Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. 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 2. Lanthanide contraction is due to increase in: Shielding by 4f electrons Atomic number Size of 4f orbital Effective nuclear charge None Hint 3. Enthalpy is a __ function. path closed isolated state None Hint 4. State Heisenberg’s uncertainty principle. Momentum is always zero. It is impossible to know both the exact position and momentum of a particle simultaneously. Position can be measured exactly. It is possible to know the exact position and momentum simultaneously. None Hint 5. 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 Postulates of Dalton’s atomic theory Law of multiple proportions None Hint 6. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 3-Chloropentane 4-Chloropentane 1-Chloropentane 2-Chloropentane None Hint 7. State Heisenberg’s uncertainty principle: Δx · Δp ≥ h/4π E = hv v = λf ΔE · Δt = h None Hint 8. Why is chloroform stored in dark colored bottles? To avoid evaporation To keep it cool To protect from light which decomposes it For aesthetic reasons None Hint 9. State the oxidation number of N and Cl in NCl3. N = +1, Cl = -3 N = 0, Cl = 0 N = +3, Cl = -1 N = -3, Cl = +1 None Hint 10. What is the pH of a 0.001 M aqueous solution of HCl? 4 2 3 1 None Hint 11. 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 12. 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 acceptance of proton and donation of proton respectively formation of H₃O⁺ ion and OH⁻ ion None Hint 13. Predict the shape of methane molecule on the basis of VSEPR theory. Octahedral Tetrahedral Trigonal planar Linear None Hint 14. Give the mathematical expression of de-Broglie equation: p = mv F = ma E = mc² λ = h/mv None Hint 15. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → NaHSO4 + HCl NaHSO4 + HCl Na2SO4 + HCl NaHSO4 + Cl2 None Hint 16. 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 required to break ionic bonds Energy change in electron transfer Energy released in bond formation None Hint 17. 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? Most of the α-particles passed straight through the foil. The α-particles lost energy while passing through the foil. The α-particles scattered uniformly in all directions. A few α-particles were deflected at large angles. None Hint 18. What is the pH of a 0.001 M aqueous solution of HCl? 1 3 7 11 None Hint 19. 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 1,4-Dibromo-3-ethylbenzene 3,4-Dibromo-1-ethylbenzene 1,3-Dibromo-4-ethylbenzene None Hint 20. A system which can exchange energy but not matter with the surroundings is called __ system. closed path open isolated None Hint 21. (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 ∝ time taken Mass ∝ concentration Mass ∝ voltage applied None Hint 22. Match the following: Tailing of mercury → (1) Conc. Sulphuric acid Decomposed in a strong beam of light → (3) Ozone Yellow and transparent crystalline substance → (4) Sulphur dioxide Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur None Hint 23. 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; carboxyl group Fatty acid; methyl group Detergent; sulphate group None Hint 24. 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 25. 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 26. What is the shape and magnetic behaviour of Ni(CO)₄? Octahedral and paramagnetic Square planar and paramagnetic Linear and diamagnetic Tetrahedral and diamagnetic None Hint 27. Adiabatic processes proceeds with: a change in temperature an exchange of heat between the system and the surroundings a change in pressure no change in temperature None Hint 28. How are hormones transported to their place of action? Through bloodstream By diffusion Through nerves By active transport None Hint 29. Which type of compound water is? Ionic Metallic Covalent Hydrogen None Hint 30. 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 4p orbita Both at the same time None Hint 31. How can you obtain propanamine using Hofmann Bromamide reaction? From alkane by nitration From amide using bromine and NaOH From alkene using HBr From alcohol using NH3 None Hint 32. Which compound forms ethyl carbocation? Ethene Ethane Ethanol Ethyl chloride None Hint 33. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From amide From ethyl bromide From ethanoic acid From ethane None Hint 34. Choose the most electronegative element from the following: Fluorine Oxygen Nitrogen Sulphur None Hint 35. State the function of oxytocin. Controls blood sugar Stimulates uterine contraction Increases heart rate Regulates metabolism None Hint 36. Which of the following is not a function of salt bridge? It prevents accumulation of charges in the two half cells. It completes the outer circuit. It completes the inner circuit. It maintains electrical neutrality. None Hint 37. 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 38. Choose the most electronegative element from the following: Oxygen Nitrogen Sulphur Fluorine None Hint 39. Vulcanization of rubber produces: an elastomer a plasticizer a thermoplastic polymer a thermosetting polymer None Hint 40. 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 41. The 3d series of transition metals/elements is from: Scandium to Zinc Actinium to Lawrencium Scandium to Copper Yttrium to Lanthanum None Hint 42. The consequence of lanthanide contraction is: 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. Radii of elements of second transition series increases. None Hint 43. The 3d series of transition metals/elements is from: Scandium to Copper Scandium to Zinc Actinium to Lawrencium Yttrium to Lanthanum None Hint 44. State the function of oxytocin: Controls digestion Controls blood pressure Controls muscle contraction Controls childbirth and lactation None Hint 45. 