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Chemistry Chemical Bonding Online Mcqs Test

Malik TahirLast Updated: October 14, 2025

Important Chemistry Chemical Bonding Question and Answer

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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Chemistry Chemical Bonding Practice Test Online With Explanation

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Page 1 of 8

Chemistry

1. Which one of these is weakest?

Covalent bond

Ionic bond

Metallic bond

Van der Waal’s forces

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

The attractive forces dominate the repulsive forces

They energy of atoms increases

The two atoms start ionization

The repulsive force dominate the attractive forces

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

Octet rule

Electropositive character of elements

Electronegative character of elements

Pauli exclusion principle

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

Electronegativity

Atomic size

Electron affinity

Ionization energy

5. The boiling point of heavy water is

108°C

99°C

101.4°C

110°C

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

Trigonal

Pyramidal

Tetrahedral

Triangular

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

SF₄

XeF₄

SiF₄

BF₃

8. Choose the correct statement

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

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

9. Which of the following molecule has Ā bond

C₃H₆

O₂

NH₃

H₂O

10. Number of π-bonds in naphthalene is

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

12. Along a period the atomic radii

First decreases then increases

Decreases

Constant

Increases

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

3, 10

4, 9

10, 3

9, 4

14. Covalent compounds are soluble in

Polar solvents

Concentrated acids

Non-polar solvents

All solvents

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

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

BrF₃

H₂O

NH₃

BF₃

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

High, very negative

None of these

Low, positive or slightly negative

Low very negative

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

Constant

Decreases

Variable trend

Increases

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

Impossible to predict

2 n

3 n

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

2, 10

2, 8

2, 9

2, 6

21. Molecular orbital picture of N₂ indicates

None of these

No unpaired electron

Two unpaired electron

One unpaired electron

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

Li⁺

He⁺

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

SP²

24. Lateral overlapping expected in

Ā-bonds

Ionic bond

Metallic bond

O-bond

25. 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

Page 2 of 8

26. Number of sigma bonds in P₄O₁₀ is

27. 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

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

Stability lower then O₂

Diamagnetic character

Three unpaired electrons

Bond order of 2.5

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

Ground state of fluorine atom

Excited state of neon

Excited state of fluorine

Excited state of O¯₂

30. Bond order for N2 molecule is

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

Electron affinity

Activation energy

Ionization potential

Electronegativity

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

33. Lewis acids are

Electron rich

No such acids exist

Octet is complete

Electron deficient

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

He⁺

Li⁺

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

36. Electronic configuration of K is

[AR]4S²

[AR]4S¹

[Kr]4S¹

[He]4S¹

37. Unit of dipole moment is

Newton

Poise

Debye

Pascal

38. An oxygen atom has mass of

5.316 x 10¯²³ g

2.657 x 10¯²³ g

5.316 x 10¯²³ g

16g

39. The nature of positive rays depends upon

The nature of electrode

The nature of discharge tube

All of these

The nature of residual gas

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

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

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

They are also known as cations

They are formed when electros are formed from atoms

They are smaller than the atoms from which they were formed

They are larger than the atoms from which they were formed

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

H₂O₂

HCN

NH₄Cl

CH₄

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

Oxygen

Nitrogen

Hydrogen

Helium

45. Energy of an atom in a compound is

Impossible to predict

Lesser than individual

No change

Higher than individual

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

Octahedral

Planar triangle

Distorted tetrahedral

Linear

47. 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

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

X – radiation, visible, infrared, microwave

Radio, visible, infrared, ultraviolet

Visible, ultraviolet, infrared, gamma rays

Microwave, infrared, visible, ultraviolet

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

SP²

50. 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

3 x ɜ₀

6 x ɜ₀

Page 3 of 8

51. XeF₄ has shape of

Sphere

Tetrahedral

Square planar

Trigonal bipyramidal

52. In O2 each oxygen atom is hybridized

Sp2

Sp3

All

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

None of these

Both A and B are correct

Orbital overlap will not occur

Bonding will not occur

54. 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

55. Molecular orbitals are filled according to

Aufbau principal

All these

Hund’s rule

Pauli’s exclusion principle

56. Hydrogen chloride molecule contains

Electrovalent bond

Covalent bond

Co-ordinate bond

Double bond

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

A stream of electrons

Move with speed as that of light

Can be deflected by magnetic fields

Charged particles

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

Distillation

Crystallization

Vaporization

Colour spectrum

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

Water

Phenol

Liquid HCl

Liquid NH3

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

61. 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

3 lone pair 1 bond pair

1 bond pair 3 lone pair

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

63. Geometry of simple molecule having SP³ hybrid orbital is

Triangular

Tetrahedral

Linear

Square planner

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

PCl₃

N⁺H₄

Pcl₄

CH₄

65. 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

107.5

102

109.5

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

One sigma, two pi

Two sigma, two pi

One sigma, one pi

Two sigma, one pi

67. 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?

