Chemical Bonding and Molecular StructureNEET MCQs with solutions
Chemical Bonding is one of NEET Chemistry's most important chapters. Lewis structures, VSEPR theory (molecular geometry), hybridisation, molecular orbital theory (MOT), bond order, hydrogen bonding and metallic bonding are all tested. Predicting shapes (linear, trigonal planar, tetrahedral, bent) from electron pairs is a NEET favourite.
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Q1Important PYQ Mixed Concepts
The formal charge on the sulphur atom in the conventional Lewis representation of SO₃ is:
Not quite — the answer is A.
The formal charge is FC = V − N − B/2. For S in the expanded-octet Lewis structure of SO₃, V = 6, N = 0 and six bonding pairs contribute B/2 = 6, giving FC = 0. The trap is +2, which comes from an incomplete-bond representation.
Q2Important PYQ Mixed Concepts
Among CH₄, NH₃ and H₂O, which statement about their bond angles is correct?
Not quite — the answer is B.
The bond-angle order is CH₄ (109.5°) > NH₃ (107°) > H₂O (104.5°). Increasing lone-pair repulsion compresses the bond angle progressively. The trap options reverse or scramble this order.
Q3Covalent Bonding
In which of the following molecules does the central atom form a coordinate bond with one of the other atoms?
Not quite — the answer is C.
In H₃O⁺, the oxygen uses a lone pair to form a coordinate (dative) bond with H⁺, contributing both electrons. BF₃ and CH₄ involve normal covalent bonds; NF₃ has standard shared-pair bonds only.
Q4Covalent Bonding
Which of the following molecules violates the octet rule?
Not quite — the answer is C.
NO has 11 total electrons, making it an odd-electron molecule — the nitrogen atom cannot achieve a complete octet. CH₄, H₂O, and CO₂ all satisfy the octet rule for their central atoms.
Q5Ionic Bonding
Which process is essential for the formation of an ionic bond?
Not quite — the answer is A.
Ionic bonds form by complete transfer of electrons from a metal to a non-metal, creating oppositely charged ions held by electrostatic attraction. Electron sharing defines covalent bonds, not ionic bonds. Orbital overlap and hydrogen bonding are unrelated to ionic bond formation.
Q6Ionic Bonding
Which quantity measures the energy required to remove an electron from a gaseous atom in its ground state?
Not quite — the answer is B.
Ionization enthalpy is the energy required to remove the outermost electron from a gaseous atom in its ground state. Electron gain enthalpy involves addition of an electron, not removal. Lattice enthalpy and bond dissociation enthalpy refer to crystal and bond energies respectively.
Q7Valence Bond Theory
Which concept explains covalent bond formation through overlap of half-filled atomic orbitals?
Not quite — the answer is A.
VBT proposes that a covalent bond forms when half-filled atomic orbitals of two atoms overlap, resulting in electron pairing and bond formation. MOT uses linear combination of orbitals rather than direct overlap. VSEPR predicts geometry but does not explain bond formation.
Q8Valence Bond Theory
Which type of orbital overlap results in the formation of a sigma bond?
Not quite — the answer is B.
Sigma bond forms by end-to-end (axial) overlap of orbitals along the internuclear axis, giving maximum overlap. Sidewise overlap of p orbitals forms a pi bond, not sigma. Only half-filled orbitals participate in bond formation under VBT.
Q9Molecular Orbital Theory
Which observation about O2 is explained by MOT but NOT by VBT?
Not quite — the answer is A.
MOT predicts two unpaired electrons in the degenerate π*2p orbitals of O2, explaining its paramagnetism. VBT incorrectly predicts all electrons are paired (diamagnetic). Bond length and bond energy are explained by both theories.
Q10Molecular Orbital Theory
Which type of molecular orbital is formed by constructive interference of atomic orbital wave functions?
Not quite — the answer is B.
Constructive interference (addition of wave functions) increases electron density between nuclei, forming a bonding molecular orbital of lower energy than the constituent atomic orbitals. Destructive interference forms antibonding orbitals.
Q11Bond Parameters
Which parameter represents the average distance between the nuclei of two covalently bonded atoms?
Not quite — the answer is A.
Bond length is defined as the equilibrium distance between nuclei of bonded atoms. Bond order affects bond length but is not the distance itself. Bond enthalpy measures energy, not distance.
Q12Bond Parameters
Which parameter is defined as the amount of energy required to break one mole of bonds in gaseous molecules?
Not quite — the answer is B.
Bond enthalpy (bond dissociation enthalpy) is the energy needed to homolytically break one mole of a specific bond in gaseous state. Dipole moment measures polarity, not energy. Bond length is a distance parameter.
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Get RankUp on Google PlayQ13Kossel–Lewis Approach to Chemical Bonding
Which noble gas configuration does sodium attain upon losing an electron in NaCl, according to Kossel's approach?
Not quite — the answer is A.
Sodium (atomic number 11) loses one electron to attain the configuration 1s²2s²2p⁶, identical to Neon. Argon (option B) is the configuration attained by chlorine in NaCl, not sodium — a common mix-up. This electron transfer is the central idea of Kossel's approach to ionic bond formation.
Q14Kossel–Lewis Approach to Chemical Bonding
The Lewis symbol of an element represents which type of electrons?
Not quite — the answer is B.
Lewis symbols represent only valence electrons, as these are involved in bonding. Core electrons (option A) are not shown because they do not participate in chemical bond formation. Paired and unpaired valence electrons are both shown as dots around the elemental symbol.
Q15VSEPR Theory
Which theory predicts molecular shape based on electron pair repulsion?
