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Chemistry Chemical Bonding Online Mcqs Test

Malik TahirLast Updated: October 14, 2025

Start your preparation for Chemistry Chemical Bonding Online Mcqs Test. This online test contains important MCQs from past papers. Attempting this test will help you prepare for Annual Exams and Entry Tests. Read the questions carefully and select the correct option below to see your result.

Important Chemistry Chemical Bonding Question and Answer

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
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Page 1 of 8

Chemistry

1. Shape of CIO₃¯ is

Tetrahedral

Triangular pyramidal

Triangular planar

Triangular bipyramidal

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

Fluorides is more electronegative

Fluorides are more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Boron trifluoride is pyramidal in shape while NH₃ is planar

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

X₂Y₃

XY₂

X₂Y

4. Geometry of simple molecule having sp3 hybrid orbital is

Triangular

Square planner

Tetrahedral

Linear

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

He⁺

Li⁺

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

Linear

Planar triangle

Octahedral

Distorted tetrahedral

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

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

109°

60°

120°

90°

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

9.1095 x 10¯³¹

6.02 x 10²³

1.7588 x 10¹¹

1.7588 x 10²⁰

10. Which of the solid does not contain covalent bond

Ice

Copper

Graphite

Diamond

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

5….0

5….1

0….5

1….5

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

Helium

Hydrogen

Oxygen

Nitrogen

13. 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

14. In O2 each oxygen atom is hybridized

All

Sp2

Sp3

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

10, 3

3, 10

9, 4

4, 9

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

H₂O

H₂Te

H₂O

H₂S3

17. 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?

