Question # 1

London dispersion forces are also called

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Hydrogen bonding

Debye forces

Van de Waal's forces

Instantaneous dipole-induced dipole forces

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

Debye forces are present in on of the following pairs:

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Na+ion and water

Argon and water

Argon and Na+ion

Ne and water

Amorphous solids:

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Have a sharp melting point

Undergo clean cleavage when cut with knife

Have a perfect arrangement of atoms

Can possesses small regions of orderly arrangement of atoms

The boiling point of NH_{3 is maximum among the hydrides of group V elementsdue to:}

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Enhanced electronegative character of Nitrogen

Pyramidal structure of NH3

Very small size of Nitrogen.

Enhanced electropositive character of Nitrogen

Which one of the following is weakest inter molecular force?

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Dipole induced dipole forces

Ionic dipole forces

Electrostatic forces b/w ions

Dipole dipole forces

A liquid on evaporation causes:

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Heating effect.

Cooling effect.

Suffocation .

All of above

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

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Diethyl ether

Acetone.

Water.

Ethyl alcohol.

A liquid on evaporation causes

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Heating effect

Cooling effect

Suffication

All of above

Which one of the following is the weakest intermolecular force

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Dipole induced dipole forces

Ionic dipole forces

Electrostatics forces between ions

Dipole-dipole forces

The gases can be converted into liquids by

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increasing the pressure only

Lowering temperature and increasing pressure

Increasing pressure and bringing temperature below critical point

Lowering temperature only

Diamond is a bad conductor because

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It has a tight structure

It has a high density

there is no free electron present in the crystal of diamond of conduct electicity

Is transparent to light

The molecules of CO₂in dry ice from the

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Ionic crystalls

Covalent crystals

Molecular crystals

Any type of crystal

The gases can be converted into liquids by:

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Increasing the pressure only.

Lowering temperature and increasing pressure

Increasing pressure and bringing temperature below critical points

Lowering temperature only

Amorphous solids

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Have sharp melting point

Undergo clean cleavage when cut with knife

Have perfect arrangement of atoms

Can possesses small regions of orderly arrangement of atoms

Hydrocarbon molecules with large chain lengths experience

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Weaker attractive forces

Stronger attractive forces

Repulsive forces

No attractive forces

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

The only forces are London dispersion forces among the

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Atoms of He in gaseous state at high temperature

Molecules of water in liquid state

Molecules of solid I₂

Molecular of hydrochloric acid gas

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

Which of the following is a pseudo solid

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CaF₂

Glass

NaCl

All

The strongest forces are:

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Debye froces

London dispersion

Dipole-dipole attraction

Hydrogen bonding

The molecules of CO_{2 in dry ice from the :}

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Ionic crystals

Coverlet crystals

Molecular crystals

Any type of crystals

In a group on going downward, polarizability generally

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Decreases

Increases

Remains constant

Negligible

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

Escape of high energy molecules from the surface of a liquid is called

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Sublimation

Distillation

Condensation

Evaporation

The intermolecular forces in liquids are

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Negligible

Very weak

Very strong

Reasonably strong

The inter-molecular forces in liquids are:

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Negligible

Very weak

Very strong

Reasonably strong

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

HF has exceptionally low acidic strengths due to

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Smaller size of fluorine

Strong polar bond between H and F

Electronegativity of fluorine

Strong hydrogen bonding

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