Among the following, identify the species with an atom in +6 oxidation state.

Options

A. `Ba_(2)XeO_(6)`
B. `XeO_(3)`
C. `CrO_(5)`
D. `SO_(2)Cl_(2)`

Explanation

To identify the species with an atom in the +6 oxidation state, we will analyze each compound provided in the question. We will calculate the oxidation states of the central atoms in each compound step by step.

### Step 1: Analyze BA2XeO6
- **Identify the oxidation states**:
- Barium (Ba) is in Group 2, so its oxidation state is +2.
- Oxygen (O) typically has an oxidation state of -2.

- **Set up the equation**:
\[ 2(\text{Ba}) + x(\text{Xe}) + 6(\text{O}) = 0 \]
\[ 2(+2) + x + 6(-2) = 0 \]
\[ 4 + x - 12 = 0 \]
\[ x - 8 = 0 \implies x = +8 \]

- **Conclusion**: In BA2XeO6, Xe is in the +8 oxidation state.

### Step 2: Analyze CrO5
- **Identify the oxidation states**:
- Oxygen (O) has an oxidation state of -2.

- **Set up the equation**:
\[ x(\text{Cr}) + 5(\text{O}) = 0 \]
\[ x + 5(-2) = 0 \]
\[ x - 10 = 0 \implies x = +10 \]

- **Consider the structure**: In CrO5, there are peroxo groups which can affect the oxidation state of Cr. The maximum oxidation state of Cr is +6.

- **Conclusion**: In CrO5, Cr can be considered in the +6 oxidation state.

### Step 3: Analyze SO2Cl2
- **Identify the oxidation states**:
- Oxygen (O) has an oxidation state of -2.
- Chlorine (Cl) typically has an oxidation state of -1.

- **Set up the equation**:
\[ x(\text{S}) + 2(\text{O}) + 2(\text{Cl}) = 0 \]
\[ x + 2(-2) + 2(-1) = 0 \]
\[ x - 4 - 2 = 0 \]
\[ x - 6 = 0 \implies x = +6 \]

- **Conclusion**: In SO2Cl2, S is in the +6 oxidation state.

### Final Conclusion
The species with an atom in the +6 oxidation state are:
- Cr in CrO5
- S in SO2Cl2

### Summary of Results
- BA2XeO6: Xe = +8
- CrO5: Cr = +6
- SO2Cl2: S = +6

### Answer
The species with an atom in +6 oxidation state are **CrO5 and SO2Cl2**.

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