18. 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

6.56 nm

0.656 nm

65.6 nm

656 nm

19. The number of significant figures in 0.00200 is

One

Five

Two

Three

20. Bond angle in water is

107°

120°

104.5°

109.5°

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

Na and F

O and F

C and F

N and F

22. The shape of H₃O⁺ is

Pyramidal

Angular

Tetrahedral

Triangular planar

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

HCl

CCl₄

CH₃Cl

H₂O

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

Both are equal

Cannot be determined

25. Which molecule is polar among the following?

Methanol

Carbon dioxide

Carbon tetrachloride

Ethane

Page 2 of 8

26. The carbon atoms in calcium carbide are held by

2 covalent, one co-ordinate bond

Ionic bonds

2π and one σ bond

2 sigma bonds

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

H₂O₂

CH₄

NH₄Cl

HCN

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

Excited state of O¯₂

Excited state of fluorine

Ground state of fluorine atom

Excited state of neon

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

HCl

HBr

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

Sulphure has high electronegativity than oxygen

Hydrogen sulphide is a weak acid

Water molecules associate through hydrogen bonding

Water has higher molecular weight

31. Which of the following has unchanged valency?

Oxygen

32. Choose the correct statement about 2nd ionization energy

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

It is equal to the 1st ionization energy

It is always less than 1st ionization energy

It is always greater than 1st ionization energy

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

PCl₅

SO₂

He₂

N₂

34. Unit of dipole moment is

Debye

Poise

Pascal

Newton

35. 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……

sp³ hybrid orbitals

s orbitals

sp² hybrid orbitals

p orbitals

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

NaCl

SiCl₄

AlCl₃

MgCl₂

37. The structure of ICl₂¯ is

Octahedral

Trigonal bipyramidal

Square planar

Trigonal

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

Pauli exclusion principle

Electropositive character of elements

Octet rule

Electronegative character of elements

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

Li⁺

He⁺

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

No effect

Greater

Lesser

Remain same

41. Which carbon is more electronegative?

always same irrespective of its hybrid state

sp³-hybridized carbon

sp- hybridized carbon

sp²- hybridized carbon

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

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

One sigma bond and two pi-bonds

Two sigma bonds and one pi-bond

Three pi-bonds

Three sigma bonds

44. 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 5

12 and 5

16 and 4

12 and 4

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

Hexagon

Prism

Cube

Tetrahedron

46. Number of sigma bonds in P₄O₁₀ is

47. On sp3 hybridization

Four p-orbitals are involved

One p-orbital is involved

One s and 3 p-orbitals are involved

All p-orbitals are involved

48. The velocity of photon is

Equal to square

Depends on its wavelength

Depends on its source

Independent of its wavelength

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

A stream of electrons

Can be deflected by magnetic fields

Charged particles

Move with speed as that of light

50. Which of the following species is paramagnetic?

O²¯

CO₂

CN¯

Page 3 of 8

51. Which has the minimum bond angle?

H₂O

NH₃

CH₄

H₂S

52. Which of the following has zero depolemoment?

SiF₄

ClF

PCl₃

CFCl₃

53. Inter molecular forces in solid hydrogen are

Van der Waal forces or London dispersion forces

Covalent forces

Hydrogen bonds

All of these

54. Which of these molecules require more bond energy?

Nitrogen

Oxygen

Hydrogen

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

Ionization energy

Electro negativity

Electron affinity

None of these

56. Effective magnetic moment of Sc³ ion is

5.92

2.83

1.73

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

2 electrons

1 electron

6 electrons

4 electrons

58. H-bonding is not present in

Glycerine

Hydrogen sulphide

Hydrogen fluoride

Water

59. Which of the following molecule has Ā bond

NH₃

H₂O

O₂

C₃H₆

60. 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

61. Maximum hydrogen bonds in water are,

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

-13.6 eV

-5.44 eV

Zero

-54.4 eV

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

3 lone pair 1 bond pair

3 bond pair one lone pair

2 bond pair 2 lone pair

1 bond pair 3 lone pair

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

65. 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

66. Molecular orbital picture of N₂ indicates

Two unpaired electron

None of these

One unpaired electron

No unpaired electron

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

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

SP²

69. 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

It has high heat of dissociation

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

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?

-1.11

-1.48

-2.96

-2.22

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

As, Sb

Se, Te

Ge, Sn

In, Pt

72. Pick out the molecule which has zero dipole moment

SO₂

BCl₃

H₂O

NH₃

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

HCI

H2O

HBr

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

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

Page 4 of 8

76. Hydrogen chloride molecule contains

Co-ordinate bond

Electrovalent bond

Covalent bond

Double bond

77. Deflection of blue light is lesser than violet because

Blue is absorbed more easily

Blue is darker colour

Blue has higher wavelength

Blue has more energy

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

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

Nine σ and seven π

Five π and nine σ

Nine σ and nine π

Eight σ and eight π

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

No specificity exist

Greater than 1.7

Equal to 1.7

Lesser then 1.7

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

Calcium

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

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

Microwave, infrared, visible, ultraviolet

Visible, ultraviolet, infrared, gamma rays

Radio, visible, infrared, ultraviolet

X – radiation, visible, infrared, microwave

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

Triangular

Pyramidal

Tetrahedral

Trigonal

85. 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 is unpredictable

Bond length in NO⁺ is equal to that in NO

Bond length in NO⁺ is greater than in NO

Bond length in NO is greater than in NO⁺

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

87. The boiling point of heavy water is

99°C

110°C

101.4°C

108°C

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

4, 1, 1, ½

4, 4, 0, ½

4, 1, 0, ½

4, 0, 0, ½

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

Liquid HCl

Liquid NH3

Water

Phenol

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

High, very negative

None of these

Low very negative

Low, positive or slightly negative

91. Ionic radius in a period from left to right

First decreases then increases

Increases

Decreases

First increases then decreases

92. Lewis acids are

Octet is complete

Electron deficient

No such acids exist

Electron rich

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

They are smaller than the atoms from which they were formed

They are formed when electros are formed from atoms

They are larger than the atoms from which they were formed

They are also known as cations

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

2 and 5

3 and 9

3 and 5

3 and 7

95. Pi bonds are produced by overlapping of

Atomic orbital and hybrid orbital

Hybrid and un hybrid orbitals

Hybrid orbitals

Un-hybrid orbitals

96. Colour of the glow produced in the discharge tube

Depends on 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

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

Triangular

Trigonal bipyramidal

Octahedral

Square planner

98. Energy of an atom in a compound is

Higher than individual

Impossible to predict

Lesser than individual

No change

99. Molecular orbitals are filled according to

Pauli’s exclusion principle

All these

Aufbau principal

Hund’s rule

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

Dispersion force

H-bonding

Ion-dipole interaction

Dipole-dipole interaction

Page 5 of 8

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

3.0 BM

4.9 BM

6.9 BM

5.9 BM

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

Variable trend

Increases

Constant

Decreases

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

They do not react with one another

They are mono atomic gases

They have high ionization energies

They have completely filled s and p orbitals

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

Bond

Attractive force

Interaction

All of above represent same entity

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

Fe²⁺

Ni³⁺

Cu⁺

Zn⁺

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

Increases

Decreases

First increases then decreases

First decreases then increases

107. A lone pair of electrons in an atom implies

A pair of electrons involved in bonding

A pair of valence electrons not involved in bonding

A pair of electrons

A pair of valence electrons

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

Ionization potential

Electronegativity

Electron affinity

Activation energy

109. Lateral overlapping expected in

Ionic bond

O-bond

Ā-bonds

Metallic bond

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

Pcl₄

PCl₃

N⁺H₄

CH₄

111. 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⁺

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

H – Cl

H – NH₂

H – OH

H – SH

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

None of these

Ionization energy

Electron affinity

Electronegativity

114. Electronic configuration of K is

[He]4S¹

[AR]4S²

[AR]4S¹

[Kr]4S¹

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

Na⁺

Cl¯

K⁺

S¯²

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

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

All these

Proton

Neutron

Electron

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

Hydrogen bond formation

Covalent attraction

Van der Waal’s forces

Dipole interaction

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

Nickel

Copper

Iron

Chromium

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

SP²

121. Anti-bonding MO is formed by

Subtraction of atomic orbitals

None of these

Addition of atomic orbitals

Multiplication of atomic orbitals

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

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

They energy of atoms increases

The attractive forces dominate the repulsive forces

The two atoms start ionization

The repulsive force dominate the attractive forces

124. 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

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

E.A

Ea.

