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