This is the Grade 9 Science self-learning module for Quarter 2 (Matter), Module 3: “IONS: How Are They Formed?” It was developed by DepEd National Capital Region as part of the Alternative Delivery Mode (First Edition, 2020). It is meant for Grade 9 learners studying at home, and for the teachers and parents who guide them. After working through it, learners should be able to explain how atoms become ions and write the chemical formulas of simple ionic compounds.
On this page 6 sections
What learners will learn
The module focuses on one learning competency: Explain how ions are formed (S9MT-IIe-f-16).
By the end of the module, learners are expected to:
- describe ions and how they are formed;
- tell cations from anions based on whether an atom tends to lose or gain electrons;
- show how ions form using Lewis Electron Dot Symbols (LEDS); and
- write the chemical formula of an ionic compound based on the charges of its ions.
The module also asks learners to think about four key questions: What are ions and how are they formed? How are cations and anions different? How do LEDS show the formation of ions? How do you write a chemical formula from the charges of ions?
Key ideas in the module
The module builds on the previous one, where learners studied ionic and covalent compounds through properties such as melting point, hardness, polarity, and conductivity. It opens with a short comic strip in which Sodium (Na) gives its one valence electron to Chlorine (Cl), so both become stable and are held together as NaCl by an ionic bond.
Chemical bonds and ions
- A chemical bond is the attraction between atoms that combine by sharing or transferring their valence electrons.
- Ions are atoms or groups of atoms that carry a positive or negative charge. They form when an atom loses or gains electrons.
- When metals combine with nonmetals, metals tend to lose electrons and nonmetals tend to gain them. Both do this to become stable.
- The octet rule says an atom is stable when it has 8 valence electrons in its outermost shell.
The module’s main example is sodium and chlorine. Sodium (Group 1A, a metal) has 1 valence electron. Chlorine (Group 7A, a nonmetal) has 7. It is easier for sodium to give away 1 electron than to gain 7, so sodium transfers its electron to chlorine. Both atoms then become stable, forming sodium chloride, commonly known as table salt.
Cations and anions
| Ion | How it forms | Charge | Usually formed by |
|---|---|---|---|
| Cation | The atom loses electrons | Positive | Metals |
| Anion | The atom gains electrons | Negative | Nonmetals |
For example, when sodium loses its electron it becomes the cation Na+, and when chlorine gains it, chlorine becomes the anion Cl-. In the activities, a nitrogen atom that gains 3 electrons is written N-3, and a lithium atom that loses 1 electron is written Li+1.
Lewis Electron Dot Structure (LEDS)
The Lewis Electron Dot Structure was introduced by Gilbert N. Lewis, an American physical chemist. It shows the symbol of an element surrounded by dots, one dot for each valence electron. You can find the number of valence electrons from the element’s group or family number in the periodic table. For example, lithium (Group IA) has 1 valence electron, so its symbol gets one dot.
Writing chemical formulas of ionic compounds
To write the formula of an ionic compound, write the cation (positive ion) first, then the anion (negative ion). The module also teaches the crisscross method, using magnesium and oxygen as the example:
- Write each ion with its charge: Mg2+ and O2-.
- Cross the number of each charge so it becomes the subscript of the other ion, and drop the plus and minus signs: Mg2O2.
- Reduce the subscripts to the lowest terms, and do not write any subscript that is 1.
- Write the final formula: MgO.
Other examples in the module include CaCl2 (calcium chloride), MgBr2 (magnesium bromide, which has 2 bromide ions for every magnesium ion), KF, AlBr3, CaS, and NaI.
What’s inside the module
- What I Know: a 10-item multiple-choice pretest
- What’s In: a review where learners label statements as describing ionic (I) or covalent (C) compounds
- What’s New: the sodium and chlorine comic strip
- What is It: the discussion of chemical bonds, ions, cations and anions, LEDS, and chemical formulas
- What’s More: Activity 1 (group, valence electrons, and Lewis symbols of ten elements), Activity 2 (metal or nonmetal, lose or gain, cation or anion), and Activity 3, “Gain or lose, you choose!” (ions formed, with guide questions)
- What I Have Learned: a fill-in-the-blanks summary using a word box
- What I Can Do: “The Perfect Match,” where learners pair elements into ionic compounds, draw the LEDS, and write the formula
- Assessment: a 10-item multiple-choice post-test
- Additional Activities: “Let’s Find Out!”, a crossword puzzle of key terms
- Answer Key for the tests and activities
How to use this module
Learners: Start with the pretest to check what you already know, then go through each part in order. Keep a periodic table nearby, since Activity 1 asks you to use one. Write all your answers on a separate sheet of paper and do not mark the module. Take the post-test at the end, then check your work with the answer key honestly.
