Periodic Table Mind Map

 

GROUP

1

P E R I O D

2

3

4

1 H* 1

2

7 Li 3

8 Be 4

3

4

5

6

7

8

9

Nucleon Number

 󰁁 󰁘

23 Na 11 39

24 Mg 12 40

K 19

Ca 20

󰁚

Proton Number

10

12

4 He 2

13

11 B 5

12 C 6

14 N 7

16 O 8

19 F 9

20 Ne 10

27 Al 13

28 Si 14

31 P 15

32 S 16

35 Cl 17 80

40 Ar 18

Br 35

TRANSITION METALS

First 20 elements

 

Group 1 –Alkali metals

 

Group 2 – Alkali-earth metals.

 

Group 3 to 12 - Transition elements

 

Group 17 – Halogens

 

Group 18 – Noble gases

The group of an element

Period number

Determine by

Determine by

The number of valence electrons

The number of shells occupied with electron

For elements with 1 to 2 valence electrons 

H

ELEMENTS Hydrogen Hajat

Na

ELEMENTS Sodium Nak

He Li Be B C N O

Helium Lithium Berylium Boron Carbon Nitrogen Oxygen

Hendak Lihat Bedah Balas Cinta Nanti Orang

Mg Al Si P S Cl Ar

Magnesium Mgorat Aluminium Alamak Silicon Si Phosporus Peli Sulphur Sedia Chlorine Clewang Argon Aku

F Ne

Flourine Neon

Fikir Niat

K Ca

Potassium Calcium

Kena Chow

1 valence

2 . 8. 8. 1  1 

Potassium has 19 electrons 

4 shells occupied with electrons

1 valence electron   Grou 1

4 electron shells  Period 4

For elements with 3 to 8 valence electrons  4 valence electron   Group 14

First shell: 2 electrons

2 . 8. 4  4  Second shell: 8 electrons Third shell: 8 electrons .

Last electron/s in the last l ast outermost shell, we called as valence electron. PREPARED BY SULAIMAN SMKSM

3 electron shells  Period 3

Add +10 for element with 3 to 8 valence electrons 

 

 

GROUP 18: NOBLE GAS

Elements   Elements Elements Helium Neon Argon Krypton Radon

Chem Chemica icall ro ert ertie iess 

Physical  

 

 

 

Colourless gas Cannot conduct electricity   Poor conductor of heat   Insoluble in water   Low melting point

Electron arrangement 2 2.8 2.8.8 2.8.18.8 2.8.18.32.18.8

Known as monoatomic gas/inert gas Chemically uncreative because 󰁣󰁨󰁥󰁭󰁩󰁣󰁡󰁬󰁬󰁹 󰁵󰁮󰁲󰁥󰁡󰁣󰁴󰁩󰁶󰁥 because they achive octet/duplet electron arrangement   arrangement   Do not release, accept or share electron with other element

Change in Physical properties down a group 18 Atomic size of element increases  increases 

Density of elements increases  increases 

Melting and boiling points of elements increases  increases 

the

Number

of occupied with electron increase  increase 

 When

atomic mass of each element eleme nt is increases. increases.  

atomic size of each element increase increase  



The forces of attraction of each element becomebetween stronger the stronger   atoms  thus more energy is energy is required to overcome the stronger stronger forces of attraction during melting or boiling.  boiling. 

Neon

Helium

Argon

 Used

to fill airships and weather balloons  Used to fill oxygen tank used

   

Used to fill light bulbs

Used in advertising lights and television tubes.

Krypton Xenon  Used

in lasers to repair the retina of the eye  Used to fill photographic flash lamp.

