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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.
Test Helpful For:	ECAT Entry Test Chemistry Online Test Interview Questions about Chemisttry All Universities Entrance Test Recruitments Tests

ECAT Chemistry Solids Test

Page 1 of 6

Chemistry

1. Crystalline solids can be identified easily by their

Sharp m.P

Transition temperature

All of these

Definite geometry

2. Which of the following is a pseudo solid?

All these

NaCl

Glass

CaF₂

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

NH₃ and BF₃

NH₃ and H⁺

CH₄ and AlCl₃

H₂O and H⁺

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

Bcc

Fcc

None of these

Both fcc and bcc

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

Trigonal

Triclimic

Mexagonal

Monoclimic

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

0.1 M

0.25 M

0.2 M

0.05 M

7. 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

3 liter atm

2 liter atm

8. Glass is a

Micro-crystalline solid

Super-cooled liquid

Gel

None of these

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

Increase of intermolecular interactions

Decrease of surface tension

Increase of K.E of molecules

Increase in potential energy of molecules

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

The carbon atoms are arranged layers

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

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

The coordination number of carbon atoms is 4

11. Amorphous substances possess

No definite heat of fusion

Sharp melting points

Sharp B.P.

Definite heat of fusion

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

13. Which solids are called true solids?

Crystalline

Vitreous

Metallic

Amorphous

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

4 x 6.02 x 10²³

6.02 x 10²³

3/2 x 6.02 x 10²³

2 x 6.02 x 10²³

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

0.32 g

0.64 g

0.16 g

0.96 g

16. 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

H₂

N₂

17. 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

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

The filtrate is quick

Filtrate runs down without crystals

This gives bigger size crystals

This gives medium size crystals

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

546 °C

200 °C

0 K

546 K

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

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

None of these

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.

21. 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

4 atm

2 atm

1 atm

3 atm

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

HgS

Agl

Csl

Cul

23. Which of the following is isotropic

Mercury

Graphite

Brass

Borax

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

Divalent impurity

Pentavalent impurity

Trivalent impurity

Tetravalent

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

Gets a single positive charge

Gets a double negative charge

Gets a single negative charge

Gets a double positive charge

Page 2 of 6

26. The mass of one mole of electron is

1.673 mg

1.008 mg

0.55 mg

0.104 mg

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

BH₃

NH₃

H₂O

CH₄

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

8.31 JK¯¹ mol¯¹

8.31 L atm K¯¹ mol¯¹

8.31 x 10⁷ dynes Cm K¯¹ mol¯¹

8.31 x 10⁷ erg³ K¯¹ mol¯¹

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

N and F

Na and F

C and F

O and F

30. Ice is ________ crystal

Metallic

Molecular

Covalent

Ionic

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

1 atm, and 273 K

15 tm, and 500 K

0.5 atm, and 500 K

15 atm, and 200 K

32. Super conductors are derived from compounds of

Transition elements

p-block elements

Actinides

Lanthanides

33. Solvent extraction is mostly applied to separate

Inorganic compounds

Both A and B

None of these

Organic compounds

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

C₃H₅O₂

C₄H₁₀O₂

C₃H₁₀O₂

C₆H₁₀O₄

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

Tetrahedron

Octahedron

Triangle

Cube

36. The most efficient solvent extraction method is by using

Repeated extraction and large portion of solvent

Single extraction and small portion of solvent

Repeated extraction and small portion of solvent

Single extraction and large portion of solvent

37. 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) + +¯

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

100 mm of Hg

1489 mm of Hg

790 mm of Hg

700 mm of Hg

39. How many allotropic forms are present in carbon?

Five

Two

Four

Three

40. 4.4 g of CO₂ contains how many liters of CO₂ at STP?

2.24 liter

44 liter

2.4 liter

22.4 liter

41. The crystal structure having face centered cubic arrangement is

CsCl

BaCl₂

NaCl

CuCl

42. Which of the following substances is not amorphous?

Rubber

Polymer

Glass

Ag NO₃

43. Which is trigonal crystal?

All

MgSO₄

NaNO₃

CaSO₄.2H₂O

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

Graham’s law

Boyle’s law

Charles’ law

Dalton’s law

45. Under what conditions real gases deviate from ideal behavior

High pressure

Both b and c

Low temperature

High temperature

46. 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:

