Republic of the Philippines

Department of Education

Regional Office IX, Zamboanga Peninsula

8

Name of Learner: ___________________________

Grade & Section: ___________________________

Name of School: ___________________________

SCIENCE Quarter 3 - Module 8

PERIODIC PROPERTIES

OF ELEMENTS

Science- Grade 8 Support Material for Independent Learning Engagement (SMILE) Quarter 3 - Module 8: Periodic Properties of Elements First Edition, 2021

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Development Team of the Module

Writer: Galo M. Salinas

Editor: Teodelen S. Aleta

Reviewers: Teodelen S. Aleta, Zyhrine P. Mayormita

Lay-out Artists: Zyhrine P. Mayormita, Chris Raymund M. Bermudo

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Ronillo S. Yarag - Education Program Supervisor, LRMS

Zyhrine P. Mayormita - Education Program Supervisor, Science

Leo Martinno O. Alejo - Project Development Officer II, LRMS

Janette A. Zamoras - Public Schools District Supervisor

Adrian G. Refugio - School Principal, Zamboanga del Norte NHS

1

What I Need to Know

The modern periodic table is a very valuable tool for predicting the chemistry of elements. It summarizes relationships that exist among elements and their compounds. Thus, many individual properties of elements need not be memorized if periodic relationships are known.

This module will further broaden your knowledge about the elements. It

allows you to explore the modern periodic table in terms of the following periodic

properties of the elements: atomic size, ionization energy, metallic character,

electronegativity, and electron affinity. After going through this module, you are

expected to:

1. Use the periodic table to predict the chemical behavior of an element

(S8MT- IIIi-j-12).

Specifically, this module will let you recognize the trends in atomic size,

ionization energy, metallic character, electronegativity, and electron affinity of

elements across the period and down the family.

What's In In the previous module, you were able to identify the elements in the modern periodic table arranged in groups and periods; representative and transition elements, metals, metalloids, and non-metals. In this module, we focus on the variations in atomic properties that are useful in predicting the chemical behavior of elements. Activity 1: The Periodic Properties Direction: Use the clues to solve the puzzle.

Across 1. ability to attract electrons 4. repeating trends in element properties Down 2. ability to accept electrons 3. adj., the character of an atom to readily lose an electron 5. energy to remove an electron from an atom

2

What's New

The periodic properties of elements can be related to human behavior. Below

is a short excerpt from the chapter Argon in Primo Levi's book "The Periodic Table".

According to Levi, a chemist, and writer, each element had an associative

value—its properties symbolizing certain thoughts and activating specific memories. He describes Argon as a rare gas, part of the air we breathe and need to survive but not always noticed or appreciated.

In what way does Levi identify with Argon?

What does the element symbolize about his Jewish background?

The rotations of planets, seasons, high and low tides are periodic processes in our solar system and nature. Ancient astronomers and astrologers used these observations to regulate the activities of individuals or even of nations. Periodicity is an essential part of our life, as evidenced by the beating of the heart and our eating, sleeping, and waking patterns.

The elements in the periodic table are arranged in order of increasing atomic number. These elements display several other trends, and we can use the periodic table to predict their chemical, physical, and atomic properties.

Activity 2: Connecting circles!

Direction: Using graphs A and B, connect all circles by increasing atomic number with a thin straight line.

“The little I know about my ancestors presents many similarities to these gases. Not all of them were materially inert, for that was not granted them. On the contrary, they were—or had to be— quite active, in order to earn a living and because of a reigning morality that held that “he who does not work shall not eat.” But there is no doubt that they were inert in their inner spirits, inclined to disinterested speculation, witty discourses, elegant, sophisticated, and gratuitous discussion. It can hardly be by chance that all deeds attributed to them, though quite various, have in common a touch of the static, an attitude of dignified abstention, of voluntary (or accepted) relegation to the margins of the great river of life.” Adopted from: What Element Are You Lesson Plan. https://kenanfellows.org//kfp-cp-sites/cp04/cp04/sites/kfp-cp-sites.localhost.com.cp04/files/What%20Element%20are%20You%20Lesson%20Plan.pdf

Figure 1. Graphical Representation of Atomic Radius vs Atomic Number Source: http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf

3

Interpret the data as presented in the graph and answer these questions:

1. How do you describe the line that connects all circles in Graph A? What about

Graph B? _________________________________________________________________ ____________________________________________________

2. What does the line in Graph A mean? What about the line in Graph B? You may refer to the periodic table for your answer. ____________________________ ____________________________________________________

What is It

The periodic law states that when the elements are arranged in order of increasing atomic number, their physical and chemical properties vary periodically. In this module, we will look at the following physical and chemical properties of an atom, namely; atomic size, ionization energy, metallic character, electronegativity, and electron affinity.

