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ECAT Chemistry Solids Online Test

Maan AliLast Updated: April 19, 2025

Chemistry Solids MCQS Online Test

ECAT Chemistry Solids Chapter Online Test

Total Questions:	150
Time Allowed:	60 Minutes
Total Marks:	150
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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ECAT Chemistry Solids Test

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Page 1 of 6

Chemistry

1. Solvents of covalent compounds include all but

Alcohol

Tetra chloromethane

Petrol

Water

2. Isomorphic substances have

Different physical and chemical properties

Different physical and same chemical properties

Same physical and different chemical properties

Same physical and chemical properties

3. The insoluble impurities in the saturated solution are removed by

Normal filter paper

Both A & B

None

Fluted filter paper

4. The existence of a substance in more than one solid modification is known as

Amorphism

Isomorphism

Polymorphism

None of these

5. 4.4 g of CO₂ contains how many liters of CO₂ at STP?

2.4 liter

44 liter

22.4 liter

2.24 liter

6. Van der Waal’s forces exist in

Polar compounds

Non-polar

All types of atoms and molecules

Covalent

7. Which of the following statements about amorphous solids is incorrect?

There is no orderly arrangement of particles

There are rigid and in-compressible

They melt over a range of temperature

They are anisotropic

8. The number of atoms contained in 11.2 L of SO₂ at S.T.P. are

6.02 x 10²³

2 x 6.02 x 10²³

4 x 6.02 x 10²³

3/2 x 6.02 x 10²³

9. Correct order of intermolecular forces

Liquid < gas < solid

Gas < liquid < solid

Gas = liquid = solid

Gas < liquid < solid

10. Hydrogen diffuses six times faster than gas A. The molar mass gas of gas A is

11. The rate of diffusion of a gas is proportional to

None of these

P/d

P/√d

√P/d

12. The major binding force of diamond, silicon and quartz is

Electrical attraction

Covalent bond

Non covalent bond force

Electrostatic force

13. Which of the following metal oxides is anti-ferromagnetic in nature?

TiO₂

CrO₂

NO₂

MnO₂

14. Amorphous solids

Have perfect arrangement of atoms

Undergo clean cleave when cut with knife

Can possess small regions of orderly arrangement of atoms

Have sharp melting point

15. A solution of 10 mL of M/10 FeSO₄ was titrated with KMnO₄ solution in acidic medium, the amount of KMnO₄ used will be

10 mL of 0.02 M

10 mL of 0.1 M

10 mL of 0.5 M

5 mL of 0.1 M

16. In which process solid phase and vapour phase are directly involved?

Vaporization

Sublimation

Filtration

Condensation

17. ‘x’ grams of calcium carbonate was completely burnt in air. The weight of the solid residue formed is 28 g. What is the value of ‘x’ in grams?

200

150

18. The molecules of air don’t settle down. The is due to

Elastic collisions of gas molecules

Different molar mass

Non-polar nature of gases

Pressure of dust particles in air

19. A compound formed by elements X and Y crystallizes in a cubic structure in which the X atoms are at the corners of a cube and the Y atoms are at the face-centered. The formula of the compound is

X₃Y

XT₃

XY₂

20. Crystals can be classified into

4 crystal systems

3 crystal systems

7 crystal systems

14 crystal systems

21. Two moles of an ideal gas at 1 atm are compressed to 2 atm at 273 K. The enthalpy change for the process is

1 liter atm

Zero

2 liter atm

3 liter atm

22. Poor conductors of electricity is a characteristic of

Metallic compounds

Ionic compounds

Diatic bonds

Covalent compounds

23. The top of funnel stem should touch the side of the beaker because

Filtrate runs down without crystals

This gives medium size crystals

The filtrate is quick

This gives bigger size crystals

24. Which of the following statement is correct if the intermolecular forces in liquids A, B and C are in the order A < B < C?

