Which of the following sequence correctly represents the decreasing acidic nature of oxides?

Options

A. `NO_2` > `CO_2` >`B_2O_3` >`BeO` > `Li_2O`
B. `CO_2`> `NO_2` g>`B_2O_3` > `BeO` > `Li_2O`
C. `Li_2O`>` BeO` >`B_2O_3` >`CO_2` > `NO_2`
D. `B_2O_3` > `CO_2` > `NO_2`>`Li_2O`>` BeO `

Answer

To determine the decreasing acidic nature of oxides, we need to understand the relationship between the non-metallic character of the elements and the acidity of their oxides. Here’s a step-by-step solution:

### Step 1: Identify the Elements
We need to identify the elements whose oxides we are comparing. Common elements that form oxides include:
- Boron (B)
- Carbon (C)
- Nitrogen (N)
- Oxygen (O)
- Fluorine (F)
- Beryllium (Be)
- Lithium (Li)

### Step 2: Understand Acidic Oxides
Acidic oxides are typically formed by non-metals. The more non-metallic an element is, the more acidic its oxide tends to be. Therefore, we can rank the oxides based on the non-metallic character of the elements.

### Step 3: Rank Non-Metallic Character
In the periodic table, non-metallic character increases from left to right across a period. Therefore, we can rank the elements based on their position in the periodic table:
- Fluorine (F) - Highest non-metallic character
- Oxygen (O)
- Nitrogen (N)
- Carbon (C)
- Boron (B)
- Beryllium (Be) - Lower non-metallic character
- Lithium (Li) - Lowest non-metallic character

### Step 4: Determine the Order of Acidic Nature
Based on the non-metallic character, we can arrange the oxides in decreasing order of acidity:
1. Nitrogen oxide (NO or N2O5)
2. Carbon oxide (CO2)
3. Boron oxide (B2O3)
4. Beryllium oxide (BeO)
5. Lithium oxide (Li2O)

### Step 5: Final Sequence
Thus, the correct sequence representing the decreasing acidic nature of the oxides is:
**N2O5 > CO2 > B2O3 > BeO > Li2O**

### Conclusion
The correct answer is the sequence of oxides based on their acidic nature, which decreases from nitrogen oxide to lithium oxide.

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