Radon  

 

Used in the brightest bulb in lighthouse

Used in the treatment of cancer.   To detect pipe leakage PREPARED BY SULAIMAN SMKSM

 

PREPARED BY SULAIMAN SMKSM

GROUP 1 (ALKALI METAL) Elements 

Chemical reaction

Soft metals 

Elements

Symbol of Element

Lithium Sodium Potassium Rubidium Caesium Francium

Li Na K Rb Cs Fr

Low melting & boiling points 

 

Reaction with water 2Na + 2H2O 2NaOH + H2

 

Reaction with oxygen 4Na + O2  2Na2O 

Good conductor of electricity 

Physical properties

  

Silvery and shiny surface 

Good conductor of heat and electricity 

Low density 

 

Reaction with halogen 2Na + Cl2  2NaCl 

Less reactive

Change in physical properties down the group 1

Size

Melting and boiling

Reactivity of group 1 depend on ability to lose electron

Densit

Reactivity When size of atom increases atom increases  

points Number of proton increases Number of shells occupied with electron increase

Size increase

When size atom increase Metal bond become weaker Melting and boiling point decrease

Increase mass is faster than increase of atomic radius

Valence electron in the outermost occupied shell becomes far away from the nucleus

The easier to

Force of attraction between the nucleus and valence electron become weaker weaker  

lose an electron, the more reactive

Density increase

It is easier for the atom to donate the single valence electron to achieve stable electron arrangement

Chemical properties and electron arrangement Example:

 

Alkali metals have one  valence  valence electron in their outermost occupied shells.   To achieving the stable electron arrangement (octet or duplet)  

They will donating one electron  from  from its outermost occupied shell to form an ion   with a charge of +1 +1  

Na 2.8.1 K 2.8.8.1

→

+

 

Na   2.8

 

+

→

K  2.8.8

+

e More reactive

+

-

e  Reactivity increase

 

Size

Number of proton increases

Melting and boiling points

Density

When size atom increase

Number of shells occupied with electron increase

Size increase

Elements

Symbol of Element

Flouroine

F

Chlorine

Cl

Bromine

Br

Iodine

I

Increase mass is faster than increase of atomic radius

Force attraction between molecules

Chemical reaction

Elements

Ch Chan an e in h sic ical al ro er erti ties es down down the ro rouu

Reactivity of group 1 depend on ability to attract electron

Reaction with iron 3Cl2  + 2Fe 2FeCl3

 

Reaction halogen with water Cl2  + H2O

 

HCl + HOCl

Reaction halogen with sodium hydroxide 2KOH + Cl2 KCl + KOCl + H2O

Reactivity decrease down a group

Less reactive

When size of atom increases atom increases  

More heat is required to overcome the

Density increase

attractive force

Melting and boiling point

 

The distance of the outermost shell becomes greater greater from  from the nucleus. GROUP 17 (HALOGEN) Valance electron 7 exist as diatomic diatomic   molecules. { F2, Cl2, Br2, I2 } 

The easier to attract an electron, the more reactive

Force of attraction between the nucleus and valence electron become weaker weaker  

increase the tendency of an atom to receive r eceive electrons to achieve an octet electron arrangement decrease decrease..

Chemical properties and electron arrangement    

Alkali metals have 7 valence electron in their outermost occupied shells.



  To achieving the stable electron arrangement (octet or  

Example: Cl2 

+

duplet)

2.8.7

They will accept one electron   to form an ion   with a charge of -1 -1  

Br2  + 2.8.18.7

2e

less reactive

2Cl-  2.8.8

2e

2Br-  2.8.18.8

Reactivity decrease

PREPARED BY SULAIMAN SMKSM

 

Going down a group 1

Change across period 3 Size of element decrease  decrease  

   

Number of proton increase The positive charge of the nucleus increase   The attraction force on nucleus on the electron el ectron become stronger   Electron pull closer to nucleus causes atomic size decrease

 

Lithium (2.1)

Electronegativity increase  increase  Sodium (2.8.1) When atomic size decrease the positive charge charge will increase   The attraction force between nucleus and electron become stronger   The element will easily to accept electron

Na2O

MgO Basic reacts with acid acid to  to form salt salt &  & H2O

Al2O3  Amphoteric can react with both acids & alkali

SiO2  P4O10  SO2  Cl2O7  Acidic reacts with base base to  to form salt & salt  & H2O

Sodium is more reactive than lithium atom   Size of sodium larger than lithium   The attraction forces between nucleus and valence electron in sodium stronger than lithium   Sodium more easily to released electron to form ositive ions

 

Change in oxide properties  properties 

Size of sodium bigger than lithium   The number of proton sodium more mor e than lithium atom   Number of shell occupied with electron of sodium more than lithium atom.

