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Solids liquids & gases

Total questions: 100

Worksheet time: 52mins

Name
Class
Date
1.

A crystal which can be divided by an imaginary plane inti two equal parts, each of which is the exact mirror image of the other, the crystal is said to have a

a)

Axis of symmetry

b)

Line of symmetry

c)

Plane of symmetry

d)

Center of symmetry

2.

A cell having the lattice point at the corner is called a

a)

Face-centered unit cell

b)

Body-centered unit cell

c)

Primitive unit cell

d)

End-centered unit cell

3.

The structure of NaCl crystal is

a)

Body centered cubic unit cell

b)

Primitive unit cell

c)

End-centered cubic unit cell

d)

Face-centered cubic unit cell

4.

The first satisfactory approach of the temperature dependence of the heat capacities of solids was made by

a)

G N Lewis

b)

Albert Einstein

c)

Peter Debye

d)

Dulong & Petti

5.

In tetragonal system

a)

All the axes are equal & are at right angle to each other

b)

2 axes are equal & are at right angle to each other

c)

All the axes are unequal & are at right angle to each other

d)

All the axes are equal & angles between them are unequal

6.

The Bragg equation relates the wavelength of X-rays to the distance between ....... and the angle of .......

a)

Atomic planes & diffraction

b)

Atomic planes & reflection

c)

Reflection and bonding energy

7.

A crystal may have a number of planes of symmetry or axes of symmetry, but it can have

a)

Only 1 center of symmetry

b)

3 centers of symmetry

c)

4 centers of symmetry

d)

2 centers of symmetry

8.

Which one of the following is a purely constitutive property?

a)

Parachor

b)

Optical rotation

c)

Molar refraction

d)

Rheochor

9.

The magnetic moment of a substance depends upon

a)

No of unpaired protons

b)

No of unpaired neutrons

c)

No of paired electrons

d)

No of unpaired electrons

10.

The height which a liwuid will rise in an open capillary tube is inversly proportional to

a)

Surface tension

b)

Density of the liquid

c)

Air pressure

d)

Viscosity of the liquid

11.

Thevcritical temperature of a gas

a)

Does not depend upon the nature of the gas

b)

Is lower than the inversion temperature

c)

Depends upon thevcritical pressure

d)

Is higher than the inversion temperature

12.

At STP the order of mran square velocity of molecules N2 , NH3, O2 & HCl is

a)

N2 > O2 > HCl > NH3

b)

H2 > NH3 > O2 > HCl

c)

HCl > NH3 > O2 > H2

d)

O2 > HCl > NH3 > H2

13.

In a gas sample at room temperature, which one of the following states will have the greatest number of molecules occupying states other than the lowest energy state

a)

Electronic energy state

b)

Vibrational energy state

c)

Rotational energy state

d)

Nuclear spin state

14.

If 04 gram of a gas occupies 11.2 dm3 at 0° and 0.25 atmosphere, then the molecular mass of tge gass is

a)

8 gram

b)

16 gram

c)

32 gram

d)

48 gram

15.

Choose the fundamental vibdational modes in a molecule of nitrocyl NO2Cl

a)

10

b)

13

c)

9

d)

6

16.

A real gas obeying the van der Waal's equation will resemble ideal gas, if

a)

Both "a" & "b" are large

b)

Both "a" & "b" are small

c)

"a" is small but "b" is large

d)

"a" is large but "b" is small

17.

The Maxwell's distribution of speeds of particles in an ideal gas is proportional to which one of the following expressions

a)

exp (-mv2/2kT)

b)

exp (-mv2/2RT)

c)

exp (-mv/2kT)

d)

exp (-mv/2RT)

18.

Which has the strongest bonding in the solid state

a)

HCl

b)

Xe

c)

NaCl

d)

Cl2

19.

What are the conditions for gas like CO to obey the ideal gas laws

a)

Low T & low P

b)

Low T & high P

c)

High T & low P

d)

High T & high P

20.

At the same T, the molar kinetic energy of N2 & CO is

a)

KE1 > KE2

b)

KE1 < KE2

c)

KE1 = KE2

d)

Insufficient information given

21.

The crystals form due to London dispersion forces interaction are

a)

Ionic

b)

Covalent

c)

Molecular

d)

Matellic

22.

