CHEMISTRY ASSIGNMENT

PERIODIC TABLE

BY
NAME : NUR AISYA BINTI MOHD NAZARUDIN SHAM

CLASS : M3T15
MATRIC NUMBER : MS2117120396

Element is a substance that cannot be decomposed or
separated into simpler substances by chemical reactions. These
elements are arranged and can be found easily in periodic table.

INTRODUCTION

GROUP AND ELEMENTS ELECTRONIC VALENCE PERIOD BLOCK GROUP >
PERIOD CONFIGURATION ELECTRON <
3 s 2
ATOMIC RADIUS Magnesium, 1s2 2s2 2p6 3s2 2 3 p 13
Mg 3 3 p 17
IONIC RADIUS Aluminium, 1s2 2s2 2p6 3s2 3p1 4 p 17
IONISATION Al 1s2 2s2 2p6 3s2 3p5 7 5 p 17
ENERGY Chlorine, 7
Cl 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p5 7
ELECTRONEGATIVITY
Bromine, 1s2 2s2 2p6 3s2 3p63d 104s24p6 4d10
Br 5s2 5p5

Iodine, I

WHY?

INTRODUCTION  The reason why I choose Magnesium, Mg, Aluminum, Al, and >
GROUP AND Chlorine, Cl elements because they are in the same period <
PERIOD which is Period 3 and is easier to compare.

ATOMIC RADIUS  I also choose Chlorine, Cl, Bromine, Br, and Iodine, I elements
because they are located in the same group which is Group 17.
IONIC RADIUS Thus, they are easier to be compared.
IONISATION

ENERGY

ELECTRONEGATIVITY

INTRODUCTION GROUP
GROUP AND
PERIOD • In Periodic Table, it consists of 18 groups.
• Each of the elements’ group is determined by the number of valence
ATOMIC RADIUS
electron. However in p Block cases, the number of valence electron is
IONIC RADIUS
IONISATION added by 10.

ENERGY ELEMENT ELECTRONIC VALENCE BLOCK >
CONFIGURATION ELECTRON s <
ELECTRONEGATIVITY Magnesium, p
Mg 1s2 2s2 2p6 3s2 2 p
Aluminium, P
Al 1s2 2s2 2p6 3s2 3p1 3 p
Chlorine, Cl
Bromine, Br 1s2 2s2 2p6 3s2 3p5 7
1s2 2s2 2p6 3s2 3p6 3d10 4s2 7
Iodine, I
4p5 7
1s2 2s2 2p6 3s2 3p63d 104s24p6
4d10 5s2 5p5

INTRODUCTION Magnesium, Mg •It number of valence electron is 2 >
GROUP AND Aluminium, Al •It is located in the s Block <
PERIOD Chlorine, Cl •Thus, Mg is in Group 2
Bromine, Br
ATOMIC RADIUS •It number of valence electron is 3
Iodine, I •It is located in the p Block
IONIC RADIUS •Thus, Al is in Group 13
IONISATION
•It number of valence electron is 7
ENERGY •It is located in the p Block
•Thus, Cl is in Group 17
ELECTRONEGATIVITY
•It number of valence electron is 7
•It is located in p Block
•Thus, Br is in Group 17

•It has number of valence electron of 7
•It is located in p Block
•Thus, I is in Group 17

Chlorine, Cl, Bromine, Br and Iodine, I are located in the same group which is
Group 17 because they have the same number of valence electron which is 7.

INTRODUCTION PERIOD

GROUP AND • In Periodic Table, it consists of 7 periods.
PERIOD • Each of the elements’ period number is determined by the number of

ATOMIC RADIUS principal quantum number, n of the valence electron shell.

