9

SCIENCE
Guided Learning Activity Kit
Quarter 2- Week 1

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Science – Grade 9
Guided Learning Activity Kit
Quantum Mechanical Model of the Atom
Quarter 2- Week 1

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 QUANTUM MECHANICAL
MODEL OF THE ATOM

Introduction

Congratulations! This second quarter covers another branch of Science,

which is Chemistry.

In Grade 8, you have learned about Rutherford’s atomic model which

pictures atom as mostly empty space. Its mass is concentrated in the nucleus,
where the protons and the neutrons are located. This model has worked well
during his time, but it was only able to explain a few simple properties of the atom.

In this lesson, you will know more about the present model of the atom,
which is the Quantum Mechanical Model. You will discover what relationship
exists between the position of the electron and the energy they possess.

Learning Competency

Explain how the Quantum Mechanical Model of the Atom describe the
energies and positions of the electrons.

Objectives

At the end of this learning activity sheet, you are expected to:
1. discuss the development of the Quantum Mechanical Model of the
Atom;
2. describe the energies and position of the electrons;
3. apply the Aufbau Principle, Pauli Exclusion Principle, and Hund’s
Rule in the distribution of electrons; and
4. build the electron configuration and orbital diagram of electrons.

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 Review

Directions: Write True if the statement is correct or False if it is wrong.

__________1. Electron has a negative charge.
__________2. The symbol for the main energy level is n.
__________3. The lowest energy level that an electron occupies is referred to as the
outermost shell.
__________4. The maximum electrons that n = 1 can hold is two.
__________5. The atomic number of an element is equal to the number of neutrons.
__________6. The lowest energy level is the one nearest to the nucleus.
__________7. Octet Rule is the basis of writing the electron configuration of the
element.
__________8. The electrons in the valence shell are called valence electrons.
__________9. The electron configuration of an atom describes the distribution of
electrons in the orbitals.
__________10. Potassium has nineteen electrons.

Rutherford’s Model of the atom was found by other scientists to be

incomplete in terms of describing the nature and location of electrons. It was
revised by other scientists who conducted more extensive experiments. They
discovered more about the atom.

Discussion

Welcome to the Chemistry class! Be ready and follow the rules included in
the discussion.

Let us look at the development of the Quantum Mechanical Model of the

Atom.

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 Bohr’s atomic model explained that the electrons of the atom are located in
the distinct energy levels which surround the nucleus.

Electrons in each orbit have definite energy. The energy increases as the
orbit moves far from the nucleus. Electrons located in their natural orbits are said
to be in the ground state. There is no emission or absorption of energy if the
electron stays in its orbit. However, when the electron absorbs extra energy from a
flame or electric arc, the electron moves to higher energy levels. When this
happens, the electron is said to be in the excited state. When the electron moves
to the orbit with lower energy, the electron emits its extra energy in a form of
colored light. This phenomenon was observed by Bohr in his experiment with the
hydrogen atom. The discovery of the spectral lines was found when the heated
hydrogen gives off light which he viewed using a prism. This led him to propose a
model of the atom popularly known as the Planetary Model as it resembles the
Solar System.

Orbits are found at definite distances from the nucleus of a specific element
but vary from atom to atom. The fixed energies that the electrons have are called
energy levels (n) where n is a whole number 1,2,3 and so forth.

n= 1 is the lowest energy level

and n=3 is a higher energy level.

Bohr’s explanation of the

discrete energy levels works well with
hydrogen and helium. However, it is
not possible for other more complex
elements. Several scientists noted
that it is not possible to know the
exact position of the electron. So,
Figure 1. An atom with three Energy Bohr’s idea about the existence of
Levels (n) definite orbits around the nucleus
where electrons move is rejected.

