Class 11 – Chemical Bonding and Molecular Structure (40 MCQs)
Ionic Bonding (1–6)
- Ionic bond is formed by:
a) Sharing of electrons
b) Transfer of electrons
c) Overlapping of orbitals
d) Nuclear reaction - Which of the following is an ionic compound?
a) H₂O
b) NaCl
c) CH₄
d) NH₃ - The lattice energy of an ionic compound depends on:
a) Charges on ions
b) Ionic radii
c) Both a & b
d) Nature of solvent only - Ionic compounds are generally:
a) Good conductors in solid state
b) Good conductors in molten/aqueous state
c) Soft solids
d) Volatile liquids - Which of the following has the highest lattice energy?
a) NaCl
b) MgO
c) KBr
d) LiF - The ionic character of a bond increases with:
a) Greater electronegativity difference
b) Smaller electronegativity difference
c) Higher temperature
d) Larger atomic mass
Covalent Bonding (7–13)
- Covalent bond is formed by:
a) Sharing of electrons
b) Transfer of electrons
c) Hydrogen bonding
d) Dipole interaction - The Lewis structure represents:
a) Electron density
b) Nucleus positions
c) Valence electrons and bonds
d) Molecular orbitals - Which of the following violates the octet rule?
a) H₂O
b) BF₃
c) CH₄
d) NH₃ - Resonance occurs when:
a) Single structure represents the molecule
b) Multiple equivalent structures can be drawn
c) Molecule is ionic
d) Molecule is polar - The bond order of O₂ molecule is:
a) 1
b) 2
c) 3
d) 1.5 - In CO₂, the C=O bond is:
a) Single bond
b) Double bond
c) Triple bond
d) Coordinate bond - Electronegativity difference less than 0.5 indicates:
a) Ionic bond
b) Polar covalent bond
c) Pure covalent bond
d) Metallic bond
Bond Parameters (14–18)
- Bond length is:
a) Distance between nuclei of two bonded atoms
b) Energy required to break a bond
c) Electron cloud overlap
d) None of the above - Which has the shortest bond length?
a) C–C
b) C=C
c) C≡C
d) All same - Bond energy is:
a) Energy released when bond is formed
b) Energy required to break 1 mole of bonds
c) Energy of electrons in atom
d) None - Higher bond order indicates:
a) Shorter bond length
b) Stronger bond
c) Both a & b
d) Weaker bond - Which molecule has bond order 2?
a) O₂
b) N₂
c) CO
d) H₂
Polar/Nonpolar Molecules & Electronegativity (19–23)
- A polar covalent bond has:
a) Equal sharing of electrons
b) Unequal sharing of electrons
c) Complete transfer of electrons
d) No electrons shared - The dipole moment of a nonpolar molecule is:
a) Zero
b) Maximum
c) 1 D
d) Infinite - HCl molecule is:
a) Polar
b) Nonpolar
c) Ionic
d) Metallic - Which element is most electronegative?
a) H
b) O
c) F
d) Cl - Polar molecules are generally:
a) Soluble in polar solvents
b) Soluble in nonpolar solvents
c) Insoluble in all solvents
d) Always ionic
VSEPR Theory & Molecular Geometry (24–29)
- The shape of CH₄ molecule is:
a) Linear
b) Trigonal planar
c) Tetrahedral
d) Bent - The shape of NH₃ molecule is:
a) Trigonal pyramidal
b) Linear
c) Tetrahedral
d) Bent - The shape of H₂O molecule is:
a) Linear
b) Bent
c) Trigonal planar
d) Tetrahedral - According to VSEPR theory, lone pairs:
a) Do not affect molecular geometry
b) Increase bond angles
c) Decrease bond angles
d) Make molecule linear - BF₃ is:
a) Polar
b) Nonpolar
c) Ionic
d) Metallic - CO₂ is:
a) Polar
b) Nonpolar
c) Ionic
d) Metallic
Hybridization (30–35)
- Carbon in CH₄ is:
a) sp
b) sp²
c) sp³
d) sp³d - Carbon in C₂H₄ is:
a) sp³
b) sp²
c) sp
d) sp³d² - Carbon in C₂H₂ is:
a) sp³
b) sp²
c) sp
d) sp³d - PCl₅ shows which hybridization?
a) sp³
b) sp³d
c) sp²
d) sp³d² - SF₆ shows which hybridization?