Which one of the following compounds has highest lattice energy

a)

NaI

b)

NaF

c)

NaCl

d)

NaBr

23.

Structure of CrO4(-2) is

a)

Cubic

b)

Triclinic

c)

Tetrahedral

d)

Octahedral

24.

Te trsnsition temperature of KNO3 is

a)

98°C

b)

32.2°C

c)

13.2°C

d)

128°C

25.

The example of hexagonal system is

a)

Sulphur

b)

NaCl

c)

Graphite

d)

Diamond

26.

Which one of them is not an isomorphic pair

a)

NaF , MgO

b)

Zn , Cd

c)

K2SO4 , K2Cr2O7

d)

NaNO3 , CaCO3

27.

What is the shape of grapgh that is drawn, when the temperature is kept constant

a)

Isobar

b)

Isochoric & isobar

c)

Isochoric

d)

Isotherm

28.

How much does the volume of the gas increase if we increase the temperature by 1 Degree?

a)

273 liters

b)

Hundred liters

c)

1 liter

d)

1 by 273rd of the original volume of the gas

29.

There is a balloon filled with a gas at 26-degree centigrade and has a volume of about 2 liters when the balloon is taken to a place which is at 39-degree centigrade, what would be the volume of the gas that is inside the balloon?

a)

7 liters

b)

5.5 liters

c)

3 liters

d)

0.67 liters

30.

An ideal gas of 10 moles occupies _________ volume.

a)

22.4 liters

b)

2.24 liters

c)

224 liters

d)

2240 liters

31.

The deviation of a gas from the ideal behaviour is maximum at

a)

-10°C and 5 atm

b)

-10°C and 2 atm

c)

100°C and 2 atm

d)

0°C and 2 atm

32.

Equal masses of methane & oxygen are mixed in an empty contsiner at 25°C. The fraction of total pressure exerted by oxygen is

a)

1/3

b)

8/9

c)

1/9

d)

16/17

33.

The critical temperature of NH3 is

a)

Less than argon

b)

Equal to argon

c)

Greater than orgon

d)

Not known

34.

The molar volume if helium is 44.8 dm3 at

a)

100•C & 1 atm

b)

0•C & 0.5 atm

c)

25•C & 0.25 atm

d)

40•C & 0.5 atm

35.

Which one of the following gases will have the highest rate of diffusion

a)

NH3

b)

N2

c)

CO2

d)

O2

36.

An ideal gas has volume 1dm3 at 303K keeping pressure constant, at which kelvin temperature its volume will become 2dm3

a)

240

b)

303

c)

330

d)

606

37.

If absolute temperature of a gas is doubled and the pressure is also doubled, the volume of gas will

a)

Reduce to 1/4

b)

Increase 4 times

c)

Remain unchanged

d)

Be doubled

38.

Na and Mg crystallize in crystals of bcc and fcc form respectively and then the amount of Na and Mg atoms present in their respective crystal unit cells is

a)

4 and 2

b)

9 and 14

c)

14 and 19

d)

2 and 4

39.

Each of the following solids shows the Frenkel defect except

a)

ZnS

b)

AgBr

c)

AgI

d)

KCl

40.

Schottky defect in a crystal is observed when

a)

The ion leaves its normal position and occupies an interstitial location

b)

the unequal number of cation and anions are missing from the lattice

c)

the density of the crystal increases.

d)

an equal number of cations and anions are missing from the lattice.

41.

 In a simple cubic, body-centred cubic and face-centred cubic structure, the ratio of the number of atoms present is respectively

a)

8:1:6

b)

1:2:4

c)

4:2:1

d)

4:2:3

42.

Copper crystalline in FCC with a unit cell length of 361pm. What is the radius of a copper atom?

a)

128pm

b)

157pm

c)

181 pm

d)

108 pm

43.

The attraction between particles gives solids a definite

a)

shape and volume

b)

shape and color

c)

shape and position

d)

flow and radius

44.

The temperature at which a solid begins to liquefy is its ______ point.

a)

freezing

b)

boiling

c)

melting

d)

mass

45.

The amount of energy required for a liquid at its boiling point to become a gas is _____________.

a)

heat of fusion

b)

heat of vaporization

c)

transpiration

d)

freezing point

46.

