LESSON PLAN
Teacher’s Name
Unit/Chapter
6,Chemical
Bonding
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.0 to6.2.1)Introduction, Causes of
chemical combination,Energetics of
Bond formation, Atomic Sizes
Class
XI
Date
Essential Prior Knowledge: Students already know about Ionic Bond & covalent bond,
The Aims of the Lesson:
Students will be able to explain the Causes of chemical combination, Energetics of Bond
formation, Atomic Sizes
Introduction: All the elements except noble gases combine with one another due to an
inherent tendency to stabilize themselves. They get their stabilization by losing, gaining
or sharing electrons to attain the nearest noble gas configuration The tendency of atoms
to attain a maximum of eight electrons in the valence shell is known as the ‘octet rule’.
Lesson Development:
DLO # 1: Student will be able to explain the causes of chemical combination &
Energetics of Bond formation
Procedure and Treatment:
 Causes of chemical combination will be explained to the students with the help of
table6.1.
 Energetics of Bond formation will be discussed with the students with the help of
fig6.1
DLO # 2: Student will be able to explain the Atomic sizes
Procedure and Treatment:
 Atomic radii will be explained to the students
 Variation of Atomic radii in the periodic table will be discussed.
DLO # 3: Student will be able to explain the ionic radii & covalent radii.
Procedure and Treatment:
 Ionic radii will be explained to the students with the help of fig6.2
 Covalent radii will be explained to the students with the help of fig 6.3
Board Summary:
Name of the Chapter, Names the topics, Fig6.1, 6.2 & 6.3
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
Explain potential energy curve for the formation of H2 molecule.
What are the difference b/w atomic radii & ionic radii?
Home Work
Learn the topics at home
Conclusion
In this lecture we learnt about the Causes of chemical combination, Energetics of Bond
formation, Atomic Sizes.
In next we will learn about the Ionization Energy, Electron Affinity & Electronegativity
LESSON PLAN
Teacher’s Name
Unit/Chapter
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.3) Ionization Energy, Electron Affinity &
6,Chemical
Bonding
Class
XI
Date
Electronegativity
Essential Prior Knowledge: Students already have the knowledge of arrangements of
elements in periodic table.
The Aims of the Lesson:
Students will be able to explain the Ionization Energy, Electron Affinity &
Electronegativity
Introduction: All the elements except noble gases combine with one another due to an
inherent tendency to stabilize themselves. They get their stabilization by losing, gaining
or sharing electrons to attain the nearest noble gas configuration The tendency of atoms
to attain a maximum of eight electrons in the valence shell is known as the ‘octet rule’.
Lesson Development:
DLO # 1: Student will be able to explain the term Ionization Energy
Procedure and Treatment:
 The process of Ionization Energy will be explained to the students.
 Factors Influencing the Ionization Energies will be discussed with the students
with the help of Table6.3.
 Variation of Ionization Energy in the Periodic Table will be discussed.
DLO # 2: Student will be able to explain the term Electron Affinity.
Procedure and Treatment:
 The process of Electron Affinity will be explained to the students.
 Factors Influencing the Electron Affinity will be discussed with the students with
the help of Table6.3.
 Variation of Electron Affinity in the Periodic Table will be discussed.
DLO # 3: Student will be able to explain the term Electronegativity.
Procedure and Treatment:
 The process of Electronegativity will be explained to the students.
 Variation of Electronegativity in the Periodic Table will be discussed with the help
of Table6.3.
Board Summary:
Name of the Chapter, Names of topics.
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
Explain the terms Ionization Energy, Electron Affinity & Electronegativity
Home Work
Learn the topics at home
Conclusion
In this lecture we learnt about the Ionization Energy, Electron Affinity & Electronegativity.
In next we will learn about the Types of Bonds.
LESSON PLAN
Teacher’s Name
Unit/Chapter
6,Chemical
Bonding
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4) Types of Bonds(Ionic & Covalent
Class
XI
Date
Bonds)
Essential Prior Knowledge: Students already have the knowledge of arrangements of
elements in periodic table.
