A covalent bond is formed by

Mutual sharing of electron pairs

A coordinate covalent (dative) bond is formed when

Both shared electrons come from the same atom

Chemical Bonding MCQs 2026

76 questions with detailed answers · 27 from past papers · 8 quiz batches available

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Page 1 of 1 Questions 1–10 of 76

Q1 medium

A double bond consists of
1. A Two sigma bonds
2. B One sigma and one pi bond
3. C Two pi bonds
4. D Three sigma bonds
💡 Explanation:
A double bond is composed of one strong sigma bond and one weaker pi bond.
Q2 easy

An ionic bond is formed by
1. A Sharing of electrons
2. B Complete transfer of electrons
3. C Sharing of protons
4. D Overlap of orbitals only
💡 Explanation:
Ionic bonds form when one atom fully transfers electrons to another, creating oppositely charged ions.
Q3 Past Paper · PPSC/FPSC/NTS easy

A covalent bond is formed by
1. A Complete transfer of electrons
2. B Attraction between ions
3. C Loss of electrons
4. D Mutual sharing of electron pairs
💡 Explanation:
Covalent bonds arise from atoms mutually sharing pairs of electrons.
Q4 Past Paper · PPSC/FPSC/NTS easy

Ionic bonds are typically formed between
1. A A metal and a non-metal
2. B Two non-metals
3. C Two metals
4. D Two noble gases
💡 Explanation:
Metals readily lose electrons while non-metals gain them, favoring ionic bond formation.
Q5 easy

A coordinate covalent (dative) bond is formed when
1. A Two atoms share electrons equally
2. B Electrons are transferred completely
3. C Two atoms repel each other
4. D Both shared electrons come from the same atom
💡 Explanation:
In a dative bond, one atom donates both electrons of the shared pair.
Q6 Past Paper · PPSC/FPSC/NTS easy

According to the octet rule, atoms tend to gain, lose, or share electrons to attain
1. A 8 electrons in the valence shell
2. B 2 electrons only
3. C A negative charge
4. D Maximum mass
💡 Explanation:
Atoms react to achieve a stable, noble-gas-like configuration of 8 valence electrons.
Q7 easy

Which of the following molecules is an exception to the octet rule (having fewer than 8 electrons)
1. A CO2
2. B H2O
3. C NH3
4. D BF3
💡 Explanation:
Boron in BF3 has only 6 electrons around it, making it electron deficient.
Q8 Past Paper · PPSC/FPSC/NTS easy

The bond formed between two atoms of the same element (e.g. Cl2) is
1. A Ionic bond
2. B Metallic bond
3. C Coordinate bond
4. D Non-polar covalent bond
💡 Explanation:
Identical atoms share electrons equally, producing a non-polar covalent bond.
Q9 easy

A polar covalent bond arises due to
1. A Equal sharing of electrons
2. B Unequal sharing of electrons due to electronegativity difference
3. C Complete electron transfer
4. D Absence of electronegativity difference
💡 Explanation:
A difference in electronegativity causes electrons to be pulled closer to the more electronegative atom.
Q10 Past Paper · PPSC/FPSC/NTS easy

The shape of a methane (CH4) molecule according to VSEPR theory is
1. A Tetrahedral
2. B Linear
3. C Trigonal planar
4. D Bent
💡 Explanation:
Four bonding pairs around carbon arrange themselves tetrahedrally to minimize repulsion.
Q11 easy

The shape of a water (H2O) molecule is
1. A Linear
2. B Tetrahedral
3. C Bent (V-shaped)
4. D Trigonal pyramidal
💡 Explanation:
Two lone pairs on oxygen push the two O-H bonds into a bent shape.
Q12 medium

The shape of an ammonia (NH3) molecule is
1. A Linear
2. B Tetrahedral
3. C Trigonal pyramidal
4. D Bent
💡 Explanation:
One lone pair on nitrogen distorts the shape into a trigonal pyramid.
Q13 Past Paper · PPSC/FPSC/NTS medium

