Presentation on Reactive series of metals .

1. CHEMISTRY PRESENTATION
THE REACTIVITY SERIES OF METALS

2. REACTIVITY SERIES
The arrangement of metals in the decreasing order of their
reactivity is called ACTIVITY SERIES OF METALS .
In Reactivity series , the most reactive metal is placed at top
whereas least reactive metal is placed at the bottom .

3. REACTIVITY SERIES OF COMMON METALS

4. Displacement reactions of metal oxides
• A more reactive metal will displace a less reactive metal from a
compound. The thermite reaction is a good example of this. It is
used to produce white hot molten (liquid) iron in remote locations
for welding. A lot of heat is needed to start the reaction, but then
it releases an incredible amount of heat, enough to melt the iron.

5. Displacement reactions of metal oxides
• Here Copper cannot displace Zinc -
so it must be the least reactive and be
at the bottom of this reactivity series.
• Zinc displaces Copper - so it must be
the most reactive and be at the top of
this reactivity series.

6. REACTION OF METALS WITH SALT SOLUTIONS
• When a more reactive metal is put in the salt solution of a less
reactive metal , then the more reactive metal displaces the less
reactive metal from its solutions.
• Metal A + Salt of metal B ⇨ Salt of metal A + Metal B
• For example , Iron displaces copper from copper sulphate
solution.
• Fe + CuSO4 ⇨ FeSO4 + Cu

7. IRON REACTS WITH
COPPER SULPHATE

8. REACTION OF METALS WITH CHLORINE
• Metals react with CHLORINE to form ionic CHLORIDES .
• In the formation of metal chlorides , the metal atoms lose
electrons and become positively charged ions , whereas chlorine
atom gains electrons and become negatively charged chloride ions
.
• For example ,
2Na + Cl ⇨ 2NaCl

9. SODIUM METAL REACTING WITH
CHLORINE GAS

10. REACTION OF METALS WITH HYDROGEN
• Metals generally do not react with hydrogen because metals form
compounds by losing electrons and hydrogen also forms compounds by
losing electron .
• Most of the metals do not combine with hydrogen . Only a few reactive
metals like sodium , potassium , calcium and magnesium react with
hydrogen to form metal hydrides .
For example ,
2Na + H2 ⇨ 2NaH

11. Sodium is reacting with
Hydrogen Gas

12. EXTRACTION OF METALS
Metals are available in the form of their ores .
Methods of extraction are based on their REACTIVITY .
Methods of Extraction are :
• Reduction
• Electrolysis
 REDUCTION : It is the process of removal of oxygen for extraction of
metals from their oxide ores .

13. REDUCTION
• It is the process of removal of
oxygen for extraction of metals
from their oxide ores .
FOR EXAMPLE ,
• copper(II) oxide + hydrogen →
copper + water
• CuO + H2 → Cu + H2O

14. ELECTROLYSIS
• The oxides of metals which are
very highly reactive cannot be
reduced by CARBON,
CARBONMONOXIDE AND
HYDROGEN .
• They are reduced by the process of
decomposition .

15. MADE BY –
SANAA SIAL
CLASS 10TH
DAV ACC PUBLIC SCHOOL
KATNI MP.