The Aims of the Lesson:
Students will be able to explain the Types of Bonds i.e. Ionic & Covalent Bonds.
Introduction: All the elements except noble gases combine with one another due to an
inherent tendency to stabilize themselves. They get their stabilization by losing, gaining
or sharing electrons to attain the nearest noble gas configuration The tendency of atoms
to attain a maximum of eight electrons in the valence shell is known as the ‘octet rule’.
Lesson Development:
DLO # 1: Student will be able to explain the term Ionic Bond
Procedure and Treatment:
 Lewis Concept will be explained to the students.
 The term Ionic bond will be explained to the students.
 Examples of NaCl & KCl will be given.
DLO # 2: Student will be able to explain the term Covalent bond (electron pair bond).
Procedure and Treatment:
 The term Ionic bond will be explained to the students.
 Non polar & polar covalent bonds will be explained to the students.
 Examples of covalent compounds will be given
DLO # 3: Student will be able to write the Lewis Structures of the covalent compounds.
Procedure and Treatment:
 Writing of Lewis structure of different compounds will be explained to the
students.
 Structures of Covalent compounds on page #164 & 165 will be discussed with
the students
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds.
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
Explain the term Ionic Bond
Explain the term Covalent Bond
Home Work
Do Q#6 on page#193 of the text book
Conclusion
In this lecture we learnt about the Ionic & Covalent Bonds.
In next we will learn about the Coordinate covalent bond.
LESSON PLAN
Teacher’s Name
Unit/Chapter
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4) Types of Bonds(Coordinate covalent
6,Chemical
Bonding
Class
XI
Date
bonds & the Limitations of Lewis Model)
Essential Prior Knowledge: Students already have the knowledge of the other types of
Bonds i.e. Ionic & Covalent Bonds.
The Aims of the Lesson:
Students will be able to explain the Coordinate Covalent Bonds & the Limitations of
Lewis Model.
Introduction: All the elements except noble gases combine with one another due to an
inherent tendency to stabilize themselves. They get their stabilization by losing, gaining
or sharing electrons to attain the nearest noble gas configuration The tendency of atoms
to attain a maximum of eight electrons in the valence shell is known as the ‘octet rule’.
Lesson Development:
DLO # 1: Student will be able to explain the term Coordinate Covalent Bond
Procedure and Treatment:
.
 Coordinate Covalent bond will be explained to the students.
 Examples of NH4Cl & H3O+will be given.
DLO # 2: Student will be able to write the Lewis Structures of the Coordinate covalent
compounds.
Procedure and Treatment:
 Writing of Lewis structure of different compounds will be explained to the
students.
 Structures of Coordinate Covalent compounds on page #166 will be discussed
with the students
DLO # 3: Student will be able to explain the Limitations of Lewis Model(Modern
Theories).
Procedure and Treatment:
 Limitations of Lewis Model will be explained to the students.
 Names of the different Modern Theories will be given to the students.
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds.
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
Explain the term Coordinate covalent bond
How these bonds are formed?
Home Work
Read the topic at home.
Conclusion
In this lecture we learnt about the Coordinate covalent bonds & the Limitations of Lewis
Model
In next we will learn about the Modern Theories of Covalent compounds.
LESSON PLAN
Teacher’s Name
Unit/Chapter
6,Chemical
Bonding
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4.3) Modern Theories (Valence Shell
Class
XI
Date
Electron Pair Repulsion Theory).
Essential Prior Knowledge: Students already have the knowledge of Covalent Bonds.
The Aims of the Lesson:
Students will be able to explain the Modern Theories (Valence Shell Electron Pair
Repulsion Theory).
.
Introduction: Sidgwick & Powell (1940) Pointed out that the shape of molecules could
be interpreted in terms of electron pairs in outer orbit of the central atom.Nylholm &
Gillespie developed VSEPR Theory, Which explains the shapes of molecules for nontransition elements.
Lesson Development:
DLO # 1: Student will be able to explain the Postulates of VSEPR Theory
Procedure and Treatment:
 Basic Assumption of the theory will be given.