a) sp³
b) sp³d
c) sp³d²
d) sp² - NH₃ is:
a) sp³ hybridized
b) sp² hybridized
c) sp hybridized
d) sp³d² hybridized
Molecular Orbital Theory & Bonding in Diatomics (36–40)
- The bond order of O₂ is:
a) 1
b) 2
c) 3
d) 1.5 - Paramagnetic molecules have:
a) All paired electrons
b) Unpaired electrons
c) No electrons
d) Ionic bonds - Diamagnetic molecules have:
a) All paired electrons
b) Unpaired electrons
c) One unpaired electron
d) Ionic bonds - The bond order of N₂ is:
a) 1
b) 2
c) 3
d) 4 - Molecules like Be₂ exist because:
a) Bond order > 0
b) Bond order = 0
c) High electronegativity
d) Ionic bonding
Answer Key – Class 11 Chemistry: Chemical Bonding and Molecular Structure (40 MCQs)
Ionic Bonding (1–6)
- b) Transfer of electrons – Ionic bonds form by complete transfer of electrons from metal to nonmetal.
- b) NaCl – Classic example of ionic compound.
- c) Both a & b – Lattice energy depends on charges and ionic radii.
- b) Good conductors in molten/aqueous state – Ions free to move in liquid/solution.
- b) MgO – Highest lattice energy due to +2 and –2 charges and small ionic radii.
- a) Greater electronegativity difference – Larger difference → more ionic character.
Covalent Bonding (7–13)
- a) Sharing of electrons – Covalent bonds result from electron sharing.
- c) Valence electrons and bonds – Lewis structures depict bonds and lone pairs.
- b) BF₃ – Boron has only 6 electrons → incomplete octet.
- b) Multiple equivalent structures can be drawn – Resonance concept.
- b) 2 – O₂ has double bond → bond order = 2.
- b) Double bond – CO₂ has two C=O double bonds.
- c) Pure covalent bond – Electronegativity difference < 0.5 indicates nonpolar covalent bond.
Bond Parameters (14–18)
- a) Distance between nuclei of two bonded atoms – Definition of bond length.
- c) C≡C – Triple bond shortest due to stronger attraction.
- b) Energy required to break 1 mole of bonds – Definition of bond energy.
- c) Both a & b – Higher bond order → shorter and stronger bond.
- a) O₂ – Double bond → bond order 2.
Polar/Nonpolar Molecules & Electronegativity (19–23)
- b) Unequal sharing of electrons – Polar covalent bond has dipole moment.
- a) Zero – Nonpolar molecules have no net dipole.
- a) Polar – HCl has dipole from H → Cl.
- c) F – Fluorine is most electronegative element.
- a) Soluble in polar solvents – Polar molecules dissolve in polar solvents.
VSEPR Theory & Molecular Geometry (24–29)
- c) Tetrahedral – CH₄ has 4 bonded pairs → tetrahedral.
- a) Trigonal pyramidal – NH₃ has 3 bonded pairs + 1 lone pair.
- b) Bent – H₂O has 2 bonded pairs + 2 lone pairs.
- c) Decrease bond angles – Lone pairs repel more → reduce angles.
- b) Nonpolar – BF₃ symmetric → no dipole.
- b) Nonpolar – CO₂ linear and symmetric → no dipole.
Hybridization (30–35)
- c) sp³ – CH₄ carbon forms 4 sigma bonds → sp³ hybridized.
- b) sp² – C₂H₄ carbon forms 3 sigma + 1 pi bond → sp².
- c) sp – C₂H₂ carbon forms 2 sigma + 2 pi bonds → sp.
- b) sp³d – PCl₅ central P → 5 sigma bonds → sp³d.
- c) sp³d² – SF₆ central S → 6 sigma bonds → sp³d².
- a) sp³ hybridized – NH₃ central N → 3 sigma + 1 lone pair → sp³.
Molecular Orbital Theory & Diatomics (36–40)
- b) 2 – O₂ bond order = (10 bonding – 6 antibonding)/2 = 2.
- b) Unpaired electrons – Paramagnetic species have unpaired electrons.
- a) All paired electrons – Diamagnetic species.
- c) 3 – N₂ bond order = 3 → triple bond.
- b) Bond order = 0 – Be₂ bond order = 0 → molecule unstable in ground state.
Disclaimer:
All MCQs on this page are created for educational purposes only. They are intended for practice and NEET/Class 11 Chemistry preparation and do not guarantee any specific exam results.