Chemistry Grade 11 (Old Course) Guess Paper 2025

Chemistry Guess Paper HSSC-I 2025 (Old Course)

Are you preparing for the FBISE Chemistry HSSC-I (1st Year) exams in 2025? This carefully curated guess paper highlights the most important exercises and questions from the syllabus to help you focus on key topics and score better.

Important Questions & Topics for FBISE Exams 2025

GUESS PAPER FOR CLASS XI CHEMISTRY

Chapter 1

• Define mole, Avogadro number, limiting reactant, theoretical yield
• Actual yield is always less than theoretical yield
• Example: (1.3, 1.5, 1.7, 1.8, 1.9, 1.10)
• Exercise problems: 2(b), 5(b), 6(b)

Chapter 2

• Write down postulates of Planck’s quantum theory
• Write defects in Bohr’s atomic theory
• Explain Hydrogen spectrum
• Rules for distribution of electrons
• Example: (2.6, 2.7)

Long Questions:

• Derive the equation for the radius of n^th orbit of hydrogen atom
• Explain Quantum numbers

Chapter 3

• Predict the geometries of molecules on the basis of VSEPR theory (a) PH₃, (b) SO₂, (c) PCl₅
• M.O.T is superior to VBT. Justify
• Difference between B, B^-, and O^-. Which one is bigger in size and why?
• Which element has the highest I.E and why?
• Difference between pi bond and sigma bond

Long Questions:

• Explain the polarity of molecules on the basis of electronegativity
• Identify polar covalent molecules from: CH₄, BF₃, H₂O, C₂H₄, C₂H₂

Chapter 4

• State and explain the postulates of Dalton’s Law of Partial Pressure
• Boyle’s law and its derivation
• Charles’s law and its derivation
• Deviation of real gases from ideal behaviour
• Derive Van der Waals equation for real gases
• Derivation of critical form of Charle’s law

Exercise Problems:

• 4.9, 4.10
• Self Check Exercises: 4.2, 4.7
• Exercise Numericals: 4.1, 4.6, 4.16

Chapter 5

• Identify the intermolecular forces in:
  • (1) CH₃OH
  • (2) CH₄
  • (3) CH₃F
  • (4) HCl(g)
  • (5) H₂
  • (6) Cl₂
  • (7) CH₃COOH
• Why is the boiling point of water much higher than the other hydrides of group VI?
• Properties and uses of group VII
• Properties and uses of liquid crystals

Long Question:

• Discuss London dispersion forces and the factors affecting it

Chapter 6

• What type of crystal will each of the following substances form in solid state?
  • (a) NaCl
  • (b) SiO₂
  • (c) Diamond
  • (d) CO₂
• Explain the allotropes of metal and transition elements
• Write the key example with features of amorphous solids
• Explain the structure of NaCl on the basis of unit cell

Long Questions:

• Difference between HCP and CCP
• Write one ionic solid and one covalent solid

Chapter 7

• Enthalpy of formation
• Examples and numericals:
  • ΔH = ΔU + ΔnRT
  • Q = mcΔT
  • Q = m × L
• Effect of temperature and pressure on equilibrium

Long Questions:

• Industrial Applications of Le Chatelier’s Principle
• Write one Common Ion Effect and its two applications

Chapter 8

• What is relationship between Ka and Kb
• Write expressions for the ionic product of water, Kw, and pH, pK_a
• Examples: 8.1, 8.7, 8.9, 8.10
• Self Check Exercise 8.1
• Exercise Q 2(b)

Long Question:

• What is hydrolysis? Discuss in detail the behavior of each of the following salts in aqueous solution:
  • KClO₃
  • NH₄Cl
  • NaNO₂
  • CH₃COONH₄
• What are Buffer solutions? Give the applications of buffers.

Chapter 9

• (i) Differentiate between instantaneous and average rate of reaction
• (ii) Define the rate constant of reaction with one unit and formula
• (iii) Define the term rate constant for different orders of reactions
• (iv) Collision theory of reaction and Maxwell Boltzmann distribution
• Self Check Exercise 9.3 & 9.4

Long Question:

• Explain collision theory

Chapter 10

• Phenol water system
• Define colligative properties. Give its three statements:
  • Molality, Molarity and Mole fraction
• Explain boiling point elevation and freezing point depression
• Explain what happens when the solute is added to a pure solvent with suitable examples
• Reverse osmosis

Numericals:

• Sample problems 10.2, 10.7, 10.9, 10.10
• Self Check Exercise 10.8

Long Question:

• In an experiment the equation is boiling point elevation of a solution is proportional to molality. Prove that the equation of boiling point elevation point is a colligative property and describe the colligative properties of non-volatile and non-electrolyte solution

Chapter 11

• Define the following:
  • (i) Enthalpy
  • (ii) State function
  • (iii) First law of thermodynamics
  • (iv) Standard enthalpy with at least one example for each part
• Sample problems: 11.1, 11.3, 11.6

Long Questions:

• State Hess's Law with example
• Write a note on Born-Haber Cycle for NaCl

Chapter 12

• What is standard hydrogen electrode? Give its use in determining electrode potential
• Write the E° values of the following set:
  • Ag⁺ + e^- → Ag E° = +0.80 V
  • NO₃^- + H⁺ + e^- → NO + H₂O E° = +0.96 V
  • H₂ → 2H⁺ + 2e^- E° = 0.00 V
• Short Questions: 12.5, 12.6
• Examples: 12.6, 12.7, 12.8, 12.9
• Self Check: 12.10

Long Question:

• What is electrochemical cell? Explain oxidation and reduction in terms of loss and gain of electrons
• Write a note on lead storage batteries