Increasing order of boiling points in the following compounds is: CH 3 COOH ( i ) CH 3 CH 2 CHO ( ii ) CH 3 CH 2 CH 2 OH ( iii ) CH 3 COCH 3 ( iv )

( ii ) < ( i v ) < ( i i i ) < ( i )

( ii ) < ( i v ) > ( i i i ) < ( i )

( iv ) < ( ii ) > ( i ) < ( iii )

( iv ) < ( iii ) < ( ii ) < ( i )

Match the type of interaction in column A with the distance dependence of their interaction energy in column B : A B (i) ion - ion (a) 1 r (ii) Dipole - dipole (b) 1 r 2 (iii) London dispersion (c) 1 r 3 (d) 1 r 6

(i) – (a); (ii) – (c); (iii) – (d)

(i) – (b); (ii) – (d); (iii) – (c)

(i) – (a); (ii) – (b); (iii) – (d)

(i) – (a); (ii) – (b); (iii) – (c)

MEDIUM

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Assertion. The ${HF}_{2}^{-}$ ion exists in the solid-state and also in the liquid state but not in an aqueous solution.

Reason. The magnitude of hydrogen bonds in between $HF - HF$ molecules are weaker than that in between $HF$ and $H_{2} O$ molecules.

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Important Questions on States of Matter

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The dipole-dipole interaction energy between stationary polar molecules and rotating polar molecules, respectively is proportional to
[

r

is the distance between the polar molecules]

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Increasing order of boiling points in the following compounds is:

$\underset{(i)}{{CH}_{3} COOH} \underset{(ii)}{{CH}_{3} {CH}_{2} CHO} \underset{(iii)}{{CH}_{3} {CH}_{2} {CH}_{2} OH} \underset{(iv)}{{CH}_{3} {COCH}_{3}}$

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The interaction energy of London forces between two particles is proportional to

r^{x}

, where

r

is the distance between the particles. The value of

x

is :

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Give reason:

H_{2} O

is a liquid and

H_{2} S

is a gas.

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

What is the actual volume occupied by water molecules present in

20 {cm}^{3}

of water?

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Given:

Question Image

On the basis of data given above, predict which of the following gases shows the least adsorption on a definite amount of charcoal?

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Rare gases are sparingly soluble in water because of

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The qualitative sketches I, II and III given below show the variation of surface tension with molar concentration of three different aqueous solutions of KCl,

C H_{3} O H

and

C H_{3} {(C H_{2})}_{11} O S O_{3}^{-} N a^{+}

at room temperature. The correct assignment of the sketches is -

Question Image

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The predominant intermolecular forces present in ethyl acetate, a liquid, are:

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The type of attractive forces that operate between gaseous

HCl

molecules is

HARD

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The dipole-dipole interaction energy between rotating polar molecules is proportional to, where '

r

' is the distance between polar molecules.

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Which intermolecular force is most responsible in allowing xenon gas to liquefy?

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Dipole - induced dipole interactions are present between which of the following pairs?

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

In which of the following solid substance dispersion forces exist?

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

A piece of ice falls from a height

h

so that it melts completely. Only one-quarter of the heat produced is absorbed by the ice and all energy of ice gets converted into heat during its fall. The value of

h

is:
(Latent heat of ice is

3.4 \times 10^{5} {J kg}^{- 1}

and

g = 10 {N kg}^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The combination of plots which does not represent isothermal expansion of an ideal gas is

$(A)$ Question Image

$(B)$

$(C)$

$(D)$

HARD

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

An ideal gas undergoes isothermal compression from

5 m^{3}

1 m^{3}

against a constant external pressure of

4 N m^{- 2}

. The heat released in this process is

24 J {mol}^{- 1} K^{- 1}

and is used to increase the pressure of

1

mole of

Al

. The temperature of

Al

increases by:

MEDIUM

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

Match the type of interaction in column $A$ with the distance dependence of their interaction energy in column $B :$

A	B
(i) ion - ion	(a) $\frac{1}{r}$
(ii) Dipole - dipole	(b) $\frac{1}{r^{2}}$
(iii) London dispersion	(c) $\frac{1}{r^{3}}$
	(d) $\frac{1}{r^{6}}$

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The relative strength of the interionic/ intermolecular forces in a decreasing order is:

EASY

Chemistry>Physical Chemistry>States of Matter>Intermolecular Forces and Thermal Energy

The intermolecular interaction that is dependent on the inverse cube of distance between the molecules is:

Assertion. The HF2- ion exists in the solid-state and also in the liquid state but not in an aqueous solution. Reason. The magnitude of hydrogen bonds in between HF-HF molecules are weaker than that in between HF and H2O molecules.

Important Questions on States of Matter

Learn and Prepare for any exam you want !

Assertion. The ${HF}_{2}^{-}$ ion exists in the solid-state and also in the liquid state but not in an aqueous solution.

Reason. The magnitude of hydrogen bonds in between $HF - HF$ molecules are weaker than that in between $HF$ and $H_{2} O$ molecules.