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

X – radiation, visible, infrared, microwave

Visible, ultraviolet, infrared, gamma rays

Radio, visible, infrared, ultraviolet

Microwave, infrared, visible, ultraviolet

2. Which of these molecules require more bond energy?

Nitrogen

Oxygen

Hydrogen

3. Bond angle in water is

109.5°

104.5°

107°

120°

4. Fluorine molecule is formed by

The overlap of two sp² hybrid orbitals

The axial p-p overlap

The sidewise p-p overlap

The axial s-p overlap

5. Effective magnetic moment of Sc³ ion is

1.73

2.83

5.92

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

He⁺

Li⁺

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

H₂O

HCl

HBr

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

Diamagnetic character

Stability lower then O₂

Three unpaired electrons

Bond order of 2.5

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

SP²

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

They are smaller than the atoms from which they were formed

They are also known as cations

They are larger than the atoms from which they were formed

They are formed when electros are formed from atoms

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

NaCl

SiCl₄

MgCl₂

AlCl₃

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

13. Shape of CIO₃¯ is

Triangular planar

Triangular bipyramidal

Triangular pyramidal

Tetrahedral

14. Geometry of simple molecule having sp3 hybrid orbital is

Triangular

Tetrahedral

Linear

Square planner

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

5….1

1….5

0….5

5….0

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

Van der Waal’s force

Dispersion force

London force

Chemical bond

17. Which has the minimum bond angle?

NH₃

H₂S

CH₄

H₂O

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

A stream of electrons

Move with speed as that of light

Charged particles

Can be deflected by magnetic fields

19. Nuclear radiation is emitted by those elements whose

Nuclei are stable

Nuclei are unstable

Molecules are unstable

Molecules are stable

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

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

1/2 x ɜ₀

6 x ɜ₀

3 x ɜ₀

9 x ɜ₀

22. Ionic radius in a period from left to right

First increases then decreases

Increases

First decreases then increases

Decreases

23. The carbon atoms in calcium carbide are held by

2 covalent, one co-ordinate bond

2π and one σ bond

Ionic bonds

2 sigma bonds

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

Both polar covalent and hydrogen bonds

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

Hydrogen bonds only

25. Which of the following has unchanged valency?

Oxygen

Page 2 of 8

26. ____________ has their outermost shell complete in atomic form

Alkali metals

Gun metals

Noble gases

Coinage metals

27. 2nd orbit is away from nucleus for H-atom as compared to first orbit

6-times

4-times

2-times

3-times

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

C and F

N and F

Na and F

O and F

29. 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

30. Deflection of blue light is lesser than violet because

Blue is darker colour

Blue has more energy

Blue is absorbed more easily

Blue has higher wavelength

31. Unit of dipole moment is

Pascal

Debye

Newton

Poise

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

10, 3

4, 9

3, 10

9, 4

33. 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

34. Unit of dipole moment is

Newton

Debye

Poise

Pascal

35. Number of π-bonds in naphthalene is

36. Which one of these is weakest?

Van der Waal’s forces

Metallic bond

Covalent bond

Ionic bond

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

N⁺H₄

Pcl₄

PCl₃

CH₄

38. Hydrogen chloride molecule contains

Double bond

Covalent bond

Electrovalent bond

Co-ordinate bond

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

Pyramidal

Tetrahedral

Triangular

Trigonal

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

Linear geometry

SP hybridization

None

Dipole moment is zero

41. On sp3 hybridization

One s and 3 p-orbitals are involved

Four p-orbitals are involved

All p-orbitals are involved

One p-orbital is involved

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

SO₂

He₂

PCl₅

N₂

43. Which of the solid does not contain covalent bond

Diamond

Graphite

Ice

Copper

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

Calcium

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

Remain same

Lesser

Greater

No effect

46. The nature of positive rays depends upon

All of these

The nature of residual gas

The nature of discharge tube

The nature of electrode

47. 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

Both A and B are correct

Bonding will not occur

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

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

Two sigma, two pi

One sigma, two pi

One sigma, one pi

Two sigma, one pi

50. 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

Page 3 of 8

51. Along a period the atomic radii

Decreases

First decreases then increases

Constant

Increases

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

-5.44 eV

Zero

-13.6 eV

-54.4 eV

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

