CHEMISTRY PRESENTATION

THE REACTIVITY SERIES OF METALS

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 .

REACTIVITY SERIES OF COMMON METALS

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.

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.

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

IRON REACTS WITH COPPER SULPHATE

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

SODIUM METAL REACTING WITH CHLORINE GAS

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

Sodium is reacting with Hydrogen Gas

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 .

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

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 .

MADE BY – SANAA SIALCLASS 10TH DAV ACC PUBLIC SCHOOL KATNI MP.