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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 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⁺

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

Tetrahedral

Pyramidal

Triangular

Trigonal

3. XeF₄ has shape of

Square planar

Sphere

Tetrahedral

Trigonal bipyramidal

4. Pi bonds are produced by overlapping of

Atomic orbital and hybrid orbital

Hybrid and un hybrid orbitals

Hybrid orbitals

Un-hybrid orbitals

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

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

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

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

6 x ɜ₀

9 x ɜ₀

1/2 x ɜ₀

3 x ɜ₀

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

N⁺H₄

PCl₃

Pcl₄

CH₄

10. 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

11. The shape of the molecule SF₂Cl₂ is

Tetrahedral

Cubic

Octahedral

Trigonal bipyramidal

12. 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

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

HCI

HBr

H2O

14. Al become isoelectronic with Ne

By losing two electrons

By gaining three electrons

By losing three electrons

By gaining two electrons

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

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

Bond pair – bond pair repulsion only

Lone pair – lone pair repulsion only

Lone pair – bond pair repulsion only

16. Molecular orbital picture of N₂ indicates

One unpaired electron

None of these

No unpaired electron

Two unpaired electron

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

H₂O

H₂Te

H₂S3

H₂O

18. The boiling point of heavy water is

99°C

101.4°C

110°C

108°C

19. The nature of positive rays depends upon

All of these

The nature of electrode

The nature of discharge tube

The nature of residual gas

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

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

Nine σ and seven π

Five π and nine σ

Eight σ and eight π

Nine σ and nine π

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

Electron affinity

Ionization energy

None of these

Electronegativity

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

Li⁺

He⁺

24. A lone pair of electrons in an atom implies

A pair of electrons

A pair of electrons involved in bonding

A pair of valence electrons

A pair of valence electrons not involved in bonding

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

5….1

5….0

1….5

0….5

Page 2 of 8

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

None of these

Both A and B are correct

Orbital overlap will not occur

Bonding will not occur

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

28. Number of π-bonds in naphthalene is

29. Which molecule is polar among the following?

Ethane

Carbon tetrachloride

Carbon dioxide

Methanol

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

CH₄

HCN

NH₄Cl

H₂O₂

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

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

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

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

6.9 BM

3.0 BM

4.9 BM

5.9 BM

33. The structure of ICl₂¯ is

Trigonal bipyramidal

Square planar

Octahedral

Trigonal

34. 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

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

Each bonding molecular orbital can accommodate only one electron

35. Geometry of simple molecule having sp3 hybrid orbital is

Square planner

Linear

Tetrahedral

Triangular

36. Lateral overlapping expected in

Metallic bond

Ionic bond

O-bond

Ā-bonds

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

Fe²⁺

Ni³⁺

Cu⁺

Zn⁺

38. Ionic radius in a period from left to right

First decreases then increases

Increases

First increases then decreases

Decreases

39. Bond angle in water is

107°

104.5°

109.5°

120°

40. When potassium metal is exposed to violet light

Ejection of some potassium atoms occurs

The absorption of electrons takes place

Ejection of electrons takes place

There is no effect

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

HCl

HBr

H₂O

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

Increases

Variable trend

Decreases

Constant

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

None

Linear geometry

SP hybridization

Dipole moment is zero

44. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 1, l = 0

n = 2, l = 0

n = 1, l = 2

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

2, 1, 1

2, 1, 0

3, 2, 1

3, 1, 1

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

SO₂

He₂

N₂

PCl₅

47. Number of sigma bonds in P₄O₁₀ is

48. Along a period the atomic radii

Decreases

First decreases then increases

Increases

Constant

49. 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

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

4, 1, 0, ½

4, 4, 0, ½

4, 1, 1, ½

4, 0, 0, ½

Page 3 of 8

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

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

Angular

Pyramidal

Trigonal bipyramidal

Planar

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

Ion-dipole interaction

Dipole-dipole interaction

H-bonding

Dispersion force

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

CH₃Cl

HCl

CCl₄

H₂O

55. Nuclear radiation is emitted by those elements whose

Nuclei are unstable

Molecules are stable

Nuclei are stable

Molecules are unstable

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

BF₃

XeF₄

SF₄

SiF₄

57. 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

58. Which of the following has zero depolemoment?

SiF₄

ClF

CFCl₃

PCl₃

59. 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

