomic mass to get moles. 3) Divide all mole values by the smallest. 4) Convert to the simplest whole-number ratio.

11. Define a limiting reactant in stoichiometry.

    The limiting reactant is the reactant that is completely consumed first in a reaction and therefore determines the maximum amount of product formed.

12. What is the difference between theoretical yield and actual yield?

    Theoretical yield is the maximum product calculated from stoichiometry; actual yield is the amount actually obtained experimentally, which is usually less.

13. Write the formula for percentage yield.

    Percentage yield = (actual yield / theoretical yield) x 100.

14. Define stoichiometry.

    Stoichiometry is the quantitative study of the relationships between the amounts of reactants and products in a balanced chemical reaction.

15. State Boyle's Law and its mathematical form.

    At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure. Mathematically, PV = constant, or P1V1 = P2V2.

16. State Charles's Law and its mathematical form.

    At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute (Kelvin) temperature. V/T = constant, or V1/T1 = V2/T2.

17. State Avogadro's Law.

    Equal volumes of all gases under the same conditions of temperature and pressure contain equal numbers of molecules.

18. Write the ideal gas equation and define each term.

    PV = nRT, where P = pressure, V = volume, n = number of moles, R = general gas constant, and T = absolute temperature.

19. State the value of the general gas constant R in SI units.

    R = 8.314 J K^-1 mol^-1 (equivalently 0.0821 dm^3 atm K^-1 mol^-1).

20. State Dalton's Law of Partial Pressures.

    The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases: P_total = P1 + P2 + P3 + ...

21. State Graham's Law of Diffusion.

    At constant temperature and pressure, the rate of diffusion of a gas is inversely proportional to the square root of its density (or molar mass): rate is proportional to 1/sqrt(M).

22. List the main postulates of the Kinetic Molecular Theory of gases.

    1) Gases consist of tiny particles in constant random motion. 2) The volume of the particles is negligible compared to total volume. 3) There are no attractive forces between particles. 4) Collisions are perfectly elastic. 5) Average kinetic energy is proportional to absolute temperature.

23. According to kinetic theory, what is the average kinetic energy of gas molecules proportional to?

    The average kinetic energy of gas molecules is directly proportional to the absolute (Kelvin) temperature.

24. Under what conditions do real gases deviate most from ideal behaviour?

    Real gases deviate most from ideal behaviour at high pressure and low temperature, where molecular volume and intermolecular forces become significant.

25. Define evaporation.

    Evaporation is the process by which molecules at the surface of a liquid escape into the vapour phase below the boiling point.

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