Three

Two

Four

Five

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

None of these

48. Amorphous solids

Have sharp melting point

Have perfect arrangement of atoms

Can possess small regions of orderly arrangement of atoms

Undergo clean cleave when cut with knife

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

Charles’ law

Boyle’s law

Dalton’s law

Avogadro’s law

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

Anisotropy

Isomorphism

Polymorphism

Allotropy

Page 3 of 6

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

1.12 dm³

22.4 dm³

2.24 dm³

112 cm³

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

Unit

None

Cleavage

Crystal

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

558.5 x 6.022 x 10²³

Twice that in 60 g carbon

6.022 x 10²²

Half that in 8 g of He

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

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

Molecules of all the gases have same size and same mass

All molecular collisions are elastic

Molecules are in chaotic motion

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

NO₂

MnO₂

TiO₂

CrO₂

56. The example of hexagonal system is

Sulphur

Diamond

Graphite

Sugar

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

Increased attraction between the molecules

Decreased volume of the solution

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

Decreased covalent and hydrogen bond forces

58. Bragg’s law is given by equation

2nλ = d sin θ

nλ = 2 d sin θ

nλ = 2 θ sin θ

nλ = 1/2d sin θ

59. Poor conductors of electricity is a characteristic of

Metallic compounds

Diatic bonds

Covalent compounds

Ionic compounds

60. 50dm³ of CO is burnt completely according to reaction 2CO + O₂ – 2CO₂ Choose the correct statement

Volume of O₂ required is 25 dm³

Volume of CO₂ formed is 25 dm³

Volume of CO₂ formed is 60 dm³

Volume of O₂ required is 50 dm³

61. 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

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

None

Slowly

Moderately

Fast

63. Which of the following are more temperature sensitive?

Ionic crystals

None of these

Solid crystals

Liquid crystals

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

Altahydral manner

Square planner manner

Tetrahedral manner

Hexagonal manner

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

Charge

Relative abundance

Number of isotopes

Mass

66. Crystalline solids can be identified easily from their

Transition temperature

Colour

Definite geometry

Sharp melting point

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

Acetic acid

Acetone

Sulphuric acid

Chloroform

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

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

Gases do not have a definite shape and volume

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

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

69. Isotopes differ in

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

Properties which depend upon mass

Arrangement of electrons in orbitals

Chemical properties

70. Which forms metallic crystals?

NaCl

SO₂

NH₄Cl

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

Polymorphism

None of these

Isomorphism

Amorphism

72. The molar volume of CO₂ is maximum at

0°C and 2 atm

S.T.P (0°C and 1 atm)

273°C and 2 atm

127°C and 1 atm

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

Copper

Zinc

Sodium

Magneisum

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

All

Chromatography

Crystallization

Solvent extraction

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

CO is 3.75 times faster than CO₂

Both diffused at the same time

CO₂ is 1.25 times faster than CO

CO is 1.25 times faster than CO₂

Page 4 of 6

76. Particles that most effects material properties

Protons

Valence electrons

Neutrons

Electrons

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

Pressure of dust particles in air

Elastic collisions of gas molecules

Non-polar nature of gases

Different molar mass

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

A gas is liberated

Oxide of the gas is strongly acidic

Colour of the gas is greenish yellow

The gas is chlorine

79. Potassium crystallizes with a

Triclinic

Orthogonal lattice

Cubic lattice

Ortho rhombic lattice

80. 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

Ascending paper chromatography

Liquid solid chromatography

Liquid gas chromatography

81. 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?

5.5 g

22 g

33 g

11 g

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

High solubility

High concentration

High ignition temperature

Low temperature

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

71g

35.5g

18.75g

142g

84. 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)

