Step-by-Step Process for Extracting Metals of Medium Reactivity
Rocks and soil contain metals, an essential component of our universe. They are not actually found in their pure form and need to be isolated. They are discovered with some naturally occurring chemicals containing one or more elements or their compounds. They are referred to as minerals. Ores are minerals that can be used to extract elements at a profit.
Reactivity Series
The arrangement of metals in decreasing order of their reactivities is referred to as the "metal reactivity series," also known as the "activity series”. The metals near the top of the reactivity series are strong reducing agents. As you move down the series, the reducing power of the metal becomes less. Therefore, it was found that the metal at the top of the reactivity series was more reactive.
The rate of the displacement reaction depends on the reactivity series. The metal at the top of the reactivity series can easily displace the metal below it in its solution. Metals with low reactivity are easily displaced by those with high reactivity.
Metal Extraction in the Middle of the Reactivity Series
Metals in the middle of the activity series are moderately reactive, i.e.; they are neither very reactive nor less reactive. This may include manganese, iron, zinc, lead etc. In nature, they are typically found as metal sulphides or metal carbonates. It is easier to extract a metal from its oxides as compared to its sulphides and carbonates. Therefore, prior to the reduction, the metal sulphides and carbonates should be converted into metal oxides.
The sulphide ores are converted into oxides by heating strongly in the presence of excess air. This process is known as roasting. The carbonate ores are changed to oxides by heating strongly in limited air or completely in the absence of air. This process is called calcination. These metal oxides are then reduced to the corresponding metals using suitable reducing agents such as carbon. Zinc oxide, for instance, is transformed into metallic zinc when heated with carbon.
Sometimes displacement reactions can be employed instead of carbon (coke) to convert metal oxides to metals. Since they can displace less reactive metals from their compounds, highly reactive metals like sodium, calcium, and aluminium are used as reducing agents.
Extraction of Zinc (Zn)
Zinc has 2 common ores, Zinc blende (ZnS) and Calamine (ZnCO3). Therefore, zinc can be extracted by 2 methods:
1. Extracting Zn from Zinc Blend (ZnS)
In zinc blend (ZnS), it is very difficult to isolate zinc alone because the affinity for Zinc and Sulphur is greater. It should be converted to corresponding oxides by the process of roasting.
Roasting
2ZnS(s) + 3O2(g)+ Heat ⟶ 2ZnO(s) + 2SO2(g)
Zinc oxide, thus on reduction, gives metallic zinc.
carbon monoxide. The carbon replaces the zinc. Here, carbon acts as a reducing agent. Industrially, coke is used as a source of carbon.
Reduction
ZnO(s) + C(s) ⟶ Zn(g) + CO(g)
2. Extracting Zinc from Calamine (ZnCO3)
Calamine is heated with constrained air before being transformed into zinc oxide (calcination). Thus, when produced zinc oxide is reduced in the presence of carbon (coke), metallic zinc is created.
Calcination
ZnCO3(s)+ Heat ⟶ ZnO(s) + CO2(g)
Reduction
ZnO(s) + C(s) ⟶ Zn(g) + CO(g)
Extracting Manganese from Pyrolusite (MnO2)
Pyrolusite (MnO2) can be reduced directly. When pyrolusite is treated with carbon, there will be no reaction. It is because carbon is less reactive than manganese and cannot displace manganese. Hence, a more reactive element should be used to reduce the ore. Pyrolusite reacts with aluminium powder to give manganese in its molten state. This is because aluminium is highly reactive, and liberates a huge amount of heat when treated with pyrolusite.
MnO2+ C ⟶ No reaction
3MnO2(s)+ 4Al(s) ⟶ 2Al2O3(s)+ 3Mn(l) + Heat
This reaction is known as a thermite reaction. In a thermite reaction, aluminium powder is used to reduce a metal oxide, and the metal is extracted in the molten state because of the heat liberated during the reaction.
Extracting Iron from Haematite
Haematite can be directly reduced to form iron. It can be reduced by both carbon and aluminium powder. Here, coke served as the source of carbon. Hence, carbon is more highly reactive than iron; it can displace iron from the ore and form metallic iron and carbon monoxide.
Fe2O3(s) + 3C(s) ⟶ 2Fe(s) + 3CO(g)
Also, iron can be extracted by this process. When the aluminium powder is treated with haematite, iron in a molten state is obtained. This reaction has many industrial applications.