Periodic trends are specific patterns present in the periodic table that illustrate different aspects of a certain element. The trends provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or periods and because of the periodic nature of the elements.

Atomic Size The atomic radius of a

chemical element is the measure of the size of its atoms. The atomic radius is one-half the distance between the nuclei of two atoms (just like a radius is half the diameter of a circle). Thus, based on the atomic radii, the atomic size patterns are observed throughout the periodic table. The following are the general trends in the size of atomic radii:

Figure 2. Graphical Representation of First Ionization Energy vs Atomic Number Source: http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf

Periodic table showing trends in atomic size Image Source: https://lavelle.chem.ucla.edu/forum/viewtopic.

4

1. Within each period (horizontal row), the atomic radius tends to decrease with the atomic number (nuclear charge). The largest atom in a period is a Group IA atom and the smallest is a Group VIIIA or noble gas atom. 2. Within each group (vertical column), the atomic radius tends to increase with the period number.

Ionization Energy

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase.

Conceptually, ionization energy is the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikely it is that the atom becomes a

cation (kat·ai·aan). Generally, elements on the right side of the periodic table have higher ionization energy because their

outermost level occupied by the electron is nearly filled. Elements on the left side of the periodic table have low ionization energies because of their willingness to lose electrons and become cations. Thus, ionization energy increases from left to

right on the periodic table. Metallic Character

The metallic character of an element can be defined as how readily an atom can lose an electron. From right to left across a period, the metallic character increases because the attraction between the outermost electron and the atomic nucleus is weaker, enabling it easier to lose electrons. Metallic character increases as you move down a group because the atomic size is increasing. When the atomic size increases, the outer level of an

atom occupied by an electron is farther away. The principal energy level of an atom occupied by an electron increases, and average electron density moves farther from the nucleus. The electrons of the valence shell have less attraction to the nucleus and, as a result, can lose electrons more readily. This causes an increase in metallic character.

● Metallic characteristics decrease from left to right across a period. This is caused by the decrease in radius of the atom that allows the outer electrons to ionize more readily

Periodic table showing ionization energy trends Source: https://chem.libretexts.org/Bookshelves/Inorganic. Chemistry/Modules_and_Websites_(Inorganic_Chemistry) /Descriptive_Chemistry/Periodic_Trends_of_Elemental_Properties/Periodic_Trends

Periodic table trends in metallic character

5

● Metallic characteristics increase down a group. Electron shielding causes the atomic radius to increase, so the outer electrons ionize more readily than electrons in smaller atoms.

● Metallic character relates to the ability to lose electrons, and nonmetallic

character relates to the ability to gain electrons.

Electronegativity Electronegativity can be

understood as a chemical property describing an atom's ability to attract and bind with electrons. In 1934, Robert S. Mulliken, an American physicist, and chemist suggested on theoretical grounds that the electronegativity (X) of an atom be given as half its ionization energy (I.E.) minus electron

affinity (E.A.).

X = 𝐼.𝐸. − 𝐸.𝐴.

2

The nature of electronegativity is effectively described thus: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons toward itself.

● From left to right across a period of elements, electronegativity increases.

● From top to bottom down a group, electronegativity decreases.

● Important exceptions to the above rules include the noble gases, lanthanides, and actinides. The noble gases possess a complete valence shell and do not usually attract electrons. The lanthanides and actinides possess more complicated chemistry that does not generally follow any trends. Therefore, noble gases, lanthanides, and actinides do not have electronegativity values.

● As for the transition metals, although they have electronegativity values, there is little variance among them across the period and up and down a group. This is because their metallic properties affect their ability to attract electrons as easily as the other elements.

Electron Affinity

As the name suggests, electron affinity is the ability of an atom to accept an electron. Unlike electronegativity, electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom. The more negative the electron affinity value, the higher an atom's affinity for electrons.

