Question # 1

In a group on going downward, polarizability generally

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Decreases

Increases

Remains constant

Negligible

Force of attraction between atoms of He is

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London dispersion forces

Hydrogen bondign

Coordinate covalent bond

Covalent bond

Which of the following liquids has low vapour pressure at 25°C:

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Diethyl ether

Acetone.

Water.

Ethyl alcohol.

At sea level and at 100°C the vapor pressure of water in an open system is:

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1000 mm Hg

760 mm Hg

730 mm Hg

670 mm Hg

Hydrogen bonding is present between the molecules of

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NH₃

H₂O

HF

All of above

Chloroform and acetone are soluble in each other due to:

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Instantaneous dipole interactions.

Dipole-dipole interactions.

Inter molecular hydrogen bonding.

All of above

Hydrocarbon molecule with large chain lengths experience:

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Weaker attractive forces

Stronger attractive forces

Repulsive forces

No attractive forces

In a group on going downward, polarizability generally:

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Decreases

Increases

Remain constant

Negligible

Heat of vapourization for liquids with strong dipole-dipole forces will have

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Negligible Values

Reasonably high values

Very high values

very low values

Polypeptide chains are coiled about one another into a spiral by

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Ionic bonds

Covalent bonds

Van der Waal's forces

Hydrogen bonds

Trend of boiling point of halogens from fluorine to Iodine is that it

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Decreases

Is negligible

Increases

Remains constant

A liquid on evaporation causes:

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Heating effect.

Cooling effect.

Suffocation .

All of above

HF has exceptionally low acidic strength due to:

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Smaller size of fluorine.

Stronger polar bond between H and F.

Electronegativity of fluorine

Strong hydrogen bonding

The intermolecular forces in liquids are

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Negligible

Very weak

Very strong

Reasonably strong

H₂S is a gas while H₂O is a liquid at room temperature. It is due to:

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Less inter-molecular forces in water.

Covalent bonding H-O in water molecule.

Hydrogen bonding in water molecules

Ionic character in water molecules

Chloroform and acetone are soluble in each other due to

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Instantaneous dipole interactions

Dipole-dipole interactions

Intermolecular hydrogen bonding

All of above

At sea level and at 100⁰C the vapour pressure of water in an open system is

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1000 mm Hg

760 mm Hg

730 mm Hg

670 mm Hg

Hydrogen bonding is present in one of the following pairs:

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NH₃

H₂O

HF

All of above

Diamond is a bad conductor because:

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Ithas tight structure

It has a high density

There is no free electron present in the crystal of diamond of conduct electricity is transparent to light

The strongest forces are

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Debye forces

London dispersion forces

Dipole-dipole attraction

Hydrogen

Polypeptide chains are coiled about one another into a spiral by:

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Ionic bonds

Covalent bonds

Van der Waal's forces

Hydrogen bonds

Which of the following is a pseudo solid

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CaF₂

Glass

NaCl

All

London dispersion forces are alos called:

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Hydrogen bonding.

Debye forces

Van der Waal's forces

Instantaneous dipole-induced dipole forces.

Which of the following liquids has low vapor pressure at 25°C:

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Diethyl ether

Acetone.

Water.

Ethyl alcohol.

Debye forces are present in one of the following pairs

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Na⁺ion and water

Argon and water

Argon and Na⁺ion

Ne and Water

Rate of evaporation and rate of condensation at equilibrium

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Become very low

Become very high

Become equal

Can never be equal

The strongest forces are:

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Debye froces

London dispersion

Dipole-dipole attraction

Hydrogen bonding

London dispersion forces are also called

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Hydrogen bonding

Debye forces

Van de Waal's forces

Instantaneous dipole-induced dipole forces

The boiling point of NH₃is maximum among the hydrides of group V elements due to

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Enhanced electronegative character of Nitrogen

Pyramidal structure of NH₃

Very small size of Nitrogen

Enhanced electropositive character of Nitrogen

The density of water decreases, When it is freezed at 0°C

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Change of bond length

Change of bond angles

Cubic structure of ice

Empty spaces present in the structure of ice

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