Chemical Bonding MCQs 2026

A double bond consists of

1. ATwo sigma bonds✓
2. BOne sigma and one pi bond✓
3. CTwo pi bonds✓
4. DThree sigma bonds✓

An ionic bond is formed by

1. ASharing of electrons✓
2. BComplete transfer of electrons✓
3. CSharing of protons✓
4. DOverlap of orbitals only✓

A covalent bond is formed by

1. AComplete transfer of electrons✓
2. BAttraction between ions✓
3. CLoss of electrons✓
4. DMutual sharing of electron pairs✓

Ionic bonds are typically formed between

1. AA metal and a non-metal✓
2. BTwo non-metals✓
3. CTwo metals✓
4. DTwo noble gases✓

A coordinate covalent (dative) bond is formed when

1. ATwo atoms share electrons equally✓
2. BElectrons are transferred completely✓
3. CTwo atoms repel each other✓
4. DBoth shared electrons come from the same atom✓

According to the octet rule, atoms tend to gain, lose, or share electrons to attain

1. A8 electrons in the valence shell✓
2. B2 electrons only✓
3. CA negative charge✓
4. DMaximum mass✓

Which of the following molecules is an exception to the octet rule (having fewer than 8 electrons)

1. ACO2✓
2. BH2O✓
3. CNH3✓
4. DBF3✓

The bond formed between two atoms of the same element (e.g. Cl2) is

1. AIonic bond✓
2. BMetallic bond✓
3. CCoordinate bond✓
4. DNon-polar covalent bond✓

A polar covalent bond arises due to

1. AEqual sharing of electrons✓
2. BUnequal sharing of electrons due to electronegativity difference✓
3. CComplete electron transfer✓
4. DAbsence of electronegativity difference✓

The shape of a methane (CH4) molecule according to VSEPR theory is

1. ATetrahedral✓
2. BLinear✓
3. CTrigonal planar✓
4. DBent✓

The shape of a water (H2O) molecule is

1. ALinear✓
2. BTetrahedral✓
3. CBent (V-shaped)✓
4. DTrigonal pyramidal✓

The shape of an ammonia (NH3) molecule is

1. ALinear✓
2. BTetrahedral✓
3. CTrigonal pyramidal✓
4. DBent✓

The shape of a carbon dioxide (CO2) molecule is

1. ALinear✓
2. BBent✓
3. CTrigonal planar✓
4. DTetrahedral✓

VSEPR theory predicts molecular shape based on

1. ARepulsion between electron pairs around the central atom✓
2. BAtomic mass of atoms✓
3. CNumber of protons✓
4. DBond length only✓

The type of hybridization present in methane (CH4) is

1. Asp3✓
2. Bsp2✓
3. Csp✓
4. Ddsp2✓

The type of hybridization present in ethene (C2H4) at each carbon is

1. Asp3✓
2. Bsp3d✓
3. Csp✓
4. Dsp2✓

The type of hybridization present in ethyne/acetylene (C2H2) is

1. Asp3✓
2. Bsp✓
3. Csp2✓
4. Dsp3d✓

A sigma (σ) bond is formed by

1. AHead-on (axial) overlap of orbitals✓
2. BSidewise overlap of p-orbitals✓
3. CTransfer of electrons✓
4. DOverlap of d-orbitals only✓

A pi (π) bond is formed by

1. AHead-on overlap of orbitals✓
2. BComplete transfer of electrons✓
3. CSidewise (lateral) overlap of parallel p-orbitals✓
4. DIonic attraction✓

A triple bond consists of

1. AOne sigma and two pi bonds✓
2. BThree sigma bonds✓
3. CTwo sigma and one pi bond✓
4. DThree pi bonds✓

Hydrogen bonding is strongest between molecules containing hydrogen attached to

1. ACarbon✓
2. BSulfur✓
3. CPhosphorus✓
4. DHighly electronegative atoms like F, O, N✓

Which of the following exhibits hydrogen bonding

1. ACH4✓
2. BCO2✓
3. CH2O✓
4. DN2✓

The high boiling point of water compared to H2S is mainly due to

1. AIonic bonding✓
2. BHydrogen bonding✓
3. CMetallic bonding✓
4. DVan der Waals forces only✓

Metallic bonding is best described as

1. ATransfer of electrons between metal atoms✓
2. BSharing of electrons between two metal atoms only✓
3. CA sea of delocalized electrons surrounding positive metal ions✓
4. DElectrostatic attraction between ions of opposite charge only✓

Which theory explains bonding using the idea of a 'sea of electrons'

