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

N⁺H₄

CH₄

PCl₃

Pcl₄

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

HCI

H2O

HBr

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

HCN

NH₄Cl

CH₄

H₂O₂

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

He⁺

Li⁺

5. The velocity of photon is

Depends on its source

Independent of its wavelength

Equal to square

Depends on its wavelength

6. Deflection of blue light is lesser than violet because

Blue is absorbed more easily

Blue has more energy

Blue has higher wavelength

Blue is darker colour

7. Bond order for N2 molecule is

8. 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

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

Tetrahedral

Pyramidal

Planar triangle

Square planar

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

Distorted tetrahedral

Linear

Octahedral

Planar triangle

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

E.N

Ea.

E.A

I.P

12. 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

s orbitals

sp³ hybrid orbitals

sp² hybrid orbitals

13. A lone pair of electrons in an atom implies

A pair of electrons

A pair of valence electrons

A pair of valence electrons not involved in bonding

A pair of electrons involved in bonding

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

9.1095 x 10¯³¹

1.7588 x 10²⁰

1.7588 x 10¹¹

6.02 x 10²³

15. 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

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

Na and F

C and F

O and F

N and F

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

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

Photosensitivity of sodium

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

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

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

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

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

2, 10

2, 9

2, 6

2, 8

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

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

SP²

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

24. Which of these molecules require more bond energy?

Nitrogen

Hydrogen

Oxygen

25. Which of the following is not isoelectronic?

O²¯

Na⁺

Mg²⁺

Cl¯

Page 2 of 8

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

Low very negative

Low, positive or slightly negative

None of these

High, very negative

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

3 and 9

2 and 5

3 and 7

3 and 5

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

HCl

HBr

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

H – Cl

H – SH

H – NH₂

H – OH

30. Molecular orbitals are filled according to

Aufbau principal

Hund’s rule

Pauli’s exclusion principle

All these

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

HCl

H₂O

HBr

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

Phenol

Liquid NH3

Water

Liquid HCl

33. Choose the correct statement

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

Each bonding molecular orbital can accommodate only one electron

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

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

Electronegativity

Electron affinity

Ionization potential

Activation energy

35. Maximum hydrogen bonds in water are,

36. 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 larger than the atoms from which they were formed

They are smaller than the atoms from which they were formed

37. 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?

38. Fluorine molecule is formed by

The axial s-p overlap

The sidewise p-p overlap

The axial p-p overlap

The overlap of two sp² hybrid orbitals

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

5….1

1….5

5….0

0….5

40. Energy of an atom in a compound is

No change

Lesser than individual

Higher than individual

Impossible to predict

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

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

Ge, Sn

Se, Te

In, Pt

As, Sb

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

Fluorides is more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides are more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

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

H₂O

H₂Te

H₂O

H₂S3

45. Which of the following molecule has Ā bond

NH₃

C₃H₆

O₂

H₂O

46. Bond angle in water is

120°

109.5°

104.5°

107°

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

The two atoms start ionization

The repulsive force dominate the attractive forces

They energy of atoms increases

The attractive forces dominate the repulsive forces

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

Decreases

Increases

First decreases then increases

First increases then decreases

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

All of above represent same entity

Attractive force

Bond

Interaction

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

Two sigma, one pi

Two sigma, two pi

One sigma, two pi

One sigma, one pi

Page 3 of 8

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

Sulphure has high electronegativity than oxygen

Water molecules associate through hydrogen bonding

Water has higher molecular weight

Hydrogen sulphide is a weak acid

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

90°

120°

60°

109°

53. 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

Dipole interaction

Van der Waal’s forces

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

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

Increases

Variable trend

Decreases

Constant

56. Lateral overlapping expected in

O-bond

Ionic bond

Metallic bond

Ā-bonds

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

Impossible to predict

2 n

3 n

58. Unit of dipole moment is

Debye

Newton

Poise

Pascal

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

Radio, visible, infrared, ultraviolet

X – radiation, visible, infrared, microwave

Microwave, infrared, visible, ultraviolet

Visible, ultraviolet, infrared, gamma rays

60. The nature of positive rays depends upon

The nature of discharge tube

The nature of electrode

The nature of residual gas

All of these

61. Ionic radius in a period from left to right

Decreases

First increases then decreases

First decreases then increases

Increases

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

Triangular

Pyramidal

Trigonal

Tetrahedral

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

6 x ɜ₀

9 x ɜ₀

3 x ɜ₀

1/2 x ɜ₀

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

Nickel

Iron

Chromium

Copper

65. Electronic configuration of K is

[Kr]4S¹

[AR]4S²

[AR]4S¹

[He]4S¹

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

Electron

All these

Proton

Neutron

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

XeF₄

SF₄

SiF₄

BF₃

68. Which of the following has unchanged valency?

Oxygen

69. 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

Sixth Bohr orbit to the third Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

