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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. Inter molecular forces in solid hydrogen are

Covalent forces

Hydrogen bonds

All of these

Van der Waal forces or London dispersion forces

2. Al become isoelectronic with Ne

By gaining three electrons

By gaining two electrons

By losing two electrons

By losing three electrons

3. 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

Both A and B are correct

None of these

Bonding will not occur

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

Variable trend

Decreases

Constant

Increases

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

HCl

H₂O

HBr

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

H₂O

NaCl

CH₄

CHCl₃

7. 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

8. Ionic radius in a period from left to right

First increases then decreases

First decreases then increases

Increases

Decreases

9. H-bonding is not present in

Hydrogen fluoride

Glycerine

Hydrogen sulphide

Water

10. 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 only

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

11. Which molecule is polar among the following?

Ethane

Carbon tetrachloride

Carbon dioxide

Methanol

12. Geometry of simple molecule having sp3 hybrid orbital is

Square planner

Linear

Tetrahedral

Triangular

13. The nature of positive rays depends upon

All of these

The nature of residual gas

The nature of discharge tube

The nature of electrode

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

Hydrogen

Helium

Oxygen

Nitrogen

15. Which of the following is not isoelectronic?

Mg²⁺

Na⁺

Cl¯

O²¯

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

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

They have completely filled s and p orbitals

They have high ionization energies

They do not react with one another

They are mono atomic gases

18. Pick out the molecule which has zero dipole moment

SO₂

BCl₃

H₂O

NH₃

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

Neutron

All these

Electron

Proton

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

All of above represent same entity

Bond

Attractive force

Interaction

21. Covalent compounds are soluble in

Non-polar solvents

Concentrated acids

All solvents

Polar solvents

22. Along a period the atomic radii

Constant

Decreases

Increases

First decreases then increases

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

Charged particles

A stream of electrons

Move with speed as that of light

Can be deflected by magnetic fields

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

SP²

25. 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 4

12 and 4

16 and 5

Page 2 of 8

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

High, very negative

Low, positive or slightly negative

None of these

Low very negative

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

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

Excited state of O¯₂

Ground state of fluorine atom

Excited state of neon

Excited state of fluorine

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

4, 9

10, 3

9, 4

3, 10

30. 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

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

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

Cannot be determined

Both are equal

33. ____________ has their outermost shell complete in atomic form

Coinage metals

Noble gases

Alkali metals

Gun metals

34. Effective magnetic moment of Sc³ ion is

1.73

5.92

2.83

35. XeF₄ has shape of

Square planar

Sphere

Tetrahedral

Trigonal bipyramidal

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

Cu⁺

Ni²⁺

Cu²⁺

37. Bond order for N2 molecule is

38. Shape of CIO₃¯ is

Triangular bipyramidal

Triangular planar

Triangular pyramidal

Tetrahedral

39. Which of the following molecule has Ā bond

C₃H₆

O₂

H₂O

NH₃

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

Remains constant

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

Decreases

Increases

41. Pi bonds are produced by overlapping of

Hybrid orbitals

Un-hybrid orbitals

Hybrid and un hybrid orbitals

Atomic orbital and hybrid orbital

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

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

SiCl₄

AlCl₃

MgCl₂

NaCl

44. An oxygen atom has mass of

5.316 x 10¯²³ g

2.657 x 10¯²³ g

16g

45. 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 greater than 1st ionization energy

