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

Options

A. Two mutually perpendicualr orbitals
B. Two orbitals at `180^(@)` .
C. Two orbitals directed tetrahedrally
D. Three orbitals in a plane

Answer

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

### Step 1: Understand the Orbitals
- The `s` orbital has a spherical shape.
- The `p` orbital has a dumbbell shape, with two lobes on either side of the nucleus.

**Hint:** Remember the shapes of the orbitals; `s` is spherical and `p` is dumbbell-shaped.

### Step 2: Determine the Number of Participating Orbitals
- In this case, we have one `s` orbital and one `p` orbital participating in the hybridization.
- The total number of participating orbitals is 2 (1s + 1p).

**Hint:** Count the number of orbitals involved in the hybridization process.

### Step 3: Identify the Hybridization Type
- When one `s` and one `p` orbital hybridize, they form two new hybrid orbitals.
- The hybridization that occurs here is called `sp` hybridization.

**Hint:** Recall that `sp` hybridization occurs when one `s` and one `p` orbital combine.

### Step 4: Determine the Shape and Orientation of Hybrid Orbitals
- The resulting `sp` hybrid orbitals will have a linear arrangement.
- The angle between the two `sp` hybrid orbitals will be 180 degrees.

**Hint:** Remember that `sp` hybridization leads to a linear geometry.

### Step 5: Conclusion
- Therefore, the hybridization of one `s` and one `p` orbital results in `sp` hybridization, which gives us two hybrid orbitals that are linear in shape.

**Final Answer:** The correct answer is `sp` hybridization.