Parents: Help your child follow the parts in order and make sure answers go on a separate sheet. The module includes notes for facilitators and parents on how to support home-based learning. If your child gets stuck, encourage them to contact their teacher.
Teachers: The lessons follow the standard sequence of the course, but the module notes that you may change the order to match the textbook you use. The pretest can show which learners need extra help before they continue.
Frequently asked questions
What grade and quarter is this module for?
It is for Grade 9 Science, Quarter 2 (Matter). It is Module 3, titled IONS: How Are They Formed?
What competency does the module cover?
It covers the competency Explain how ions are formed, with the code S9MT-IIe-f-16.
What is the difference between a cation and an anion?
A cation is a positively charged ion formed when an atom loses electrons, usually a metal. An anion is a negatively charged ion formed when an atom gains electrons, usually a nonmetal.
What is the crisscross method?
It is a way to write the formula of an ionic compound. You cross the number of each ion’s charge to become the other ion’s subscript, drop the signs, reduce to lowest terms, and leave out subscripts of 1, so Mg2+ and O2- give MgO.
Does the module have an answer key?
Yes. Answer keys are included for the pretest, the review, the activities, the summary, the crossword, and the post-test.
Full text of the module
The text below is a transcription of the PDF above, as printed.
Science Quarter 2- Matter Module 3: Ions: How Are They Formed?
[illustration: students studying outdoors and at home, a teacher with a student, a student with a globe, and a lamp]
GOVERNMENT PROPERTY NOT FOR SALE
Science – Grade 9
Alternative Delivery Mode Quarter 2: Matter – Module 3: IONS: How Are They Formed? First Edition, 2020
Republic Act 8293, section 176 states that: No copyright shall subsist in any work of the Government of the Philippines. However, prior approval of the government agency or office wherein the work is created shall be necessary for exploitation of such work for profit. Such agency or office may, among other things, impose as a condition the payment of royalties.
Borrowed materials (i.e., songs, stories, poems, pictures, photos, brand names, trademarks, etc.) included in this module are owned by their respective copyright holders. Every effort has been exerted to locate and seek permission to use these materials from their respective copyright owners. The publisher and authors do not represent nor claim ownership over them.
Published by the Department of Education Secretary: Leonor Magtolis Briones Undersecretary: Diosdado M. San Antonio
Development Team of the Module
Writer: Melissa F. Ranay Editor: Loreta E. Santos Reviewers: Aurora T. Alcazar, Anthony D. Angeles, Lonida A. Caiña, Mariel G. de Jesus, Mary Grace C. Dimacutac, Mary Grace G. Fuentes, Myla D. German, Myrla D. Guevarra, Marilou I. Ignacio, Rosemarie V. Rodanilla, Avie John Tesorero Language: Elvira P. Emerenciana, Nova V. Tarcena, Lilibeth M. De Lansig Design and Layout: Edgardo Q. Reyes, Ana Lisa M. Mesina Layout Artist: Melissa F. Ranay, Mark Joseph Y. Samarita Management Team: Malcolm S. Garma, Genia V. Santos, Dennis M. Mendoza, Micah S. Pacheco, Josefina M. Pablo, Manolo C. Davantes Jr., Dalisay E. Esguerra, Hilda C. Valencia
Printed in the Philippines by _____
Department of Education – National Capital Region
Office Address: Misamis St. Bago Bantay, Quezon City Telefax: (632)8929-0153 E-mail Address: depedncr@deped.gov.ph
9
Science Quarter 2- Matter Module 3: IONS: How Are They Formed?
Introductory Message
This Self-Learning Module (SLM) is prepared so that you, our dear learners, can continue your studies and learn while at home. Activities, questions, directions, exercises, and discussions are carefully stated for you to understand each lesson.
Each SLM is composed of different parts. Each part shall guide you step-by-step as you discover and understand the lesson prepared for you.
