Question # 1

The forces which are present between the ions and the water molecules are known as

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dipole-induced dipole forces

dipole-dipole forces

ion-dipole forces

London dispersion forces

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

Polarizability is responsible for intermolecular forces and it

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increases down the group

decreases down the group

almost remains the same

increased along a period

The boiling point of higher alkanes are greater than those of lower alkanes due to reason that

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higher alkanes have greater number of atoms

the polarizabilities of higher alkanes are greater

higher alkanes have greater hydrogen bonding

higher alkanes have zig-zag structures

Which of the following liquid has highest bolling point

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HCI

HBr

H2O

Br2

Ice floats on water because

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the hydrogen bonding in ice is stronger than that of in water

empty spaces are left in ice

ice has two-dimensional structure

the bond length of the oxygen and hydrogen bond is different in water and ice

The nature of the attractive force in acetone and chloroform are

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dipole-induced dipole forces

dipole-dipole forces

ion-dipole forces

instantaneous forces

The B.P of glycerine at 760 torr pressure is

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200°C

290C°

250C°

262C°

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

Point out the substance which has maximum vapour pressure at a given temperature?

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Acetone

Water

Ethanol

Acetic acid

The vapour pressure of a liquid depends upon

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amount of the liquid

surface area

temperature

size of container

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

Which of following factor affect vapour pressure of a liquid?

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temperature

inter molecules forces

size of the molecules

all of these

The nature of crystals formed due to London forces of interaction are

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molecular

metallic

ionic

covalent

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

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

H2O and HF are the hydrides of the second period. Fluorine is more electronegative than oxygen. Anyhow, the boiling point of water is greater than that of HF. This is due to:

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water is more polar than HF

water has a bent structure

HF has a zig zag structure after making hydrogen bonding

the number of hydrogen bonds produced by water are greater than that of HF

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

Dipole-induced dipole forces are also called

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dipole-dipole forces

ion-dipole forces

Debye forces

London-dispersion forces

Dipole-dipole interaction are present in the

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atoms of the He gas

molecules of CCl4

molecules of solid iodine

molecules of :NH3

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