How many equitorial bonds are there are in `PCl_(5)` ?

Explanation

To determine the number of equatorial bonds in \( PCl_5 \), we can follow these steps:

### Step 1: Understand the Structure of \( PCl_5 \)
Phosphorus pentachloride (\( PCl_5 \)) has a specific molecular geometry. It is important to know that phosphorus is in group 15 of the periodic table and has 5 valence electrons.

**Hint:** Remember that the molecular geometry can help you visualize the arrangement of bonds.

### Step 2: Determine the Hybridization
The hybridization of phosphorus in \( PCl_5 \) is \( sp^3d \). This indicates that one s orbital, three p orbitals, and one d orbital are mixed to form five equivalent hybrid orbitals.

**Hint:** Hybridization helps in understanding the bonding and geometry of the molecule.

### Step 3: Identify the Molecular Geometry
The geometry of \( PCl_5 \) is trigonal bipyramidal. In this geometry, there are two types of positions for the bonds: axial and equatorial.

**Hint:** Visualizing the geometry can clarify the arrangement of different types of bonds.

### Step 4: Count the Types of Bonds
In a trigonal bipyramidal structure:
- There are 3 equatorial bonds that lie in a plane.
- There are 2 axial bonds that are positioned above and below this plane.

**Hint:** Focus on the arrangement of bonds in the trigonal bipyramidal geometry to differentiate between equatorial and axial bonds.

### Step 5: Conclusion
Thus, in \( PCl_5 \), there are **3 equatorial bonds**.

**Final Answer:** The number of equatorial bonds in \( PCl_5 \) is **3**.

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