Pre-tests are provided to measure your prior knowledge on lessons in each SLM. This will tell you if you need to proceed on completing this module or if you need to ask your facilitator or your teacher’s assistance for better understanding of the lesson. At the end of each module, you need to answer the post-test to self-check your learning. Answer keys are provided for each activity and test. We trust that you will be honest in using these.
In addition to the material in the main text, Notes to the Teacher are also provided to our facilitators and parents for strategies and reminders on how they can best help you on your home-based learning.
Please use this module with care. Do not put unnecessary marks on any part of this SLM. Use a separate sheet of paper in answering the exercises and tests. And read the instructions carefully before performing each task.
If you have any questions in using this SLM or any difficulty in answering the tasks in this module, do not hesitate to consult your teacher or facilitator.
Thank you.
What I Need to Know
This module was designed and written with you in mind. It is here to help you master IONS: How Are They Formed? The scope of this module permits it to be used in many different learning situations. The language used recognizes the diverse vocabulary level of students. The lessons are arranged to follow the standard sequence of the course, but the order in which you read them can be changed to correspond with the textbook you are now using.
The module focuses on achieving this learning competency:
Explain how ions are formed. (S9MT-IIe-f-16)
After going through this module, you are expected to:
- describe ions and how it is formed;
- differentiate cations from anions based on their tendency to lose or gain electrons;
- show the formation of ions using Lewis Electron Dot Symbols (LEDS); and
- write chemical formula of ionic compounds based on the charges of ions.
What I Know
Choose the letter of the best answer. Write your answer on a separate sheet of paper.
What do you call the ion which carry positive charge in its atom?
A. Anions
B. Cations
C. Polyatomic ions
D. Polymers ionWhat do you call the ion which carry negative charge in its atom?
A. Anions
B. Cations
C. Polyatomic ions
D. Polymers ionAn element is found in Family II and Period III of the Periodic Table of elements. What is its valence electron?
A. 1
B. 2
C. 3
D. 5What is the basis of Lewis Dot Structure?
A. Anions
B. Cations
C. Period Number
D. Valence NumberWhich LEDS is the correct structure for Chlorine (Cl)?
A. [illustration: Lewis dot symbol of Cl, option A]
B. [illustration: Lewis dot symbol of Cl, option B]
C. [illustration: Lewis dot symbol of Cl, option C]
D. [illustration: Lewis dot symbol of Cl, option D]
[transcriber’s note: the dot positions in the four options are not reliably legible at this resolution, so they are not transcribed]Which type of elements tend to gain electron/s during ionic bonding?
A. metals
B. metalloid
C. non- metal
D. super alloyDuring the experiment, a scientist found out the following characteristics of elements.
| Characteristics | A | B | C | D |
|---|---|---|---|---|
| Mass | 0.10 g | 0.20 g | 0.30g | 0.40g |
| Transfer of Electron | Gain | Lose | Lose | Gain |
| Reactivity | YES | YES | YES | YES |
As a scientist, which do you think are the metals in the results of the experiment as stated in the Table above? A. A and B B. A and D C. B and C D. B and D
Which type of elements tends to lose electron/s during ionic bonding?
A. metals
B. metalloid
C. non- metal
D. super alloyWhat is the correct chemical formula for the ionic compound containing Calcium ion and Chlorine ion?
A. CaCl
B. Ca2Cl
C. CaCl3
D. CaCl2MgBr2 is the chemical formula for magnesium bromide. What does the number “2” in the formula mean?
A. Bromine has 2+ charge
B. Bromine has 2- charge
C. There are 2 Bromine ions in every magnesium ion
D. There are 2 Magnesium ions in every bromine ion
Lesson 1 IONS: How Are They Formed?
In the previous module, you have learned the different types of compounds based on their properties such as melting point, hardness, polarity and electrical and thermal conductivity. In this module, you will learn about ions and how they are formed. You are going to figure out what types of ions are formed when atom lose and gain electrons during chemical bonding.
Here are some key questions for you to ponder after finishing this module:
- What are ions and how are they formed?
- What is the difference between cations and anions?
- How is the formation of ions using Lewis Electron Dot Symbols (LEDS) shown?
- How is the chemical formula based on the charges of ions written?
What’s In
Let’s recall your understanding of the different types of compounds based on their property.