The shape of a carbon dioxide (CO2) molecule is
1. A Linear
2. B Bent
3. C Trigonal planar
4. D Tetrahedral
💡 Explanation:
With no lone pairs on carbon, the two double bonds arrange linearly at 180 degrees.
Q14 medium

VSEPR theory predicts molecular shape based on
1. A Repulsion between electron pairs around the central atom
2. B Atomic mass of atoms
3. C Number of protons
4. D Bond length only
💡 Explanation:
VSEPR theory states electron pairs arrange to minimize mutual repulsion, determining molecular geometry.
Q15 Past Paper · PPSC/FPSC/NTS medium

The type of hybridization present in methane (CH4) is
1. A sp3
2. B sp2
3. C sp
4. D dsp2
💡 Explanation:
Carbon forms four equivalent sigma bonds using sp3 hybrid orbitals in methane.
Q16 medium

The type of hybridization present in ethene (C2H4) at each carbon is
1. A sp3
2. B sp3d
3. C sp
4. D sp2
💡 Explanation:
Each carbon in ethene forms three sigma bonds and one pi bond using sp2 hybridization.
Q17 medium

The type of hybridization present in ethyne/acetylene (C2H2) is
1. A sp3
2. B sp
3. C sp2
4. D sp3d
💡 Explanation:
Each carbon in acetylene forms two sigma bonds and two pi bonds using sp hybridization.
Q18 Past Paper · PPSC/FPSC/NTS medium

A sigma (σ) bond is formed by
1. A Head-on (axial) overlap of orbitals
2. B Sidewise overlap of p-orbitals
3. C Transfer of electrons
4. D Overlap of d-orbitals only
💡 Explanation:
Sigma bonds result from direct, head-on overlap of atomic orbitals along the bond axis.
Q19 medium

A pi (π) bond is formed by
1. A Head-on overlap of orbitals
2. B Complete transfer of electrons
3. C Sidewise (lateral) overlap of parallel p-orbitals
4. D Ionic attraction
💡 Explanation:
Pi bonds form from the sideways overlap of unhybridized parallel p-orbitals.
Q20 Past Paper · PPSC/FPSC/NTS medium

A triple bond consists of
1. A One sigma and two pi bonds
2. B Three sigma bonds
3. C Two sigma and one pi bond
4. D Three pi bonds
💡 Explanation:
A triple bond contains one sigma bond and two perpendicular pi bonds.
Q21 medium

Hydrogen bonding is strongest between molecules containing hydrogen attached to
1. A Carbon
2. B Sulfur
3. C Phosphorus
4. D Highly electronegative atoms like F, O, N
💡 Explanation:
Hydrogen bonded to small, highly electronegative atoms forms the strongest hydrogen bonds.
Q22 medium

Which of the following exhibits hydrogen bonding
1. A CH4
2. B CO2
3. C H2O
4. D N2
💡 Explanation:
Water's O-H bonds allow extensive hydrogen bonding between molecules.
Q23 Past Paper · PPSC/FPSC/NTS medium

The high boiling point of water compared to H2S is mainly due to
1. A Ionic bonding
2. B Hydrogen bonding
3. C Metallic bonding
4. D Van der Waals forces only
💡 Explanation:
Extensive hydrogen bonding in water requires more energy to break, raising its boiling point.
Q24 medium

Metallic bonding is best described as
1. A Transfer of electrons between metal atoms
2. B Sharing of electrons between two metal atoms only
3. C A sea of delocalized electrons surrounding positive metal ions
4. D Electrostatic attraction between ions of opposite charge only
💡 Explanation:
Metallic bonding involves valence electrons delocalized throughout a lattice of metal cations.
Q25 medium

