Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. What is the shape and magnetic behaviour of Ni(CO)₄? Tetrahedral and diamagnetic Square planar and paramagnetic Linear and diamagnetic Octahedral and paramagnetic None Hint 2. 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 3,4-Dibromo-1-ethylbenzene 1,2-Dibromo-4-ethylbenzene None Hint 3. 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 4. Give the mathematical expression of de-Broglie equation. λ = h × mv λ = h / mv ) λ = mv / h λ = m / hv None Hint 5. Predict the shape of methane molecule on the basis of VSEPR theory. Octahedral Linear Trigonal planar Tetrahedral None Hint 6. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From ethane From amide From ethanoic acid From ethyl bromide 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 Tetrahedral and paramagnetic Linear and paramagnetic Square planar and diamagnetic None Hint 8. State the function of oxytocin: Controls childbirth and lactation Controls muscle contraction Controls blood pressure Controls digestion None Hint 9. 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 10. How can you obtain propanamine using Hofmann Bromamide reaction? From alcohol using NH3 From amide using bromine and NaOH From alkane by nitration From alkene using HBr None Hint 11. 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 Depends on temperature False True None Hint 12. 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 13. What is the pH of a 0.001 M aqueous solution of HCl? 1 7 3 11 None Hint 14. The consequence of lanthanide contraction is: Radii of third transition series is smaller than elements of second transition series. Radii of elements of second and third transition series becomes similar. Radii of elements of second transition series increases. Radii of elementstransition series decreases. None Hint 15. What is the oxidation number of atoms in their elemental form? +2 +1 -1 0 None Hint 16. State the oxidation number of N and Cl in NCl3. N = 0, Cl = 0 N = +3, Cl = -1 N = -3, Cl = +1 N = +1, Cl = -3 None Hint 17. Which type of compound water is? Metallic Hydrogen Covalent Ionic None Hint 18. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 3-Chloropentane 2-Chloropentane 1-Chloropentane 4-Chloropentane None Hint 19. 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 multiple proportions Postulates of Dalton’s atomic theory Law of constant proportions None Hint 20. Bronsted-Lowry concept of an acid and a base is based on: donation of proton and acceptance of proton respectively donation of H⁺ ion and OH⁻ ion respectively formation of H₃O⁺ ion and OH⁻ ion acceptance of proton and donation of proton respectively None Hint 21. 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 CHO₂ CH₂O CHO None Hint 22. Why does an ice cube float on water? Ice has higher melting point Water contracts on freezing Ice is denser than water Ice is less dense than water None Hint 23. 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 −1574 kJ mol⁻¹ B. +20 kJ +80 kJ None Hint 24. 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 25. 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 26. Classify the following oxides into acidic, basic or amphoteric oxides: FeO, SiO2, SO2, Al2O3 FeO - Acidic, SiO2 - Amphoteric, SO2 - Basic, Al2O3 - Acidic FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic FeO - Acidic, SiO2 - Basic, SO2 - Amphoteric, Al2O3 - Acidic FeO - Basic, SiO2 - Acidic, SO2 - Acidic, Al2O3 - Amphoteric None Hint 27. 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 28. What is the oxidation number of atoms in their elemental form? +1 +2 −1 0 None Hint 29. Which of the following is equal to 1 mole O₂? 6.022 × 10²³ molecules of Oxygen 6.022 × 10²³ atoms of Oxygen 60.22 × 10²² molecules of Oxygen 60.22 × 10²³ atoms of Oxygen None Hint 30. 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 31. 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 inversely related to each other directly related to each other None Hint 32. 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 33. 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 34. Vulcanization of rubber produces: an elastomer a thermoplastic polymer a plasticizer a thermosetting polymer None Hint 35. The percentage of oxygen in Fe₃O₄ is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) 27.89% 72.41% None of these 27.59% None Hint 36. Which compound forms ethyl carbocation? Ethane Ethene Ethanol Ethyl chloride None Hint 37. State Heisenberg’s uncertainty principle: Δx · Δp ≥ h/4π E = hv ΔE · Δt = h v = λf None Hint 38. State Heisenberg’s uncertainty principle. It is possible to know the exact position and momentum simultaneously. Position can be measured exactly. It is impossible to know both the exact position and momentum of a particle simultaneously. Momentum is always zero. None Hint 39. What is the pH of a 0.001 M aqueous solution of HCl? 2 1 4 3 None Hint 40. 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 41. 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 conservation of mass Law of constant proportions None Hint 42. Match the following: Yellow and transparent crystalline substance → (4) Sulphur dioxide Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur Decomposed in a strong beam of light → (3) Ozone Tailing of mercury → (1) Conc. Sulphuric acid None Hint 43. