Chemistry 1st Year Chapter 4 Liquids and Solids Notes MCQs Bank

chemistry 11th notes chapter 4

1. Kerosene oil is used to kill mosquitoes because it has surface tension:


2. The sudden expansion of the gas from high pressure towards the low-pressure causes?


3. Which one of the following is isotropic:


4. Polarizability generally down the group:


5. Ammonia shows the maximum boiling point among the hydrides of the 5th group because:


6. The number of amino acid units for each turn of helix, on average are:


7. When external pressure is 23.7 torr, boiling point of water is:


8. The boiling point increases down the zero group element due to:


9. The forces which are present between the ions and water molecules are known as:


10. Which of the liquid has the lowest vapor pressure?


11. The graph between pressure and the inverse of volume at constant temperature and number of moles:


12. Which substance shows anisotropic behaviour in electrical conductivity?


13. Hydrogen bonding is extensively present in protein which forms the spiral. The hydrogen bond being produced is between.


14. If both temperature and volume of a gas are doubled, the pressure:


15. 110°C boiling water of water corresponds to the external pressure:


16. Vapour pressure of water at 100°C is:


17. The strength of hydrogen bonding is:


18. Ice is _____ crystal.


19. The attractive forces between the partially positive end of one molecule and partial negative end of other molecules are called:


20. The number of molecules in 0.0112m³ of methane at 25°C and pressure of 760mm Hg is:


21. Gases deviate from ideal behavior at high pressure. Which of the following is correct for non-ideality:


22. Rising of a wetting liquid in a capillary tube is due to:


23. The conversion of vapours back into their liquid state is called:


24. The molecules of gas show more deviation from ideal behavior at low temperature, because;


25. Which one of the following is pseudo solid:


26. Plastics are amorphous solids and:


27. Which solids are called true solids:


28. Ice occupies more space than liquid water:


29. The crystal of diamond is:


30. Hydrogen bonding involves in:


31. Evaporating water depends upon the following:


32. Molar heat of vaporization of water is:


33. Which solids does not contain covalent bonds?


34. Which pair of compounds are isomorphic in nature:


35. Which one of the following liquid has low vapour pressure at 25°C:


36. Crystalline solids do not have:


37. The number of CI ions per unit cell of NaCl are:


38. Lower alcohols in spite of being organic are soluble in water because:


39. Molecular crystals are generally:


40. Ice float on the liquid water because:


41. Evaporation of water is possible at:


42. Which one is the form of a general gas equation?


43. The vapor pressure of a liquid depends upon the following:


44. Evaporation is designated as a cooling process because of the reason:


45. Which one is false for evaporation:


46. The shape of diamond crystal is:


47. Vapour pressure is not affected by:


48. Type of hybridization in diamond:


49. A solid may be made up of:


50. The boiling point of H₂O is 100°C while that of C₂H₅OH is 78.5°C. The reason is that:


51. Which of the following will have the same number of molecules at STP:


52. In a closed vessel of 1000 cm³, H₂ gas is heated from 27°C to 127°C. Which statement is not correct?


53. Liquid crystal is discovered by:


54. Which pair of molecules have Debye forces in them:


55. The overall structure of the diamond looks:


56. Instantaneous dipole and induce dipole force is also called:


57. a≠ b ≠ c≠, α≠β≠γ≠90° is representation of crystal system:


