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