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ECAT Chemistry Chemical Bonding Online Test

Maan AliLast Updated: April 19, 2025

Chemistry Chemical Bonding MCQS Online Test

ECAT Chemistry Chemical Bonding Chapter Online Test

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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ECAT Chemistry Chemical Bonding Test

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Page 1 of 8

Chemistry

1. 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.

Zero

2. Lateral overlapping expected in

Ā-bonds

Metallic bond

Ionic bond

O-bond

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

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

10 in bonding molecular orbitals and 2 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

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

Cannot be determined

Both are equal

5. Bohr’s model atom is contradicted by

Heisenberg’s uncertainty principle

Quarternization of angular members

Quarternization of energy of electrons

Plank’s quantum theory

6. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 1, l = 0

n = 1, l = 2

n = 2, l = 0

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

Ge, Sn

As, Sb

In, Pt

Se, Te

8. ____________ has their outermost shell complete in atomic form

Gun metals

Alkali metals

Coinage metals

Noble gases

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

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

Both polar covalent and hydrogen bonds

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

Hydrogen bonds only

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

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

MgCl₂

NaCl

SiCl₄

AlCl₃

13. The nature of positive rays depends upon

The nature of residual gas

All of these

The nature of electrode

The nature of discharge tube

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

Impossible to predict

2 n

3 n

15. Which one of these is weakest?

Ionic bond

Metallic bond

Van der Waal’s forces

Covalent bond

16. Molecular orbital picture of N₂ indicates

No unpaired electron

One unpaired electron

None of these

Two unpaired electron

17. Ionic radius in a period from left to right

First increases then decreases

Decreases

First decreases then increases

Increases

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

4, 1, 1, ½

4, 1, 0, ½

4, 4, 0, ½

4, 0, 0, ½

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

6.63 x 10¯³³ m

6.63 x 10¯³⁴ m

6.65 x 10¯³⁵ m

6.63 x 10¯³⁵ m

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

Fluorides is more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides are more electronegative

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

A stream of electrons

Move with speed as that of light

Charged particles

Can be deflected by magnetic fields

22. 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

HCl

HBr

23. Which of the following species is paramagnetic?

O²¯

CN¯

CO₂

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

None of these

Electron affinity

Ionization energy

Electro negativity

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

The two atoms start ionization

The repulsive force dominate the attractive forces

They energy of atoms increases

The attractive forces dominate the repulsive forces

Page 2 of 8

26. 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

Sixth Bohr orbit to the third Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

