Chemistry Nios Plus Two PQ Welcome to your Chemistry Nios Plus Two PQ 1. The 3d series of transition metals/elements is from: Scandium to Zinc Scandium to Copper Actinium to Lawrencium Yttrium to Lanthanum None Hint 2. Define bond enthalpy. Calculate the bond enthalpy of CH4 molecule if average bond enthalpy of C-H bond is 414 kJ/mol. Energy released in bond formation Energy required to break one mole of bonds in gaseous molecules Energy required to break ionic bonds Energy change in electron transfer None Hint 3. Which compound forms ethyl carbocation? Ethene Ethanol Ethyl chloride Ethane None Hint 4. 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 True False 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: Postulates of Dalton’s atomic theory Law of constant proportions Law of conservation of mass Law of multiple proportions None Hint 6. Predict the shape of methane molecule on the basis of VSEPR theory. Linear Trigonal planar Octahedral Tetrahedral None Hint 7. What is the shape and magnetic behaviour of Ni(CO)₄? Linear and diamagnetic Tetrahedral and diamagnetic Square planar and paramagnetic Octahedral and paramagnetic None Hint 8. What is the pH of a 0.001 M aqueous solution of HCl? 4 1 2 3 None Hint 9. 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) B. +20 kJ −1574 kJ mol⁻¹ +1574 kJ mol⁻¹ +80 kJ None Hint 10. State the function of oxytocin. Increases heart rate Controls blood sugar Stimulates uterine contraction Regulates metabolism None Hint 11. Why is chloroform stored in dark colored bottles? To protect from light which decomposes it To avoid evaporation For aesthetic reasons To keep it cool None Hint 12. 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 13. 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 14. 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 15. The factors affecting conductivity of an electrolyte are: nature of the electrolyte, temperature and concentration nature of the electrolyte and temperature temperature and concentration nature of the electrolyte and concentration None Hint 16. State the function of oxytocin: Controls blood pressure Controls muscle contraction Controls childbirth and lactation Controls digestion None Hint 17. Which type of compound water is? Covalent Metallic Ionic Hydrogen None Hint 18. 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 19. 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 20. 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 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. None Hint 21. The 3d series of transition metals/elements is from: Actinium to Lawrencium Scandium to Copper Scandium to Zinc Yttrium to Lanthanum None Hint 22. Complete and balance the following chemical equations: NaCl + Conc. H2SO4 (423K) → NaHSO4 + Cl2 NaHSO4 + HCl NaHSO4 + HCl Na2SO4 + HCl None Hint 23. 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 50 g/mol 100 g/mol 75 g/mol None Hint 24. Lanthanide contraction is due to increase in: Atomic number Size of 4f orbital Shielding by 4f electrons Effective nuclear charge None Hint 25. 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 26. 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 1,3-Dibromo-4-ethylbenzene 1,4-Dibromo-3-ethylbenzene 1,2-Dibromo-4-ethylbenzene None Hint 27. Geometrical isomerism is shown by isomers... possible for coordination number: equal to two less than or equal to four greater than or equal to four greater than or equal to two None Hint 28. Which liquid pairs show negative deviation from Raoult's Law? Water and ethanol Water and salt solution Benzene and toluene Chloroform and acetone None Hint 29. Low density polythene: Has branching in polymer chains Is harder and stronger than polypropylene Has linear chain of molecules Is packed in a compact fashion None Hint 30. 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 31. Vulcanization of rubber produces: an elastomer a thermosetting polymer a plasticizer a thermoplastic polymer None Hint 32. Enthalpy is a __ function. path closed isolated state None Hint 33. 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 34. A system which can exchange energy but not matter with the surroundings is called: Isolated system Open system State system Closed system None Hint 35. 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 36. 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 37. Vulcanization of rubber produces: a thermosetting polymer a thermoplastic polymer an elastomer a plasticizer None Hint 38. 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 39. The percentage of oxygen in Fe₃O₄ is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) 27.59% None of these 27.89% 72.41% None Hint 40. 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 Fatty acid; methyl group Alcohol; hydroxyl group Fatty acid; carboxyl group None Hint 41. What is the oxidation number of atoms in their elemental form? +2 +1 0 -1 None Hint 42. Give the mathematical expression of de-Broglie equation. λ = h × mv ) λ = mv / h λ = h / mv λ = m / hv None Hint 43. Enthalpy is a __ function. Path State Open Closed None Hint 44. Choose the most electronegative element from the following: Oxygen Nitrogen Sulphur Fluorine None Hint 45. Give the mathematical expression of de-Broglie equation: p = mv λ = h/mv F = ma E = mc² None Hint 46. Match the following: Yellow and transparent crystalline substance → (4) Sulphur dioxide Tailing of mercury → (1) Conc. Sulphuric acid Decomposed in a strong beam of light → (3) Ozone Blue CuSO4 → white CuSO4 → (2) Rhombic sulphur None Hint 47. State Heisenberg’s uncertainty principle. Momentum is always zero. 