Not quite — the answer is A.
VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry by minimising repulsion between all electron pairs around the central atom. VBT explains bonding through orbital overlap, not shape prediction.
Q16VSEPR Theory
Which type of repulsion is strongest according to VSEPR theory?
Not quite — the answer is B.
Lone pair–lone pair repulsion is strongest because lone pairs are held by only one nucleus and occupy more space, exerting greater repulsive force. The repulsion order is: lp–lp > lp–bp > bp–bp.
Q17Hydrogen Bonding
Hydrogen bonding is best classified as a special type of which interaction?
Not quite — the answer is A.
Hydrogen bonding is an exceptionally strong dipole-dipole interaction where H bonded to F, O, or N acts as a partial positive centre attracting a lone pair on an electronegative atom. Ion-ion and ion-dipole interactions involve full charges, not partial ones. London forces are non-polar in origin.
Q18Hydrogen Bonding
Which element forms the strongest hydrogen bond when covalently bonded to hydrogen?
Not quite — the answer is B.
Fluorine has the highest electronegativity (4.0) and smallest atomic size among all halogens and electronegative elements, creating the most polarised X–H bond and strongest H-bond. Chlorine, despite being electronegative, is too large — its diffuse electron cloud weakens H-bond formation.
Q19Grand Test
Which order of bond angle is correct?
Not quite — the answer is A.
NH₃ has a bond angle of about 107°. In NF₃, the highly electronegative F withdraws bonding electron density away from N, reducing bond-pair repulsion and compressing the angle to about 102.5°. PH₃ has far less hybridisation character, giving an angle of about 93.5°. Therefore NH₃ > NF₃ > PH₃.
Q20Grand Test
Which molecule contains one σ bond and two π bonds between the same pair of atoms?
Not quite — the answer is D.
The N≡N triple bond in N₂ consists of one head-on σ bond and two lateral π bonds formed by sideways overlap of p orbitals. O₂ has a double bond (1σ + 1π). H₂ and Cl₂ have single bonds containing only one σ bond each.
Q21Mixed Revision
Which of the following correctly represents the hybridisation of the central atom and molecular shape of H₂O?
Not quite — the answer is B.
Oxygen has two bond pairs and two lone pairs giving steric number 4 and sp³ hybridisation. The electron-pair geometry is tetrahedral while the molecular geometry is bent.
Q22Mixed Revision
Which species has the highest bond order among the following?
Not quite — the answer is B.
N₂ has bond order 3, the highest among these species. N₂⁺ has 2.5, O₂ has 2 and O₂⁻ has 1.5. Bond order = (bonding electrons minus antibonding electrons) divided by 2.
Q23Kossel–Lewis Approach to Chemical Bonding
Which of the following species does NOT obey the octet rule?
Not quite — the answer is C.
BF₃ has only 6 electrons around boron (three bonding pairs), making it an electron-deficient species with an incomplete octet. NH₃ and H₂O both satisfy the octet around nitrogen and oxygen respectively. CH₄ also completes carbon's octet through four bonding pairs.
Q24Kossel–Lewis Approach to Chemical Bonding
Which of the following correctly explains why noble gases are chemically inert?
Not quite — the answer is B.
Completely filled valence shells (ns²np⁶) place noble gases at the lowest possible energy state, leaving no tendency to gain or lose electrons. High ionisation enthalpy (option A) explains resistance to cation formation but not overall inertness. Option D is factually incorrect — noble gases do form compounds (e.g., XeF₂) under certain conditions.
ELITE question · AIR under 50 level
This chapter has 361 ELITE questions for students aiming at the very top. They are only in the app.
Unlock ELITE questions in the appKey Bonding Concepts
Quick revision: most questions in this chapter test these facts.
| Concept | Key Fact |
|---|---|
| VSEPR shapes | 2 bp = linear; 3 bp = trigonal planar; 4 bp = tetrahedral; 2 bp + 2 lp = bent |
| Hybridisation | sp = linear (180°), sp² = trigonal (120°), sp³ = tetrahedral (109.5°) |
| Bond order (MOT) | BO = (Nb − Na)/2; BO = 0 means molecule doesn't exist |
| Dipole moment | μ = q × d; linear symmetric molecules (CO₂, BF₃) have μ = 0 despite polar bonds |
| Hydrogen bonding | F−H···F > O−H···O > N−H···N; intramolecular H-bond lowers boiling point |
| Resonance | Delocalisation of electrons; actual structure is hybrid of all contributing structures |
What the app covers in this chapter
762 questions in total, each with a detailed explanation.
| Important PYQ Mixed Concepts | 99 |
| Covalent Bonding | 80 |
| Ionic Bonding | 79 |
| Valence Bond Theory | 79 |
| Molecular Orbital Theory | 78 |
| Bond Parameters | 60 |
| Kossel–Lewis Approach to Chemical Bonding | 59 |
| VSEPR Theory | 59 |
| Hydrogen Bonding | 59 |
| Grand Test | 59 |
| Mixed Revision | 51 |
Questions students ask
Is Chemical Bonding important for NEET?
Very important — it carries high weightage. Questions on VSEPR shapes, hybridisation, MOT bond order, dipole moment and hydrogen bonding appear every year.
Which topics should I revise first?
Focus on VSEPR theory with common shapes, hybridisation prediction, MOT for O₂ and N₂ (bond order, magnetic nature), dipole moment (why CO₂ is zero), and types of hydrogen bonding.
How many questions from this chapter are on RankUp?
The RankUp app has 762 questions on Chemical Bonding and Molecular Structure, including 361 ELITE questions. Every question has a detailed explanation.
