PERIODIC TABLE - NUR ATHINA BINTI ROSMAN

SK015 CHEMISTRY ASSIGNMENT PERIODIC TABLE

NAME: NUR ATHINA BINTI ROSMAN
CLASS: M3T15
MATRIC NUMBER: MS2017174540
LECTURER’S NAME: MUHAMAD AZRANI BIN
ZAMERAHIM

Introduction Analysis Comparison Application Conclusion References

Index

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Introduction Analysis Comparison

SK015 CHEMISTRY ASSIGNMENT Application Conclusion References

Introduction Analysis Comparison Application Conclusion References

Introduction

01 The 5 elements I have chosen are Potassium, Calcium, Boron, Aluminum

and Gallium.

02 The reason I have chosen Potassium (K) and Calcium (Ca) because they

are located in the same period (Period 4). Thus, they can show variation of

atomic radius, ionic radius, ionization energy and electronegativity across

a period.

03 The reason I have chosen Boron (B), Aluminium (Al) and Gallium (Ga)
because they are located in the same group (Group 13). Thus, they can
SK015 CHEMISTRY ASSIGNMENT
show variation of atomic radius, ionic radius, ionization energy and

electronegativity across a group.

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Elements in Group

Elements Potassium Calcium Boron Aluminium Gallium
13
Group 12 13 13
1s2 2s2 2p1
Electronic 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2
Configuration 3p6 4s1 3p6 4s2 3p1 3p6 3d10 4s2 4p1

Number of valence 1 2 3 3 3
electron p-block p-block p-block
s-block Semimetal Basic metal Basic metal
SK015 CHEMISTRY ASSIGNMENT Types of block s-block Alkaline earth

Classification Alkaline metal metal

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Elements in Period

❏ The od t er i t ar be f 1 to 7 m o r t.
❏ Per um = Pri p u n nu r ( ) o t ec n va c el

Elements Potassium Calcium Boron Aluminium Gallium

Period 4 4 2 3 4

Electronic 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 1s2 2s2 2p1 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2
Configuration 3p6 4s1 3p6 4s2 3p1 3p6 3d10 4s2 4p1

SK015 CHEMISTRY ASSIGNMENT Principal quantum 4 4 2 3 4
of the electrons in s-block s-block p-block p-block p-block
valence shell (n)

Types of block

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Analysis

SK015 CHEMISTRY ASSIGNMENT Elements Group Explanation
Potassium 1
Calcium 2 Potassium is located at s-block. It has 1 valence electron in 4s orbital. Thus, it is
13 located in Group 1.
Boron 13
Aluminum 13 Calcium is located at s-block. It has 2 valence electrons in 4s orbital. Thus, it is
located in Group 2.
Gallium
Boron is located at p-block. It has 3 valence electrons in 2s and 2p orbitals. Thus,
it is located in Group 13.

Aluminum is located at p-block. It has 3 valence electrons in 3s and 3p orbitals.
Thus, it is located in Group 13.

Gallium is located at p-block. It has 3 valence electrons in 4s and 4p orbitals.
Thus, it is located in Group 13.

Introduction Analysis Comparison Application Conclusion References

SK015 CHEMISTRY ASSIGNMENT Analysis

● Elements in periodic table are arranged in ascending order of proton number.
● Elements of the periodic table in the same group as the same number of

valence electrons.
● Potassium, Calcium and Gallium have the highest principal quantum number

(n) of the valence electrons, 4 thus they are in the same period (Period 4)
● Boron, Aluminium and Gallium are located at p-block and have 3 valence

electrons therefore they are in the same group (Group 13).
● Group number for elements in block-s and block-d = Number of valence

electron
● Group number for elements in block-p = Number of valence electron + 10

Introduction Analysis Comparison Application Conclusion References

SK015 CHEMISTRY ASSIGNMENT Atomic Radius

● Size/radius of atom is difficult to be defined because the electron cloud has
no clear boundary.

● Atomic radius DECREASES across the period and INCREASES down the
group.

● The atomic radii of an element is determined by two factors:
★ E-ffeNcettiv e n tui c le ha r c eh ax r g ei ,nZ e f f b he t o .

