The chemical properties of a substance can be determined by performing experiments that use specific materials or processes with known characteristics. If a material affects the substance in a given way, the substance has a particular property. If a process changes the substance, more properties can be deduced.

1. CHEMISTRY
METALS AND NON
METALS
CHEMICAL PROPERTIES OF METALS

2. Chemical properties of metals
► Action of oxygen on metals
► Metal + Oxygen → Metal oxide (basic)
► Sodium and potassium are kept immersed in kerosene
oil as they react vigorously with air and catch fire.
4K(s)+O2(g)→2K2O(s) (vigorous reaction)
► Copper reacts with oxygen when it is heated. Silver,
platinum, and gold do not react with air.

3. Burning of magnesium ribbon
► 2Mg(s)+O2(g)→2MgO(s)
Magnesium burns with a
white dazzling light in air
and produces a powder
of magnesium oxide. It is
basic in nature.

4. Corrosion
► Metals like Iron, magnesium, aluminum, zinc and copper
rust by prolonged exposure to moist air.
► Copper develops a dull green coating when exposed to
moist air for a long time.
2Cu+H2O+O2+CO2 Cu (OH)2+CuCO3
Iron rusts in moist air as iron reacts with oxygen to form iron
oxide and water.
4Fe +3O2+H20 Fe3O4 +4H2O

5. CORROSION
► A chemical reaction between
metal and its environment is called
corrosion.
► It causes deterioration of material
and its properties.
► Corrosion of iron is called as rusting

6. Reactivity series

7. Reaction of metals with water

8. Reaction of Metals with Water
► Metals react with water to form metal oxide or metal
hydroxide and hydrogen gas.
► Sodium and potassium reacts vigorously with cold water
to produce hydroxides and hydrogen gas that burns
with a pop sound.
2Na+2H2O(cold)→2NaOH+H2+heat
► Ca+2H2O(cold)→Ca(OH)2+H2
► Mg+2H2O(hot)→Mg(OH)2+H2
► 2Al+3H2O(steam)→Al2O3+3H2
► Zn+H2O(steam)→ZnO+H2

9. Action of acids on metals
► Metal + acid salt + hydrogen gas + heat
► 2Na(s)+2HCl(dilute)→2NaCl(aq)+H2(g)
► 2K(s)+H2SO4(dilute)→K2SO4(aq)+H2(g)

10. Reaction of Metals with Bases
► Metal do not react with bases. Aluminium, lead and zinc
reacts with strong bases like sodium hydroxide and
potassium hydroxide to form complex compounds and
evolution of hydrogen gas.
► Base+metal→salt+hydrogen
► 2NaOH(aq)+Zn(s)→Na2ZnO2(aq)+H2(g),
► when zinc reacts with aqueous sodium hydroxide it
gives sodium zincate and hydrogen gas.

11. Displacement reaction
► Reaction of Metals with Solutions of Other Metal Salts
► Metal A + Salt Solution of Metal B → Salt Solution of Metal
A + Metal B
► More reactive metals replaces less reactive metals.
► Less reactive metals cannot replace more reactive
metals.
► For Example:
► Iron + Copper Sulphate → Iron Sulphate + Copper
► Fe + CuSO4 → FeSO4 + Cu