Slide 2: Examples of Common Metals

• Iron (Fe)
• Aluminium (Al)
• Copper (Cu)
• Zinc (Zn)
• Silver (Ag)
• Gold (Au)
• Lead (Pb)
• Tin (Sn)
• Mercury (Hg)

Slide 3: Types of Ores

• Definition of ore
• Types of ores:
  • Oxides
  • Sulphides
  • Carbonates
  • Halides

Slide 4: Extraction of Iron from its Ore

• Iron extraction flowchart
• Steps involved in the extraction of iron:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Calcination
  4. Smelting
  5. Refining

Slide 5: Extraction of Aluminium from its Ore

• Aluminium extraction flowchart
• Steps involved in the extraction of aluminium:
  1. Crushing and grinding the ore
  2. Digestion or leaching of the ore
  3. Concentration of the ore
  4. Electrolytic reduction of aluminium oxide
  5. Purification of aluminium

Slide 6: Extraction of Copper from its Ore

• Copper extraction flowchart
• Steps involved in the extraction of copper:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Roasting
  4. Smelting
  5. Refining

Slide 7: Extraction of Zinc from its Ore

• Zinc extraction flowchart
• Steps involved in the extraction of zinc:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Roasting
  4. Smelting
  5. Refining

Slide 8: Extraction of Silver from its Ore

• Silver extraction flowchart
• Steps involved in the extraction of silver:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Roasting
  4. Smelting
  5. Refining

Slide 9: Extraction of Gold from its Ore

• Gold extraction flowchart
• Steps involved in the extraction of gold:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Roasting
  4. Smelting
  5. Refining

Slide 10: Extraction of Lead from its Ore

• Lead extraction flowchart
• Steps involved in the extraction of lead:
  1. Crushing and grinding the ore
  2. Concentration of the ore
  3. Roasting
  4. Smelting
  5. Refining

11. Physical Properties of Metals

• High electrical and thermal conductivity
• Malleability and ductility
• Lustre and reflectivity
• High melting and boiling points
• Solid state at room temperature (except mercury)
• Good conductors of heat and electricity

12. Chemical Properties of Metals

• Reactivity with oxygen: Examples include rusting of iron and tarnishing of silver
• Reaction with acids: Metals react with acids to produce salts and hydrogen gas
• Reaction with water: Some metals react with water to form metal oxides or hydroxides and hydrogen gas
• Reactivity series: Arrangement of metals in a decreasing order of their reactivity

13. Displacement Reactions

• Definition of a displacement reaction
• The more reactive metal displaces the less reactive metal from its compound
• Example: Zinc displaces copper from copper sulfate solution
  • Zn(s) + CuSO4(aq) -> ZnSO4(aq) + Cu(s)

14. Acid-Base Reactions Involving Metals

• Reaction of metals with bases: Metals react with bases to produce metal hydroxides and hydrogen gas
• Reaction of metals with metal salts: Metals react with metal salts to produce another metal and a salt solution

15. Metal Oxides and Metal Hydroxides

• Formation of metal oxides: Metals combine with oxygen to form metal oxides
• Formation of metal hydroxides: Metals react with water to form metal hydroxides
• Example: Sodium oxide + water -> Sodium hydroxide

16. Metal Carbonates and Hydrogencarbonates

• Reaction of metals with carbonates: Metals react with carbonates to form metal oxides and carbon dioxide gas
• Reaction of metals with hydrogencarbonates: Metals react with hydrogencarbonates to form metal carbonates, water, and carbon dioxide gas

17. Reactivity Series of Metals

• Definition of the reactivity series
• Arrangement of metals in a decreasing order of their reactivity
• Importance of the reactivity series in predicting displacement reactions

18. Extraction of Metals using Electrolysis

• Definition of electrolysis
• Extraction of metals like sodium, aluminium, and magnesium using electrolysis
• Electrolysis of molten compounds and aqueous solutions

19. Redox Reactions involving Metals

• Definition of redox reactions
• Examples of redox reactions involving metals:
  • Formation of metal oxide from Metal + Oxygen
  • Reaction of metal with acid
  • Reaction of metal with water
  • Displacement reactions

20. Environmental Impact of Metal Extraction

• Environmental issues caused by mining and metal extraction
• Pollution of air, water, and soil
• Efforts to reduce environmental impact: Recycling and sustainable extraction methods

21. Properties of Metalloids

• Metalloids have properties intermediate between metals and nonmetals
• They have both metallic and nonmetallic characteristics
• Examples of metalloids: Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te)

22. Chemical Properties of Metalloids

• Metalloids can form both positive and negative ions
• They can act as both conductors and insulators of electricity
• They exhibit varying reactivity with acids and bases
• Metalloids can form covalent compounds with nonmetals

23. Applications of Metalloids

• Silicon: Used in the production of semiconductors and computer chips
• Germanium: Used in infrared optics, fiber optic communication, and solar cells
• Arsenic: Used in wood preservation, pesticides, and in electronic devices
• Antimony: Used in flame retardants, batteries, and as an alloying agent
• Tellurium: Used in solar panels, thermoelectric devices, and in alloys for metals

24. Extraction of Metalloids from Ores

• Metalloids are usually extracted from their ores using a combination of pyrometallurgical and hydrometallurgical methods
• The ore is first crushed and then subjected to roasting or smelting processes
• The resulting metalloid compound is then purified through chemical processes such as leaching or electrolysis

25. Reactivity of Nonmetals

• Nonmetals tend to have high ionization energies and electronegativities
• Nonmetals generally do not form positively charged ions (cations)
• Nonmetals can form negative ions (anions) by gaining electrons
• The reactivity of nonmetals varies depending on their position in the periodic table

26. Physical Properties of Nonmetals

• Nonmetals are generally poor conductors of heat and electricity
• Nonmetals are brittle and can be in solid, liquid, or gaseous states at room temperature
• Nonmetals have low melting and boiling points compared to metals

27. Chemical Properties of Nonmetals

• Nonmetals tend to gain electrons during chemical reactions
• Nonmetals can react with metals to form ionic compounds
• Nonmetals can react with other nonmetals to form covalent compounds
• Nonmetals can react with oxygen to form oxides, many of which are acidic in nature

28. Importance of Nonmetals in Daily Life

• Oxygen: Essential for respiration and combustion
• Carbon: Forms the basis of organic compounds and is present in all living organisms
• Nitrogen: Key component in DNA, proteins, and fertilizers
• Hydrogen: Used in the production of ammonia, petroleum refining, and as an energy carrier
• Chlorine: Used as a disinfectant, in the production of PVC, and in water treatment

29. Noble Gases - Properties and Applications

• Noble gases have full valence electron shells and are chemically stable
• They are inert and do not readily form compounds with other elements
• Examples of noble gases: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)
• Applications of noble gases include lighting, lasers, cryogenics, and as an inert atmosphere in scientific research

30. Summary and Recap

• Recap of key concepts covered in the lecture:
  • Isolation of metals and metalloids from ores
  • Properties and chemical reactions of metalloids and nonmetals
  • Importance and applications of nonmetals in daily life
  • Properties and applications of noble gases
• Emphasize the importance of understanding the properties and behavior of metals, metalloids, and nonmetals in various industries and everyday life