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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. Nuclear radiation is emitted by those elements whose

Molecules are stable

Nuclei are unstable

Nuclei are stable

Molecules are unstable

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

N₂

He₂

PCl₅

SO₂

3. 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 – bond pair repulsion only

Lone pair – lone pair repulsion only

4. 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

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

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

SP²

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

8. Which of the solid does not contain covalent bond

Diamond

Ice

Copper

Graphite

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

SP²

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

Gamma rays

Larger wavelength

X-rays not produced

Shorter wavelength

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

HBr

HCl

12. Choose the correct statement

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

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

Each bonding molecular orbital can accommodate only one electron

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

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

CCl₄

CH₃Cl

HCl

H₂O

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

Electro negativity

Electron affinity

Ionization energy

None of these

15. The structure of ICl₂¯ is

Trigonal

Octahedral

Trigonal bipyramidal

Square planar

16. 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

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

Ionization potential

Activation energy

Electron affinity

Electronegativity

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

Two sigma bonds and one pi-bond

One sigma bond and two pi-bonds

Three sigma bonds

Three pi-bonds

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¯³⁵ m

6.65 x 10¯³⁵ m

6.63 x 10¯³³ m

20. 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

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

Copper

Nickel

Iron

Chromium

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

Liquid HCl

Liquid NH3

Water

Phenol

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

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

25. The shape of the molecule SF₂Cl₂ is

Cubic

Trigonal bipyramidal

Tetrahedral

Octahedral

Page 2 of 8

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

Constant

Variable trend

Increases

Decreases

27. The shape of H₃O⁺ is

Triangular planar

Angular

Tetrahedral

Pyramidal

28. 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

Fifth Bohr orbit to the second Bohr orbit

Fourth Bohr orbit to the first Bohr orbit

Sixth Bohr orbit to the third Bohr orbit

29. 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

XY₂

X₂Y₃

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

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

It has high heat of dissociation

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

It has high electronegativity

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

2 and 5

3 and 9

3 and 5

3 and 7

32. Covalent compounds are soluble in

Polar solvents

Concentrated acids

All solvents

Non-polar solvents

33. Electronic configuration of K is

[AR]4S¹

[AR]4S²

[He]4S¹

[Kr]4S¹

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

5….0

5….1

1….5

0….5

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

Chemical bond

Dispersion force

Van der Waal’s force

London force

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

37. Along a period the atomic radii

Increases

Constant

First decreases then increases

Decreases

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

Fluorides are more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

Fluorides is more electronegative

Boron trifluoride is pyramidal in shape while NH₃ is planar

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

40. 2nd orbit is away from nucleus for H-atom as compared to first orbit

2-times

4-times

6-times

3-times

41. H-bonding is not present in

Hydrogen sulphide

Water

Glycerine

Hydrogen fluoride

42. 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⁺

43. Number of π-bonds in naphthalene is

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

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

Hydrogen bonds only

Both polar covalent and hydrogen bonds

Ionic and nonpolar hydrogen bonds

Nonpolar covalent bonds only

46. The carbon atoms in calcium carbide are held by

2π and one σ bond

Ionic bonds

2 sigma bonds

2 covalent, one co-ordinate bond

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

BH₃

CH₄

H₂O

NH₃

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

H₂O

CHCl₃

CH₄

NaCl

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

H₂O

HCl

HBr

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

Hydrogen

Oxygen

Nitrogen

Helium

Page 3 of 8

51. Geometry of simple molecule having SP³ hybrid orbital is

Square planner

Triangular

Linear

Tetrahedral

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

Fe²⁺

Cu⁺

Ni³⁺

Zn⁺

53. 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?

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

Prism

Tetrahedron

Hexagon

Cube

55. Inter molecular forces in solid hydrogen are

Covalent forces

Van der Waal forces or London dispersion forces

All of these

Hydrogen bonds

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

Two sigma, two pi

One sigma, one pi

Two sigma, one pi

One sigma, two pi

57. Which of the following has unchanged valency?

Oxygen

58. The number of significant figures in 0.00200 is

One

Five

Three

Two

59. Maximum hydrogen bonds in water are,

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

61. Which of the following has zero depolemoment?

CFCl₃

PCl₃

ClF

SiF₄

62. In O2 each oxygen atom is hybridized

Sp2

Sp3

All

63. 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?