Electron affinity generally decreases down a group of elements because each atom is larger than the atom above it. This means that when an atom is getting larger due to an added electron, this makes an electron to be farther away from the atom's nucleus compared with its position in the smaller atom. With a larger distance between the negatively-charged electron and the positively-charged nucleus, the force of attraction is relatively weaker. Therefore, electron affinity decreases. Moving from left to right across a period, atoms become smaller as the forces of attraction

Periodic table trends in electronegativity

6

become stronger. This causes the electron to move closer to the nucleus, thus increasing the electron affinity from left to right across a period.

● Electron affinity increases from left to right within a period. This is caused

by the decrease in atomic radius. ● Electron affinity decreases from top to bottom within a group. This is caused

by the increase in atomic radius.

Figure 6. Periodic table showing electron affinity trend. Source: https://socratic.org/chemistry/the-periodic-table/periodic-trends-in-electron-affinity

What's More

Activity 3. Chart Chat

Values of Ionization Energy, Atomic Size & Electron Affinities for Halogens

Halogen

Ionization

Energy

(eV)

Atomic Size

(nm)

Electron Affinity

(eV)

F 17.18 0.072 4.27

Cl 13.01 0.099 4.01

Br 11.84 0.114 3.78

I 10.454 0.133 3.43

From the given chart above, answer the following questions.

1. What trend in the electron affinity values of the halogen elements do you

observe from top to bottom of the family?

2. Which atoms release more energy as they gain or accept electrons, the

smaller or bigger atoms? Why?

3. Which atoms easily gain or accept electrons, the smaller or bigger atoms?

Why?

7

4. Which atoms have greater electron affinity, those with low ionization energy

or those with high ionization energy? Why?

5. Which atoms have the greater electron affinity, metals or non-metals? Why?

What I Have Learned

Periodic trends are specific patterns that are present in the periodic table that

illustrate different aspects of a certain element, including its size and its electronic properties.

The atomic size of a chemical element is a measure of the size of its atoms.

Within each period (horizontal row), the atomic size through its radius tends to decrease with increasing atomic number (nuclear charge). The largest atom in a period is a Group IA atom, and the smallest is a noble-gas atom. Within each group

(vertical column), the atomic size tends to increase with the period number. Ionization energy is the energy required to remove an electron from a neutral

atom in its gaseous phase. Conceptually, ionization energy is the opposite of

electronegativity. Ionization energy increases from left to right (across the period) on

the periodic table because of increasing attraction between the positive nucleus and negative outermost electron of the atom. On the other hand, as a family is descended, the number of energy levels occupied by the electron of an atom increases because this outweighs the effect of a higher nuclear charge. As the distance of the outer electrons from the nucleus increases, ionization energy decreases.

The metallic character of an element can be defined as how readily an atom can lose an electron. From right to left across a period, the metallic character increases because the attraction between the level of an atom occupied by the electron and the nucleus is weaker, enabling an easier loss of electrons. Metallic character increases as you move down a group because the atomic size is increasing.

Electronegativity can be understood as a chemical property describing an atom's ability to attract and bind with electrons. It increases from bottom to top in groups and increases from left to the right across periods.

Electron affinity is the ability of an atom to accept an electron. Electron affinity increases from left to right within a period and decreases from top to bottom within a group.

What I Can Do Activity 4. Supply me!

Direction: Answer what is asked in each of the items below. 1. Order the following elements by increasing atomic radius according to what

you expect from periodic trends: Se, S, As. 2. Using periodic trends, arrange the following elements by increasing ionization

energy: Ar, Na, Cl, Al. 3. In terms of electron affinity, which member of each of the following pairs has

the greater negative value: (a) As, Br (b) F, Li.

8

Assessment Direction: Read each question carefully and choose the best answer. Circle the letter that corresponds to your answer.

1. Consider the following sequence: I. Al < Si < P < S II. Be < Mg < Ca < Sr III. I < Br < Cl < F Which of these give(s) a correct trend in increasing atomic size? a. I only c. III only b. II only d. I and II only

2. Compared with the electronegativities of the elements on the left side of the period, the electronegativities of the elements on the right side of the same period tend to be _____. a. lower c. the same

b. higher d. unpredictable

3. Which of the following is NOT a trend that varies periodically in the periodic table? a. Electronegativity c. Ionization energy b. Symbols of elements d. Atomic radius

4. Use the periodic table to predict which element has the largest ionization

energy. a. Phosphorus c. Arsenic b. Sulfur d. Selenium

5. Use the periodic table to predict which element has the largest atomic size.

a. Lithium c. Sodium b. Beryllium d. Magnesium

6. Electronegativity tends to increase as you:

a. go down a column of the periodic table b. go from left to right across the periodic table c. go toward the middle of the periodic table d. go from upper left-hand corner to the lower right-hand corner of the

periodic table

7. From the position of elements in the periodic table, the most metallic element is ___. a. lead c. tin b. bismuth d. antimony

