# NCERT solutions for Class 11 Chemistry Textbook chapter 4 - Chemical Bonding and Molecular Structure [Latest edition]

## Chapter 4: Chemical Bonding and Molecular Structure

[Pages 129 - 131]

### NCERT solutions for Class 11 Chemistry Textbook Chapter 4 Chemical Bonding and Molecular Structure[Pages 129 - 131]

Q 1 | Page 129

Explain the Formation of a Chemical Bond.

Q 2 | Page 129

Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.

Q 3.1 | Page 129

Write Lewis symbols for the following atoms and ions: S and S2–

Q 3.2 | Page 129

Write Lewis symbols for the following atoms and ions: Al and Al3+

Q 3.3 | Page 129

Write Lewis symbols for the following atoms and ions H and H

Q 4.1 | Page 129

Draw the Lewis structures for the following molecules and ions: H2S

Q 4.2 | Page 129

Draw the Lewis structures for the given molecules and ions: SiCl4

Q 4.3 | Page 129

Draw the Lewis structures for the given molecules and ions BeF2

Q 4.4 | Page 129

Draw the Lewis structures for the given molecules and ions CO_3^(2-)

Q 4.5 | Page 129

Draw the Lewis structures for the following molecules and ions HCOOH

Q 5.1 | Page 129

Define octet rule

Q 5.2 | Page 129

Write its significance and limitations octet rule

Q 6 | Page 129

Write the favourable factors for the formation of the ionic bond.

Q 7 | Page 130

Discuss the shape of the following molecules using the VSEPR model:

BeCl2, BCl3, SiCl4, AsF5, H2S, PH3

Q 8 | Page 130

Although geometries of NH3 and H2O molecules are distorted tetrahedral, bond angle in water is less than that of ammonia. Discuss.

Q 9 | Page 130

How do you express the bond strength in terms of bond order?

Q 10 | Page 130

Define the bond length.

Q 11 | Page 130

Explain the important aspects of resonance with reference to the CO_3^(2-) ion.

Q 12 | Page 130

H3PO3 can be represented by structures 1 and 2 shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing H3PO3? If not, give reasons for the same.

Q 13.1 | Page 130

Write the resonance structures for SO3

Q 13.2 | Page 130

Write the resonance structures for NO2

Q 13.3 | Page 130

Write the resonance structures for NO_3^(-)

Q 14.1 | Page 130

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:-

K and S

Q 14.2 | Page 130

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:

Ca and O

Q 14.3 | Page 130

Use Lewis symbols to show electron transfer between the following atoms to form cations and anions:

Al and N

Q 15 | Page 130

Although both CO2 and H2O are triatomic molecules, the shape of H2O molecule is bent while that of CO2 is linear. Explain this on the basis of dipole moment.

Q 16 | Page 130

Write the significance/applications of dipole moment.

Q 17.1 | Page 130

Define electronegativity

Q 17.2 | Page 130

How does electronegativity differ from electron gain enthalpy?

Q 18 | Page 130

Explain with the help of suitable example polar covalent bond.

Q 19 | Page 130

Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.

Q 20 | Page 130

The skeletal structure of CH3COOH as shown below is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid.

Q 21 | Page 130

Apart from tetrahedral geometry, another possible geometry for CH4 is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why CH4 is not square planar?

Q 22 | Page 130

Explain why BeH2 molecule has a zero dipole moment although the Be–H bonds are polar.

Q 23 | Page 130

Which out of NH3 and NF3 has higher dipole moment and why?

Q 24.1 | Page 130

What is meant by hybridisation of atomic orbitals?

Q 24.2 | Page 130

Describe the shapes of sp, sp2,sp3 hybrid orbitals.

Q 25 | Page 130

Describe the change in hybridisation (if any) of the Al atom in the following reaction.

AlCl_3 + Cl^(-) -> AlCl_4^(-)

Q 26 | Page 130

Is there any change in the hybridisation of B and N atoms as a result of the following reaction?

