1. The document discusses the periodic table and provides details about various groups of elements. It describes the physical and chemical properties of Group 1 alkali metals, Group 17 halogens, transition elements, and Group 18 noble gases. 2. Key physical trends mentioned are that properties like melting point, boiling point, and density increase down a group as atomic size increases. Chemical reactivity also increases down a group as electropositivity increases. 3. The periodic table arranges elements based on proton number and electron configuration, allowing prediction of trends in properties across periods and down groups.

1. CHAPTER 4: PERIODIC TABLE
1.Position element in Periodic Table 3. GROUP 17 (HALOGENS) PHYSICAL PROPERTIES
GROUP - The number of valence electrons Physical properties • colourless gases
PERIOD - The number of shells occupied with electrons Boiling • cannot dissolve in water.
Physical Melting
2. Group 1 (alkali metal) Symbol Colour point • cannot conduct electricity and heat.
state at point
PHYSICAL PROPERTIES • low melting and boiling point.
• Softmetals • low melting & boiling F Gas Yellow • low densities.
points Greenish
Cl Gas
• silvery and • good conductors of yellow M.P and B.P INCREASE DOWN A GROUP
shiny surfaces heat and electricity Reddish because the atomic size of each element
Br Liquid
Melting Boiling brown increases
Density Purplish Increase Increase
symbol Size points points -3
I Solid the forces of attraction between the atoms of
(g cm ) black
(°C) (°C) each element become stronger
Li thus more energy is required to overcome the
M.P and B.P INCREASE DOWN A GROUP
Na stronger forces of attraction
K • the molecular size increases 4.TRANSITION ELEMENTS
Rb Increase Decrease Decrease Decrease • Forces of attraction between molecules becomes Between Group 2 to Group 13
stronger Special Characteristics:
• Need more energy to overcome the forces of attraction i) Form coloured ions or compounds
PHYSICAL CHANGES DOWN A GROUP ii) Have different oxidation numbers
between molecules
The atomic size increases - the number of shells iii) Acts as catalysts
increases. CHEMICAL PROPERTIES
The density increases - increasing in atomic mass is faster X2 + 2NaOH NaX + NaOX + H2O ; X is halogen 5.ELEMENTS IN A PERIOD
than the increasing in atomic volume/size. Fe + 3X2 2FeX3 ; X is halogen - Basic oxides reacts with acid to form salt & H2O
The melting and boiling points decreases - the atomic size X2 + H2O HX + HOX ; X is halogen - Acidic oxides reacts with alkali to form salt & H2O
increases, the metal bond between the metal atoms REACTIVITY decrease down a group - Amphoteric oxides can react with both acids &
becomes weaker. The atomic size increases down the group. alkali
The hardness of the metal decreases. The distance of the outermost shell becomes greater
CHEMICAL PROPERTIES from the nucleus. Atomic size DECREASE
G1 + H2O → alkali + H2 The force of attraction between nucleus valence electrons
G1 + O2 → white solid oxide decrease.
G1 + Cl2 → white solid chloride the proton number increases
the tendency of an atom to receive one/two/three
G1 + Br2 → metal bromide the increasing of the attraction force
electron to achieve an octet electron arrangement
REACTIVITY increase down a group between nucleus and valence electrons.
decrease.
♠ the atomic size increases This causes the electronegativity decreases down the Electronegativity INCREASE
♠ valence electron in the outermost occupied shell becomes group.
far away from the nucleus 4. GROUP 18 ELEMENT
♠ the attraction between the nucleus and the valence electron Size of atom decrease
becomes weaker the increasing of the attraction force
Known as Noble gas
♠ Therefore, it is easier for the atom to donate the single between nucleus and valence electrons.
Monoatomic
valence electron to achieve the stable electron arrangement. chemically unreactive because they achive octet/duplet
♠This causes the electropositivity increase down the group electron arrangement.
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2. Group 1 –Alkali metals
GROUP
Group 2 – Alkali-earth metals.
