PCl5 has five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal shape.
Questions & Step-by-step Solutions
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Q
Q: What is the shape of the PCl5 molecule?
Solution: PCl5 has five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal shape.
Steps: 5
Step 1: Identify the central atom in the PCl5 molecule, which is phosphorus (P).
Step 2: Count the number of chlorine (Cl) atoms bonded to the phosphorus atom. There are five Cl atoms.
Step 3: Determine the number of bonding pairs. Since there are five Cl atoms, there are five bonding pairs.
Step 4: Check for lone pairs on the central atom (P). In PCl5, there are no lone pairs on phosphorus.
Step 5: Use the number of bonding pairs and lone pairs to determine the molecular shape. With five bonding pairs and no lone pairs, the shape is trigonal bipyramidal.