IONIC RADIUS ELEMENT ELECTRONIC NUMBER OF PRINCIPAL BLOCK >
CONFIGURATION QUANTUM NUMBER, n s <
IONISATION Magnesium, p
ENERGY Mg 1s2 2s2 2p6 3s2 3 p
Aluminium, P
ELECTRONEGATIVITY Al 1s2 2s2 2p6 3s2 3p1 3 p
Chlorine, Cl
Bromine, Br 1s2 2s2 2p6 3s2 3p5 3
4
Iodine, I 1s2 2s2 2p6 3s2 3p6 3d10 4s2
4p5 5

1s2 2s2 2p6 3s2 3p63d 104s24p6
4d10 5s2 5p5

INTRODUCTION Magnesium, Mg •The principal quantum number of valence shells, n=3 >
Aluminium, Al •Thus, Mg is in Period 3 <
GROUP AND Chlorine, Cl
PERIOD Bromine, Br •The principal quantum number of valence shells, n=3
•Thus, Al is in Period 3
ATOMIC RADIUS Iodine, I
•The principal quantum number of valence shells, n=3
IONIC RADIUS •Thus, Cl is in Period 3

IONISATION •The principal quantum number of valence shells, n=4
ENERGY •Thus, Br is in Period 4

ELECTRONEGATIVITY •The principal quantum number of valence shells, n=5
•Thus, I is Period 5

Magnesium. Mg, Aluminium, Al and Chlorine, Cl are located in the same period
which is Period 3 because they have the same principal quantum number of
valence shells, n=3.

Atomic radius

is the distance from the atom’s nucleus to the outer part of the
electron cloud of an element.

INTRODUCTION 1. Effective nuclear charge, Zeff TWO FACTORS
GROUP AND
PERIOD • The effective nuclear charge, Zeff is the 2. Screening effect >
“positive charge” felt by an electron. <
ATOMIC RADIUS • Is also known as shielding effect.
Zeff=Z-S
IONIC RADIUS • Screening effect is caused by the
• Electrons moving around the nucleus do mutual repulsion between the
IONISATION not experience the same nucleus inner shell electrons and the outer
ENERGY attraction. shell electrons.

ELECTRONEGATIVITY • Electrons closer to the nucleus • Also occur between electrons of
experience greater nucleus attraction. the same shell but is less effective.

Cl, Al, Mg, Br, I

Ascending order of atomic radius

INTRODUCTION ELEMENT PROTON ELECTRONIC >
GROUP AND Magnesium, Mg NUMBER CONFIGURATION <
PERIOD
12 1s2 2s2 2p6 3s2
ATOMIC RADIUS
Aluminium, Al 13 1s2 2s2 2p6 3s2 3p1
IONIC RADIUS
Chlorine, Cl 17 1s2 2s2 2p6 3s2 3p5
IONISATION Bromine, Br 35 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p5
ENERGY Iodine, I 53 1s2 2s2 2p6 3s2 3p63d 104s24p6 4d10 5s2 5p5

ELECTRONEGATIVITY

Cl, Al, Mg, Br, I

Ascending order of atomic radius

INTRODUCTION  Cl, Al, and Mg, are  Cl is the smallest between  I is the biggest between >
smaller than Br and <
GROUP AND I elements because the 5 elements. the 5 elements.
PERIOD they are located in  It has less shielding effect  It has more shielding
Period 3 and
ATOMIC RADIUS consists only 3 because of less number of effect because of more
shells compared to
IONIC RADIUS Br that is located in shells. number of shells.
IONISATION Period 4 and  So, the distance between  So, the distance
ENERGY consists of 4 shells
and I that is located valence electron and between valence
ELECTRONEGATIVITY in Period 5 and
consists of 5 shells. nucleus decreases. electron and nucleus
 Nucleus attraction towards
increases.
valence electron is  Nucleus attraction

stronger. towards valence
 Therefore, the atomic
stronger is weaker.
radius of Cl is the smallest  Therefore, the atomic

compare to the others radius of I is the biggest

compare to the others.

ATOMIC RADIUS (IN GENERAL)

WHEN MOVING ACROSS THE WHEN MOVING DOWN THE
PERIOD GROUP

• number of protons increase (more protons are added • principal quantum number, n of the valence
to the nucleus, hence nuclear charge also increase) electrons increase.