1 4 Group 3 to 12 - Transition elements
3 4 5 6 7 8 9 10 12
1 H* 2 11 12 13 He Group 17 – Halogens
1 2
Group 18 – Noble gases
7 8 11 12 14 16 19 20
P Nucleon Number
Li Be A B C N O F Ne
E 2 3 4 X 5 6 7 8 9 10 The group of an Period
R
Z Proton Number element number
I 23 24 27 28 31 32 35 40
O 3 Na Mg Al Si P S Cl Ar
D 11 12 13 14 15 16 17 18 Determine by
Determine by
39 40 80
4 K Ca TRANSITION METALS Br
19 20 35 The number of shells
The number of valence
occupied with electron
electrons
First 20 elements For elements with 1 to
2 valence electrons
ELEMENTS ELEMENTS 1 valence 1 valence electron
Group 1
H Hydrogen Hajat Na Sodium Nak 2 . 8. 8. 1
He Helium Hendak Mg Magnesium Mgorat
Li Lithium Lihat Al Aluminium Alamak
Be Berylium Bedah Si Silicon Si 4 shells 4 electron shells
B Boron Balas P Phosporus Peli occupied Period 4
C Carbon Cinta S Sulphur Sedia with
Potassium has 19 electrons
N Nitrogen Nanti Cl Chlorine Clewang electrons
O Oxygen Orang Ar Argon Aku
F Flourine Fikir K Potassium Kena
Ne Neon Niat Ca Calcium Chow For elements with 3 to 8 valence
electrons
First shell: 2 electrons 4 valence electron
Group 14
2 . 8. 4
Second shell: 8 electrons
Third shell: 8 electrons
3 electron shells
Period 3 Add +10 for element
. with 3 to 8 valence
Last electron/s in the last outermost
electrons
shell, we called as valence electron.
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3. GROUP 18: NOBLE GAS
Elements Physical Chemical properties
Elements Electron Colourless gas Known as monoatomic gas/inert gas
arrangement Cannot conduct electricity Chemically uncreative because chemically unreactive
Helium 2 Poor conductor of heat because they achive octet/duplet electron
Neon 2.8 Insoluble in water arrangement
Argon 2.8.8 Low melting point Do not release, accept or share electron with other
element
Krypton 2.8.18.8
Radon 2.8.18.32.18.8
Change in Physical properties down a group 18
Atomic size of element increases Melting and boiling points of Density of elements increases
elements increases
the atomic mass of each element
Number of occupied with
When atomic size of each element increase is increases.
electron increase
The forces of attraction between the atoms
of each element become stronger
thus more energy is required to overcome
the stronger forces of attraction during
melting or boiling.
Helium Argon Neon
Used to fill airships and
weather
Used in advertising lights and
balloons
Used to fill light bulbs television tubes.
Used to fill oxygen tank used
by divers.
Krypton
Xenon Radon
Used in lasers to repair the Used in the treatment of
retina of the eye cancer.
Used in the brightest bulb in
Used to fill photographic flash To detect pipe leakage
lighthouse
lamp. PREPARED BY SULAIMAN SMKSM

4. PREPARED BY SULAIMAN SMKSM
GROUP 1 (ALKALI METAL)
Elements Chemical reaction
Soft metals
Reaction with water
Symbol of Low melting &
Elements Good conductor 2Na + 2H2O 2NaOH + H2
Element boiling points
Li of electricity
Lithium Reaction with oxygen
Physical
Sodium Na 4Na + O2 2Na2O
properties
Potassium K
Rubidium Rb Silvery and shiny Good conductor Reaction with halogen
Caesium Cs surface of heat and 2Na + Cl2 2NaCl
Fr electricity
Francium Low density
Less reactive
Change in physical properties down the group 1
Reactivity of
group 1 depend
Reactivity
Melting and Density on ability to
Size boiling lose electron
points When size of atom increases
Number of proton
When size Increase mass
increases Valence electron in the outermost occupied
atom increase is faster than
increase of shell becomes far away from the nucleus
Number of shells
atomic radius
occupied with Metal bond
electron increase become weaker The easier to
Force of attraction between the nucleus
lose an electron,
Melting and and valence electron become weaker
Density the more
boiling point
Size increase increase reactive
decrease
It is easier for the atom to donate the
Chemical properties and electron arrangement single valence electron to achieve stable
Example: electron arrangement
Alkali metals have one valence electron in their
Na → Na+ + e
outermost occupied shells.
