Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. 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 required to break one mole of bonds in gaseous molecules Energy change in electron transfer None Hint 2. (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 ∝ charge passed Mass ∝ time taken Mass ∝ voltage applied None Hint 3. A system which can exchange energy but not matter with the surroundings is called __ system. path open closed isolated None Hint 4. Low density polythene: Is harder and stronger than polypropylene Has branching in polymer chains Is packed in a compact fashion Has linear chain of molecules None Hint 5. 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 6. Vulcanization of rubber produces: a thermosetting polymer a plasticizer an elastomer a thermoplastic polymer None Hint 7. 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 +80 kJ +20 kJ +1574 kJ mol⁻¹ None Hint 8. What is the oxidation number of atoms in their elemental form? +2 -1 +1 0 None Hint 9. Why does an ice cube float on water? Water contracts on freezing Ice has higher melting point Ice is less dense than water Ice is denser than water None Hint 10. Choose the most electronegative element from the following: Fluorine Nitrogen Sulphur Oxygen None Hint 11. State Heisenberg’s uncertainty principle: v = λf Δx · Δp ≥ h/4π ΔE · Δt = h E = hv None Hint 12. Lanthanide contraction is due to increase in: Atomic number Shielding by 4f electrons Effective nuclear charge Size of 4f orbital None Hint 13. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Molality Mole fraction Molarity Normality None Hint 14. Which type of compound water is? Covalent Ionic Metallic Hydrogen None Hint 15. 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 16. Which of the following is not a function of salt bridge? It completes the outer circuit. It maintains electrical neutrality. It completes the inner circuit. It prevents accumulation of charges in the two half cells. None Hint 17. Enthalpy is a __ function. Closed Path Open State None Hint 18. 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 19. 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 20. Give the mathematical expression of de-Broglie equation: p = mv λ = h/mv F = ma E = mc² None Hint 21. 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 Always true False None Hint 22. Low density polyethylene: has branching in polymer chains has linear chain of molecules is packed in a compact fashion is harder and stronger than polypropylene None Hint 23. 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 24. Vulcanization of rubber produces: an elastomer a plasticizer a thermoplastic polymer a thermosetting polymer None Hint 25. The 3d series of transition metals/elements is from: Yttrium to Lanthanum Actinium to Lawrencium Scandium to Zinc Scandium to Copper None Hint 26. 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 27. 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 directly related to each other inversely related to each other None Hint 28. 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 29. 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. 100 g/mol 200 g/mol 250 g/mol 150 g/mol None Hint 30. How are hormones transported to their place of action? By blood By air By water By diffusion None Hint 31. Choose the most electronegative element from the following: Oxygen Fluorine Sulphur Nitrogen None Hint 32. 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 27.89% 27.59% 72.41% None Hint 33. Write True (T) or False (F) for the following statements: Raoult’s law is applicable only if the liquids are volatile and miscible. True False Sometimes true Depends on temperature None Hint 34. 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 multiple proportions Law of conservation of mass None Hint 35. Enthalpy is a __ function. state path isolated closed None Hint 36. 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 1,3-Dibromo-4-ethylbenzene 1,4-Dibromo-3-ethylbenzene 3,4-Dibromo-1-ethylbenzene None Hint 37. 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 38. Match the following: Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur Yellow and transparent crystalline substance → (4) Sulphur dioxide Decomposed in a strong beam of light → (3) Ozone Tailing of mercury → (1) Conc. Sulphuric acid None Hint 39. A system which can exchange energy but not matter with the surroundings is called: Isolated system Closed system Open system State system None Hint 40. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration temperature and concentration nature of the electrolyte and concentration nature of the electrolyte and temperature None Hint 41. What is the pH of a 0.001 M aqueous solution of HCl? 3 2 4 1 None Hint 42. What is the oxidation number of atoms in their elemental form? 0 +1 +2 −1 None Hint 43. 