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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. Molecular orbitals are filled according to

Aufbau principal

Hund’s rule

Pauli’s exclusion principle

All these

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

Greater than 1.7

Equal to 1.7

No specificity exist

Lesser then 1.7

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

Water molecules associate through hydrogen bonding

Hydrogen sulphide is a weak acid

Water has higher molecular weight

Sulphure has high electronegativity than oxygen

4. Which carbon is more electronegative?

sp³-hybridized carbon

sp- hybridized carbon

always same irrespective of its hybrid state

sp²- hybridized carbon

5. 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

6. 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

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

8. 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

-2.22

-1.11

9. 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

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

Remain same

No effect

Lesser

Greater

11. Which of the following molecule has Ā bond

NH₃

C₃H₆

O₂

H₂O

12. Quantum umber values for 2p orbitals are

n = 1, l = 0

n = 1, l = 2

n = 2, l = 0

n = 2, l = 1

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

Distorted tetrahedral

Octahedral

Linear

Planar triangle

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

CH₄

H₂O

CHCl₃

NaCl

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

Nonpolar covalent bonds only

Both polar covalent and hydrogen bonds

Hydrogen bonds only

Ionic and nonpolar hydrogen bonds

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

Trigonal

Pyramidal

Tetrahedral

Triangular

17. 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

18. Which of the solid does not contain covalent bond

Ice

Diamond

Graphite

Copper

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

Ground state of fluorine atom

Excited state of O¯₂

Excited state of neon

Excited state of fluorine

20. Along a period the atomic radii

First decreases then increases

Constant

Decreases

Increases

21. 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

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

23. An oxygen atom has mass of

2.657 x 10¯²³ g

5.316 x 10¯²³ g

16g

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

25. Which of the following has zero depolemoment?

CFCl₃

ClF

PCl₃

SiF₄

Page 2 of 8

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

Se, Te

As, Sb

Ge, Sn

In, Pt

27. 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

3 x ɜ₀

6 x ɜ₀

28. Hydrogen chloride molecule contains

Electrovalent bond

Double bond

Co-ordinate bond

Covalent bond

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

Impossible to predict

3 n

2 n

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

BF₃

SF₄

XeF₄

SiF₄

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

He₂

PCl₅

N₂

SO₂

32. 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

33. Bond order for N2 molecule is

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

Fe²⁺

Ni³⁺

Cu⁺

Zn⁺

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

Linear geometry

Dipole moment is zero

None

SP hybridization

36. ____________ has their outermost shell complete in atomic form

Gun metals

Noble gases

Alkali metals

Coinage metals

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

Atomic size

Ionization energy

Electronegativity

Electron affinity

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

Ionization potential

Electron affinity

Activation energy

Electronegativity

39. 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

Radio, visible, infrared, ultraviolet

X – radiation, visible, infrared, microwave

40. The boiling point of heavy water is

99°C

110°C

101.4°C

108°C

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

Sublimation of metallic sodium to give yellow vapour

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

Low ionization energy of sodium

Photosensitivity of sodium

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

Dispersion force

Van der Waal’s force

Chemical bond

London force

43. Ionic radius in a period from left to right

Increases

Decreases

First decreases then increases

First increases then decreases

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

4, 9

3, 10

10, 3

9, 4

45. Electronic configuration of K is

[He]4S¹

[Kr]4S¹

[AR]4S¹

[AR]4S²

46. 2nd orbit is away from nucleus for H-atom as compared to first orbit

2-times

4-times

3-times

6-times

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

109°

90°

120°

60°

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

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

Triangular

Trigonal bipyramidal

Octahedral

Square planner

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

First decreases then increases

Decreases

First increases then decreases

Increases

Page 3 of 8

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

SP²

52. Shape of CIO₃¯ is

Triangular planar

Tetrahedral

Triangular pyramidal

Triangular bipyramidal

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

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

H – Cl

H – SH

H – NH₂

H – OH

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

N and F

Na and F

C and F

O and F

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

They are mono atomic gases

They have completely filled s and p orbitals

They do not react with one another

They have high ionization energies

57. Which of the following is not isoelectronic?

O²¯

Mg²⁺

Cl¯

Na⁺

58. Bond angle in water is

120°

107°

104.5°

109.5°

59. Covalent compounds are soluble in

All solvents

Concentrated acids

Non-polar solvents

Polar solvents

60. 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 electronegativity

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

It has high heat of dissociation

61. The structure of ICl₂¯ is

Trigonal

Square planar

Trigonal bipyramidal

Octahedral

62. 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

Fluorides are more electronegative

NH₃ is pyramidal in shape while BF₃ is planar

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

3 and 5

3 and 9

3 and 7

2 and 5

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

NH₃

H₂O

BH₃

CH₄

65. In O2 each oxygen atom is hybridized

All

Sp3

Sp2

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

67. Which one of these is weakest?

Metallic bond

Ionic bond

Covalent bond

Van der Waal’s forces

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

Cannot be determined

Both are equal

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

104.5

109.5

107.5

102

70. 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 equal to the 1st ionization energy