1. AVSEPR theory✓
2. BValence bond theory✓
3. CMolecular orbital theory✓
4. DElectron sea (metallic bonding) theory✓

The bond angle in a water molecule is approximately

1. A180°✓
2. B120°✓
3. C109.5°✓
4. D104.5°✓

The bond angle in a methane molecule is

1. A109.5°✓
2. B90°✓
3. C120°✓
4. D104.5°✓

The bond angle in ammonia (NH3) is approximately

1. A107°✓
2. B109.5°✓
3. C120°✓
4. D180°✓

Lattice energy is defined as the energy released when

1. AA covalent bond is broken✓
2. BGaseous ions combine to form one mole of an ionic solid✓
3. CAn ionic solid dissolves in water✓
4. DA molecule vaporizes✓

Which of the following compounds is expected to have the highest lattice energy

1. AMgO✓
2. BNaCl✓
3. CKCl✓
4. DNaBr✓

Resonance occurs when a molecule or ion

1. AHas only one possible Lewis structure✓
2. BChanges its actual structure repeatedly✓
3. CCan be represented by two or more valid Lewis structures with the same atomic arrangement✓
4. DLoses electrons permanently✓

Which of the following molecules/ions shows resonance

1. ACH4✓
2. BCO3^2- (carbonate ion)✓
3. CNH3✓
4. DH2O✓

Van der Waals forces are

1. AStronger than ionic bonds✓
2. BStronger than covalent bonds✓
3. CThe same as hydrogen bonds✓
4. DWeak intermolecular forces of attraction✓

Dipole-dipole interactions occur between molecules that are

1. ANon-polar✓
2. BIonic compounds only✓
3. CPolar✓
4. DNoble gases only✓

Which of the following bonds is generally the strongest

1. AVan der Waals force✓
2. BCovalent bond✓
3. CHydrogen bond✓
4. DDipole-induced dipole force✓

The electron-dot representation of bonding in molecules was introduced by

1. ABohr✓
2. BPauling✓
3. CLewis✓
4. DRutherford✓

Linus Pauling is best known for his contribution to the concept of

1. AAtomic number✓
2. BRadioactivity✓
3. CElectronegativity scale✓
4. DThe neutron✓

A non-polar covalent bond forms when the electronegativity difference between bonded atoms is

1. AGreater than 1.7✓
2. BApproximately zero✓
3. CBetween 0.5 and 1.7✓
4. DAlways negative✓

An ionic bond is generally expected when the electronegativity difference between two atoms is

1. ALess than 0.5✓
2. BBetween 0.5 and 1.7✓
3. CGreater than about 1.7✓
4. DExactly zero✓

Which of the following molecules is non-polar despite having polar bonds

1. AH2O✓
2. BNH3✓
3. CCO2✓
4. DHCl✓

Boron trifluoride (BF3) has a ___ shape

1. ATetrahedral✓
2. BTrigonal planar✓
3. CBent✓
4. DLinear✓

Phosphorus pentachloride (PCl5) exhibits ___ hybridization

1. Asp3✓
2. Bsp3d✓
3. Csp3d2✓
4. Dsp2✓

Sulfur hexafluoride (SF6) exhibits ___ hybridization

1. Asp3✓
2. Bsp3d✓
3. Csp2✓
4. Dsp3d2✓

Which of the following is an example of a coordinate covalent bond

1. ABond in Cl2✓
2. BBond in NaCl✓
3. CBond in CH4✓
4. DBond in NH4+ (ammonium ion)✓

The bond length between two atoms is inversely related to the

1. AAtomic mass✓
2. BNumber of lone pairs✓
3. CElectronegativity difference✓
4. DBond order (higher bond order, shorter bond length)✓

Bond dissociation energy is generally highest for

1. ATriple bonds✓
2. BSingle bonds✓
3. CHydrogen bonds✓
4. DVan der Waals interactions✓

The molecule with a linear shape and sp hybridization at the central atom is

1. AH2O✓
2. BNH3✓
3. CBeCl2✓
4. DCH4✓

Which theory considers bond formation in terms of overlapping atomic orbitals retaining their identity

1. AMolecular orbital theory✓
2. BValence bond theory✓
3. CVSEPR theory✓
4. DCrystal field theory✓

Molecular orbital theory explains bonding using the concept of

1. AElectron transfer only✓
2. BLocalized bonds between two atoms only✓
3. CCombination of atomic orbitals into bonding and antibonding molecular orbitals✓
4. DLattice energy✓

A bond order of zero, according to molecular orbital theory, indicates that

1. AThe bond is a triple bond✓
2. BThe molecule does not exist (unstable)✓
3. CThe bond is ionic✓
4. DThe bond is very strong✓