The correct Answer is Both A and R are true but R is NOT the correct explanation of A
Explanation
This question pertains to the chemical properties of non-metallic oxides and the nature of bonding in compounds formed by non-metals with oxygen.
Statement-wise Analysis
- Assertion (A): Non-metallic oxides are generally acidic in nature.
- Correct. Non-metallic oxides typically react with water to form acids or react with bases to form salt and water, demonstrating their acidic character. Examples include CO₂ (carbonic acid), SO₂ (sulfurous acid), and P₄O₁₀ (phosphoric acid).
- Reason (R): Non-metals are electronegative elements that form covalent bonds with oxygen.
- Correct. Non-metals have high electronegativity and tend to share electrons with oxygen rather than transfer them, resulting in the formation of covalent bonds. For instance, in CO₂, sulfur dioxide (SO₂), and nitrogen dioxide (NO₂), the bonds between the non-metal and oxygen are covalent.
While both the Assertion and the Reason are individually true, the Reason does not correctly explain the acidic nature of non-metallic oxides. The acidic nature is primarily due to the formation of acidic solutions when these oxides react with water, or their ability to accept electrons (Lewis acid) or donate protons (Brønsted-Lowry acid) in aqueous solutions. The covalent bonding itself does not directly explain the acidic character; rather, it is the polarity of these covalent bonds and the resulting structure that allows for proton donation or electron acceptance in solution.
Key Takeaway
Non-metallic oxides are generally acidic, and non-metals form covalent bonds with oxygen, but the covalent bonding itself is not the direct explanation for the acidic nature of these oxides.