70. Lewis acids are

Electron rich

Electron deficient

No such acids exist

Octet is complete

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

3, 2, 1

2, 1, 0

3, 1, 1

2, 1, 1

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

Calcium

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

-13.6 eV

-5.44 eV

Zero

-54.4 eV

74. When potassium metal is exposed to violet light

Ejection of electrons takes place

The absorption of electrons takes place

Ejection of some potassium atoms occurs

There is no effect

75. Unit of dipole moment is

Pascal

Poise

Debye

Newton

Page 4 of 8

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

CH₃Cl

HCl

CCl₄

H₂O

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

SO₂

He₂

N₂

PCl₅

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

79. Which of the following species is paramagnetic?

CO₂

O²¯

CN¯

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

81. 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

82. XeF₄ has shape of

Square planar

Sphere

Tetrahedral

Trigonal bipyramidal

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

Dispersion force

Chemical bond

London force

Van der Waal’s force

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

Three pi-bonds

One sigma bond and two pi-bonds

Two sigma bonds and one pi-bond

Three sigma bonds

85. Geometry of simple molecule having sp3 hybrid orbital is

Triangular

Linear

Tetrahedral

Square planner

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

87. Which of the following has zero depolemoment?

PCl₃

CFCl₃

ClF

SiF₄

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

Bonding molecular orbitals have low electron density between the two nuclei

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

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

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

89. 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

65.6 nm

0.656 nm

6.56 nm

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

Eight σ and eight π

Five π and nine σ

Nine σ and seven π

Nine σ and nine π

91. 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

92. Quantum umber values for 2p orbitals are

n = 1, l = 2

n = 1, l = 0

n = 2, l = 0

n = 2, l = 1

93. 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

102

104.5

94. The shape of H₃O⁺ is

Angular

Pyramidal

Tetrahedral

Triangular planar

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

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

97. Covalent compounds are soluble in

Non-polar solvents

Polar solvents

All solvents

Concentrated acids

98. 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⁺

Cu⁺

Ni²⁺

99. Number of π-bonds in naphthalene is

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

Planar

Trigonal bipyramidal

Angular

Pyramidal

Page 5 of 8

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

None of these

Electron affinity

Electronegativity

Ionization energy

102. The carbon atoms in calcium carbide are held by

2 sigma bonds

Ionic bonds

2π and one σ bond

2 covalent, one co-ordinate bond

103. Pi bonds are produced by overlapping of

Un-hybrid orbitals

Atomic orbital and hybrid orbital

Hybrid and un hybrid orbitals

Hybrid orbitals

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

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

It has high electronegativity

It has high heat of dissociation

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

105. 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

Crystallization

Distillation

Vaporization

106. Pick out the molecule which has zero dipole moment

SO₂

H₂O

NH₃

BCl₃

107. Number of sigma bonds in P₄O₁₀ is

108. Which has the minimum bond angle?

H₂S

NH₃

CH₄

H₂O

109. Which one of these is weakest?

Ionic bond

Metallic bond

Covalent bond

Van der Waal’s forces

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

4 electrons

6 electrons

2 electrons

1 electron

111. Nuclear radiation is emitted by those elements whose

Nuclei are unstable

Nuclei are stable

Molecules are unstable

Molecules are stable

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

K⁺

S¯²

Cl¯

Na⁺

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

NaCl

SiCl₄

AlCl₃

MgCl₂

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

115. Choose the correct statement about 2nd ionization energy

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

It is always less than 1st ionization energy

It is equal to the 1st ionization energy

It is always greater than 1st ionization energy

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

Zn⁺

Ni³⁺

Cu⁺

Fe²⁺

117. 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

118. Effective magnetic moment of Sc³ ion is

2.83

1.73

5.92

119. H-bonding is not present in

Hydrogen sulphide

Glycerine

Hydrogen fluoride

Water

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

X₂Y₃

X₂Y

XY₂

121. 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

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

X-rays not produced

Larger wavelength

Gamma rays

Shorter wavelength

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

Decreases

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

Remains constant

Increases

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

9, 4

4, 9

3, 10

10, 3

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

None of these

Bonding will not occur

Both A and B are correct

Orbital overlap will not occur

Page 6 of 8

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

None

Linear geometry

Dipole moment is zero

SP hybridization

127. Al become isoelectronic with Ne

By losing three electrons

By losing two electrons

By gaining three electrons