• Zeff increase significantly. • more inner electrons and inner shells.
• outer electrons are pulled closer to nucleus.
• nucleus-electron attraction increases. • inner electrons shield the outer electrons
• atomic radius becomes smaller. effectively.
• atomic radius generally decrease across a period from
• Screening effect increase.
left to right.
• Valence electrons are attracted weaker and
further away from the nucleus.

• atomic radius generally increase in a group from
top to bottom.

ATOMIC RADIUS (ANALYSIS)

WHEN MOVING ACROSS THE PERIOD WHEN MOVING DOWN THE GROUP

Mg, Al, Cl Cl, Br, I

Descending order of atomic radius Ascending order of atomic radius

• The size of element decreases from Chlorine, Cl Aluminium, Al, • The size of element increases from Chlorine, Cl, Bromine, Br and
and Magnesium, Mg across Period 3. Iodine, I down Group 17.

• This is because, the proton number increases from Cl to Mg. • They are located in the same group because they have 7 valence
electrons.
• Thus, the effective nuclear charge from Cl to Mg is more
significant. • However, the principal quantum number, n and number of shells
increases from Cl to I.
• It pulled electron closer to nucleus and the attraction between
nucleus and valence electron become stronger. • Therefore, the shielding effect also increases from Cl to I because
there are greater number of inner electrons shielding the valence
• Therefore, the atomic radius decreases from Chlorine, Cl electrons in I.
Aluminium, Al, and Magnesium, Mg across Period 3.
• It pushed electrons further from nucleus so, the attraction
between nucleus and valence electron become weaker.

• Therefore, the atomic radius increases from Chlorine, Cl, Bromine,
Br and Iodine, I down Group 7.

IONIC RADIUS

is the distance between the nucleus and the electron in
outermost shell of an ion.

Al3+, Mg2+, Cl-, Br-, I-

INTRODUCTION ELEMENT Ascending order of ionic radius IONIC ELECTRONIC >
GROUP AND CONFIGURATION <
PERIOD Magnesium, Mg CHARGE
Aluminium, Al 1s2 2s2 2p6
ATOMIC RADIUS Chlorine, Cl +2
Bromine, Br
IONIC RADIUS Iodine, I +3 1s2 2s2 2p6
IONISATION
-1 1s2 2s2 2p6 3s2 3p6
ENERGY -1 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

ELECTRONEGATIVITY -1 1s2 2s2 2p6 3s2 3p63d 104s24p6
4d10 5s2 5p6

IN GENERAL

INTRODUCTION POSITIVE IONS cation is smaller than its
atom.
GROUP AND P (CATIONS) smaller than
PERIOD O their neutral atoms. electron cloud shrink.

ATOMIC RADIUS S remaining electrons are
pulled closer towards
IONIC RADIUS I the nucleus.
IONISATION
T >
ENERGY <
I when electrons are
ELECTRONEGATIVITY
V removed from an atom,
repulsion between
E electrons decrease.

I
O

number of proton

N remain, nuclear charge
S remain the same.

INTRODUCTION Al3+, Mg2+, Cl-, Br-, I- >
<
GROUP AND Ascending order of ionic radius
PERIOD
POSITIVE IONS (CATIONS)
ATOMIC RADIUS
o Mg: 1s2 2s2 2p6 3s2
IONIC RADIUS o Mg2+ : 1s2 2s2 2p6

IONISATION  Mg2+ smaller than its neutral atoms, Mg.
ENERGY  this is because when electrons are removed from an atom, repulsion

ELECTRONEGATIVITY between electrons decrease.
 However, number of proton and nuclear charge remain the same.
 So, the remaining electrons are pulled closer towards the nucleus.
 Electron cloud shrink. So, Mg2+ smaller than its neutral atoms, Mg.

