Group VI - Sulfur and it's Compounds (Chemistry Summary Notes)
Ø Sulfur is a brittle yellow solid at r.t.p.
Ø It is a non-metal.
Ø It does not conduct electricity.
Ø It is insoluble in water but is soluble in Carbon dissulfate.
Ø Sulfate is found in metal ores such as copper pyrites (CuFeS2).
Ø Uses of sulfur: large quantities are used in the manufacture of sulfuric acid, to make drugs, matches, pesticides and gunpowder, it is also a bleaching agent in the manufacture of paper.
Ø There are 2 main Allotropes of sulfur. These are the rhombic and monoclinic. Both are made up of S8 molecules packed in different ways. In Rhombic sulfur the molecules are found packed more closely than in monoclinic form.
Ø Hydrogen sulfide is a compound of sulfur. It is a colourless gas and has a repulsive smell of rotten eggs. It is fairly soluble in water giving a weakly acidic solution. Hydrogen sulfide is slightly denser than air.
Ø Sulfur dioxide is another compound of sulfur. It is a colourless gas with a sharp unpleasant smell. It is denser than air and is extremely toxic. When sulfur is heated in the presence of oxygen it produces sulfur dioxide. S(s) ---Heat----> SO2 (g)
Ø Sulfur dioxide is used to manufacture sulfuric acid, and as a preservative in canned fruit and fruit juices.
Ø Sulfur dioxide is acidic in nature. It dissolves in water to form sulfurous acid but it easily decomposes from water to form sulfur dioxide.
Ø Sulfur dioxide is a good reducing agent.
Ø Sulfuric acid is a strong acid.
Ø Concentrated sulfuric acid is a drying agent. It absorbs water vapour, so it is suitable for drying gases.
Ø Concentrated sulfuric acid is a powerful dehydrating agent.
Ø Hot concentrated H2SO4 is a powerful oxidizing agent, and in the process it is reduced to SO2. It takes electrons from the copper atoms to form copper ions.
Cu (s) + 2H2SO4 (l) -> CuSO4 (aq) + 2H2O(l) + SO2 (g)
2H2SO4 (aq) + 2 e - -> SO4 2- (aq) + 2H2O (l) + SO2 (g)
Ø It is a non-metal.
Ø It does not conduct electricity.
Ø It is insoluble in water but is soluble in Carbon dissulfate.
Ø Sulfate is found in metal ores such as copper pyrites (CuFeS2).
Ø Uses of sulfur: large quantities are used in the manufacture of sulfuric acid, to make drugs, matches, pesticides and gunpowder, it is also a bleaching agent in the manufacture of paper.
Ø There are 2 main Allotropes of sulfur. These are the rhombic and monoclinic. Both are made up of S8 molecules packed in different ways. In Rhombic sulfur the molecules are found packed more closely than in monoclinic form.
Ø Hydrogen sulfide is a compound of sulfur. It is a colourless gas and has a repulsive smell of rotten eggs. It is fairly soluble in water giving a weakly acidic solution. Hydrogen sulfide is slightly denser than air.
Ø Sulfur dioxide is another compound of sulfur. It is a colourless gas with a sharp unpleasant smell. It is denser than air and is extremely toxic. When sulfur is heated in the presence of oxygen it produces sulfur dioxide. S(s) ---Heat----> SO2 (g)
Ø Sulfur dioxide is used to manufacture sulfuric acid, and as a preservative in canned fruit and fruit juices.
Ø Sulfur dioxide is acidic in nature. It dissolves in water to form sulfurous acid but it easily decomposes from water to form sulfur dioxide.
Ø Sulfur dioxide is a good reducing agent.
Ø Sulfuric acid is a strong acid.
Ø Concentrated sulfuric acid is a drying agent. It absorbs water vapour, so it is suitable for drying gases.
Ø Concentrated sulfuric acid is a powerful dehydrating agent.
Ø Hot concentrated H2SO4 is a powerful oxidizing agent, and in the process it is reduced to SO2. It takes electrons from the copper atoms to form copper ions.
Cu (s) + 2H2SO4 (l) -> CuSO4 (aq) + 2H2O(l) + SO2 (g)
2H2SO4 (aq) + 2 e - -> SO4 2- (aq) + 2H2O (l) + SO2 (g)