Question

Among the following the acidic oxide is :
A.${\text{N}}{{\text{a}}_{\text{2}}}{\text{O}}$
B.${\text{MgO}}$
C.${\text{CuO}}$
D.${\text{S}}{{\text{O}}_{\text{2}}}$

Answer 1

There are different types of oxide. The acidic oxide is defined as the oxide which tends to combine with the water so that it can form acid. Generally we see the non metals which react with oxygen to form the oxides which are acidic and are held by the covalent bonds. They are also known as acid anhydrides.

Complete step by step answer:
The sulphur dioxide is considered as the non metallic oxide which is acidic in nature as it has the tendency to form sulphurous acid on the reaction with water. The sulphur is the non-metal and the oxide of it forms the sulphurous acid on the reaction with water. the reaction which is been involved on showing the acidic nature of the sulphur dioxide or forming the sulphurous acid is the following:
${\text{S}}{{\text{O}}_{\text{2}}}{\text{ + }}{{\text{H}}_{\text{2}}}{\text{O}} \to {{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{3}}}$
So the correct answer is option d.
The sodium oxide is the basic oxide as it contains oxide ion in it and sodium is a metal. It reacts with the water and forms sodium hydroxide on reaction. The acidic oxides are not considered as the Bronsted Lowry acid but they are considered as the Arrhenius acids.

So, the correct answer is Option D.

Note: We say these acidic oxides are not considered as the Bronsted Lowry acid but they are considered as the Arrhenius acid because they have the tendency to increase the concentration of hydrogen ion of water. The Bronsted Lowry concept is based on the concept of the donation and acceptance of the proton.