Which theory explains bonding using the idea of a 'sea of electrons'
1. A VSEPR theory
2. B Valence bond theory
3. C Molecular orbital theory
4. D Electron sea (metallic bonding) theory
💡 Explanation:
The electron sea model describes metallic bonding as delocalized electrons surrounding fixed metal ions.
Q26 Past Paper · PPSC/FPSC/NTS medium

The bond angle in a water molecule is approximately
1. A 180°
2. B 120°
3. C 109.5°
4. D 104.5°
💡 Explanation:
Lone pair repulsion compresses the ideal tetrahedral angle to about 104.5° in water.
Q27 medium

The bond angle in a methane molecule is
1. A 109.5°
2. B 90°
3. C 120°
4. D 104.5°
💡 Explanation:
Methane's tetrahedral geometry gives a bond angle of 109.5°.
Q28 medium

The bond angle in ammonia (NH3) is approximately
1. A 107°
2. B 109.5°
3. C 120°
4. D 180°
💡 Explanation:
The lone pair on nitrogen compresses the H-N-H angle to about 107°.
Q29 Past Paper · PPSC/FPSC/NTS medium

Lattice energy is defined as the energy released when
1. A A covalent bond is broken
2. B Gaseous ions combine to form one mole of an ionic solid
3. C An ionic solid dissolves in water
4. D A molecule vaporizes
💡 Explanation:
Lattice energy measures the energy released as gaseous ions come together to form a solid ionic lattice.
Q30 medium

Which of the following compounds is expected to have the highest lattice energy
1. A MgO
2. B NaCl
3. C KCl
4. D NaBr
💡 Explanation:
MgO's smaller ionic radii and higher ionic charges (2+/2-) give it a much larger lattice energy.
Q31 medium

Resonance occurs when a molecule or ion
1. A Has only one possible Lewis structure
2. B Changes its actual structure repeatedly
3. C Can be represented by two or more valid Lewis structures with the same atomic arrangement
4. D Loses electrons permanently
💡 Explanation:
Resonance structures are different ways of distributing electrons while keeping atoms in the same positions.
Q32 Past Paper · PPSC/FPSC/NTS medium

Which of the following molecules/ions shows resonance
1. A CH4
2. B CO3^2- (carbonate ion)
3. C NH3
4. D H2O
💡 Explanation:
The carbonate ion's negative charge and double bond are delocalized among all three oxygens.
Q33 medium

Van der Waals forces are
1. A Stronger than ionic bonds
2. B Stronger than covalent bonds
3. C The same as hydrogen bonds
4. D Weak intermolecular forces of attraction
💡 Explanation:
Van der Waals forces are comparatively weak attractions between molecules.
Q34 medium

Dipole-dipole interactions occur between molecules that are
1. A Non-polar
2. B Ionic compounds only
3. C Polar
4. D Noble gases only
💡 Explanation:
Polar molecules have permanent dipoles that attract oppositely charged ends of neighboring molecules.
Q35 Past Paper · PPSC/FPSC/NTS medium

Which of the following bonds is generally the strongest
1. A Van der Waals force
2. B Covalent bond
3. C Hydrogen bond
4. D Dipole-induced dipole force
💡 Explanation:
Covalent bonds involve shared electron pairs and are far stronger than intermolecular forces.
Q36 medium

The electron-dot representation of bonding in molecules was introduced by
1. A Bohr
2. B Pauling
3. C Lewis
4. D Rutherford
💡 Explanation:
G.N. Lewis introduced dot diagrams to represent valence electrons and bonding.
Q37 medium

Linus Pauling is best known for his contribution to the concept of
1. A Atomic number
2. B Radioactivity
3. C Electronegativity scale
4. D The neutron
💡 Explanation:
Pauling developed the widely used electronegativity scale for elements.
Q38 Past Paper · PPSC/FPSC/NTS medium