8. The willingness of an atom to receive electrons is measured by its ____.

a. electron affinity c. ionization energy b. atomic size d. electronegativity

9. Given the elements inside the box below, which order shows an increasing

electronegativity? [S, Se, Cl, Br and P] a. P, Se, S, Br, Cl c. S, P, Se, Cl, Br b. S, Br, P, Se, Cl d. P, Se, Br, S, Cl

9

10. Which of the following elements has the lowest electron affinity?

a. Manganese c. Iron b. Technetium d. Ruthenium

Additional Activities

Activity 5: Graphing Periodic Trends Directions: Do at least one of the three graphs. Remember that the Periodic Table arranged the elements according to the Periodic Law: when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern. Graph 1 – Atomic Radius as a function of Atomic Number

A. Create a graph of the atomic radius as a function of atomic number. Plot atomic number on the X axis and atomic radius on the Y axis. Remember to label the axes!

B. Use a colored pen, pencil or highlighter to trace over the element's period (horizontal row on the periodic table). For example: use GREEN to trace for all of the elements in row 1, then use YELLOW to trace for all of the elements in row 2, then use ORANGE to trace for all the elements in row 3, then use BLUE to trace for all the elements in row 4.

Symbol Atomic Number

Atomic Radius(pm)

Symbol Atomic Number

Atomic Radius(pm)

H 1 37 Na 11 157

He 2 50 Mg 12 136

Li 3 123 Al 13 125

Be 4 89 Si 14 117

B 5 80 P 15 110

C 6 77 S 16 104

N 7 70 Cl 17 99

O 8 66 Ar 18 98

F 9 64 K 19 203

Ne 10 67 Ca 20 174

10

1. Describe the trend in atomic

radius as the atomic number increases across a period.

2. Describe the trend in atomic

radius as the atomic number increases down a group.

Graph 2 – First Ionization

Energy as a function of Atomic Number A. Create a graph of the

ionization energy as a function of atomic number. Plot atomic number on the X axis and ionization energy on the Y axis. Remember to label the axes!

B. Use a colored pen, pencil or highlighter to trace over the element's period (horizontal row on the periodic table). For example: use GREEN to trace for all of the elements in row 1, then use YELLOW to trace for all of the elements in row 2, then use ORANGE to trace for all the elements in row 3, then use BLUE to trace for all the elements in row 4.

Symbol Atomic Number

First Ionization

Energy (kJ/mol)

Symbol Atomic Number

First Ionization

Energy (kJ/mol)

H 1 314 Na 11 119

He 2 688 Mg 12 176

Li 3 124 Al 13 138

Be 4 215 Si 14 188

B 5 191 P 15 242

C 6 260 S 16 239

N 7 335 Cl 17 299

O 8 314 Ar 18 363

F 9 402 K 19 100

Ne 10 497 Ca 20 141

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3. Describe the trend in

ionization energy as the atomic number increases

across a period. 4. Describe the trend in

ionization energy as the atomic number increases down a group.

Graph 3 – Electronegativity as a function of Atomic Number A. Create a graph of the

electronegativity as a function of atomic number. Plot atomic number on the

X-axis and electronegativity on the Y-axis. Remember to label the axes!

B. Use a colored pen, pencil, or highlighter to trace over the element's period (horizontal row on the periodic table). For example: use GREEN to trace for all of the elements in row 1, then use YELLOW to trace for all of the elements in row 2, then use ORANGE to trace for all the elements in row 3, then use BLUE to trace for all the elements in row 4.

Symbol Atomic Number

Electronegativity

H 1 2.1

He 2 0

Li 3 1.0

Be 4 1.5

B 5 2.0

C 6 2.5

N 7 3.0

O 8 3.5

F 9 4.0

Ne 10 0

Na 11 0.9

Mg 12 2.0

Al 13 1.5

Si 14 1.8

P 15 2.1

S 16 2.5

Cl 17 3.0

Ar 18 0

K 19 0.8

Ca 20 1.0

12

5. Describe the trend in electronegativity as the atomic number increases across a period.

6. Describe the trend in electronegativity as the atomic number increases down a group.

7. Why do you think the electronegativity of He, Ne, and Ar is 0?

Answer Key Gr8Q3 Module 8

Activity 1. The Periodic Properties Across 1. Electronegativity Across 4. Periodicity Down 2. Affinity Down 3. Metallic Down 5. Ionization Activity 2. Connecting circles Answers may vary.