IN GENERAL

NEGATIVE IONS electrons cloud enlarge. anions is larger than its
(ANIONS) always larger atom.
than their neutral atoms.
INTRODUCTION outer orbital expands, NEGATIVE >
GROUP AND has more electrons as it nuclear charge remain IONS <
PERIOD gains electron during its
the same.
ATOMIC RADIUS formation.
caused its to spread out
IONIC RADIUS when electrons are & experienced less
IONISATION added to an atom, attraction from the
repulsion between nucleus.
ENERGY electrons increase.

ELECTRONEGATIVITY

INTRODUCTION Al3+, Mg2+, Cl-, Br-, I- >
GROUP AND <
PERIOD Ascending order of ionic radius

ATOMIC RADIUS NEGATIVE IONS (ANIONS)

IONIC RADIUS o Cl: 1s2 2s2 2p6 3s2 3p5
IONISATION o Cl- :1s2 2s2 2p6 3s2 3p6

ENERGY  Cl- is always larger than its neutral atoms, Cl. Cl- has more electrons as it gains
electron during its formation.
ELECTRONEGATIVITY
 When electrons are added to an atom, repulsion between electrons increase.
 This caused electrons to spread out and experienced less attractions from the

nucleus.
 Outer orbital expands, but nuclear charge remain the same.
 So, electrons cloud enlarge.
 Thus, Cl- is always larger than its neutral atoms, Cl.

INTRODUCTION COMPARISON OF IONIC RADIUS >
GROUP AND BETWEEN CATIONS AND ANIONS <
PERIOD
The radius of negative
ATOMIC RADIUS ions are larger than
positive ions.
IONIC RADIUS
IN It is because the
IONISATION GENERAL negative ions have an
ENERGY additional shell. The
additional shell leads to
ELECTRONEGATIVITY
an increase in the
shielding effect.

INTRODUCTION Al3+, Mg2+, Cl-, Br-, I- >
GROUP AND <
Ascending order of ionic radius
PERIOD
o Al3+ : 1s2 2s2 2p6
ATOMIC RADIUS o Mg2+ : 1s2 2s2 2p6
o Cl- :1s2 2s2 2p6 3s2 3p6
IONIC RADIUS o Br- :1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
IONISATION o I- :1s2 2s2 2p6 3s2 3p63d 104s24p6 4d10 5s2 5p6

ENERGY  The ionic radius of negative ions Cl-, Br- and I- are bigger than the ionic
radius of positive ions Al3+ and Mg2+.
ELECTRONEGATIVITY
 This is because the negative ions Cl-, Br- and I- have an additional shell that
leads to the increase of shielding effect.

 So, the attraction between nucleus and valence electron in Cl-, Br- and I-
become more weaker.

 Therefore, the ionic radius of negative ions Cl-, Br- and I- are bigger than
the positive ions Al3+ and Mg2+.

INTRODUCTION Al3+ < Mg2+ < Cl- >
<
GROUP AND o Al3+ : 1s2 2s2 2p6
PERIOD o Mg2+ : 1s2 2s2 2p6
o Cl- :1s2 2s2 2p6 3s2 3p6
ATOMIC RADIUS
• Al3+, Mg2+ and Cl- are located in the same period which is Period 3.
IONIC RADIUS • However, the ionic radius of negative ion Cl- is bigger than the ionic radius of positive

IONISATION ions Al3+ and Mg2+.
ENERGY • This is because the negative ion, Cl- have an additional shell that leads to the increase

ELECTRONEGATIVITY of shielding effect.
• So, the attraction between nucleus and valence electron in Cl- becomes more weaker.
• Therefore, the ionic radius of negative ion, Cl- is bigger than the positive ions, Al3+ and

Mg2+.

