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

10, 3

4, 9

3, 10

9, 4

2. 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?

Van der Waal’s forces

Hydrogen bond formation

Covalent attraction

Dipole interaction

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

Low, positive or slightly negative

Low very negative

None of these

High, very negative

4. Bond angle in water is

120°

107°

109.5°

104.5°

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

Vaporization

Crystallization

Distillation

Colour spectrum

6. Geometry of simple molecule having SP³ hybrid orbital is

Triangular

Tetrahedral

Square planner

Linear

7. Lateral overlapping expected in

Metallic bond

Ā-bonds

Ionic bond

O-bond

8. Choose the correct statement

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

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

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

Each bonding molecular orbital can accommodate only one electron

9. 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 7

3 and 5

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

11. XeF₄ has shape of

Tetrahedral

Sphere

Square planar

Trigonal bipyramidal

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

Nitrogen

Hydrogen

Helium

Oxygen

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

H₂O

NaCl

CH₄

CHCl₃

14. H-bonding is not present in

Hydrogen fluoride

Glycerine

Water

Hydrogen sulphide

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

16. 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

65.6 nm

6.56 nm

656 nm

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

London force

Dispersion force

Chemical bond

Van der Waal’s force

18. Hydrogen chloride molecule contains

Double bond

Electrovalent bond

Co-ordinate bond

Covalent bond

19. Pi bonds are produced by overlapping of

Un-hybrid orbitals

Hybrid orbitals

Hybrid and un hybrid orbitals

Atomic orbital and hybrid orbital

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

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

Fourth Bohr orbit to the first Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

22. Number of π-bonds in naphthalene is

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

Excited state of fluorine

Excited state of neon

Excited state of O¯₂

Ground state of fluorine atom

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

Planar triangle

Octahedral

Distorted tetrahedral

Linear

25. The boiling point of heavy water is

108°C

110°C

101.4°C

99°C

Page 2 of 8

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

Ni³⁺

Cu⁺

Zn⁺

Fe²⁺

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

He⁺

Li⁺

28. A lone pair of electrons in an atom implies

A pair of valence electrons not involved in bonding

A pair of valence electrons

A pair of electrons

A pair of electrons involved in bonding

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

Tetrahedral

Planar triangle

Pyramidal

Square planar

30. The shape of the molecule SF₂Cl₂ is

Octahedral

Tetrahedral

Trigonal bipyramidal

Cubic

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

Five π and nine σ

Nine σ and seven π

Eight σ and eight π

Nine σ and nine π

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

Electropositive character of elements

Electronegative character of elements

Pauli exclusion principle

Octet rule

33. Which of the solid does not contain covalent bond

Diamond

Copper

Graphite

Ice

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

Three unpaired electrons

Stability lower then O₂

Diamagnetic character

Bond order of 2.5

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

1 electron

2 electrons

4 electrons

6 electrons

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

Dipole moment is zero

Linear geometry

SP hybridization

None

37. Unit of dipole moment is

Poise

Pascal

Newton

Debye

38. Energy of an atom in a compound is

Impossible to predict

No change

Lesser than individual

Higher than individual

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

2 n

3 n

Impossible to predict

40. The velocity of photon is

Independent of its wavelength

Depends on its source

Equal to square

Depends on its wavelength

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

42. 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

HCl

43. Which of the following has zero depolemoment?

ClF

CFCl₃

SiF₄

PCl₃

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

H₂O

NH₃

BrF₃

BF₃

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

46. When potassium metal is exposed to violet light

Ejection of some potassium atoms occurs

There is no effect

Ejection of electrons takes place

The absorption of electrons takes place

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

Electron affinity

None of these

Electro negativity

Ionization energy

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

49. Ionic radius in a period from left to right

First increases then decreases

Decreases

Increases

First decreases then increases

50. 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⁺

Page 3 of 8

51. Which carbon is more electronegative?

always same irrespective of its hybrid state

sp³-hybridized carbon

sp²- hybridized carbon

sp- hybridized carbon

52. 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?

