# NCERT solutions for Chemistry Part 1 and 2 Class 11 chapter 4 - Chemical Bonding and Molecular Structure [Latest edition]

## Chapter 4: Chemical Bonding and Molecular Structure

EXERCISES
EXERCISES [Pages 133 - 135]

### NCERT solutions for Chemistry Part 1 and 2 Class 11 Chapter 4 Chemical Bonding and Molecular StructureEXERCISES [Pages 133 - 135]

EXERCISES | Q 4.1 | Page 133

Explain the Formation of a Chemical Bond.

EXERCISES | Q 4.2 | Page 133

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

EXERCISES | Q 4.3 - (a) | Page 133

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

EXERCISES | Q 4.3 - (b) | Page 133

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

EXERCISES | Q 4.3 - (c) | Page 133

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

EXERCISES | Q 4.4 - (a) | Page 133

Draw the Lewis structures for the following molecule and ion:

H2S

EXERCISES | Q 4.4 - (b) | Page 133

Draw the Lewis structures for the given molecule and ion:

SiCl4

EXERCISES | Q 4.4 - (c) | Page 133

Draw the Lewis structures for the given molecule and ion:

BeF2

EXERCISES | Q 4.4 - (d) | Page 133

Draw the Lewis structures for the given molecule and ion:

"CO"_3^(2-)

EXERCISES | Q 4.4 - (e) | Page 133

Draw the Lewis structures for the following molecule and ion:

HCOOH

EXERCISES | Q 4.5 - (a) | Page 134

Define octet rule.

EXERCISES | Q 4.5 - (b) | Page 134

Write the significance and limitations of octet rule.

EXERCISES | Q 4.6 | Page 134

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

EXERCISES | Q 4.7 | Page 134

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

BeCl2, BCl3, SiCl4, AsF5, H2S, PH3

EXERCISES | Q 4.8 | Page 134

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

EXERCISES | Q 4.9 | Page 134

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

EXERCISES | Q 4.10 | Page 134

Define the bond length.

EXERCISES | Q 4.11 | Page 134

Explain the important aspects of resonance with reference to the "CO"_3^(2-) ion.

EXERCISES | Q 4.12 | Page 134

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.

 (1) (2)
EXERCISES | Q 4.13 - (a) | Page 134

Write the resonance structure for SO3.

EXERCISES | Q 4.13 - (b) | Page 134

Write the resonance structures for NO2.

EXERCISES | Q 4.13 - (c) | Page 134

Write the resonance structures for "NO"_3^(-).

EXERCISES | Q 4.14 - (a) | Page 134

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

K and S

EXERCISES | Q 4.14 - (b) | Page 134

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

Ca and O

EXERCISES | Q 4.14 - (c) | Page 134

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

Al and N

EXERCISES | Q 4.15 | Page 134

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.

EXERCISES | Q 4.16 | Page 134

Write the significance/applications of dipole moment.

EXERCISES | Q 4.17 - (a) | Page 134

Define electronegativity.

EXERCISES | Q 4.17 - (b) | Page 134

How does electronegativity differ from electron gain enthalpy?

EXERCISES | Q 4.18 | Page 134

Explain with the help of suitable example polar covalent bond.

EXERCISES | Q 4.19 | Page 134

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

EXERCISES | Q 4.20 | Page 134

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.

EXERCISES | Q 4.21 | Page 134

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?

EXERCISES | Q 4.22 | Page 134

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

EXERCISES | Q 4.23 | Page 134

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

EXERCISES | Q 4.24 - (a) | Page 134

What is meant by hybridisation of atomic orbitals?

EXERCISES | Q 4.24 | Page 134

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

EXERCISES | Q 4.25 | Page 135

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

$\ce{AlCl_3 + Cl- -> AlCl_4-}$

EXERCISES | Q 4.26 | Page 135

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

$\ce{BF3 + NH3 → F3B.NH3}$

EXERCISES | Q 4.27 | Page 135

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

EXERCISES | Q 4.28 | Page 135

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

(a) C2H2 (b) C2H4

EXERCISES | Q 4.29 | Page 135

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

EXERCISES | Q 4.30 | Page 135

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

EXERCISES | Q 4.31 | Page 135

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

EXERCISES | Q 4.32 | Page 135

Distinguish between a sigma and a pi bond.

EXERCISES | Q 4.33 | Page 135

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

EXERCISES | Q 4.34 | Page 135

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

EXERCISES | Q 4.35 | Page 135

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

EXERCISES | Q 4.36 | Page 135

Compare the relative stability of the following species and indicate their magnetic properties;

"O"_2, "O"_2^+, "O"_2^-(superoxide), "O"_2^(2-)(peroxide)

EXERCISES | Q 4.37 | Page 135

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

EXERCISES | Q 4.38 | Page 135

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

EXERCISES | Q 4.39 | Page 135

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

EXERCISES | Q 4.40 | Page 135

What is meant by the term bond order? Calculate the bond order of: N2, O2, "O"_2^+and "O"_2^-?

EXERCISES

## NCERT solutions for Chemistry Part 1 and 2 Class 11 chapter 4 - Chemical Bonding and Molecular Structure

NCERT solutions for Chemistry Part 1 and 2 Class 11 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 Chemistry Part 1 and 2 Class 11 solutions in a manner that help students grasp basic concepts better and faster.

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Concepts covered in Chemistry Part 1 and 2 Class 11 chapter 4 Chemical Bonding and Molecular Structure are Kossel and Lewis Approach to Chemical Bonding, Kossel-lewis Approach to Chemical Bonding - Octet Rule, Kossel-lewis Approach to Chemical Bonding - Covalent Bond, Lewis Structures (Lewis Representation of Simple Molecules), Kossel-lewis Approach to Chemical Bonding - Formal Charge, Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule, Ionic or Electrovalent Bond, Bond Length, Bond Angle, Bond Enthalpy, Bond Order, Resonance Structures, Polarity of Bonds, Valence Shell Electron Pair Repulsion Theory (VSEPR), 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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