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 False Never true Always true None Hint 46. The extent of ionisation of weak acids or bases and the strength of weak acids or bases are: inversely related to each other exponentially related to each other not related to each other directly related to each other None Hint 47. What is the oxidation number of atoms in their elemental form? -1 +1 +2 0 None Hint 48. 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 49. 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 50. Enthalpy is a __ function. Closed Open State Path None Hint 51. Geometrical isomerism is shown by isomers... possible for coordination number: less than or equal to four greater than or equal to two equal to two greater than or equal to four None Hint 52. 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 125 g/mol 100 g/mol 75 g/mol None Hint 53. A system which can exchange energy but not matter with the surroundings is called: Open system Closed system Isolated system State system None Hint 54. 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 55. 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 56. What is the oxidation number of atoms in their elemental form? 0 −1 +1 +2 None Hint 57. 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 Molality Molarity None Hint 58. Low density polyethylene: has linear chain of molecules is packed in a compact fashion is harder and stronger than polypropylene has branching in polymer chains None Hint 59. Why is the shape of ammonia molecule trigonal pyramidal? Due to repulsion between lone pair electrons. Due to the presence of three bonded pairs only. Because of double bonds between nitrogen and hydrogen. Because of linear arrangement of atoms. None Hint 60. The empirical formula of fructose is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) CH₂O None of these CHO CHO₂ None Hint 61. 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 62. State one physical property which is same for lithium and magnesium. Large atomic radius Low electronegativity High melting point Low density None Hint 63. 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 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. None Hint 64. Complete and balance the following chemical equations: XeF6 + 2H2O → XeOF4 + 2HF XeF4 + 4HF XeO2F2 + 4HF XeO3 + 6HF None Hint 65. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 119, 80, 119 199, 80, 199 80, 119, 80 80, 199, 80 None Hint 66. 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 +20 kJ +80 kJ −1574 kJ mol⁻¹ None Hint 67. One atomic mass unit is equal to: Mass of one mole of C–12 atoms ÷ 12 Mass of one mole of C–12 atoms Mass of one C–12 atom × 12 Mass of one C–12 atom ÷ 12 None Hint 68. 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 Law of constant proportions Postulates of Dalton’s atomic theory None Hint 69. 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 acceptance of proton and donation of proton respectively donation of proton and acceptance of proton respectively None Hint 70. Adiabatic processes proceeds with: A change in pressure A change in temperature An exchange of heat between the system and the surroundings No change in temperature None Hint 71. Which liquid pairs show negative deviation from Raoult's Law? Water and ethanol Benzene and toluene Chloroform and acetone Water and salt solution None Hint 72. What are ozonides? Give chemical equation for their formation. Compounds formed by oxygen and water Compounds formed by hydrogen and ozone Compounds formed by alkenes and ozone Compounds formed by alkali metals and ozone None Hint 73. 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 27.59% 72.41% None Hint 74. Low density polythene: Has linear chain of molecules Is harder and stronger than polypropylene Has branching in polymer chains Is packed in a compact fashion None Hint 75. Give the mathematical expression of de-Broglie equation. ) λ = mv / h λ = h × mv λ = h / mv λ = m / hv None Hint 76. 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 B. +20 kJ +80 kJ −1574 kJ mol⁻¹ None Hint 77. 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 - Basic, SO2 - Amphoteric, Al2O3 - Acidic FeO - Amphoteric, SiO2 - Basic, SO2 - Acidic, Al2O3 - Basic FeO - Acidic, SiO2 - Amphoteric, SO2 - Basic, Al2O3 - Acidic None Hint 78. Vulcanization of rubber produces: an elastomer a thermosetting polymer a thermoplastic polymer a plasticizer None Hint 79. 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 Substitution, Addition, Elimination Reduction, Oxidation, Addition None Hint 80. The factors affecting conductivity of an electrolyte are: nature of the electrolyte and temperature temperature and concentration nature of the electrolyte, temperature and concentration nature of the electrolyte and concentration 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 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 82. 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 250 g/mol 200 g/mol 100 g/mol None Hint 83. Write True (T) or False (F) for the following statements: Raoult’s law is applicable only if the liquids are volatile and miscible. Depends on temperature Sometimes true False True None Hint 84. How are hormones transported to their place of action? By diffusion By air By water By blood 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
