ECAT Chemistry Chemical Bonding Chapter Online Test

Page 1 of 8

Chemistry

1. Which of the sub – atomic particles is not charged?

Electron

Neutron

All these

Proton

2. Which of the following will have highest value of electron affinity

F

I

Cl

Br

3. The value of e/m ratio of electron is:

1.7588 x 10²⁰

9.1095 x 10¯³¹

6.02 x 10²³

1.7588 x 10¹¹

4. Which of the following is not isoelectronic?

Cl¯

Na⁺

O²¯

Mg²⁺

5. Elements with ________ first ionization energies and ________ electron affinities generally from cations. Choose the correct point

Low, positive or slightly negative

Low very negative

High, very negative

None of these

6. In a double bond connecting two atoms there is a sharing of

2 electrons

1 electron

6 electrons

4 electrons

7. The correct set of quantum numbers (n, l and m) respectively of the unpaired electron of chlorine atom is:

2, 1, 0

3, 2, 1

2, 1, 1

3, 1, 1

8. The energy of a photon is given as, ∆ E/atom = 3.03 x 10¯¹⁹ J atom¯¹ then, the wavelength (λ) of the photon is

65.6 nm

6.56 nm

0.656 nm

656 nm

9. Fluorine has an atomic number 9 and Chlorine has 17. Which one has the highest electron affinity?

F

Cl

Cannot be determined

Both are equal

10. According to VESPR Model the geometry of molecule having 5 bond pair in outer most shell will be

Trigonal bipyramidal

Octahedral

Square planner

Triangular

11. Covalent compounds are soluble in

Polar solvents

Concentrated acids

Non-polar solvents

All solvents

12. Outermost shells of two elements X and Y have two and six electrons respectively. If they combine, the expected formula of compound will be

XY

X₂Y

X₂Y₃

XY₂

13. Which of the following has zero depolemoment?

ClF

CFCl₃

PCl₃

SiF₄

14. Pick out the molecule which has zero dipole moment

NH₃

H₂O

SO₂

BCl₃

15. In Millikan oil – drop experiment, the charges on several different oil drops were as: -5.92. – 4.44, -2.96, -8.88. The units are arbitrary. Choose the likely value of the electronic charge in these arbitrary units?

-1.48

-1.11

-2.96

-2.22

16. Geometry of simple molecule having sp3 hybrid orbital is

Square planner

Linear

Tetrahedral

Triangular

17. The number of anti-bonding electron pairs in O₂²¯ molecular ion on the basis of MOT is

3

4

2

5

18. Formulation of chemical bond between atoms of elements is based on

Electropositive character of elements

Octet rule

Electronegative character of elements

Pauli exclusion principle

19. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers l = 1 and l = 2 are respectively

12 and 4

16 and 4

12 and 5

16 and 5

20. Which orbital of the following has a principal quantum number of 3 and an angular momentum quantum number of 27?

3d

3s

4f

3f

21. Lewis acids are

Electron rich

Octet is complete

No such acids exist

Electron deficient

22. Which one of the following pairs of atoms is most likely to form an ionic bond?

C and F

N and F

Na and F

O and F

23. An electron has principal quantum number 3. The number of its (i) subshells and (ii) orbitals would be respectively

3 and 7

2 and 5

3 and 5

3 and 9

24. Which of the following orbitals have a dumb bell shape?

f

s

d

p

25. Which of the following has more unpaired d-electrons?

Ni³⁺

Fe²⁺

Cu⁺

Zn⁺

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26. Which one shows high % age of the ionic character?

H2O

HCI

HBr

HF

27. Energy released or absorbed when electrons are added in atom is

Activation energy

Electronegativity

Electron affinity

Ionization potential

28. H-bonding is not present in

Hydrogen sulphide

Hydrogen fluoride

Water

Glycerine

29. The shape of H₃O⁺ is

Angular

Pyramidal

Tetrahedral

Triangular planar

30. Al become isoelectronic with Ne

By gaining three electrons

By losing two electrons

By losing three electrons

By gaining two electrons

31. Nuclear radiation is emitted by those elements whose

Molecules are stable

Molecules are unstable

Nuclei are unstable

Nuclei are stable

32. Inter molecular forces in solid hydrogen are

Hydrogen bonds

All of these

Covalent forces

Van der Waal forces or London dispersion forces

33. The number of σ and π-bonds present in pent-4-en-l yne is

9, 4

4, 9

10, 3

3, 10

34. A molecule in which sp² hybrid orbitals are used by the central atom in forming covalent bonds is

SO₂

N₂

He₂

PCl₅

35. Which of the following phenomena will occur when two atoms of the elements having same spin of electron approach for bonding?