_______________ is an increase in the size of a substance when the temperature is increased.

a)

kinetic energy

b)

potential energy

c)

thermal point

d)

thermal expansion

47.

According to the kinetic theory of matter, all matter is composed of

a)

waves

b)

particles

c)

solid material

d)

plasma

48.

Which of the following is a state of matter?

a)

particle

b)

thermal

c)

plasma

d)

diffuse

49.

When the temperature of a substance is lowered, its particles

a)

vibrate more quickly

b)

stop vibrating completely

c)

escape the attractive forces of the other particles

d)

vibrate more slowly

50.

The amount of energy needed to change a substance from the solid phase to the liquid phase is the substance's

a)

heat of vaporization

b)

heat of transformation

c)

melting point

d)

heat of fusion

51.

Why can people on one side of a room smell the scent of an air freshener sprayed on the opposite side of the room?

a)

The molecules of air freshener have thermally expanded

b)

The air pressure where the freshener was sprayed is greater than in the rest of the room

c)

The molecules of air freshener spread out until they are evenly distributed throughout the room

d)

The molecules of air freshener are amorphous

52.

What is the most common state of matter in the universe?

a)

solid

b)

liquid

c)

gas

d)

plasma

53.

An example of an amorphous solid is

a)

glass

b)

dry ice

c)

liquid crystals

d)

water

54.

An example of a substance that can undergo sublimation is

a)

glass

b)

liquid crystals

c)

water

d)

dry ice (frozen carbon dioxide)

55.

When a gas becomes a liquid it is called

a)

condensation

b)

evaporation

c)

sublimation

d)

freezing

56.

The energy an object has due to its motion

a)

thermal energy

b)

potential energy

c)

kinetic energy

d)

gravitational energy

57.

A measure of the average kinetic energy of all the particles in an object

a)

kinetic energy

b)

temperature

c)

thermal energy

d)

particle motion

58.

Change of state from a solid to a gas without going through the liquid form

a)

deposition

b)

evaporation

c)

condensation

d)

sublimation

59.

The change of state of a gas to a solid without going through the liquid state

a)

evaporation

b)

sublimation

c)

deposition

d)

condensation

60.

The amount of force applied per unit of area

a)

density

b)

mass

c)

volume

d)

pressure

61.

States that pressure of a gas increases if the volume decreases and pressure of a gas decreases if the volume increases, when temperature is constant

a)

Boyle's Law

b)

Kinetic Molecular Theory

c)

Charles' Law

d)

Newton's First Law

62.

States that the volume of a gas increases with increasing temperature, if the pressure is constant

a)

Boyle's Law

b)

Kinetic Molecular Theory

c)

Charles' Law

d)

Newton's Laws of Motion

63.

The motion of gas particles is described as

a)

constant

b)

rapid

c)

random

d)

all of these

64.

The temperature at which a substance has no kinetic energy is

a)

-273 degree Celsius

b)

zero Kelvin

c)

absolute zero

d)

all of these

65.

An ideal gas has _____ attractions between particles.

a)

no

b)

weak

c)

strong

d)

many types of

66.

Gases can be compressed because the particles are

a)

small

b)

large

c)

close together

d)

far apart

67.

The boiling point of a given liquid

a)

is a constant

b)

depends on temperature

c)

depends on atmospheric pressure

d)

depends on the size of the container

68.

The tendency of a liquid to minimize its surface area is called:

a)

capillary action.

b)

viscosity.

c)

surface tension.

d)

vaporization.

69.

Which intermolecular force is present in all molecules and atoms?

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

d)

none of the above

70.

Carbon Monoxide containing an electronegativity difference of 1 would contain what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

71.

Ammonia, NH3, would have what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

72.

the spontaneous rising of a liquid in a narrow tube

a)

Surface Tension

b)

Capillary Action

c)

Viscosity

d)

None of the above

e)

All of the above

73.

solids with considerable disorder in their arrangements

a)

Crystalline Solids

b)

Amorphous Solids

c)

Metallic Sollids

d)

All of the above

e)

None of the above

74.

Which of the following states of matter are compressible?

a)

solid

b)

liquid

c)

gas

75.

Which is NOT an intermolecular force?

a)

Hydrogen bonding

b)

ion-dipole forces

c)

dipole-dipole forces

d)

dispersion forces

e)

Gravity

76.