2.8.1 2.8
To achieving the stable electron arrangement (octet or More reactive
duplet) K → K+
+ -
e
They will donating one electron from its outermost 2.8.8.1 2.8.8
occupied shell to form an ion with a charge of +1 Reactivity increase

5. Elements Chemical reaction
Change in physical properties down the group
Reaction with iron
Symbol of 3Cl2 + 2Fe 2FeCl3
Elements
Element
Melting and
Size Flouroine F Reaction halogen with water
boiling Density
Cl2 + H2O HCl + HOCl
points Chlorine Cl
Bromine Br Reaction halogen with sodium hydroxide
When size atom 2KOH + Cl2 KCl + KOCl + H2O
Number of proton Iodine I
increase
increases Increase mass
is faster than
Force increase of Reactivity
attraction atomic radius Reactivity of decrease down
Number of shells
between group 1 depend a group Less reactive
occupied with
molecules on ability to
electron increase
attract electron
More heat is When size of atom increases
required to Density
Size increase overcome the increase
attractive force The distance of the outermost shell
becomes greater from the nucleus.
GROUP 17 (HALOGEN)
Valance electron 7 The easier to
Force of attraction between the nucleus
exist as diatomic attract an
Melting and and valence electron become weaker
molecules. electron, the
boiling point
{ F2, Cl2, Br2, I2 } more reactive
increase
the tendency of an atom to receive
Chemical properties and electron arrangement
electrons to achieve an octet electron
arrangement decrease.
Example:
Alkali metals have 7 valence electron in their outermost
occupied shells. less reactive
Cl2 + 2e 2Cl-
To achieving the stable electron arrangement (octet or
2.8.7 2.8.8
duplet)
They will accept one electron to form an ion with a Br2 + 2e 2Br- Reactivity decrease
charge of -1 2.8.18.7 2.8.18.8
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6. Going down a group 1
Change across period 3 Size of sodium bigger than lithium
The number of proton sodium more than
lithium atom
Size of element decrease
Number of shell occupied with electron
Number of proton increase of sodium more than lithium atom.
Lithium (2.1)
The positive charge of the nucleus increase
The attraction force on nucleus on the electron become stronger Sodium is more reactive than lithium atom
Electron pull closer to nucleus causes atomic size decrease Size of sodium larger than lithium
The attraction forces between nucleus
and valence electron in sodium stronger
Electronegativity increase than lithium
Sodium (2.8.1) Sodium more easily to released electron
to form positive ions
When atomic size decrease the positive charge will increase
The attraction force between nucleus and electron become
stronger Going down group 17
The element will easily to accept electron
Fluorine more reactive/electronegative than
chlorine:
Change in oxide properties Size of Fluorine larger than lithium
Fluorine(2.7)
The attraction forces between nucleus and
valence electron in fluorine stronger than
Na2O MgO Al2O3 SiO2 P4O10 SO2 Cl2O7 chlorine
Basic Amphoteric Acidic Fluorine atom easily to accept electron to
reacts with acid to can react with both reacts with base to form form negative ions
form salt & H2O acids & alkali salt & H2O
Chlorine ( 2.8.7)
Metallic properties Across period of 3
Chlorine atom smaller than sodium:
Na Mg Al Si P S Cl Number of proton chlorine more than sodium
Metal Metalloid Non metal The attraction force on nucleus on the electron
become stronger
Electron pull closer to nucleus causes atomic size
Transition metal Form colour of ions decrease
Example: Sodium (2.8.1)
Cu2+ - blue
Copper, iron, zinc, Nickel Fe2+ - Green Chlorine atom more electronegative than sodium:
Size of chlorine atom smaller than sodium
The attraction forces between nucleus and
valence electron in chlorine stronger than sodium
Act as catalyst
Form complex ions Have different Chlorine atom easily to accept electron to form
Fe – Haber process
oxidation number Chlorine (2.8.7) negative ions
Pt – ostwald process

7. Chemical reaction of Group 1(alkali metal)
Aim: To investigate the reactivity of alkali metal toward React with oxygen gas to produce metal oxides [white React with chlorine gas to produce metal chlorides
water solids]. [white solids].