Bonding will not occur

Both A and B are correct

None of these

Orbital overlap will not occur

36. Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to the highest energy

Radio, visible, infrared, ultraviolet

Visible, ultraviolet, infrared, gamma rays

X – radiation, visible, infrared, microwave

Microwave, infrared, visible, ultraviolet

37. A chemist poured juice on soil. Which idea may he have in his mind?

There may be a possibility of a chemical reaction

There may not be a possibility of chemical reaction

Water should be preferred over lemon Juice for drinking

Lemon juice is dangerous for health

38. Noble gases are most stable of all other elements because

They have high ionization energies

They do not react with one another

They have completely filled s and p orbitals

They are mono atomic gases

39. Which one of these is weakest?

Metallic bond

Covalent bond

Ionic bond

Van der Waal’s forces

40. If the molecule of HCl were totally polar, the expected value of dipole moment is 6.12 D (Debye) but the experimental value of dipole moment was 1.03 D. Calculate the percentage ionic character.

50

83

17

Zero

41. Which of the following is a non-directional orbital

3S

4f

SP²

4d

42. If atomic numbers of nickel and copper are 28 and 29 respectively. Which of the following does the electronic configuration 1s² 2s² 2p⁶3s²3p⁶3d⁹ represent?

Ni

Cu⁺

Cu²⁺

Ni²⁺

43. The number and type of bonds between carbon atoms in calcium carbide are

Two sigma, one pi

One sigma, one pi

One sigma, two pi

Two sigma, two pi

44. When 6d orbital is complete, the entering electron goes into

7d

7s

7f

7p

45. Which of the following geometry is associated with the compound in which the central atom assumes sp³ d hybridization?

Angular

Trigonal bipyramidal

Pyramidal

Planar

46. Which of the solid does not contain covalent bond

Ice

Copper

Diamond

Graphite

47. Which of the following element’s outermost orbits last electron has magnetic quantum number m = 0?

Na

Cl

O

N

48. Geometry of molecule will be pyramidal if the outer post shell of the central atom has

1 bond pair 3 lone pair

3 bond pair one lone pair

3 lone pair 1 bond pair

2 bond pair 2 lone pair

49. Which of the following species is paramagnetic?

CO₂

CN¯

NO

O²¯

50. The central atom in BrF₅ has _?_ bonding pairs of electrons and _?_ non-bonding pairs of electrons.

1….5

0….5

5….0

5….1

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51. Which of the bonds, shown by the ___________ has the greatest polarity?

H – Cl

H – SH

H – OH

H – NH₂

52. Bond angle in water is

104.5°

107°

120°

109.5°

53. The electronegativity of elements in a period from left to right

First decreases then increases

First increases then decreases

Increases

Decreases

54. Molecular orbitals are filled according to

Aufbau principal

All these

Hund’s rule

Pauli’s exclusion principle

55. The nature of inter-particle forces in benzene is

Dispersion force

Ion-dipole interaction

H-bonding

Dipole-dipole interaction

56. The ionization energy

Increase from top to bottom in a group

Does not change in a group

Does not change in a period

Generally increases from left to right in a period

57. Which of the following species has lone pair of electrons on central atom?

N⁺H₄

CH₄

Pcl₄

PCl₃

58. Ionic radius in a period from left to right

First increases then decreases

Increases

Decreases

First decreases then increases

59. Colour of the glow produced in the discharge tube

Does not depend on the nature of the gas used in the discharge tube

Depends on the pressure in the discharge tube

Depends on the gas used in the discharge tube

60. Which has the minimum bond angle?

H₂S

H₂O

CH₄

NH₃

61. Azimuthal quantum number of last electron of ₁₁Na is

1

2

3

0

62. When two ice cubes are pressed over each other, they unite to form one cube. Which of the following forces is responsible to hold them together?

