Question # 1

At freezing point of water, the density decreases due to

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change of bond angles

change of bond lengths

cubic structure of ice

empty spaces present in the structure of ice

Strong dipole-dipole forces among the liquid molecules are responsible for

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very high heat of vaporization

very low heat of vaporization

cannot be predicted

negligible forces are these

Dipole-induced dipole forces are also called

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dipole-dipole forces

ion-dipole forces

Debye forces

London-dispersion forces

The boiling of water may be 120°C, when the external pressure is

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greater than 760 torr

less than 760 torr

equal to 760 torr

variable

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 behaviour of the elements remain the same

The vapour pressure of a liquid depends upon

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amount of the liquid

surface area

temperature

size of container

Amount of heat absorbed when one mole of a solid melts into liquid form at its melting point is called:

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heat of vaporization

latent heat of fusion

molar heat of fusion

molar heat of sublimation

Hydrogen bonding is extensively present in proteins which form the spiral. The hydrogen bond being produced is between

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nitrogen and hydrogen atom

oxygen and hydrogen atom

carbon and hydrogen atom

oxygen and carbon atom

The long chains of amino acids are coiled around one another into a spiral by

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ionic bond

Van der Waal's forces

hydrogen bonding

overlapping of orbitals

Vapour pressure of a substance does not depend upon:

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physical state of matter

temperature

intermolecular forces

surface area

The boiling point of glycerin at 1 atmospheric pressure is:

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290°C

390°C

190C°

210°C

The weakest intermolecular forces present in a liquid may be

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Dipole-induced dipole forces

dipole-dipole forces

instantaneous forces

electrostatic forces between ions in a ionic solid

The boiling point of H2O is 100°C while that of C2H5-OH is 78.5C°. The reason is that:

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H2O molecules are small-sized

the bond angles at oxygen atom are different

C2H5-group is electron donating

the number of H-bonds are greater in H20, than C2H5-OH

Oxygen and sulphur are present in VI-A group of the periodic table The hydride of oxygen i.e., H2O is liquid at room temperature but the hydride of sulphur (H2S) is a gas. This is due to

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greater bond angle of water than Hs

greater bond lengths in HS than H2O

hydrogen bonding in water

acidic character of HS

The B.P. of compound is mostly raised by

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dipole-induced dipole interactions

london dispersion forces

intramolecular H-bonding

intermolecular H-bonding

Liquids evaporate at every temperature. When the temperature becomes constant for a liquid, then:

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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 become equal

it depends upon the nature of the liquid

The B.P of glycerine at 760 torr pressure is

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200°C

290C°

250C°

262C°

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