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ECAT Chemistry Chemical Bonding Online Test

Maan AliLast Updated: April 19, 2025

Chemistry Chemical Bonding MCQS Online Test

ECAT Chemistry Chemical Bonding Chapter Online Test

Total Questions:	187
Time Allowed:	60 Minutes
Total Marks:	187
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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ECAT Chemistry Chemical Bonding Test

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Page 1 of 8

Chemistry

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

6 x ɜ₀

1/2 x ɜ₀

9 x ɜ₀

3 x ɜ₀

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

CHCl₃

CH₄

NaCl

H₂O

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

There may not be a possibility of chemical reaction

Lemon juice is dangerous for health

Water should be preferred over lemon Juice for drinking

There may be a possibility of a chemical reaction

4. Effective magnetic moment of Sc³ ion is

2.83

5.92

1.73

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

H₂O

HCl

CH₃Cl

CCl₄

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

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

H₂O

H₂Te

H₂S3

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

2, 6

2, 10

2, 8

2, 9

9. When potassium metal is exposed to violet light

Ejection of electrons takes place

There is no effect

Ejection of some potassium atoms occurs

The absorption of electrons takes place

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

11. 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?

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

O and F

Na and F

N and F

C and F

13. 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

X₂Y₃

XY₂

14. Lewis acids are

Electron deficient

Electron rich

Octet is complete

No such acids exist

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

3, 10

10, 3

4, 9

9, 4

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

Pyramidal

Planar triangle

Square planar

Tetrahedral

17. 1 erg of energy corresponds to

10¯⁷ J/mol

6.02 x 10²³ J/mol

1 erg/mol

6.02 x 10¹⁶ J/mol

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

BF₃

NH₃

BrF₃

H₂O

19. 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

6.63 x 10¯³⁵ m

6.65 x 10¯³⁵ m

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

Stability lower then O₂

Diamagnetic character

Bond order of 2.5

Three unpaired electrons

21. 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 equal to that in NO

Bond length is unpredictable

Bond length in NO⁺ is greater than in NO

Bond length in NO is greater than in NO⁺

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

Increases

Remains constant

Decreases

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

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

Excited state of fluorine

Excited state of neon

Ground state of fluorine atom

Excited state of O¯₂

24. H-bonding is not present in

Water

Glycerine

Hydrogen fluoride

Hydrogen sulphide

25. Which of the solid does not contain covalent bond

Graphite

Diamond

Copper

Ice

Page 2 of 8

26. 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

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

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

Octet rule

Electronegative character of elements

Electropositive character of elements

Pauli exclusion principle

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

SP hybridization

Dipole moment is zero

None

Linear geometry

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

Copper

Nickel

Iron

Chromium

31. Which molecule is polar among the following?

Ethane

Carbon tetrachloride

Carbon dioxide

Methanol

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

Zn⁺

Fe²⁺

Cu⁺

Ni³⁺

33. The structure of ICl₂¯ is

Square planar

Octahedral

Trigonal bipyramidal

Trigonal

34. Shape of CIO₃¯ is

Triangular pyramidal

Triangular bipyramidal

Triangular planar

Tetrahedral

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

Electronegativity

Activation energy

Ionization potential

Electron affinity

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

1.7588 x 10²⁰

1.7588 x 10¹¹

6.02 x 10²³

9.1095 x 10¯³¹

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

Dispersion force

H-bonding

Dipole-dipole interaction

Ion-dipole interaction

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

HCI

H2O

HBr

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

102

104.5

107.5

109.5

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

Water molecules associate through hydrogen bonding

Sulphure has high electronegativity than oxygen

Hydrogen sulphide is a weak acid

Water has higher molecular weight

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

They are mono atomic gases

They have high ionization energies

They do not react with one another

They have completely filled s and p orbitals

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

NH₃

CH₄

H₂O

BH₃

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

Prism

Cube

Hexagon

Tetrahedron

44. ____________ has their outermost shell complete in atomic form

Noble gases

Coinage metals

Alkali metals

Gun metals

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

Nine σ and seven π

Nine σ and nine π

Eight σ and eight π

Five π and nine σ

46. The shape of H₃O⁺ is

Tetrahedral

Angular

Pyramidal

Triangular planar

47. Covalent compounds are soluble in

Polar solvents

All solvents

Non-polar solvents

Concentrated acids

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

H – OH

H – NH₂

H – SH

H – Cl

49. 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?

-1.48

-1.11

-2.22

-2.96

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

6 electrons

1 electron

2 electrons

4 electrons

Page 3 of 8

51. 2nd orbit is away from nucleus for H-atom as compared to first orbit

4-times

6-times

3-times

2-times

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

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

Ni²⁺

Cu²⁺

Cu⁺

54. Hydrogen chloride molecule contains

Co-ordinate bond

Double bond

Electrovalent bond

Covalent bond

55. Bohr’s model atom is contradicted by

Heisenberg’s uncertainty principle

Quarternization of angular members

Quarternization of energy of electrons

Plank’s quantum theory

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

E.N

E.A

Ea.

