If the formula of basic Beryllium nitrate is `[Be_(x)O(NO_3)_(6)]`. What is the value of 'n' here

Options

A. 2
B. 3
C. 4
D. 5

Answer

To find the value of 'x' in the formula of basic Beryllium nitrate, `[Be_(x)O(NO_3)_(6)]`, we will analyze the charges of the components involved.

### Step-by-Step Solution:

1. **Identify the Charges:**
- Beryllium (Be) typically has a charge of +2.
- Oxygen (O) in the nitrate ion (NO₃⁻) has a charge of -2.
- Each nitrate ion (NO₃) has a charge of -1.

2. **Set Up the Equation:**
- The overall charge of the compound must equal zero.
- The formula can be expressed in terms of charges:
\[ \text{Total charge} = (\text{Charge of Be}) + (\text{Charge of O}) + (\text{Charge from NO}_3) \]
- This gives us:
\[ +2x + (-2) + 6(-1) = 0 \]

3. **Calculate the Charges:**
- The charge from the oxygen is -2 (since there is one O²⁻).
- The charge from the six nitrate ions is \(6 \times (-1) = -6\).
- Therefore, the equation simplifies to:
\[ +2x - 2 - 6 = 0 \]

4. **Simplify the Equation:**
- Combine the constants:
\[ +2x - 8 = 0 \]

5. **Solve for x:**
- Rearranging the equation gives:
\[ 2x = 8 \]
- Dividing both sides by 2 results in:
\[ x = 4 \]

### Conclusion:
The value of 'x' in the formula of basic Beryllium nitrate `[Be_(x)O(NO_3)_(6)]` is **4**.