Question # 1

Dipole-induced dipole forces are also called

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dipole-dipole forces

ion-dipole forces

Debye forces

London-dispersion forces

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

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

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 nature of crystals formed due to London forces of interaction are

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molecular

metallic

ionic

covalent

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

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

Liquid hydrocarbon is

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methane

propane

ethane

hexane

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 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 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

Saturated hydrocarbons having carbon atoms more than 20 in a molecule are solids due to

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higher densities

higher molar masses

the chain, are more zig-zag

all are correct

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

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

lce occupies more space than liquid water

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9%

10%

11%

12%

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

The boiling points of the halogens

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increases down the group

decreases down the group

remains constant

can not be predicted

Which of the following liquid has highest bolling point

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HCI

HBr

H2O

Br2

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

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

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