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

90°

109°

120°

60°

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

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

Dispersion force

H-bonding

Ion-dipole interaction

Dipole-dipole interaction

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

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

Neutron

Electron

Proton

All these

73. 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

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

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

74. 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⁺

Cu²⁺

Ni²⁺

75. 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

Page 4 of 8

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

Dipole moment is zero

Linear geometry

None

SP hybridization

77. The ionization energy

Does not change in a period

Generally increases from left to right in a period

Increase from top to bottom in a group

Does not change in a group

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

Gamma rays

X-rays not produced

Larger wavelength

Shorter wavelength

79. The number of significant figures in 0.00200 is

One

Three

Two

Five

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

Na⁺

K⁺

Cl¯

S¯²

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

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

Both are equal

Cannot be determined

83. 2nd orbit is away from nucleus for H-atom as compared to first orbit

4-times

2-times

3-times

6-times

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

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

Sixth Bohr orbit to the third Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

86. ____________ has their outermost shell complete in atomic form

Coinage metals

Gun metals

Alkali metals

Noble gases

87. The shape of the molecule SF₂Cl₂ is

Octahedral

Trigonal bipyramidal

Tetrahedral

Cubic

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

Three pi-bonds

Two sigma bonds and one pi-bond

Three sigma bonds

One sigma bond and two pi-bonds

89. On sp3 hybridization

One p-orbital is involved

Four p-orbitals are involved

All p-orbitals are involved

One s and 3 p-orbitals are involved

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

They have completely filled s and p orbitals

They are mono atomic gases

They do not react with one another

They have high ionization energies

91. The structure of ICl₂¯ is

Square planar

Trigonal

Octahedral

Trigonal bipyramidal

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

4 electrons

2 electrons

6 electrons

1 electron

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

NaCl

MgCl₂

AlCl₃

SiCl₄

94. Choose the correct statement about 2nd ionization energy

It is equal to the 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

It is always greater than 1st ionization energy

95. The carbon atoms in calcium carbide are held by

2π and one σ bond

Ionic bonds

2 sigma bonds

2 covalent, one co-ordinate bond

96. 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

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

Ionization energy

Electron affinity

None of these

Electro negativity

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

Dispersion force

Van der Waal’s force

London force

Chemical bond

99. Which has the minimum bond angle?

NH₃

H₂O

CH₄

H₂S

100. 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

Page 5 of 8

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

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

-13.6 eV

Zero

-54.4 eV

-5.44 eV

103. The velocity of photon is

Depends on its wavelength

Independent of its wavelength

Equal to square

Depends on its source

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

Se, Te

As, Sb

In, Pt

Ge, Sn

105. 1 erg of energy corresponds to

10¯⁷ J/mol

6.02 x 10¹⁶ J/mol

6.02 x 10²³ J/mol

1 erg/mol

106. The shape of H₃O⁺ is

Tetrahedral

Pyramidal

Triangular planar

Angular

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

O and F

N and F

C and F

Na and F

108. Which of the solid does not contain covalent bond

Copper

Graphite

Diamond

Ice

109. When potassium metal is exposed to violet light

The absorption of electrons takes place

There is no effect

Ejection of some potassium atoms occurs

Ejection of electrons takes place

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

PCl₅

He₂

N₂

SO₂

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

H₂O

H₂Te

H₂S3

H₂O

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

Pyramidal

Planar triangle

Tetrahedral

Square planar

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

No specificity exist

Lesser then 1.7

Equal to 1.7

Greater than 1.7

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

Copper

Nickel

Chromium

Iron

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. Which of the following has unchanged valency?

Oxygen

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

5….1

1….5

0….5

5….0

118. A lone pair of electrons in an atom implies

A pair of electrons involved in bonding

A pair of valence electrons

A pair of valence electrons not involved in bonding

A pair of electrons

119. Which of the following has zero depolemoment?

ClF

CFCl₃

PCl₃

SiF₄

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

H₂O

NH₃

CH₄

BH₃

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

None of these

Electronegativity

Electron affinity

Ionization energy

122. Which of these molecules require more bond energy?

Oxygen

Nitrogen

Hydrogen

123. 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 not be a possibility of chemical reaction