It is always less than 1st ionization energy

It is always greater than 1st ionization energy

71. 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 formed when electros are formed from atoms

They are smaller than the atoms from which they were formed

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

6.65 x 10¯³⁵ m

6.63 x 10¯³³ m

6.63 x 10¯³⁴ m

6.63 x 10¯³⁵ m

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

SiCl₄

AlCl₃

MgCl₂

NaCl

74. Maximum hydrogen bonds in water are,

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

Bond pair – bond pair repulsion only

Lone pair – bond pair repulsion only

Lone pair – lone pair repulsion only

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

Page 4 of 8

76. The velocity of photon is

Equal to square

Depends on its source

Independent of its wavelength

Depends on its wavelength

77. Which of the following species is paramagnetic?

CO₂

CN¯

O²¯

78. H-bonding is not present in

Glycerine

Water

Hydrogen fluoride

Hydrogen sulphide

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

PCl₃

CH₄

N⁺H₄

Pcl₄

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

Na⁺

S¯²

K⁺

Cl¯

81. Geometry of simple molecule having sp3 hybrid orbital is

Tetrahedral

Linear

Square planner

Triangular

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

HCl

HBr

83. Number of sigma bonds in P₄O₁₀ is

84. Which of these molecules require more bond energy?

Oxygen

Hydrogen

Nitrogen

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

All of above represent same entity

Interaction

Attractive force

Bond

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

9.1095 x 10¯³¹

6.02 x 10²³

1.7588 x 10¹¹

1.7588 x 10²⁰

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

88. 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

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

Depends on the gas used in the discharge tube

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

2, 6

2, 8

2, 9

2, 10

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

Gamma rays

X-rays not produced

Shorter wavelength

Larger wavelength

91. Deflection of blue light is lesser than violet because

Blue has higher wavelength

Blue is darker colour

Blue is absorbed more easily

Blue has more energy

92. The ionization energy

Generally increases from left to right in a period

Increase from top to bottom in a group

Does not change in a group

Does not change in a period

93. Molecular orbital picture of N₂ indicates

None of these

Two unpaired electron

No unpaired electron

One unpaired electron

94. The nature of positive rays depends upon

All of these

The nature of electrode

The nature of discharge tube

The nature of residual gas

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

X₂Y₃

X₂Y

XY₂

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

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

1 electron

2 electrons

6 electrons

4 electrons

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

5.9 BM

3.0 BM

4.9 BM

6.9 BM

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

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

Calcium

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

1….5

0….5

5….0

5….1

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

Vaporization

Crystallization

Distillation

Colour spectrum

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

H₂O

HCl

CCl₄

CH₃Cl

105. Unit of dipole moment is

Poise

Pascal

Newton

Debye

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

Electron

All these

Proton

Neutron

107. Anti-bonding MO is formed by

Subtraction of atomic orbitals

Addition of atomic orbitals

None of these

Multiplication of atomic orbitals

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

H₂S3

H₂O

H₂Te

109. The number of significant figures in 0.00200 is

One

Three

Two

Five

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

NH₄Cl

HCN

CH₄

H₂O₂

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

SP²

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

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

Zero

-54.4 eV

-13.6 eV

-5.44 eV

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

Li⁺

He⁺

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

Dipole-dipole interaction

H-bonding

Ion-dipole interaction

Dispersion force

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

Electro negativity

None of these

Electron affinity

Ionization energy

117. 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?