9.333 atm

10.33 atm

9.2 atm

9.74 atm

85. A solid may be made up of

Atoms

Molecules

Ions

A, B and C

86. 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

XY₂

X₃Y

XT₃

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

Anisotropy

Allotropy

Polymorphism

Isomorphism

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

Vaporization

Filtration

Sublimation

Condensation

89. ‘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

90. Repeatable entity of a crystal structure is known as

Crystal

Lattice

Unit cell

Miller indices

91. Solvents of covalent compounds include all but

Alcohol

Water

Petrol

Tetra chloromethane

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

4 and 4

6 and 4

8 and 4

6 and 6

93. The material possessing superconducting properties is

Yb Ba₂Cu₂O₈

Hg Be₂Ca₂Cu₂O₈

Y B₂Cu₃O₇

Y Ba₂Cu₃O₇

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

P/d

√P/d

P/√d

None of these

95. Crystals can be classified into

7 crystal systems

3 crystal systems

14 crystal systems

4 crystal systems

96. The allotropic forms of an element are called

Unit Cell

Isoelectronic

Cleavage

Allotropes

97. 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

Decrease twice

Be a function of the molecular mass of substance

Remains unchanged

Increase two fold

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

4400

4800

3200

1524

99. In case of elements the polymorphism is called

Isomorphism

Isotopic form

Crystalline forms

Allotropy

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

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

A high pressure, the volume of the gas becomes insignificant

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

At high pressure, the intermolecular attraction becomes significant

Page 5 of 6

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

0°C and 2.0 atm

100°C and 2.0 atm

-10°C and 5.0 atm

-10°C and 2.0 atm

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

B evaporates more readily than A

A and B evaporates at the same rate

B evaporates less readily than C

A evaporates more readily than C

103. 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

Add water to the mixture and filter

Add dilute acid to the mixture and filter

Place the mixture in a separating funnel

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

Double

Same

Half

None

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

2.016

22.4

20.16

2.24

106. Isomorphic substances have

Same physical and different chemical properties

Different physical and same chemical properties

Different physical and chemical properties

Same physical and chemical properties

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

Graphite

Kcl

Sugar

Plastic

108. Correct order of intermolecular forces

Gas = liquid = solid

Liquid < gas < solid

Gas < liquid < solid

109. Which is distilled first?

Liquid H₂

Liquid CO₂

Liquid O₂

Liquid N₂

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

5.0 moles of SO₂

44.8 dm3 CO₂ at S.T.P

20 moles of S8

6 moles of S

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

159 torr

159 g/m³

159 mm Hg.

159 g/Cm²

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

1.4 x 10¯²¹ g

5.01 x 10¯²¹ g

3.72 x 10¯²³ g

1.3 x 10¯²⁰ g

113. 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 0.5 M

10 mL of 0.02 M

5 mL of 0.1 M

10 mL of 0.1 M

114. Fluted filter paper is used for

Increasing the rate of filtration

Filtering the hot saturated solution

To dissolve large amount of substance at its boiling point

To avoid premature crystallization of the solute

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

Ammonia

Water

Ether

Ethanol

116. Half atmospheric pressure is

101.325 Pa

400 torr

50 662 Pa

8.5 Pounds

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

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

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

One mole of NH₃ will produce ½ mole of N₂

One mole of NH₃ will produce 6 moles of N₂

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

1.5057 x 10 ²⁴

2.0478 x 10 ²⁴

4.0956 x 10 ²⁴

3.0115 x 10 ²⁴

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

Free valence electrons

Anions

Ione pair of electrons

Cations

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

AB₂ type ionic compound

NaCl type structure

ZnS type structure

CsCl type structure

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

√π/2

2/π

2/√π

π/2

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

Causing pressure

Randomly moving

Having wide spaces

Orderly arranged

123. Isomorphic substance have

Different physical and same chemical properties

Different physical and chemical properties

Same physical and difference chemical properties

Same physical and chemical properties

124. Simple molecules or giant macromolecules are examples of

Metallic bonds

Ionic compounds

Diatic bond

Covalent bonds

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

They melt over a range of temperature

They are anisotropic

There are rigid and in-compressible

There is no orderly arrangement of particles

Page 6 of 6

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

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

128. 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 unchanged

Is changed by about 26%

129. 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

Isomorphous crystals

Allotropic crystal

Liquid Crystals

Isomeric crystals

130. Which of the following has least mass?

2 gram atom of nitrogen

1 mole of S

3 x 10²³ atoms of C

7.0 g of Ag.

131. Mean distance between atoms in the range of

25 nm

2.5 nm

0.25 nm

0.025 nm

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

Isotropical

Triclinic

Monoclinic

Rhombohedral

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

1 liter

22.4 liters

2.24 liters

11.2 liters

134. Formation of a cation is?

Redox

Reduction

Oxidation

None

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

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

1 : 2

1 : 3

2 : 1

1 : 1

137. A malleable solid is one which can be

Melted easily

Converted into sheets

All of these

Converted into wires

138. Ionic solids are characterized by

Good conductivity in solid state

Low melting points

High vapour pressures

Solubility in polar solvents

139. Triple point of water is

193 K

373 K

203 K

273 K

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

Electrical attraction

Covalent bond

Non covalent bond force

Electrostatic force

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

7.0

3.0

8.0

142. 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

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

He will feel warmth

He will feel cool

His blood pressure will increase

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

Ionic solids

Covalent solids

Pseudo solids

Molecular solids

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

Rhombic

Tetragonal

Monoclinic

Trigonal

145. 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

Little bit less than the molar volumes of solids

Much larger than the molar volumes of liquids and solids

About the same as the molar volumes of liquids

Little bit greater than the molar volumes of liquid

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

1/5

1/25

147. Van der Waal’s forces exist in

Non-polar

All types of atoms and molecules

Covalent

Polar compounds

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

Both A & B

None

Normal filter paper

Fluted filter paper

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

CsBr

AgBr

NH₄Br

CuBr

150. Amorphous substance posses

No definite geometry

No sharp melting points

No definite heat of fusion

All of these

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Maan AliLast Updated: April 19, 2025

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ECAT Chemistry Solids Online Test

Chemistry Solids MCQS Online Test

ECAT Chemistry Solids Chapter Online Test

ECAT Chemistry Solids Test

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Chemistry Solids MCQS Online Test

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