There may be a possibility of a chemical reaction

124. Effective magnetic moment of Sc³ ion is

5.92

1.73

2.83

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

9.1095 x 10¯³¹

1.7588 x 10²⁰

6.02 x 10²³

1.7588 x 10¹¹

Page 6 of 8

126. 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

127. 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

Sublimation of metallic sodium to give yellow vapour

Photosensitivity of sodium

128. Deflection of blue light is lesser than violet because

Blue has more energy

Blue is darker colour

Blue is absorbed more easily

Blue has higher wavelength

129. Quantum umber values for 2p orbitals are

n = 2, l = 0

n = 2, l = 1

n = 1, l = 2

n = 1, l = 0

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

XY₂

X₂Y

X₂Y₃

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

HCl

HBr

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

Remains constant

Increases

Decreases

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

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

Zn⁺

Fe²⁺

Ni³⁺

Cu⁺

134. Pi bonds are produced by overlapping of

Atomic orbital and hybrid orbital

Un-hybrid orbitals

Hybrid orbitals

Hybrid and un hybrid orbitals

135. Which carbon is more electronegative?

sp²- hybridized carbon

sp³-hybridized carbon

sp- hybridized carbon

always same irrespective of its hybrid state

136. 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

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

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

138. Inter molecular forces in solid hydrogen are

Hydrogen bonds

Covalent forces

All of these

Van der Waal forces or London dispersion forces

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

Lone pair – lone pair repulsion only

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

Lone pair – bond pair repulsion only

Bond pair – bond pair repulsion only

140. Ionic radius in a period from left to right

Increases

Decreases

First decreases then increases

First increases then decreases

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

First decreases then increases

Decreases

First increases then decreases

Increases

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

CHCl₃

CH₄

NaCl

H₂O

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

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

Triangular

Trigonal bipyramidal

Octahedral

Square planner

145. Bond angle in water is

109.5°

107°

120°

104.5°

146. Anti-bonding MO is formed by

Subtraction of atomic orbitals

Multiplication of atomic orbitals

Addition of atomic orbitals

None of these

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

H₂O

HCl

HBr

148. 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

-2.96

-1.48

149. Al become isoelectronic with Ne

By losing three electrons

By losing two electrons

By gaining three electrons

By gaining two electrons

150. Bohr’s model atom is contradicted by

Plank’s quantum theory

Heisenberg’s uncertainty principle

Quarternization of energy of electrons

Quarternization of angular members

Page 7 of 8

151. Colour of the glow produced 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

Depends on the pressure in the discharge tube

152. 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

153. Nuclear radiation is emitted by those elements whose

Molecules are unstable

Molecules are stable

Nuclei are unstable

Nuclei are stable

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

H – OH

H – Cl

H – NH₂

H – SH

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

Hydrogen sulphide is a weak acid

Sulphure has high electronegativity than oxygen

Water molecules associate through hydrogen bonding

Water has higher molecular weight

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

Cube

Hexagon

Prism

Tetrahedron

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

Bond

Interaction

Attractive force

All of above represent same entity

158. H-bonding is not present in

Hydrogen fluoride

Water

Glycerine

Hydrogen sulphide

159. Unit of dipole moment is

Poise

Debye

Newton

Pascal

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

4, 4, 0, ½

4, 0, 0, ½

4, 1, 1, ½

4, 1, 0, ½

161. 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

Covalent attraction

Dipole interaction

Hydrogen bond formation

162. Shape of CIO₃¯ is

Tetrahedral

Triangular pyramidal

Triangular bipyramidal

Triangular planar

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

Lesser

Greater

Remain same

No effect

164. 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

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

Boron trifluoride is pyramidal in shape while NH₃ is planar

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides is more electronegative

Fluorides are more electronegative

166. 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

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

168. Which of the following species is paramagnetic?

CN¯

O²¯

CO₂

169. Which of the following is not isoelectronic?

O²¯

Cl¯

Na⁺

Mg²⁺

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

Hydrogen bonds only

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

Both polar covalent and hydrogen bonds

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

HCI

HBr

H2O

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

5.9 BM

3.0 BM

4.9 BM

6.9 BM

173. Which molecule is polar among the following?

Ethane

Carbon tetrachloride

Carbon dioxide

Methanol

174. Geometry of simple molecule having sp3 hybrid orbital is

Square planner

Linear

Tetrahedral

Triangular

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

Planar

Angular

Trigonal bipyramidal

Pyramidal

Page 8 of 8

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

H₂O

HCl

CCl₄

CH₃Cl

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

I.P

E.A

Ea.

E.N

178. Pick out the molecule which has zero dipole moment

NH₃

BCl₃

SO₂

H₂O

179. Maximum hydrogen bonds in water are,

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

Calcium

181. 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

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

Eight σ and eight π

Nine σ and nine π

Nine σ and seven π

Five π and nine σ

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Malik TahirLast Updated: October 14, 2025

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