Three physicists, Louie de Broglie, Erwin Schrödinger, and Werner Karl

Heisenberg, worked together to develop a new model of the atom. De Broglie
proposed that the particles could as well behave like waves. Schrödinger was
impressed by the idea of De Broglie which he used to devise an equation to explain
the probability of electrons around the nucleus of the atom. Heisenberg, on the
other hand, laid the Uncertainty Principle which describes that it is impossible to
determine the exact position, movement, and speed of an electron.

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 De Broglie proposed that the particles could as well behave like waves.
Schrödinger was impressed by the idea of De Broglie which he used to devise an
equation to explain the probability of electrons around the nucleus of the atom.
Heisenberg, on the other hand, laid the Uncertainty Principle which describes that
it is impossible to determine the exact position, movement, and speed of an
electron.

The three scientists believed that the region around the nucleus is a space
where the probability of electrons can be found. An atomic orbital is a region where
the electron is most likely to be found. Through Schrödinger’s equation, the
Quantum Mechanical Model of the atom comes out.

The quantum mechanical model views the geometrical shape of an electron

as a cloud of negative charge. This model gives an idea about the different locations
of electrons around the nucleus.

Figure 2. The average distance of electrons having

high and low energies

Figure 2 shows that the probability of the number of electrons in the area is
based on the density of the “electron cloud”.The darker the area, the more chance
of finding an electron in that area. The quantum mechanical model also gives
information about the energy of the electron. Electrons occupy a certain shell.
These shells are also called the principal or main energy levels. The principal energy
levels or shells have one or more sublevels. These sublevels are assigned with
letters: s, p, d, and f. Each sublevel has orbitals as shown in Table 1.

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 Table 1. Principal Energy Levels and Sublevels of Electrons

Total
Sublevel Number of
Principal Number of
Designation/ Electrons
Energy Sublevels/ Number of Orbitals
Subshells per
Level (n) Shells
(Letter) Sublevel

1 1 1s 2

2s 2

2 2
2p 6
3s 2

3 3 3p 6

3d 10

4s 2

4p 6

4 4
10
4d

4f 14

The squares in Table 1 represent the atomic orbitals. Each orbital can hold
a maximum of 2 electrons. The s sublevel has 1 orbital and can hold a maximum of
2 electrons; p sublevel has 3 orbitals and can hold a maximum of 6 electrons; the
d sublevel with 5 orbitals can hold a maximum of 10 electrons, and f sublevel can
hold a maximum of 14 electrons with its 7 orbitals. The minimum number of
electrons per sublevels is 1.

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Electron Configuration
The electron configuration shows the arrangement and distribution of
electrons in an atom. When writing an atom’s electron configuration, you represent
the electron shell, subshell, and number as illustrated in the diagram below. For
Helium (He), we have:

2 Electron Number
Shell
1s
Subshell

Electron Configuration is a way of distributing electrons to the orbitals of the

atom. In the distribution of electrons, we need to follow the rules of the Aufbau
Principle, Pauli Exclusion Principle, and Hund’s Rule.

1. The Aufbau Principle, explains the building up of the electron

configuration of the atom. The diagram below shows the increasing energy level
(n=1,2,3,4,5,6,7) the flow of assigning electrons to the different sublevel (s, p, d, f).

This diagram is what we call the

mnemonic device or electron configuration
mnemonics. It assumes that the energy of
orbitals that are filled up first is lower than
the succeeding orbitals of a given sublevel.

2. Pauli Exclusion Principle states

that an orbital may be occupied by a
maximum of two electrons. These electrons
should have different spins. Make sure that
every orbital has an arrow up ↑ and arrow
down ↑ if it meets the maximum number of
electrons. The arrows represent the spins of
Figure 3. The Electron the electrons.
Configuration Mnemonics
3. Hund’s Rule states that the
electron entering orbitals of equal energy (orbitals of p,d, and f sublevels) tend to fill
out singly first. Supply the arrow up ↑ first before the arrow down ↓ in the orbital/s
of each subshell. Take note: always look at the number of electrons to have the
correct distribution of electrons.

