DAILY SCIENCE LESSON PLAN

GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.

12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

At the end of the lesson, the learners will be able to:

 Define VSEPR Theory.
 Explain the concept of electron pair repulsion.
 Draw Lewis Dot Structures for elements and compounds.
I. OBJECTIVES
 Predict the shape of a molecule using VSEPR Theory.
 Understand the significance of VSEPR Theory in predicting the
chemical properties of elements and compounds.

The Learners will demonstrate the understanding of

a. How the uses of different materials are related to their
A. Content Standards properties and structures.
b. The relationship between the function and structure of
biological macromolecules
B. Performance
Standards
C. Learning Determine if a molecule is polar or non-polar given its structure
Competencies/
Objectives
(Write the LC S11/12PS-IIIc-15
code)
II. CONTENT VALENCE SHELL ELECTRON PAIR REPULSION THEORY
III. LEARNING
RESOURCES
A. References
1. Teacher’s Guide
pages
2. Learner’s Materials
pages
3. Textbook pages
4. Additional
Materials from
Learning Resource
(LR) portal
B. Other Learning http://misterguch.brinkster.net/PRA024.pdf
Resources https://youtu.be/r2XmaiEC0Vw
IV. PROCEDURES
ELICIT
Review question:
A. Reviewing  What is a Lewis dot structure and how does it represent the
previous lesson or bonding in a molecule?
presenting the new  How do you determine the total number of valence electrons in
lesson a molecule?
 What is the octet rule and how does it apply to Lewis dot
structures?
B. Establishing a ENGAGE
purpose for the  Introduce the topic of VSEPR Theory by asking the students if
lesson they have ever heard of it before.
 Ask the students what they know about the structure of a
molecule.
C. Presenting
 Use a whiteboard or chalkboard to draw a simple molecule and
examples/instance
label the different parts of the molecule.
s of the new lesson
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

D. Discussing new EXPLORE

concepts and  The teacher will show a video clip about the VSEPR theory.
practicing new  Explain that VSEPR Theory is a way of predicting the shape of a
skills #1 molecule based on the electron pairs surrounding the central
atom.
 Demonstrate the concept of electron pair repulsion and how it
E. Discussing new determines the shape of a molecule.
concepts and  Use the periodic table to demonstrate the valence electrons of
practicing new different elements.
skills #2  Demonstrate how to draw the Lewis Dot Structure for different
elements.
F. Developing EXPLAIN
mastery (leads to  Define VSEPR Theory in detail.
Formative The VSEPR theory (Valence Shell Electron Pair Repulsion
Assessment 3) theory)
 is a molecular geometry model used to predict the three-
dimensional shape of a molecule based on the number of
valence electron pairs surrounding the central atom.
 The theory is based on the principle that electron pairs in
the valence shell of an atom repel each other and try to
get as far apart as possible to minimize repulsion, which
results in a specific molecular shape.
 According to the VSEPR theory, the first step in
determining the molecular geometry of a molecule is to
count the number of valence electron pairs around the
central atom.
 This includes both bonding pairs (shared between two
atoms) and lone pairs (not involved in bonding). Once the
total number of electron pairs is known, the geometry of
the molecule can be predicted by minimizing the
repulsion between them.
 The VSEPR theory predicts the following molecular geometries
based on the number of electron pairs around the central atom:
1. Linear: Two electron pairs with a bond angle of 180 degrees.
2. Trigonal Planar: Three electron pairs with a bond angle of 120
degrees.
3. Tetrahedral: Four electron pairs with a bond angle of 109.5
degrees.
4. Trigonal Bipyramidal: Five electron pairs with bond angles of 90
and 120 degrees.
5.Octahedral: Six electron pairs with bond angles of 90 degrees.
 The VSEPR theory also predicts the shape of molecules with
lone pairs.
 The presence of lone pairs affects the bond angles, which
results in different molecular shapes.
 For example, if there are three bonding pairs and one lone pair,
the molecular shape will be trigonal pyramidal with a bond angle
of less than 109.5 degrees.
 In summary, the VSEPR theory is a powerful tool that predicts
the shape of a molecule based on the number of valence
electron pairs around the central atom. This helps to understand
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