Al3+ < Mg2+

ISOELECTRONIC o Al3+ : 1s2 2s2 2p6 Isoelectronic
o Mg2+ : 1s2 2s2 2p6
 Isoelectronic species is a group of
INTRODUCTION atoms or ions having the same • Both Al3+ and Mg2+ are isoelectronic >
GROUP AND electronic configuration. <
PERIOD because they have the same number of
 Across the period, sizes of cations and
ATOMIC RADIUS anions decrease due to the increase electrons and same number of electronic
of proton number and effective
IONIC RADIUS nuclear charge, Zeff. configuration.
IONISATION • However, the ionic radius of Al3+ is smaller

ENERGY than Mg2+.
• This is because, Al3+ has more proton number
ELECTRONEGATIVITY
than Mg2+ .
• This leads to an increase in effective nuclear

charge.
• So, the attraction between nucleus and

valence electron become stronger.
• Thus, the ionic radius of Al3+ is smaller than

Mg2+ .

IONISATION ENERGY, IE

is the minimum energy required to remove an electron from an
isolated gaseous atom or ion in its ground state.

INTRODUCTION FIRST IONISATION ENERGY
GROUP AND
PERIOD is defined as the minimum amount of energy required to remove
an electron from a gaseous atom in its ground state.
ATOMIC RADIUS
FACTOR ATOMIC RADIUS >
IONIC RADIUS AFFECTING <
IONISATION The valence electrons of EFFECTIVE NUCLEAR ENERGY
THE SHIELDING EFFECT
ENERGY IONISATION an atom with a larger The higher the effective
radius experience a less nuclear charge, the The shielding effect of
ELECTRONEGATIVITY ENERGY attraction towards stronger the attraction the electrons of the inner
nucleus, hence possesses forces between the shells causes the outer
a low ionisation energy. nucleus and electrons. electrons to be less
This causes the ionisation attracted to the nucleus
energy to increase. and thus decrease the

magnitude of ionisation

energy.

IONISATION ENERGY (IN GENERAL)

WHEN MOVING ACROSS THE WHEN MOVING DOWN THE
PERIOD GROUP

• Effective nuclear charge increase causes the • Number of shell increase, the shielding effect
size of the atoms to decrease. increase, atomic size also increase.

• Valence electrons are closer to the nucleus . • Valence electrons are farther away from the
• Attractions between the nucleus and the nucleus and held less tightly by the nucleus.

valence electrons are stronger. • Attractions between the nucleus and the
• More difficult to remove an electrons from valence electrons are weaker.

each atom. • Easier to remove an electron from each
• More energy is needed to remove the atom.

outermost electron from an atom. • So, less energy is needed to remove the first
• Thus, ionisation energy (IE) increase. electron.
• In general, IE increases from left to right.
• Thus, ionisation energy decrease.

IONISATION ENERGY

WHEN MOVING ACROSS THE PERIOD WHEN MOVING DOWN THE GROUP

Mg, Al, Cl Cl, Br, I

Ascending order of first ionization energy descending order of first ionization energy

• Cl has higher first ionization energy than Mg and Al because it has • I has lower ionization energy than Cl and Br. This is because, when
more proton numbers. The effective nuclear charge increase. number of shell increases, the shielding also increases. So the
atomic size also increases.
• Valence electrons of Cl are closer to the nucleus than Mg and Cl.
• Valence electrons in I are farther away from the nucleus and held
• So, the attractions between the nucleus and the valence electrons less tightly by the nucleus.
become more stronger and electrons are more difficult to be
removed. • So, attractions between the nucleus and the valence electrons are
weaker.
• So, more energy is needed to remove the outermost electron from
Cl than Mg and Al. • This makes electrons in I are easier to be removed.

• Thus, we can see that the first ionization energy, IE increases • So, less energy is needed to remove the first electron.
across the period from Mg to Cl.
• Thus, we can see that the first ionization energy, IE decreases
when moving down the group from Cl to I.