A evaporates more readily than C

B evaporates more readily than A

B evaporates less readily than C

A and B evaporates at the same rate

25. Crystal can be classified in to _______ basic crystal habits

Page 2 of 6

26. Particles that most effects material properties

Protons

Neutrons

Valence electrons

Electrons

27. Which of the following equations represents the 2nd ionization energy of Na?

Na(g) → N²⁺ (g) + e¯

Na(s) → N²⁺ (g) + e¯

Na(s) → N²⁺ (g) + 2e¯

Na(g) → N²⁺ (g) + +¯

28. The total number of protons in 10 g of calcium carbonate in (N₀ = 6.023 x 10²³)

1.5057 x 10 ²⁴

4.0956 x 10 ²⁴

3.0115 x 10 ²⁴

2.0478 x 10 ²⁴

29. Which of the following crystal does not possess the cubic closed packed arrangement?

Cul

Agl

Csl

HgS

30. Imagine a man is sitting in a room. The room is closed from all sides, no entry, no exit of any gas. If the room expands suddenly then

His blood pressure will increase

He will feel warmth

There will be no change in the internal environment of the room

He will feel cool

31. Bragg’s law is given by equation

2nλ = d sin θ

nλ = 2 θ sin θ

nλ = 2 d sin θ

nλ = 1/2d sin θ

32. Under what conditions real gases deviate from ideal behavior

Both b and c

High pressure

Low temperature

High temperature

33. The material possessing superconducting properties is

Y B₂Cu₃O₇

Y Ba₂Cu₃O₇

Yb Ba₂Cu₂O₈

Hg Be₂Ca₂Cu₂O₈

34. Which of the following statements is (are correct)?

A unit cell of an ionic crystal shares some of its ions with other unit cells.

The coordination number of each type of ion in CsCl crystal is 8.

None of these

A metal that crystallizes in BCC structure has coordination number equal to 12

35. What will be the external pressure at which water may boil at 120°C?

790 mm of Hg

1489 mm of Hg

700 mm of Hg

100 mm of Hg

36. Which of the following are more temperature sensitive?

None of these

Liquid crystals

Ionic crystals

Solid crystals

37. Which of the following is isotropic

Brass

Mercury

Borax

Graphite

38. The example of hexagonal system is

Sugar

Graphite

Sulphur

Diamond

39. What is the pressure of 2 mole of NH₃ at 27°C when its volume is 5 lit in Van der Waals equation? (a = 0.17, b = 0.03711)

9.2 atm

9.333 atm

10.33 atm

9.74 atm

40. Which of the following does not represent a type of crystal system?

Triclinic

Isotropical

Monoclinic

Rhombohedral

41. A solid may be made up of

Ions

Molecules

Atoms

A, B and C

42. Which of the following substances is not amorphous?

Polymer

Rubber

Ag NO₃

Glass

43. Which one is not postulated in the kinetic molecular theory among the followings?

Molecules of all the gases have same size and same mass

All molecular collisions are elastic

The volume of the molecules is negligible as compared to volume occupied by the gas

Molecules are in chaotic motion

44. The body centered cubic arrangement is found in the crystal of

AgBr

NH₄Br

CuBr

CsBr

45. An alkaloid contains 17.28% of nitrogen and its molecular mass is 162. The number of nitrogen atoms present in one molecule of alkaloid is:

Five

Two

Four

Three

46. 3.2 g of oxygen (At. Wt. = 16) and 0.2 g of hydrogen (At. Wt. = 1) are placed in a 1.12 L flask at 0°C. The total pressure of the gas mixture will be

3 atm

2 atm

4 atm

1 atm

47. Which one of the following pair of atoms is most likely to from an ionic bond?

O and F

Na and F

N and F

C and F

48. To prepare the medium sized crystal the hot filtrate is cooled

Moderately

Slowly

None

Fast

49. A bottle of copper (II) oxide has been contaminated with some solid, NaCl, How can NaCl be removed from the Copper (II) oxide?