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. 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 two Equal to two Greater than or equal to four Less than or equal to two None Hint 49. 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 50. A system which can exchange energy but not matter with the surroundings is called __ system. open isolated path closed None Hint 51. Write the IUPAC name of the compound: CH3-CH2-CH(Cl)-CH2-CH3 2-Chloropentane 3-Chloropentane 1-Chloropentane 4-Chloropentane None Hint 52. What is the oxidation number of atoms in their elemental form? −1 0 +2 +1 None Hint 53. What is the active component of soap? What is the polar part in: (i) a soap molecule (ii) a synthetic detergent molecule Ketone, -NH2 Ester, -OH Hydrocarbon chain, -COONa Alcohol group, -CH3 None Hint 54. 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 55. State Heisenberg’s uncertainty principle: E = hv ΔE · Δt = h Δx · Δp ≥ h/4π v = λf None Hint 56. State the oxidation number of N and Cl in NCl₃. N = +1, Cl = −3 N = +3, Cl = −1 N = +5, Cl = −1 N = −3, Cl = +1 None Hint 57. Which of the following is equal to 1 mole O₂? 60.22 × 10²² molecules of Oxygen 6.022 × 10²³ molecules of Oxygen 60.22 × 10²³ atoms of Oxygen 6.022 × 10²³ atoms of Oxygen None Hint 58. (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 ∝ voltage applied Mass ∝ concentration Mass ∝ time taken Mass ∝ charge passed None Hint 59. Choose the most electronegative element from the following: Nitrogen Sulphur Oxygen Fluorine None Hint 60. How can you obtain ethanamine using Hofmann Bromomide reaction? Write chemical equation involved. From ethane From ethanoic acid From amide From ethyl bromide None Hint 61. One atomic mass unit is equal to: Mass of one mole of C–12 atoms Mass of one C–12 atom × 12 Mass of one mole of C–12 atoms ÷ 12 Mass of one C–12 atom ÷ 12 None Hint 62. Low density polyethylene: is harder and stronger than polypropylene has branching in polymer chains has linear chain of molecules is packed in a compact fashion None Hint 63. The consequence of lanthanide contraction is: 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. Radii of elements of second and third transition series becomes similar. None Hint 64. Adiabatic processes proceeds with: An exchange of heat between the system and the surroundings No change in temperature A change in temperature A change in pressure None Hint 65. 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 66. What is the shape and magnetic behavior of [Ni(CN)4]2- ion according to Valence Bond Theory (VBT)? Square planar and diamagnetic Linear and paramagnetic Octahedral and diamagnetic Tetrahedral and paramagnetic None Hint 67. 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 scattered uniformly in all directions. A few α-particles were deflected at large angles. The α-particles lost energy while passing through the foil. None Hint 68. In the species ₈₀¹⁹⁹Hg, the number of protons, neutrons and electrons respectively are: 80, 119, 80 119, 80, 119 199, 80, 199 80, 199, 80 None Hint 69. 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 70. 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 100 g/mol 200 g/mol 150 g/mol None Hint 71. Adiabatic processes proceeds with: an exchange of heat between the system and the surroundings a change in temperature a change in pressure no change in temperature None Hint 72. Why is the shape of ammonia molecule trigonal pyramidal? Because of linear arrangement of atoms. Because of double bonds between nitrogen and hydrogen. Due to repulsion between lone pair electrons. Due to the presence of three bonded pairs only. None Hint 73. State one physical property which is same for lithium and magnesium. Low density Low electronegativity High melting point Large atomic radius None Hint 74. What are ozonides? Give chemical equation for their formation. Compounds formed by hydrogen and ozone Compounds formed by alkali metals and ozone Compounds formed by oxygen and water Compounds formed by alkenes and ozone None Hint 75. 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 76. The ratio of the number of moles of one component to the total number of moles in the solution is known as: Normality Mole fraction Molality Molarity None Hint 77. How can you obtain propanamine using Hofmann Bromamide reaction? From alkene using HBr From alcohol using NH3 From amide using bromine and NaOH From alkane by nitration None Hint 78. What is the pH of a 0.001 M aqueous solution of HCl? 1 11 7 3 None Hint 79. How are hormones transported to their place of action? By water By diffusion By blood By air None Hint 80. 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 81. If 3d and 4p orbitals are to be filled in an atom by an electron then which orbital will be occupied first? 4p orbita 3d orbital Depends on the element Both at the same time None Hint 82. How are hormones transported to their place of action? Through bloodstream By diffusion Through nerves By active transport None Hint 83. Complete and balance the following chemical equations: XeF6 + 2H2O → XeO3 + 6HF XeF4 + 4HF XeOF4 + 2HF XeO2F2 + 4HF None Hint 84. The empirical formula of fructose is: Complete the following by given options below: (CHO, CH₂O, CHO₂, 27.59%, 72.41%, 27.89%) CHO₂ CH₂O None of these CHO 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
