🧪 NCERT Class 11 • Chapter 4

Chemical Bonding True / False

VSEPR • Hybridisation • Bond Order • Molecular Orbital Theory

Test your conceptual clarity with carefully designed True/False statements covering the most important ideas in Chemical Bonding and Molecular Structure. Each statement targets the subtle conceptual traps that frequently appear in JEE and NEET examinations.

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Chemical Bonding – True / False NCERT Class 11 · Chapter 4

Instant feedback

Chemical bonding often feels straightforward until subtle conceptual traps appear. A misplaced lone pair, incorrect hybridisation count, or misunderstood bond order can turn a correct statement into a false one.

These True/False statements test whether your understanding of VSEPR theory, hybridisation, and molecular orbital theory is precise enough for competitive exams.

📘 Editorial Review

  • 25 concept-focused statements
  • NCERT aligned concepts
  • Geometry & hybridisation checks
  • Molecular orbital reasoning
  • Common exam traps

Academia Aeternum Editorial Team Updated February 2026

🧠 Concept Precision

True/False questions reveal whether you truly understand bonding models rather than memorising shapes or formulas.

🎯 Trap Detection

Most exam mistakes arise from subtle conceptual traps involving lone pairs, polarity, and hybridisation.

⚛️ Faster MCQ Solving

Recognising correct and incorrect statements quickly improves elimination strategies in MCQs.

📊 Exam Trend Insight

Recent JEE and NEET papers increasingly use conceptual traps inside MCQs. Statements about molecular geometry, bond order, and polarity are embedded inside answer options.

Students who practise statement-based reasoning identify incorrect options faster and avoid common conceptual mistakes.

🎯 Quick Knowledge Check

Is BF₃ polar or non-polar? Does O₂⁻ have a bond order greater than 1.5? Does hybridisation always determine molecular shape?

Start Checking Statements →
Your Progress 0 / 25 attempted
Q 01 / 25
Atoms form chemical bonds to achieve lower potential energy.
Q 02 / 25
Noble gases are generally unreactive because they have completely filled valence shells.
Q 03 / 25
Ionic bonding involves transfer of electrons from one atom to another.
Q 04 / 25
A covalent bond is formed by mutual sharing of electrons.
Q 05 / 25
The bond length decreases as bond order increases.
Q 06 / 25
The shape of a molecule depends only on the number of bonded atoms.
Q 07 / 25
According to VSEPR theory, lone pair–lone pair repulsion is strongest.
Q 08 / 25
In BeCl2, the central atom uses sp hybridisation.
Q 09 / 25
The formal charge of an atom is given by: $$FC = V - N - \frac{B}{2}$$
Q 10 / 25
A molecule with zero dipole moment must always be non-polar.
Q 11 / 25
SF6 has octahedral geometry.
Q 12 / 25
All covalent bonds are non-polar.
Q 13 / 25
In BF3, boron completes its octet.
Q 14 / 25
The bond order of O2 is $$2$$ according to molecular orbital theory.
Q 15 / 25
Paramagnetism arises due to presence of unpaired electrons.
Q 16 / 25
Hydrogen bonding is stronger than covalent bonding.
Q 17 / 25
p bonds are formed by end-to-end overlap of orbitals.
Q 18 / 25
In NH3, the bond angle is less than the tetrahedral angle due to lone pair repulsion.
Q 19 / 25
The hybridisation of carbon in ethyne (C2H2) is sp.
Q 20 / 25
Molecules with identical atoms always show zero dipole moment.
Q 21 / 25
The greater the s-character of a hybrid orbital, the shorter the bond formed.
Q 22 / 25
The stability of MO increases with increasing number of nodes.
Q 23 / 25
In NO, the bond order is \(2.5\).
Q 24 / 25
The magnetic nature of O2 supports molecular orbital theory over valence bond theory.
Q 25 / 25
Higher electronegativity difference always results in purely ionic bonding.
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