Write I if the statement describes an ionic compound, C if the statement describes a covalent compound.
_____ 1. It conducts electricity when dissolved in water. _____ 2. It has a high melting point. _____ 3. Does not conduct electricity. _____ 4. Insoluble in water. _____ 5. It has a low boiling point _____ 6. It is formed through losing and gaining electrons. _____ 7. Consist of positive and negative charged particles. _____ 8. Bond between two nonmetals. _____ 9. Bond between a metal and a nonmetal. _____ 10. Formed through sharing of electrons.
What’s New
Read the comic strip below. Identify the main focus of the lesson. Point out some important details that will be discussed to answer the activities provided for you.
[illustration: comic strip in five panels showing Na and Cl characters exchanging an electron and forming NaCl]
Panel 1 (Na): “I wish to become stable. But I have one valence electron.”
Panel 2 (Cl): “(Weeping) I am SO close to having a full valence electron!!”
Panel 3 (Na): “Excuse me Miss Chlorine. I have an idea. I can give you my valence electron so that you and I will both become stable.” Panel 3 (Cl): “You’re right Mr. Sodium! I can accept your valence electron so that both of us will become stable”
Panel 4 (Na): “I am now a cation because I gave away an electron.” Panel 4 (Cl): “I am anion now because I accepted an electron.”
Panel 5 (label: NaCl): “Our positive and negative charges attract! We are now held together by an ionic bond.”
What is It
Chemical Bonding
Chemical bond is a term use to describe the attraction of atoms that are combined together through sharing and transferring their valence electrons.
IONS: How Are They Formed?
Ions are atoms or groups of atoms that has positive or negative charge.
Ions are formed when an atom lose or gain its electrons. If metals were chemically combined to nonmetals, metals would tend to lose electron while nonmetals gain electrons during chemical bonding to attain stability. For an atom to attain stability, they must have 8 valence electrons in their outermost shell. This is known as OCTET RULE.
Let us consider Sodium and Chlorine. Sodium is a metallic element under Group 1A. It has one (1) valence electron. Chlorine on the other hand, is a non-metallic element under Group 7A, it has seven (7) valence electrons. Sodium needs 7 electrons to follow the Octet rule, while Chlorine needs 1 valence electron. It is easier for Sodium to give away its one (1) valence electron to become more stable than to get seven (7) valence electrons. Therefore, when Sodium (Na) and Chlorine (Cl) bond together, Sodium will give its one (1) valence electron to Chlorine so that Sodium will become stable. On the other hand, Chlorine also becomes stable when it accepts the one (1) valence electrons given by Sodium.
Cation and Anion
When an atom loses or gains electrons, they formed ions. An atom that loses electrons becomes a positively charged ion known as cation. An atom that gains electrons become negatively charged ion known as anion.
Lewis Electron Dot Structure (LEDS)
Lewis Electron Dot Structure is introduced by Gilbert N. Lewis, an American Physical Chemist. LEDS is composed of the symbol of the element and dots which represent the number of valence electrons of an atom that can easily be determined through the group/family number in the Periodic Table of Elements. Consider the following example:
[chart: diagram; Lewis Electron Dot Structure of sodium and chlorine, with the electron transfer from Na to Cl. Labels as printed: “Na•” “LEDS Diagram of Sodium”; “Cl” “LEDS Diagram of Chlorine”; “Na○” with red arrow to “Cl:” labeled “Sodium (Na) transfer its electron to Chlorine (Cl)”; “Na+” “Sodium (Na) ion” “cation”; “Cl-” “Chlorine (Cl) ion” “anion”; “NaCl” “Sodium Chloride”. Values are not labeled on the chart.]
Writing Chemical Formula of Ionic Compounds Based on the Charges of Ions
Chemical compound can be described using chemical formula which represents the elements that are found in a compound. In writing the chemical formula of ionic compound, first identify the cation and write its symbol and charge. Then, identify the anion and write down its symbol and charge. After doing so, write the symbol of the ions to form the compound. Another way of writing the chemical formula of ionic compound is using the crisscross method. In this method, cross the value of charge of each ion to become subscript, the positive and the negative sign will be omitted. Reduce the number of the charges to lowest term and leave out all subscripts that are 1.