Hydrogen bond formation

Van der Waal’s forces

Dipole interaction

Covalent attraction

63. Ammonia has a net dipole moment while boron trifluoride has zero dipole moment because

Fluorides are more electronegative

Fluorides is more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Boron trifluoride is pyramidal in shape while NH₃ is planar

64. According to VSPER theory, ammonia molecule has --------- shape

Triangular

Pyramidal

Trigonal

Tetrahedral

65. In which of the following pairs, the numbers of electrons in the outermost shell are different?

As, Sb

Ge, Sn

In, Pt

Se, Te

66. Bond order for N2 molecule is

2

1

3

4

67. The total number of possible values of magnetic quantum number for the value of l = 3 is

1

7

5

3

68. Nitrogen gas is chemically inert gas due to the reason that

It has high heat of dissociation

Some of the electrons are also present in anti-bonding molecular orbitals

There is triple bond between nitrogen atoms which make the molecule quite stable

It has high electronegativity

69. Which of the following is to isoelectronic with rest of three?

Cl¯

Na⁺

S¯²

K⁺

70. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 2, l = 0

n = 1, l = 0

n = 1, l = 2

71. The shape of the molecule SF₂Cl₂ is

Trigonal bipyramidal

Cubic

Tetrahedral

Octahedral

72. With increasing principle quantum number, the energy difference between adjacent energy levels in H atom

Decreases for low value of Z and increases for higher value of Z

Decreases

Remains constant

Increases

73. Effective magnetic moment of Sc³ ion is

1.73

0

5.92

2.83

74. By combining n atomic orbital, numbers of hybrid orbitals will be

n

2 n

Impossible to predict

3 n

75. The spectrum of He is expected to be similar to that of

He⁺

H

Na

Li⁺

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76. The force which holds the atoms together to form a compound is known as

Chemical bond

Van der Waal’s force

London force

Dispersion force

77. The energy of the first electron in helium will be

-54.4 eV

-5.44 eV

-13.6 eV

Zero

78. Sodium chloride imparts a yellow colour to the Bunsen flame. This can be interpreted due to the

Emission of excess energy absorbed as a radiation in the visible region

Low ionization energy of sodium

Photosensitivity of sodium

Sublimation of metallic sodium to give yellow vapour

79. The shape of ClO₃ according to valence shell electron pair repulsion theory will be

Square planar

Tetrahedral

Pyramidal

Planar triangle

80. On sp3 hybridization

Four p-orbitals are involved

One p-orbital is involved

All p-orbitals are involved

One s and 3 p-orbitals are involved

81. The bond order in NO is 2.5 while that is NO⁺ is 3. Which of the following statements is true for these two species?

Bond length in NO⁺ is greater than in NO

Bond length in NO⁺ is equal to that in NO

Bond length in NO is greater than in NO⁺

Bond length is unpredictable

82. Which of the following is the best explanation that CO₂ is a non-polar molecule?

Dipole moment is zero

SP hybridization

None

Linear geometry

83. Which hydrogen halide among the following has the highest percentage of ionic character?

HF

HCl

HBr

HI

84. Which molecule is polar among the following?

Ethane

Carbon tetrachloride

Carbon dioxide

Methanol

85. Which of the following has the greatest covalent character?

SiCl₄

AlCl₃

MgCl₂

NaCl

86. Which of the following is a non-directional orbital?

SP²

3S

4f

4d

87. In O2 each oxygen atom is hybridized

All

Sp2

Sp

Sp3

88. Molecular orbital picture of N₂ indicates

Two unpaired electron

No unpaired electron

One unpaired electron

None of these

89. Water (H₂O) is liquid while hydrogen sulphide (H₂O) is a gas because

Hydrogen sulphide is a weak acid

Water has higher molecular weight

Water molecules associate through hydrogen bonding

Sulphure has high electronegativity than oxygen

90. The relative attraction of the nucleus for the electrons in a chemical bond is called

Ionization energy

Electro negativity

None of these

Electron affinity

91. The spectrum of helium is expected to be similar to that of

Li⁺

Na

H

He⁺

92. Which of the following would have a permanent dipole moment?

XeF₄

SiF₄

SF₄

BF₃

93. When 2 lone pair and 2 bond pair are around the central atom reduction in the bond angle is up to. (in degrees)

102

107.5

104.5

109.5

94. The third line of the Balmer series, in the emission spectrum of the hydrogen atom, is due to the transition from the