I.P

E.N

Page 6 of 8

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

2, 10

2, 6

2, 9

2, 8

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

128. Unit of dipole moment is

Debye

Poise

Newton

Pascal

129. ____________ has their outermost shell complete in atomic form

Gun metals

Coinage metals

Alkali metals

Noble gases

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

BrF₃

NH₃

H₂O

BF₃

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

Planar

Angular

Pyramidal

Trigonal bipyramidal

132. 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

10.234

10.234017

10.2340178

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

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

Both polar covalent and hydrogen bonds

Hydrogen bonds only

134. 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

6.63 x 10¯³⁵ m

6.65 x 10¯³⁵ m

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

HBr

H₂O

HCl

136. Quantum umber values for 2p orbitals are

n = 2, l = 0

n = 2, l = 1

n = 1, l = 2

n = 1, l = 0

137. 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

138. XeF₄ has shape of

Sphere

Tetrahedral

Trigonal bipyramidal

Square planar

139. 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

Fifth Bohr orbit to the second Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

140. Number of π-bonds in naphthalene is

141. 2nd orbit is away from nucleus for H-atom as compared to first orbit

6-times

2-times

3-times

4-times

142. Along a period the atomic radii

Decreases

Increases

Constant

First decreases then increases

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

109.5

102

104.5

107.5

144. Geometry of simple molecule having SP³ hybrid orbital is

Square planner

Tetrahedral

Triangular

Linear

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

X-rays not produced

Shorter wavelength

Larger wavelength

Gamma rays

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

SiF₄

XeF₄

SF₄

BF₃

147. 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

Sublimation of metallic sodium to give yellow vapour

Photosensitivity of sodium

Low ionization energy of sodium

148. Bond order for N2 molecule is

149. Bohr’s model atom is contradicted by

Plank’s quantum theory

Quarternization of angular members

Heisenberg’s uncertainty principle

Quarternization of energy of electrons

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

Bonding will not occur

Orbital overlap will not occur

None of these

Both A and B are correct

Page 7 of 8

151. Which one of these is weakest?

Metallic bond

Van der Waal’s forces

Covalent bond

Ionic bond

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

Tetrahedral

Planar triangle

Square planar

Pyramidal

153. Which of the following is not isoelectronic?

Cl¯

O²¯

Na⁺

Mg²⁺

154. An oxygen atom has mass of

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

155. Choose the correct statement

Each bonding molecular orbital can accommodate only one electron

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

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

156. 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

157. Nuclear radiation is emitted by those elements whose

Nuclei are stable

Molecules are unstable

Molecules are stable

Nuclei are unstable

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

6 x ɜ₀

9 x ɜ₀

1/2 x ɜ₀

3 x ɜ₀

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

Increases

Remains constant

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

Decreases

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

None

Linear geometry

SP hybridization

Dipole moment is zero

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

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

BH₃

NH₃

CH₄

H₂O

163. Covalent compounds are soluble in

Concentrated acids

Non-polar solvents

All solvents

Polar solvents

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

165. Al become isoelectronic with Ne

By losing two electrons

By losing three electrons

By gaining three electrons

By gaining two electrons

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

Impossible to predict

2 n

3 n

167. When potassium metal is exposed to violet light

The absorption of electrons takes place

There is no effect

Ejection of electrons takes place

Ejection of some potassium atoms occurs

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

Bond order of 2.5

Stability lower then O₂

Three unpaired electrons

Diamagnetic character

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

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

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

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

Dispersion force

Chemical bond

Van der Waal’s force

London force

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

Electron affinity

Electro negativity

None of these

Ionization energy

172. The nature of positive rays depends upon

The nature of residual gas

The nature of discharge tube

All of these

The nature of electrode

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

174. Fluorine molecule is formed by

The axial p-p overlap

The axial s-p overlap

The overlap of two sp² hybrid orbitals

The sidewise p-p overlap

175. 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

Colour spectrum

Vaporization

Page 8 of 8

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

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

2, 1, 1

2, 1, 0

3, 2, 1

3, 1, 1

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

Electron affinity

Atomic size

Electronegativity

Ionization energy

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

Two sigma, two pi

Two sigma, one pi

One sigma, one pi

One sigma, two pi

180. The shape of the molecule SF₂Cl₂ is

Cubic

Octahedral

Tetrahedral

Trigonal bipyramidal

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

CHCl₃

NaCl

CH₄

H₂O

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

Lone pair – lone pair repulsion only

Lone pair – bond pair repulsion only

Bond pair – bond pair repulsion only

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

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