Jkbose 11th Class Chemistry Guess Paper 2026 Bi-Annual Private Exam
Q1. N and O combine with H to form NH₃ and H₂O and they combine with each other to form NO₂. Which law is illustrated? Explain briefly.
Q2. What are Quantum Numbers? Explain the significance of any two quantum numbers.
Q3. State Modern Periodic Law. What are the main features of the long form of the periodic table?
Q4. How will you prepare the following compounds from benzene? (a) Chlorobenzene (b) Nitrobenzene (c) Benzene sulphonic acid (d) Toluene (e) Benzene hexachloride
Q5. Give the mechanism of electrophilic substitution in benzene.
Q6. Write notes on:
(a) Markownikoff's rule (b) Peroxide effect (c) Friedel-Crafts reaction
Q7. What is Ozonolysis? How can it be used to determine the position of double bond in an unknown alkene?
Q8. Write short notes on: (a) Markovnikoff's rule (b) Friedel-Crafts acylation (c) Benzene resonance
Q9. What is hybridisation? Explain sp² hybridisation with an example.
Q10. State first law of thermodynamics and give a mathematical expression for it. Mention two examples to support the law.
Q11. Explain term enthalpy. How does it differ from internal energy?
Q12. What are strong and weak electrolytes? Derive an expression for the calculation of the degree of ionisation of a weak electrolyte.
Q13. H₂S acts only as reductant whereas SO₂ acts as both oxidant and reductant. Why?
Q14. Discuss various types of organic reactions (any three) with examples.
Q15. State and explain Heisenberg's uncertainty principle.
Q16. Define an atomic orbital. Discuss the shapes of s, p and d orbitals.
Q17. Define Molecular Mass. What is the relation between vapour density and molecular mass of a gas?
Q18. In how many blocks have the elements of long form periodic table been divided? Name them.
Q19. Draw the shapes of XeF₂ and SF₆ on the basis of VSEPR theory.
Q20. What is an adiabatic process?
Q21. Define pH. What is the pH of a solution whose [H₃O⁺] = 2×10⁻⁵ M?
Q22. What do you mean by Buffer solution? Give one example.
Q23. Define Functional Group. Write functional groups of alcohols, aldehydes, ketones and carboxylic acids.
Q24. What are Conformations? Draw the sawhorse projection of ethane.
Q25. Complete the following reactions.
Q26. Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% oxygen by mass. (Atomic mass of Fe = 56 and O = 16)
Q27. Define an atomic orbital. Differentiate between orbit and orbital.
Q28. Account for the following: (a) Ionization enthalpy of nitrogen is more than oxygen. (b) Electron gain enthalpy of fluorine is lesser than chlorine.
Q29. What are Quantum Numbers? Briefly explain the significance of each quantum number.
Q30. Write the main postulates of Bohr's theory and what are its limitations?
Q31. How this model helped in calculating the energy of an electron in different energy levels of hydrogen atom?
Q32. What are Carbocations and Carbanions? How are they generated?
Q33. Explain the relative stability of alkyl carbocations and carbanions.
Q34. Draw the molecular orbital diagram for O₂ molecule. Write its molecular orbital electronic configuration and predict its magnetic behaviour.
Q35. State first law of Thermodynamics. Derive its mathematical relation.
Q36. Define entropy and free energy. How are they related to each other?
Q37. (a) Define oxidation and reduction on the basis of electron transfer concept. Give example in each case. (b) In the reactions given below, identify the species undergoing oxidation and reduction.
Q38. State Le-Chatelier's principle. Apply this principle on the following reaction in terms of concentration, temperature and pressure to obtain maximum yield of ammonia.
Q39. Give a brief description of the principles of the following techniques taking an example in each case: (a) Crystallisation (b) Distillation (c) Chromatography
Q40. Difference between empirical and molecular formula.
Q41. State law of multiple proportion and reciprocal proportion.
Q42. What is limiting reagent?
Q43. Calculation of number of moles, molecules and atoms.
Q44. Calculation of molecular formula from percentage composition.
Q45. Law of chemical combination.
Q46. Describe Rutherford's model and its limitations.
Q47. Bohr's atomic model and its limitations.
Q48. De-Broglie's equation and its significance.
Q49. Heisenberg's Uncertainty principle and its significance.
Q50. Quantum numbers with significance of each quantum number.
Q51. Atomic orbitals and shapes of s, p and d orbitals.
Q52. (a) Aufbau’s principle (b) Pauli’s exclusion principle (c) Hund’s Rule
Q53. Exceptional electronic configuration.
Q54. What is ionisation enthalpy? Why does it increase across a period and decrease down a group?
Q55. Periodic trends in properties of elements: (a) Electron gain enthalpy (b) Atomic and ionic radii (c) Electronegativity
Q56. Periodicity and its cause.
Q57. What are entropy and free energy? How are they related?
Q58. What are intensive and extensive properties? Define state function with examples.
Q59. Hess’s law of constant heat summation.
Q60. Heat capacity, specific heat capacity and molar heat capacity.
Q61. Postulates of VSEPR theory.
Q62. Molecular orbital energy level diagram of O₂, N₂ etc.
Q63. Discuss hybridisation in detail.
Q64. Postulates of Valence Bond Theory (VBT).
Q65. Features of Molecular Orbital Theory (MOT).
Q66. Common ion effect with example.
Q67. Buffer solutions and its types with example.
Q68. Law of mass action in detail.
Q69. Le-Chatelier’s principle and factors affecting equilibrium.
Q70. pH calculations.
Q71. Balancing of redox reactions using: (a) Oxidation number method (b) Half reaction method
Q72. Oxidation number and its calculation.
Q73. Define oxidation, reduction and redox reaction with examples.
Q74. Homolytic and heterolytic fission of covalent bond with examples.
Q75. Free radicals, carbocations and carbanions – definition and generation.
Q76. Inductive effect, electromeric effect, resonance effect and hyperconjugation effect.
Q77. Difference between electrophiles and nucleophiles with suitable examples.
Q78. Role of electrophiles and nucleophiles in chemical reactions.
Q79. What are conformations? Draw Newman and Sawhorse projection of ethane.
Q80. Electrophilic substitution reaction of benzene.
Q81. Define pyrolysis with example.
Q82. Chemical properties of alkenes: (a) Electrophilic addition (Markovnikov’s rule) (b) Ozonolysis of alkenes
Q83. Methods of preparation of alkenes and alkynes.
Q84. Friedel–Crafts alkylation and acylation reactions.
Q85. Write IUPAC names of the following compounds: (a) CH₃-C(CH₃)₂-CH₂-CH₃ (b) CH₃-CH(CH₃)-CH=CH₂ (c) CH₃-CH(CH₃)-CH₂-CH₂-Cl (d) CH₃-C(CH₃)₂-CH₂-CH(OH)-CH₃ (e) CH₃-CH₂-CH-C≡N
Q86. State and explain law of conservation of Mass.
Q87. Define Pauli exclusion principle. Why is it called exclusion principle?
Q88. Define the term Ionization enthalpy. How does it vary along a period and along a group?
Q89. Define Hybridisation. Describe the formation of Sp³, Sp² and Sp hybrid orbitals of carbon atom. Give example of each.