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

Decreases

Constant

Variable trend

Increases

119. Which has the minimum bond angle?

NH₃

H₂S

CH₄

H₂O

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

4, 4, 0, ½

4, 1, 0, ½

4, 1, 1, ½

4, 0, 0, ½

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

Pyramidal

Trigonal bipyramidal

Angular

Planar

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

123. The shape of H₃O⁺ is

Triangular planar

Tetrahedral

Pyramidal

Angular

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

Decreases

Remains constant

Increases

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

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

Page 6 of 8

126. Number of π-bonds in naphthalene is

127. Lewis acids are

Electron rich

Octet is complete

No such acids exist

Electron deficient

128. 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

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

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

Hydrogen

Nitrogen

Helium

Oxygen

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

H₂O

HBr

HCl

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

Stability lower then O₂

Diamagnetic character

Bond order of 2.5

Three unpaired electrons

133. 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

134. 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

None of these

Both A and B are correct

Bonding will not occur

135. Unit of dipole moment is

Newton

Poise

Debye

Pascal

136. Fluorine molecule is formed by

The sidewise p-p overlap

The overlap of two sp² hybrid orbitals

The axial s-p overlap

The axial p-p overlap

137. Nuclear radiation is emitted by those elements whose

Molecules are stable

Nuclei are unstable

Nuclei are stable

Molecules are unstable

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

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

Low, positive or slightly negative

High, very negative

Low very negative

None of these

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

There may be a possibility of a chemical reaction

There may not be a possibility of chemical reaction

Water should be preferred over lemon Juice for drinking

Lemon juice is dangerous for health

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

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

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

Bonding molecular orbitals have low electron density between the two nuclei

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

142. Which molecule is polar among the following?

Ethane

Carbon dioxide

Methanol

Carbon tetrachloride

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

Electronegative character of elements

Electropositive character of elements

Pauli exclusion principle

Octet rule

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

Tetrahedron

Hexagon

Cube

Prism

145. Geometry of simple molecule having SP³ hybrid orbital is

Linear

Tetrahedral

Square planner

Triangular

146. 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

656 nm

6.56 nm

65.6 nm

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

Chromium

Nickel

Iron

Copper

148. Al become isoelectronic with Ne

By gaining three electrons

By gaining two electrons

By losing three electrons

By losing two electrons

149. When potassium metal is exposed to violet light

The absorption of electrons takes place

There is no effect

Ejection of electrons takes place

Ejection of some potassium atoms occurs

150. Inter molecular forces in solid hydrogen are

Covalent forces

Hydrogen bonds

All of these

Van der Waal forces or London dispersion forces

Page 7 of 8

151. 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⁺

152. The carbon atoms in calcium carbide are held by

2 covalent, one co-ordinate bond

2 sigma bonds

2π and one σ bond

Ionic bonds

153. 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

Fourth Bohr orbit to the first Bohr orbit

Fifth Bohr orbit to the second Bohr orbit

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

Eight σ and eight π

Nine σ and seven π

Nine σ and nine π

Five π and nine σ

155. Energy of an atom in a compound is

No change

Higher than individual

Impossible to predict

Lesser than individual

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

NH₃

BF₃

BrF₃

H₂O

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

Move with speed as that of light

Charged particles

A stream of electrons

Can be deflected by magnetic fields

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

Ionization energy

Electronegativity

Electron affinity

None of these

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

He⁺

Li⁺

160. Pick out the molecule which has zero dipole moment

SO₂

BCl₃

NH₃

H₂O

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

None of these

Electro negativity

Electron affinity

Ionization energy

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

2, 1, 1

3, 1, 1

3, 2, 1

2, 1, 0

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

I.P

Ea.

E.N

E.A

164. The shape of the molecule SF₂Cl₂ is

Tetrahedral

Cubic

Trigonal bipyramidal

Octahedral

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

166. Effective magnetic moment of Sc³ ion is

5.92

1.73

2.83

167. 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

168. 1 erg of energy corresponds to

6.02 x 10¹⁶ J/mol

10¯⁷ J/mol

1 erg/mol

6.02 x 10²³ J/mol

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

Tetrahedral

Planar triangle

Square planar

Pyramidal

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

HBr

H2O

HCI

171. 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

sp² hybrid orbitals

sp³ hybrid orbitals

p orbitals

172. Which of the following has unchanged valency?

Oxygen

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

174. XeF₄ has shape of

Square planar

Sphere

Tetrahedral

Trigonal bipyramidal

175. Bohr’s model atom is contradicted by

Quarternization of energy of electrons

Quarternization of angular members

Heisenberg’s uncertainty principle

Plank’s quantum theory

Page 8 of 8

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

Phenol

Water

Liquid HCl

Liquid NH3

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

One sigma bond and two pi-bonds

Three sigma bonds

Two sigma bonds and one pi-bond

Three pi-bonds

178. 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

179. Lateral overlapping expected in

Ionic bond

O-bond

Metallic bond

Ā-bonds

180. 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?

10.234

10.234017

10.23

10.2340178

181. Pi bonds are produced by overlapping of

Hybrid and un hybrid orbitals

Atomic orbital and hybrid orbital

Un-hybrid orbitals

Hybrid orbitals

182. 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⁺

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Malik TahirLast Updated: May 24, 2025

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