Class 11 Chemistry MCQ Chapter 4 Chemical Bonding and Molecular Structure
Welcome to Class 11 Chemistry MCQ Chapter 4 Chemical Bonding and Molecular Structure English Medium. This article contains important multiple-choice questions (MCQs) with answers to help AHSEC Higher Secondary First Year students strengthen their Chemistry preparation.
The chapter Chemical Bonding and Molecular Structure explains how atoms combine to form molecules and compounds. Students will learn about ionic bonds, covalent bonds, coordinate bonds, Lewis structures, VSEPR theory, hybridization, molecular geometry, and intermolecular forces. These concepts are among the most important topics in Class 11 Chemistry and provide the foundation for understanding chemical reactions and molecular behavior.
All MCQs are prepared according to the latest AHSEC syllabus and examination pattern. These questions are designed to help students revise key concepts, improve their understanding, and become familiar with the types of objective questions asked in examinations.
Whether you are preparing for class tests, annual examinations, or the AHSEC HS First Year Final Examination, these MCQ solutions will help you build confidence and achieve better results in Chemistry.
Part: I
Chemical Bonding and Molecular Structure
Selected VSA & MCQ
I. Very Short Answer Questions (VSA)
Q What is a chemical bond?
Ans: Force of attraction that holds atoms together in a molecule.
Q What is ionic bond?
Ans: Bond formed by transfer of electrons.
Q What is covalent bond?
Ans: Bond formed by sharing of electrons.
Q What is coordinate bond?
Ans: Covalent bond where one atom donates both electrons.
Q What is valence shell?
Ans: Outermost shell of an atom.
Q What is octet rule?
Ans: Atoms tend to complete eight electrons in valence shell.
Q What is electronegativity?
Ans: Ability to attract bonding electrons.
Q What is bond length?
Ans: Distance between nuclei of bonded atoms.
Q What is bond angle?
Ans: Angle between two bonds.
Q What is bond energy?
Ans: Energy required to break a bond.
Q What is dipole moment?
Ans: Measure of polarity of a bond.
Q What is hybridisation?
Ans: Mixing of atomic orbitals to form new orbitals.
Q What is sp hybridisation?
Ans: Mixing of one s and one p orbital.
Q What is sp² hybridisation?
Ans: Mixing of one s and two p orbitals.
Q What is sp³ hybridisation?
Ans: Mixing of one s and three p orbitals.
Q What is VSEPR theory?
Ans: Predicts shape based on electron pair repulsion.
Q What is sigma bond?
Ans: Bond formed by head-on overlap.
Q What is pi bond?
Ans: Bond formed by sidewise overlap.
Q What is polarity?
Ans: Separation of charge in a bond.
Q What is hydrogen bond?
Ans: Weak attraction between H and electronegative atom.
Q What is lattice energy?
Ans: Energy released when ions form solid lattice.
Q What is resonance?
Ans: Delocalisation of electrons in molecule.
Q What is formal charge?
Ans: Charge assigned to atom in molecule.
Q What is bond order?
Ans: Number of bonds between atoms.
Q What is molecular geometry?
Ans: Spatial arrangement of atoms.
Q What is linear shape?
Ans: Atoms arranged in straight line.
Q What is trigonal planar shape?
Ans: Three atoms in a plane at 120°.
Q What is tetrahedral shape?
Ans: Four atoms arranged at 109.5°.
Q What is bent shape?
Ans: Angular shape due to lone pairs.
Q What is lone pair?
Ans: Pair of electrons not involved in bonding.