the physical and chemical properties of molecules and their

reactivity.
 Explain how to count the number of valence electrons in an
atom or compound.
 Valence electrons are the electrons in the outermost shell of an
atom that are involved in chemical bonding.
 The valence electrons are important because they determine
the chemical properties of an atom and how it will bond with
other atoms.
 Here are the steps to count the number of valence electrons in
an atom or compound:
1.Determine the group number of the element. The group
number is the number of the column on the periodic table where
the element is located. For example, group 1 contains elements
like lithium and sodium, while group 2 contains elements like
magnesium and calcium.
2.Count the number of valence electrons in the outermost
shell. For elements in groups 1 and 2, the number of valence
electrons is equal to the group number. For example, lithium in
group 1 has one valence electron, and calcium in group 2 has
two valence electrons.
3.For elements in groups 3-12 (transition metals), the
valence electrons are in the outermost d and s orbitals. To
count the number of valence electrons for these elements, you
need to look at the electron configuration. For example, iron (Fe)
has the electron configuration of [Ar] 3d6 4s2. The valence
electrons are in the 4s and 3d orbitals, so the number of valence
electrons is 2 + 6 = 8.
4.For compounds, add up the number of valence electrons
for each atom. For example, in water (H2O), the two hydrogen
atoms each have one valence electron, and the oxygen atom
has six valence electrons. So, the total number of valence
electrons in water is 2 + 6 = 8.
 In summary, to count the number of valence electrons in an
atom or compound, you need to determine the group number of
the element and add up the number of valence electrons for
each atom in the compound. Knowing the number of valence
electrons is essential for understanding how atoms bond to form
molecules and how they interact with each other chemically.

 Explain how to draw the Lewis Dot Structure for different

compounds.
 The Lewis dot structure is a way of representing the bonding
and non-bonding electrons in a molecule.
 Here are the general steps to draw the Lewis dot structure for
different compounds:
1.Determine the total number of valence electrons in the
molecule. For example, in water (H2O), there are 2 valence
electrons for each hydrogen atom and 6 valence electrons for
the oxygen atom, so the total number of valence electrons is
2x2 + 6 = 10.
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

2.Identify the central atom in the molecule. This is usually the

least electronegative element in the compound or the one that
forms the most bonds. In water, the central atom is oxygen.
3.Draw a single bond between the central atom and each of
the surrounding atoms. In water, there is a single bond
between the oxygen atom and each of the hydrogen atoms.
4.Arrange the remaining electrons around the atoms to
satisfy the octet rule, which means that each atom (except for
hydrogen) should have 8 electrons around it. Place the
electrons around the atoms in pairs until there are no more
electrons left. In water, there are 8 electrons around the oxygen
atom (2 in each bond and 2 lone pairs) and 2 electrons around
each hydrogen atom.
5.Check that all atoms have a full outer shell of electrons. If
any atoms do not have 8 electrons around them, you can move
a lone pair of electrons from an adjacent atom to form a double
or triple bond. This is known as resonance. In water, the Lewis
dot structure is complete with all atoms having a full outer shell
of electrons, so there is no need for resonance.
6. Finally, determine the formal charge on each atom in
the molecule to make sure the Lewis dot structure is the
most stable arrangement of electrons. The formal charge is
the difference between the number of valence electrons in the
free atom and the number of electrons assigned to the atom in
the molecule. A stable Lewis dot structure is one where the
formal charges on the atoms are minimized.
 In summary, drawing the Lewis dot structure for different
compounds involves determining the total number of valence
electrons, identifying the central atom, arranging the electrons
around the atoms to satisfy the octet rule, checking for
resonance, and calculating the formal charges to ensure
stability.
 Explain how to determine the shape of a molecule using
VSEPR Theory.
 The VSEPR (Valence Shell Electron Pair Repulsion) theory is
used to predict the shape of a molecule based on the number of
valence electrons around the central atom and the repulsion
between electron pairs.
 Here are the general steps to determine the shape of a
molecule using VSEPR Theory:
1.Draw the Lewis dot structure for the molecule to determine the
number of valence electrons around the central atom.
2.Identify the number of electron pairs (bonded and non-
bonded) around the central atom. Count each lone pair of
electrons as one electron pair.
3.Determine the electron pair geometry by arranging the
electron pairs around the central atom as far apart as possible
to minimize repulsion. The electron pair geometry is determined
by the number of electron pairs and not the number of atoms.
For example, in a molecule with the formula AB3, the electron
pair geometry is trigonal planar, even though there are only
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

three atoms around the central atom.

