Question # 1

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

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 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

Hydrogen bonding is not present in which of following compound?

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Ammonia

Ethanol

Ether

Water

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

Dipole-induced dipole forces are also called

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dipole-dipole forces

ion-dipole forces

Debye forces

London-dispersion forces

Vapour pressure of a substance does not depend upon:

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physical state of matter

temperature

intermolecular forces

surface area

Liquid hydrocarbon is

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methane

propane

ethane

hexane

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 B.P of glycerine at 760 torr pressure is

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200°C

290C°

250C°

262C°

The vapour pressure of a liquid depends upon

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amount of the liquid

surface area

temperature

size of container

Halogens form halogen acids. HF is the weakest among all of them This is due to the reason that

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fluorine is a very small-sized atom

fluorine is highly electronegative atom

there is strong hydrogen bonding in HF

the polarity of HF bond is less

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

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

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

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

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

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

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molecular

metallic

ionic

covalent

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