One hybridization of one `s` and one `p` orbital we get

Options

A. Two mutually perpendicular hybrid orbitals
B. Two equivalent hybrid orbitals at `180^(@)`
C. Four hybrid orbitals directed tetrahedrally
D. Three hybrid orbitals in the plane

Answer

To solve the question about the hybridization of one `s` and one `p` orbital, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Orbitals Involved**:
We are given one `s` orbital and one `p` orbital. The `s` orbital is spherical, while the `p` orbital has a dumbbell shape.

2. **Understand Hybridization**:
Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals. In this case, the mixing of one `s` orbital and one `p` orbital will lead to the formation of hybrid orbitals.

3. **Determine the Type of Hybridization**:
When one `s` orbital and one `p` orbital hybridize, they form two equivalent hybrid orbitals. This is known as `sp` hybridization.

4. **Geometry of Hybrid Orbitals**:
The `sp` hybrid orbitals are oriented linearly, which means they are arranged at an angle of 180 degrees to each other. This arrangement is characteristic of linear molecules.

5. **Examples of `sp` Hybridization**:
A common example of a molecule with `sp` hybridization is carbon dioxide (CO₂), which has a linear shape.

6. **Evaluate the Options**:
- **Option A**: Two mutually perpendicular hybrid orbitals - **Incorrect** (they are at 180 degrees, not perpendicular).
- **Option B**: Two equivalent hybrid orbitals at 180 degrees - **Correct** (this describes `sp` hybridization).
- **Option C**: Four hybrid orbitals - **Incorrect** (only two are formed).
- **Option D**: Three hybrid orbitals in the same plane - **Incorrect** (only two `sp` hybrid orbitals are formed).

7. **Conclusion**:
The correct answer is **Option B**, which states that we get two equivalent hybrid orbitals at 180 degrees.