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Steps in Writing the Electron Configuration

Example 1. Build the electron configuration of the Neon atom

Step 1. First, you need to identify the number of electron of the element using the
periodic table of the elements. The number of electrons is equal to the atomic
number in a neutral atom. The atomic number of Neon is 10, so the number of
electrons of Neon is 10. We can write the number of the electron of the Neon as
10Ne.

10 Atomic Number

Ne Symbol

Neon Name of the Element

Step 2. Using the mnemonic device, follow the arrow when writing the electron
configuration. The electron configuration always starts with 1s.
Step 3. From the 10 electrons of Neon, assign how many electrons will occupy 1s.
Keep in mind that the s sublevel can hold a maximum of 2 electrons only.
10Ne = 1s2

Step 4. Continue following the arrow in the mnemonics. The next level to fill with
electrons is 2s. Again, the sublevel s can hold a maximum of 2 electrons.
10Ne = 1s2 2s2

Step 5. We have distributed 4 electrons already. We still have 6 electrons to

distribute. Continue following the arrow in the mnemonics. The next level to fill
with electrons is 2p. The p sublevel can hold a maximum of 6 electrons.
10Ne = 1s2 2s2 2p6

The remaining 6 electrons have been distributed to 2p. Therefore, no more

electrons are left to be distributed. This means that the electron configuration is
complete.
Step 6. To check your work, add the exponents in the electron configuration. This
should be equal to the number of electrons of Neon.
The sum of the exponents
2 + 2 + 6 = 10 is 10. It is equal to the
number of electrons of
Neon. Therefore, the
Number of 10Ne = 1s2 2s2 2p6 electron configuration is
Electrons
correct and complete.

We can also represent the electron configuration using orbits and dots just
like the one below. Observe that the second energy level has 2 occupied sublevels:
2s2 and 2p6. Therefore, the second energy level has a total of 8 electrons.

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 1s2

2s2 2p6

Figure 4. Electron Distribution Using Orbits and Dots

Example 2. Build the electron configuration of the Sulfur atom, (16S).

Step 1. Identify the number of electron of Sulfur. We can write the number of the
electron of the Sulfur as 16S.

Step 2. Using the mnemonic device, follow the arrow when writing the electron
configuration. The electron configuration always starts with 1s.
Step 3. From the 16 electrons of Sulfur, assign how many electrons will occupy 1s.
16S = 1s2

Step 4. Continue following the arrow in the mnemonics. The next level to fill with
electrons is 2s. Again, the sublevel s can hold a maximum of 2 electrons.
16S = 1s2 2s2

Step 5. We have distributed 4 electrons already. We still have 12 electrons to

distribute. Continue following the arrow in the mnemonics. The next level
to fill with electrons is 2p. The p sublevel can hold a maximum of 6
electrons.
16S = 1s2 2s2 2p6

Step 6. We have distributed 10 electrons already. We still have 6 electrons to

distribute. Continue following the arrow in the mnemonics. The next level
to fill with electrons is 3s. The s sublevel can hold a maximum of 2
electrons.
16S = 1s2 2s2 2p6 3s2

Step 7. We have distributed 12 electrons already. We still have 4 electrons to

distribute. Continue following the arrow in the mnemonics. The next level
to fill with electrons is 3p. The s sublevel can hold a maximum of 6
electrons but we only have 4 electrons left. So, we will assign the 4
electrons to 3p. Do not worry. The last sublevel can have less than the
maximum number of electrons it can hold.
16S = 1s2 2s2 2p6 3s2 3p4

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Step 8. To check your work, add the exponents in the electron configuration. This
should be equal to the number of electrons of Sulfur. Is the sum of the
exponents equal to 16? Yes! Therefore, the electron configuration is
correct and complete.
Following the Aufbau Principle electron configuration, you can also build the
orbital diagram of electrons following the Pauli Exclusion Principle and Hund’s
Rule.