By gaining two electrons

128. Geometry of simple molecule having SP³ hybrid orbital is

Linear

Square planner

Tetrahedral

Triangular

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

Dipole-dipole interaction

Dispersion force

Ion-dipole interaction

H-bonding

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

Trigonal bipyramidal

Square planner

Octahedral

Triangular

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

Greater than 1.7

Lesser then 1.7

No specificity exist

Equal to 1.7

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

Helium

Nitrogen

Hydrogen

Oxygen

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

CHCl₃

H₂O

CH₄

NaCl

134. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers l = 1 and l = 2 are respectively

12 and 5

16 and 5

16 and 4

12 and 4

135. Along a period the atomic radii

First decreases then increases

Decreases

Increases

Constant

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

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

Diamagnetic character

Three unpaired electrons

Stability lower then O₂

Bond order of 2.5

138. 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

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

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

141. 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

Lemon juice is dangerous for health

There may not be a possibility of chemical reaction

142. The boiling point of heavy water is

110°C

101.4°C

99°C

108°C

143. Which carbon is more electronegative?

sp- hybridized carbon

always same irrespective of its hybrid state

sp³-hybridized carbon

sp²- hybridized carbon

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

He⁺

Li⁺

145. 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

146. Shape of CIO₃¯ is

Tetrahedral

Triangular pyramidal

Triangular bipyramidal

Triangular planar

147. The structure of ICl₂¯ is

Square planar

Trigonal

Octahedral

Trigonal bipyramidal

148. 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?

10.2340178

10.234017

10.23

10.234

149. 1 erg of energy corresponds to

6.02 x 10²³ J/mol

6.02 x 10¹⁶ J/mol

1 erg/mol

10¯⁷ J/mol

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

Lesser

Remain same

No effect

Greater

Page 7 of 8

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

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

H₂O

BF₃

BrF₃

NH₃

153. 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

154. Molecular orbital picture of N₂ indicates

One unpaired electron

Two unpaired electron

None of these

No unpaired electron

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

Electronegative character of elements

Octet rule

Pauli exclusion principle

Electropositive character of elements

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

CH₄

BH₃

NH₃

H₂O

157. Hydrogen chloride molecule contains

Co-ordinate bond

Double bond

Electrovalent bond

Covalent bond

158. The number of significant figures in 0.00200 is

One

Five

Two

Three

159. Which of the solid does not contain covalent bond

Diamond

Ice

Copper

Graphite

160. Bohr’s model atom is contradicted by

Heisenberg’s uncertainty principle

Quarternization of angular members

Quarternization of energy of electrons

Plank’s quantum theory

161. 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

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

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

Electronegativity

Atomic size

Ionization energy

Electron affinity

164. 2nd orbit is away from nucleus for H-atom as compared to first orbit

2-times

4-times

6-times

3-times

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

Hexagon

Cube

Tetrahedron

Prism

166. 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

167. On sp3 hybridization

All p-orbitals are involved

One s and 3 p-orbitals are involved

One p-orbital is involved

Four p-orbitals are involved

168. 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

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

Electro negativity

Electron affinity

Ionization energy

None of these

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

SP²

171. ____________ has their outermost shell complete in atomic form

Noble gases

Gun metals

Alkali metals

Coinage metals

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

Hydrogen bonds only

Both polar covalent and hydrogen bonds

Nonpolar covalent bonds only

Ionic and nonpolar hydrogen bonds

173. The shape of the molecule SF₂Cl₂ is

Octahedral

Trigonal bipyramidal

Cubic

Tetrahedral

174. In O2 each oxygen atom is hybridized

Sp2

Sp3

All

175. Anti-bonding MO is formed by

Subtraction of atomic orbitals

None of these

Multiplication of atomic orbitals

Addition of atomic orbitals

Page 8 of 8

176. 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

177. Which molecule is polar among the following?

Methanol

Carbon tetrachloride

Carbon dioxide

Ethane

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

Both are equal

Cannot be determined

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

Electro negativity

Ionization energy

Electron affinity

None of these

180. 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

181. 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

182. Inter molecular forces in solid hydrogen are

All of these

Hydrogen bonds

Van der Waal forces or London dispersion forces

Covalent forces

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Malik TahirLast Updated: October 14, 2025

Chemistry Chemical Bonding Online Mcqs Test

Important Chemistry Chemical Bonding Question and Answer

Chemistry Chemical Bonding Practice Test Online With Explanation

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