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Online Tests
Chemistry Fsc Part 1 Chapter 4 Online Test MCQs With Answers
Question # 1
London dispersion force are the only forces present among the.
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Molecules of water in liquid state
Atoms of helium in gaseous state at high temperature
Molecule of solid iodine
Molecules of hydrogen chloride gas
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Question # 2
Exceptionally low acidic strength of HF is due to.
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Strong polar bond between H and F
Smaller size of fluorine
Strong hydrogen bonding
electronegativity of fluorine
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Question # 3
On which factor boiling point of a liquid depends.
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Amount of the liquid
Shape of the container of the liquid
Type of burner used for boiling
External pressure
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Question # 4
The repulsion of electronic clouds of the molecules are responsible for the attractive forces among the molecules. These forces are
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Dipole-induced dipole forces
Ion-dipole forces
Instantaneous dipole-induced dipole forces
Dipole-dipole forces
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Question # 5
Acetone and chloroform are soluble in each other due to.
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Intermolecular hydrogen bonding
Dipole dipole interaction
Instantaneous dipoles
All of the above
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Question # 6
The boiling point of water at Murree Hills.
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90
o
C
98
o
C
100
o
C
120
o
C
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Question # 7
In which system all the three axes are of equal length and all angles are at right angle.
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Cubic
Tetragonal
Orthorhombic
Hexagonal
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Question # 8
The boiling point of glycerin at one atm is.
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280
o
C
290
o
C
100
o
C
110
o
C
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Question # 9
Polymorphic substances have
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Same physical and chemical properties
Different physical and chemical properties.
Same physical but different chemical properties
Different physical and same chemical properties.
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Question # 10
Boiling point of a liquid is high when
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There is no hydrogen bonding
Dipole moment is zero
Inter molecular forces are weak
Hydrogen bonding is present
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Question # 11
The boiling point of pure water at 1 atm pressure is.
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98
o
C
100
o
C
69
o
C
120
o
C
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Question # 12
The distillation of a solution under reduced pressure is called
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Fractional distillation
Destructive distillation
Distillation
Vacuum distillation
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Question # 13
Diamond is bad conductor because.
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It has a tight structure
It has a high density
It is transparent to light
There are o free electros present in the crystal of diamond to conduct electricity.
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Question # 14
In order to mention the B.P of water at 110
o
C the external pressure should be.
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Between 760 torr and 1200 torr
Between 200 torr and 760 torr
765 torr
Any value of pressure
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Question # 15
NaCI is face centered cubic structure. The Na ion at the face of the unit cell is shared by
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2-unit cells
4-unit cells
Only one unit cell
8-unit cells
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Question # 16
The molecule of CO2 in dry ice form the.
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Ionic crystals
Covalent crystals
Molecular crystals
Any type of crystals
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Question # 17
Long chains of amino acids are coiled about one another into a spiral by
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Covalent bond
Ionic bond
Hydrogen bond
Van Der Waal's forces
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Question # 18
Isomorphic crystals show
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Same chemical properties
Same physical properties
Same crystalline form
Same melting point
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Question # 19
Which one of the following substances is not amorphous
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Polymer
Rubber
Glass
AgNO
3
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Question # 20
Conductivity of metal decreases by increasing temperature because.
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Atoms are converted to ions
Atoms oscillates and hinder the movement of free electrons.
Ions are converted into atoms
Velocity of mobile electrons increases
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Question # 21
The polarizabilities of elements mostly increase down the group due to the reason that
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The atomic numbers increase
Number of protons increase
Number of shells increase along, with increase of shielding effect
The behavior of the elements remain the same
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Question # 22
Ionic solids are characterized by.
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Low melting points
High vapour pressures
Good conductivity in solid state
Solubility in polar solvents
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Question # 23
Ionic solid are characterized by.
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Low melting point
Good conductivity in solid state
High vapours pressure
solubility in polar solvent
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Question # 24
When liquid water changes to ice its volume expands. The expansion in volume is.
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5%
9%
10%
18%
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Question # 25
When water freezes at 0°C, its density decreases due to
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Cubic structure of ice
Empty spaces present in the structure of ice
Change of bond lengths
Change of bond angles
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