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? Octahedral and paramagnetic Tetrahedral and diamagnetic Linear and diamagnetic Square planar and paramagnetic None Hint 2. What is the pH of a 0.001 M aqueous solution of HCl? 4 3 2 1 None Hint 3. 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 4. 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 True Always true Never true None Hint 5. 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 C–12 atom × 12 Mass of one mole of C–12 atoms None Hint 6. 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 7. 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 8. Choose the most electronegative element from the following: Sulphur Fluorine Nitrogen Oxygen None Hint 9. A system which can exchange energy but not matter with the surroundings is called: Open system Isolated system State system Closed system None Hint 10. Enthalpy is a __ function. isolated state closed path None Hint 11. Low density polyethylene: has linear chain of molecules has branching in polymer chains is packed in a compact fashion is harder and stronger than polypropylene None Hint 12. 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 CH₂O CHO CHO₂ None Hint 13. Adiabatic processes proceeds with: A change in pressure An exchange of heat between the system and the surroundings A change in temperature No change in temperature None Hint 14. 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 15. The 3d series of transition metals/elements is from: Yttrium to Lanthanum Actinium to Lawrencium Scandium to Copper Scandium to Zinc None Hint 16. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: not related to each other directly related to each other inversely related to each other exponentially related to each other None Hint 17. Write the IUPAC name of the compound (benzene ring with two Br at 1,3 positions and CH2CH3 at 4): 3,4-Dibromo-1-ethylbenzene 1,4-Dibromo-3-ethylbenzene 1,2-Dibromo-4-ethylbenzene 1,3-Dibromo-4-ethylbenzene None Hint 18. 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 19. State the function of oxytocin: Controls blood pressure Controls childbirth and lactation Controls muscle contraction Controls digestion None Hint 20. 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 Greater than or equal to four Equal to two Less than or equal to two None Hint 21. 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 −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ B. +20 kJ None Hint 22. Enthalpy is a __ function. State Closed Path Open None Hint 23. How are hormones transported to their place of action? Through nerves Through bloodstream By active transport By diffusion None Hint 24. State the function of oxytocin. Stimulates uterine contraction Increases heart rate Controls blood sugar Regulates metabolism None Hint 25. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 80, 199, 80 80, 119, 80 199, 80, 199 119, 80, 119 None Hint 26. 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. A few α-particles were deflected at large angles. The α-particles scattered uniformly in all directions. Most of the α-particles passed straight through the foil. None Hint 27. 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 28. 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 29. Which liquid pairs show negative deviation from Raoult's Law? Chloroform and acetone Water and ethanol Benzene and toluene Water and salt solution None Hint 30. 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% None of these 72.41% 27.59% None Hint 31. Which of the following is equal to 1 mole O₂? 6.022 × 10²³ atoms of Oxygen 60.22 × 10²³ atoms of Oxygen 60.22 × 10²² molecules of Oxygen 6.022 × 10²³ molecules of Oxygen None Hint 32. The 3d series of transition metals/elements is from: Actinium to Lawrencium Yttrium to Lanthanum Scandium to Zinc Scandium to Copper None Hint 33. 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 34. 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 35. 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 required to break ionic bonds Energy change in electron transfer None Hint 36. 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. 200 g/mol 150 g/mol 100 g/mol 250 g/mol None Hint 37. Predict the shape of methane molecule on the basis of VSEPR theory. Linear Trigonal planar Octahedral Tetrahedral None Hint 38. How are hormones transported to their place of action? By blood By diffusion By water By air None Hint 39. Why does an ice cube float on water? Ice is denser than water Water contracts on freezing Ice is less dense than water Ice has higher melting point None Hint 40. 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 41. Choose the most electronegative element from the following: Nitrogen Oxygen Fluorine Sulphur None Hint 42. Vulcanization of rubber produces: a plasticizer a thermoplastic polymer a thermosetting polymer an elastomer None Hint 43. The consequence of lanthanide contraction is: Radii of elementstransition series decreases. 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 elements of second transition series increases. None Hint 44. (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 45. State the oxidation number of N and Cl in NCl₃. N = −3, Cl = +1 N = +1, Cl = −3 N = +5, Cl = −1 N = +3, Cl = −1 None Hint 46. 