-2.22

-1.48

-2.96

-1.11

64. Bond angle in water is

120°

104.5°

107°

109.5°

65. 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……

sp² hybrid orbitals

p orbitals

sp³ hybrid orbitals

s orbitals

66. 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

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

None of these

Ionization energy

Electron affinity

Electronegativity

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

Neutron

All these

Proton

Electron

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

1 electron

2 electrons

4 electrons

6 electrons

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

Na⁺

K⁺

Cl¯

S¯²

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

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

H2O

HCI

HBr

73. 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

74. Choose the correct statement about 2nd ionization energy

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

It is always greater than 1st ionization energy

It is equal to the 1st ionization energy

It is always less than 1st ionization energy

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

Hydrogen sulphide is a weak acid

Sulphure has high electronegativity than oxygen

Water molecules associate through hydrogen bonding

Water has higher molecular weight

Page 4 of 8

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

2 n

Impossible to predict

3 n

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

NH₄Cl

HCN

CH₄

H₂O₂

78. 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

104.5

102

109.5

79. Molecular orbital picture of N₂ indicates

One unpaired electron

Two unpaired electron

None of these

No unpaired electron

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

Electron affinity

None of these

Electro negativity

Ionization energy

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

82. On sp3 hybridization

One s and 3 p-orbitals are involved

One p-orbital is involved

All p-orbitals are involved

Four p-orbitals are involved

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

Dispersion force

Ion-dipole interaction

H-bonding

Dipole-dipole interaction

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

Calcium

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

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

I.P

Ea.