Example 3. Build the electron configuration of the Neon atom (10Ne) and show the
orbital diagram of electrons.

Step 1. From the electron configuration of neon, draw the number of orbitals for
each sublevel. Refer to Table 1.

1s2 2s2 2p6

Step 2. Distribute the electrons to 1s orbital. The electrons are represented by

arrows. Keep in mind that the arrows should have opposite directions .
1s2 2s2 2p6
↑↓

Step 3. Distribute the electrons to 2s orbital.

1s2 2s2 2p6

↑↓ ↑↓

Step 4. Distribute the electrons to 2p orbitals. Remember that according to Hund’s

Rule, the electrons should occupy the orbitals singly first before pairing
up.
1s2 2s2 2p6 1s2 2s2 2p6
↑↓ ↑↓ ↑ ↑ ↑ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓

The completed orbital distribution of electrons for neon is:

1s2 2s2 2p6

10Ne = ↑↓ ↑↓ ↑↓ ↑↓ ↑↓

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Example 4. Build the electron configuration of Beryllium atom ( 4Be) and show the
distribution of electrons.
1s2 2s2
The answer will be 4Be =
↑↓ ↑↓

Example 5. Build the electron configuration of Sulfur atom ( 16S) and show the
distribution of electrons.
1s2 2s2 2p6 3s2 3p4
The answer will be 16S =
↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑

Now that you have learned how electrons are arranged in the atom, you can now
proceed to the activities I prepared for your practice. Please have with you
a periodic table of elements.

Activities

Guided Activity 1: Follow the order.

Directions: Build the electron configuration of the following elements. Follow the
Aufbau Principle using the Electron Configuration Mnemonics.

1. 20Ca = ____________________________________________________
2. 28Ni = _____________________________________________________
3. 14Si = _____________________________________________________

4. 1H = ______________________________________________________
5. 42Mo = ____________________________________________________
6. Bromine (_____)= __________________________________________
7. Chlorine (_____)= __________________________________________
8. Silver (_____)= _____________________________________________
9. Lanthanum(_____)= ________________________________________
10. Tungsten (_____)= __________________________________________

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Guided Activity 2: Follow my rule!
Directions: Copy your answer in Guided Activity 1 and show the orbital diagram of
the electron configuration of each element. Follow Pauli Exclusion Principle and
Hund’s Rule.
1. ____________________________________________________________
2. ____________________________________________________________
3. ____________________________________________________________
4. ____________________________________________________________
5. ____________________________________________________________
6. ____________________________________________________________
7. ____________________________________________________________
8. ____________________________________________________________
9. ____________________________________________________________
10. ____________________________________________________________

Independent Activity: I am an illustrator.

Directions: Draw the atom of the following elements using orbits to show the
location of the electrons. Use dots to represent the electrons. The number of dots is
based on the number of electrons. You can use more than one orbit if needed. Use
the example below for your basis. (2pts each)

For example:

4Be = 1s2 2s2 15P = 1s2 2s2 2p6 3s2 3p3

1. Carbon 2. Sulfur

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 3. Titanium 4. Zinc

5. Rubidium

Assessment

Directions: Read and analyze the questions. Write the letter that corresponds to the
correct answer.
1. Which of the following scientists devised an equation about the wave-like
motion of electrons around the nucleus of the atom?
A. Louis De Broglie C. Erwin Schrodinger
B. Niels Bohr D. Werner Heisenberg
2. Which of the following principal energy levels has the highest energy?
A. n=1 B. n= 2 C. n= 3 D. n= 4
3. If the first and second energy levels of an atom are full, what would be the
total number of electrons in the atom?
A. 10 B. 16 C. 8 D. 18
4. What do you call the representation of the arrangement of all the electrons
in an atom?
A. Orbital C. Electron Configuration
B. Subshells D. Energy level

