Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. The consequence of lanthanide contraction is: Radii of elements of second and third transition series becomes similar. Radii of elements of second transition series increases. Radii of elementstransition series decreases. Radii of third transition series is smaller than elements of second transition series. None Hint 2. 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 conservation of mass Law of constant proportions Law of multiple proportions None Hint 3. Low density polythene: Is packed in a compact fashion Has branching in polymer chains Is harder and stronger than polypropylene Has linear chain of molecules None Hint 4. Geometrical isomerism is shown by isomers... possible for coordination number: less than or equal to four greater than or equal to four equal to two greater than or equal to two None Hint 5. 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 Hydrocarbon chain, -COONa Ketone, -NH2 None Hint 6. 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 7. Vulcanization of rubber produces: a plasticizer an elastomer a thermosetting polymer a thermoplastic polymer None Hint 8. 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. 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. None Hint 9. 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 10. What are ozonides? Give chemical equation for their formation. Compounds formed by alkali metals and ozone Compounds formed by hydrogen and ozone Compounds formed by alkenes and ozone Compounds formed by oxygen and water None Hint 11. 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 Fatty acid; methyl group Fatty acid; carboxyl group Detergent; sulphate group None Hint 12. How are hormones transported to their place of action? By water By diffusion By blood By air None Hint 13. What is the oxidation number of atoms in their elemental form? +2 0 -1 +1 None Hint 14. Match the following: Yellow and transparent crystalline substance → (4) Sulphur dioxide Decomposed in a strong beam of light → (3) Ozone Tailing of mercury → (1) Conc. Sulphuric acid Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur None Hint 15. Enthalpy is a __ function. closed isolated path state None Hint 16. Lanthanide contraction is due to increase in: Effective nuclear charge Size of 4f orbital Shielding by 4f electrons Atomic number None Hint 17. Which type of compound water is? Covalent Ionic Hydrogen Metallic None Hint 18. State the oxidation number of N and Cl in NCl₃. N = +1, Cl = −3 N = +5, Cl = −1 N = −3, Cl = +1 N = +3, Cl = −1 None Hint 19. Write True (T) or False (F) for the following statements: Raoult’s law is applicable only if the liquids are volatile and miscible. True Depends on temperature Sometimes true False None Hint 20. How are hormones transported to their place of action? Through nerves By diffusion Through bloodstream By active transport None Hint 21. Which compound forms ethyl carbocation? Ethanol Ethyl chloride Ethene Ethane None Hint 22. 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: 125 g/mol 100 g/mol 75 g/mol 50 g/mol None Hint 23. The 3d series of transition metals/elements is from: Scandium to Copper Yttrium to Lanthanum Actinium to Lawrencium Scandium to Zinc None Hint 24. State the function of oxytocin: Controls muscle contraction Controls digestion Controls childbirth and lactation Controls blood pressure None Hint 25. Why is the shape of ammonia molecule trigonal pyramidal? Due to the presence of three bonded pairs only. Because of double bonds between nitrogen and hydrogen. Due to repulsion between lone pair electrons. Because of linear arrangement of atoms. None Hint 26. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration nature of the electrolyte and concentration nature of the electrolyte and temperature temperature and concentration None Hint 27. 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 28. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 2-Chloropentane 4-Chloropentane 1-Chloropentane 3-Chloropentane None Hint 29. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: not related to each other inversely related to each other directly related to each other exponentially related to each other None Hint 30. A system which can exchange energy but not matter with the surroundings is called __ system. path isolated open closed None Hint 31. Why does an ice cube float on water? Ice has higher melting point Ice is less dense than water Water contracts on freezing Ice is denser than water None Hint 32. What is the shape and magnetic behaviour of Ni(CO)₄? Square planar and paramagnetic Tetrahedral and diamagnetic Octahedral and paramagnetic Linear and diamagnetic None Hint 33. 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 34. 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 35. 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: +20 kJ −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ +80 kJ None Hint 36. 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 Equal to two Greater than or equal to four Less than or equal to two None Hint 37. State the function of oxytocin. Regulates metabolism Increases heart rate Controls blood sugar Stimulates uterine contraction None Hint 38. 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 39. Complete and balance the following chemical equations: XeF6 + 2H2O → XeF4 + 4HF XeOF4 + 2HF XeO3 + 6HF XeO2F2 + 4HF None Hint 40. State Heisenberg’s uncertainty principle: E = hv v = λf Δx · Δp ≥ h/4π ΔE · Δt = h None Hint 41. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → Na2SO4 + HCl NaHSO4 + HCl NaHSO4 + Cl2 NaHSO4 + HCl None Hint 42. A system which can exchange energy but not matter with the surroundings is called: Isolated system State system Closed system Open system None Hint 43. 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 44. Choose the most electronegative element from the following: Oxygen Sulphur Nitrogen Fluorine None Hint 45. Give the mathematical expression of de-Broglie equation. λ = h / mv ) λ = mv / h λ = m / hv λ = h × mv None Hint 46. Predict the shape of methane molecule on the basis of VSEPR theory. Trigonal planar Octahedral Tetrahedral Linear None Hint 47. Bronsted–Lowry concept of an acid and a base is based on: donation of proton and acceptance of proton respectively formation of H₃O⁺ ion and OH⁻ ion acceptance of proton and donation of proton respectively donation of H⁺ ion and OH⁻ ion respectively None Hint 48. Which liquid pairs show negative deviation from Raoult's Law? Water and salt solution Water and ethanol Chloroform and acetone Benzene and toluene None Hint 49. 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 200 g/mol 250 g/mol None Hint 50. How can you obtain propanamine using Hofmann Bromamide reaction? From alkane by nitration From alkene using HBr From amide using bromine and NaOH From alcohol using NH3 None Hint 51. 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 formation of H₃O⁺ ion and OH⁻ ion donation of H⁺ ion and OH⁻ ion respectively None Hint 52. 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 Oxidation, Grignard reaction, Substitution Reduction, Oxidation, Addition Substitution, Addition, Elimination None Hint 53. 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 +80 kJ −1574 kJ mol⁻¹ B. +20 kJ None Hint 54. What is the pH of a 0.001 M aqueous solution of HCl? 4 1 3 2 None Hint 55. The empirical formula of fructose is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) None of these CHO CHO₂ CH₂O None Hint 56. Enthalpy is a __ function. State Path Closed Open None Hint 57. Vulcanization of rubber produces: an elastomer a thermosetting polymer a plasticizer a thermoplastic polymer None Hint 58. 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 59. 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 inner circuit. It completes the outer circuit. None Hint 60. What is the oxidation number of atoms in their elemental form? 0 +1 −1 +2 None Hint 61. 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 62. 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 63. Adiabatic processes proceeds with: an exchange of heat between the system and the surroundings a change in pressure a change in temperature no change in temperature None Hint 64. 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 65. 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 True Always true False None Hint 66. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From ethyl bromide From amide From ethane From ethanoic acid None Hint 67. 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 conservation of mass Law of constant proportions Law of multiple proportions None Hint 68. What is the pH of a 0.001 M aqueous solution of HCl? 7 1 3 11 None Hint 69. Why is chloroform stored in dark colored bottles? To keep it cool For aesthetic reasons To avoid evaporation To protect from light which decomposes it None Hint 70. State one physical property which is same for lithium and magnesium. Low density Large atomic radius Low electronegativity High melting point None Hint 71. 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 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 25°C and 1 bar pressure. None Hint 72. Give the mathematical expression of de-Broglie equation: λ = h/mv F = ma p = mv E = mc² None Hint 73. 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 74. The 3d series of transition metals/elements is from: Scandium to Copper Yttrium to Lanthanum Scandium to Zinc Actinium to Lawrencium None Hint 75. 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 76. Which of the following is not a function of salt bridge? It maintains electrical neutrality. It completes the inner circuit. It prevents accumulation of charges in the two half cells. It completes the outer circuit. None Hint 77. State Heisenberg’s uncertainty principle. Position can be measured exactly. It is impossible to know both the exact position and momentum of a particle simultaneously. It is possible to know the exact position and momentum simultaneously. Momentum is always zero. None Hint 78. 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 3,4-Dibromo-1-ethylbenzene 1,2-Dibromo-4-ethylbenzene 1,4-Dibromo-3-ethylbenzene None Hint 79. The factors affecting conductivity of an electrolyte are: nature of the electrolyte and concentration nature of the electrolyte, temperature and concentration temperature and concentration nature of the electrolyte and temperature None Hint 80. Choose the most electronegative element from the following: Fluorine Oxygen Nitrogen Sulphur None Hint 81. (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 ∝ concentration Mass ∝ voltage applied Mass ∝ time taken None Hint 82. The percentage of oxygen in Fe₃O₄ is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) 72.41% None of these 27.59% 27.89% None Hint 83. 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 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 84. 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 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