H – NH₂

H – SH

H – OH

H – Cl

54. An oxygen atom has mass of

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

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

Neutron

Proton

All these

Electron

56. In O2 each oxygen atom is hybridized

Sp3

All

Sp2

57. Which of the following species is paramagnetic?

O²¯

CN¯

CO₂

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

3, 2, 1

3, 1, 1

2, 1, 1

2, 1, 0

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

Electron affinity

Atomic size

Electronegativity

Ionization energy

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

Fe²⁺

Cu⁺

Ni³⁺

Zn⁺

61. 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

107.5

104.5

102

62. 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

63. The boiling point of heavy water is

101.4°C

108°C

99°C

110°C

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

BF₃

XeF₄

SF₄

SiF₄

65. Electronic configuration of K is

[AR]4S²

[Kr]4S¹

[AR]4S¹

[He]4S¹

66. Choose the correct statement about 2nd ionization energy

It is always greater than 1st ionization energy

It is always less than 1st 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

67. 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

Photosensitivity of sodium

Sublimation of metallic sodium to give yellow vapour

Low ionization energy of sodium

68. Geometry of simple molecule having SP³ hybrid orbital is

Linear

Triangular

Square planner

Tetrahedral

69. 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

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

They are mono atomic gases

They have high ionization energies

They have completely filled s and p orbitals

They do not react with one another

71. Pi bonds are produced by overlapping of

Hybrid and un hybrid orbitals

Un-hybrid orbitals

Hybrid orbitals

Atomic orbital and hybrid orbital

72. Maximum hydrogen bonds in water are,

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

H₂S3

H₂O

H₂Te

74. Choose the correct statement

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

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

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

X-rays not produced

Shorter wavelength

Gamma rays

Larger wavelength

Page 4 of 8

76. Lateral overlapping expected in

O-bond

Ā-bonds

Ionic bond

Metallic bond

77. 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

65.6 nm

6.56 nm

656 nm

0.656 nm

78. Energy of an atom in a compound is

Higher than individual

No change

Lesser than individual

Impossible to predict

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

Nickel

Iron

Chromium

Copper

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

4 electrons

2 electrons

1 electron

6 electrons

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

Colour spectrum

Distillation

Crystallization

Vaporization

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

Square planar

Pyramidal

Tetrahedral

Planar triangle

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

Increases

Decreases

First increases then decreases

First decreases then increases

84. 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⁺

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

Cannot be determined

Both are equal

86. 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 7

3 and 5

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

H₂O₂

NH₄Cl

CH₄

HCN

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

SP²

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

90. The structure of ICl₂¯ is

Octahedral

Trigonal

Trigonal bipyramidal

Square planar

91. Which of the following has zero depolemoment?

SiF₄

ClF

PCl₃

CFCl₃

92. The number of significant figures in 0.00200 is

Three

One

Two

Five

93. Which of the following molecule has Ā bond

C₃H₆

NH₃

H₂O

O₂

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

Liquid HCl

Liquid NH3

Phenol

Water

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

BH₃

H₂O

NH₃

CH₄

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

97. Inter molecular forces in solid hydrogen are

Hydrogen bonds

Van der Waal forces or London dispersion forces

All of these

Covalent forces

98. Which carbon is more electronegative?

sp- hybridized carbon

sp³-hybridized carbon

sp²- hybridized carbon

always same irrespective of its hybrid state

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

Trigonal bipyramidal

Pyramidal

Planar

Angular

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

6.9 BM

4.9 BM

5.9 BM

3.0 BM

Page 5 of 8

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

6.63 x 10¯³⁴ m

6.63 x 10¯³³ m

6.65 x 10¯³⁵ m

6.63 x 10¯³⁵ m

102. XeF₄ has shape of

Tetrahedral

Trigonal bipyramidal

Sphere

Square planar

103. When a double bond is formed between two atoms, one of the bonds is a sigma bond and the other is a pi bond. The pi bond is created by the overlap of……

s orbitals

sp³ hybrid orbitals

sp² hybrid orbitals

p orbitals

104. Covalent compounds are soluble in

All solvents

Concentrated acids

Polar solvents

Non-polar solvents

105. The shape of H₃O⁺ is

Pyramidal

Triangular planar

Angular

Tetrahedral

106. 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 have low electron density between the two nuclei