ANAMALOUS CASE OF IE
The increase of IE with proton number is not uniform

INTRODUCTION ELEMENTS MAGNESIUM, Mg ALUMINIUM, Al >
GROUP AND 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 3p1 <
PERIOD ELECTRONIC
CONFIGURATION 3 3
ATOMIC RADIUS
PRINCIPAL QUANTUM +2 +3
IONIC RADIUS NUMBER
IONISATION 145 pm 118 pm
EFFECTIVE NUCLEAR 737.7 kJ/mol 577.9 kJ/mol
ENERGY CHARGE PARTIALLY FILLED =
LESS STABLE
ELECTRONEGATIVITY ATOMIC RADIUS

FIRST IONISATION ENERGY

FULLY FILLED = MORE
STABLE

INTRODUCTION Mg > Al >
GROUP AND <
PERIOD o Mg: 1s2 2s2 2p6 3s1 (fully filled 3s orbital)
o Al: 1s2 2s2 2p6 3s2 3p1 (partially filled 2p orbital)
ATOMIC RADIUS
 More energy is required to remove electrons from Mg because the
IONIC RADIUS electronic structure of Mg is more stable than expected.

IONISATION  Moreover, the electron in 2p orbital Al is higher in energy, hence less
ENERGY stable and is easier to be removed.

ELECTRONEGATIVITY  Thus, the first ionization energy, IE of Mg is higher than Al.

INTRODUCTION ELECTRONEGATIVITY
GROUP AND
PERIOD is the relative ability of an atom to attract the bonding electrons
to itself when combined with another atom by a chemical bond.
ATOMIC RADIUS
Mg, Al, I, Br, Cl
IONIC RADIUS
IONISATION Ascending order of electronegativity

ENERGY >
<
ELECTRONEGATIVITY

ELECTRONEGATIVITY (IN GENERAL)

WHEN MOVING ACROSS THE WHEN MOVING DOWN THE
PERIOD GROUP

• Proton number increase, nucleus charge • Although the positive charge on the nucleus
become more positive, effective nuclear increases, this is more than the offset by the
charge, Zeff increase. increase in the atomic radius and the additional
screening effect of the extra electron shells.
• So, atomic radius decreases (atomic size
become smaller). • So, going down a group, number of shell
increase, the atomic size increase because the
• Attraction between nucleus and outer screening effect increases.
electron become stronger.
• The attraction of the nucleus and outer
• Hence, the atom has greater relative electron become weaker.
tendency to attract electron to itself.
• Hence, the atom has smaller relative tendency
• Therefore when across a period, the to attract electron to itself.
electronegativity increases.
• Therefore when going down a group, the
electronegativity decreases.

WHEN MOVING ACROSS A PERIOD

INTRODUCTION Mg, Al, Cl,  Mg, Al and Cl are elements that are located in Period 3. >
GROUP AND  But, Cl has stronger electronegativity than Al and Mg. <
PERIOD Ascending order of  This is because, Cl has more proton number than Al and
electronegativity
ATOMIC RADIUS Mg.
 So, effective nuclear charge of Cl is more than Al and Mg.
IONIC RADIUS
Atomic radius in Cl also is smaller than Al and Mg.
IONISATION  So, it pulled electrons in Cl closer to nucleus and the
ENERGY
attraction between nucleus and valence electron is
ELECTRONEGATIVITY stronger.
 Therefore, Cl has greater relative tendency to attract
electron to itself.
 Thus, electronegativity increases when moving down a
group, from Mg to Cl.

WHEN MOVING DOWN A GROUP

INTRODUCTION Cl, Br, I  I, Br, Cl and are elements that are located in Group 17. >
GROUP AND  But, I has weaker electronegativity than Cl and Br. <
PERIOD Descending order of  This is because I has more principal quantum number, n
electronegativity
ATOMIC RADIUS and more number of shells than Br and Cl.
 So, the screening effect also increases from Cl to I
IONIC RADIUS  The electrons in I are pushed further from nucleus so the

IONISATION attraction between nucleus and valence electron is
ENERGY weaker.
 Therefore, I has smaller relative tendency to attract
ELECTRONEGATIVITY electron to itself.
 Thus, electronegativity decreases when moving down a
group, from Cl to I.