[chart: diagram; “Consider the Magnesium Ion and Oxygen Ion.” Steps as printed: 1. Mg2+ O2− (write the charges of each ion); 2. Mg2+ crossed with O2− (cross the charges to become subscript); 3. Mg2 O2 (reduce to lowest term, do not write the value if it is 1); 4. MgO (then write the chemical formula). Values are not labeled on the chart.]
What’s More
Activity 1: Lewis Electron Dot Structure (LEDS)
Identify the group/family and valence electron of each element, then draw their Lewis Dot Structure. (Note: Use your Periodic Table). You may write your answer on a separate sheet of paper.
| Elements | Family/Group | Valence Electron/s | Lewis Symbol |
|---|---|---|---|
| Lithium | IA | 1 | Li· |
| Aluminum | |||
| Bromine | |||
| Sulfur | |||
| Potassium |
(Table continued from the previous page.)
| Elements | Family/Group | Valence Electron/s | Lewis Symbol |
|---|---|---|---|
| Nitrogen | |||
| Carbon | |||
| Fluorine | |||
| Magnesium | |||
| Barium |
Activity 2. Metals versus Non-metals/ Cation vs. Anion
Complete the table below following the given example on number 1 (Lithium). Write your answer on a separate sheet of paper.
| Element | Metal or Nonmetal | Lose or Gain Electrons | Cation or Anion |
|---|---|---|---|
| 1. Lithium | Metal | Lose | Cation |
| 2. Aluminum | |||
| 3. Bromine | |||
| 4. Sulfur | |||
| 5. Potassium | |||
| 6. Nitrogen | |||
| 7. Carbon | |||
| 8. Fluorine | |||
| 9. Magnesium | |||
| 10.Barium |
Activity 3. Gain or lose, you choose!
Identify the valence electrons of the following elements. Determine if they are going to lose or gain an electron, then write their ions. Write your answer on a separate sheet of paper.
| Element | Valence Electron | # of electrons to lose | # of electrons to gain | Ion formed |
|---|---|---|---|---|
| N | 0 | N-3 | ||
| Li | 1 | 1 | ||
| Ca | 2 | |||
| Br | Br- | |||
| Mg | 2 | 0 |
Guide Questions:
- If N gains 3 electrons from another atom, why is it written N-3 (with -3 valence number)?
- If Li loses an electron to another atom, why is it written Li+1 (with +1 valence number)?
- What type of element is Ca as it loses its electrons?
- If Br gains an electron, what type of ion is formed?
- If Mg loses its electron, what type of ion is formed?
What I Have Learned
Write the word that correctly completes the statement. Choose your answer from the box below. Word/s can be used twice. Write your answer on a separate sheet of paper.
Anion, Cation, Crisscross, Eight, Gain, Group, Ionic Bond, LEDS, Loss, Positive, Negative, Stable, Valence Electron
- The _____________ are the outermost electrons which directly involved in chemical bonding.
- _____________ is composed of the symbol of the elements and dots which represent the number of valence electrons of an atom that can easily be determined through the 3. _____________ number in the Periodic Table of Elements.
- An _____________ involves complete transfer of electrons; thus, ions are formed. It involves metals with low electronegativity and non-metals with high electronegativity.
- Metallic elements tend to _____________ their electrons thus forming 6. _____________, positively charged ions.
- Non-metallic elements tend to _____________ electrons thus forming 8. _____________, negatively charged ions.
- In writing the chemical formula of an ionic compound, we write first the symbol of _____________, then followed by the symbol of 10. _____________.
- An atom wants to fill its outermost energy level with _____________ electrons and become 12. _____________.
- Another way of writing the chemical formula of ionic compound is the _____________ method. In this method, cross the value of charge of each ion to become subscript, the 14. _____________ and the 15. _____________ sign will be omitted.
What I Can Do
The Perfect Match
Sodium is a metallic element willing to lose its electron and give to Chlorine during chemical reaction to forms NaCl (Sodium Chloride) commonly known as table salt. Now, it is your turn to match the elements to form an ionic compound. After doing so, determine its cation and anion, illustrate the LEDS, and then write the Chemical Formula on the chart below. Write your answer on a separate sheet of paper.