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 a given temperature 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 molecule of a substance is converted into its atoms in gaseous state at 25°C and 1 bar pressure. None Hint 44. What are ozonides? Give chemical equation for their formation. Compounds formed by oxygen and water Compounds formed by alkenes and ozone Compounds formed by hydrogen and ozone Compounds formed by alkali metals and ozone None Hint 45. How are hormones transported to their place of action? Through nerves By active transport Through bloodstream By diffusion None Hint 46. What is the shape and magnetic behaviour of Ni(CO)₄? Linear and diamagnetic Octahedral and paramagnetic Tetrahedral and diamagnetic Square planar and paramagnetic None Hint 47. Why is chloroform stored in dark colored bottles? To protect from light which decomposes it To avoid evaporation To keep it cool For aesthetic reasons None Hint 48. State the function of oxytocin. Increases heart rate Stimulates uterine contraction Regulates metabolism Controls blood sugar None Hint 49. 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; methyl group Alcohol; hydroxyl group Fatty acid; carboxyl group Detergent; sulphate group None Hint 50. State the function of oxytocin: Controls blood pressure Controls muscle contraction Controls childbirth and lactation Controls digestion None Hint 51. 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 Ester, -OH Alcohol group, -CH3 None Hint 52. 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 four Greater than or equal to two None Hint 53. Bronsted-Lowry concept of an acid and a base is based on: formation of H₃O⁺ ion and OH⁻ ion donation of H⁺ ion and OH⁻ ion respectively donation of proton and acceptance of proton respectively acceptance of proton and donation of proton respectively None Hint 54. 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 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 atom in gaseous state at a given temperature and 1 bar pressure. None Hint 55. 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 56. State one physical property which is same for lithium and magnesium. Low electronegativity High melting point Large atomic radius Low density None Hint 57. 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 58. Which liquid pairs show negative deviation from Raoult's Law? Water and ethanol Water and salt solution Chloroform and acetone Benzene and toluene None Hint 59. 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 Normality Molarity None Hint 60. Predict the shape of methane molecule on the basis of VSEPR theory. Linear Octahedral Trigonal planar Tetrahedral None Hint 61. State Heisenberg’s uncertainty principle. 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. Position can be measured exactly. None Hint 62. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 4-Chloropentane 1-Chloropentane 3-Chloropentane 2-Chloropentane None Hint 63. The 3d series of transition metals/elements is from: Yttrium to Lanthanum Scandium to Copper Scandium to Zinc Actinium to Lawrencium None Hint 64. Complete and balance the following chemical equations: XeF6 + 2H2O → XeO2F2 + 4HF XeF4 + 4HF XeO3 + 6HF XeOF4 + 2HF None Hint 65. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From ethyl bromide From ethane From ethanoic acid From amide None Hint 66. 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 Oxidation, Grignard reaction, Substitution Reduction, Oxidation, Addition Elimination, Substitution, Oxidation None Hint 67. 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) +80 kJ B. +20 kJ +1574 kJ mol⁻¹ −1574 kJ mol⁻¹ None Hint 68. Which compound forms ethyl carbocation? Ethanol Ethane Ethyl chloride Ethene None Hint 69. 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 70. 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. 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. None Hint 71. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → NaHSO4 + HCl Na2SO4 + HCl NaHSO4 + HCl NaHSO4 + Cl2 None Hint 72. Geometrical isomerism is shown by isomers... possible for coordination number: greater than or equal to two greater than or equal to four equal to two less than or equal to four None Hint 73. 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 74. Which of the following is equal to 1 mole O₂? 60.22 × 10²² molecules of Oxygen 60.22 × 10²³ atoms of Oxygen 6.022 × 10²³ molecules of Oxygen 6.022 × 10²³ atoms of Oxygen None Hint 75. 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 maintains electrical neutrality. It completes the outer circuit. None Hint 76. 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 - Amphoteric, SO2 - Basic, Al2O3 - Acidic FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic FeO - Acidic, SiO2 - Basic, SO2 - Amphoteric, Al2O3 - Acidic None Hint 77. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration temperature and concentration nature of the electrolyte and concentration nature of the electrolyte and temperature None Hint 78. What is the pH of a 0.001 M aqueous solution of HCl? 1 3 11 7 None Hint 79. 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 80. 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 81. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 199, 80, 199 80, 199, 80 80, 119, 80 119, 80, 119 None Hint 82. Give the mathematical expression of de-Broglie equation. λ = h × mv λ = h / mv λ = m / hv ) λ = mv / h None Hint 83. State the oxidation number of N and Cl in NCl₃. N = +5, Cl = −1 N = −3, Cl = +1 N = +1, Cl = −3 N = +3, Cl = −1 None Hint 84. 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 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