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Mole fraction Normality Molarity Molality None Hint 44. State the function of oxytocin. Stimulates uterine contraction Increases heart rate Regulates metabolism Controls blood sugar None Hint 45. The factors affecting conductivity of an electrolyte are: temperature and concentration nature of the electrolyte and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature None Hint 46. 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 Always true Never true False None Hint 47. State one physical property which is same for lithium and magnesium. Low electronegativity Low density Large atomic radius High melting point None Hint 48. How are hormones transported to their place of action? By air By water By diffusion By blood None Hint 49. Bronsted–Lowry concept of an acid and a base is based on: donation of H⁺ ion and OH⁻ ion respectively formation of H₃O⁺ ion and OH⁻ ion donation of proton and acceptance of proton respectively acceptance of proton and donation of proton respectively None Hint 50. State the oxidation number of N and Cl in NCl₃. N = +1, Cl = −3 N = +3, Cl = −1 N = −3, Cl = +1 N = +5, Cl = −1 None Hint 51. 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 52. How are hormones transported to their place of action? By active transport By diffusion Through nerves Through bloodstream None Hint 53. 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 125 g/mol 50 g/mol 100 g/mol None Hint 54. 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 Detergent; sulphate group Alcohol; hydroxyl group Fatty acid; carboxyl group None Hint 55. 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 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. None Hint 56. Complete and balance the following chemical equations: XeF6 + 2H2O → XeOF4 + 2HF XeF4 + 4HF XeO3 + 6HF XeO2F2 + 4HF None Hint 57. One atomic mass unit is equal to: Mass of one mole of C–12 atoms Mass of one mole of C–12 atoms ÷ 12 Mass of one C–12 atom ÷ 12 Mass of one C–12 atom × 12 None Hint 58. The 3d series of transition metals/elements is from: Scandium to Zinc Scandium to Copper Yttrium to Lanthanum Actinium to Lawrencium None Hint 59. The factors affecting conductivity of an electrolyte are: temperature and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and concentration nature of the electrolyte and temperature None Hint 60. Give the mathematical expression of de-Broglie equation: F = ma p = mv λ = h/mv E = mc² None Hint 61. A system which can exchange energy but not matter with the surroundings is called __ system. isolated path open closed None Hint 62. Choose the most electronegative element from the following: Sulphur Nitrogen Oxygen Fluorine None Hint 63. (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 64. If 3d and 4p orbitals are to be filled in an atom by an electron then which orbital will be occupied first? 3d orbital Both at the same time 4p orbita Depends on the element None Hint 65. Enthalpy is a __ function. path closed isolated state None Hint 66. 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 Greater than or equal to two Less than or equal to two Equal to two None Hint 67. Choose the most electronegative element from the following: Sulphur Oxygen Fluorine Nitrogen None Hint 68. Enthalpy is a __ function. Open Path State Closed None Hint 69. 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 70. Which of the following is not a function of salt bridge? It completes the outer circuit. It maintains electrical neutrality. It prevents accumulation of charges in the two half cells. It completes the inner circuit. None Hint 71. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → Na2SO4 + HCl NaHSO4 + HCl NaHSO4 + HCl NaHSO4 + Cl2 None Hint 72. Lanthanide contraction is due to increase in: Atomic number Effective nuclear charge Shielding by 4f electrons Size of 4f orbital None Hint 73. The 3d series of transition metals/elements is from: Actinium to Lawrencium Yttrium to Lanthanum Scandium to Zinc Scandium to Copper None Hint 74. A system which can exchange energy but not matter with the surroundings is called: State system Open system Closed system Isolated system None Hint 75. 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 Elimination, Substitution, Oxidation Reduction, Oxidation, Addition None Hint 76. Vulcanization of rubber produces: an elastomer a thermoplastic polymer a thermosetting polymer a plasticizer None Hint 77. Low density polyethylene: is packed in a compact fashion has branching in polymer chains has linear chain of molecules is harder and stronger than polypropylene None Hint 78. 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 Alcohol group, -CH3 Ester, -OH Ketone, -NH2 None Hint 79. 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 80. 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 outer circuit. It completes the inner circuit. None Hint 81. 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 82. Geometrical isomerism is shown by isomers... possible for coordination number: equal to two greater than or equal to two less than or equal to four greater than or equal to four None Hint 83. Low density polythene: Has branching in polymer chains Is harder and stronger than polypropylene Is packed in a compact fashion Has linear chain of molecules 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: Molality Molarity 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
