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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

Page 1 of 8

Chemistry

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

Nine σ and seven π

Eight σ and eight π

Five π and nine σ

Nine σ and nine π

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

SP²

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

4. Which of the following has unchanged valency?

Oxygen

5. The structure of ICl₂¯ is

Square planar

Trigonal

Octahedral

Trigonal bipyramidal

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

Ge, Sn

As, Sb

In, Pt

Se, Te

7. Lateral overlapping expected in

O-bond

Ionic bond

Ā-bonds

Metallic bond

8. Choose the correct statement

Each bonding molecular orbital can accommodate only one electron

In molecular orbitals, the number of bonding electrons equals the number of anti-bonding electrons

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

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

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

Water has higher molecular weight

Hydrogen sulphide is a weak acid

Sulphure has high electronegativity than oxygen

Water molecules associate through hydrogen bonding

10. An oxygen atom has mass of

2.657 x 10¯²³ g

5.316 x 10¯²³ g

16g

5.316 x 10¯²³ g

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

Bond order of 2.5

Stability lower then O₂

Three unpaired electrons

Diamagnetic character

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

Na and F

N and F

C and F

O and F

13. Number of sigma bonds in P₄O₁₀ is

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

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

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

15. On sp3 hybridization

All p-orbitals are involved

Four p-orbitals are involved

One p-orbital is involved

One s and 3 p-orbitals are involved

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

SP hybridization

None

Linear geometry

Dipole moment is zero

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

He⁺

Li⁺

18. Al become isoelectronic with Ne

By gaining two electrons

By gaining three electrons

By losing two electrons

By losing three electrons

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

Trigonal bipyramidal

Octahedral

Square planner

Triangular

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

-13.6 eV

Zero

-5.44 eV

-54.4 eV

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

Oxygen

Helium

Nitrogen

Hydrogen

22. Bohr’s model atom is contradicted by

Plank’s quantum theory

Heisenberg’s uncertainty principle

Quarternization of angular members

Quarternization of energy of electrons

23. 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

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

25. 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

Page 2 of 8

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

27. In Millikan oil – drop experiment, the charges on several different oil drops were as: -5.92. – 4.44, -2.96, -8.88. The units are arbitrary. Choose the likely value of the electronic charge in these arbitrary units?

-2.96

-1.11

-2.22

-1.48

28. The carbon atoms in calcium carbide are held by

Ionic bonds

2π and one σ bond

2 sigma bonds

2 covalent, one co-ordinate bond

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

30. Electronic configuration of K is

[AR]4S¹

[Kr]4S¹

[AR]4S²

[He]4S¹

31. The number of significant figures in 0.00200 is

Five

One

Two

Three

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

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

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

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

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

33. 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

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

Cu⁺

Cu²⁺

Ni²⁺

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

H₂S3

H₂O

H₂Te

36. Which of the solid does not contain covalent bond

Diamond

Copper

Ice

Graphite

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

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

It has high electronegativity

38. 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

39. 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 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

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

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

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

CCl₄

CH₃Cl

HCl

H₂O

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

The attractive forces dominate the repulsive forces

They energy of atoms increases

The two atoms start ionization

The repulsive force dominate the attractive forces

44. The shape of H₃O⁺ is

Triangular planar

Tetrahedral

Pyramidal

Angular

45. A lone pair of electrons in an atom implies

A pair of valence electrons

A pair of electrons

A pair of valence electrons not involved in bonding

A pair of electrons involved in bonding

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

Bond

Interaction

Attractive force

All of above represent same entity

47. Which molecule is polar among the following?

Ethane

Methanol

Carbon tetrachloride

Carbon dioxide

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

49. 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

50. Bond angle in water is

104.5°

120°

107°

109.5°

Page 3 of 8

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

2, 6

2, 8

2, 9

2, 10

52. The velocity of photon is

Depends on its wavelength

Independent of its wavelength

Equal to square

Depends on its source

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

Vaporization

Distillation

Crystallization

Colour spectrum

54. Shape of CIO₃¯ is

Triangular pyramidal

Triangular planar

Tetrahedral

Triangular bipyramidal

55. Unit of dipole moment is

Debye

Poise

Newton

Pascal

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

H – SH

H – Cl

H – NH₂

H – OH

57. Which one of these is weakest?

Van der Waal’s forces

Ionic bond

Metallic bond

Covalent bond

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

HBr

HCl

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

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

3 x ɜ₀

9 x ɜ₀

6 x ɜ₀

1/2 x ɜ₀

61. 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?

