If an element X forms the highest oxide of the formula `XO_3`, then it belongs to Group

Options

A. 14
B. 15
C. 16
D. 17

Answer

To determine the group of the element X that forms the highest oxide with the formula \( XO_3 \), we can follow these steps:

### Step 1: Analyze the Oxide Formula
The oxide formula given is \( XO_3 \). This indicates that the element X is combined with three oxygen atoms.

### Step 2: Determine the Oxidation State of X
In the oxide \( XO_3 \), the oxidation state of oxygen is typically \(-2\). Therefore, we can set up the equation for the oxidation state of X:
\[ \text{Oxidation state of } X + 3 \times (-2) = 0 \]
This simplifies to:
\[ \text{Oxidation state of } X - 6 = 0 \]
Thus, the oxidation state of X is:
\[ \text{Oxidation state of } X = +6 \]

### Step 3: Identify Possible Groups
Now, we need to determine which group of the periodic table can have an element with a maximum oxidation state of +6:
- **Group 14 (Carbon Family)**: Elements in this group can have a maximum oxidation state of +4.
- **Group 15 (Nitrogen Family)**: Elements in this group can have a maximum oxidation state of +5.
- **Group 16 (Oxygen Family)**: Elements in this group can have a maximum oxidation state of +6.
- **Group 17 (Halogens)**: Elements in this group can have a maximum oxidation state of +7, but they typically do not form oxides with a +6 state.

### Step 4: Conclusion
Since the element X has an oxidation state of +6, it must belong to **Group 16**, which is the oxygen family.

### Final Answer
Element X belongs to **Group 16**.

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