Metals and non-metals have unique properties. Sodium and potassium have low melting points while mercury is liquid. Most metals like gold and silver are malleable and ductile, allowing them to be formed into wires. Electric wires are coated in plastic to prevent electric shock from conduction. Non-metals like carbon exist in different allotropes with varying properties. Metals react with oxygen to form metal oxides, and react with water to form metal hydroxides and hydrogen gas. More reactive metals can displace less reactive metals from their salt solutions. Metals are extracted from ores through processes like enrichment, roasting, and electrolytic refining.

1. Metals and Non-metals
Jegatheeswari karthik

2. Exception in Metals
• Sodium and potassium are soft and can be cut with a knife. They
have low densities and low melting points.
• Mercury is a liquid.
• Gallium and caesium have very low melting points. It will melt if you
keep them on your hand.

3. Metals
• Most malleable metals - Gold and silver
• Most ductile metal - Gold. From one gram of Gold, a wire of
about 2 km length can be drawn.
It is because of malleability and ductility metals can be given different
shapes according to our needs.
• The best conductors of heat - Silver and Copper
• The poor conductors of heat - Lead and mercury

4. Why electric wires are coated with PVC?
To prevent electric shock.
PVC (Poly vinyl chloride) is the most common insulating material used.
Electric wires are coated in plastic or a rubber like material to prevent
conduction of electricity to people or other metallic and conductive
materials.

5. Exception in Non- metals
• Iodine is a non-metal with Lustrous property.
• Carbon exhibits allotropic nature.
• Allotrope – An element can exist in two or more different physical
forms. Each form is called an allotrope.
• Carbon exits in three allotropic forms.
• Charcoal, Diamond and Graphite.
• Diamond – Natural hardest substance and it has very high melting
and boiling point.
• Graphite - Best Conductor of electricity.

6. Action of metals with Air
• Metals combine with oxygen to form metal oxide.
• Metal + O2 → Metal oxide
• Examples :
• (i) 2Cu + O2 → 2CuO Copper oxide (black)
(ii) 4Al + 3O2 → 2Al2O3 Aluminium oxide
(iii) 2Mg + O2 → 2MgO Magnesium oxide

7. Different metals react in a different way
• Sodium and potassium must be kept immersed in kerosene oil.
Because both of them reacts so vigorously that they catch fire if it
kept open.
• To protect them and to prevent accidental fires.
• Mg, Al, Zn, Pb forms one layer of oxide and it further prevent
oxidation at ordinary temperatures.
• Iron does not burn but iron fillings burn vigorously when sprinkled in
the flame.
• Silver and Gold do not react with oxygen even at high temperature.

8. Action of metals with water
• Metal + Water → Metal oxide + Hydrogen
• Metal oxide + Water → Metal hydroxide
• Examples :
(i) 2Na + 2H2O → 2NaOH + H2 + Heat
(ii) Ca + 2H2O → Ca(OH) 2 + H2
(iii)Mg + 2H2O → Mg(OH)2 + H2
(iv) 2Al + 3H2O → Al2O3 + 3H2
(v) 3Fe + 4H2O → Fe3O4 + 4H2

9. Amphoteric Oxides
Metal oxides which react with both acids as well as bases to produce salts
and water are called amphoteric oxides.
• Examples :
• Al2O3 + 6HCl →2AlCl3 + H2O
• Al2O3 + 2NaOH →2NaAlO2 + H2O
Sodium Aluminate

11. • Calcium and magnesium starts floating because the bubbles of
Hydrogen gas formed stick to the surface of the metal.

12. Action of metals with dilute acids
• Metal + Dilute acid →Salt + H2
• Cu, Ag, Hg do not react with dil. acids.
• Examples :
• (i) Fe + 2HCl →FeCl2 + H2
• (ii) Mg + 2HCl →MgCl2 + H2
• (iii)Zn + 2HCl →ZnCl2 + H2
• (iv) 2Al + 6HCl →2AlCl3 + 3H2

13. Reaction of metal with nitric acid
• Hydrogen gas is not evolved.
• Nitric acid is a strong oxidising agent.
• It oxidises the Hydrogen and reduces itself to form nitrogen oxides.
• Exception
• Magnesium and Manganese
• Initially both will form water but being very strong reducing agents
they remove oxygen from water.

14. Reaction of Metals with Solutions
of other Metal Salts
• Metal A + Salt solution B →Salt solution A + Metal B
• Reactive metals can displace less reactive metals from their
compounds in solution form.
Fe + CuSo4 →FeSo4 + Cu

16. Extraction of Metals from Ores
• Step 1. Enrichment of ores.
• Step 2. Extraction of metals.
• Step 3. Refining of metals.

17. Enrichment of ore
• Usually mineral ores are contaminated by lot of impurities.
• It should be removed before extraction
• Hydraulic washing will be widely used.

19. Extracting Metals Low in the Activity Series
• Metals low in the activity series are very unreactive. The oxides of these
metals can be reduced to metals by heating alone. For example, cinnabar
(HgS) is an ore of mercury.
• When it is heated in air, it is first converted into mercuric oxide (HgO).
• Mercuric oxide is then reduced to mercury on further heating.
2HgS(s) + 3O 2(g)----heat----- 2HgO(s) + 2SO 2 (g)
2HgO(s) -----heat------2Hg(l) + O2(g)
Similarly, copper which is found as Cu2S in nature can be obtained from its
ore by just heating in air.
2Cu 2S + 3O 2 (g) -----heat-----2Cu2O(s) + 2SO2 (g)
2Cu 2O+ Cu2S-----------6Cu(s) + SO2 (g)

20. Extracting Metals in the Middle of the Activity
Series
• The metals in the middle of the activity series such as iron, zinc, lead,
copper, etc., are moderately reactive.
• These are usually present as sulphides or carbonates in nature. It is
easier to obtain a metal from its oxide, as compared to its sulphides
and carbonates.
• The sulphide ores are converted into oxides by heating strongly in the
presence of excess air. This process is known as roasting.

21. • Roasting
• 2ZnS(s) + 3O2 (g) → 2ZnO(s) + 2SO 2 (g)
• Calcination
• ZnCO (s) →ZnO(s) + CO 2 (g)
• The metal oxides are then reduced to the corresponding metals by
using suitable reducing agents such as carbon.
• For example, when zinc oxide is heated with carbon, it is reduced to
metallic zinc.
• ZnO(s) + C(s) →Zn(s) + CO(g)

22. Reduction process
• Heat
• Carbon (coke)
• Sometimes displacement reactions also be used
• High reactive metals Na, Ca and Al is used as reducing agents.
• Example
• Manganese dioxide is treated with Aluminium powder to extract
manganese

23. Thermit reaction

24. Extracting Metals towards the Top of the
Activity Series
• The metals high up in the reactivity series are very reactive. They
cannot be obtained from their compounds by heating with carbon
these metals have more affinity for oxygen than carbon.
• These metals are obtained by electrolytic reduction.
For example, Sodium, magnesium and calcium are obtained by the
electrolysis of their molten chlorides
• The metals are deposited at the cathode (the negatively charged
electrode), whereas, chlorine is liberated at the anode (the positively
charged electrode)

26. Refining of Metals
• The most widely used method for refining impure metal is electrolytic
refining.
Anode : Impure copper
Cathode : Strip of pure copper
Electrolyte : Solution of acidified copper sulphate
(a) On passing the current through electrolyte, the impure metal from
anode dissolves into the electrolyte.
(b) An equivalent amount of pure metal from the electrolyte is
deposited at the cathode.
(c) The insoluble impurities settle down at the bottom of the anode
and is called anode mud.