A non-polar covalent bond forms when the electronegativity difference between bonded atoms is
1. A Greater than 1.7
2. B Approximately zero
3. C Between 0.5 and 1.7
4. D Always negative
💡 Explanation:
Nearly identical electronegativities result in equal sharing of electrons, giving a non-polar bond.
Q39 medium

An ionic bond is generally expected when the electronegativity difference between two atoms is
1. A Less than 0.5
2. B Between 0.5 and 1.7
3. C Greater than about 1.7
4. D Exactly zero
💡 Explanation:
A large electronegativity difference favors complete electron transfer rather than sharing.
Q40 medium

Which of the following molecules is non-polar despite having polar bonds
1. A H2O
2. B NH3
3. C CO2
4. D HCl
💡 Explanation:
CO2's linear symmetric shape causes the two polar C=O bond dipoles to cancel out.
Q41 Past Paper · PPSC/FPSC/NTS hard

Boron trifluoride (BF3) has a ___ shape
1. A Tetrahedral
2. B Trigonal planar
3. C Bent
4. D Linear
💡 Explanation:
With three bonding pairs and no lone pairs, BF3 adopts a trigonal planar geometry.
Q42 hard

Phosphorus pentachloride (PCl5) exhibits ___ hybridization
1. A sp3
2. B sp3d
3. C sp3d2
4. D sp2
💡 Explanation:
PCl5 has five bonding pairs, requiring sp3d hybridization for a trigonal bipyramidal shape.
Q43 hard

Sulfur hexafluoride (SF6) exhibits ___ hybridization
1. A sp3
2. B sp3d
3. C sp2
4. D sp3d2
💡 Explanation:
SF6's six bonding pairs require sp3d2 hybridization, giving an octahedral shape.
Q44 Past Paper · PPSC/FPSC/NTS hard

Which of the following is an example of a coordinate covalent bond
1. A Bond in Cl2
2. B Bond in NaCl
3. C Bond in CH4
4. D Bond in NH4+ (ammonium ion)
💡 Explanation:
In NH4+, nitrogen's lone pair alone forms the bond to the fourth hydrogen (as H+).
Q45 hard

The bond length between two atoms is inversely related to the
1. A Atomic mass
2. B Number of lone pairs
3. C Electronegativity difference
4. D Bond order (higher bond order, shorter bond length)
💡 Explanation:
Higher bond order means more shared electron pairs pulling atoms closer, shortening bond length.
Q46 hard

Bond dissociation energy is generally highest for
1. A Triple bonds
2. B Single bonds
3. C Hydrogen bonds
4. D Van der Waals interactions
💡 Explanation:
Triple bonds involve three shared electron pairs, requiring the most energy to break.
Q47 Past Paper · PPSC/FPSC/NTS hard

The molecule with a linear shape and sp hybridization at the central atom is
1. A H2O
2. B NH3
3. C BeCl2
4. D CH4
💡 Explanation:
Beryllium in BeCl2 has only two bonding pairs and no lone pairs, giving sp hybridization and linear shape.
Q48 hard

Which theory considers bond formation in terms of overlapping atomic orbitals retaining their identity
1. A Molecular orbital theory
2. B Valence bond theory
3. C VSEPR theory
4. D Crystal field theory
💡 Explanation:
Valence bond theory describes bonds as localized overlaps of atomic orbitals from individual atoms.
Q49 hard

Molecular orbital theory explains bonding using the concept of
1. A Electron transfer only
2. B Localized bonds between two atoms only
3. C Combination of atomic orbitals into bonding and antibonding molecular orbitals
4. D Lattice energy
💡 Explanation:
MO theory combines atomic orbitals into new molecular orbitals spanning the whole molecule.
Q50 hard

A bond order of zero, according to molecular orbital theory, indicates that
1. A The bond is a triple bond
2. B The molecule does not exist (unstable)
3. C The bond is ionic
4. D The bond is very strong
💡 Explanation:
A bond order of zero means bonding and antibonding effects cancel out, so no stable bond forms.
Q51 medium