Heat the mixture and allow it to cool

Place the mixture in a separating funnel

Add dilute acid to the mixture and filter

Add water to the mixture and filter

50. In diamond, the carbon atoms are arranged in a

Tetrahedral manner

Square planner manner

Hexagonal manner

Altahydral manner

Page 3 of 6

51. The relative atomic mass of chlorine is 35.5. What is the m ass of 2 moles of chlorine gas?

18.75g

71g

35.5g

142g

52. Air at sea level is dense. This is a practical application of

Charles’ law

Boyle’s law

Dalton’s law

Avogadro’s law

53. A real gas most closely approaches the behavior of an ideal gas at

15 atm, and 200 K

1 atm, and 273 K

15 tm, and 500 K

0.5 atm, and 500 K

54. Which of the following is an example of body centered cube?

Magneisum

Zinc

Sodium

Copper

55. At constant temperature, the pressure of an ideal gas is doubled, its density becomes

None

Double

Half

Same

56. If we consider that 1/6, in place of 1/12, mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of substance will

Remains unchanged

Increase two fold

Be a function of the molecular mass of substance

Decrease twice

57. Graphite is a good conductor of electricity due to the presence of ________.

Cations

Free valence electrons

Anions

Ione pair of electrons

58. At STP, a container has 1 mole of Ar, 2 moles of CO₂, 3 moles of O₂ and 4 moles of N₂, Without changing the total pressure if one mole of O₂ is removed, the partial pressure of O₂

Change by 33%

Is halved

Is changed by about 26%

Is unchanged

59. An organic compound contains 49.3% carbon, 6.84% hydrogen and its vapour density is 73. Molecular formula of compound is

C₄H₁₀O₂

C₃H₅O₂

C₃H₁₀O₂

C₆H₁₀O₄

60. Wt. of 112 ml of oxygen at STP on liquefaction would be

0.64 g

0.32 g

0.16 g

0.96 g

61. If rate of diffusion of A is 5 times that of B, what will be the density ratio of A and B?

1/25

1/5

62. The kinetic energy of 4 moles of nitrogen gas at 127°C is? cals. (R = 2 cal mol¯¹ K¯¹)

4800

1524

3200

4400

63. The allotropic forms of an element are called

Unit Cell

Cleavage

Allotropes

Isoelectronic

64. The ratio of close packed atoms to tetrahedral holes in cubic close packing is

1 : 1

1 : 3

2 : 1

1 : 2

65. How many allotropic forms are present in carbon?

Four

Three

Two

Five

66. In a cubic lattice, a unit cell is shared equally by how many unit cells?

67. Which of the following has least mass?

3 x 10²³ atoms of C

1 mole of S

2 gram atom of nitrogen

7.0 g of Ag.

