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