What dispersion forces cause ice to have an open hexagonal structure in the solid state and float?

a)

H-bonding

b)

dispersion forces

c)

D-D interactions

d)

Ion - D interactions

77.

Which property is not dependent on intermolecular forces?

a)

viscosity

b)

surface tension

c)

boiling point

d)

melting point

e)

temperature

78.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

79.

The measure of the resistance to the flow of a liquid is called:

a)

vapor pressure.

b)

sublimation.

c)

viscosity.

d)

condensation.

80.

Is the pressure exerted by its vapor when in equilibrium with its liquid or solid

a)

Surface Tension

b)

Viscosity

c)

Vapor Pressure

d)

Boiling Point

81.

Have considerable disorder in their structure

a)

Heat of Vaporization

b)

Amorphous Solids

c)

Crystalline Solids

d)

Heat of Fusion

82.

Force of attraction that exist between molecules

a)

INTERMOLECULAR FORCE

b)

CHEMICAL BONDING

c)

ELECTROSTATIC FORCE

83.

The following are properties of Liquids except

a)

Surface Tension

b)

Density

c)

Crystal Structure

d)

Vapor Pressure

84.

Ammonia, NH3, would have what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

85.

Carbon Monoxide containing an electronegativity difference of 1 would contain what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

86.

F2 would contain what type of intermolecular forces if any?

a)

Hydrogen Bonding

b)

Dipole-Dipole

c)

London Dispersion

d)

None

87.

According to the phase diagram given what change occurs at a pressure of 10 atm and a temperature change from -150 to -100?

a)

Freezing

b)

Melting

c)

Evaporation

d)

Condensation

e)

Deposition

88.

At what temperature according to the phase diagram can this substance no longer exist in the liquid phase regardless of pressure?

a)

0 degrees

b)

15 degrees

c)

-90 degrees

d)

-110 degrees

89.

What change occurs at a pressure of .5 atm and a temperature change of -100 to -150?

a)

freezing

b)

melting

c)

evaporation

d)

sublimation

e)

deposition

90.

The mixing of orbitals to create a more energy favorable and stable sub-shell is called...

a)

Delocalization

b)

Subshell Formation

c)

Hybridization

d)

None of the above

e)

All of the above

91.

What type of mixed orbitals would occur in the compound methane? (CH4)

a)

sp

b)

sp2

c)

sp3

d)

All of the above

e)

None of the above

92.

Temporary but instantaneous dipoles created in nonpolar substances are referred to as...

a)

Hydrogen bonding

b)

Dipole-Dipole forces

c)

London Dispersion forces

d)

None of the above

e)

All of the above

93.

the spontaneous rising of a liquid in a narrow tube

a)

Surface Tension

b)

Capillary Action

c)

Viscosity

d)

None of the above

e)

All of the above

94.

solids with considerable disorder in their arrangements

a)

Crystalline Solids

b)

Amorphous Solids

c)

Metallic Sollids

d)

All of the above

e)

None of the above

95.

Crystalline Solids usually contain a three dimensional system of points which illustrate the position of its components...called a...

a)

Network

b)

Dipole Unit

c)

Lattice

d)

None of the above

e)

All of the above

96.

X rays of wavelength 1.54 A were used to analyze an aluminum crystal. A reflection was produced at an angle of 19.3 degrees. Assuming n = 1, calculate the distance between the planes of atoms producing this reflection.

a)

3.43 A

b)

2.33 A

c)

0.53 A

d)

None of the above

97.

When a very large number of orbitals results in metals forming a continuum of levels, they are called...

a)

Hybridized

b)

Bands

c)

Lattices

d)

None of the above

e)

All of the above

98.

Which of the following are examples of substitutional alloys?

a)

Brass

b)

Sterling Silver

c)

Pewter

d)

None of the above

e)

All of the above

99.

What results when Silica is heated to temperatures exceeding 1600 degrees C and then cooled rapidly?

a)

Ceramics

b)

Steel

c)

Glass

d)

None of the above

e)

All of the above

100.
Why is it hard to breath at high altitudes?
a)
There is too much oxygen in this location.
b)
There is a higher density of air molecules.
c)
There is a low density of air molecules.
d)
The air pressure is greater than at low altitudes.

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