68. The phenomenon in which a single substance exist in two or more crystalline forms is called

Anisotropy

Isomorphism

Allotropy

Polymorphism

69. The coordination number 8:8 is found in the arrangement of

NaCl type structure

CsCl type structure

AB₂ type ionic compound

ZnS type structure

70. Potassium crystallizes with a

Ortho rhombic lattice

Cubic lattice

Triclinic

Orthogonal lattice

71. Distribution law is employed in which one of the following

Solvent extraction

Chromatography

Crystallization

All

72. The following statements contained in a student’s laboratory report is a conclusion

The gas is chlorine

Colour of the gas is greenish yellow

A gas is liberated

Oxide of the gas is strongly acidic

73. The mass of one mole of electron is

0.55 mg

1.008 mg

0.104 mg

1.673 mg

74. Gooch crucible is used for the filtration of precipitates having

Low temperature

High ignition temperature

High concentration

High solubility

75. The weight of one molecule of a compound C₆₀H₁₂₂ is

1.4 x 10¯²¹ g

1.3 x 10¯²⁰ g

5.01 x 10¯²¹ g

3.72 x 10¯²³ g

Page 4 of 6

76. A semiconductor of Ge can be made p-type by adding

Trivalent impurity

Divalent impurity

Pentavalent impurity

Tetravalent

77. When the following reaction equations is properly balanced, the number of moles of O₂ will be
C₃H₈ + O₂ → CO₂ + H₂O

3 moles

10 moles

3.5 moles

1.5 moles

78. Coordination number of Zn and ZnS (Zinc blends) is

None of these

79. For c coordination number of four, anion sits at the center of ________ where corners are occupied by cations

Triangle

Cube

Octahedron

Tetrahedron

80. When the temperature is raised, the viscosity of the liquid decreases. This is because of

Decreased volume of the solution

Increased attraction between the molecules

Increase in temperature increases the average kinetic energy of molecules which overcome the attractive force between them

Decreased covalent and hydrogen bond forces

81. In forming an ionic bond in potassium fluoride, the potassium ion

Gets a single negative charge

Gets a double positive charge

Gets a single positive charge

Gets a double negative charge

82. The increasing vapour caused by heating a liquid is due to

Increase in potential energy of molecules

Increase of K.E of molecules

Decrease of surface tension

Increase of intermolecular interactions

83. The volume in liters of CO₂ liberated at STP when 10 grams of 90% pure limestone is heated completely is

2.016

20.16

2.24

22.4

84. Which one is not usually used for the crystallization?

Acetic acid

Acetone

Sulphuric acid

Chloroform

85. a ≠ b ≠ c, ∞ ≠ β ≠ r ≠ 90 is representation of

Triclimic

Mexagonal

Trigonal

Monoclimic

86. Isotopes differ in

The extent to which they may be affected in electron magnetic field

Properties which depend upon mass

Chemical properties

Arrangement of electrons in orbitals

87. The surface formed by the breakage of a crystal is called _________ plane.

Unit

None

Cleavage

Crystal

88. The volume occupied by 1.4g of N₂ at S.T.P is

112 cm³

1.12 dm³

2.24 dm³

22.4 dm³

89. The reaction 4NH₃ + 3O₂ → 2N₂ + 6H₂O indicates that

For the complete reaction of 2 moles of NH₃ 40g of O₂ are required

One mole of NH₃ will produce 6 moles of N₂

One mole of NH₃ will produce ½ mole of N₂

For the complete reaction of 2 mole of NH₃ 20g of O₂ are required

90. Fluted filter paper is used for

Increasing the rate of filtration

Filtering the hot saturated solution

To avoid premature crystallization of the solute

To dissolve large amount of substance at its boiling point

91. In a crystal a ≠ b ≠ c, a = ϒ = 90° and β ≠ 90°. It is

Tetragonal

Monoclinic

Rhombic

Trigonal

92. Which solids are called true solids?

Amorphous

Crystalline

Metallic

Vitreous

93. In the equation PV = nRT which one cannot be numerically equal to R

8.31 x 10⁷ dynes Cm K¯¹ mol¯¹

8.31 JK¯¹ mol¯¹

8.31 x 10⁷ erg³ K¯¹ mol¯¹

8.31 L atm K¯¹ mol¯¹

94. Formation of a cation is?

Oxidation

Redox

Reduction

None

95. Which of the following contain maximum number of atoms?

5.0 moles of SO₂

20 moles of S8

6 moles of S

44.8 dm3 CO₂ at S.T.P

96. The deviation of a gas from ideal behavior is maximum at

-10°C and 5.0 atm

-10°C and 2.0 atm

100°C and 2.0 atm

0°C and 2.0 atm

97. Repeatable entity of a crystal structure is known as

Unit cell

Miller indices

Lattice

Crystal

98. Consider the physical properties of the gases. Which of the following statements about particles of gasses is incorrect? The particles are

