FSC 1st year chemistry 4th chapter MCQs

Chapter 4: Liquids and Solids

In this article, the author has explained the most important chemistry MCQs from the fourth chapter( Liquids and solids ) of FSC chemistry. All the correct answers have been highlighted in blue color.

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1: The reason for high boiling point of H2O as compared to HF is

a) Absence of Hydrogen bonding in HF

b) The high electronegativity of O

c) The presence of more extensive hydrogen bonding in water

d) None of these

2: Boiling points of different  substances are given below

CH4 = 161 oC

C2H6 = -89 oC

Cl2 = -34.6 oC

F2 = -168 oC

a) Cl2 > C2H> CH> F2

b) C2H> CH> F> Cl2

c) Cl2 > F2 > CH>  C2H

d) F> CH>  C2H> Cl2

3: Ice is less dense than liquid water because of

a) More hydrogen bonds present in ice

b) Regular arrangement of water molecules in ice

c) Impurity of ice

d) None of these

4: All of the following phenomena are due to vaporization except

a) Drying up of wet soil

b) Melting of glaciers

c) Appearance of salts at the beds of salt lakes

d) Wilting of plant leaves

5: The vapour pressure of liquid depends on

a) The amount of liquid taken

b) Both amount and temperature

c) The volume of the vessel

d) The temperature of liquid

6: Increasing the temperature increases the rate of evaporation because

a) The intermolecular forces goes on weakening

b) Molecules lose their energies

c) Molecules collide with the walls of container more freely

d) None of these

7: Phenol has boiling point of 182oC at 1 atm pressure. If the atmospheric pressure were increased to 5 atm then the boiling point of phenol

a) Does not change

b) Increases

c) Decreases

d) None of these

8: Which of the following is not a crystalline solid?

a) Graphite

b) Rhombic Sulfur

c) Crystal glass

d) Grey tin

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9: Ionic solids are non-conductors of electricity because

a) They lack charged particles

b) They are neutral as a whole

c) The ions can’t show translator motions

d) Ions are static completely

10: All of the following are wrong except,

a) Ionic crystals are highly flexible

b) Brittleness in a crystal is due to the strong attractive forces between particles

c) Lattice energy of NaF is smaller than that of NaCl

d) Diamond and silicon carbide are only soluble in benzene as both have non-polar structures

11: Ethanol is much more soluble in water than ethyl ethanoate. Which one of the following statements correctly accounts for this?

a) Ethanol is polar but ethyl ethanoate is non-polar

b) A hydrogen bond forms, between the H-atoms of the –OH group in ethanol and O-atom of water molecule

c) Ethanol is non polar but ethyl ethanoate is polar

d) A Hydrogen bond between the O-atoms of the –OH group in ethanol and hydrogen atom of water molecule

12: Which of the followings elements in crystalline form, will have the lowest enthalpy change in vaporization?

a) Chlorine

b) Phosphorous

c) Argon

d) Silicon

13: Which of the following form molecular crystal?

a) Naphthalene

b) CO2 at -10 oC and room pressure

c) Diamond

d) Copper sulphate

14: Which of the followings is not true?

a) Evaporation causes cooling

b) Evaporation is a surface phenomenon

c) Evaporation is directly proportional to the external pressure

d) Evaporation is directly proportional to the temperature

15: Compounds with same Crystal shape but different composition and properties are called as

a) Allotrope

b) Polymorphs

c) Isomorphs

d) Isotopes

16: Which of the following has high heat of vaporization?

a) F2

b) Cl2

c) Br2

d) I2

17: Which of the following is most important characteristic property of the crystalline solids?

a) They are transparent

b) They have sharp melting point

c) They are quite hard

d) They are non-conductor of electricity in molten state

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18: Vapor pressure increases as temperature increases, this is because of ______?

a) K.E of the molecules increases

b) Intermolecular forces are weakened

c) Capability of the molecules to leave surface increases

d) All of the above

19: Which of the following is not true?