Covalent attraction

Dipole interaction

Hydrogen bond formation

Van der Waal’s forces

62. Pi bonds are produced by overlapping of

Atomic orbital and hybrid orbital

Hybrid and un hybrid orbitals

Hybrid orbitals

Un-hybrid orbitals

63. 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

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

Shorter wavelength

X-rays not produced

Larger wavelength

Gamma rays

65. 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

66. Which of the following is not isoelectronic?

Cl¯

Mg²⁺

Na⁺

O²¯

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

None of these

High, very negative

Low very negative

Low, positive or slightly negative

68. Which of the following molecule has Ā bond

H₂O

C₃H₆

O₂

NH₃

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

Remains constant

Decreases

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

Increases

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

Excited state of fluorine

Excited state of O¯₂

Ground state of fluorine atom

Excited state of neon

71. Covalent compounds are soluble in

Concentrated acids

All solvents

Non-polar solvents

Polar solvents

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

H-bonding

Dipole-dipole interaction

Dispersion force

Ion-dipole interaction

73. Which of the following has zero depolemoment?

ClF

PCl₃

SiF₄

CFCl₃

74. The shape of the molecule SF₂Cl₂ is

Octahedral

Tetrahedral

Cubic

Trigonal bipyramidal

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

Page 4 of 8

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

Fe²⁺

Ni³⁺

Cu⁺

Zn⁺

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

Chemical bond

London force

Van der Waal’s force

Dispersion force

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

Pyramidal

Square planar

Planar triangle

Tetrahedral

80. Bond order for N2 molecule is

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

Hydrogen bonds only

Nonpolar covalent bonds only

Ionic and nonpolar hydrogen bonds

Both polar covalent and hydrogen bonds

82. 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

83. Maximum hydrogen bonds in water are,

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

Both are equal

Cannot be determined

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

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

60°

120°

90°

109°

87. 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¯³⁵ m

6.63 x 10¯³³ m

6.65 x 10¯³⁵ m

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

First increases then decreases

Increases

Decreases

First decreases then increases

89. Choose the correct statement about 2nd ionization energy

It is equal to the 1st ionization energy

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

It is always greater than 1st ionization energy

It is always less than 1st ionization energy

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

Electronegativity

Electron affinity

Activation energy

Ionization potential

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

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

NaCl

H₂O

CH₄

CHCl₃

93. Pick out the molecule which has zero dipole moment

SO₂

H₂O

NH₃

BCl₃

94. Hydrogen chloride molecule contains

Co-ordinate bond

Covalent bond

Electrovalent bond

Double bond

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

96. Energy of an atom in a compound is

Lesser than individual

Higher than individual

No change

Impossible to predict

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

Ea.

E.N

E.A

I.P

98. Which carbon is more electronegative?

sp³-hybridized carbon

sp²- hybridized carbon

always same irrespective of its hybrid state

sp- hybridized carbon

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

H₂O

NH₃

BrF₃

BF₃

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

Distorted tetrahedral

Octahedral

Linear

Planar triangle

Page 5 of 8

101. Lewis acids are

Electron deficient

Octet is complete

No such acids exist

Electron rich

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

He⁺

Li⁺

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

None of these

Electron affinity

Electro negativity

Ionization energy

104. 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

Low ionization energy of sodium

Sublimation of metallic sodium to give yellow vapour

105. Fluorine molecule is formed by

The axial s-p overlap

The axial p-p overlap

The sidewise p-p overlap

The overlap of two sp² hybrid orbitals

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

Calcium

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

Decreases

Variable trend

Constant

Increases

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

Impossible to predict

2 n

3 n

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

Pcl₄

CH₄

N⁺H₄

PCl₃

110. Number of π-bonds in naphthalene is

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

SP²

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

3 lone pair 1 bond pair

2 bond pair 2 lone pair

1 bond pair 3 lone pair

3 bond pair one lone pair

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

None of these

Ionization energy

Electro negativity

Electron affinity

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

They have completely filled s and p orbitals

They do not react with one another

They are mono atomic gases

They have high ionization energies

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

N₂

He₂

PCl₅

SO₂

116. 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?