II. Multiple Choice Questions (MCQs)
Q Ionic bond is formed by:
(a) sharing electrons
(b) transfer of electrons
(c) overlap
(d) attraction
Ans: (b)
Q Covalent bond involves:
(a) transfer
(b) sharing
(c) loss
(d) gain
Ans: (b)
Q Octet rule states:
(a) 2 electrons
(b) 8 electrons
(c) 6 electrons
(d) 10 electrons
Ans: (b)
Q Bond length is:
(a) angle
(b) energy
(c) distance
(d) charge
Ans: (c)
Q Sigma bond is formed by:
(a) side overlap
(b) head-on overlap
(c) no overlap
(d) ionic
Ans: (b)
Q Pi bond is formed by:
(a) head-on
(b) sidewise
(c) ionic
(d) none
Ans: (b)
Q Hybridisation explains:
(a) energy
(b) shape
(c) charge
(d) mass
Ans: (b)
Q sp³ hybridisation gives:
(a) linear
(b) trigonal
(c) tetrahedral
(d) bent
Ans: (c)
Q VSEPR theory is based on:
(a) attraction
(b) repulsion
(c) energy
(d) mass
Ans: (b)
Q Dipole moment measures:
(a) mass
(b) polarity
(c) energy
(d) charge
Ans: (b)
Q Hydrogen bond is:
(a) strong
(b) weak
(c) ionic
(d) covalent
Ans: (b)
Q Bond energy indicates:
(a) strength
(b) length
(c) angle
(d) charge
Ans: (a)
Q Lone pair affects:
(a) shape
(b) mass
(c) energy
(d) size
Ans: (a)
Q Bond angle in tetrahedral is:
(a) 90°
(b) 120°
(c) 109.5°
(d) 180°
Ans: (c)
Q Linear shape angle is:
(a) 90°
(b) 120°
(c) 109°
(d) 180°
Ans: (d)
Q Trigonal planar angle is:
(a) 90°
(b) 120°
(c) 109°
(d) 180°
Ans: (b)
Q Resonance stabilises molecule by:
(a) localisation
(b) delocalisation
(c) energy increase
(d) none
Ans: (b)
Q Coordinate bond has:
(a) one donor
(b) two donors
(c) none
(d) transfer
Ans: (a)
Q Ionic compounds have:
(a) low melting
(b) high melting
(c) low boiling
(d) none
Ans: (b)
Q Covalent compounds are:
(a) hard
(b) soft
(c) ionic
(d) metallic
Ans: (b)
Q Bond order increases with:
(a) stability
(b) instability
(c) size
(d) none
Ans: (a)
Q Formal charge helps in:
(a) stability prediction
(b) shape
(c) mass
(d) none
Ans: (a)
Q Polar molecule has:
(a) zero dipole
(b) non-zero dipole
(c) no bond
(d) none
Ans: (b)
Q Non-polar molecule has:
(a) dipole
(b) no dipole
(c) ionic bond
(d) none
Ans: (b)
Q Overlap forms:
(a) bond
(b) charge
(c) energy
(d) none
Ans: (a)
Q Lattice energy is:
(a) energy released
(b) absorbed
(c) neutral
(d) none
Ans: (a)
Q Bent shape due to:
(a) bonding
(b) lone pairs
(c) atoms
(d) none
Ans: (b)
Q Sigma bond is stronger than pi bond because:
(a) less overlap
(b) more overlap
(c) no overlap
(d) none
Ans: (b)
Q Number of sigma bonds in double bond is:
(a) 2
(b) 1
(c) 3
(d) 0
Ans: (b)
Q Assertion: Ionic bonds are strong.
Reason: Strong electrostatic forces exist between ions.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (b)
Q Assertion: Covalent compounds have low melting points.
Reason: They have weak intermolecular forces.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (a)
Q Assertion: Lone pairs affect molecular shape.
Reason: They repel more strongly than bond pairs.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (d)
Q Assertion: Sigma bonds are stronger than pi bonds.
Reason: Sigma bonds involve greater overlap.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (a)
Q Assertion: Resonance increases stability.
Reason: Electrons are delocalised.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (c)
Q Assertion: Polar molecules have dipole moment.
Reason: Unequal sharing of electrons occurs.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (a)
Q Assertion: Hybridisation explains geometry.
Reason: Orbitals mix to form equivalent orbitals.
(a) Both A and R are true, and R is the correct explanation of A
(b) Both A and R are true, but R is not the correct explanation of A
(c) A is true, but R is false
(d) A is false, but R is true
Ans: (b)
