Which one of the following orders presents the correct sequence of the increasing basicnature ofthe given oxides

To determine the correct sequence of increasing basic nature among a set of oxides, we first need to understand what basic nature means in the context of oxides. Basic nature refers to the ability of an oxide to react with acids to form salts and water. Generally, metal oxides tend to be more basic than non-metal oxides. The position of the element in the periodic table also plays a significant role in determining the basicity of its oxide.

Factors Influencing Basicity

Several factors influence the basic nature of oxides:

• Metallic Character: As you move from right to left across a period in the periodic table, the metallic character increases, which typically enhances the basicity of the corresponding oxides.
• Oxidation State: Higher oxidation states usually lead to more acidic oxides. For example, FeO (iron(II) oxide) is more basic than Fe2O3 (iron(III) oxide).
• Electronegativity: Oxides of elements with lower electronegativity are generally more basic. Elements with high electronegativity tend to form acidic oxides.

Example of Oxides

Let’s consider a few common oxides to illustrate this concept:

• Na2O (Sodium Oxide): A strong basic oxide due to sodium's low electronegativity and metallic character.
• MgO (Magnesium Oxide): Also basic, but less so than Na2O.
• Al2O3 (Aluminum Oxide): Amphoteric in nature, meaning it can act as both an acid and a base, but is less basic than Na2O and MgO.
• SiO2 (Silicon Dioxide): Generally considered acidic, as silicon has a higher electronegativity compared to the metals listed above.

Arranging the Oxides

Now, if we were to arrange these oxides in order of increasing basicity, we would start with the most acidic and move towards the most basic. Based on the examples provided, the order would be:

• SiO2 (least basic)
• Al2O3
• MgO
• Na2O (most basic)

Thus, the correct sequence of increasing basic nature for these oxides would be SiO2 < Al2O3 < MgO < Na2O. This sequence highlights how the properties of the elements and their oxides can be understood through periodic trends and chemical behavior.