The Extraction Of Metals and The Preparation and Collection Of Non-Metals. Ashvini Jagassar- 5C Chemistry. Mr. Dookoo

Section B- Descriptive Chemistry. B.2. Inorganic Chemistry Extraction Of Metals: 2.1 relate to the principles underlying the extraction of a metal and to its position in the electrochemical series; 2.2 describe the extraction of aluminium and iron.

Metals in Nature Metals can be found in nature: -uncombined or free they are limited to metals of very low reactivity, for example silver, gold, copper, platinum, nickel. -combined in the form of ores These include the majority of metals. Chief ores of economic importance are metal oxides, sulphides, chlorides and carbonates.

The method used to extract a metal from its ore is guided by the position of the element on the Reactivity Series. Metals high up on the series are strongly bonded in their compounds. Electrolysis is the only method strong enough to extract these. Example: Na(sodium), Mg(magnesium) and Al(aluminium)

Metals in the middle of the series are less strongly bonded in their compounds. Their oxides can be reduced by carbon to give the metal. Example: Zn(zinc) and Fe(iron) 2 ZnO (s) + C (s) 2 Zn (s) + CO 2(g) zinc oxide+carbon zinc+carbon dioxide

Metals at the bottom of the series can be found uncombined in nature. They simply need to be purified of unwanted materials. When they do occur in ores, example copper sulphide, heating is strong enough to displace the metal from the ore. Example: Cu(copper), Ag(silver) and Au(gold)

The Reactivity Series. The Reactivity Series is a list of metals arranged in order of reactivity. Potassium is the most reactive metal and thus is on top of the series. Hydrogen is a non-metal but is placed in this series to show that the metals below it do not react with acids to produce Hydrogen gas.

The Reactivity Series. Metal Potassium Sodium Calcium Magnesium Aluminium Zinc Iron Lead Hydrogen Copper Mercury Silver Gold Symbol K Na Ca Mg Al Zn Fe Pb H Cu Hg Ag Au

The Electrochemical Series. The electrochemical series is a listing that places ions in order of ease of electrical discharge. The lower an element is in the series then the easier it is to discharge.

The Electrochemical Series. Cations K + Ca 2+ Na + Al 3+ Zn 2+ Fe 2+ Pb 2+ H + Cu 2+ Ag + Au + Anions SO 4 2- NO 3 - Cl - Br - I - OH -

The Extraction Of Metals Iron. Several iron ores exist. The most popular method of iron extraction uses the Blast Furnace. This is a cylindrical, tapering tower about 30-40m high, constructed of steel lined with refractory bricks. The principle of the method is the reduction of iron(III) oxide with carbon.

The Blast Furnace (automated).

The Extraction Of Iron using the Blast Furnace. Step 1: Dried heated iron ore, limestone (calcium carbonate) and coke (carbon) are fed into the top of the furnace. Step 2: Hot air is blown into the furnace near the bottom. The hot air burns the coke producing carbon dioxide and generating great heat. C (s) + O 2(g) CO 2(g)

Step 3: The carbon dioxide is then reduced to carbon monoxide by the hot coke. CO 2(g) + C (s) 2CO (g) Step 4: The carbon monoxide reduces the hot iron ore to molten iron which runs to the bottom of the furnace Fe 2 O 3(s) + 3CO (g) 2Fe (l) + 3CO 2(g) OR Fe 3 O 4(s) + 4CO (g) 3Fe (l) + 4CO 2(g)

If limestone were not used, the iron produced in the furnace would have many impurities. The limestone, at the furnace’s temperature, breaks down. CaCO 3(s) CaO (s) + CO 2(g) The calcium oxide formed combines with silicon dioxide, the main impurity in iron ore, to form a molten slag. CaO (s) + SiO 2(s) CaSiO 3(l) The slag, being less dense than the molten iron, floats on it and runs off separately from it.