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

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

Lone pair – bond pair repulsion only

Lone pair – lone pair repulsion only

Bond pair – bond pair repulsion only

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

Dispersion force

London force

Chemical bond

Van der Waal’s force

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

3, 2, 1

3, 1, 1

2, 1, 0

2, 1, 1

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

Distillation

Colour spectrum

Crystallization

Vaporization

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

N₂

PCl₅

He₂

SO₂

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

Two sigma, one pi

One sigma, one pi

Two sigma, two pi

One sigma, two pi

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

Increases

First decreases then increases

First increases then decreases

Decreases

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

Decreases

Increases

Remains constant

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

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

Nine σ and nine π

Five π and nine σ

Eight σ and eight π

Nine σ and seven π

36. The structure of ICl₂¯ is

Octahedral

Trigonal bipyramidal

Trigonal

Square planar

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

Bonding molecular orbitals have low electron density between the two nuclei

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

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

38. Which of the following is not isoelectronic?

Mg²⁺

Cl¯

O²¯

Na⁺

39. Inter molecular forces in solid hydrogen are

Van der Waal forces or London dispersion forces

All of these

Hydrogen bonds

Covalent forces

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

C and F

O and F

N and F

Na and F

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

One sigma bond and two pi-bonds

Three pi-bonds

Two sigma bonds and one pi-bond

Three sigma bonds

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

Visible, ultraviolet, infrared, gamma rays

X – radiation, visible, infrared, microwave

Radio, visible, infrared, ultraviolet

Microwave, infrared, visible, ultraviolet

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

Larger wavelength

Shorter wavelength

X-rays not produced

Gamma rays

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

109°

60°

120°

90°

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

3 bond pair one lone pair

2 bond pair 2 lone pair

1 bond pair 3 lone pair

3 lone pair 1 bond pair

46. Which has the minimum bond angle?

CH₄

NH₃

H₂S

H₂O

47. Bond angle in water is

104.5°

120°

107°

109.5°

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

Water should be preferred over lemon Juice for drinking

Lemon juice is dangerous for health

There may be a possibility of a chemical reaction

There may not be a possibility of chemical reaction

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

-5.44 eV

-13.6 eV

Zero

-54.4 eV

50. A lone pair of electrons in an atom implies

A pair of electrons

A pair of electrons involved in bonding

A pair of valence electrons not involved in bonding

A pair of valence electrons

Page 3 of 8

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

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

Ion-dipole interaction

Dispersion force

H-bonding

Dipole-dipole interaction

53. Which of these molecules require more bond energy?

Nitrogen

Oxygen

Hydrogen

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

H₂Te

H₂O

H₂S3

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

9 x ɜ₀

1/2 x ɜ₀

6 x ɜ₀

3 x ɜ₀

56. Unit of dipole moment is

Newton

Pascal

Debye

Poise

57. 2nd orbit is away from nucleus for H-atom as compared to first orbit

3-times

6-times

2-times

4-times

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

Cu²⁺

Ni²⁺

Cu⁺

59. Effective magnetic moment of Sc³ ion is

2.83

5.92

1.73

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

Bond

Interaction

All of above represent same entity

Attractive force

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

Greater

No effect

Remain same

Lesser

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

Helium

Oxygen

Nitrogen

Hydrogen

63. The shape of H₃O⁺ is

Angular

Tetrahedral

Pyramidal

Triangular planar

64. 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?

Dipole interaction

Hydrogen bond formation

Van der Waal’s forces

Covalent attraction

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

107.5

104.5

102

109.5

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

SP²

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

2, 10

2, 6

2, 8

2, 9

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

Greater than 1.7

Lesser then 1.7

Equal to 1.7

No specificity exist

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

Stability lower then O₂

Diamagnetic character

Bond order of 2.5

Three unpaired electrons

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

HBr

HCl

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

They are smaller than the atoms from which they were formed

They are larger than the atoms from which they were formed

They are formed when electros are formed from atoms

They are also known as cations

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

Trigonal bipyramidal

Square planner

Octahedral

Triangular

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

Liquid NH3

Water

Liquid HCl

Phenol

74. Lewis acids are

Electron deficient

Electron rich

No such acids exist

Octet is complete

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

1.7588 x 10¹¹

1.7588 x 10²⁰

6.02 x 10²³

9.1095 x 10¯³¹

Page 4 of 8

76. Unit of dipole moment is

Poise

Debye

Pascal

Newton

77. Energy of an atom in a compound is

Higher than individual

No change

Lesser than individual

Impossible to predict

78. Al become isoelectronic with Ne

By losing two electrons

By gaining two electrons

By losing three electrons

By gaining three electrons

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

Calcium

80. The velocity of photon is

Depends on its source

Depends on its wavelength

Equal to square

Independent of its wavelength

81. Geometry of simple molecule having sp3 hybrid orbital is

Tetrahedral

Triangular

Square planner

Linear

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

83. The number of significant figures in 0.00200 is

Five

Three

Two

One

84. 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?

-2.22

-1.11

-1.48

-2.96

85. The boiling point of heavy water is

99°C

110°C

101.4°C

108°C

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

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

He⁺

Li⁺

88. 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

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

Depends on the gas used in the discharge tube

89. Geometry of simple molecule having SP³ hybrid orbital is

Linear

Square planner

Tetrahedral

Triangular

90. Fluorine molecule is formed by

The axial s-p overlap

The sidewise p-p overlap

The axial p-p overlap

The overlap of two sp² hybrid orbitals

91. Which of the solid does not contain covalent bond

Diamond

Graphite

Ice

Copper

92. H-bonding is not present in

Glycerine

Water

Hydrogen sulphide

Hydrogen fluoride

93. Hydrogen chloride molecule contains

Covalent bond

Co-ordinate bond

Electrovalent bond

Double bond

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

95. Which of the following has zero depolemoment?

PCl₃

CFCl₃

ClF

SiF₄

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

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

H – Cl

H – SH

H – NH₂

H – OH

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

X₂Y

XY₂

X₂Y₃

99. Covalent compounds are soluble in

Polar solvents

All solvents

Concentrated acids

Non-polar solvents

100. The carbon atoms in calcium carbide are held by

2 sigma bonds

2π and one σ bond

2 covalent, one co-ordinate bond

Ionic bonds

Page 5 of 8

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

5.9 BM

3.0 BM

6.9 BM

4.9 BM

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

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

Electronegativity

Ionization energy

None of these

Electron affinity

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

Chromium

Iron

Copper

Nickel

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

Distorted tetrahedral

Linear

Octahedral

Planar triangle

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

Angular

Trigonal bipyramidal

Pyramidal

Planar

107. 1 erg of energy corresponds to

6.02 x 10²³ J/mol

10¯⁷ J/mol

1 erg/mol

6.02 x 10¹⁶ J/mol

108. Nuclear radiation is emitted by those elements whose

Nuclei are unstable

Molecules are stable

Molecules are unstable

Nuclei are stable

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

SP hybridization

None

Linear geometry

Dipole moment is zero

110. Number of π-bonds in naphthalene is

111. Which of the following molecule has Ā bond

H₂O

O₂

NH₃

C₃H₆

112. Molecular orbitals are filled according to

Hund’s rule

Pauli’s exclusion principle

All these

Aufbau principal

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

Excited state of neon

Ground state of fluorine atom

Excited state of fluorine

Excited state of O¯₂

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

Ni³⁺

Fe²⁺

Cu⁺

Zn⁺

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

Electronegative character of elements

Octet rule

Pauli exclusion principle

Electropositive character of elements

116. Choose the correct statement

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

Each bonding molecular orbital can accommodate only one electron

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

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

9, 4

10, 3

3, 10

4, 9

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

It has high electronegativity

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

It has high heat of dissociation

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

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

CH₃Cl

CCl₄

HCl

H₂O

120. 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?