A double bond consists of
1. A Two sigma bonds
2. B One sigma and one pi bond
3. C Two pi bonds
4. D Three sigma bonds
💡 Explanation:
A double bond is composed of one strong sigma bond and one weaker pi bond.
Q52 Past Paper · PPSC/FPSC/NTS medium

A triple bond consists of
1. A One sigma and two pi bonds
2. B Three sigma bonds
3. C Two sigma and one pi bond
4. D Three pi bonds
💡 Explanation:
A triple bond contains one sigma bond and two perpendicular pi bonds.
Q53 medium

Hydrogen bonding is strongest between molecules containing hydrogen attached to
1. A Carbon
2. B Sulfur
3. C Phosphorus
4. D Highly electronegative atoms like F, O, N
💡 Explanation:
Hydrogen bonded to small, highly electronegative atoms forms the strongest hydrogen bonds.
Q54 medium

Which of the following exhibits hydrogen bonding
1. A CH4
2. B CO2
3. C H2O
4. D N2
💡 Explanation:
Water's O-H bonds allow extensive hydrogen bonding between molecules.
Q55 Past Paper · PPSC/FPSC/NTS medium

The high boiling point of water compared to H2S is mainly due to
1. A Ionic bonding
2. B Hydrogen bonding
3. C Metallic bonding
4. D Van der Waals forces only
💡 Explanation:
Extensive hydrogen bonding in water requires more energy to break, raising its boiling point.
Q56 medium

Metallic bonding is best described as
1. A Transfer of electrons between metal atoms
2. B Sharing of electrons between two metal atoms only
3. C A sea of delocalized electrons surrounding positive metal ions
4. D Electrostatic attraction between ions of opposite charge only
💡 Explanation:
Metallic bonding involves valence electrons delocalized throughout a lattice of metal cations.
Q57 medium

Which theory explains bonding using the idea of a 'sea of electrons'
1. A VSEPR theory
2. B Valence bond theory
3. C Molecular orbital theory
4. D Electron sea (metallic bonding) theory
💡 Explanation:
The electron sea model describes metallic bonding as delocalized electrons surrounding fixed metal ions.
Q58 Past Paper · PPSC/FPSC/NTS medium

The bond angle in a water molecule is approximately
1. A 180°
2. B 120°
3. C 109.5°
4. D 104.5°
💡 Explanation:
Lone pair repulsion compresses the ideal tetrahedral angle to about 104.5° in water.
Q59 medium

The bond angle in a methane molecule is
1. A 109.5°
2. B 90°
3. C 120°
4. D 104.5°
💡 Explanation:
Methane's tetrahedral geometry gives a bond angle of 109.5°.
Q60 medium

The bond angle in ammonia (NH3) is approximately
1. A 107°
2. B 109.5°
3. C 120°
4. D 180°
💡 Explanation:
The lone pair on nitrogen compresses the H-N-H angle to about 107°.
Q61 Past Paper · PPSC/FPSC/NTS medium

Lattice energy is defined as the energy released when
1. A A covalent bond is broken
2. B Gaseous ions combine to form one mole of an ionic solid
3. C An ionic solid dissolves in water
4. D A molecule vaporizes
💡 Explanation:
Lattice energy measures the energy released as gaseous ions come together to form a solid ionic lattice.
Q62 medium

Which of the following compounds is expected to have the highest lattice energy
1. A MgO
2. B NaCl
3. C KCl
4. D NaBr
💡 Explanation:
MgO's smaller ionic radii and higher ionic charges (2+/2-) give it a much larger lattice energy.
Q63 medium

Resonance occurs when a molecule or ion
1. A Has only one possible Lewis structure
2. B Changes its actual structure repeatedly
3. C Can be represented by two or more valid Lewis structures with the same atomic arrangement
4. D Loses electrons permanently
💡 Explanation:
Resonance structures are different ways of distributing electrons while keeping atoms in the same positions.
Q64 Past Paper · PPSC/FPSC/NTS medium

