Most acidic oxide among the following is

Options

A. `N_a 2_O `
B. `N_2 O_3 `
C. `N_2 O_5 `
D. `P_2 O_5`

Answer

To determine the most acidic oxide among the given options, we can follow these steps:

### Step 1: Identify the nature of the oxides
- **Metal oxides** are generally basic in nature.
- **Non-metal oxides** are generally acidic in nature.

### Step 2: Identify the elements and their classifications
- Given elements include sodium (Na), nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).
- Sodium is a metal (basic oxide).
- Nitrogen and phosphorus are non-metals (acidic oxides).
- Arsenic, antimony, and bismuth are metalloids and have varying acidic/basic properties.

### Step 3: Focus on non-metal oxides
- Since we are looking for the most acidic oxide, we will focus on the oxides of nitrogen and phosphorus, as they are non-metals.

### Step 4: Compare the oxides of nitrogen
- The relevant oxides of nitrogen are:
- \( N_2O_3 \)
- \( N_2O_5 \)

### Step 5: Determine the oxidation states
- For \( N_2O_3 \):
- Let the oxidation state of nitrogen be \( x \).
- The equation is: \( 2x + 3(-2) = 0 \)
- Solving gives: \( 2x - 6 = 0 \) → \( 2x = 6 \) → \( x = +3 \)

- For \( N_2O_5 \):
- The equation is: \( 2x + 5(-2) = 0 \)
- Solving gives: \( 2x - 10 = 0 \) → \( 2x = 10 \) → \( x = +5 \)

### Step 6: Compare the acidity based on oxidation states
- The higher the oxidation state of the central atom (nitrogen in this case), the more acidic the oxide.
- \( N_2O_3 \) has an oxidation state of +3.
- \( N_2O_5 \) has an oxidation state of +5.

### Conclusion
- Since \( N_2O_5 \) has a higher oxidation state (+5) compared to \( N_2O_3 \) (+3), it is the most acidic oxide among the options provided.

### Final Answer
The most acidic oxide among the given options is \( N_2O_5 \).

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