The line is crooked (like the saw teeth with sharp edges or amplitude of a speaker) for both the graphs. Both graphs also show a periodic pattern.

In Graph A, atomic radius is greater at certain atomic numbers. It shows that as x increases, y sometimes increases and sometimes decreases. With reference to the periodic table, the pattern is indeed periodic showing that atomic radius decreases from right to left and bottom to top. In Graph B, at certain atomic numbers, first ionization energy appears to be higher. With reference to the periodic table, ionization energy increases from left

to right and from bottom to top.

Activity 3. Chart Chat Decreasing

Smaller atom. It is because the

smaller the atom is, the closer the

outermost shell is; therefore, it has

stronger attraction between the positive

nucleus and the negative incoming

electron.

Smaller atom. It is because when

the atom is smaller, the outermost shell is

closer to the nucleus, making their

attraction stronger as it gains electron.

High ionization energy. It is

because when the ability of an atom to

accept electron is stronger, then its ability

to release an electron is likewise stronger.

Nonmetals. It is because

nonmetals will prefer to accept electrons

for the attraction between the nucleus and

the gained electron is stronger.

Activity 4. Supply me! S, Se, As

Na, Al, Cl, Ar

a. Br

b. F

ASSESSMENT B

B B C C B A A D

B

13

References Book Ebbing, D. D., & Gammon, S. D. (2009). General Chemistry Ninth Edition. New York:

Houghton Mifflin Company. Mendoza, E.E., & Religioso, T.F. (1990). Chemistry, Phoenix Publishing House, Inc, Quezon City. DECS, SEDP. (1991). Science and Technology III Textbook, First Edition. Instructional

Materials Corporation. DepEd. (2009). Chemistry Textook, Science and Technology for Third Year High School. The Editors of Encyclopaedia Britannica. 2021. "The Periodic Table." Britannica. Accessed

January 10, 2021. https://www.britannica.com/topic/The-Periodic-Table. The Jewish Community Library. n.d. "Guide to Primo Levi Periodic Table." The Periodic

Table. Accessed January 10, 2021. https://static1.squarespace.com/static/54402d4fe4b0f9a2742ba309/t/564639a6e4b09d684e5c50d1/1447442854437/Periodic+Table+Guide.pdf.

Online Sources https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Modules_and_Websites_(Ino

rganic_Chemistry)/Descriptive_Chemistry/Periodic_Trends_of_Elemental_Properties/Periodic_Trends

https://courses.lumenlearning.com/introchem/chapter/atomic-size/ http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf https://studylib.net/doc/5891887/graphing-periodic-trends

Images http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map%3A_Introductory_

Chemistry_(Tro)/09%3A_Electrons_in_Atoms_and_the_Periodic_Table/9.09%3A_Periodic_Trends-_Atomic_Size_Ionization_Energy_and_Metallic_Character

https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Modules_and_Websites_(Ino

rganic_Chemistry)/Descriptive_Chemistry/Periodic_Trends_of_Elemental_Properties/Periodic_Trends

https://www.google.com/url?sa=i&url=https%3A%2F%2Fchem.libretexts.org%2FBookshelv

es%2FInorganic_Chemistry%2FModules_and_Websites_(Inorganic_Chemistry)%2FDescriptive_Chemistry%2FPeriodic_Trends_of_Elemental_Properties%2FPeriodic_Trends&psig=AOvVaw2Zk_o_xuKumKJzxtwW07OT&ust=1610536106701000&source=images&cd=vfe&ved=0CA0QjhxqFwoTCKDEndiglu4CFQAAAAAdAAAAABAD

https://socratic.org/chemistry/the-periodic-table/periodic-trends-in-electron-affinity

14

Region IX: Zamboanga Peninsula Hymn – Our Eden Land Here the trees and flowers bloom

Here the breezes gently Blow,

Here the birds sing Merrily,

The liberty forever Stays,

Here the Badjaos roam the seas

Here the Samals live in peace

Here the Tausogs thrive so free

With the Yakans in unity

Gallant men And Ladies fair

Linger with love and care

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Are visions you’ll never forget

Oh! That’s Region IX

Hardworking people Abound,

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Zamboangueños, Tagalogs, Bicolanos,

Cebuanos, Ilocanos, Subanons, Boholanos, Ilongos,

All of them are proud and true

Region IX our Eden Land

Region IX

Our..

