Question

Which among the following oxides is acidic in nature?

• A. $\text{N}_2\text{O}_5$
• B. NO
• C. $\text{Na}_2\text{O}$
• D. CO

Hint:

Commit the standard neutral non-metal oxides to memory so you can eliminate them instantly: CO, NO, and $\text{N}_2\text{O}$ are completely neutral! Once you rule those out, identifying the acidic option becomes incredibly easy.

Answer 1

The Correct Option is A

Step 1: Understanding the Question:
The problem requires us to evaluate four different chemical oxides and identify which one displays acidic properties.

Step 2: Key Formula or Approach:
As a general periodic guideline, metallic oxides tend to be basic, whereas non-metallic oxides are typically acidic. However, certain non-metal oxides with low oxidation states can be completely neutral. Acidic oxides react with water to yield their corresponding oxyacids.

Step 3: Detailed Explanation:
Let us analyze each oxide option individually:
(A) $\text{N}_2\text{O}_5$ (Dinitrogen Pentoxide): Nitrogen is a non-metal in a high oxidation state ($+5$). When dissolved in water, it readily reacts to form nitric acid:
$$\text{N}_2\text{O}_5 + \text{H}_2\text{O} \rightarrow 2\text{HNO}_3$$ This chemical behavior classifies it clearly as an acidic oxide.
(B) NO (Nitric Oxide): This is a well-known neutral non-metal oxide that does not react with acids or bases.
(C) $\text{Na}_2\text{O}$ (Sodium Oxide): Sodium is a highly electropositive alkali metal. Its oxide reacts with water to generate a strong base:
$$\text{Na}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{NaOH}$$ This makes it a basic oxide.
(D) CO (Carbon Monoxide): This is another classic example of a neutral non-metal oxide.
Therefore, option (A) is the correct choice.

Step 4: Final Answer:
The oxide that is acidic in nature is $\text{N}_2\text{O}_5$, corresponding to option (A).