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MDCAT Chemistry Chemical Bonding Test Online

Malik TahirLast Updated: May 24, 2025

Chemistry Chemical Bonding MCQS Online Test

MDCAT 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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MDCAT Chemistry Chemical Bonding Test

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Page 1 of 8

Chemistry

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

Greater than 1.7

No specificity exist

Lesser then 1.7

Equal to 1.7

2. Geometry of simple molecule having SP³ hybrid orbital is

Square planner

Linear

Tetrahedral

Triangular

3. 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

0.656 nm

656 nm

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

Ni³⁺

Fe²⁺

Cu⁺

Zn⁺

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

6.9 BM

5.9 BM

4.9 BM

3.0 BM

6. 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

7. 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

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

9. 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

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

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

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

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

None of these

Ionization energy

Electro negativity

Electron affinity

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

Lone pair – bond pair repulsion only

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

Lone pair – lone pair repulsion only

Bond pair – bond pair repulsion only

13. 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 4

16 and 5

12 and 4

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

London force

Chemical bond

Van der Waal’s force

Dispersion force

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

He⁺

Li⁺

16. The shape of the molecule SF₂Cl₂ is

Cubic

Tetrahedral

Trigonal bipyramidal

Octahedral

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

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

Low ionization energy of sodium

Sublimation of metallic sodium to give yellow vapour

Photosensitivity of sodium

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

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

Three sigma bonds

Two sigma bonds and one pi-bond

One sigma bond and two pi-bonds

Three pi-bonds

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

Li⁺

He⁺

21. Effective magnetic moment of Sc³ ion is

2.83

1.73

5.92

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

Ge, Sn

Se, Te

As, Sb

In, Pt

23. Which of the solid does not contain covalent bond

Graphite

Ice

Copper

Diamond

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

Planar

Angular

Trigonal bipyramidal

Pyramidal

25. Al become isoelectronic with Ne

By losing three electrons

By gaining two electrons

By gaining three electrons

By losing two electrons

Page 2 of 8

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

H – OH

H – NH₂

H – Cl

H – SH

27. 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

Covalent attraction

Hydrogen bond formation

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

2, 8

2, 9

2, 6

2, 10

29. Molecular orbital picture of N₂ indicates

Two unpaired electron

No unpaired electron

None of these

One unpaired electron

30. Nuclear radiation is emitted by those elements whose

Nuclei are unstable

Molecules are unstable

Molecules are stable

Nuclei are stable

31. Bohr’s model atom is contradicted by

Quarternization of angular members

Quarternization of energy of electrons

Plank’s quantum theory

Heisenberg’s uncertainty principle

32. 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⁺

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

34. 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

s orbitals

p orbitals

sp² hybrid orbitals

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

Trigonal

Triangular

Tetrahedral

Pyramidal

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

Lemon juice is dangerous for health

Water should be preferred over lemon Juice for drinking

There may not be a possibility of chemical reaction

There may be a possibility of a chemical reaction

37. Number of π-bonds in naphthalene is

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

2 n

3 n

Impossible to predict

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

Linear geometry

None

SP hybridization

Dipole moment is zero

40. Which of the following species is paramagnetic?

CN¯

O²¯

CO₂

41. 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

42. Which of these molecules require more bond energy?

Nitrogen

Hydrogen

Oxygen

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

Tetrahedral

Planar triangle

Square planar

Pyramidal

44. Bond angle in water is

104.5°

107°

120°

109.5°

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

Oxygen

Nitrogen

Helium

Hydrogen

46. The shape of H₃O⁺ is

Angular

Pyramidal

Tetrahedral

Triangular planar

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

6.02 x 10²³

9.1095 x 10¯³¹

1.7588 x 10²⁰

1.7588 x 10¹¹

48. Energy of an atom in a compound is

Impossible to predict

No change

Higher than individual

Lesser than individual

49. 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

50. Which one of these is weakest?

Van der Waal’s forces

Covalent bond

Metallic bond

Ionic bond

Page 3 of 8

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

Octahedral

Planar triangle

Linear

Distorted tetrahedral

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

Copper

Iron

Chromium

Nickel

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

54. Ionic radius in a period from left to right

First decreases then increases

Decreases

Increases

First increases then decreases

55. In O2 each oxygen atom is hybridized

All

Sp2

Sp3

56. 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

2 and 5

3 and 9

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

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

Increases

Remains constant

Decreases

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

SiCl₄

NaCl

MgCl₂

AlCl₃

59. Lateral overlapping expected in

O-bond

Ā-bonds

Metallic bond

Ionic bond

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

61. The structure of ICl₂¯ is

Trigonal

Octahedral

Trigonal bipyramidal

Square planar

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

XeF₄

SiF₄

BF₃

SF₄

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

Two sigma, one pi

Two sigma, two pi

One sigma, one pi

One sigma, two pi

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

Ionic and nonpolar hydrogen bonds

Both polar covalent and hydrogen bonds

Hydrogen bonds only

Nonpolar covalent bonds only

65. Maximum hydrogen bonds in water are,

66. Unit of dipole moment is

Debye

Pascal

Poise

Newton

67. 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

Fourth Bohr orbit to the first Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