It is always less than 1st ionization energy

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

First increases then decreases

First decreases then increases

Increases

Decreases

47. Lewis acids are

Electron rich

No such acids exist

Octet is complete

Electron deficient

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

One sigma, two pi

Two sigma, one pi

Two sigma, two pi

One sigma, one pi

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

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

Stability lower then O₂

Three unpaired electrons

Bond order of 2.5

Diamagnetic character

Page 3 of 8

51. Bond angle in water is

120°

104.5°

109.5°

107°

52. The shape of H₃O⁺ is

Angular

Triangular planar

Pyramidal

Tetrahedral

53. 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

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

4.9 BM

5.9 BM

6.9 BM

3.0 BM

55. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 1, l = 0

n = 1, l = 2

n = 2, l = 0

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

BrF₃

H₂O

NH₃

BF₃

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

Electron affinity

Electronegativity

Activation energy

Ionization potential

58. Molecular orbital picture of N₂ indicates

One unpaired electron

None of these

No unpaired electron

Two unpaired electron

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

Ionization energy

Electro negativity

None of these

Electron affinity

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

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

Dispersion force

H-bonding

Dipole-dipole interaction

Ion-dipole interaction

62. 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

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

Microwave, infrared, visible, ultraviolet

Radio, visible, infrared, ultraviolet

X – radiation, visible, infrared, microwave

Visible, ultraviolet, infrared, gamma rays

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

65. The carbon atoms in calcium carbide are held by

2π and one σ bond

2 covalent, one co-ordinate bond

Ionic bonds

2 sigma bonds

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

102

104.5

107.5

109.5

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

68. Number of π-bonds in naphthalene is

69. 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

10.2340178

10.234

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

Calcium

71. 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

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

1 electron

2 electrons

6 electrons

4 electrons

73. Molecular orbitals are filled according to

Hund’s rule

All these

Pauli’s exclusion principle

Aufbau principal

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

Three pi-bonds

Three sigma bonds

Two sigma bonds and one pi-bond

One sigma bond and two pi-bonds

75. Electronic configuration of K is

[Kr]4S¹

[He]4S¹

[AR]4S²

[AR]4S¹

Page 4 of 8

76. Fluorine molecule is formed by

The axial s-p overlap

The overlap of two sp² hybrid orbitals

The sidewise p-p overlap

The axial p-p overlap

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

SP²

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

HBr

HCl

79. Number of sigma bonds in P₄O₁₀ is

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

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

CH₄

HCN

NH₄Cl

H₂O₂

82. Which of the solid does not contain covalent bond

Ice

Graphite

Copper

Diamond

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

Li⁺

He⁺

84. Maximum hydrogen bonds in water are,

85. Lateral overlapping expected in

Metallic bond

O-bond

Ā-bonds

Ionic bond

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

As, Sb

Ge, Sn

Se, Te

In, Pt

87. Which of the following has zero depolemoment?

PCl₃

CFCl₃

ClF

SiF₄

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

109°

120°

60°

90°

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

Copper

Chromium

Iron

Nickel

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

Zero

-5.44 eV

-13.6 eV

-54.4 eV

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

They are formed when electros are formed from atoms

They are also known as cations

They are larger than the atoms from which they were formed

They are smaller than the atoms from which they were formed

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

Both polar covalent and hydrogen bonds

Hydrogen bonds only

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

93. 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

3 bond pair one lone pair

2 bond pair 2 lone pair

94. Anti-bonding MO is formed by

None of these

Multiplication of atomic orbitals

Addition of atomic orbitals

Subtraction of atomic orbitals

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

They energy of atoms increases

The attractive forces dominate the repulsive forces

The repulsive force dominate the attractive forces

The two atoms start ionization

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

Water has higher molecular weight

Hydrogen sulphide is a weak acid

Water molecules associate through hydrogen bonding

Sulphure has high electronegativity than oxygen

97. In O2 each oxygen atom is hybridized

Sp3

All

Sp2

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

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 heat of dissociation

It has high electronegativity

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

Pauli exclusion principle

Electropositive character of elements

Electronegative character of elements

Octet rule

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

Electronegativity

Electron affinity

Ionization energy

Atomic size

Page 5 of 8

101. 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

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

Nine σ and nine π

Nine σ and seven π

Five π and nine σ

Eight σ and eight π

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

Liquid NH3

Phenol

Liquid HCl

Water

104. The boiling point of heavy water is

99°C

110°C

108°C

101.4°C

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

H – OH

H – Cl

H – SH

H – NH₂

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

Trigonal

Triangular

Pyramidal

Tetrahedral

107. Unit of dipole moment is

Debye

Poise

Pascal

Newton

108. Energy of an atom in a compound is

Lesser than individual

Higher than individual

Impossible to predict

No change

109. Hydrogen chloride molecule contains

Double bond

Co-ordinate bond

Covalent bond

Electrovalent bond

110. Geometry of simple molecule having SP³ hybrid orbital is

Triangular

Linear

Tetrahedral

Square planner

111. 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

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

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

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

112. Bohr’s model atom is contradicted by

Quarternization of energy of electrons

Plank’s quantum theory