E.A

E.N

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

In, Pt

Ge, Sn

Se, Te

As, Sb

88. 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

89. An oxygen atom has mass of

5.316 x 10¯²³ g

16g

5.316 x 10¯²³ g

2.657 x 10¯²³ g

90. Lateral overlapping expected in

Metallic bond

Ionic bond

O-bond

Ā-bonds

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

Li⁺

He⁺

92. 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

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

CH₄

PCl₃

Pcl₄

N⁺H₄

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

-13.6 eV

Zero

-54.4 eV

-5.44 eV

95. Effective magnetic moment of Sc³ ion is

1.73

5.92

2.83

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

Lesser

Remain same

No effect

Greater

97. Unit of dipole moment is

Poise

Debye

Newton

Pascal

98. 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

99. 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

0.656 nm

6.56 nm

65.6 nm

656 nm

100. 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 5 of 8

101. Which of the following is not isoelectronic?

Mg²⁺

O²¯

Cl¯

Na⁺

102. Which one of these is weakest?

Van der Waal’s forces

Metallic bond

Covalent bond

Ionic bond

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

Octahedral

Planar triangle

Linear

Distorted tetrahedral

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

There may be a possibility of a chemical reaction

Water should be preferred over lemon Juice for drinking

Lemon juice is dangerous for health

There may not be a possibility of chemical reaction

105. Bohr’s model atom is contradicted by

Plank’s quantum theory

Quarternization of angular members

Quarternization of energy of electrons

Heisenberg’s uncertainty principle

106. 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

16 and 4

12 and 5

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

10, 3

4, 9

9, 4

3, 10

108. Anti-bonding MO is formed by

Addition of atomic orbitals

None of these

Subtraction of atomic orbitals

Multiplication of atomic orbitals

109. Geometry of simple molecule having sp3 hybrid orbital is

Linear

Tetrahedral

Triangular

Square planner

110. Pick out the molecule which has zero dipole moment

SO₂

NH₃

BCl₃

H₂O

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

BF₃

H₂O

NH₃

BrF₃

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

The two atoms start ionization

They energy of atoms increases

The attractive forces dominate the repulsive forces

The repulsive force dominate the attractive forces

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

Trigonal bipyramidal

Triangular

Square planner

Octahedral

114. Which carbon is more electronegative?

always same irrespective of its hybrid state

sp- hybridized carbon

sp³-hybridized carbon

sp²- hybridized carbon

115. Which has the minimum bond angle?

NH₃

CH₄

H₂O

H₂S

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

They have high ionization energies

They do not react with one another

They are mono atomic gases

They have completely filled s and p orbitals

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

Both are equal

Cannot be determined

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

BF₃

XeF₄

SiF₄

SF₄

119. XeF₄ has shape of

Square planar

Trigonal bipyramidal

Tetrahedral

Sphere

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

Equal to 1.7

Greater than 1.7

No specificity exist

Lesser then 1.7

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

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

Tetrahedral

Planar triangle

Pyramidal

Square planar

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

124. Pi bonds are produced by overlapping of

Hybrid and un hybrid orbitals

Un-hybrid orbitals

Hybrid orbitals

Atomic orbital and hybrid orbital

125. Which of the following molecule has Ā bond

H₂O

NH₃

C₃H₆

O₂

Page 6 of 8

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

SiCl₄

MgCl₂

AlCl₃

NaCl

127. 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

128. Which of the following species is paramagnetic?

O²¯

CN¯

CO₂

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

Octet rule

Electronegative character of elements

Electropositive character of elements

Pauli exclusion principle

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

60°

120°

90°

109°

131. Which molecule is polar among the following?

Carbon tetrachloride

Carbon dioxide

Ethane

Methanol

132. Energy of an atom in a compound is

Higher than individual

Impossible to predict

Lesser than individual

No change

133. Quantum umber values for 2p orbitals are

n = 2, l = 1

n = 1, l = 2

n = 1, l = 0

n = 2, l = 0

134. Which of these molecules require more bond energy?

Hydrogen

Nitrogen

Oxygen

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

136. Hydrogen chloride molecule contains

Double bond

Electrovalent bond

Co-ordinate bond

Covalent bond

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

They are smaller than the atoms from which they were formed

They are formed when electros are formed from atoms

They are larger than the atoms from which they were formed

They are also known as cations

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

2, 10

2, 6

2, 9

2, 8

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

H – SH

H – NH₂

H – OH

H – Cl

140. A lone pair of electrons in an atom implies

A pair of valence electrons

A pair of electrons

A pair of electrons involved in bonding

A pair of valence electrons not involved in bonding

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

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

142. 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 is unpredictable

Bond length in NO⁺ is equal to that in NO

Bond length in NO is greater than in NO⁺

143. ____________ has their outermost shell complete in atomic form

Gun metals

Coinage metals

Noble gases

Alkali metals

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

Microwave, infrared, visible, ultraviolet

Radio, visible, infrared, ultraviolet

X – radiation, visible, infrared, microwave

Visible, ultraviolet, infrared, gamma rays

145. The nature of positive rays depends upon

The nature of residual gas

All of these

The nature of electrode

The nature of discharge tube

146. Ionic radius in a period from left to right

Increases

First increases then decreases

Decreases

First decreases then increases

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

Nine σ and nine π

Nine σ and seven π

Eight σ and eight π

Five π and nine σ

148. The boiling point of heavy water is

108°C

101.4°C

110°C

99°C

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

Orbital overlap will not occur

Bonding will not occur

None of these

Both A and B are correct

150. The ionization energy

Generally increases from left to right in a period

Does not change in a period

Does not change in a group

Increase from top to bottom in a group

Page 7 of 8

151. When potassium metal is exposed to violet light

There is no effect

Ejection of some potassium atoms occurs

The absorption of electrons takes place

Ejection of electrons takes place

152. Number of sigma bonds in P₄O₁₀ is

153. Lewis acids are

No such acids exist

Electron deficient

Octet is complete

Electron rich

154. Bond order for N2 molecule is

155. 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

156. Molecular orbitals are filled according to

Pauli’s exclusion principle

Aufbau principal

Hund’s rule

All these

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

Diamagnetic character

Bond order of 2.5

Three unpaired electrons

Stability lower then O₂

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

5.9 BM

3.0 BM

6.9 BM

4.9 BM

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

Trigonal bipyramidal

Pyramidal

Planar

Angular

160. Deflection of blue light is lesser than violet because

Blue has more energy

Blue is darker colour

Blue has higher wavelength

Blue is absorbed more easily

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

First decreases then increases

Increases

First increases then decreases

Decreases

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

Li⁺

He⁺

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

N and F

Na and F

O and F

C and F

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

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

SP hybridization

None

Linear geometry

Dipole moment is zero

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

4, 1, 0, ½

4, 0, 0, ½

4, 4, 0, ½

4, 1, 1, ½

167. 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

10.234

10.234017

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

All of above represent same entity

Interaction

Attractive force

Bond

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

H₂S3

H₂Te

H₂O

170. 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

Covalent attraction

Hydrogen bond formation

Dipole interaction

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

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

Tetrahedral

Trigonal

Pyramidal

Triangular

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

Excited state of neon

Excited state of O¯₂

Ground state of fluorine atom

Excited state of fluorine

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

Remains constant

Increases

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

Decreases

175. Unit of dipole moment is

Poise

Pascal

Debye

Newton

Page 8 of 8

176. Fluorine molecule is formed by

The sidewise p-p overlap

The overlap of two sp² hybrid orbitals

The axial p-p overlap

The axial s-p overlap

177. 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

178. Al become isoelectronic with Ne

By gaining two electrons

By losing two electrons

By losing three electrons

By gaining three electrons

179. The velocity of photon is

Equal to square

Depends on its wavelength

Depends on its source

Independent of its wavelength

180. Shape of CIO₃¯ is

Triangular bipyramidal

Triangular planar

Triangular pyramidal

Tetrahedral

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

Ionization energy

Electron affinity

Atomic size

Electronegativity

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

Low very negative

None of these

Low, positive or slightly negative

High, very negative

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Malik TahirLast Updated: May 24, 2025

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