Eden...

Land...

My Final Farewell Farewell, dear Fatherland, clime of the sun caress'd

Pearl of the Orient seas, our Eden lost!,

Gladly now I go to give thee this faded life's best,

And were it brighter, fresher, or more blest

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On the field of battle, 'mid the frenzy of fight,

Others have given their lives, without doubt or heed;

The place matters not-cypress or laurel or lily white,

Scaffold or open plain, combat or martyrdom's plight,

T is ever the same, to serve our home and country's need.

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Through the gloom of night, to herald the day;

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Pour'd out at need for thy dear sake

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My dreams, when life first opened to me,

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Were to see thy lov'd face, O gem of the Orient sea

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If over my grave some day thou seest grow,

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Draw it to thy lips and kiss my soul so,

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The touch of thy tenderness, thy breath's warm power.

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Let it trill there its hymn of peace to my ashes.

Let the sun draw the vapors up to the sky,

And heavenward in purity bear my tardy protest

Let some kind soul o 'er my untimely fate sigh,

And in the still evening a prayer be lifted on high

From thee, 0 my country, that in God I may rest.

Pray for all those that hapless have died,

For all who have suffered the unmeasur'd pain;

For our mothers that bitterly their woes have cried,

For widows and orphans, for captives by torture tried

And then for thyself that redemption thou mayst gain

And when the dark night wraps the graveyard around

With only the dead in their v igil to see

Break not my repose or the mystery profound

And perchance thou mayst hear a sad hymn resound

'T is I, O my country, raising a song unto thee.

And even my grave is remembered no more

Unmark'd by never a cross nor a stone

Let the plow sweep through it, the spade turn it o 'er

That my ashes may carpet earthly f loor,

Before into nothingness at last they are blown.

Then will obliv ion bring to me no care

As over thy vales and plains I sweep;

Throbbing and cleansed in thy space and air

With color and light, with song and lament I fare,

Ever repeating the faith that I keep.

My Fatherland ador'd, that sadness to my sorrow lends

Beloved Filipinas, hear now my last good-by!

I give thee all: parents and kindred and friends

For I go where no slave before the oppressor bends,

Where faith can never kill, and God reigns e'er on high!

Farewell to you all, from my soul torn away,

Friends of my chi ldhood in the home dispossessed!

Give thanks that I rest from the wearisome day!

Farewell to thee, too, sweet friend that lightened my way;

Beloved creatures al l, farewell ! In death there is rest !

I Am a Filipino, by Carlos P. Romulo I am a Filipino–inheritor of a glorious past, hostage to the uncertain

future. As such I must prove equal to a two-fold task–the task of

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I am a Filipino. In my blood runs the immortal seed of heroes–seed

that flowered down the centuries in deeds of courage and defiance.

In my veins yet pulses the same hot blood that sent Lapulapu to

battle against the first invader of this land, that nerved Lakandula

in the combat against the alien foe, that drove Diego Silang and

Dagohoy into rebellion against the foreign oppressor.

The seed I bear within me is an immortal seed. It is the mark of my

manhood, the symbol of dignity as a human being. Like the seeds

that were once buried in the tomb of Tutankhamen many thousand

years ago, it shall grow and flower and bear fruit again. It is the

insignia of my race, and my generation is but a stage in the

unending search of my people for freedom and happiness.

I am a Filipino, child of the marriage of the East and the West. The

East, with its languor and mysticism, its passivity and endurance,

was my mother, and my sire was the West that came thundering

across the seas with the Cross and Sword and the Machine. I am of

the East, an eager participant in its spirit, and in its struggles for

liberation from the imperialist yoke. But I also know that the East

must awake from its centuried sleep, shake off the lethargy that has

bound his limbs, and start moving where destiny awaits.

I am a Filipino, and this is my inheritance. What pledge shall I give

that I may prove worthy of my inheritance? I shall give the pledge

that has come ringing down the corridors of the centuries, and it

shall be compounded of the joyous cries of my Malayan forebears

when first they saw the contours of this land loom before their eyes,

of the battle cries that have resounded in every field of combat from

Mactan to Tirad Pass, of the voices of my people when they sing:

“I am a Filipino born to freedom, and I shall not rest until freedom

shall have been added unto my inheritance—for myself and my

children and my children’s children—forever.”