a) NaNO3 and CaCO3 are isomporphic

b) Rhombic sulfur and monoclinic sulfur are isomorphic to each other

c) The transition temperature of grey tin and white tin is 13.2 oC

d) SO42- and CrO42- are tetrahedral in geometry

20: Which of the following is not a property of crystalline solids?

a) Definite shape

b) Isotropy

c) High density

d) Low compressibility

21: Some substances are good conductor of electricity in both solid and liquid states. These substances are generally

a) Metallic Substances

b) Molecular solids

c) Ionic substances

 d) Covalent network solids

22: All of the following have cleavage planes except

a) Ionic Crystals

b) Molecular crystals

c) Covalent Crystals

d) Metallic Crystals

23: All of the following are network solids except

a) SiO2

b) Graphite

c) S8

d) Diamond

24: All of the following acids have hydrogen bonding in liquid state except

a) Sulfuric acid

b) Nitric acid

c) Hydrochloric acid

d) Hydrofluoric acid

25: Out of seven crystal systems how many can have both body-centered unit cell?

a) 3

b) 4

c) 3

d) 5

26: The empty spaces left in a hexagonal close packing of spheres in three dimensions is

a) 64%

b) 26%

c) 14%

d) 52.4%

27: Which of the following is not a close Packed arrangement?

a) BCC

b) CCP

c) HCP

d) All of these

28: Which of the following Statements about NaCl crystal is correct?

a) Cl ions are present at the corners and Na+ ions at the body center

b) Cl ions adopt bcc arrangement

c) Cl ions are packed following  ABC pattern of hexagonal close packing

d) Na+ ions are at the edge centers only

29: Which substances will conduct electric current in a solid state?

a) Diamond

b) Sodium Chloride

c) Graphite

d) Both b and c

30: Which choice is the best for the occurrence of hydrogen bonding?

a) H2O > C2H5OH > CHCl3

b) C2H5OH > CHCL3 > H2O

c) CHCl3 > H2O > C2H5OH

d) None of these

31: Dipole-dipole interactions are not present in

a) Ethanol

b) Acetone

c) n-butane

d) Highly compressed CO2

32: Which of the following is the correct order for the strength of intermolecular forces?

a) Ion-dipole > dipole-dipole > Hydrogen bonding > London forces

b) dipole-dipole > Hydrogen bonding > London forces > Ion-dipole

c) Hydrogen bonding > dipole-dipole > Ion-dipole > London forces

d) None of these

33: Which of the followings has the weakest intermolecular forces?

a) He

b) Ne

c) Ar

d) Xe

34: A permanent dipole is present in

a) Benzene

b) Xenon

c) Chlorobenzene

d) Iso-octane

35: The London-forces are not affected by

a) The number of atoms per molecule

b) The intermolecular distances

c) The size of the electronic cloud

d) None of these

36: Which of the followings is true for liquid crystals?

a) These cannot diffract light when heated

b) These can never conduct electricity at normal temperature

c) These may appear colored upon illumination by light, although previously colorless

d) All of these

37: The whole molecule of a liquid crystal

a) has the same response towards change in temperature

b) is a single unit

c) Is in motion alike when the substance is in the liquid state

d) All of these above are true

38: A crystal system with the crystallographic description

 A = b ≠ c and α = β = Υ = 90o is called

a) Trigonal

b) Hexagonal

c) Tetragonal

d) Monoclinic

39: Rhombohedral system is also called

a) trigonal system

b) Hexagonal system

c) Rhombic system

d) Orthorhombic system

40: High value of lattice energy shows

a) Strong attractions among the particles

b) Non-motile nature of particles

c) High charge density

d) Particles have a natural tendency to be in crystalline form

41: All of the followings are correct except

a) Molar heat of sublimation is greater than molar heat of vaporization

b) Change of matter from one state to the other is due to change in the energy content

c) Liquid crystals are sensitive to temperature

d) At dynamic equilibrium between a liquid and its vapors the rate of change on both sides is different