The Extraction Of Metals Aluminium. Aluminium is very abundant in the earth’s crust, but is never found in its free state. Aluminium is found mainly in the form of aluminosilicates, of which bauxite (Al 2 O 3 ) is the chief source. The crude/mined bauxite is either: heated to 3000 o C to produce calcined bauxite Converted to pure alumina (Al 2 O 3 )

The process for extracting aluminium from aluminia is electrolysis. Electrolysis is the process by which the passage of an electric current through a substance causes it to decompose. In the current process of extracting aluminium from bauxite, an electrolytic cell made of steel using graphite electrodes is used. The current used is 100,000A and the temperature is 1,223K.

Pure aluminia (aluminium oxide) which melts at 2050 o C is dissolved in molten cryolite (sodium aluminium fluoride), Na 2 AlF 6. The addition of the cryolite lowers the temperature to 950 o C, because the presence of an impurity lowers the melting point of a substance. The presence of the cryolite also gives the melt better conducting properties and, in addition, it does not mix with the aluminium metal formed in the electrolysis.

Aluminium is discharged at the graphite cathode, which lines the chamber. The product is 99% pure, the chief impurities being silicon and iron. Liquid aluminium is tapped off at the end of the cell. Al 3+ (l) + 3e - Al (l) Oxygen is the other product that is produced at the anode. 2O 2- (l) - 4e - O 2(g)

Electrolysis of Aluminium.

Section B- Descriptive Chemistry B.2. Inorganic Chemistry Preparation and Collection of Non- Metals: 3.1 describe the industrial preparation of chlorine, sulphuric acid and ammonia;

The Preparation and Collection Of Chlorine. The main method for the manufacture of chlorine is The Flowing Mercury Cathode Cell. Sodium hydroxide and hydrogen are co products. This is the electrolysis of brine (aqueous sodium chloride) using a continuously flowing mercury cathode and a graphite or titanium anode. The raw material used is concentrated sodium chloride solution (NaCl). The power requirement is approximately 4.5 V, 300,000 A, and the process is carried out at a pH of about 4.5.

The Flowing Mercury Cathode Cell.

Reactions involved in the Electrolysis of Chlorine. Cl is discharged at the anode because it is of higher concentration than OH - 2Cl - (aq) - 2e - Cl 2(g) Chlorine gas produced is collected. At the cathode Na + is discharged because of the mercury cathode. The normal order of discharge is reversed on a fresh metal surface (mercury). Na + + e - Na (s)

The Preparation and Collection of Sulphuric Acid. Contact Process Sulphuric acid is widely manufactured using the Contact Process. This process can be divided into three stages: The production of sulphur dioxide. Mainly by burning sulphur in air S (s) + O 2(g) SO 2(g)

Oxidation of sulphur dioxide to sulphur trioxide. vanadium (V) oxide in silica gel catalyst. Pure dry sulphur dioxide and oxygen are heated to 450 o C and passed over a vanadium (V) oxide in silica gel catalyst. 2SO 2(g) + O 2(g) 2SO 3(g) Hydration of sulphur trioxide. Sulphur trioxide is hydrated indirectly by initially dissolving in concentrated sulphuric acid. Oleum is formed which is diluted to give concentrated sulphuric acid. H 2 SO 4(aq) + SO 3(g) H 2 S 2 O 7(aq) Oleum H 2 S 2 O 7(aq)_ + H 2 O (l) 2H 2 SO 4(aq)

The Contact Process

The Preparation and Collection of Ammonia. Ammonia is commercially manufactured by the Haber Process. In this process a purified nitrogen/hydrogen mixture is compressed to atm and passed over a finely divided iron catalyst. The heat evolved during the reaction maintains the optimum reaction temperature, o C.

N 2(g) + 3H 2(g) 2NH 3(g) The gases leaving the reaction chamber contain 10-20% ammonia, which is removed by condensation under refrigeration or absorption by water. Uncombined nitrogen and hydrogen are recycled atm o C Iron catalyst

Preparation of Ammonia Gas.