I.P

57. In O2 each oxygen atom is hybridized

Sp3

Sp2

All

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

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

N₂

PCl₅

He₂

SO₂

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

Oxygen

Helium

Nitrogen

Hydrogen

61. The ionization energy

Does not change in a period

Generally increases from left to right in a period

Does not change in a group

Increase from top to bottom in a group

62. XeF₄ has shape of

Trigonal bipyramidal

Square planar

Tetrahedral

Sphere

63. 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

16 and 4

12 and 4

12 and 5

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

None of these

High, very negative

Low, positive or slightly negative

Low very negative

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

He⁺

Li⁺

66. Choose the correct statement

Each bonding molecular orbital can accommodate only one electron

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

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

3 and 5

3 and 7

3 and 9

2 and 5

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

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

None of these

Electron affinity

Electronegativity

Ionization energy

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

Constant

Variable trend

Increases

Decreases

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

Electronegativity

Atomic size

Ionization energy

Electron affinity

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

No specificity exist

Lesser then 1.7

Greater than 1.7

Equal to 1.7

73. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 2, l = 0

n = 1, l = 2

n = 1, l = 0

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

SiF₄

XeF₄

BF₃

SF₄

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……

s orbitals

p orbitals

sp³ hybrid orbitals

sp² hybrid orbitals

Page 4 of 8

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

They are formed when electros are formed from atoms

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

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

Bond pair – bond pair repulsion only

Lone pair – bond pair repulsion only

Lone pair – lone pair repulsion only

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

78. 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

79. The boiling point of heavy water is

110°C

101.4°C

99°C

108°C

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

One sigma, two pi

One sigma, one pi

Two sigma, one pi

Two sigma, two pi

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

3.0 BM

6.9 BM

4.9 BM

5.9 BM

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

2 n

Impossible to predict

3 n

83. Nuclear radiation is emitted by those elements whose

Nuclei are stable

Nuclei are unstable

Molecules are stable

Molecules are unstable

84. Geometry of simple molecule having SP³ hybrid orbital is

Linear

Tetrahedral

Triangular

Square planner

85. Deflection of blue light is lesser than violet because

Blue is absorbed more easily

Blue has higher wavelength

Blue is darker colour

Blue has more energy

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

4, 1, 0, ½

4, 1, 1, ½

4, 0, 0, ½

4, 4, 0, ½

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

SP²

88. Pi bonds are produced by overlapping of

Hybrid orbitals

Atomic orbital and hybrid orbital

Un-hybrid orbitals

Hybrid and un hybrid orbitals

89. Unit of dipole moment is

Pascal

Poise

Newton

Debye

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

91. On sp3 hybridization

One p-orbital is involved

Four p-orbitals are involved

One s and 3 p-orbitals are involved

All p-orbitals are involved

92. Geometry of simple molecule having sp3 hybrid orbital is

Tetrahedral

Square planner

Triangular

Linear

93. Lateral overlapping expected in

Ionic bond

O-bond

Metallic bond

Ā-bonds

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

Tetrahedral

Pyramidal

Triangular

Trigonal

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

Liquid NH3

Phenol

Liquid HCl

Water

96. 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

97. Fluorine molecule is formed by

The overlap of two sp² hybrid orbitals

The sidewise p-p overlap

The axial p-p overlap

The axial s-p overlap

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

Crystallization

Vaporization

Colour spectrum

Distillation

99. Electronic configuration of K is

[Kr]4S¹

[He]4S¹

[AR]4S²

[AR]4S¹

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

Larger wavelength

X-rays not produced

Gamma rays

Shorter wavelength

Page 5 of 8

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

No effect

Lesser

Remain same

Greater

102. Which of the following has zero depolemoment?

SiF₄

ClF

CFCl₃

PCl₃

103. Number of sigma bonds in P₄O₁₀ is

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

HCl

H₂O

HBr

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

Na⁺

Cl¯

K⁺

S¯²

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

Two sigma bonds and one pi-bond

Three sigma bonds

One sigma bond and two pi-bonds

Three pi-bonds

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

All of above represent same entity

Bond

Attractive force

Interaction

108. A lone pair of electrons in an atom implies

A pair of electrons

A pair of valence electrons not involved in bonding

A pair of valence electrons

A pair of electrons involved in bonding

109. 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

Dipole interaction

Hydrogen bond formation

Covalent attraction

110. 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

111. Which of the following species is paramagnetic?

O²¯

CO₂

CN¯

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

113. 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

10.23

10.234017

10.234

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

SP²

115. Unit of dipole moment is

Pascal

Debye

Poise

Newton

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

-13.6 eV

Zero

-5.44 eV

-54.4 eV

117. Maximum hydrogen bonds in water are,

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

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

120. Which of the following is not isoelectronic?

Cl¯

Mg²⁺

O²¯

Na⁺

121. Ionic radius in a period from left to right

Increases

Decreases

First decreases then increases