42: The crystal size of a solid may be changed by

a) Presence of an impurity

b) Time for crystallization

c) Solvent used for crystallization

d) All of these

43: The share that a particular unit cell gains from each of the particles present at the corners of a face centered cube is

a) One eight

b) One sixth

c) Two eight

d) None of these

44: Keeping in mind the concept of charge density compound having highest lattice energy is

a) KCl

b) LiBr

c) MgO

d) NaF

45: Isomorphic crystals always show

a) Same chemical properties

b) Same crystalline form

c) Same physical properties

d) Same melting point

46: Honey contain glucose and fructose along with some other ingredients, it has greater viscosity dye to

a) Hydrogen bonding

b) Irregular shape of the molecules

c) Irregular shape of the molecules and strong intermolecular forces

d) Greater molecular size

47: Boiling point of phosphine( PH3) is -87.8 oC while that of saline ( SiH4) is -111oC. Phophine has greater boiling point because

a) Dipole moment of PH3 is greater than that of SiH4

b) PH3 has greater molecular size

c) Molecular weight of SiH4 is less than that of PH3

d) Actually the boiling of SiH4 is greater than that of PH3

48: A chemist was able to measure the value of lattice energy of KCl to be 690 kj.mol. From this experiment he concluded that

a) Lattice energy of KBr is 630 kj/mol and that of KI is 665 kj/mol

b) Lattice energy of KBr is 765 kj/mol and that of KI is 730 kj/mol

c) Lattice energy of KBr is 665 kj/mol and that of KI is 630 kj/mol

d) Lattice energy of KBr is 730 kj/mol and that of KI is 765 kj/mol

49: If four different compounds have same molecular formula but different structures and hence intermolecular forces, the compound with the lowest boiling point would be that which has

a) Dipole-Dipole forces

b) Hydrogen bonding

c) Debye forces

d) London forces

50: Which of the following compounds do you expect to have the highest boiling point at the surface of the Dead Sea, the lowest place on the surface of earth?

a) H2S

b) H2O

c) NH3

d) PH3

51: Amorphous solids

a) Have sharp melting point

b) Undergo clean cleavage

c) Have regular geometry

d) Are isotropic in nature

52: Which of the following statements regarding covalent solids is incorrect?

a) These are very hard

b) These are very high melting points

c) These are good conductors of heat

d) These have high heats of fusion

53: Dry ice a

a) Molecular solid

b) Ionic solid

c) Atomic solid

d) Metallic solids

54: For a certain reaction, PV= 2 dm3 atm and volume is 4 dm3 then corresponding pressure is

a) 1 atm

b) 0.5 atm

c) 4 atm

d) 2 atm

55: The collision of molecules of gases at reduced volume causes?

a) Lower pressure

b) Medium pressure

c) Higher pressure

d) No effect on pressure

56: A graph between pressure and inverse of volume and constant temperature and number of moles?

a) Straight line parallel to y-axis

b) Straight line parallel to x-axis

c) Straight line passing through the origin

d) The curve showing the maximum

57: A gas occupies a volume of 4 dm3 at 25 oC and 1 atm pressure. What volume it occupies at STP?

a) 4.36 dm3

b) 325.4 dm3

c) 40.4 dm3

d) 3.66 dm3

58: If both temperature and volume of a gas doubled the pressure?

a) Also doubled

b) Is reduced to half

c) Increases four times

d) Remain unchanged

59: The gas which behaves more ideal under similar conditions of temperature and pressure?

a) He

b) CO2

c) H2

d) N2

60: Standard temperature and pressure (STP) of gases refers to?

a) 273 K and 760 mm Hg

b) 273 K and 76 mm Hg

c) 273 oC and 760 mm Hg

d) 273 oC and 76 mm Hg