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

1 bond pair 3 lone pair

3 lone pair 1 bond pair

2 bond pair 2 lone pair

3 bond pair one lone pair

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

HBr

HCl

55. Bohr’s model atom is contradicted by

Heisenberg’s uncertainty principle

Quarternization of energy of electrons

Quarternization of angular members

Plank’s quantum theory

56. Lewis acids are

Electron deficient

Octet is complete

No such acids exist

Electron rich

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

H – Cl

H – SH

H – OH

H – NH₂

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

6.63 x 10¯³³ m

6.65 x 10¯³⁵ m

6.63 x 10¯³⁵ m

6.63 x 10¯³⁴ m

59. Which one of these is weakest?

Metallic bond

Covalent bond

Ionic bond

Van der Waal’s forces

60. Unit of dipole moment is

Debye

Newton

Poise

Pascal

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

Orbital overlap will not occur

None of these

Bonding will not occur

Both A and B are correct

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

Move with speed as that of light

Charged particles

Can be deflected by magnetic fields

A stream of electrons

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

CH₄

N⁺H₄

PCl₃

Pcl₄

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

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

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

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

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

65. Inter molecular forces in solid hydrogen are

All of these

Van der Waal forces or London dispersion forces

Covalent forces

Hydrogen bonds

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

67. Shape of CIO₃¯ is

Tetrahedral

Triangular pyramidal

Triangular bipyramidal

Triangular planar

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

He⁺

Li⁺

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

70. 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

-2.22

-2.96

-1.11

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

First decreases then increases

First increases then decreases

Decreases

Increases

72. In O2 each oxygen atom is hybridized

Sp3

Sp2

All

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

2, 8

2, 9

2, 6

2, 10

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

75. Geometry of simple molecule having sp3 hybrid orbital is

Triangular

Linear

Square planner

Tetrahedral

Page 4 of 8

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

All these

Electron

Proton

Neutron

77. 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

78. Electronic configuration of K is

[Kr]4S¹

[AR]4S²

[He]4S¹

[AR]4S¹

79. Pick out the molecule which has zero dipole moment

H₂O

NH₃

SO₂

BCl₃

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

Decreases

Increases

Constant

Variable trend

81. Fluorine molecule is formed by

The axial s-p overlap

The axial p-p overlap

The overlap of two sp² hybrid orbitals

The sidewise p-p overlap

82. The structure of ICl₂¯ is

Trigonal

Trigonal bipyramidal

Octahedral

Square planar

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

HCl

H₂O

HBr

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

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

It has high electronegativity

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

It has high heat of dissociation

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

All of above represent same entity

Interaction

Bond

Attractive force

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

N₂

SO₂

He₂

PCl₅

87. Colour of the glow produced 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

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

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

Lone pair – bond pair repulsion only

Bond pair – bond pair repulsion only

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

Lone pair – lone pair repulsion only

89. 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 5

16 and 5

16 and 4

12 and 4

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

91. 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

92. Deflection of blue light is lesser than violet because

Blue is darker colour

Blue is absorbed more easily

Blue has higher wavelength

Blue has more energy

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

Planar

Angular

Trigonal bipyramidal

Pyramidal

94. 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 is unpredictable

Bond length in NO⁺ is equal to that in NO

Bond length in NO⁺ is greater than in NO

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

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

E.A

E.N

I.P

Ea.

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

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

XeF₄

SF₄

BF₃

SiF₄

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

H₂Te

H₂S3

H₂O

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

In, Pt

Ge, Sn

Se, Te

As, Sb

Page 5 of 8

101. Effective magnetic moment of Sc³ ion is

1.73

2.83

5.92

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

103. 1 erg of energy corresponds to

10¯⁷ J/mol

1 erg/mol

6.02 x 10¹⁶ J/mol

6.02 x 10²³ J/mol

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

60°

90°

109°

120°

105. The shape of H₃O⁺ is

Tetrahedral

Angular

Pyramidal

Triangular planar

106. ____________ has their outermost shell complete in atomic form

Coinage metals

Alkali metals

Gun metals

Noble gases

107. 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

108. 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

109. The ionization energy

Does not change in a period

Increase from top to bottom in a group

Generally increases from left to right in a period

Does not change in a group

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

SP²

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

3.0 BM

4.9 BM

5.9 BM

6.9 BM

112. Quantum umber values for 2p orbitals are

n = 1, l = 2

n = 2, l = 0

n = 1, l = 0

n = 2, l = 1

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

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

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

1.7588 x 10²⁰

1.7588 x 10¹¹

9.1095 x 10¯³¹

6.02 x 10²³

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

1/2 x ɜ₀

9 x ɜ₀

6 x ɜ₀

3 x ɜ₀

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

Na and F

C and F

N and F

O and F

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

Two sigma, two pi

One sigma, two pi

Two sigma, one pi

One sigma, one pi

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

2, 1, 0

2, 1, 1

3, 1, 1

3, 2, 1

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

They are also known as cations

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

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

The two atoms start ionization

They energy of atoms increases

The repulsive force dominate the attractive forces

The attractive forces dominate the repulsive forces

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

Equal to 1.7

Greater than 1.7

No specificity exist

Lesser then 1.7

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

HCN

NH₄Cl

CH₄

H₂O₂

123. 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?