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

O and F

Na and F

C and F

N and F

61. 2nd orbit is away from nucleus for H-atom as compared to first orbit

2-times

4-times

6-times

3-times

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

6.63 x 10¯³⁴ m

6.65 x 10¯³⁵ m

6.63 x 10¯³⁵ m

6.63 x 10¯³³ m

63. The energy of a photon is given as, ∆ E/atom = 3.03 x 10¯¹⁹ J atom¯¹ then, the wavelength (λ) of the photon is

6.56 nm

656 nm

65.6 nm

0.656 nm

64. In O2 each oxygen atom is hybridized

All

Sp2

Sp3

65. 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

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

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

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

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

Na⁺

S¯²

Cl¯

K⁺

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

There may be a possibility of a chemical reaction

Lemon juice is dangerous for health

There may not be a possibility of chemical reaction

Water should be preferred over lemon Juice for drinking

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

Bond

Interaction

Attractive force

All of above represent same entity

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

Ge, Sn

Se, Te

In, Pt

As, Sb

70. Inter molecular forces in solid hydrogen are

Hydrogen bonds

Covalent forces

All of these

Van der Waal forces or London dispersion forces

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

9.1095 x 10¯³¹

1.7588 x 10¹¹

6.02 x 10²³

1.7588 x 10²⁰

72. Geometry of simple molecule having SP³ hybrid orbital is

Tetrahedral

Linear

Square planner

Triangular

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

3 and 7

3 and 5

3 and 9

2 and 5

74. The shape of H₃O⁺ is

Angular

Tetrahedral

Triangular planar

Pyramidal

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

BrF₃

H₂O

NH₃

BF₃

Page 4 of 8

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

MgCl₂

NaCl

SiCl₄

AlCl₃

77. Shape of CIO₃¯ is

Triangular planar

Tetrahedral

Triangular pyramidal

Triangular bipyramidal

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

Ionic and nonpolar hydrogen bonds

Hydrogen bonds only

Nonpolar covalent bonds only

Both polar covalent and hydrogen bonds

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

They do not react with one another

They are mono atomic gases

They have high ionization energies

They have completely filled s and p orbitals

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

None of these

Ionization energy

Electro negativity

Electron affinity

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

Activation energy

Ionization potential

Electron affinity

Electronegativity

82. Bond order for N2 molecule is

83. Pick out the molecule which has zero dipole moment

SO₂

BCl₃

NH₃

H₂O

84. Unit of dipole moment is

Newton

Debye

Poise

Pascal

85. 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

16 and 5

12 and 5

16 and 4

86. 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

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

H – Cl

H – NH₂

H – SH

H – OH

88. Which of the following has unchanged valency?

Oxygen

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

Hydrogen

Nitrogen

Oxygen

Helium

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

HCl

HBr

91. Unit of dipole moment is

Newton

Poise

Pascal

Debye

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

X-rays not produced

Larger wavelength

Gamma rays

Shorter wavelength

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

Ionization energy

Atomic size

Electronegativity

Electron affinity

94. 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?

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

SP²

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

97. Energy of an atom in a compound is

Higher than individual

No change

Lesser than individual

Impossible to predict

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

London force

Dispersion force

Van der Waal’s force

Chemical bond

99. 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

100. 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

Page 5 of 8

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

Nickel

Iron

Copper

Chromium

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

NH₃

CH₄

H₂O

BH₃

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

104. 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

105. Effective magnetic moment of Sc³ ion is

1.73

2.83

5.92

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

107. The bond order in NO is 2.5 while that is NO⁺ is 3. Which of the following statements is true for these two species?

Bond length is unpredictable

Bond length in NO is greater than in NO⁺

Bond length in NO⁺ is equal to that in NO

Bond length in NO⁺ is greater than in NO

108. 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

Dipole interaction

Van der Waal’s forces

Covalent attraction

109. 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

110. The carbon atoms in calcium carbide are held by

2 sigma bonds

2 covalent, one co-ordinate bond

Ionic bonds

2π and one σ bond

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

None of these

Ionization energy

Electro negativity

Electron affinity

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

4, 9

10, 3

3, 10

9, 4

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

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

2, 9

2, 8

2, 6

2, 10

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

Planar triangle

Octahedral

Distorted tetrahedral

Linear

116. 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 smaller than the atoms from which they were formed