Which of the following molecules/ions shows resonance
1. A CH4
2. B CO3^2- (carbonate ion)
3. C NH3
4. D H2O
💡 Explanation:
The carbonate ion's negative charge and double bond are delocalized among all three oxygens.
Q65 medium

Van der Waals forces are
1. A Stronger than ionic bonds
2. B Stronger than covalent bonds
3. C The same as hydrogen bonds
4. D Weak intermolecular forces of attraction
💡 Explanation:
Van der Waals forces are comparatively weak attractions between molecules.
Q66 medium

Dipole-dipole interactions occur between molecules that are
1. A Non-polar
2. B Ionic compounds only
3. C Polar
4. D Noble gases only
💡 Explanation:
Polar molecules have permanent dipoles that attract oppositely charged ends of neighboring molecules.
Q67 Past Paper · PPSC/FPSC/NTS medium

Which of the following bonds is generally the strongest
1. A Van der Waals force
2. B Covalent bond
3. C Hydrogen bond
4. D Dipole-induced dipole force
💡 Explanation:
Covalent bonds involve shared electron pairs and are far stronger than intermolecular forces.
Q68 medium

The electron-dot representation of bonding in molecules was introduced by
1. A Bohr
2. B Pauling
3. C Lewis
4. D Rutherford
💡 Explanation:
G.N. Lewis introduced dot diagrams to represent valence electrons and bonding.
Q69 medium

Linus Pauling is best known for his contribution to the concept of
1. A Atomic number
2. B Radioactivity
3. C Electronegativity scale
4. D The neutron
💡 Explanation:
Pauling developed the widely used electronegativity scale for elements.
Q70 Past Paper · PPSC/FPSC/NTS medium

A non-polar covalent bond forms when the electronegativity difference between bonded atoms is
1. A Greater than 1.7
2. B Approximately zero
3. C Between 0.5 and 1.7
4. D Always negative
💡 Explanation:
Nearly identical electronegativities result in equal sharing of electrons, giving a non-polar bond.
Q71 medium

An ionic bond is generally expected when the electronegativity difference between two atoms is
1. A Less than 0.5
2. B Between 0.5 and 1.7
3. C Greater than about 1.7
4. D Exactly zero
💡 Explanation:
A large electronegativity difference favors complete electron transfer rather than sharing.
Q72 medium

Which of the following molecules is non-polar despite having polar bonds
1. A H2O
2. B NH3
3. C CO2
4. D HCl
💡 Explanation:
CO2's linear symmetric shape causes the two polar C=O bond dipoles to cancel out.
Q73 Past Paper · PPSC/FPSC/NTS hard

Boron trifluoride (BF3) has a ___ shape
1. A Tetrahedral
2. B Trigonal planar
3. C Bent
4. D Linear
💡 Explanation:
With three bonding pairs and no lone pairs, BF3 adopts a trigonal planar geometry.
Q74 hard

Phosphorus pentachloride (PCl5) exhibits ___ hybridization
1. A sp3
2. B sp3d
3. C sp3d2
4. D sp2
💡 Explanation:
PCl5 has five bonding pairs, requiring sp3d hybridization for a trigonal bipyramidal shape.
Q75 hard

Sulfur hexafluoride (SF6) exhibits ___ hybridization
1. A sp3
2. B sp3d
3. C sp2
4. D sp3d2
💡 Explanation:
SF6's six bonding pairs require sp3d2 hybridization, giving an octahedral shape.
Q76 Past Paper · PPSC/FPSC/NTS hard

Which of the following is an example of a coordinate covalent bond
1. A Bond in Cl2
2. B Bond in NaCl
3. C Bond in CH4
4. D Bond in NH4+ (ammonium ion)
💡 Explanation:
In NH4+, nitrogen's lone pair alone forms the bond to the fourth hydrogen (as H+).

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