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

Atomic size

Ionization energy

Electronegativity

Electron affinity

118. 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

Both A and B are correct

None of these

119. 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

p orbitals

sp² hybrid orbitals

s orbitals

120. Molecular orbital picture of N₂ indicates

None of these

No unpaired electron

Two unpaired electron

One unpaired electron

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

Cube

Tetrahedron

Prism

Hexagon

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

Water should be preferred over lemon Juice for drinking

There may be a possibility of a chemical reaction

Lemon juice is dangerous for health

There may not be a possibility of chemical reaction

123. 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

X – radiation, visible, infrared, microwave

Radio, visible, infrared, ultraviolet

124. ____________ has their outermost shell complete in atomic form

Gun metals

Coinage metals

Alkali metals

Noble gases

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

They are smaller than the atoms from which they were formed

They are larger than the atoms from which they were formed

They are formed when electros are formed from atoms

They are also known as cations

Page 6 of 8

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

K⁺

S¯²

Cl¯

Na⁺

127. 1 erg of energy corresponds to

1 erg/mol

6.02 x 10²³ J/mol

10¯⁷ J/mol

6.02 x 10¹⁶ J/mol

128. H-bonding is not present in

Glycerine

Hydrogen sulphide

Hydrogen fluoride

Water

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

Electronegative character of elements

Pauli exclusion principle

Octet rule

Electropositive character of elements

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

0….5

5….0

5….1

1….5

131. Which has the minimum bond angle?

H₂S

CH₄

H₂O

NH₃

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

Ionization energy

None of these

Electron affinity

Electronegativity

133. 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

10.2340178

10.234

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

Chromium

Copper

Iron

Nickel

135. Anti-bonding MO is formed by

Subtraction of atomic orbitals

None of these

Multiplication of atomic orbitals

Addition of atomic orbitals

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

HBr

HCI

H2O

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

Three sigma bonds

Three pi-bonds

One sigma bond and two pi-bonds

Two sigma bonds and one pi-bond

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

139. Unit of dipole moment is

Pascal

Debye

Newton

Poise

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

Move with speed as that of light

Can be deflected by magnetic fields

Charged particles

A stream of electrons

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

5.9 BM

6.9 BM

3.0 BM

4.9 BM

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

3 and 9

3 and 5

3 and 7

2 and 5

143. Which of these molecules require more bond energy?

Hydrogen

Nitrogen

Oxygen

144. Which of the following species is paramagnetic?

CN¯

O²¯

CO₂

145. Molecular orbitals are filled according to

All these

Aufbau principal

Pauli’s exclusion principle

Hund’s rule

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

Fluorides is more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides are more electronegative

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

Lone pair – lone pair repulsion only

Bond pair – bond pair repulsion only

Lone pair – bond pair repulsion only

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

148. Inter molecular forces in solid hydrogen are

Hydrogen bonds

Covalent forces

Van der Waal forces or London dispersion forces

All of these

149. Geometry of simple molecule having SP³ hybrid orbital is

Square planner

Triangular

Linear

Tetrahedral

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

Trigonal

Tetrahedral

Pyramidal

Triangular

Page 7 of 8

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

XY₂

X₂Y

X₂Y₃

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

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

Liquid NH3

Liquid HCl

Water

Phenol

154. Nuclear radiation is emitted by those elements whose

Nuclei are unstable

Molecules are stable

Nuclei are stable

Molecules are unstable

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

2, 1, 0

3, 2, 1

2, 1, 1

3, 1, 1

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

Trigonal bipyramidal

Planar

Angular

Pyramidal

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

Greater than 1.7

Equal to 1.7

Lesser then 1.7

No specificity exist

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

H₂O

CH₄

BH₃

NH₃

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

4 electrons

6 electrons

1 electron

2 electrons

160. Ionic radius in a period from left to right

First increases then decreases

Increases

Decreases

First decreases then increases

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

SF₄

SiF₄

XeF₄

BF₃

162. The boiling point of heavy water is

99°C

101.4°C

108°C

110°C

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

All these

Electron

Neutron

Proton

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

165. Along a period the atomic radii

Increases

Constant

Decreases

First decreases then increases

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

107.5

109.5

104.5

102

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

AlCl₃

SiCl₄

MgCl₂

NaCl

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

NH₄Cl

H₂O₂

HCN

CH₄

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

HBr

HCl

H₂O

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

3, 10

10, 3

9, 4

4, 9

171. The nature of positive rays depends upon

The nature of electrode

The nature of residual gas

All of these

The nature of discharge tube

172. In O2 each oxygen atom is hybridized

All

Sp3

Sp2

173. XeF₄ has shape of

Square planar

Tetrahedral

Trigonal bipyramidal

Sphere

174. Effective magnetic moment of Sc³ ion is

1.73

5.92

2.83

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

Lesser

No effect

Remain same

Greater

Page 8 of 8

176. Quantum umber values for 2p orbitals are

n = 1, l = 0

n = 1, l = 2

n = 2, l = 0

n = 2, l = 1

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

Fourth Bohr orbit to the first Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

178. Geometry of simple molecule having sp3 hybrid orbital is

Square planner

Linear

Triangular

Tetrahedral

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

180. 2nd orbit is away from nucleus for H-atom as compared to first orbit

6-times

4-times

2-times

3-times

181. 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

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

12 and 4

12 and 5

16 and 5

16 and 4

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Maan AliLast Updated: April 19, 2025

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