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

Options

A. `NO_2`gt `CO_2` gt`B_2O_3` gt BeO gt `Li_2O`
B. `CO_2`gt `NO_2` gt`B_2O_3` gt BeO gt `Li_2O`
C. `Li_2O`gt BeO gt`B_2O_3` gt `CO_2` gt `NO_2`
D. `B_2O_3` gt `CO_2` gt `NO_2`gt`Li_2O`gt BeO

Answer

To determine the decreasing acidic nature of oxides, we need to analyze the oxides of different elements based on their position in the periodic table and their corresponding acidic properties.

### Step-by-Step Solution:

1. **Identify the Oxides**: We have the following oxides to consider:
- Nitrogen oxide (NO or N2O5)
- Carbon dioxide (CO2)
- Boron oxide (B2O3)
- Beryllium oxide (BeO)
- Lithium oxide (Li2O)

2. **Understand Acidic Nature**: The acidic nature of oxides generally increases with the increase in electronegativity of the element forming the oxide. Non-metals tend to form more acidic oxides compared to metals.

3. **Position in the Periodic Table**:
- Nitrogen (N) is a non-metal and has a high electronegativity.
- Carbon (C) is also a non-metal, but less electronegative than nitrogen.
- Boron (B) is a metalloid and has a lower acidic character compared to carbon and nitrogen.
- Beryllium (Be) is a metal and forms a less acidic oxide compared to boron.
- Lithium (Li) is also a metal and has the least acidic oxide among these.

4. **Order of Acidic Nature**:
- Nitrogen oxides (NO or N2O5) are the most acidic due to the high electronegativity of nitrogen.
- Carbon dioxide (CO2) follows, as carbon is less electronegative than nitrogen but still a non-metal.
- Boron oxide (B2O3) is next; boron is a metalloid and has a lower acidic character.
- Beryllium oxide (BeO) is less acidic than boron oxide because beryllium is a metal.
- Lithium oxide (Li2O) is the least acidic as lithium is also a metal and forms a basic oxide.

5. **Final Sequence**: Based on the analysis, the correct sequence representing the decreasing acidic nature of the oxides is:
- N2O5 > CO2 > B2O3 > BeO > Li2O