Going down group 17 Fluorine more reactive/electronegative than chlorine:   Size of Fluorine larger than lithium   The attraction forces between nucleus and valence electron in fluorine stronger than chlorine   Fluorine atom easily to accept accept electron to form negative ions

Fluorine(2.7)

Chlori Chlorine ne 2.8.7 2.8.7 Across period of 3

Metallic properties  properties  Na

Mg Metal

Al

Si Metalloid

Transition metal Example: Copper, iron, zinc, Nickel

Form complex ions

Have different oxidation number

P

S Non metal

Cl

Form colour of ions Cu2+ - blue Fe2+ - Green

Act as catalyst Fe – Haber process

Sodium (2.8.1)

Chlorine (2.8.7)

Chlorine atom smaller than sodium:   Number of proton chlorine more than sodium   The attraction force on nucleus on the electron become stronger   Electron pull closer to nucleus causes atomic size decrease

Chlorine atom more electronegat electronegative ive than sodium:   Size of chlorine atom smaller than sodium   The attraction forces between nucleus and valence electron electron in chlorine stronger than than sodium   Chlorine atom easily easily to accept electron to form negative ions

Pt ostwald process

 

2.  Reaction with water, H2O 

1.  Reaction with iron wool,

 

Aim : To : To investigate the halogen with water Problem statements : statements : How does halogen react with water Hypothesis : When : When going down a group of 17, reactivity of halogen toward iron decrease

Aim : To investigate the reactivity of halogen toward iron Problem statements : How does the reactivity of halogen toward iron Hypothesis : When going down a group of 17, reactivity of halogen toward iron decrease

Chlorine 

gas

Iron wool

water Iron

Concentrated

hydrochloric acid

wool

Heat

Variables: Manipulated Responding Constant

Potassium manganate(VII) Heat

liquid

Halogen

Observation Dissolve quickly in water to form

Chlorine, Cl2 

light yellowish solution. blue litmus paper to redTurn and then white Dissolve slowly in water to form brown solution. Turn blue litmus paper to red and then white Dissolve very slowly in water to form brown solution. Turn blue litmus paper to red very slowly

bromine /

Solid Iodine 

Variable

Heat

Action to be taken Repeat the experiment by using different halogen

Bromine, Br2 

Manipulated

Type of halogen

Responding

Reactivity of halogen

Observe the burning of iron

Iodine,

Constant

Size of iron

Use same size of iron metal

I2 

Observation: Halogen

Observation

Chlorine, Cl2 

Iron wool ignites rapidly with bright flame

Bromine,

Iron wool glow moderately

Br2  Iodine, I2 

bright, moderate fast Iron wool glow dimly

PREPARED BY SULAIMAN SMKSM

: Type of halogen used : The rate at which the halogen dissolves in water and product of reaction : temperature of water

3. Reaction with NaOH

Equation 2Fe + 3Cl2 

2FeCl3 

2Fe + 3Br2  2Fe + 3I2 

2FeBr3  2FeI3 

Sodium hydroxide solution

Cl2 + 2H2O

2HCl + 2HOCl

Br2 + H2O

2HBr + 2HOBr

I2 + 2H2O

2HI + 2HOI

Halogen Chlorine, Cl2 

Observation Dissolve rapidly in sodium hydroxide to produce colourless solution.

Bromine, Br2 

Dissolve steadily in sodium hydroxide to produce colourless solution. Dissolve steadily in sodium hydroxide to produce colourless solution.

Chlorine 

gas

Equation

Iodine, I2