PS : How does the reactivity of alkali metal toward water
HyPo: when going down a group 1, reactivity of A.M toward Metal G1 + O2 → metal oxide Metal G1 + Cl2 metal chloride
water increase
Gas jar spoon Gas jar spoon
Metal*
White fume Gas jar White fume
water White
Gas jar
Variable Action to be taken Metal* Metal*
Repeat exp using diff. alkali Oxygen gas
M Metal G1 PROCEDURE:
Chlorine gas
Chlorine
metal
Reactivity of Observe movement alkali PROCEDURE:
R
alkali metal metal on water surface PROCEDURE
Size of alkali Use same size of alkali The lithium is heated in jar spoon until its start
C burn and put into gas jar containing oxygen gas The lithium is heated in jar spoon until its start
metal metal
The observation is recorded burn and put into gas jar containing chlorine gas
When the reaction stops, 5 cm3 of distilled water The observation is recorded
RESULT: is poured into gas jar and solution formed is The experiment is repeated with sodium and
Metal* tested with red litmus paper potassium
Observation
Reaction becomes more vigorous
The experiment is repeated with sodium and
Lithium moves slowly on water surface potassium RESULT:
with ‘hiss’ sound. Metal
Reaction becomes more vigorous
Li The colourless solution formed; turns red Observations
RESULT:
litmus paper to blue.
Sodium moves quickly on water surface Metal* Observations Lithium burns slowly with a red flame.
Na with ‘hiss’ sound. Li A white solid is produced.
The colourless solution formed; turns red Lithium burns slowly with a red flame.
litmus paper to blue. Li A white / fume solid is produced. Sodium burns brightly with a yellow
Potassium moves vigorously on water flame.
Na
K surface with ‘hiss’ sound. Sodium burns brightly with a yellow A white solid is produced.
The colourless solution formed; turns red flame. Potassium burns very bright with a
Na
litmus paper to blue. A white solid is produced. purple flame.
K
Potassium burns very bright with a A white solid is produced.
Chemical equation: purple/lilac flame.
K
A white solid is produced.
Chemical Equation
2Li + 2H2O 2LiOH + H2
2Na + 2H2O 2NaOH + H2 Chemical equation
2K + 2H2O 2KOH + H2
2Li + O2 2Li2O 2Li + Cl2 2LiCl2
4Na + O2 2Na2O 2Na + Cl2 2NaCl2
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4K + O2 2K2O 2K + Cl2 2KCl2

8. 1. Reaction with iron wool, 2. Reaction with water, H2O
Aim : To investigate the reactivity of halogen toward iron Aim : To investigate the halogen with water
Problem statements : How does the reactivity of halogen toward iron Problem statements : How does halogen react with water
Hypothesis : When going down a group of 17, reactivity of Hypothesis : When going down a group of 17, reactivity of
halogen toward iron decrease halogen toward iron decrease
Chlorine
gas
Iron wool
water
Variables:
Concentrated Iron
Manipulated : Type of halogen used
hydrochloric acid Heat wool
Responding : The rate at which the halogen dissolves in water and
product of reaction
Potassium Constant : temperature of water
manganate(VII)
liquid Heat Halogen Observation Equation
bromine/ Dissolve quickly in water to form
Solid
Chlorine, light yellowish solution. Turn
Iodine Cl2 + 2H2O 2HCl + 2HOCl
Heat Cl2 blue litmus paper to red and
then white
Variable Action to be taken Dissolve slowly in water to form
Bromine,
Repeat the experiment by using brown solution. Turn blue litmus Br2 + H2O 2HBr + 2HOBr
Manipulated Type of halogen Br2
different halogen paper to red and then white
Reactivity of Dissolve very slowly in water to
Responding Observe the burning of iron Iodine,
halogen form brown solution. Turn blue I2 + 2H2O 2HI + 2HOI
Constant Size of iron Use same size of iron metal I2
litmus paper to red very slowly
Observation:
Halogen Observation Equation 3. Reaction with NaOH Halogen Observation
Chlorine, Iron wool ignites rapidly with Chlorine, Dissolve rapidly in sodium
2Fe + 3Cl2 2FeCl3
Cl2 bright flame Cl2 hydroxide to produce
Bromine, Iron wool glow moderately colourless solution.
2Fe + 3Br2 2FeBr3 Chlorine
Br2 bright, moderate fast Bromine, Dissolve steadily in sodium
gas
Iodine, I2 Iron wool glow dimly 2Fe + 3I2 2FeI3 Br2 hydroxide to produce
colourless solution.
Sodium Iodine, Dissolve steadily in sodium
hydroxide solution I2 hydroxide to produce
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colourless solution.