Randomly moving

Causing pressure

Orderly arranged

Having wide spaces

99. Amorphous substance posses

No definite geometry

All of these

No definite heat of fusion

No sharp melting points

100. How many Cl¯ ions are there around Na⁺ ion in NaCl crystal?

Page 5 of 6

101. 50dm³ of CO is burnt completely according to reaction 2CO + O₂ – 2CO₂ Choose the correct statement

Volume of O₂ required is 50 dm³

Volume of CO₂ formed is 60 dm³

Volume of CO₂ formed is 25 dm³

Volume of O₂ required is 25 dm³

102. Half atmospheric pressure is

400 torr

101.325 Pa

8.5 Pounds

50 662 Pa

103. The crystal structure having face centered cubic arrangement is

NaCl

CuCl

CsCl

BaCl₂

104. Ionic solids are characterized by

Low melting points

High vapour pressures

Good conductivity in solid state

Solubility in polar solvents

105. Which of the following pairs do not form a dative covalent bond to each other?

CH₄ and AlCl₃

NH₃ and H⁺

H₂O and H⁺

NH₃ and BF₃

106. Which forms metallic crystals?

NH₄Cl

NaCl

SO₂

107. In crystal structure of sodium chloride, the arrangement of Cl ions is

Bcc

None of these

Fcc

Both fcc and bcc

108. Which of the following is a pseudo solid?

Glass

CaF₂

NaCl

All these

109. Isomorphic substance have

Different physical and same chemical properties

Same physical and difference chemical properties

Same physical and chemical properties

Different physical and chemical properties

110. Simple molecules or giant macromolecules are examples of

Ionic compounds

Metallic bonds

Diatic bond

Covalent bonds

111. Which of the following statements about graphite is not true?

The carbon atoms use only three of their four outer electrons for covalent bonding

The layers in graphite are attracted to each other by weak forces

The coordination number of carbon atoms is 4

The carbon atoms are arranged layers

112. In case of elements the polymorphism is called

Isotopic form

Crystalline forms

Isomorphism

Allotropy

113. When one of the following statements is wrong for gases?

Gases do not have a definite shape and volume

Mass of gas cannot be determined by weighing a container in which it is enclosed

Confined gas exerts uniform pressure on the walls of its container in all directions

Volume of the gas is equal to volume of container confining the gas

114. The vapour density of a gas is 11.2. The volume occupied by 11.2 g of this gas at N.T.P. is

22.4 liters

11.2 liters

2.24 liters

1 liter

115. The beaker contains slurry of ice and water, the three thermometers Fahrenheit, Kelvin and centigrade placed in it. The thermometers are represented as A, B and C respectively. On which thermometer the lowest reading will be?

A and C have same reading and are less then B

116. What is the concentration of nitrate ions, if equal volumes of 0.1 M AgNO₃ and 0.1 M NaCl are mixed together?

0.25 M

0.1 M

0.05 M

0.2 M

117. 100 g of CaCO₃ is treated with 1 liter of 1 NHCl. What would be the weight of CO₂ liberated after the completion of the reaction?

22 g

5.5 g

11 g

33 g

118. In which one of the following does the central atom not possess an ‘octet’ in its outer shell?

CH₄

NH₃

H₂O

BH₃

119. Crystalline solids can be identified easily from their

Colour

Definite geometry

Transition temperature

Sharp melting point

120. The pure crystalline substance on being heated gradually first forms a turbid liquid at constant temperature and still at higher temperature turbidity completely disappears. The behavior is a characteristic of substance forming

Liquid Crystals

Isomeric crystals

Allotropic crystal

Isomorphous crystals

121. The introduction of Kelvin scale in thermometry is according to

Charles’ law

Graham’s law

Boyle’s law

Dalton’s law

122. A malleable solid is one which can be

Converted into wires

Melted easily

Converted into sheets

All of these

123. Among solids, the highest melting point is exhibited by

Covalent solids

Molecular solids

Ionic solids

Pseudo solids

124. Gases deviate from ideal behavior at high pressure. Which of the following is correct for non – ideality?

A high pressure, the volume of the gas becomes insignificant

At high pressure, the gas molecules move in one direction only

At high pressure, the intermolecular attraction becomes significant

At high pressure, the collisions between the gas molecules are increased manifold

