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Class 11 Chemistry
States Of Matter Chapter 5
Quiz 1
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Dipole-dipole forces act between molecules possessing:
0%
No dipole moment
0%
Electronic charges
0%
Permanent dipole
0%
Induced dipole
Partial charges are involved in:
0%
Dipole-dipole forces
0%
London forces
0%
Dipole-induced dipole forces
0%
Vander waals forces
Interaction energy associated with London force is
0%
Proportional to the third power of the distance between two interacting particles.
0%
Proportional to the sixth power of the distance between two interacting particles.
0%
Inversely proportional to the sixth power of the distance between two interacting particles.
0%
Inversely proportional to the third power of the distance between two interacting particles.
The force of attraction between two permanent dipoles is known as
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Dipole - dipole force
0%
London force
0%
Repulsive force
0%
Dipole Induced dipole force
Dipole-dipole interaction energy between stationary polar molecules is:
0%
Inversely proportional to the third power of the distance between two interacting particles
0%
Directly proportional to the third power of the distance between two interacting particles
0%
Directly proportional to the sixth power of the distance between two interacting particles
0%
Inversely proportional to the sixth power of the distance between two interacting particles
For dipole-induced dipole forces, interaction energy is:
0%
Inversely proportional to the third power of the distance between two interacting particles
0%
Directly proportional to the third power of the distance between two interacting particles
0%
Inversely proportional to the sixth power of the distance between two interacting particles
0%
Directly proportional to the sixth power of the distance between two interacting particles
London forces are important only at:
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Distance between the two particles
0%
Long distances
0%
Short distances
0%
Infinite distance
The strength of London forces do not increase with the increase in
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The distance between two interacting particles
0%
Surface area of molecule
0%
Number of electrons
0%
Molecular size
London forces are also known as
0%
vander Waals forces
0%
Dipole-dipole forces
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Dispersion forces
0%
Keesom forces
In dipole-induced dipole forces, the dipole moments (μ) of polar and non polar molecules are
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μ = 0 and μ < 0
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μ > 0 and μ = 0
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μ < 0 and μ > 0
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μ = 0 for both
The influence of permanent electrical dipole in dipole-Induced Dipole forces
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Depend on the ionic radii
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Decreases with the decrease in size of the molecule
0%
Increases with the increase in size of the molecule
0%
Does not depend on the size of the molecule
Magnitude of repulsion rises as the distance separating the molecules:
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Remains constant
0%
Increases
0%
Has no effect on repulsion
0%
Decreases
A strong type of dipole-dipole interaction is:
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Electrostatic bond
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Covalent bond
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Ionic bond
0%
Hydrogen bond
High polarisability increases the strength of:
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Dipole-dipole forces
0%
Dipole-induced dipole forces
0%
Vander waals forces
0%
London forces
The force of attraction between the polar molecules having permanent dipole and the molecules lacking permanent dipole is
0%
Dipole Induced dipole force
0%
Dipole - dipole force
0%
Repulsive force
0%
London force
Atoms and non-polar molecules are electrically:
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Polarized
0%
Ionized
0%
Symmetrical
0%
Unsymmetrical
Among the following, the force that is not included in vander Waals forces is
0%
Dipole-dipole forces
0%
Dipole-induced dipole forces
0%
London forces
0%
Covalent bond
A polar and a non-polar molecule interact by:
0%
London forces
0%
Dipole-induced dipole forces
0%
Hydrogen bond
0%
Dipole-dipole forces
The partial charges present on an atom are
0%
Equal to the unit charge
0%
Greater than the unit charge
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Less than the unit charge
0%
Does not depend on the unit charge
Dipole-dipole forces are:
0%
Equal in strength to London forces
0%
Stronger than London forces
0%
Not comparable to London forces
0%
Weaker than London forces
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