Which of the following leads to bonding?

Options

A.
B.
C.
D.

Explanation

To determine which of the given options leads to bonding, we will analyze the types of orbital overlaps presented in each option.

### Step-by-Step Solution:

1. **Identify the Orbitals in Each Option:**
- **Option A:** S orbital (spherical) and P orbital (dumbbell).
- **Option B:** S orbital and P orbital.
- **Option C:** Two P orbitals.
- **Option D:** One P orbital and one D orbital.

2. **Analyze Option A:**
- The S orbital and P orbital overlap unsymmetrically.
- This type of overlap is referred to as "zero overlapping" and does not lead to bonding.
- **Conclusion:** Option A does not lead to bonding.

3. **Analyze Option B:**
- The S orbital and P orbital overlap head-on.
- This is a symmetrical overlap and is considered the most stable type of overlap.
- The lobes of both orbitals have the same sign, which promotes bonding.
- **Conclusion:** Option B leads to bonding.

4. **Analyze Option C:**
- Two P orbitals are overlapping with opposite signs.
- This results in "negative overlapping," which is not effective for bond formation.
- **Conclusion:** Option C does not lead to bonding.

5. **Analyze Option D:**
- One P orbital and one D orbital are overlapping, but both have negative signs.
- This also results in "negative overlapping," which is insufficient for bond formation.
- **Conclusion:** Option D does not lead to bonding.

6. **Final Conclusion:**
- The only option that leads to bonding is **Option B**.