Important Trends and Anomalous Properties of Boron

Table of Content

Introduction to Boron
Anomalous Properties of Boron
Diagonal Resemblance of Boron With Silicon

Fig. 1: Introduction to Boron

Introduction to Boron

Certain vital patterns can be seen in the chemical conduct of group 13 elements. The trichlorides, iodides as well as bromides of every one of these elements being covalent in nature are hydrolyzed in water. Species like tetrahedral [M(OH)₄]- and octahedral [M(OH)₆]³⁺ with the exception of boron exist in fluid medium.

The monomeric trihalides, being electron lacking, are strong Lewis acids. Boron trifluoride effortlessly react with Lewis bases, for example, NH₃ to finish octet around boron.

F₃B + : N H₃ → F₃B – NH₃

It is because of the nonattendance of d-orbitals that the greatest covalence of B is 4. Since the d-orbitals are accessible with Al and different elements, the most extreme covalency can be normal past 4. A large portion of other metal halides (e.g., AlCl₃) are dimerized through halide bridging (e.g., Al2Cl₆). The metal species finishes its octet with the help of electrons accepted from halogen in these halogen bridged particles.

Anomalous Properties of Boron

Though aluminum is a metal, Boron is a non-metal.
Aluminium is a good conductor of electricity but Boron is not.
Boron exists in two structures amorphous and crystalline. Aluminum is a delicate metal and does not exist in various structures.
The boiling point and melting point of boron are much higher as compared to those of aluminum.
Boron frames just covalent compounds while aluminum shapes even some ionic compounds.
The oxides and hydroxides of boron are acidic in nature though those of aluminum are amphoteric.
The trihalides of boron (BX₃) are monomers whereas, aluminum halides subsists as dimers (Al₂X₆).
The hydrides of boron are quite inert while those of aluminum are flimsy.

Fig. 2: Physical Properties of Boron

Diagonal Resemblance of Boron With Silicon

Boron and Silicon show the distinctive properties of non-metals. These don't shape cations. Both exist in crystalline and amorphous structures.
Boron Oxide (B₂O₃) and silica (SiO₂) are both acidic and break up in solutions that are alkaline in nature to frame borates and silicates separately.

B₂O₃ + 6NaOH → 2Na BO₃ + 3H₂O

SiO₂ + 2NaOH → Na₂SiO₃ + H₂O

Silicates and borates have tetrahedral SiO₄ and BO₄ auxiliary units individually.

The chlorides of both Si and B get hydrolyzed by water to form respective silicic acid and boric acid.

BCl₃ + 3H₂O → H₃BO₃ + 3HCl

SiCl₄ + 3H₂O → H₂SiO₃ + 4HCl

The hydrides of Boron and Silicon are very stable. Various unstable hydrides are additionally known which burst into flames on introduction to air and are effortlessly hydrolyzed.
Both these elements are semiconductor by nature.

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