Seventh Bohr orbit to the third Bohr orbit

68. The number of significant figures in 0.00200 is

Five

One

Three

Two

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

3, 10

10, 3

9, 4

4, 9

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

Boron trifluoride is pyramidal in shape while NH₃ is planar

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides is more electronegative

Fluorides are more electronegative

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

72. Shape of CIO₃¯ is

Triangular pyramidal

Tetrahedral

Triangular planar

Triangular bipyramidal

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

74. Deflection of blue light is lesser than violet because

Blue has higher wavelength

Blue is absorbed more easily

Blue has more energy

Blue is darker colour

75. Electronic configuration of K is

[AR]4S²

[He]4S¹

[Kr]4S¹

[AR]4S¹

Page 4 of 8

76. The boiling point of heavy water is

108°C

110°C

99°C

101.4°C

77. 2nd orbit is away from nucleus for H-atom as compared to first orbit

3-times

4-times

2-times

6-times

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

Na⁺

Cl¯

S¯²

K⁺

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

H₂O

HBr

HCl

80. 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

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

Excited state of neon

Ground state of fluorine atom

Excited state of O¯₂

Excited state of fluorine

82. Inter molecular forces in solid hydrogen are

Van der Waal forces or London dispersion forces

Covalent forces

All of these

Hydrogen bonds

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

SO₂

PCl₅

N₂

He₂

84. Which of the following has unchanged valency?

Oxygen

85. Bond order for N2 molecule is

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

1/2 x ɜ₀

9 x ɜ₀

6 x ɜ₀

3 x ɜ₀

87. Lewis acids are

Electron deficient

Electron rich

Octet is complete

No such acids exist

88. Covalent compounds are soluble in

Polar solvents

All solvents

Non-polar solvents

Concentrated acids

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

N⁺H₄

Pcl₄

CH₄

PCl₃

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

Liquid HCl

Liquid NH3

Water

Phenol

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

It has high heat of dissociation

It has high electronegativity

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

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

92. 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

Distillation

Colour spectrum

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

HCI

H2O

HBr

94. The carbon atoms in calcium carbide are held by

2 sigma bonds

Ionic bonds

2 covalent, one co-ordinate bond

2π and one σ bond

95. 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 greater than in NO⁺

Bond length is unpredictable

Bond length in NO⁺ is equal to that in NO

96. Which of the following is not isoelectronic?

Mg²⁺

Cl¯

O²¯

Na⁺

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

6.63 x 10¯³⁵ m

6.63 x 10¯³⁴ m

6.65 x 10¯³⁵ m

6.63 x 10¯³³ m

98. The ionization energy

Generally increases from left to right in a period

Does not change in a period

Increase from top to bottom in a group

Does not change in a group

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

Stability lower then O₂

Three unpaired electrons

Diamagnetic character

Bond order of 2.5

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

CH₃Cl

H₂O

CCl₄

HCl

Page 5 of 8

101. Pick out the molecule which has zero dipole moment

H₂O

NH₃

SO₂

BCl₃

102. Which molecule is polar among the following?

Carbon tetrachloride

Carbon dioxide

Ethane

Methanol

103. 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

10.234

10.23

10.234017

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

105. Unit of dipole moment is

Poise

Newton

Debye

Pascal

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

1 electron

6 electrons

2 electrons

4 electrons

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

Dispersion force

H-bonding

Ion-dipole interaction

Dipole-dipole interaction

108. Anti-bonding MO is formed by

Multiplication of atomic orbitals

Subtraction of atomic orbitals

None of these

Addition of atomic orbitals

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

1 bond pair 3 lone pair

3 bond pair one lone pair

2 bond pair 2 lone pair

3 lone pair 1 bond pair

110. The velocity of photon is

Independent of its wavelength

Depends on its source

Depends on its wavelength

Equal to square

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

Eight σ and eight π

Nine σ and nine π

Five π and nine σ

Nine σ and seven π

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

H₂O

H₂Te

H₂S3

H₂O

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

CH₄

H₂O

BH₃

NH₃

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

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

E.A

E.N

I.P

Ea.

116. Which carbon is more electronegative?

sp³-hybridized carbon

always same irrespective of its hybrid state

sp²- hybridized carbon

sp- hybridized carbon

117. Colour of the glow produced 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

Depends on the gas used in the discharge tube

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

118. On sp3 hybridization

One p-orbital is involved

All p-orbitals are involved

Four p-orbitals are involved

One s and 3 p-orbitals are involved

119. Molecular orbitals are filled according to

All these

Pauli’s exclusion principle

Aufbau principal

Hund’s rule

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

HCN

H₂O₂

CH₄

NH₄Cl

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

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

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

Electron

Proton

All these

Neutron

123. 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

124. Geometry of simple molecule having sp3 hybrid orbital is

Linear

Triangular

Tetrahedral

Square planner

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

The attractive forces dominate the repulsive forces

The repulsive force dominate the attractive forces

They energy of atoms increases

The two atoms start ionization

Page 6 of 8

126. 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?