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

I.P

Ea.

E.A

E.N

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

Water molecules associate through hydrogen bonding

Sulphure has high electronegativity than oxygen

Hydrogen sulphide is a weak acid

Water has higher molecular weight

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

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

SP²

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

None of these

Bonding will not occur

Orbital overlap will not occur

Both A and B are correct

Page 6 of 8

126. The shape of the molecule SF₂Cl₂ is

Tetrahedral

Octahedral

Trigonal bipyramidal

Cubic

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

Low, positive or slightly negative

None of these

High, very negative

Low very negative

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

Pyramidal

Trigonal

Triangular

Tetrahedral

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

Electron

All these

Neutron

Proton

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

131. Shape of CIO₃¯ is

Tetrahedral

Triangular planar

Triangular bipyramidal

Triangular pyramidal

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

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

S¯²

Cl¯

Na⁺

K⁺

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

They are mono atomic gases

They do not react with one another

They have completely filled s and p orbitals

They have high ionization energies

135. Which carbon is more electronegative?

sp²- hybridized carbon

always same irrespective of its hybrid state

sp- hybridized carbon

sp³-hybridized carbon

136. Maximum hydrogen bonds in water are,

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

HBr

H2O

HCI

138. Along a period the atomic radii

Increases

Constant

First decreases then increases

Decreases

139. 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

0.656 nm

656 nm

65.6 nm

6.56 nm

140. In O2 each oxygen atom is hybridized

All

Sp2

Sp3

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

NH₃

BrF₃

H₂O

BF₃

142. The ionization energy

Increase from top to bottom in a group

Does not change in a group

Generally increases from left to right in a period

Does not change in a period

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

2 electrons

4 electrons

6 electrons

1 electron

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

Ionization energy

Electro negativity

None of these

Electron affinity

145. Number of sigma bonds in P₄O₁₀ is

146. Bond order for N2 molecule is

147. An oxygen atom has mass of

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

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

PCl₃

N⁺H₄

Pcl₄

CH₄

149. Pi bonds are produced by overlapping of

Hybrid and un hybrid orbitals

Un-hybrid orbitals

Hybrid orbitals

Atomic orbital and hybrid orbital

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

Page 7 of 8

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

Ionization energy

Electron affinity

Atomic size

Electronegativity

152. Deflection of blue light is lesser than violet because

Blue is absorbed more easily

Blue has more energy

Blue has higher wavelength

Blue is darker colour

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

H₂O

CH₄

NH₃

BH₃

154. 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

16 and 4

12 and 5

16 and 5

12 and 4

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

He⁺

Li⁺

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

XeF₄

BF₃

SiF₄

SF₄

157. Choose the correct statement about 2nd ionization energy

It is equal to the 1st ionization energy

It is always greater than 1st ionization energy

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

It is always less than 1st ionization energy

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

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

Electron affinity

Electronegativity

Ionization potential

Activation energy

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

161. 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?

10.23

10.234017

10.234

10.2340178

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

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

5….0

0….5

1….5

5….1

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

Hexagon

Cube

Prism

Tetrahedron

165. Pick out the molecule which has zero dipole moment

SO₂

H₂O

BCl₃

NH₃

166. Which molecule is polar among the following?

Methanol

Ethane

Carbon tetrachloride

Carbon dioxide

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

Low ionization energy of sodium

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

Sublimation of metallic sodium to give yellow vapour

Photosensitivity of sodium

168. XeF₄ has shape of

Trigonal bipyramidal

Sphere

Square planar

Tetrahedral

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

Decreases

Constant

Increases

Variable trend

170. When potassium metal is exposed to violet light

Ejection of electrons takes place

There is no effect

The absorption of electrons takes place

Ejection of some potassium atoms occurs

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

H₂O

CH₄

CHCl₃

NaCl

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

HBr

H₂O

HCl

173. Which of the following has unchanged valency?

Oxygen

174. 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……

s orbitals

sp³ hybrid orbitals

sp² hybrid orbitals

p orbitals

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

HCN

NH₄Cl

CH₄

H₂O₂

Page 8 of 8

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

Pyramidal

Tetrahedral

Planar triangle

Square planar

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

178. 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 greater than in NO⁺

Bond length is unpredictable

Bond length in NO⁺ is equal to that in NO

179. Electronic configuration of K is

[He]4S¹

[Kr]4S¹

[AR]4S²

[AR]4S¹

180. Anti-bonding MO is formed by

Addition of atomic orbitals

Multiplication of atomic orbitals

None of these

Subtraction of atomic orbitals

181. On sp3 hybridization

One p-orbital is involved

All p-orbitals are involved

Four p-orbitals are involved

One s and 3 p-orbitals are involved

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

3 and 9

2 and 5

3 and 5

3 and 7

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Maan AliLast Updated: April 19, 2025

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