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 125 g/mol 75 g/mol None Hint 47. Give the mathematical expression of de-Broglie equation: λ = h/mv p = mv F = ma E = mc² None Hint 48. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → NaHSO4 + Cl2 NaHSO4 + HCl NaHSO4 + HCl Na2SO4 + HCl None Hint 49. 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 Law of conservation of mass Law of constant proportions Postulates of Dalton’s atomic theory None Hint 50. 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. Position can be measured exactly. Momentum is always zero. None Hint 51. Vulcanization of rubber produces: a thermoplastic polymer a plasticizer a thermosetting polymer an elastomer 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 Substitution, Addition, Elimination Oxidation, Grignard reaction, Substitution Reduction, Oxidation, Addition None Hint 53. Match the following: Tailing of mercury → (1) Conc. Sulphuric acid Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur Yellow and transparent crystalline substance → (4) Sulphur dioxide Decomposed in a strong beam of light → (3) Ozone None Hint 54. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Molarity Mole fraction Molality Normality None Hint 55. What is the oxidation number of atoms in their elemental form? 0 +2 -1 +1 None Hint 56. Low density polythene: Is packed in a compact fashion Is harder and stronger than polypropylene Has branching in polymer chains Has linear chain of molecules None Hint 57. Why is chloroform stored in dark colored bottles? For aesthetic reasons To protect from light which decomposes it To keep it cool To avoid evaporation None Hint 58. Complete and balance the following chemical equations: XeF6 + 2H2O → XeO3 + 6HF XeO2F2 + 4HF XeF4 + 4HF XeOF4 + 2HF None Hint 59. What are ozonides? Give chemical equation for their formation. Compounds formed by alkali metals and ozone Compounds formed by alkenes and ozone Compounds formed by hydrogen and ozone Compounds formed by oxygen and water None Hint 60. 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 Alcohol; hydroxyl group Fatty acid; methyl group Fatty acid; carboxyl group 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? Depends on the element 3d orbital 4p orbita Both at the same time None Hint 62. 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 63. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Normality Molality Mole fraction Molarity None Hint 64. 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 65. Why is the shape of ammonia molecule trigonal pyramidal? Due to repulsion between lone pair electrons. Because of linear arrangement of atoms. Because of double bonds between nitrogen and hydrogen. Due to the presence of three bonded pairs only. None Hint 66. State Heisenberg’s uncertainty principle: ΔE · Δt = h E = hv Δx · Δp ≥ h/4π v = λf None Hint 67. Give the mathematical expression of de-Broglie equation. λ = h / mv ) λ = mv / h λ = h × mv λ = m / hv None Hint 68. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 4-Chloropentane 3-Chloropentane 1-Chloropentane 2-Chloropentane None Hint 69. Lanthanide contraction is due to increase in: Shielding by 4f electrons Atomic number Size of 4f orbital Effective nuclear charge None Hint 70. 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: +80 kJ −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ +20 kJ None Hint 71. 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 acceptance of proton and donation of proton respectively formation of H₃O⁺ ion and OH⁻ ion None Hint 72. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature nature of the electrolyte and concentration temperature and concentration None Hint 73. What is the pH of a 0.001 M aqueous solution of HCl? 1 3 11 7 None Hint 74. How can you obtain propanamine using Hofmann Bromamide reaction? From alkane by nitration From alkene using HBr From alcohol using NH3 From amide using bromine and NaOH None Hint 75. 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 76. Classify the following oxides into acidic, basic or amphoteric oxides: FeO, SiO2, SO2, Al2O3 FeO - Acidic, SiO2 - Basic, SO2 - Amphoteric, Al2O3 - Acidic FeO - Basic, SiO2 - Acidic, SO2 - Acidic, Al2O3 - Amphoteric FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic FeO - Acidic, SiO2 - Amphoteric, SO2 - Basic, Al2O3 - Acidic None Hint 77. State one physical property which is same for lithium and magnesium. High melting point Low electronegativity Large atomic radius Low density None Hint 78. Which type of compound water is? Covalent Ionic Hydrogen Metallic None Hint 79. 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 80. What is the shape and magnetic behavior of [Ni(CN)4]2- ion according to Valence Bond Theory (VBT)? Octahedral and diamagnetic Linear and paramagnetic Square planar and diamagnetic Tetrahedral and paramagnetic None Hint 81. 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 Ketone, -NH2 Ester, -OH None Hint 82. Which compound forms ethyl carbocation? Ethene Ethanol Ethane Ethyl chloride None Hint 83. A system which can exchange energy but not matter with the surroundings is called __ system. open isolated path closed None Hint 84. What is the oxidation number of atoms in their elemental form? 0 +2 −1 +1 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