10.234017

10.23

10.234

10.2340178

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

Ion-dipole interaction

H-bonding

Dispersion force

Dipole-dipole interaction

125. Along a period the atomic radii

Decreases

Constant

First decreases then increases

Increases

Page 6 of 8

126. Which of the following is not isoelectronic?

Cl¯

Mg²⁺

O²¯

Na⁺

127. Bond order for N2 molecule is

128. Maximum hydrogen bonds in water are,

129. 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 always less than 1st ionization energy

It is equal to the 1st ionization energy

It is always greater than 1st ionization energy

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

0….5

1….5

5….1

5….0

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

Electronegativity

Ionization potential

Electron affinity

Activation energy

132. 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

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

104.5

102

107.5

109.5

134. Number of sigma bonds in P₄O₁₀ is

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

Lesser

Greater

No effect

Remain same

136. The number of significant figures in 0.00200 is

Three

One

Five

Two

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

Both are equal

Cannot be determined

138. Nuclear radiation is emitted by those elements whose

Nuclei are stable

Nuclei are unstable

Molecules are stable

Molecules are unstable

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

Increases

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

Remains constant

Decreases

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……

sp² hybrid orbitals

sp³ hybrid orbitals

s orbitals

p orbitals

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

Electronegativity

Ionization energy

Electron affinity

None of these

142. Which of the following has unchanged valency?

Oxygen

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

None of these

Electron affinity

Electro negativity

Ionization energy

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

CH₃Cl

CCl₄

HCl

H₂O

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

H2O

HBr

HCI

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

Electronegativity

Electron affinity

Ionization energy

Atomic size

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

Trigonal bipyramidal

Octahedral

Square planner

Triangular

148. Molecular orbitals are filled according to

Pauli’s exclusion principle

Hund’s rule

All these

Aufbau principal

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

Tetrahedral

Pyramidal

Triangular

Trigonal

150. Which of these molecules require more bond energy?

Oxygen

Hydrogen

Nitrogen

Page 7 of 8

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

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

-13.6 eV

-54.4 eV

-5.44 eV

Zero

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

154. The carbon atoms in calcium carbide are held by

Ionic bonds

2 covalent, one co-ordinate bond

2 sigma bonds

2π and one σ bond

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

Calcium

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

Prism

Tetrahedron

Hexagon

Cube

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

Larger wavelength

Shorter wavelength

Gamma rays

X-rays not produced

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

MgCl₂

AlCl₃

SiCl₄

NaCl

159. Anti-bonding MO is formed by

Subtraction of atomic orbitals

None of these

Multiplication of atomic orbitals

Addition of atomic orbitals

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

4, 4, 0, ½

4, 1, 0, ½

4, 0, 0, ½

4, 1, 1, ½

161. Which of the following molecule has Ā bond

NH₃

H₂O

C₃H₆

O₂

162. Covalent compounds are soluble in

Non-polar solvents

Polar solvents

All solvents

Concentrated acids

163. On sp3 hybridization

Four p-orbitals are involved

One s and 3 p-orbitals are involved

All p-orbitals are involved

One p-orbital is involved

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

S¯²

K⁺

Cl¯

Na⁺

165. An oxygen atom has mass of

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

166. 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

Photosensitivity of sodium

Sublimation of metallic sodium to give yellow vapour

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

SP²

168. The nature of positive rays depends upon

The nature of electrode

All of these

The nature of discharge tube

The nature of residual gas

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

Fluorides is more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides are more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

170. Molecular orbital picture of N₂ indicates

No unpaired electron

Two unpaired electron

None of these

One unpaired electron

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

Nonpolar covalent bonds only

Hydrogen bonds only

Both polar covalent and hydrogen bonds

Ionic and nonpolar hydrogen bonds

172. Which molecule is polar among the following?

Carbon dioxide

Ethane

Carbon tetrachloride

Methanol

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

NH₃

CH₄

H₂O

BH₃

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

Liquid HCl

Phenol

Water

Liquid NH3

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

Two sigma bonds and one pi-bond

One sigma bond and two pi-bonds

Three sigma bonds

Three pi-bonds

Page 8 of 8

176. Which has the minimum bond angle?

H₂S

CH₄

H₂O

NH₃

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

Copper

Nickel

Chromium

Iron

178. Al become isoelectronic with Ne

By losing two electrons

By gaining two electrons

By gaining three electrons

By losing three electrons

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

180. Which of the following species is paramagnetic?

O²¯

CN¯

CO₂

181. 2nd orbit is away from nucleus for H-atom as compared to first orbit

6-times

2-times

4-times

3-times

182. 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

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Maan AliLast Updated: April 19, 2025

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