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 5. What model of the atom describes an atom as having a nucleus surrounded
by electrons found in regions of high probability?
A. Rutherford’s Atomic Model C. Bohr’s Atomic Model
B. Quantum Mechanical Model D. Thomson’s Atomic Model
6. What do we call the letters s, p, d, and f in writing the electron configuration
of the elements?
A. Shells B. Sublevels C. Electron Number D. Orbitals
7. How many orbitals are there in the d sublevel?
A. 1 B. 3 C. 4 D. 5
8. Who proposed the idea that particles could as well behave like waves?
A. Louis De Broglie C. Erwin Schrodinger
B. Niels Bohr D. Werner Heisenberg
9. Who proposed the assumption that one cannot exactly determine the
location and movement of electrons?
A. Louis De Broglie C. Erwin Schrodinger
B. Niels Bohr D. Werner Heisenberg
10. What is the maximum number of electrons that the f sublevel can hold?
A. 1 B. 14 C. 6 D. 10
11. How many electrons are there in the Phosphorus atom?
A. 10 B. 15 C. 30 D. 60
12. How many electrons are there in a Cesium atom?
A. 25 B. 78 C. 92 D. 55
13. How many orbitals are there in the p sublevel?
A. 1 B. 3 C. 5 D. 7
14. How many orbitals are there in the s sublevel?
A. 1 B. 3 C. 5 D. 7
15. Which of the following statement is not true of the atomic model of Bhor?
A. The hydrogen is made up of a positively charged nucleus.
B. The electron revolves around the nucleus in a circular orbit.
C. The energy of the electron in a given orbit is not fixed.
D. The electron can absorb or emit a quantity of radiation.

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 Reflection

Directions:Fill in the missing word/s to complete the paragraphs. Choose your

answer from the box below.

Orbitals s Aufbau Principle Sublevel Nucleus

Electron Configuration n=3 Electrons Two
Principal Energy Level Pauli Exclusion Principle
Maximum Hund’s Rule d and f Increases
The Quantum Mechanical Model of the atom describes the atom as having a
1.________________ at the center around which the 2._______________ move.
3.________________, 4.__________________, and 5._______________ are the processes of
distributing the electrons to the various 6._______________. This is called
7._______________. Aufbau process states that as the number of the main energy
increases, the energy also 8._______________. Pauli Exclusion Principle states that
an orbital may be occupied by a 9._______________ of two electrons of opposite
spins. Hund’s Rule states that no electron enters an already occupied orbital if
there are unoccupied orbitals in the same 10._______________.

N=1, n=2, n=3, and soon are what we call 11._______________. In n=1, there is only
one sublevel, which is the sublevel 12._____. In n=2, there are 13._______ sublevels,
s and p. In 14._______, there are three sublevels, which are the sublevels s, p, and
d. In n=4, there are four sublevels. These are s, p, 15.__________.

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 References

"7.4: The Quantum-Mechanical Model Of The Atom". 2020. Chemistry Libretexts.

https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Ch
emistry__The_Molecular_Nature_of_Matter_and_Change_(Silberberg)/07%3
A_Quantum_Theory_and_Atomic_Structure/7.04%3A_The_Quantum-
Mechanical_Model_of_the_Atom.
"Atomic Structure: The Quantum Mechanical Model - Dummies". 2020. Dummies.
https://www.dummies.com/education/science/chemistry/atomic-
structure-the-quantum-mechanical-model/.
"Electron Configuration - Detailed Explanation With Examples". 2020. BYJUS.
https://byjus.com/chemistry/electron-configuration/.
"Electron Configurations". 2020. Chem.Fsu.Edu.
https://www.chem.fsu.edu/chemlab/chm1045/e_config.html.