Fe2O3(s)+ 2Al(s) ⟶ Al2O3(s)+ 2Fe(l) + Heat
Interesting Facts
A Thermite reaction occurs when the aluminium powder is used to reduce a metal oxide, and the metal is extracted in the molten state as a result of the heat liberated during the reaction.
These displacement reactions are highly exothermic.
The amount of heat evolved is so large that the metals are produced in the molten state.
Iron (III) oxide (Fe2O3) is used to join railway tracks and crack machine parts. Therefore, this molten iron can be used in the welding railway cracks (Thermite welding).
Key Features
Through electrolysis or reduction, a metal can be separated from its ore.
Manganese, iron, zinc, and other metals in the middle of the reactivity series have a slightly lower reactivity than the top-ranking metals and a higher reactivity than the lowest-ranking metals.
Metal oxides are more easily reducible than metal sulphides or carbonates.
Prior to the extraction of the metal, roasting or calcination is used to convert the metal sulphides or metal carbonates to metal oxides.
FAQs on Extracting Metals in the Middle of the Activity Series
1. What is the general process for extracting metals in the middle of the reactivity series?
Metals like iron, zinc, and lead are moderately reactive and are usually found as sulphide or carbonate ores. The extraction process typically involves three main steps:
- Concentration of the Ore: Removing impurities (gangue) from the ore.
- Conversion to Metal Oxide: The concentrated ore is converted into its metal oxide by either roasting (for sulphide ores) or calcination (for carbonate ores).
- Reduction to Metal: The metal oxide is then reduced to get the pure metal, commonly using carbon as a reducing agent.
2. Why can't moderately reactive metals like zinc be extracted just by heating their ores?
The oxides of moderately reactive metals like zinc or iron are quite thermally stable. This means simple heating alone isn't enough to break the strong bond between the metal and oxygen. A chemical reaction is needed, which is why a reducing agent like carbon is used to forcefully remove the oxygen and isolate the metal.
3. What is the main difference between roasting and calcination?
Both are processes to convert ores into metal oxides, but they differ based on the presence of air.
- Roasting: This process involves heating a sulphide ore strongly in the presence of excess air. For example, zinc sulphide (ZnS) is roasted to form zinc oxide (ZnO).
- Calcination: This process involves heating a carbonate ore strongly in the limited supply or absence of air. For example, zinc carbonate (ZnCO₃) is calcined to form zinc oxide (ZnO).
4. How does a metal's position in the reactivity series help decide its extraction method?
The reactivity series is like a guide for metallurgists. It shows how easily a metal reacts and, therefore, how difficult it is to extract:
- High Reactivity (Top): Metals like potassium and sodium are very reactive. Their oxides are extremely stable, so they are extracted using electrolysis.
- Medium Reactivity (Middle): Metals like zinc, iron, and lead are less reactive. Their oxides can be broken down using a chemical reducing agent like carbon.
- Low Reactivity (Bottom): Metals like mercury and copper are least reactive. Their oxides are unstable and can be reduced to metal by heating alone.
5. What is the role of carbon in extracting iron from its ore in a blast furnace?
In a blast furnace, carbon (in the form of coke) acts as the reducing agent. It is more reactive than iron, so at high temperatures, it effectively 'steals' the oxygen from the iron oxide (haematite). This displacement reaction reduces the iron oxide to molten iron, which is then collected.
6. Why is zinc able to displace copper from a copper sulphate solution?
This happens because of their different positions in the reactivity series. Zinc is more reactive than copper, which means it has a stronger tendency to lose electrons and form ions. When zinc is added to a copper sulphate solution, it displaces the less reactive copper, taking its place in the solution and turning solid copper out.
7. Besides carbon, what other substances can be used to reduce metal oxides?
Yes, sometimes more reactive metals are used as reducing agents in highly exothermic displacement reactions. A well-known example is the Thermite reaction, where aluminium powder is used to reduce iron oxide to produce molten iron. This method is often used for welding railway tracks because of the intense heat it generates.
8. What are some common examples of metals extracted using these methods?
The primary examples of metals found in the middle of the reactivity series that are extracted using reduction are:
- Iron (Fe) from its oxide ore, haematite.
- Zinc (Zn) from its ores, zinc blende (sulphide) or calamine (carbonate).
- Lead (Pb) from its sulphide ore, galena.