BF3 + NH3 → F3B.NH3

Q 27 | Page 131

Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in C2H4 and C2H2 molecules.

Q 28 | Page 131

What is the total number of sigma and pi bonds in the following molecules?

(a) C2H2 (b) C2H4

Q 29 | Page 131

Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why? (a) 1and 1(b) 1and 2px (c) 2py and 2py (d) 1and 2s.

Q 30 | Page 131

Which hybrid orbitals are used by carbon atoms in the following molecules?

CH3–CH3; (b) CH3–CH=CH2; (c) CH3-CH2-OH; (d) CH3-CHO (e) CH3COOH

Q 31 | Page 131

What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.

Q 32 | Page 131

Distinguish between a sigma and a pi bond.

Q 33 | Page 131

Explain the formation of H2 molecule on the basis of valence bond theory.

Q 34 | Page 131

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

Q 35 | Page 131

Use molecular orbital theory to explain why the Be2 molecule does not exist.

Q 36 | Page 131

Compare the relative stability of the following species and indicate their magnetic properties; O_2, O_2^+, O_2^-(superoxide), O_2^(2-)(peroxide)

Q 37 | Page 131

Write the significance of a plus and a minus sign shown in representing the orbitals.

Q 38 | Page 131

Describe the hybridisation in case of PCl5. Why are the axial bonds longer as compared to equatorial bonds?

Q 39 | Page 131

Define hydrogen bond. Is it weaker or stronger than the van der Waals forces?

Q 40 | Page 131

What is meant by the term bond order? Calculate the bond order of: N2, O2, O_2^+and O_2^-

## NCERT solutions for Class 11 Chemistry Textbook chapter 4 - Chemical Bonding and Molecular Structure

NCERT solutions for Class 11 Chemistry Textbook chapter 4 (Chemical Bonding and Molecular Structure) include all questions with solution and detail explanation. This will clear students doubts about any question and improve application skills while preparing for board exams. The detailed, step-by-step solutions will help you understand the concepts better and clear your confusions, if any. Shaalaa.com has the CBSE Class 11 Chemistry Textbook solutions in a manner that help students grasp basic concepts better and faster.

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Concepts covered in Class 11 Chemistry Textbook chapter 4 Chemical Bonding and Molecular Structure are Concept of Kossel-lewis Approach to Chemical Bonding, Kossel-lewis Approach to Chemical Bonding - Octet Rule, Kossel-lewis Approach to Chemical Bonding - Covalent Bond, Kossel-lewis Approach to Chemical Bonding - Lewis Representation of Simple Molecules (The Lewis Structures), Kossel-lewis Approach to Chemical Bonding - Formal Charge, Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule, Concept of Ionic Or Electrovalent Bond, Bond Length, Bond Angle, Bond Enthalpy, Bond Order, Resonance Structures, Polarity of Bonds, The Valence Shell Electron Pair Repulsion (Vsepr) Theory, Valence Bond Theory, Valence Bond Theory - Orbital Overlap Concept, Valence Bond Theory - Directional Properties of Bonds, Valence Bond Theory - Overlapping of Atomic Orbitals, Valence Bond Theory - Types of Overlapping and Nature of Covalent Bonds, Valence Bond Theory - Strength of Sigma and Pi Bonds, Hybridisation - Introduction, Types of Hybridisation, Hybridisation of Elements Involving d Orbitals, Molecular Orbital Theory - Introduction, Formation of Molecular Orbitals - Linear Combination of Atomic Orbitals (Lcao), Conditions for the Combination of Atomic Orbitals, Types of Molecular Orbitals, Energy Level Diagram for Molecular Orbitals, Electronic Configuration and Molecular Behaviour, Bonding in Some Homonuclear Diatomic Molecules, Hydrogen Bonding - Introduction, Cause of Formation of Hydrogen Bond, Types of H-Bonds, Chemical Bonding and Molecular Structure Numericals, States of Matter:- Gases and Liquids Numericals.

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