"Electronic Configurations Intro". 2020. Chemistry Libretexts.

https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemi
stry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Ch
emistry)/Electronic_Structure_of_Atoms_and_Molecules/Electronic_Config
urations/Electronic_Configurations_Intro.
Alvarez, Lisa et.al. 2014.Science Learner’s Module. First Edition. Pasig City:
Department of Education
Foundation, CK-12. 2020. "Welcome To CK-12 Foundation | CK-12
Foundation". CK-12 Foundation. https://www.ck12.org/book/ck-12-
chemistry-concepts-intermediate/section/5.11/.
Martin, Purita R. 2007. Connecting with Science Chemistry. Makati City: Salesiana
Books.
Santos, Gil Nonato et.al 2003. E-Chemistry III: The Next Generation. Manila: Rex
Book Store, Inc.
The Quantum Mechanical Model of the Atom. Khan Academy.
https://www.khanacademy.org/science/physics/quantum-
physics/quantum-numbers-and-orbitals/a/the-quantum-mechanical-
model-of-the-atom
The Quantum Mechanical Model of the Atom. Khan Academy.
https://www.khanacademy.org/science/physics/quantum-
physics/quantum-numbers-and-orbitals/a/the-quantum-mechanical-
model-of-the-atom.

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Reflection Assessment
1. Nucleus 2. Electron 1. C 2. D
3. Aufbau Principle 3. A 4. C
4. Pauli Exclusion Principle 5. B 6. B
5. Hund’s Rule 6. Orbitals 7. D 8. A
7. Electron Configuration 9. D 10. B
8. Increases 11. B 12. D
9. Maximum 10 Sublevel 13. B 14A
11. Principal Energy Level 15. C
12. s 13. Two
14. n=3 15. d and f
Activities
Review
A. Follow the order.
1. 20Ca = 1s2 2s2 2p6 3s2 3p6 4s2 1. True
2. 28Ni = 1s2 2s2 2p6 3s2 3p6 4s2 3d8 2. True
3. 14Si = 1s2 2s2 2p6 3s2 3p2
3. False
4. 1H = 1s1
4. True
5. False
5. 42Mo = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d4
6. True
6. Bromine (35Br)= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
7. False
7. Chlorine (17Cl)= 1s2 2s2 2p6 3s2 3p5 8. True
8. Silver (47AG)= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9 9. True
9. Lanthanum(57La)= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f1 10. True
10. Tungsten (74W)= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d4
Key to Corrections
 Acknowledgment
The Schools Division of Zambales would like to express its heartfelt
gratitude to the following, who in one way or the other, have contributed to the
successful preparation, development, quality assurance, printing, and distribution
of the Quarter 2 Guided Learning Activity Kits (GLAKs) in all learning areas across
grade levels as a response to providing the learners with developmentally-
appropriate, contextualized and simplified learning resources with most essential
learning competencies (MELCs)-based activities anchored on the principles of
guided learning and explicit instruction:

First, the Learning Resources (LR) Development Team composed of the

writers and graphic artists for devoting much of their time and exhausting their
best efforts to produce these indispensable learning kits used for the
implementation of learning delivery modalities.

Second, the content editors, language reviewers, and layout evaluators

making up the Division Quality Assurance Team (DQAT) for having carefully
evaluated all GLAKs to ensure quality and compliance to DepEd standards;

Third, the Provincial Government of Zambales, for unceasingly extending its

financial assistance to augment the funds for the printing of these learning
resources for use by learners and parents at home;

Fourth, the teacher-advisers and subject teachers, in close coordination

with the school heads, for their weekly distribution and retrieval of the GLAKs and
for their frequent monitoring of the learners’ progress through various means; and

Finally, the parents and other home learning facilitators for giving the
learners the needed guidance and support for them to possibly accomplish the
tasks and for gradually helping them become independent learners.

To deliver learning continuity in this challenging circumstance would not be

possible without your collective effort and strong commitment to serving our
Zambaleño learners.

Again, our sincerest thanks!

The Management Team

 For inquiries or feedback, please write or call:

Department of Education – Region III – Division of Zambales

Learning Resource Management Section (LRMS)
Zone 6, Iba, Zambales
Tel/Fax No. (047) 602 1391