They are larger than the atoms from which they were formed

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

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

Lesser

No effect

Greater

Remain same

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

Cannot be determined

Both are equal

120. Lewis acids are

Electron rich

Electron deficient

No such acids exist

Octet is complete

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

122. 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

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

Visible, ultraviolet, infrared, gamma rays

X – radiation, visible, infrared, microwave

Microwave, infrared, visible, ultraviolet

Radio, visible, infrared, ultraviolet

124. The velocity of photon is

Equal to square

Depends on its source

Independent of its wavelength

Depends on its wavelength

125. 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

Page 6 of 8

126. Fluorine molecule is formed by

The axial p-p overlap

The overlap of two sp² hybrid orbitals

The sidewise p-p overlap

The axial s-p overlap

127. 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

128. Which carbon is more electronegative?

sp- hybridized carbon

sp³-hybridized carbon

always same irrespective of its hybrid state

sp²- hybridized carbon

129. The ionization energy

Does not change in a group

Generally increases from left to right in a period

Increase from top to bottom in a group

Does not change in a period

130. Choose the correct statement about 2nd ionization energy

It is always less than 1st ionization energy

It is always greater than 1st ionization energy

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

It is equal to the 1st ionization energy

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

Bond order of 2.5

Diamagnetic character

Three unpaired electrons

Stability lower then O₂

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

120°

60°

109°

90°

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

134. Maximum hydrogen bonds in water are,

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

He⁺

Li⁺

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

It has high electronegativity

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 heat of dissociation

137. Which of the following species is paramagnetic?

O²¯

CO₂

CN¯

138. Hydrogen chloride molecule contains

Double bond

Electrovalent bond

Co-ordinate bond

Covalent bond

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

Increases

Decreases

First decreases then increases

First increases then decreases

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

141. 1 erg of energy corresponds to

1 erg/mol

10¯⁷ J/mol

6.02 x 10¹⁶ J/mol

6.02 x 10²³ J/mol

142. The number of significant figures in 0.00200 is

Two

Three

Five

One

143. 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

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

145. Bohr’s model atom is contradicted by

Plank’s quantum theory

Quarternization of angular members

Quarternization of energy of electrons

Heisenberg’s uncertainty principle

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

147. Anti-bonding MO is formed by

Addition of atomic orbitals

Subtraction of atomic orbitals

Multiplication of atomic orbitals

None of these

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

Calcium

149. Covalent compounds are soluble in

Non-polar solvents

All solvents

Concentrated acids

Polar solvents

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

Move with speed as that of light

Can be deflected by magnetic fields

A stream of electrons

Charged particles

Page 7 of 8

151. Electronic configuration of K is

[AR]4S²

[AR]4S¹

[He]4S¹

[Kr]4S¹

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

Liquid HCl

Liquid NH3

Water

Phenol

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

6 electrons

2 electrons

1 electron

4 electrons

154. 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

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

Octahedral

Trigonal bipyramidal

Square planner

Triangular

156. Which has the minimum bond angle?

NH₃

H₂O

CH₄

H₂S

157. Which one of these is weakest?

Metallic bond

Covalent bond

Van der Waal’s forces

Ionic bond

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

They energy of atoms increases

The two atoms start ionization

The repulsive force dominate the attractive forces

The attractive forces dominate the repulsive forces

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

E.N

Ea.

E.A

I.P

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

Electropositive character of elements

Pauli exclusion principle

Octet rule

Electronegative character of elements

161. Which of the following is not isoelectronic?

O²¯

Na⁺

Mg²⁺

Cl¯

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

Proton

All these

Neutron

Electron

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

SP²

164. ____________ has their outermost shell complete in atomic form

Coinage metals

Gun metals

Alkali metals

Noble gases

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

CH₄

H₂O

NaCl

CHCl₃

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

Zero

-5.44 eV

-54.4 eV

-13.6 eV

167. Molecular orbitals are filled according to

Hund’s rule

All these

Pauli’s exclusion principle

Aufbau principal

168. H-bonding is not present in

Hydrogen fluoride

Glycerine

Hydrogen sulphide

Water

169. Which of the following molecule has Ā bond

C₃H₆

H₂O

NH₃

O₂

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

102

109.5

104.5

107.5

171. 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

-1.48

-1.11

-2.22

172. On sp3 hybridization

All p-orbitals are involved

One s and 3 p-orbitals are involved

Four p-orbitals are involved

One p-orbital is involved

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

Hexagon

Prism

Tetrahedron

Cube

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

2 n

Impossible to predict

3 n

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

Distillation

Colour spectrum

Vaporization

Crystallization

Page 8 of 8

176. 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

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

Seventh Bohr orbit to the third Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

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

Pyramidal

Tetrahedral

Planar triangle

Square planar

179. Which of the solid does not contain covalent bond

Ice

Copper

Graphite

Diamond

180. Which of these molecules require more bond energy?

Hydrogen

Oxygen

Nitrogen

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

Excited state of neon

Excited state of O¯₂

Excited state of fluorine

Ground state of fluorine atom

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

Fluorides is more electronegative

Fluorides are more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Boron trifluoride is pyramidal in shape while NH₃ is planar

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Maan AliLast Updated: April 19, 2025

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