Seventh Bohr orbit to the third Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

95. 1 erg of energy corresponds to

6.02 x 10¹⁶ J/mol

6.02 x 10²³ J/mol

1 erg/mol

10¯⁷ J/mol

96. Which quantum number is sufficient to describe the electron is hydrogen atom?

s

l

n

m

97. In the ground state, an element has 13 electrons in its M shell. The element is

Iron

Nickel

Chromium

Copper

98. Unit of dipole moment is

Poise

Newton

Pascal

Debye

99. The bond angle H – O – H in ice is closest to

109°

90°

120°

60°

100. Anti-bonding MO is formed by

Addition of atomic orbitals

None of these

Subtraction of atomic orbitals

Multiplication of atomic orbitals

Page 5 of 8

101. The carbon atoms in calcium carbide are held by

2 covalent, one co-ordinate bond

2π and one σ bond

Ionic bonds

2 sigma bonds

102. Number of sigma bonds in P₄O₁₀ is

17

7

16

6

103. The number of d-electrons retained in Fe²⁺ (At. No. of Fe = 26) ions is

3

6

4

5

104. The number of significant figures in 0.00200 is

Two

Five

Three

One

105. In BrF₃ molecule, the lone pairs occupy equatorial positions to minimize

Lone pair – lone pair repulsion only

Bond pair – bond pair repulsion only

Lone pair – bond pair repulsion only

Lone pair – lone pair repulsion and lone pair – bond pair repulsion

106. The electro negativities of F, Cl, Br and I are 4.0, 3.0, 2.8, 2.5 respectively. Hydrogen halide with a high percentage of ionic character is

HBr

HF

HCl

Hl

107. A lone pair of electrons in an atom implies

A pair of electrons

A pair of valence electrons

A pair of electrons involved in bonding

A pair of valence electrons not involved in bonding

108. Which of the following hydrides has the lowest boiling point?

H₂S3

H₂O

H₂Te

109. Which is not true with respect to cathode rays?

Can be deflected by magnetic fields

A stream of electrons

Charged particles

Move with speed as that of light

110. When potassium metal is exposed to violet light

Ejection of some potassium atoms occurs

The absorption of electrons takes place

There is no effect

Ejection of electrons takes place

111. Which one among the following does not have the hydrogen bond?

Water

Liquid NH3

Liquid HCl

Phenol

112. The energy required to remove electron from an atom is called

I.P

Ea.

E.A

E.N

113. Fluorine molecule is formed by

The axial s-p overlap

The axial p-p overlap

The sidewise p-p overlap

The overlap of two sp² hybrid orbitals

114. The velocity of photon is

Depends on its wavelength

Independent of its wavelength

Depends on its source

Equal to square

115. Maximum hydrogen bonds in water are,

2

3

8

4

116. Choose the correct statement about 2nd ionization energy

It may be greater or less than the 1st ionization depending upon ht nature of the element

