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Aluminium has the electronic configuration 1s2 2s2 2p6 3s2 3p1. Aluminium has an additional electron orbit in comparison to Boron, the sum of the first three ionisation enthalpies of Aluminium is lower than that of Boron, and as a result, Aluminium is capable of forming Al3+
ions in comparison to Boron. In most cases, it produces +3 oxidation states, as in the case of Aluminum Oxide, indicating that it is a highly electropositive element (Al2O3).
Other oxidation states that are known are +2 and +1. This layer of inert transparent Aluminium oxide (Al2O3), which forms rapidly in the air but is found to be highly reactive in nature, is frequently used to protect it. Aluminium forms amphoteric oxides, which means that it exhibits both acidic and basic properties at the same time.
Aluminium’s Physical Properties
The density of aluminium is lower than that of any other commercial metal, with the exception of magnesium. Aluminium, when coated with the appropriate surface treatment, is an excellent reflector of light, particularly ultraviolet light.
Aluminium is an odourless, tasteless, silvery white metal with no discernible taste or odour. With increasing silicon and ductility, the material becomes quite soft. The cubic structure of the aluminium crystal is centred on the face of the crystal.
In less pure metals, the formation of impurity segregations causes the lattice to be concentrated in greater concentrations than in pure metals. Purity has an impact on the majority of other physical properties as well.
The density of aluminium is lower than that of any other commercial metal, with the exception of magnesium.
Aluminium can also be used as a selective cold or hot wall, as well as a body that simulates the effect of a black body, depending on the application. In the infrared region, the reflectivity of aluminium is only marginally exceeded by that of gold and silver, which are both highly reflective metals.
Aluminium’s Chemical Properties
- The Reaction of Aluminium with the Environment:
As a rule, aluminium metal does not react with air because its surface is covered with a thin layer of oxide, which helps to protect the metal from being attacked by air. However, there are some exceptions. However, if the oxide layer is damaged and the aluminium metal is exposed, it reacts with oxygen again, forming amphoteric oxide (Aluminium (lll) Oxide), Al2O3
4Al(s) + 3O2(l) → 2Al2O3(s)
if the oxide layer is damaged and the aluminium metal is exposed
- The Reaction of Aluminium with Acids consists of the following:
Aluminium reacts readily with mineral acids to form solutions containing the aquated Al (lll) ion as well as the liberation of hydrogen gas, H2. Aluminium reacts with mineral acids to form solutions containing the aquated Al (lll) ion as well as the liberation of hydrogen gas, H2. When it dissolves in hydrochloric acid (HCl), it releases dihydrogen gas, which is useful in many applications.
2Al(s) + 6HCl (aq) → 2Al3+ (aq) + 6Cl– (aq) + 3H2O. (g)
In the case of a reaction with Nitric acid, it reacts passively by forming a protective oxide layer of Aluminium Oxide on the surface of the reaction product.
HNO3 + Al2O3 + 6 HNO3 → 2Al(NO3)3 + 3H2O
Aluminates are formed when aluminium reacts with alkalis, and hydrogen gas, H2, is released as a byproduct of the reaction. It is possible for Aluminium to form covalent bonds with oxygen because of the similar electronegativity of oxygen and aluminium. This can be viewed as a significant contributing factor to the formation of aluminates. In one example, when aluminium reacts with a hot, concentrated sodium hydroxide solution, it produces a colourless solution of sodium tetrahydroxoaluminate, which is followed by the formation of dihydrogen gas in the process.
2Al (s) + 2NaOH (aq) + 6H2O → 2Na+ (aq) + 2[Al(OH)4]– + 3H2O(g)
Conclusion
Therefore, we can finally conclude that Aluminium is a prominent Group 13 element and a member of the Boron family, which makes it a valuable metal. Aluminum has the electronic configuration 1s2 2s2 2p6 3s2 3p1. Aluminium has an additional electron orbit in comparison to Boron, the sum of the first three ionisation enthalpies of Aluminium is lower than that of Boron, and as a result, Aluminium is capable of forming Al3+ ions in comparison to Boron. In most cases, it produces +3 oxidation states, as in the case of Aluminum Oxide, indicating that it is a highly electropositive element (Al2O3). Other oxidation states that are known are +2 and +1.
