Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. State Heisenberg’s uncertainty principle: E = hv Δx · Δp ≥ h/4π ΔE · Δt = h v = λf None Hint 2. Vulcanization of rubber produces: a thermosetting polymer a plasticizer an elastomer a thermoplastic polymer None Hint 3. Why is the shape of ammonia molecule trigonal pyramidal? Because of linear arrangement of atoms. Due to repulsion between lone pair electrons. Due to the presence of three bonded pairs only. Because of double bonds between nitrogen and hydrogen. None Hint 4. State Heisenberg’s uncertainty principle. Momentum is always zero. It is possible to know the exact position and momentum simultaneously. Position can be measured exactly. It is impossible to know both the exact position and momentum of a particle simultaneously. None Hint 5. Why is chloroform stored in dark colored bottles? To avoid evaporation For aesthetic reasons To keep it cool To protect from light which decomposes it None Hint 6. State the oxidation number of N and Cl in NCl3. N = +3, Cl = -1 N = -3, Cl = +1 N = +1, Cl = -3 N = 0, Cl = 0 None Hint 7. How will you carry out the following conversions? (i) Ethanol to But-2-enal (ii) Propanone to 2-Methyl Butan-2-ol (iii) Butanoic acid to 2-Bromobutanoic acid Oxidation, Grignard reaction, Substitution Substitution, Addition, Elimination Elimination, Substitution, Oxidation Reduction, Oxidation, Addition None Hint 8. The consequence of lanthanide contraction is: Radii of elements of second and third transition series becomes similar. Radii of third transition series is smaller than elements of second transition series. Radii of elements of second transition series increases. Radii of elementstransition series decreases. None Hint 9. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature temperature and concentration nature of the electrolyte and concentration None Hint 10. In every chemical reaction, total mass of all the reactants is equal to the total mass of all the products. This statement is according to: Law of multiple proportions Law of constant proportions Postulates of Dalton’s atomic theory Law of conservation of mass None Hint 11. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Molality Normality Molarity Mole fraction None Hint 12. Which of the following is equal to 1 mole O₂? 60.22 × 10²³ atoms of Oxygen 60.22 × 10²² molecules of Oxygen 6.022 × 10²³ molecules of Oxygen 6.022 × 10²³ atoms of Oxygen None Hint 13. The empirical formula of fructose is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) CH₂O CHO₂ None of these CHO None Hint 14. Write True (T) or False (F) for the following statements: Raoult’s law is applicable only if the liquids are volatile and miscible. False Sometimes true Depends on temperature True None Hint 15. When a certain change is accompanied by absorption of 50 kJ of heat and expenditure of 30 kJ of work, then the change in internal energy is: Complete the following by given options below: (+20 kJ, +80 kJ, −1574 kJ mol⁻¹, +1574 kJ mol⁻¹) B. +20 kJ +80 kJ −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ None Hint 16. What is the active component of soap? What is the polar part in: (i) a soap molecule (ii) a synthetic detergent molecule Alcohol group, -CH3 Ester, -OH Hydrocarbon chain, -COONa Ketone, -NH2 None Hint 17. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 119, 80, 119 80, 199, 80 80, 119, 80 199, 80, 199 None Hint 18. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → NaHSO4 + Cl2 Na2SO4 + HCl NaHSO4 + HCl NaHSO4 + HCl None Hint 19. If the bond enthalpy of C–H and C–Cl bonds are 415 kJ mol⁻¹ and 339 kJ mol⁻¹ respectively, then the energy released in the formation of one mole of CH₃Cl molecules is: −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ +80 kJ +20 kJ None Hint 20. State the oxidation number of N and Cl in NCl₃. N = −3, Cl = +1 N = +1, Cl = −3 N = +5, Cl = −1 N = +3, Cl = −1 None Hint 21. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: exponentially related to each other not related to each other directly related to each other inversely related to each other None Hint 22. Geometrical isomerism is shown by isomers... possible for coordination number: equal to two less than or equal to four greater than or equal to four greater than or equal to two None Hint 23. Adiabatic processes proceeds with: A change in temperature A change in pressure No change in temperature An exchange of heat between the system and the surroundings None Hint 24. Define bond enthalpy. Calculate the bond enthalpy of CH4 molecule if average bond enthalpy of C-H bond is 414 kJ/mol. Energy required to break ionic bonds Energy released in bond formation Energy change in electron transfer Energy required to break one mole of bonds in gaseous molecules None Hint 25. Which of the following is not a function of salt bridge? It prevents accumulation of charges in the two half cells. It maintains electrical neutrality. It completes the outer circuit. It completes the inner circuit. None Hint 26. A system which can exchange energy but not matter with the surroundings is called __ system. open path closed isolated None Hint 27. What is the shape