It is equal to the 1st ionization energy

It is always less than 1st ionization energy

It is always greater than 1st ionization energy

117. Along a period the atomic radii

Constant

Decreases

Increases

First decreases then increases

118. When two hydrogen atoms approach to form a chemical bond

The attractive forces dominate the repulsive forces

The repulsive force dominate the attractive forces

They energy of atoms increases

The two atoms start ionization

119. Geometry of simple molecule having SP³ hybrid orbital is

Square planner

Tetrahedral

Linear

Triangular

120. For principle quantum number, n = 4, the total number of orbitals having 1 = 3 is

5

7

3

9

121. In which one of the following does the central atom not possess can octet in its outer shell?

H₂O

CH₄

BH₃

NH₃

122. Which kinds of bonding can be found in a sample of H₂O(l)?

Hydrogen bonds only

Both polar covalent and hydrogen bonds

Nonpolar covalent bonds only

Ionic and nonpolar hydrogen bonds

123. Which of these molecules require more bond energy?

Nitrogen

Oxygen

CO

Hydrogen

124. An oxygen atom has mass of

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

5.316 x 10¯²³ g

125. A long a period E.N __________ from left to right

Variable trend

Increases

Decreases

Constant

Page 6 of 8

126. The relative attraction of the nucleus for the electrons in a chemical bond is called

None of these

Ionization energy

Electronegativity

Electron affinity

127. Deflection of blue light is lesser than violet because

Blue has higher wavelength

Blue is absorbed more easily

Blue is darker colour

Blue has more energy

128. According to VSEPR theory, the shape of the water molecule is

Distorted tetrahedral

Planar triangle

Linear

Octahedral

129. Choose the correct statement

In molecular orbitals, the number of bonding electrons equals the number of anti-bonding electrons

As bonding molecular orbitals become more stable, anti-bonding molecular orbital become equally less stable

Each bonding molecular orbital can accommodate only one electron

The molecular orbitals in a molecule equals twice the number of constituent atomic orbitals

130. If the radius of first Bohr orbit be ɜ₀, then the radius of third Bohr orbit would be

3 x ɜ₀

1/2 x ɜ₀

6 x ɜ₀

9 x ɜ₀

131. The boiling point of heavy water is

99°C

108°C

101.4°C

110°C

132. In acetylene molecule, the two carbon atoms are linked by

Two sigma bonds and one pi-bond

Three sigma bonds

One sigma bond and two pi-bonds

Three pi-bonds

133. The relative attraction of the nucleus for the electrons in a chemical bond is called

Ionization energy

Electron affinity

None of these

Electro negativity

134. The structure of ICl₂¯ is

Square planar

Trigonal bipyramidal

Octahedral

Trigonal

135. The configuration 1s² 2s² 2p⁵ 3s¹ shows

Excited state of neon

Ground state of fluorine atom

Excited state of O¯₂

Excited state of fluorine

136. The twelve enter most electrons in O₂ molecule are distributed according to MOT as under. Find the correct one.

10 in bonding molecular orbitals and 2 in anti-bonding molecular orbitals

12 in bonding molecular orbitals, and zero in anti-bonding molecular orbitals

9 in bonding molecular orbitals and 3 in anti-bonding molecular orbitals

8 in bonding molecular orbitals, 4 in anti-bonding molecular orbitals

137. Number of π-bonds in naphthalene is

4

6

3

5

138. Which of the following contains both polar and non-polar bonds?

CH₄

NH₄Cl

H₂O₂

HCN

139. Which of the following is the correct electron – dot formula of CO₂?

A

B

D

C

140. When a double bond is formed between two atoms, one of the bonds is a sigma bond and the other is a pi bond. The pi bond is created by the overlap of……

p orbitals

sp³ hybrid orbitals

sp² hybrid orbitals

s orbitals

141. Shape of CIO₃¯ is

Triangular planar

Triangular bipyramidal

Tetrahedral

Triangular pyramidal

142. Which of the following molecules does not have a net dipole moment?

H₂O

BF₃

NH₃

BrF₃

143. Which one of the following molecules shows high percentage of ionic character?

H₂O

HCl

HBr

HF

144. Energy of an atom in a compound is

Higher than individual

Lesser than individual

Impossible to predict

No change

145. How many sigma and pi bonds are present in tetra cyano ethylene?

Nine σ and seven π

Eight σ and eight π

Five π and nine σ

Nine σ and nine π

146. Which carbon is more electronegative?

sp- hybridized carbon

always same irrespective of its hybrid state

sp²- hybridized carbon

sp³-hybridized carbon

147. Unit of dipole moment is

Poise

Debye

Pascal

Newton

148. Which of the following has unchanged valency?

Oxygen

Na

Fe

H

149. Which of the following has maximum e/m value for positive rays?

Nitrogen

Helium

Hydrogen

Oxygen

150. Hydrogen chloride molecule contains

Covalent bond

Double bond

Electrovalent bond

Co-ordinate bond

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151. Pi bonds are produced by overlapping of