125. Number of atoms in 558.5 g of Fe (At. Mass of Fe = 55.85 g mole¯¹) is

Twice that in 60 g carbon

Half that in 8 g of He

558.5 x 6.022 x 10²³

6.022 x 10²²

Page 6 of 6

126. In which of the following compounds H – bonding is not present?

Ether

Ammonia

Water

Ethanol

127. Which one is not the partial pressure of oxygen in air

159 torr

159 mm Hg.

159 g/m³

159 g/Cm²

128. Which is distilled first?

Liquid H₂

Liquid CO₂

Liquid O₂

Liquid N₂

129. Current strength measure by electrometer by each type of ions in mass spectrometry shows?

Mass

Number of isotopes

Relative abundance

Charge

130. Solvent extraction is mostly applied to separate

Organic compounds

Both A and B

Inorganic compounds

None of these

131. The M.P of ice at Kelvin scale is 237K° and B.P of water is 373 K. This is a known fact that the molar volumes of different gases at S.T.P are

About the same as the molar volumes of liquids

Much larger than the molar volumes of liquids and solids

Little bit less than the molar volumes of solids

Little bit greater than the molar volumes of liquid

132. If the four tubes of a car are filled to the same pressure with N₂, O₂, H₂ and helium separately, then which one will be filled first

O₂

N₂

H₂

133. The ratio of most probable velocity to that of average velocity is

π/2

2/√π

√π/2

2/π

134. Triple point of water is

193 K

273 K

373 K

203 K

135. The most efficient solvent extraction method is by using

Single extraction and large portion of solvent

Repeated extraction and large portion of solvent

Repeated extraction and small portion of solvent

Single extraction and small portion of solvent

136. The total number of lattice arrangements in different crystal system is

8.0

3.0

7.0

137. Pressure remaining constant at which temperature the volume of a gas will become twice o what it is at 0°C

546 °C

0 K

546 K

200 °C

138. Ice is ________ crystal

Covalent

Molecular

Ionic

Metallic

139. Amorphous substances possess

Sharp melting points

Sharp B.P.

Definite heat of fusion

No definite heat of fusion

140. The phenomenon in which a compound exists in two or more crystalline forms is called

Polymorphism

Isomorphism

Anisotropy

Allotropy

141. Which of the following techniques is a type paper chromatography in which solvent is in a pool at the bottom of the vessel?

Descending paper chromatography

Liquid solid chromatography

Liquid gas chromatography

Ascending paper chromatography

142. What is the relative rate of effusion of CO and CO₂?

CO is 3.75 times faster than CO₂

CO is 1.25 times faster than CO₂

CO₂ is 1.25 times faster than CO

Both diffused at the same time

143. In NaCl type structure, the coordination numbers of cation and anions are

8 and 4

6 and 4

4 and 4

6 and 6

144. Which of the following substance is amorphous in nature?

Kcl

Sugar

Graphite

Plastic

145. Which is trigonal crystal?

CaSO₄.2H₂O

All

NaNO₃

MgSO₄

146. Crystalline solids can be identified easily by their

All of these

Transition temperature

Definite geometry

Sharp m.P

147. Glass is a

Super-cooled liquid

None of these

Gel

Micro-crystalline solid

148. Mean distance between atoms in the range of

2.5 nm

0.25 nm

25 nm

0.025 nm

149. The molar volume of CO₂ is maximum at

S.T.P (0°C and 1 atm)

0°C and 2 atm

273°C and 2 atm

127°C and 1 atm

150. Super conductors are derived from compounds of

Actinides

Lanthanides

p-block elements

Transition elements

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Maan AliLast Updated: April 19, 2025

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Chemistry Solids MCQS Online Test

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