Electronic Configuration of Aluminium:

Aluminium (also known as aluminium in American English and Canadian English) is a chemical element with the symbol Al and atomic number 13. It occurs naturally as a metallic element in the environment. Aluminium has a lower density than most other common metals, with a density that is approximately one-third that of steel. It is also lighter than steel. It has a strong affinity for oxygen, and when exposed to air, it creates a protective coating of oxide on the surface of the material. Aluminium has a silvery sheen to it, both in terms of colour and in terms of its exceptional capacity to reflect light. A soft, non-magnetic, and ductile feel can be felt when handling this material. A stable isotope of aluminium exists in the form of 27Al, which is extremely abundant, making aluminium the tenth most abundant element in the universe. The radioactivity of 26Al is used in the process of radiodating items to determine their age. 

Natural occurrence of aluminium: 

In all, the Earth contains around 1.59 percent aluminium by mass (seventh in abundance by mass). Due to the ease with which aluminium forms oxide and becomes bound to rocks, it is found in greater abundance in the Earth’s crust than in the rest of the universe. Less reactive metals, on the other hand, sink to the Earth’s core, resulting in a higher proportion of aluminium in the Earth’s crust. Aluminium is the most prevalent metallic element in the Earth’s crust (8.23 percent by mass) and the third most abundant element overall in the Earth’s atmosphere (after oxygen and silicon). Aluminium can be found in huge quantities in the Earth’s crust in the form of silicates. The Earth’s mantle, on the other hand, contains only 2.38 percent aluminium by mass. Aluminium may also be found in saltwater at a concentration of 2 μg/kg, which is quite low. 

Electronic configuration of aluminium: 

In the case of aluminium, the atom possesses 13 electrons, which are placed in an electron configuration of [Ne]3s²3p¹, which is three electrons more than the number of electrons in a stable noble gas configuration. This results in a combination of the first three ionisation energies of aluminium that are significantly lower than the fourth ionisation energy on its own. This electron configuration is shared by the other well-characterised members of its group, such as boron, gallium, indium, and thallium; it is also expected for nihonium, which belongs to the boron group. 

Properties of aluminium: 

The following are some of the physical properties of aluminium that have been discussed: 

• The element has a high degree of reactivity. It is stiffer and denser than steel, but only about one-third the weight.
• Aluminium has a high level of corrosion resistance.
• It has the ability to conduct electricity at superconducting speeds.
• There are several unknown hydrogen isotopes with mass numbers ranging from twenty-one to forty-one that have been discovered. 

Chemical properties of aluminium: 

Aluminium reaction with HCl: 

At room temperature, aluminium combines with dilute hydrochloric acid to form aluminium hydroxide. In hydrochloric acid, the metal aluminium dissolves, resulting in the formation of aluminium chloride and colourless hydrogen gas. The reaction that is going place between aluminium and hydrochloric acid is unstoppable and cannot be stopped. 

2Al + 6HCl → 2AlCl₃ + 3H₂↑ 

Aluminium reaction with sodium hydroxide: 

It is also generated as a result of the action of sodium hydroxide on elemental aluminium, which is an amphoteric metal, and is known as sodium aluminate. Once formed, the reaction becomes highly exothermic, and the rapid development of hydrogen gas is a byproduct of the reaction. 

2NaOH + 2H2O → 2NaAlO2 + 3H2 

Aluminium reaction with water: 

A tiny coating of aluminium oxide, only a few millimetres thick, forms on the surface of aluminium metal very quickly, preventing the metal from interacting with water. According to the equation, aluminium reacts with water to produce hydrogen gas as a byproduct. 

2Al + 3H2O → 3H2 + Al2O3 

Extraction of aluminium: 

A soft, silvery-white metal with good corrosion resistance. Due to its abundance in the earth’s crust, which accounts for 8 percent of the crust, it is the third most abundant element after oxygen and silicon. It is the most abundant metal on the face of the earth. Bauxite ore (Al2O3.xH2O) has been the primary source of aluminium until recently, and it is a mixture of hydrated aluminium oxide and other elements.

Aluminium can also be extracted from cryolite (Na3AlF6) and alunite, which are both minerals. Garnet, topaz, and chrysoberyl are all examples of gemstones that contain this element. This metal is represented by the chemical symbol Al. Aluminium is a chemical element that is a member of the boron group and is represented by the letter Al. It is the most commonly used non-ferrous metal and is found in the boron group. 

Ores of aluminium: 

Aluminium is a highly reactive metal that belongs to the IIIA group of the periodic table. It is also a metal that is highly reactive. Aluminium is present in nature in the form of its oxide, which can be found in ores. The most important aluminium ores are as follows: 

• Bauxite – Al2O3.2H2O
• Corundum – Al2O3
• Cryolite – Na3AlF6

Concentration of ore: 

Impurities such as ferric oxide and silica can be found in the bauxite ore. It is first concentrated by gravity separation of ferric oxide impurities, followed by a process of magnetic separation to achieve its final concentration. The ore is subsequently concentrated by the use of a chemical procedure.

Bauxite is the name given to the ore that contains aluminium. Bauxite is purified to produce aluminium oxide, which is a white powder from which aluminium can be extracted. Bauxite is used in the production of aluminium oxide. Because aluminium oxide has a very high melting point of more than 2000°C, melting it would be extremely expensive. When placed in water, aluminium oxide does not dissolve, but when placed in molten cryolite, it dissolves. 

Uses of aluminium: 

1. In the transportation industry, it is utilised in the production of castings for railroad cars, trucks and automobiles.
2. It is employed in the packaging industry.
3. In the reactions of Al metal with oxidants, Al(II) compounds are formed, which are toxic.
4. The presence of aluminium can be discovered in qualitative analysis by using the aluminon method.

Conclusion: 

Aluminium is utilised in a wide variety of applications in the transportation, building, and other industries. Aluminium foils are used in the food industry to wrap food and keep it fresh. This metal’s dust is utilised in the production of paints. It is employed in the extraction of manganese and chromium from their respective oxides, among other things. Because it is a soft metal that can be shaped into any shape, it is commonly employed in the production of storage cans and other containers.