Question # 1

A liquid on evaporation causes:

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Heating effect.

Cooling effect.

Suffocation .

All of above

Hydrogen bonding is present in one of the following pairs:

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NH₃

H₂O

HF

All of above

The molecules of CO₂in dry ice from the

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Ionic crystalls

Covalent crystals

Molecular crystals

Any type of crystal

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

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 sharp melting point

Undergo clean cleavage when cut with knife

Have perfect arrangement of atoms

Can possesses small regions of orderly arrangement of atoms

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

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Ionic crystals

Coverlet crystals

Molecular crystals

Any type of crystals

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

In a group on going downward, polarizability generally

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Decreases

Increases

Remains constant

Negligible

The strongest forces are:

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Debye froces

London dispersion

Dipole-dipole attraction

Hydrogen bonding

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

H₂S is a gas which H₂O is liquid at room temperature. it is due to

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Less intermolecular forces in water

Covalent bond in H-O in water molecule

Hydrogen bonding in water molecules

Ionic characters in water molecules

Evaporation of water is possible at:

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Above 100°C

0°C

100°C

At all temperature

London dispersion forces are also called

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Hydrogen bonding

Debye forces

Van de Waal's forces

Instantaneous dipole-induced dipole 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

Force of attraction between atoms of He is

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London dispersion forces

Hydrogen bondign

Coordinate covalent bond

Covalent bond

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

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

Which of the following is a pseudo solid

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CaF₂

Glass

NaCl

All

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

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

Ionic solids are characterized by :

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Low meeting points

Good conductivity in solid state

High vapor pressure

Solubility in polar solvents

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

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Diethyl ether

Acetone.

Water.

Ethyl alcohol.

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

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

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 forces

London dispersion forces

Dipole-dipole attraction

Hydrogen

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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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

Ionic Solids are characterized by

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Low melting points

Good conductivity in solid state

High vapour pressure

Solubility in polar solvents

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