Question

Which of the following represents correct acidity order$L{i_2}O$,$BeO$ and ${B_2}{O_3}$
A.$L{i_2}O$<$BeO$<${B_2}{O_3}$
B.${B_2}{O_3}$<$BeO$<$L{i_2}O$
C.$BeO$<$L{i_2}O$<${B_2}{O_3}$
D.$BeO$<${B_2}{O_3}$<$L{i_2}O$

Answer 1

Hint: Acidity is defined as the tendency of a compound to liberate a hydrogen ion. Here, the acidity of oxides in the form of the compounds can be determined based on the presence of the element across the period. Across the period, the chemical nature of oxides increases, i.e., Basic oxide -> Amphoteric oxide -> acid oxide.

Complete answer:
The correct order acidity depends on the ability of a presence of the particular element in the periodic table. As we know that across the period, the chemical nature of oxides is as follows: Basic oxide followed by Amphoteric oxide and ultimately Acid oxide. Hence, the acidity order of boron oxide will be more compared to the beryllium oxide, and the lithium oxide being the least acidic compared to boron oxide and beryllium oxide. Therefore, the order of acidity is as follows: Lithium oxide < beryllium oxide < boron oxide.

Thus, the correct option is option A. $L{i_2}O$<$BeO$<${B_2}{O_3}$.

Note:
In general, the strength of an acid in a compound is directly proportional to the stability of the acid’s conjugate base. In other words, an acid that has a more stable conjugate base will be more acidic than an acid that has a less stable conjugate base. The acidity can be affected by atoms present, hybridization, electronegativity, resonance. Acidic oxides react with water to form acidic compounds. Acid oxides are formed when they react with non-metals.