Zeff = Z –

★ Screening effect
- Ca s y e m a r si t e t i n h el r an h u s l
el r .
- Al o c et el r of s e h b i l ffec

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Ionic Radius

Smaller than Larger than
neutral neutral
atoms atoms

Electron Positive Electrons removed Electron Negative Electrons are
cloud shrink ions from an atom, cloud ions added to an atom,
repulsion between
(Cations) repulsion between enlarge (Anions)
electrons electrons
decreases increases

SK015 CHEMISTRY ASSIGNMENT Number of Outer orbital Has more
protons and expands,
Remaining Zeff remain the electrons as it
electrons are same experienced gains electron
pulled closer less attraction
to the nucleus during its
from the forremmaatiinonthZeeff
nucleus.
same

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Overview of Ionic Radius

SK015 CHEMISTRY ASSIGNMENT Ion Ele r Num f Zeff ● Since all of the elements I have chosen are positive ions (cations),
K+ co fi r i el r therefore they are smaller than their neutral atoms.
Ca2+ 1s2 2s2 2p6 3s2 19-18
B+ 18 = +1 ● Across a period: K+ > Ca2+> Ga3+
Al3+ 3p6 18 20 - 18
Ga3+ 1s2 2s2 2p6 3s2 4 = +2 (increasing size)
10 5-4
3p6 28 = +1 ● Down a group: B+ < Al3+ < Ga3+
1s2 2s2 13 - 10
= +3 (increasing size)
1s2 2s2 2p6 31 - 28
= +3 ● Across period 4, the ionic radii of cations from K+ decrease to Ga3+ (1s2
1s2 2s2 2p6 3s2 2s2 2p6 3s2 3p6)
3p6 3d10
● Down the Group 13, the ionic radii of cations increase from B+ to Ga3+

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Ionization Energy

★ General definition: The minimum energy required to remove an electron
from a gaseous atom or ion in its gaseous state.

Ac o s P i Ac o s G u Factors affecting the
Zeff in se e s o d as Num f el n as , s i d eff c c e , ionisation energy:
- Atomic radius
Val el r ar se t uc at si so r a
A ra n e w he l u d va c Val el r ar t e w ro c u - Effective nuclear
A ra n e w he l u d va c e t s charge
el r ar r er
ar a r - Shielding effect

SK015 CHEMISTRY ASSIGNMENT Mor ffi ul r o n e t s er e m Eas o r e n e t f e c om s e r
en y e d is ed mo h e t

Ion i n e g c a Ion i n e g c a

I in se m o r t I de se n g o

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Analysis

Com so t e P t i m Cal Com so t e B r a d G um
Cal at s (Z = 20) mo nu r ro s, Z t a p si om The p i c qu m u b , n of n e c on in l u m (n =
(Z = 19). 4) is te h ro (n = 2)

Epffo e c s u nua t r( Z e ffar= + 1()Zeff ) of ca m at (Zeff = +2) hi r n Gal at s o n er ne c on d er l t a
bo at .

A ra n e w al el r an c u n Ca at s on Shi n eff t Ga at g e r an B at . A ac of n e
co r o K at . H ce, ic us C a m s a l t a K at el r an r r a f nu s i Ga at we t a B at .
be e t ec n ud Ca at re r d an K at . Ato s e Ga at bi r co r o B at .

SK015 CHEMISTRY ASSIGNMENT It i mo fficu to l e t in Ca at m a d K at . It i mo a r to ve t o s Ga at h B at . H ce, s
The re, en y e d em he e m le r n Ca at en y e d o r e t le le r n Ga at t e t B
t a K at . at .

By at, fi t i at e r f Ca at hi r t a K at . The re, fi t i at e r f Ga at lo t a B at .

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Electronegativity

❏ Electronegativity is a chemical property that describes the tendency of an atom to attract electrons (or electron
density) of covalent bonds towards itself.

❏ Atom with strong attraction of the nucleus and the outer electron have the high electronegativity.

Electronegativity

Across a period Down a group

Proton number, nucleus Atomic radius Number of shell increase, Atom has weaker relative
charge more positive decreases the atomic size increase tendency to attract
and Zeff increase. electron to itself
SK015 CHEMISTRY ASSIGNMENT because of screening
effect

Atom has greater Across a period, Down a group,
tendency to attract electronegativity electronegativity

electron to itself increases. decreases.