LET’S PLAY A GAME! >
<
https://wordwall.net/resource
/22303906/chemistry-quiz

EXPLANATION

1. Given the electronic configuration of element Y is 1s2 2s2 2p6 3s2 3p5 determine the group and the period. >
The answer is Group 17 and Period 3 because the valence electron for element Y is 7 and the principal quantum number is 3. <

2. choose ALL correct points to explain the trend of atomic radius when moving down Group 2 in the Periodic Table.
When moving down a group, the principle quantum number increases. The screening effect increases because more number of inner electrons
is shielding the valence electrons. The valence and nucleus attraction become stronger. Thus, atomic radius increases down a group.

3. which one is the WRONG statement about ionic radius
NEGATIVE IONS (ANIONS) smaller than their neutral atom is wrong because anions are bigger than their natural atoms in term of ionic radius
due to the gaining of electrons while formation.

4. Mg2+ is smaller than Al3+
The statement is false because Al3+ has more proton number than Mg2+ . This leads to an increase in effective nuclear charge. So, the attraction between nucleus and
valence electron become stronger. Thus, the ionic radius of Al3+ is smaller than Mg2+ .

5. why does anomalous case happen?
Because the ionization energy, IE with proton number is not uniform.

6. choose the correct statement of electronegativity
N is less electronegative than O when moving across the period is the correct statement because electronegativity increases w hen moving across a period.

APPLICATION

Camera’s Window’s
body frame

MAGNESIUM, Power lines ALUMINIUM,
Mg Al

As a health A vehicle
supplement for body
heart disease.

APPLICATION

Water An antiseptic Iodine, I
disinfectant
animal feed
CHLORINE, Cl supplements

Pharmaceutical Printing inks
used in the and dyes

manufacture of BROMINE, Br Used in
various drugs pesticides
including those
used to treat As a sedative

diabetes

CONCLUSION

 From this individual assignment, I can conclude that Periodic Table >
is one of the most crucial and biggest achievement in the field of <

Chemistry. It is sufficient and able to give us a better understanding
in the prospect of our daily life. Moreover, I have learnt and know

the trend of the Periodic Table in terms of the elements both in
groups and periods, atomic radius, ionic radius, ionisation energy
and also electronegativity. I have also gain knowledge and develop

a deeper understanding about the use and the trend of the
elements that I have chosen, which is Aluminium, Al, Magnesium,

Mg, Chlorine, Cl, Bromine, Br, and Iodine, I.

REFERENCES:

• chemical element | Definition, Origins, Distribution, & Facts. (n.d.). Encyclopedia Britannica. Retrieved >
<
September 26, 2021, from https://www.britannica.com/science/chemical-element
• periodic table | Definition, Elements, Groups, Charges, Trends, & Facts. (n.d.). Encyclopedia Britannica. Retrieved

September 26, 2021, from https://www.britannica.com/science/periodic-table
• Flagel, J. (2020, July 14). Top 10 Uses of Aluminium in the Industry Today. Materials Blog - Matmatch.

https://matmatch.com/blog/top-10-uses-of-aluminium-in-the-industry-today/
• Worldofchemicals. (2014, February 12). Chlorine role in day to day life. Worldofchemicals.Com.

https://www.worldofchemicals.com/435/chemistry-articles/chlorine-role-in-day-to-day-life.html
• Iodine - Element information, properties and uses | Periodic Table. (n.d.). RSC. Retrieved September 26, 2021,

from https://www.rsc.org/periodic-

table/element/53/iodine#:%7E:text=Today%2C%20iodine%20has%20many%20commercial,polarising%20filters%

20for%20LCD%20displays.
• West, R. H. D. (2019, March 7). Magnesium Supplements: Benefits, Side Effects, and Dosage. Healthline.

https://www.healthline.com/nutrition/magnesium-supplements#magnesium
• A. (2021, February 8). Bromine (Br): Properties & Uses. STUDIOUS GUY. https://studiousguy.com/bromine-uses/
• CHEMISTRY for MATRICULATION Semester 1. (2021). SAP PUBLICATIONS (M) SDN. BHD.

THANK YOU