Atomic orbital and hybrid orbital

Hybrid orbitals

Un-hybrid orbitals

Hybrid and un hybrid orbitals

152. ____________ has their outermost shell complete in atomic form

Coinage metals

Alkali metals

Noble gases

Gun metals

153. Which of the following value of Electronegativity difference corresponds the formation of Ionic Bond?

Equal to 1.7

Lesser then 1.7

No specificity exist

Greater than 1.7

154. The four quantum numbers of the valency electron of potassium are

4, 1, 0, ½

4, 1, 1, ½

4, 0, 0, ½

4, 4, 0, ½

155. The de-Broglie wavelength of a particle with mass 1 g and velocity 100 m/s is

6.63 x 10¯³⁴ m

6.65 x 10¯³⁵ m

6.63 x 10¯³³ m

6.63 x 10¯³⁵ m

156. What happens to IP value if shielding effect is greater?

Remain same

Lesser

Greater

No effect

157. Which of the following molecule has Ā bond

C₃H₆

O₂

H₂O

NH₃

158. Which of the following molecules has no net dipole moment?

CCl₄

CH₃Cl

HCl

H₂O

159. Keeping in view the bonding molecular orbitals, find the incorrect statement

Bonding molecular orbitals have low electron density between the two nuclei

Bonding molecular possess less energy than atomic orbitals from which they are formed

Every electron in the bonding molecular orbital contributes to the attraction between atoms

Bonding molecular orbitals are formed when the electrons waves are undergo constructive interference

160. Which of the following compounds can form hydrogen bond?

CHCl₃

NaCl

CH₄

H₂O

161. Element having the smallest atomic radius among the following is

Rb

Sr

Ne

Li

162. XeF₄ has shape of

Tetrahedral

Sphere

Trigonal bipyramidal

Square planar

163. Among the alkaline earth metals the element forming predominantly covalent compounds is

Be

Calcium

Sr

Mg

164. In CCl₄, the four valencies of carbon are directed towards the corners of a

Prism

Hexagon

Cube

Tetrahedron

165. Atom with higher atomic number produces X-rays of

Larger wavelength

X-rays not produced

Shorter wavelength

Gamma rays

166. According to MO theory, the species O⁺₂ possesses

Stability lower then O₂

Three unpaired electrons

Diamagnetic character

Bond order of 2.5

167. Find the magnetic moment of a divalent ion in aqueous solution if its atomic number is 25

6.9 BM

3.0 BM

4.9 BM

5.9 BM

168. Which of the following is not absolute term of element?

Ionization energy

Electron affinity

Atomic size

Electronegativity

169. Bohr’s model atom is contradicted by

Quarternization of angular members

Quarternization of energy of electrons

Heisenberg’s uncertainty principle

Plank’s quantum theory

170. The most suitable method of the separation of a mixture of ortho and para-nitrophenol mixed in the ratio of 1 : 1 is

Crystallization

Vaporization

Colour spectrum

Distillation

171. The atomic number of an element is 35. What is the total number of electrons present in all the p-orbitals of the ground state atom of that element?

23

11

6

17

172. The nature of positive rays depends upon

All of these

The nature of electrode

The nature of discharge tube

The nature of residual gas

173. In OF₂, number of bond pairs and lone pairs of electrons are respectively

2, 10

2, 9

2, 6

2, 8

174. Lateral overlapping expected in

Ā-bonds

O-bond

Metallic bond

Ionic bond

175. Which of the following statements about positive ions is incorrect?

They are smaller than the atoms from which they were formed

They are also known as cations

They are formed when electros are formed from atoms

They are larger than the atoms from which they were formed

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176. 2nd orbit is away from nucleus for H-atom as compared to first orbit

6-times

4-times

3-times

2-times

177. A student subtracted 0.00055 from 10.2345678 and reported the result as 10.23401. But his friend told him that result was wrong. What is the correct result?

10.234

10.23

10.234017

10.2340178

178. Force responsible to hold atoms together in a compound is called

All of above represent same entity

Bond

Attractive force

Interaction

179. Which of the following equation represents the 1^st ionization energy of Na?

B

C

A

D

180. If the value of principal quantum number is 3, the total possible values for magnetic quantum number will be

9

1

12

4

181. How many molecular orbitals may be constructed from the valence shell orbitals of the constituent atoms in CH₄?

7

8

4

6

182. Electronic configuration of K is

[AR]4S¹

[AR]4S²

[Kr]4S¹

[He]4S¹

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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