 Postulates of VSEPR Theory will be explained to the students.
DLO # 2: Student will be able to understand the shapes of molecules according to
VSEPR Theory.
Procedure and Treatment:
 Table6.4 will be discussed with the students
 Type AB2,AB3, AB4 will be discussed with the students one by one.
DLO # 3: Student will be able to draw the structures of different molecules according to
VSEPR Theory.
Procedure and Treatment:
 Examples on page#169 will be explained one by one
 Q#8 will be solved to make clear understanding of the topic.
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds.
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
Give the Postulates of VSEPR Theory
Home Work
Read the topic at home.
Conclusion
In this lecture we learnt about the Postulates of VSEPR Theory
In next we will learn about the VBT.
LESSON PLAN
Teacher’s Name
Unit/Chapter
6,Chemical
Bonding
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4.3) Modern Theories (Valence Bond
Class
XI
Date
Theory, Atomic orbital hybridization).
Essential Prior Knowledge: Students already have the knowledge of Covalent Bonds
& Valence Shell Electron Pair Repulsion Theory.
The Aims of the Lesson:
Students will be able to explain the Modern Theories (Valence Bond Theory).
.
Introduction: VSEPR Theory predicts & explains the shapes of the molecule but does
not give reasons for the formation of bonds. VBT is concerned with both the formation of
bonds & the shapes of molecules. This method of describing a covalent bon considers
the molecule as a combination of atoms
Lesson Development:
DLO # 1: Student will be able to explain the Valence Bond Theory
Procedure and Treatment:
 Students will be told that how single bond is formed with the help of fig6.4
 Students will be given the concept of overlapping of orbitals.
DLO # 2: Student will be able to explain the Limitation of Valence Bond Theory
Procedure and Treatment:
 Students will be told about the limitations of VBT
 Bonding in H2S will be discussed.
DLO # 3: Student will be able to explain the concept of Hybridization in Atomic orbitals.
Procedure and Treatment:
 Concept of Hybridization will be given to the students.
 Types of Hybridization will be told to the students.
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds, fig6.4, 6.5, 6.6, 6.7,
6.8, and 6.9.
Recapitulation:
Quick recap of the lesson will be done.
Consolidation:
What is the basis of VBT?
Home Work
Read the topic at home.
Conclusion
In this lecture we learnt about the VBT & Hybridization.
In next we will learn about the Types of hybridization.
LESSON PLAN
Teacher’s Name
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.5.4) Dipole Moment & Molecular
Unit/Chapter
6,Chemical
Bonding
Class
XI
Date
Structure
Essential Prior Knowledge: Students already have the knowledge of Ionic Bond &
Covalent Bond.
The Aims of the Lesson:
Students will be able to explain the Dipole Moment & Molecular Structure.
Introduction: For homonuclear diatomic molecule e.g. H2, the bonding pair of electron is
equally shared b/w the atoms. On the other hand, in bond b/w dissimilar atoms such as
in HF, the electron density of the bonding electrons lies more toward the fluorine atom
than towards the hydrogen atoms.
Lesson Development:
DLO # 1: Students will be able to explain the Dipole Moment in a chemical bond.
Procedure and Treatment:
 Dipole Moment will be explained to the students
 Dipole Moment in different bonds will be explained.
 Table6.8 will be explained.
DLO # 2: Student will be able to determine the Percentage Ionic character of a bond.
Procedure and Treatment:
 Students will be told that how Percentage Ionic character of a bond is
determined.

DLO # 3: Student will be able to explain the
Procedure and Treatment:
 .
Board Summary:
Name of the Chapter, Names of topics Table 6.6 &6.7.
Recapitulation:
Quick recap of the lesson will be done.
LESSON PLAN
Teacher’s Name
Unit/Chapter
6,Chemical
Bonding
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4.5) Atomic Orbital Hybridization &
Class
XI
Date
Shape Of the Molecule.
Essential Prior Knowledge: Students already have the knowledge of Concept of
Hybridization.
