In which of the following molecule, central atom has more than 8 electrons in outermost orbit?

Options

A. `SO_(3)`
B. `SO_(2)`
C. `P_(2)O_(5)`
D. All of these

Answer

To determine which of the given molecules has a central atom with more than 8 electrons in its outermost orbit, we will analyze each molecule step by step.

### Step 1: Analyze SO3 (Sulfur Trioxide)
1. **Identify the central atom**: In SO3, the central atom is sulfur (S).
2. **Count valence electrons**: Sulfur has 6 valence electrons.
3. **Count monovalent atoms**: There are three oxygen atoms, and since they form double bonds with sulfur, we treat them as bonded atoms.
4. **Calculate hybridization**:
- Using the formula:
\[ \text{Hybridization} = \frac{1}{2} \left( V + M \right) \]
where \( V = 6 \) (valence electrons of sulfur) and \( M = 3 \) (number of oxygen atoms).
- Calculation:
\[ \text{Hybridization} = \frac{1}{2} (6 + 3) = \frac{9}{2} = 4.5 \text{ (which corresponds to sp}^2\text{ hybridization)} \]
5. **Draw the structure**: SO3 has a trigonal planar structure with three double bonds.
6. **Count total electrons around sulfur**:
- Each double bond contributes 4 electrons (2 from sulfur and 2 from oxygen).
- Total: \( 4 \times 3 = 12 \) electrons around sulfur.
7. **Conclusion for SO3**: Sulfur has 12 electrons in its outermost shell, which is more than 8.

### Step 2: Analyze SO2 (Sulfur Dioxide)
1. **Identify the central atom**: In SO2, the central atom is sulfur (S).
2. **Count valence electrons**: Sulfur has 6 valence electrons.
3. **Count monovalent atoms**: There are two oxygen atoms.
4. **Calculate hybridization**:
- Using the formula:
\[ \text{Hybridization} = \frac{1}{2} (6 + 2) = 4 \]
- This corresponds to sp2 hybridization.
5. **Draw the structure**: SO2 has a bent structure with one lone pair and two double bonds.
6. **Count total electrons around sulfur**:
- Each double bond contributes 4 electrons.
- Total: \( 4 \times 2 + 2 \text{ (from lone pair)} = 10 \) electrons around sulfur.
7. **Conclusion for SO2**: Sulfur has 10 electrons in its outermost shell, which is more than 8.

### Step 3: Analyze P2O5 (Diphosphorus Pentoxide)
1. **Identify the central atoms**: In P2O5, the central atoms are phosphorus (P).
2. **Count valence electrons**: Each phosphorus has 5 valence electrons.
3. **Count monovalent atoms**: There are five oxygen atoms.
4. **Calculate hybridization for each phosphorus**:
- Using the formula:
\[ \text{Hybridization} = \frac{1}{2} (5 + 5) = 5 \]
- This corresponds to sp3d hybridization.
5. **Draw the structure**: Each phosphorus is bonded to four oxygen atoms with double bonds.
6. **Count total electrons around each phosphorus**:
- Each double bond contributes 4 electrons.
- Total: \( 4 \times 2 + 1 \text{ (from lone pair)} = 10 \) electrons around each phosphorus.
7. **Conclusion for P2O5**: Each phosphorus has 10 electrons in its outermost shell, which is more than 8.

### Final Conclusion
All three molecules (SO3, SO2, and P2O5) have central atoms that possess more than 8 electrons in their outermost orbit.

### Answer
The answer is: **All of these (SO3, SO2, P2O5)**.

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