58. The distillation of a solution under reduced pressure is called?


59. At 1atm pressure, a liquid 1 has the boiling point less than a liquid 2, what can we predict about both the liquids:


60. Water has maximum density at:


61. Which one of the following does not show hydrogen bonding:


62. In liquids, intermolecular forces are:


63. Existence of an element in more than one form is known as:


64. The partial pressure of oxygen in the lungs is:


65. The crystals formed due to London forces of interaction are:


66. Bucky balls is an allotropic form of:


67. The boiling point of a compound is mostly raised by:


Short Questions

1. Amorphous solid like glass is also called super cooled liquid.Why?
2. Briefly consider some of the effects on our lives if water has only a very weak hydrogen bonding present among its molecules?
3. Cleavage is an anisotropic behaviour. Explain it.
4. Cleavage of crystals is anisotropic behaviour?
5. Crystals have their own habits.Justify it?
6. Define allotropy. Give its one example.
7. Define isomorphism and polymorphism with examples.
8. Define molar heat of fusion and molar heat of vaporization.
9. Define polymorphism. Give an example.
10. Define polymorpism and metamorphism.Give one example of each?
11. Define transition temperature. Give two examples.
12. Describe that heat of sublimation is greater than heat of vaporization.
13. Diamond an allot-rope of graphite is hard and an electrical insulator.Why?
14. Diamond and graphite which are allot-ropes are covalent solids.Graphite can be used as a lubricant but diamond cannot be?
15. Diamond is hard and an electrical insulator. Give reason?
16. Earthen ware vessels keep water cool. Explain.
17. Explain why evaporation takes place at all temperatures?
18. Give four properties of molecular solids.
19. Give the reason for low boiling point of HF(19.5 ᵒC)as compared to H₂O(100 ᵒC) although the hydrogen in HF is stronger than that of water.
20. H-bonding is present i chloroform and acetone.Justify it?
21. Heat of sublimation of iodine is very high, justify it.
22. HF is weaker acid than HCl. Why?
23. How are liquid crystals used to locate veins, arteries, infections and tumors?
24. How do you justify that the structure of ice is just like that of diamond?
25. How does the solid maintain a definite volume and shape?
26. How in a very cold water fish in garden ponds owe their lives to hydrogen bonding?
27. How is that some of crystalline solid substances show anisotropy?
28. How the cleaning action of soaps and detergents is partially due to the hydrogen bonding?
29. How the liquid crystals help in the detection of blockages in veins and arteries.
30. How the rate of evaporation depends on the surface area?
31. Ice floats on water.justify it?
32. Ice occupies more space than water. Give reason.
33. In a very cold winter fish in garden ponds owe their lives to hydrogen bonding?
34. In the hydrogen bonded structure of HF which is the stronger bond;the shorter coalescent bond or the longer hydrogen bond between different molecules?
35. Ionic crystals don’t conduct electricity in the solid state.Why?
36. Ionic solids do not conduct electricity in solid state. Give reason.
37. Is it true that polar compounds are soluble in polar solvents?
38. London dispersion forces are weaker than dipole-dipole forces.Why?
39. Lower alcohols are soluble into water but hydrocarbons not. Give reason.
40. Lower alcohols are water soluble but corresponding alkalies are insoluble in water.Why?
41. Metals are good conductors of heat and electricity.The conduction of electrical current decreases with the increase of temperature.Why?
42. Molecular solids are soft and easily compressible.why?
43. Naphthalene can be purified by sublimation process.why?
44. Sodium is softer than copper but both are very good electrical conductors?
45. Solid and liquid sodium is a good conductor of electricity but NaCI is only in molten state.Give reasons?
46. Solid sodium is a good conductor of electricity but solid sodium chloride is not.Give reason?
47. Steam causes more severe burns than does the boiling water.Give reason?
48. Symmetry is one of the properties of a crystalline solid.Justify it?
49. The transition temperature is given by elements having allotropic forms and by compounds showing polymorphism.justify?
50. The vapor pressure of diethyl ethyl is higher than water at same temperature?
51. Transition temperature is the term used for elements as well as compounds. Explain.
52. Vacuum distillation can be used to avoid decomposition of sensitive liquids. Explain.
53. Water and ethanol can mix easily in all proportions.Why?
54. Water and ethanol can mix in all proportions. Give reason.
55. Water is a liquid at room temperature but H₂S is a gas.Give reason?
56. What are crystallographic elements?
57. What are Debye forces?
58. What are dipole-dipole forces of attraction? Explain with examples.
59. What are dipole-induced dipole force?
60. What are London dispersion forces?
61. What is cleavage plane?
62. What is Isomorphism? Give example?
63. What is meant by dynamic equilibrium? Give an example.
64. What is polarizability?How its increase down the group in noble gases is responsible for increase in melting and boiling points?
65. What is reason for low lattice energy of NaCI as compared to MgCI₂?
66. What is relationship between polymorphism and allotropy?
67. What is the origin of the inter-molecular forces in water?
68. Why boiling point of water is different at Murree Hills and at Mount Everest?
69. Why boiling point of water is greater than HF?
70. Why different liquids evaporate at different rates even at the same temperature.
71. Why dipole-dipole forces are much stronger than dipole-induced dipole forces?
72. Why evaporation causes cooling?
73. Why graphite is an-isotropic in electrical conductivity?
74. Why heat of sublimation of iodine is very high?
75. Why ice floats over the surface of water?
76. Why inter molecular forces are weaker than intramuscular forces?
77. Why ionic solids are highly brittle?
78. Why most of the molecular solids have low melting and boiling points?
79. Why the electrical conductivity of metals decrease by increasing temperature?
80. Why the heat of vaporization of water is greater than that of CH₄?
81. Why the ionic crystalline solids have high melting points?
82. Why the ionic crystals are highly brittle?
83. Why the lattice energy of NaCI is greater than that of KCI which is greater than KBr?
84. Why the melting and boiling points of alkalies increase with increase in molar masses and are less than that of H₂O?
85. Why the melting and boiling points of halogens and noble gas increase down the group?
86. Why vapor pressure increases with temperature?
87. Write a brief note on solubility oh hydrogen bonded molecules.
88. Write down two applications of liquid crystals.
89. Write two properties of molecular solids.

Long Questions

1. Define hydrogen bonding. How does it explain the solubility of hydrogen bonded molecules and structure of ice?
2. What are solids? Give general properties of solids. How do you diferentiate between crystalline solids and amorphous solids?
3. Explain hydrogen bonding in NH₃, H₂O and HF. How is it helpful in explaining the structure of ice?
4. Classify solids on the basis of Bonding
5. Write brief not on Anisotropy and polymorphism.
6. What is boiling point? What is the effect of external pressure on the boiling point? Why the temperature remains constant at boiling point although heat is continuously supplied.
7. What are ionic solids? Give their properties in details.
8. What are liquid crystals? Give their uses in daily life.
9. What are molecular solids? Give examples and explain their properties?
10. Write down four properties of molecular solids.
11. What is hydrogen bonding? Discuss hydrogen bonding in biological properties.
12. What is vapor pressure of a liquid? Also discuss its measurement by Manometric method.
13. Discuss London dispersion forces. Elaborate two factors on which it depends.
14. Define unit cell. Draw diagram and give dimensions of hexagonal system of crystals.
15. Define ionic solids. Discuss properties of ionic solids in detail
16. Classify solids on the basis of Bonding. How ionic solids are formed. Give two properties of ionic solids.
17. Discuss electron gas theory to explain the properties of metallic solids.
18. Explain electron pool theory.
“19. Explain with the help of a diagram
(i) Cubic close packing in the structure of metals.
(ii) Hexagonal close packing in the structure of metals.”

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