Chapter EH, Problem 27R

Solution

Interpretation : The properties of boron are different from the other group 13 elements to be described.

Concept Introduction : The group 13 elements make up the first group in the periodic table's p-block. Each member of group 13 has an electron configuration that ends in $n{s}^{2}n{p}^1$ and three valence electrons.

Boron is a metalloid and hard in nature with greater ionization energy and the shortest atomic and ionic radii.

The solar system and the crust of the earth include traces of the chemical element boron, which has atomic number five.

Boron is the only element in group 13 elements to be black whereas other elements are silvery-white.

The elements in group 13 are metals except for boron which is a metalloid.

The nature of boron is hard whereas all other elements in group 13 are soft and light in weight.

Metallic lattices are typically formed by Group 13 elements.

The electron pair is utilized to join three or more atoms in multicenter bonds, which are the kind of structures that Boron creates.

Compared to other elements, boron has initial ionization energy that is noticeably greater at 800.6 kJ/mol.

The ionization energy for aluminum, for instance, is 577.5 kJ/mol.

Since B lacks a d-subshell, it has the shortest atomic and ionic radii of the Group 13 elements.

Boron has much greater melting and boiling points than other elements.

Due to its very high electronegativity, only covalent compounds are formed by the element borax.

Other Group 13 elements, however, can combine to produce covalent and ionic compounds.

While the hydroxides of other elements are basic and amphoteric, those of boron are acidic.