4.Determine the molecular geometry by taking into account the
positions of the atoms and the lone pairs of electrons. The
molecular geometry is the shape of the molecule as it appears
in three-dimensional space. The molecular geometry may be the
same as the electron pair geometry if there are no lone pairs of
electrons, but if there are lone pairs of electrons, the molecular
geometry will be different.
5.Determine the bond angles between the atoms in the
molecule. The bond angles are determined by the positions of
the atoms and the lone pairs of electrons.
 Here are some examples of molecular geometries using VSEPR
Theory:
1.In water (H2O), the central atom is oxygen with two lone pairs
of electrons and two hydrogen atoms. The electron pair
geometry is tetrahedral, and the molecular geometry is bent with
a bond angle of approximately 104.5 degrees.
2.In carbon dioxide (CO2), the central atom is carbon with two
oxygen atoms. There are no lone pairs of electrons around the
central atom. The electron pair geometry is linear, and the
molecular geometry is also linear with a bond angle of 180
degrees.
3.In methane (CH4), the central atom is carbon with four
hydrogen atoms. There are no lone pairs of electrons around
the central atom. The electron pair geometry is tetrahedral, and
the molecular geometry is also tetrahedral with bond angles of
approximately 109.5 degrees.
.
G. Finding practical ELABORATE
applications of  Distribute the VSEPR Theory worksheet.
concepts and skills  Instruct the students to draw the Lewis Dot Structure for
in daily living
different compounds and predict the shape of the molecule
H. Making
using VSEPR Theory.
generalizations
and abstractions  Walk around the classroom to provide assistance and
about the lesson answer any questions.
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

 Ask the students to turn in their completed worksheets.

 Review the worksheets to assess the students' understanding of
the topic.
I. Evaluating learning EVALUATE
 The teacher will administer a short quiz to check whether the
learners learned from the topic.
1. What does VSEPR stand for?
a) Valence Shell Electron Pair Repulsion
b) Valence State Electron Pair Repulsion
c) Van der Waals Electron Pair Repulsion
d) Virtual State Electron Pair Repulsion
2.What is the main factor that determines the shape of a molecule
according to VSEPR theory?
a) The number of atoms in the molecule
b) The type of atoms in the molecule
c) The number and arrangement of electron pairs around the central
atom
d) The bond strengths between atoms in the molecule
3. What is electron pair geometry in VSEPR theory?
a) The shape of the molecule as determined by the positions of
the atoms
b) The shape of the molecule as determined by the positions of
the electron pairs around the central atom
c) The number of lone pairs of electrons around the central atom
d) The type of bond between the central atom and the other
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

atoms in the molecule

4. What is molecular geometry in VSEPR theory?
a) The shape of the molecule as determined by the positions of
the atoms
b) The shape of the molecule as determined by the positions of
the electron pairs around the central atom
c) The number of lone pairs of electrons around the central
atom
d) The type of bond between the central atom and the other
atoms in the molecule
5. What is the bond angle in a molecule?
a) The angle between the central atom and a neighboring atom
in the molecule
b) The angle between two lone pairs of electrons around the
central atom
c) The angle between two bonded atoms in the molecule
d) The angle between the central atom and a lone pair of
electrons
6. Which molecule has a linear molecular geometry?
a) H2O b) CO2 c) NH3 d) CH4
7. Which molecule has a trigonal planar electron pair geometry?
a) H2O b) CO2 c) NH3 d) BF3
8. Which molecule has a tetrahedral molecular geometry?
a) H2O b) CO2 c) NH3 d) CH4
9. Which molecule has a bent molecular geometry?
a) CO2 b) BF3 c) H2O d) CH4
10. Which type of electron pair is more likely to affect the molecular
geometry of a molecule in VSEPR theory?
a) Bonding pairs
b) Non-bonding (lone) pairs
c) Both types of electron pairs have equal influence
d) None of the above
EXTEND
11. Additional activities  Discuss the significance of VSEPR Theory in predicting the
for application or chemical properties of elements and compounds.
remediation  Ask the students to research and present a real-world
application of VSEPR Theory..
V. REMARKS
VI. REFLECTION
A. No. of learners who earned 80% in the evaluation
B. No. of learners who require additional activities for
remediation
C. Did the remedial lessons work? No. of learners who
have caught up with the lesson
D. No. of learners who continue to require remediation
E. Which of my teaching strategies worked well? Why did
this work?
F. What difficulties did I encounter which my principal or
supervisor can help me solve?
G. What innovation or localized materials did I
use/discover which I wish to share with other teachers?
 DAILY SCIENCE LESSON PLAN
GRADE LEVEL LEARNING AREA/ QUARTER / DOMAIN DATE PAGE NO.
12 SCIENCE QUARTER 4-PHYSICAL SCIENCE April 26-27,2023

Subject Teacher:

HAROLD C. PAYUNAN
Teacher -II

Checked by:

LETECIA S. VILLORENTE
Master Teacher I (Science)