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

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

107. Which molecule is polar among the following?

Carbon tetrachloride

Ethane

Carbon dioxide

Methanol

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

Water has higher molecular weight

Water molecules associate through hydrogen bonding

Sulphure has high electronegativity than oxygen

Hydrogen sulphide is a weak acid

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

Ionization potential

Electron affinity

Electronegativity

Activation energy

110. H-bonding is not present in

Hydrogen sulphide

Hydrogen fluoride

Glycerine

Water

111. Colour of the glow produced in the discharge tube

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

Depends on the pressure in the discharge tube

Depends on the gas used in the discharge tube

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

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

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

115. 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

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

NH₃

BrF₃

H₂O

BF₃

117. When potassium metal is exposed to violet light

There is no effect

Ejection of electrons takes place

The absorption of electrons takes place

Ejection of some potassium atoms occurs

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

The two atoms start ionization

The repulsive force dominate the attractive forces

The attractive forces dominate the repulsive forces

They energy of atoms increases

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

Five π and nine σ

Nine σ and nine π

Nine σ and seven π

Eight σ and eight π

120. 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

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

There may be a possibility of a chemical reaction

Water should be preferred over lemon Juice for drinking

There may not be a possibility of chemical reaction

Lemon juice is dangerous for health

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

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

Dispersion force

H-bonding

Dipole-dipole interaction

Ion-dipole interaction

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

HCl

HBr

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

Page 6 of 8

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

Cl¯

K⁺

Na⁺

S¯²

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

128. Bohr’s model atom is contradicted by

Quarternization of energy of electrons

Heisenberg’s uncertainty principle

Plank’s quantum theory

Quarternization of angular members

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

Increases

Constant

Variable trend

Decreases

130. Lewis acids are

Electron deficient

Electron rich

No such acids exist

Octet is complete

131. 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

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

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

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

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

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

3 lone pair 1 bond pair

1 bond pair 3 lone pair

2 bond pair 2 lone pair

3 bond pair one lone pair

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

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides is more electronegative

Fluorides are more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

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

Electron affinity

Electro negativity

None of these

Ionization energy

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

Octahedral

Distorted tetrahedral

Planar triangle

Linear

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

1.7588 x 10¹¹

6.02 x 10²³

1.7588 x 10²⁰

9.1095 x 10¯³¹

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

Electron affinity

None of these

Ionization energy

Electro negativity

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

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

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

It has high electronegativity

It has high heat of dissociation

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

Se, Te

Ge, Sn

As, Sb

In, Pt

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

4, 4, 0, ½

4, 1, 1, ½

4, 0, 0, ½

4, 1, 0, ½

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

143. The velocity of photon is

Depends on its source

Depends on its wavelength

Independent of its wavelength

Equal to square

144. 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

145. Which of the following is not isoelectronic?

Cl¯

Mg²⁺

Na⁺

O²¯

146. 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?

147. The ionization energy

Generally increases from left to right in a period

Does not change in a period

Increase from top to bottom in a group

Does not change in a group

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

He⁺

Li⁺

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

Bond

Attractive force

All of above represent same entity

Interaction

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

Page 7 of 8

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

Ionization energy

Electronegativity

None of these

Electron affinity

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

Dipole interaction

Van der Waal’s forces

Hydrogen bond formation

Covalent attraction

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

Three sigma bonds

One sigma bond and two pi-bonds

Two sigma bonds and one pi-bond

Three pi-bonds

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

155. Pick out the molecule which has zero dipole moment

SO₂

NH₃

H₂O

BCl₃

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

109°

90°

120°

60°

157. The shape of the molecule SF₂Cl₂ is

Octahedral

Cubic

Trigonal bipyramidal

Tetrahedral

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

2, 6

2, 8

2, 9

2, 10

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

HCI

H2O

HBr

160. 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

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

Greater than 1.7

No specificity exist

Equal to 1.7

Lesser then 1.7

162. 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

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

Triangular

Trigonal bipyramidal

Octahedral

Square planner

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

H₂O

NaCl

CH₄

CHCl₃

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

H₂O

CH₃Cl

HCl

CCl₄

166. Anti-bonding MO is formed by

Multiplication of atomic orbitals

Subtraction of atomic orbitals

None of these

Addition of atomic orbitals

167. Number of sigma bonds in P₄O₁₀ is

168. Molecular orbitals are filled according to

All these

Pauli’s exclusion principle

Hund’s rule

Aufbau principal

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

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

Lone pair – bond pair repulsion only

Bond pair – bond pair repulsion only

Lone pair – lone pair repulsion only

170. 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

-2.22

-2.96

-1.48

171. Quantum umber values for 2p orbitals are

n = 1, l = 0

n = 2, l = 0

n = 1, l = 2

n = 2, l = 1

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

Low very negative

High, very negative

Low, positive or slightly negative

None of these

173. Al become isoelectronic with Ne

By gaining three electrons

By losing three electrons

By gaining two electrons

By losing two electrons

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

Oxygen

Helium

Nitrogen

Hydrogen

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

Impossible to predict

2 n

3 n

Page 8 of 8

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

Electropositive character of elements

Pauli exclusion principle

Electronegative character of elements

Octet rule

177. Bond order for N2 molecule is

178. Molecular orbital picture of N₂ indicates

Two unpaired electron

None of these

One unpaired electron

No unpaired electron

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

E.N

E.A

I.P

Ea.

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

Tetrahedron

Cube

Hexagon

Prism

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

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

Excited state of neon

Excited state of fluorine

Ground state of fluorine atom

Excited state of O¯₂

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