Properties of Aluminium

Aluminium which is also written as Al belongs to Group 13 in the periodic table. The properties of Aluminium are that it is tasteless, odorless, and exhibits both acidic and basic characteristics when present in its amphoteric oxides. The electronic configuration of Aluminium is 1s² 2s² 2p⁶ 3s² 3p¹. It is a silvery-white metal and is the most abundant metallic element that is present in the earth’s crust. It is not present in its metallic form but is present in the form of its compound. Al does not react with air due to the presence of a layer of oxides. 

Key Terms: Aluminium, tasteless, amphoteric oxides, periodic table, metallic form, electronic configuration. 

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What is Aluminium?

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Aluminium belongs to the Boron family and has the atomic number 13. The occurrence of Aluminium is in the igneous rocks mainly as aluminosilicates. Bauxite is the main ore of Aluminium and contains Aluminium oxides. Aluminium form Al³⁺ ions and is highly electropositive and has a +3 oxidation state. Even in the presence of a layer, it is highly reactive in nature. Other physical and chemical properties are as given below. 

Read more: Bauxite 

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Physical properties of Aluminium 

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The physical properties of Alunimum are as follows: 

• Aluminium is tasteless, silvery-white metal, and odorless. 
• They have the property of being ductile and soft. 
• The structure of Al is face-centered cubic. 
• The density of Al is lower in comparison to other metals except for Magnesium. 
• Aluminium can be drawn into wire or thin foil due to its malleable and ductile nature.
• Al is corrosion-resistant but is chemically active. 
• It is an excellent conductor of electricity and heat. 

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Chemical Properties of Aluminium 

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The chemical properties of Aluminium are as follows: 

• Reaction of Aluminium with Air 

Aluminium does not react with air due to the layer present on its surface. But if the oxide layer gets damaged and Al is exposed to air, it will react with oxygen to form amphoteric oxide (Al₂O₃). The chemical reaction for the same is mentioned below. 

4Al (s) + 3O₂ (l) → 2Al₂O₃(s)

• Reaction of Aluminium with Acid 

Al is readily dissolved in acids. When Al reacts with acids it liberates hydrogen gas (H₂) and forms Al³⁺ ions. The use of concentrated nitric acid can passivate Aluminium metal as it reacts passively with Aluminium and does not release hydrogen gas. 

2Al(s) + 6HCl (aq) → 2Al₃⁺ (aq) + 6Cl^– (aq) + 3H₂(g)

Al₂O₃ +6 HNO₃ → 2Al(NO₃)₃+ 3H₂O

• Reaction of Aluminium with Alkali 

The reaction of Aluminium with alkalis will liberate hydrogen gas along with the formation of aluminates. In aluminates, the covalent bond is formed between oxygen and Aluminium due to the comparable electronegativity. Example: when Al reacts with concentrated sodium hydroxide, it produces sodium tetrahydroxoaluminate which is a colorless solution and also liberates hydrogen gas (H₂). 

2Al (s) + 2NaOH (aq) + 6H₂O → 2Na⁺ (aq) + 2[Al(OH)₄]^– + 3H₂ (g)

Read more: Chemical compounds 

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What is Aluminium Alloy?

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Aluminium alloys have Al as the predominant metal. The other elements in the Aluminium alloy are magnesium, manganese, copper, silicon, etc. The alloys can be cast alloy or wrought alloys. Majorly Al is used for wrought products like foils, plates, etc. On the other hand, cast alloy is cost-effective due to its low melting point. Aluminium alloys have a white protective layer of Aluminium oxides. 

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Uses of Aluminium 

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Some of the important uses of Aluminium are as follows: 

• It is used for the formation of foils, cans, and utensils as it is easy to shape and cast. 
• It is mainly used as a form of alloy as it does not have a robust nature. 
• Al is a good electrical conductor of electricity, therefore, is used for the formation of electrical wires. 
• It has a reflective surface for both heat and light and does not corrode easily. 

Aluminium has both acidic and basic characteristics. It belongs to the Boron family and belongs to Group 13. It is a good conductor of electricity and is silvery-white in appearance. It is most abundant in the earth’s crust and does not corrode easily due to the protective covering. 

Also Read:

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Things to Remember 

• The electronic configuration of Al is 1s² 2s² 2p⁶ 3s² 3p¹ 
• Aluminium is tasteless, silvery-white metal, and odorless
• Pure Aluminium is not present naturally and is mostly used in the form of alloy. 
• Aluminium is highly reactive, ductile, and malleable. 
• It is used for the formation of cans, electrical wires, foils, etc. 

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