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Overview Electronegativity

Ac o s P ri 4 Dow h G u 13

K at s e s b o p n (Z = 19) t a C to h h B at s (Z = 5), Al a h (Z = 13) an G s (Z = 31). Ga t
mo m e f to (Z = 20). ha r u b el r he w p ci q a m be ,
(n = 4) be n a f m.

Epffo e c s u nua t r( Z e ffar= + 1()Zeff ) of ca m at (Zeff = +2) hi r n Bor om t g e r e d y a c ec n to l
t a l i m a n al at .

SK015 CHEMISTRY ASSIGNMENT The ic of C ma r pa t K a . A ra n Gal ha h hi s lu n an p i c he t el g
be n u l a d n e c on C is r r an K eff c h or d a ni .
at .

Ca t i m e c ne ve n K o b u C at s Al a s o le r at ha G we B to t os
g e r e t e n c o r el r to l om d o K el r e t e n he .
at .

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Application

Quiz: Periodic Table

SK015 CHEMISTRY ASSIGNMENT Click Me To improve your knowledge about periodic
table, do click the icon on your left! Or, you can
simply click the ‘Application folder’ at the
bottom. A very simple quiz to determine your
understanding.
Link: https://forms.gle/2jP6yUFens6HsRuG7

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SK015 CHEMISTRY ASSIGNMENT Application

Explanations:

1. The elements in periodic table are arranged in ascending order of proton number.
2. Shielding effect is caused by the mutual repulsion between inner shell electrons and the outer shell electrons.
3. Inner electrons and outer shell electrons created the mutual repulsion.
4. Dmitri Mendeleev stated that if the element is in block p, its group number equal to number of valence electron +
10.
5. In his periodic table, Mendeleev arranged elements in rows by increasing atomic mass. Within a row, elements with
lower atomic masses were on the left. Mendeleev started a new row every time the chemical properties of the
elements repeated.
6. Silicon is used because it can be used as either an insulator. This is important for making chips.
7. The vast majority of the elements in the periodic table are metals. Metal show a wide range of chemical and
physical properties.
8. Horizontal row = period and vertical column = group.
9. He found that the properties of the elements seemed to repeat every eighth element. He called this the Law of
Octaves, comparing it to musical scales.
10. Ionization energy is the minimum energy required to remove an electron from a gaseous atom or ion in its ground
state.

Introduction Analysis Comparison Application Conclusion References

SK015 CHEMISTRY ASSIGNMENT Conclusion

From this assignment, I could conclude that I have truly explored and thoroughly discussed the
topic of periodic table based on its atomic radii, ionic radii, electronegativity, ionisation energy
with the chosen elements.

❏ Across a period, electronegativity and ionisation energy increased however atomic radius
and ionic radius decrease.

❏ Across a period meanwhile down a group, atomic radii and ionic radii increase but
electronegativity decrease.

I would like to give an appreciation notes with huge thanks to my lecturer, Sir Muhamad Azrani
who guided me through this assignment journey. Thank you to all of you who participated
directly or indirectly with me thru the process of finalizing my assignment.

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See you next time!

SK015 CHEMISTRY ASSIGNMENT Click Me

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SK015 CHEMISTRY ASSIGNMENT References

Websites
1. Academy, K. (2019, September 13). Periodic trends and Coulomb’s law | Atomic structure and properties | AP Chemistry | Khan Academy. YouTube.

Accessed on September 27, 2021. Retrieved from https://www.youtube.com/watch?v=gi2Y-kbrjCw&feature=youtu.be
2. Periodic Table - Quiz. (2016, July 31). Quizziz. Accessed on September 23, 2021. Retrieved from

https://quizizz.com/admin/quiz/58292ce5086db54b75f9900d/periodic-table
3. Michael, D. (2021, September 8). Periodic Table - Ptable. Ptable. Accessed on September 25, 2021. Retrieved from https://ptable.com/?lang=en#Properties
4. Lagowski, J. J. (1998, October 30). periodic table | Definition, Elements, Groups, Charges, Trends, & Facts. Encyclopedia Britannica.

https://www.britannica.com/science/periodic-table
Books
1. Ternstrom, T. (1964). A periodic table. Journal of Chemical Education, 41(4), 190. Accessed on September 28,2021. Retrieved from
https://doi.org/10.1021/ed041p190

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