The Aims of the Lesson:
Students will be able to explain sp3, sp2 &sp type of Hybridization.
.
Introduction: Atomic orbitals differing slightly in energy intermix to form new orbitals,
which are called hybrid atomic orbitals. They differ from the parent atomic orbitals in
shape & possess specific geometry. Depending upon number & nature of the orbitals,
participating in hybridization, different types of hybridization take place. For example s &
p orbitals simple atoms are hybridized to give sp3, sp2 & sp hybrid orbitals.
Lesson Development:
DLO # 1: Student will be able to explain the sp3 Hybridization.
Procedure and Treatment:
 Students will be told that how sp3 hybridization takes place
 Examples will be explained..
DLO # 2: Student will be able to explain the sp2 Hybridization.
Procedure and Treatment:
 Students will be told that how sp 2 hybridization takes place
 Examples will be explained
DLO # 3: Student will be able to explain the sp Hybridization.
Procedure and Treatment:
 Students will be told that how sp hybridization takes place
 Examples will be explained
.
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds,
fig6.10,6.11,6.12,6.13,6.14,6.15,6.16,6.17,6.18
LESSON PLAN
Teacher’s Name
Unit/Chapter
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.4.6) Molecular Orbital Theory
Class
XI
Date
6,Chemical
Bonding
Essential Prior Knowledge: Students already have the knowledge of Concept of
Hybridization.
The Aims of the Lesson:
Students will be able to explain the Molecular Orbital Theory.
.
Introduction: The molecular orbital approach considers the whole molecule as a single
unit. It assumes that the atomic orbital of the combining atoms overlap to form new
orbitals called molecular orbitals which are characteristics of the whole molecule.
Lesson Development:
DLO # 1: Students will be able to explain the Head on Approach & Side way approach.
Procedure and Treatment:
 Formation of molecular orbitals from p-orbitals will be explained to the students
 Fig6.20 &6.21 will be discussed.
DLO # 2: Student will be able to expla0in the Relative energies of the molecular Orbitals.
Procedure and Treatment:
 Relative energies of the molecular Orbitals will be explained.
 Fig6.22 will be discussed.
DLO # 3: Student will be able to explain the molecular Orbital Structure of some
diatomic molecules.
Procedure and Treatment:
 Molecular Orbital Structure of some diatomic molecules will be discussed.
 Fig6.23,6.24,6.25 will be discussed
Board Summary:
Name of the Chapter, Names of topics Structures of the compounds,
Recapitulation:
Quick recap of the lesson will be done.
LESSON PLAN
Teacher’s Name
Unit/Chapter
Institution
Subject
FDC,Faisal
Chemistry
Lesson Topic
(6.5) Bond Energy & Bond Length
Class
XI
Date
6,Chemical
Bonding
Essential Prior Knowledge: Students already have the knowledge of Ionic Bond &
Covalent Bond.
The Aims of the Lesson:
Students will be able to explain the Bond Energy & Bond Length.
.
Introduction: When bond is formed b/w two atoms, energy is released. The same
amount of energy is absorbed when bond is broken to form neutral atoms. The distance
b/w the nucleus of two atoms forming a covalent bond is called the bond length.
Lesson Development:
DLO # 1: Students will be able to explain the Bond Energy (Bond Enthalpy) of a
chemical bond.
Procedure and Treatment:
 Bond energy will be explained to the students
 Bond energy of different bonds will be explained.
 Table6.5 will be explained.
DLO # 2: Student will be able to explain the Ionic character of a bond on the basis of
Bond Energy.
Procedure and Treatment:
 Factors, affecting the strength of a bond will be discussed.
 Table6.6 will be discussed.
 Example of HCl bond will be discussed.
DLO # 3: Student will be able to explain the Bond length of a chemical bond.
Procedure and Treatment:
 Bond length will be explained to the students
 Bond length of different bonds will be explained.
 Table6.7 will be explained.
Board Summary:
Name of the Chapter, Names of topics Table 6.6 &6.7.
LESSON PLAN