127. XeF₄ has shape of

Square planar

Trigonal bipyramidal

Tetrahedral

Sphere

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

Activation energy

Electronegativity

Electron affinity

Ionization potential

129. 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

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

131. Hydrogen chloride molecule contains

Double bond

Electrovalent bond

Covalent bond

Co-ordinate bond

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

Visible, ultraviolet, infrared, gamma rays

Microwave, infrared, visible, ultraviolet

X – radiation, visible, infrared, microwave

Radio, visible, infrared, ultraviolet

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

They are larger than the atoms from which they were formed

They are also known as cations

They are smaller than the atoms from which they were formed

They are formed when electros are formed from atoms

134. Pi bonds are produced by overlapping of

Un-hybrid orbitals

Hybrid orbitals

Atomic orbital and hybrid orbital

Hybrid and un hybrid orbitals

135. Choose the correct statement

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

Each bonding molecular orbital can accommodate only one electron

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

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

136. Quantum umber values for 2p orbitals are

n = 2, l = 0

n = 2, l = 1

n = 1, l = 0

n = 1, l = 2

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

SP²

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

HCl

HBr

139. Fluorine molecule is formed by

The axial s-p overlap

The sidewise p-p overlap

The overlap of two sp² hybrid orbitals

The axial p-p overlap

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

141. A lone pair of electrons in an atom implies

A pair of electrons involved in bonding

A pair of valence electrons not involved in bonding

A pair of electrons

A pair of valence electrons

142. Number of sigma bonds in P₄O₁₀ is

143. The nature of positive rays depends upon

The nature of electrode

The nature of discharge tube

All of these

The nature of residual gas

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

Cannot be determined

Both are equal

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

Variable trend

Constant

Increases

Decreases

146. ____________ has their outermost shell complete in atomic form

Coinage metals

Gun metals

Noble gases

Alkali metals

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

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

SP²

149. H-bonding is not present in

Glycerine

Hydrogen fluoride

Hydrogen sulphide

Water

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

Greater

Remain same

No effect

Lesser

Page 7 of 8

151. An oxygen atom has mass of

2.657 x 10¯²³ g

16g

5.316 x 10¯²³ g

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

They have completely filled s and p orbitals

They are mono atomic gases

They have high ionization energies

They do not react with one another

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

154. Which has the minimum bond angle?

NH₃

CH₄

H₂O

H₂S

155. Which of the following molecule has Ā bond

C₃H₆

O₂

NH₃

H₂O

156. Choose the correct statement about 2nd 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

It is always greater than 1st ionization energy

It is equal to the 1st ionization energy

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

Triangular

Trigonal bipyramidal

Square planner

Octahedral

158. 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

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

Water has higher molecular weight

Sulphure has high electronegativity than oxygen

Water molecules associate through hydrogen bonding

Hydrogen sulphide is a weak acid

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

Ionization energy

Electro negativity

None of these

Electron affinity

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

Larger wavelength

Shorter wavelength

Gamma rays

X-rays not produced

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

5….0

5….1

1….5

0….5

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

None of these

Low, positive or slightly negative

High, very negative

Low very negative

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

H₂O

BrF₃

BF₃

NH₃

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

166. When potassium metal is exposed to violet light

Ejection of some potassium atoms occurs

There is no effect

Ejection of electrons takes place

The absorption of electrons takes place

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

Electronegativity

Electron affinity

Atomic size

Ionization energy

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

Na and F

O and F

C and F

N and F

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

Interaction

Attractive force

Bond

All of above represent same entity

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

Calcium

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

Tetrahedron

Prism

Cube

Hexagon

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

Electropositive character of elements

Octet rule

Pauli exclusion principle

Electronegative character of elements

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

3, 2, 1

2, 1, 1

3, 1, 1

2, 1, 0

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

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

-13.6 eV

-5.44 eV

-54.4 eV

Zero

Page 8 of 8

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

90°

109°

120°

60°

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

4, 1, 1, ½

4, 1, 0, ½

4, 4, 0, ½

4, 0, 0, ½

178. Which of the following has zero depolemoment?

ClF

CFCl₃

SiF₄

PCl₃

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

Electronegativity

Ionization energy

Electron affinity

None of these

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

H₂O

NaCl

CH₄

CHCl₃

181. Along a period the atomic radii

Increases

Decreases

First decreases then increases

Constant

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

First increases then decreases

Increases

Decreases

First decreases then increases

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Malik TahirLast Updated: May 24, 2025

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Chemistry Chemical Bonding MCQS Online Test

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