Quarternization of angular members

Heisenberg’s uncertainty principle

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

H₂O

H₂Te

H₂S3

H₂O

114. 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

Boron trifluoride is pyramidal in shape while NH₃ is planar

Fluorides are more electronegative

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

None of these

Electron affinity

Electro negativity

Ionization energy

116. 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

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

None of these

Electronegativity

Ionization energy

Electron affinity

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

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

Gamma rays

X-rays not produced

Larger wavelength

Shorter wavelength

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

6.63 x 10¯³⁵ m

6.63 x 10¯³³ m

6.65 x 10¯³⁵ m

6.63 x 10¯³⁴ m

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

Lesser

Greater

No effect

Remain same

122. Which has the minimum bond angle?

H₂S

H₂O

NH₃

CH₄

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

Zn⁺

Ni³⁺

Fe²⁺

Cu⁺

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

125. Unit of dipole moment is

Poise

Newton

Pascal

Debye

Page 6 of 8

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

N⁺H₄

CH₄

Pcl₄

PCl₃

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

3 x ɜ₀

6 x ɜ₀

9 x ɜ₀

1/2 x ɜ₀

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

H2O

HBr

HCI

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

Trigonal bipyramidal

Square planner

Triangular

Octahedral

130. Which of the following species is paramagnetic?

CN¯

O²¯

CO₂

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

Dispersion force

London force

Van der Waal’s force

Chemical bond

132. 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?

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

3 and 5

2 and 5

3 and 9

3 and 7

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

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

Li⁺

He⁺

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

Square planar

Planar triangle

Tetrahedral

Pyramidal

137. Which of these molecules require more bond energy?

Hydrogen

Oxygen

Nitrogen

138. Which of the following has unchanged valency?

Oxygen

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

Octahedral

Planar triangle

Distorted tetrahedral

Linear

140. Which carbon is more electronegative?

always same irrespective of its hybrid state

sp- hybridized carbon

sp³-hybridized carbon

sp²- hybridized carbon

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

Fifth Bohr orbit to the second Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

142. The velocity of photon is

Independent of its wavelength

Equal to square

Depends on its source

Depends on its wavelength

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

Cube

Hexagon

Prism

Tetrahedron

144. The ionization energy

Does not change in a period

Increase from top to bottom in a group

Does not change in a group

Generally increases from left to right in a period

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

CH₄

H₂O

NH₃

BH₃

146. 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

147. The structure of ICl₂¯ is

Octahedral

Square planar

Trigonal bipyramidal

Trigonal

148. 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

149. 2nd orbit is away from nucleus for H-atom as compared to first orbit

3-times

2-times

6-times

4-times

150. Nuclear radiation is emitted by those elements whose

Molecules are stable

Nuclei are unstable

Molecules are unstable

Nuclei are stable

Page 7 of 8

151. The shape of the molecule SF₂Cl₂ is

Cubic

Trigonal bipyramidal

Tetrahedral

Octahedral

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

Angular

Pyramidal

Trigonal bipyramidal

Planar

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

S¯²

Na⁺

Cl¯

K⁺

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

1.7588 x 10²⁰

6.02 x 10²³

9.1095 x 10¯³¹

1.7588 x 10¹¹

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

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

3, 1, 1

2, 1, 0

2, 1, 1

3, 2, 1

157. 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

Dipole interaction

Covalent attraction

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

H₂O

CCl₄

HCl

CH₃Cl

159. 1 erg of energy corresponds to

6.02 x 10¹⁶ J/mol

1 erg/mol

6.02 x 10²³ J/mol

10¯⁷ J/mol

160. 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?

-2.96

-2.22

-1.11

-1.48

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

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

PCl₅

SO₂

He₂

N₂

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

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

Photosensitivity of sodium

Sublimation of metallic sodium to give yellow vapour

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

Low ionization energy of sodium

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

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

SF₄

SiF₄

XeF₄

BF₃

167. Which one of these is weakest?

Van der Waal’s forces

Metallic bond

Ionic bond

Covalent bond

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

Ea.

E.N

E.A

I.P

169. On sp3 hybridization

One s and 3 p-orbitals are involved

All p-orbitals are involved

One p-orbital is involved

Four p-orbitals are involved

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

Greater than 1.7

No specificity exist

Lesser then 1.7

Equal to 1.7

171. 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

172. When potassium metal is exposed to violet light

Ejection of electrons takes place

Ejection of some potassium atoms occurs

There is no effect

The absorption of electrons takes place

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

1….5

0….5

5….0

5….1

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

Crystallization

Distillation

Colour spectrum

Vaporization

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

4, 1, 1, ½

4, 0, 0, ½

4, 4, 0, ½

4, 1, 0, ½

Page 8 of 8

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

Water should be preferred over lemon Juice for drinking

There may be a possibility of a chemical reaction

Lemon juice is dangerous for health

There may not be a possibility of chemical reaction

177. The number of significant figures in 0.00200 is

One

Three

Five

Two

178. 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

656 nm

0.656 nm

65.6 nm

6.56 nm

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

3 n

Impossible to predict

2 n

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

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

Dipole moment is zero

None

Linear geometry

SP hybridization

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

2, 10

2, 8

2, 9

2, 6

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Maan AliLast Updated: April 19, 2025

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