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Chapter 4
Liquids & Solids
1. Which one is the example of cubic crystals?
- Graphite
- Sugar
- Borax
- Diamond
2. The boiling point of the halogens:
- Increase down the group
- Decrease down the group
- Remains constant
- can’t be predicted
3. Vapor pressure of a liquid in a closed container depends upon:
- Surface area of container
- Temperature
- Amount of liquid
- All of these
4. A crystal system in which all the axes and angles are unequal is called:
- Tetragonal system
- Monoclinic system
- Triclinic system
- Cubic system
5. At Murree hills water boils at:
- 98°C
- 100°C
- 0°C
- 50°C
6. Coordination number of Nation in NaCl is:
- One
- Two
- Four
- Six
7. Water may boil at 120°C when external pressure is:
- 369 torre
- 700 torr
- 760 torr
- 1489 torr
8. Crystals formed due to London forces of interaction are:
- lonic
- Covalent
- Molecular
- Metallic
9. Forces which are preset between ions and water molecules are
- Dipole-induced dipole forces
- Dipole-dipole forces
- Ion dipole forces
- London dispersion forces
10. How many allotropic forms are present in carbon?
- TWO
- Three
- Four
- Five
11. Transition temperature of tin is
- 95.5°C
- 13.2°C
- 0°C
- 128.5°C
12. The crystal of diamond is:
- Ionic
- Covalent
- Molecular
- Metallic
13. Liquid hydrocarbon is:
- Methane
- Propane
- Ethane
- Hexane
14. The example of hexagonal system is:
- Sulphur
- Naci
- Graphite
- Diamond
15. Hydrogen bonding is strongest in:
- Hl
- HBO
- HCI
- HF
16. Allotropy is the property of:
- Element
- Compound
- Mixture
- Ions
17. Ice occupies more space than liquid water.
- 9%
- 10%
- 11%
- 12%
18. Structure of ice is:
- Tetrahedral
- Octahedral
- Cubic
- Triclinic
19. In orthorhombic crystal, the unit cell dimensions are:
- a = b = ca = B = y = 90°
- a+b+ca = B = y = 90°
- Sab+ca = B = y + 90°
- a+b+c a = B = y + 90°
20. London dispersion forces are significant for:
- Polar molecules
- Ionic solids
- Metals
- Non polar molecules
21. Which substance shows anisotropic behavior in electrical conductivity?
- Diamond
- Graphite
- KC
- Ice
22. The boiling points of higher alkanes are greater than those of lower alkanes due to the reasons that:
- Higher alkanes have greater number of atoms
- The polarizability of higher alkanes is greater
- Higher alkanes have zigzag structures
- Higher alkanes have greater hydrogen bonding
23. Water has maximum density at:
- 4°C
- 0°C
- 100°C
- 10°C
24. K2SO4 and K2CrO4 are isomorphic solids and exist in:
- Cubic form
- Orthorhombic form
- Trigonal form
- Tetragonal
25. The transition temperature of KNO3 is:
- 13.2°C
- 95.5°C
- 128oC
- 32.02oC
26. The distillation of liquid under reduced pressure is called:
- Destructive distillation
- Vacuum distillation
- Fractional distillation
- Simple distillation
27. The structure of sodium chloride is:
- Body centered cube
- Face centered cube
- Simple cube
- None
28. The forces which are present between the ions and the water molecules are known as:
- Dipole induced forces
- Ion-dipole forces
- Dipole-dipole forces
- London dispersion forces
29. LiF is a crystalline substance and has:
- Ionic crystals
- Metallic crystals
- Covalent crystals
- Molecular crystals
30. Which of the following liquid has highest boiling point?
- HCI
- HBr
- CHO
- Br2
31. The number of Nations which surround each cl ion in the NaCl crystal is:
- 4
- 6
- 8
- 12
32. Liquids evaporate at every temperature. When the temperature becomes constant for a liquid then:
- Rate of evaporation is greater than the rate of condensation.
- The rate of condensation is greater than the rate of evaporation.
- The rate of condensation and evaporation becomes equal
- Depends upon the nature of the liquid
33. Ionic solid don’t conduct the electrical current because:
- ons do not have translatory motion
- Free electrons are less
- The coordination number of the ion is very high
- Strong covalent bonds are present in their structure
34. Amorphous means:
- Ordered
- Arranged
- Shaped
- Shapeless
35. Polarizability is measure of extent of distortion:
- Qualitative
- Quantitative
- Systematic
- None of these
36. Heat change for one mole of a solid during converting into liquid is called:
- Molar heat of vaporization
- Molar heat of sublimation
- Molar heat of fusion
- Enthalpy change
37. Which of the following does not form a molecular crystal?
- Ice
- Graphite
- Iodine
- Sugar
38. Evaporation causes:
- Cooling
- Heating
- Boiling
- irritation
39. Diamond and graphite are example of:
- Isomorphism
- Polymorphism
- Isomerism
- Allotropy
40. Dipole-induced dipole forces are also called:
- London dispersion forces
- Debye forces
- Huckel forces
- Electrostatic forces
41. The size of diameter of double helix of DNA is:
- 18-20 Å
- 20-30 Å
- 1-10 Å
- 25-30 Å
42. Which statement is incorrect about tetragonal crystal system?
- a = b = c
- a = b = c
- a = B = y = 90°
- NONE
43. Crystal system shown by diamond is:
- Cubic
- Tetragonal
- Monoclinic
- Hexagonal
44. The strongest acid among halogen acids is:
- HF
- HCI
- HBO
- HI
45. The number of Cl+ ions per unit cell of NaCl is:
- 8
- 6
- 4
- 2
46. How much more space is occupied by water on freezing:
- 9%
- 8%
- 7%
- 6%
47. Boiling point of H2O at Mount Everest would be:
- 98°C
- 100°C
- 101°C
- 69oC
48. Allotropy is the property of:
- Compound
- Element
- Atoms
- Mixture
49. Hydrogen bonding is maximum for:
- Ethanol
- Water
- Benzene
- Diethyl ether
50. The existence of an element in more than one crystalline forms:
- Allotropy
- Isotropy
- Isomorphism
- Polymorphism
51. Dry ice (Solid CO2) is an example of solid:
- Covalent
- Molecular
- Ionic
52. Glycerine decomposes at its:
- Melting point
- Boiling point
- Freezing point
- Critical point
53. Which one is the following is a pseudo solid:
- CaF2
- Naci
- Borax
- Glass