[illustration: shapes (heart, cloud, star, diamond, oval) each containing an element symbol: K, I, Br, Ca, Ba, S, O, Al, Na, F]
| Cation | Anions | LEDS | Chemical Formula |
|---|---|---|---|
| K+ | F- | K• → :F: [transcriber’s note: the LEDS cell is a printed diagram showing K with a red arrow to F with dots] | KF |
Assessment
Choose the letter of the best answer. Write your answers on a separate sheet of paper.
Why do atoms tend to lose or gain electrons during chemical bonding?
a. to attain beauty
b. to attain stability
c. to become reactive
c. to attain malleabilityWhat do we mean by stable configuration?
a. having 5 electrons in the outermost shell
b. having 6 electrons in the outermost shell
c. having 7 electrons in the outermost shell
d. having 8 electrons in the outermost shellWhat type of element should bond together to form an ionic compound?
a. Metal and Nonmetal
b. Metal and Metalloids
c. Nonmetal and metalloid
d. Nonmetal and another NonmetalWhen a metal and nonmetal atom bond together to form an ionic compound they become ions, what type of ion is formed by the metal atom?
a. Negative Ions
b. Neutral Ions
c. Positive Ions
d. Reactive IonsWhen a metal and nonmetal atom bond together to form an ionic compound they become ions, what type of ion is formed by the nonmetal atom?
a. Negative Ions
b. Neutral Ions
c. Positive Ions
d. Reactive IonsWhat does it mean if K atom becomes K+ ions?
a. it has lost 1 electron
b. it has lost 2 electrons
c. it has gain 1 electron
d. it has gain 2 electronsWhich atom is most likely to form a 3+ ion?
a. Al b. Kr c. Li d. SiWhich is true about the elements in a particular group in the periodic table?
a. they have the same number of protons
b. they have the same number of electrons
c. they have the same number of energy levels
d. they have the same number of valence electronsWhen writing the chemical formula for an ionic compound, which will you write first?
a. Positive ion
b. Negative ion
c. Charge of the ion
d. Subscript of the ionHow will you write the ion of Bromine that gains 1 electron during the process of chemical bonding?
a. B+1 b. B-1 c. Br+1 d. Br-1
Additional Activities
Let’s Find Out!
Complete the crossword puzzle by filling in a word that fits the given clue. Write your answer on a separate sheet of paper.
[chart: crossword puzzle; Let’s Find Out!]
Across
- It refers to the positively charge ions.
- A type of element that tend to gain electrons after chemical bonding.
- It refers to the electrons involved in chemical bonding.
Down
- It refers to the rule when atom is stable and has 8 valence electrons in their outermost shell after chemical bond.
- It refers to the negatively-charge ion.
- A term used when atoms combined through sharing and transferring of electrons.
- It is the columnar arrangement of the elements in the periodic table of elements. This determines the number of valence elect
- These are types of elements that tend to lose electrons during chemical bonding.
- It refers to the arrangement of elements in the periodic table of elements that determines the number or energy shell of each
- It uses dots to represent the valence electrons of the atom.
Created using the Crossword Maker on TheTeachersCorner.net
Answer Key
What I Know
- B
- A
- B
- D
- D
- C
- C
- A
- D
- C
What’s In
- I
- I
- C
- C
- C
- I
- I
- C
- I
- C
What’s More
Activity 1
| Elements | Family/Group | Valence Electron/s | Lewis Symbol |
|---|---|---|---|
| Lithium | IA | 1 | [illustration: Lewis dot symbol of Li] |
| Aluminum | IIIA | 3 | [illustration: Lewis dot symbol of Al] |
| Bromine | VIIA | 7 | [illustration: Lewis dot symbol of Br] |
| Sulfur | VIA | 6 | [illustration: Lewis dot symbol of S] |
| Potassium | IA | 1 | [illustration: Lewis dot symbol of K] |
| Nitrogen | VA | 5 | [illustration: Lewis dot symbol of N] |
| Carbon | IVA | 4 | [illustration: Lewis dot symbol of C] |
| Fluorine | VIIA | 7 | [illustration: Lewis dot symbol of F] |
