Reactivity of Group 13 towards Acids and Alkalis

The semi-metal boron (B) and the metals aluminium (Al), gallium (Ga), indium (In), and thallium (Tl) are all members of the boron family. The boron family has two different oxidation states. One is +3 and +1, respectively. Due to the inert pair effect, heavier elements like thallium which have an oxidation state of +1, are more stable. Other elements possess a +3 oxidation state due to this effect. With few anomalies, the periodic group follows a unique trend. In this article, we are talking about group 13 elements’ reactivity with acids and alkalis. This article explains the reactivity of Group 13 towards Acids and Alkalis and the reactivity of Group 13 towards Acids and Alkalis importance. 

Elements Of Group 13 

• Boron 

Boron does not form hydrides, but it does form compounds such as diborane (B2H6). Organic molecules are synthesized using boron hydrides. Boric acid, which is a weak acid, is produced through a two-step process. It is one of the most common chemicals used to make additional boron compounds.

Boron can also be crystallised from hydrogen peroxide and borax solution that later forms sodium perborate, which is a bleach substitute. The two peroxo groups which are linked to the boron atoms produce perborate that has bleaching content. 

• Aluminium

Aluminium is an active metal with the electron configuration of  [Ne] 2s²2p¹. It also has an oxidation state of +3. Aluminium is one of the most abundant metals in the Earth’s crust i.e. about  7.5 – 8.4 percent. 

Aluminium was known as a semiprecious metal until 1886. But, despite its abundance, it is difficult to isolate and also possesses a high melting point. It is also extremely expensive to produce as one mole of aluminium requires three moles of electrons to electrolyze. 

Aluminium is also amphoteric which means it can dissolve in both acids and bases. It also produces Al(OH)4– in an aqueous OH- solution and [Al(H2O)6]³+ in an aqueous H3O+ solution. Aluminium’s oxidation state is +3 which makes it a good reducing agent. Due to this, Aluminium can decrease H+(aq) to H2 by reacting with acids (g). 

• Gallium 

Gallium is a group 13 element with the atomic number 31 and its symbolic representation is Ga. It also has an oxidation state of +3 and the electron configuration of [Ar] 2s²2p¹. Gallium is useful in many manufacturing industries because it can be used to make gallium arsenide (GaAs). This element later transforms light into electricity.

Gallium is also combined with aluminium to produce hydrogen. It also absorbs oxygen from water and releases hydrogen gas in a process similar to a thermite reaction. Aluminium, on the other hand, creates a protective shell when exposed to water but when it is combined with gallium, it doesn’t form a protective layer. This process allows aluminium to convert water to hydrogen. 

• Indium

Indium exhibits electron configuration of [Kr] 2s²2p¹. And is oxidised in one of two states i.e +1 or +3. However, the +3 state is more common. At room temperature, indium is soluble in acids but doesn’t react with oxygen.

Indium is produced from zinc ores after they have been separated. Indium is also used to manufacture alloys, and a little bit of aluminium is used to improve mental strength.  

• Thallium 

Thallium has an oxidation state of +3 or +1. It also has an electron configuration of [Xe] 2s²2p¹. Thallium is heavy and is more stable because of its +1 oxidation state. Due to the inert pair effect, thallium can possess a +1 oxidation state. Thallium is a soft, pliable metal but It is poisonous. This metal is used in superconductors that operate at high temperatures.

Beryllium and Aluminium have a diagonal relationship with each other. 

• Hydration of Be²+ produces [Be(H2O)4]²+ and Al³+ produces Al(H2O)6³+. Both of these compounds give hydronium ions when they combine with water which makes them mildly acidic.

• Another similarity between aluminium and beryllium is that both are amphoteric. These metals form with basic hydroxides. In addition, these metals react with air to form oxide coatings that protect other metals from corrosion. Both these metals are extremely reactive. 

Group 13 elements basic properties 

Boron’s chemistry differs from other heavier metals in Group III (A). The following are some of the ways it differs from them (basically we compare aluminium): 

• Aluminium oxide and hydroxide both are acidic. But their oxides and hydroxide are amphoteric. 

• Boron is a semiconductor that is available in various polymorphs that vary based on icosahedral boron cages. Whereas aluminium is a metal with a dense structure.

• Boron is a relatively innocuous metal and is affected by highly concentrated oxidising acids.

• B³+ does not have any salts whereas Al3+ salts are abundant and researched well. Boron can be found in a variety of cage-structured hydrides. The polymeric structure of (AlH3) is similar to that of AlF3.

• Many boron compounds have stereochemistry based on their trigonal sp² and tetrahedral sp³ geometries.

• The octet rule is later formed in these elements. aluminium possesses different geometries, including tetrahedral, trigonal bipyramidal, and octahedral.

• In the +3 oxidation state metals like aluminium, gallium, indium, and thallium produce various compounds. While compounds in the +1 oxidation state grow more stable as you move down group III (A).
• Aluminium and gallium oxides are amphoteric, but indium and thallium oxides are basic.

conclusion

You can use reactivity of Group 13 towards Acids and Alkalis questions to understand the concepts of reactivity. Six chemical elements that makeup Group 13 (III-A) of the periodic table are known as the Boron family.  Boron (B), aluminium (Al), gallium (Ga), indium (In), thallium (Tl), and Nihonium (Ni) are part of this family. They form a group because the outermost orbitals of their atomic structure contain three electrons.