Saturday, 18 January 2014


1. Reactivity series with chemical symbols in brackets. Memorize them!

Potassium (K)  <----- Most reactive
Sodium (Na)
Calcium (Ca)
Aluminium (Al)
Zinc (Zn)
Iron (Fe)
Lead (Pb)
Hydrogen (H)
Copper (Cu)
Silver (Ag)
Gold  (Au) <--- least reactive

2. Reaction of metals

reactivity series for o level chemistry, secondary school chemistry, senior high school chemistry, reaction of metals with water, reaction of metals with steam, reaction of metals with acid
Reactivity Series - with the most reactive metal at the top of the series

3. Reaction of the metal compounds

3.1 Extraction of metals

extraction of metals, reactivity series,  how to extract metals from their ores
Extraction method of different metals from their iron ores

3.2 Thermal decomposition of metal carbonates (i.e. heating the metal carbonates)

thermal stability of different metal carbonates, and reaction with metal reactivity
Thermal stability of different metals carbonates

4. Displacement reaction of metals
A more reactive metal will displace a less reactive metal.
[i.e. for reaction to occur, the more reactive metal must exist as an element (be by itself), while the less reactive metal must exist as an ionic compound. This is the condition that must be satisfied, for reaction to occur!]

Zn  + CuSO4 ---> ZnSO4 + Cu

Thought process:
Zn vs Cu
Zn is more reactive.

More reactive metal must be by itself, less reactive metal must be in ionic form (or compoud). 
--> Condition satisfied 
--> Got reaction!

Ex. 2
Fe + MgCl2 à No reaction
Thought process:
Fe vs Mg.
Mg is more reactive.
More reactive metal must be by itself, less reactive metal must be in ionic form (or compound). 
--> But magnesium exists as compound here 
--> Condition NOT satisfied 
--> No reaction!

5. Physical Properties of metals

Pure metals are soft because layers of atoms can slide pass each other easily. Alloys are mixtures of metal with other element. Alloys are strong as the different element will disrupt the orderly arrangement of the metal, preventing layers of atoms from sliding pass each other easily.

Metals can conduct electricity because of presence of free moving electrons.

Metals have high melting/ boiling point because of the strong electrostatic forces of attraction between the positive metal cation and negatively charged electrons.

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1 comment:

  1. this is great but could you please include the names of the ores and their chemical formulae for those of us doing the 8-4-4 system.. Thanks a bunch!!!


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