Republic of the Philippines
Department of Education
Regional Office IX, Zamboanga Peninsula
8
SCIENCE
Quarter 3 - Module 8
PERIODIC PROPERTIES
OF ELEMENTS
Name of Learner: ___________________________
Grade & Section: ___________________________
Name of School:
___________________________
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
Management Team: Virgilio P. Batan Jr.
Lourma I. Poculan
- Schools Division Superintendent
- Asst. Schools Division Superintendent
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Ronillo S. Yarag
- Education Program Supervisor, LRMS
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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
1
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".
“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-cpsites.localhost.com.cp04/files/What%20Element%20are%20You%20Lesson%20Plan.pdf
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.
Figure 1. Graphical Representation of Atomic Radius vs Atomic Number
Source: http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf
2
Figure 2. Graphical Representation of First Ionization Energy vs Atomic Number
Source: http://homework.sdmesa.edu/dgergens/chem100l/periodicity/periodic_table_lab.pdf
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:
Periodic table showing trends in atomic size
Image Source: https://lavelle.chem.ucla.edu/forum/viewtopic.
3
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,
Periodic table showing ionization energy trends
elements
on the right side of
Source: https://chem.libretexts.org/Bookshelves/Inorganic.
Chemistry/Modules_and_Websites_(Inorganic_Chemistry)
the
periodic
table have higher
/Descriptive_Chemistry/Periodic_Trends_of_Elemental_Properties/Periodic_Trends
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
Periodic table trends in metallic character
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
4
●
●
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.).
𝐼.𝐸. − 𝐸.𝐴.
X=
2
Periodic table trends in electronegativity
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
5
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
Ionization
Halogen
Energy
Atomic Size
Electron Affinity
(nm)
(eV)
(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?
6
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.
7
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
8
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
H
He
Li
Be
B
C
N
O
F
Ne
Atomic
Number
1
2
3
4
5
6
7
8
9
10
Atomic
Radius(pm)
37
50
123
89
80
77
70
66
64
67
Symbol
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
9
Atomic
Number
11
12
13
14
15
16
17
18
19
20
Atomic
Radius(pm)
157
136
125
117
110
104
99
98
203
174
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
H
He
Li
Be
B
C
N
O
F
Ne
1
2
3
4
5
6
7
8
9
10
First
Ionization
Energy
(kJ/mol)
314
688
124
215
191
260
335
314
402
497
10
Symbol
Atomic
Number
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
11
12
13
14
15
16
17
18
19
20
First
Ionization
Energy
(kJ/mol)
119
176
138
188
242
239
299
363
100
141
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
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
2.1
0
1.0
1.5
2.0
2.5
3.0
3.5
4.0
0
0.9
2.0
1.5
1.8
2.1
2.5
3.0
0
0.8
1.0
11
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
Nonmetals. It is because
nonmetals will prefer to accept electrons
for the attraction between the nucleus and
the gained electron is stronger.
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.
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.
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.
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.
Activity 3. Chart Chat
Decreasing
b. F
a. Br
Na, Al, Cl, Ar
Activity 4. Supply
me!
S, Se, As
B
B
C
C
B
A
A
D
B
ASSESSMENT
B
12
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/564639a6e
4b09d684e5c50d1/1447442854437/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_Pe
riodic_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_Propertie
s/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)%2F
Descriptive_Chemistry%2FPeriodic_Trends_of_Elemental_Properties%2FPeriodic_Tr
ends&psig=AOvVaw2Zk_o_xuKumKJzxtwW07OT&ust=1610536106701000&sourc
e=images&cd=vfe&ved=0CA0QjhxqFwoTCKDEndiglu4CFQAAAAAdAAAAABAD
https://socratic.org/chemistry/the-periodic-table/periodic-trends-in-electron-affinity
13
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Here the trees and flowers bloom
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The liberty forever Stays,
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Linger with love and care
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Are visions you’ll never forget
Oh! That’s Region IX
Here the Badjaos roam the seas
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With the Yakans in unity
Hardworking people Abound,
Every valleys and Dale
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
Still would I give it thee, nor count the cost.
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.
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.
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
I die just when I see the dawn break,
Through the gloom of night, to herald the day;
And if color is lacking my blood thou shalt take,
Pour'd out at need for thy dear sake
To dye with its crimson the waking ray.
An d when t he d ar k night wr a p s t he gr av eyar d ar o un d
Wit h only t he de a d in t heir v igil t o se e
Br ea k n ot my r e p os e or t he m yst er y pr of o un d
An d p er ch anc e t ho u m ayst he ar a sa d hy mn r es o un d
'T i s I, O m y c ou nt r y, r aising a s ong unt o t hee.
My dreams, when life first opened to me,
My dreams, when the hopes of youth beat high,
Were to see thy lov'd face, O gem of the Orient sea
From gloom and grief, from care and sorrow free;
No blush on thy brow, no tear in thine eye.
An d ev en my gr av e i s r em em ber ed n o m or e
Unmar k' d by nev er a cr os s nor a st on e
Let t he pl ow sw ee p t hr o ugh it , t he s p ad e t ur n it o 'er
That m y ash es m ay c ar p et ear t hly f l oor ,
Bef or e int o not hi ngne ss at l ast t hey ar e bl own.
Dream of my life, my living and burning desire,
All hail ! cries the soul that is now to take flight;
All hail ! And sweet it is for thee to expire ;
To die for thy sake, that thou mayst aspire;
And sleep in thy bosom eternity's long night.
The n will o bliv i on br in g t o m e no car e
As ov er t hy v ales an d plai ns I swe ep;
Thr o b bing an d cle ans e d in t hy s pac e an d air
Wit h col or an d light , wit h s ong an d l ame nt I f ar e,
Ev er r e pe at ing t he f ait h t hat I ke ep.
If over my grave some day thou seest grow,
In the grassy sod, a humble flower,
Draw it to thy lips and kiss my soul so,
While I may feel on my brow in the cold tomb below
The touch of thy tenderness, thy breath's warm power.
My F at her lan d a d or ' d, t hat s adn es s t o m y s or r ow le n ds
Bel ov e d Fili pin as, h ear no w my la st go o d - by!
I giv e t hee all: par ent s an d kin dr e d an d f r ien ds
For I g o wher e no slav e bef or e t he op pr ess or ben ds,
Wher e f ait h c an nev er k ill, an d G o d r eig n s e' er on hi gh!
Let the moon beam over me soft and serene,
Let the dawn shed over me its radiant flashes,
Let the wind with sad lament over me keen ;
And if on my cross a bird should be seen,
Let it trill there its hymn of peace to my ashes.
Far ew ell t o y o u all, f r o m my s o ul t or n a way,
Fr ien ds of my chi ldh o o d in t he h om e di s po ss es se d!
Giv e t han ks t hat I r est f r om t h e wear i so me da y!
Far ew ell t o t hee, t o o, swe et f r ien d t hat lig ht ene d my way;
Bel ov e d cr e at ur es al l, f ar ewell ! In d eat h t her e is r est !
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
meeting my responsibility to the past, and the task of performing
my obligation to the future.
I sprung from a hardy race, child many generations removed of
ancient Malayan pioneers. Across the centuries the memory comes
rushing back to me: of brown-skinned men putting out to sea in
ships that were as frail as their hearts were stout. Over the sea I see
them come, borne upon the billowing wave and the whistling wind,
carried upon the mighty swell of hope–hope in the free abundance
of new land that was to be their home and their children’s forever.
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.”
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