and magnetic behaviour of Ni(CO)₄? Square planar and paramagnetic Octahedral and paramagnetic Linear and diamagnetic Tetrahedral and diamagnetic None Hint 28. (i) State Faraday's first law of electrolysis. (ii) What is the mass of silver deposited when 300 coulomb electricity is passed through AgNO3 solution? (Atomic mass Ag = 108 u) Mass ∝ time taken Mass ∝ charge passed Mass ∝ voltage applied Mass ∝ concentration None Hint 29. Predict the shape of methane molecule on the basis of VSEPR theory. Octahedral Trigonal planar Tetrahedral Linear None Hint 30. The factors affecting conductivity of an electrolyte are: temperature and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature nature of the electrolyte and concentration None Hint 31. Which compound forms ethyl carbocation? Ethene Ethanol Ethane Ethyl chloride None Hint 32. A solution containing 12.5 g of a non-electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. The molar mass of the substance is: 75 g/mol 50 g/mol 100 g/mol 125 g/mol None Hint 33. Geometrical isomerism is shown by isomers in which first coordination sphere is same but geometrical arrangement of ligands varies. This isomerism is only possible for coordination number: Equal to two Less than or equal to two Greater than or equal to two Greater than or equal to four None Hint 34. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: inversely related to each other not related to each other directly related to each other exponentially related to each other None Hint 35. State the function of oxytocin. Increases heart rate Controls blood sugar Regulates metabolism Stimulates uterine contraction None Hint 36. Why does an ice cube float on water? Ice is denser than water Ice has higher melting point Ice is less dense than water Water contracts on freezing None Hint 37. If 3d and 4p orbitals are to be filled in an atom by an electron then which orbital will be occupied first? Depends on the element 3d orbital Both at the same time 4p orbita None Hint 38. Choose the most electronegative element from the following: Nitrogen Fluorine Sulphur Oxygen None Hint 39. Complete and balance the following chemical equations: XeF6 + 2H2O → XeO3 + 6HF XeOF4 + 2HF XeF4 + 4HF XeO2F2 + 4HF None Hint 40. Write the IUPAC name of the compound (benzene ring with two Br at 1,3 positions and CH2CH3 at 4): 1,2-Dibromo-4-ethylbenzene 3,4-Dibromo-1-ethylbenzene 1,4-Dibromo-3-ethylbenzene 1,3-Dibromo-4-ethylbenzene None Hint 41. Bronsted–Lowry concept of an acid and a base is based on: acceptance of proton and donation of proton respectively donation of H⁺ ion and OH⁻ ion respectively formation of H₃O⁺ ion and OH⁻ ion donation of proton and acceptance of proton respectively None Hint 42. What are ozonides? Give chemical equation for their formation. Compounds formed by alkali metals and ozone Compounds formed by alkenes and ozone Compounds formed by oxygen and water Compounds formed by hydrogen and ozone None Hint 43. What is the pH of a 0.001 M aqueous solution of HCl? 7 11 3 1 None Hint 44. Give the mathematical expression of de-Broglie equation: p = mv λ = h/mv E = mc² F = ma None Hint 45. The 3d series of transition metals/elements is from: Yttrium to Lanthanum Scandium to Copper Scandium to Zinc Actinium to Lawrencium None Hint 46. How are hormones transported to their place of action? By blood By air By water By diffusion None Hint 47. Classify the following oxides into acidic, basic or amphoteric oxides: FeO, SiO2, SO2, Al2O3 FeO - Acidic, SiO2 - Amphoteric, SO2 - Basic, Al2O3 - Acidic FeO - Basic, SiO2 - Acidic, SO2 - Acidic, Al2O3 - Amphoteric FeO - Acidic, SiO2 - Basic, SO2 - Amphoteric, Al2O3 - Acidic FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic None Hint 48. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 119, 80, 119 80, 119, 80 199, 80, 199 80, 199, 80 None Hint 49. Which observation of Rutherford’s α-ray scattering experiment led to the conclusion that all the positive charge of the atom was contained in the nucleus? The α-particles lost energy while passing through the foil. A few α-particles were deflected at large angles. Most of the α-particles passed straight through the foil. The α-particles scattered uniformly in all directions. None Hint 50. Enthalpy is a __ function. Closed State Open Path None Hint 51. State the function of oxytocin: Controls digestion Controls childbirth and lactation Controls muscle contraction Controls blood pressure None Hint 52. Which of the following is not a function of salt bridge? It maintains electrical neutrality. It prevents accumulation of charges in the two half cells. It completes the inner circuit. It completes the outer circuit. None Hint 53. How can you obtain propanamine using Hofmann Bromamide reaction? From alkane by nitration From alkene using HBr From alcohol using NH3 From amide using bromine and NaOH None Hint 54. What is the active component of soap? What is the polar part in (i) a soap molecule and (ii) a synthetic detergent molecule? Alcohol; hydroxyl group Detergent; sulphate group Fatty acid; methyl group Fatty acid; carboxyl group None Hint 55. What is the oxidation number of atoms in their elemental form? +1 0 -1 +2 None Hint 56. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From amide From ethane From ethanoic acid From ethyl bromide None Hint 57. What is the shape and magnetic behavior of [Ni(CN)4]2- ion according to Valence Bond Theory (VBT)? Linear and paramagnetic Octahedral and diamagnetic Square planar and diamagnetic Tetrahedral and paramagnetic None Hint 58. Write True (T) or False (F) for the following statements: Boiling point of a liquid is the temperature at which the vapor pressure of the liquid becomes zero. False Never true True Always true None Hint 59. The percentage of oxygen in Fe₃O₄ is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) None of these 72.41% 27.89% 27.59% None Hint 60. Which type of compound water is? Metallic Hydrogen Covalent Ionic None Hint 61. Low density polyethylene: is packed in a compact fashion has linear chain of molecules is harder and stronger than polypropylene has branching in polymer chains None Hint 62. What is the oxidation number of atoms in their elemental form? +2 +1 0 −1 None Hint 63. Match the following: Tailing of mercury → (1) Conc. Sulphuric acid Decomposed in a strong beam of light → (3) Ozone Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur Yellow and transparent crystalline substance → (4) Sulphur dioxide None Hint 64. The 3d series of transition metals/elements is from: Actinium to Lawrencium Scandium to Copper Scandium to Zinc Yttrium to Lanthanum None Hint 65. The standard enthalpy of atomisation of a substance is the change in enthalpy when: One molecule of a substance is converted into its atom in gaseous state at a given temperature and 1 bar pressure. One molecule of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at a given temperature and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. None Hint 66. Low density polythene: Is packed in a compact fashion Has branching in polymer chains Has linear chain of molecules Is harder and stronger than polypropylene None Hint 67. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Mole fraction Molarity Molality Normality None Hint 68. How are hormones transported to their place of action? Through nerves By diffusion By active transport Through bloodstream None Hint 69. State one physical property which is same for lithium and magnesium. Low density Large atomic radius Low electronegativity High melting point None Hint 70. One atomic mass unit is equal to: Mass of one C–12 atom × 12 Mass of one C–12 atom ÷ 12 Mass of one mole of C–12 atoms ÷ 12 Mass of one mole of C–12 atoms None Hint 71. Which liquid pairs show negative deviation from Raoult's Law? Benzene and toluene Water and salt solution Chloroform and acetone Water and ethanol None Hint 72. Vulcanization of rubber produces: a thermosetting polymer an elastomer a thermoplastic polymer a plasticizer None Hint 73. A system which can exchange energy but not matter with the surroundings is called: Open system Closed system Isolated system State system None Hint 74. What is the pH of a 0.001 M aqueous solution of HCl? 3 1 2 4 None Hint 75. A solution containing 12.5 g of a non-electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. Calculate the molar mass of the substance. 250 g/mol 100 g/mol 150 g/mol 200 g/mol None Hint 76. Enthalpy is a __ function. state isolated path closed None Hint 77. Adiabatic processes proceeds with: an exchange of heat between the system and the surroundings a change in temperature no change in temperature a change in pressure None Hint 78. Choose the most electronegative element from the following: Fluorine Sulphur Nitrogen Oxygen None Hint 79. Give the mathematical expression of de-Broglie equation. λ = h / mv λ = m / hv ) λ = mv / h λ = h × mv None Hint 80. Lanthanide contraction is due to increase in: Atomic number Effective nuclear charge Size of 4f orbital Shielding by 4f electrons None Hint 81. Bronsted-Lowry concept of an acid and a base is based on: donation of proton and acceptance of proton respectively acceptance of proton and donation of proton respectively donation of H⁺ ion and OH⁻ ion respectively formation of H₃O⁺ ion and OH⁻ ion None Hint 82. In every chemical reaction, total mass of all the reactants is equal to the total mass of all the products. This statement is according to: Law of constant proportions Postulates of Dalton’s atomic theory Law of conservation of mass Law of multiple proportions None Hint 83. The standard enthalpy of atomisation of a substance is the change in enthalpy when: One mole of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One mole of a substance is converted into its atoms in gaseous state at a given temperature and 1 bar pressure. One molecule of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. One molecule of a substance is converted into its atom in gaseous state at a given temperature and 1 bar pressure. None Hint 84. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 4-Chloropentane 3-Chloropentane 2-Chloropentane 1-Chloropentane None Hint Time's up Share: admin Previous post Physics Nios Plus Two PQ III July 5, 2025 Next post Malayalam Nios plus two II July 10, 2025