First increases then decreases

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

123. Number of π-bonds in naphthalene is

124. Bond angle in water is

104.5°

107°

120°

109.5°

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

Cannot be determined

Both are equal

Page 6 of 8

126. The carbon atoms in calcium carbide are held by

2π and one σ bond

2 sigma bonds

2 covalent, one co-ordinate bond

Ionic bonds

127. Energy of an atom in a compound is

No change

Impossible to predict

Higher than individual

Lesser than individual

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

Electron

All these

Proton

Neutron

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

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

Trigonal bipyramidal

Planar

Angular

Pyramidal

131. 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

Microwave, infrared, visible, ultraviolet

Radio, visible, infrared, ultraviolet

132. Which one of these is weakest?

Metallic bond

Van der Waal’s forces

Ionic bond

Covalent bond

133. The velocity of photon is

Equal to square

Independent of its wavelength

Depends on its source

Depends on its wavelength

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

First decreases then increases

Decreases

First increases then decreases

Increases

135. Along a period the atomic radii

Constant

First decreases then increases

Increases

Decreases

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

Trigonal bipyramidal

Triangular

Octahedral

Square planner

137. Anti-bonding MO is formed by

None of these

Subtraction of atomic orbitals

Addition of atomic orbitals

Multiplication of atomic orbitals

138. Which of the following molecule has Ā bond

O₂

NH₃

C₃H₆

H₂O

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

It has high electronegativity

It has high heat of dissociation

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

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

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

142. Choose the correct statement about 2nd ionization energy

It is always greater than 1st ionization energy

It is equal to the 1st ionization energy

It is always less than 1st ionization energy

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

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

144. 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, 0

2, 1, 1

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

Calcium

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

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

5….1

1….5

5….0

0….5

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

90°

120°

109°

60°

149. Pick out the molecule which has zero dipole moment

SO₂

BCl₃

H₂O

NH₃

150. Which of the following has unchanged valency?

Oxygen

Page 7 of 8

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

The repulsive force dominate the attractive forces

The two atoms start ionization

The attractive forces dominate the repulsive forces

They energy of atoms increases

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

65.6 nm

656 nm

0.656 nm

6.56 nm

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

Fluorides are more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides is more electronegative

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

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

H₂O₂

CH₄

HCN

NH₄Cl

156. Which carbon is more electronegative?

always same irrespective of its hybrid state

sp³-hybridized carbon

sp- hybridized carbon

sp²- hybridized carbon

157. Molecular orbitals are filled according to

Aufbau principal

All these

Hund’s rule

Pauli’s exclusion principle

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

Ge, Sn

As, Sb

In, Pt

Se, Te

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

Photosensitivity of sodium

Low ionization energy of sodium

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

Sublimation of metallic sodium to give yellow vapour

160. 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

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

N⁺H₄

CH₄

PCl₃

Pcl₄

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

None of these

Orbital overlap will not occur

Bonding will not occur

Both A and B are correct

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

Ionization energy

Electron affinity

Electro negativity

None of these

164. Al become isoelectronic with Ne

By losing three electrons

By gaining two electrons

By gaining three electrons

By losing two electrons

165. Which has the minimum bond angle?

CH₄

H₂O

NH₃

H₂S

166. 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

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

Li⁺

He⁺

168. Inter molecular forces in solid hydrogen are

Covalent forces

Hydrogen bonds

All of these

Van der Waal forces or London dispersion forces

169. An oxygen atom has mass of

16g

2.657 x 10¯²³ g

5.316 x 10¯²³ g

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

Octahedral

Distorted tetrahedral

Planar triangle

Linear

171. The number of significant figures in 0.00200 is

One

Three

Two

Five

172. Which of these molecules require more bond energy?

Hydrogen

Nitrogen

Oxygen

173. Molecular orbital picture of N₂ indicates

No unpaired electron

Two unpaired electron

One unpaired electron

None of these

174. The shape of the molecule SF₂Cl₂ is

Cubic

Octahedral

Tetrahedral

Trigonal bipyramidal

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

Van der Waal’s force

London force

Dispersion force

Chemical bond

Page 8 of 8

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

NaCl

SiCl₄

MgCl₂

AlCl₃

177. Bond order for N2 molecule is

178. The nature of positive rays depends upon

The nature of residual gas

The nature of electrode

All of these

The nature of discharge tube

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

HBr

HCl

180. 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

1 bond pair 3 lone pair

2 bond pair 2 lone pair

181. 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

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

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

Ionization energy

Electro negativity

None of these

Electron affinity

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Maan AliLast Updated: April 19, 2025

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