| Magnesium | IIA | 2 | [illustration: Lewis dot symbol of Mg] |
| Barium | IIA | 2 | [illustration: Lewis dot symbol of Ba] |
Activity 2
| Elements | Metal or Nonmetal | Loss or Gain of Electrons | Cation or Anion |
|---|---|---|---|
| Lithium | Metal | Loss | Cation |
| Aluminum | Metal | Loss | Cation |
| Bromine | Nonmetal | Gain | Anion |
| Sulfur | Nonmetal | Gain | Anion |
| Potassium | Metal | Loss | Cation |
| Nitrogen | Nonmetal | Gain | Anion |
| Carbon | Nonmetal | Gain | Anion |
| Fluorine | Nonmetal | Gain | Anion |
| Magnesium | Metal | Loss | Cation |
| Barium | Metal | Loss | Cation |
What I Can Do
[transcriber’s note: this page is printed rotated 180 degrees; the text has been read in its upright orientation]
| Cation | Anions | LEDS | Chemical Formula |
|---|---|---|---|
| K⁺ | F⁻ | [illustration: LEDS with electron transfer arrow from K to F] | KF |
| Be²⁺ | O²⁻ | [illustration: LEDS with electron transfer arrows from Be to O] | BeO |
| Al³⁺ | Br⁻ | [illustration: LEDS with arrows from Al to two Br atoms; Br⁻ with dots] | AlBr₃ |
| Ca²⁺ | S²⁻ | [illustration: LEDS with electron transfer arrow from Ca to S] | CaS |
| Na⁺ | I⁻ | [illustration: LEDS with electron transfer arrow from Na to I] | NaI |
What I Have Learned
- Valence electron
- LEDS
- Group
- Ionic Bond
- Loss
- Cation
- Gain
- Anion
- Cation
- Anion
- Eight
- Stable
- Crisscross
- Positive
- Negative
Activity 3
| Element | Valence Electron | # of electrons to lose | # of electrons to gain | Ion formed |
|---|---|---|---|---|
| N | 5 | 0 | 3 | N⁻³ |
| Li | 1 | 1 | 0 | Li⁺¹ |
| Ca | 2 | 2 | 0 | Ca⁺² |
| Br | 7 | 0 | 1 | Br⁻¹ |
| Mg | 2 | 2 | 0 | Mg⁺² |
- It is written as N⁻³ since it has 3 more electrons than protons
- It is written as Li⁺¹ since it has 1 more proton than electrons
- Metal
- Anion
- Cation
Across
- (cation) It refers to the positively charge ions.
- (nonmetal) A type of element that tend to gain electrons after chemical bonding.
- (valenceelectron) It refers to the electrons involved in chemical bonding.
Down
- (octet) It refers to the rule when atom is stable and has 8 valence electrons in their outermost shell after chemical bond.
- (anion) It refers to the negatively-charge ion.
- (chemicalbond) A term used when atoms combined through sharing and transferring of electrons.
- (group) It is the columnar arrangement of the elements in the periodic table of elements. This determines the number of valence electrons.
- (metals) These are types of elements that tend to lose electrons during chemical bonding.
- (period) It refers to the arrangement of elements in the periodic table of elements that determines the number or energy shell of each
- (leds) It uses dots to represent the valence electrons of the atom.
[chart: crossword puzzle; answer key for Let’s Find Out!]
[transcriber’s note: the printed page has no heading; the letters in the grid cells are not transcribed]
Assessment
- B
- D
- A
- C
- A
- A
- A
- D
- C
- D
References
Books:
Alvarez, Liza A., Dave G. Angeles, Hernan L. Apurada, Ma. Pilar P. Carmona, Oliver A. Lahorra, Judith F. Marcaida, Ma. Regaele A. Olarte, Estrella C. Osorio, Digna C. Paningbatan, Marivic S. Rosales, and Ma. Teresa B. Delos Santos. Science – Grade 9 Learner’s Module. Pasig City: Department of Education, 2014, 50-71.
Online Resources:
Ionic Bonding Comic Strip – Comic Book Strip by 2cc2c2d1. 5/6/2019. https://www.storyboardthat.com/storyboards/2cc2c2d1/ionic-bondingcomic-strip
Others:
Ignacio, Marilou A., Teacher-made SIM, Are They The Perfect Match?
For inquiries or feedback, please write or call:
Department of Education – Bureau of Learning Resources (DepEd-BLR)
Ground Floor, Bonifacio Bldg., DepEd Complex Meralco Avenue, Pasig City, Philippines 1600
Telefax: (632) 8634-1072; 8634-1054; 8631-4985
Email Address: blr.lrqad@deped.gov.ph * blr.lrpd@deped.gov.ph
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