The reaction between phosphorus (P) and chlorine (Cl₂) produces phosphorus trichloride (PCl₃). Phosphorus can also react with chlorine to form phosphorus pentachloride (PCl₅) depending on the stoichiometry of the reactants used.
Reaction Overview:
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Formation of Phosphorus Trichloride (PCl₃): \[ P + 3Cl_2 \rightarrow PCl_3 \]
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Formation of Phosphorus Pentachloride (PCl₅): \[ P + 5Cl_2 \rightarrow PCl_5 \]
Lewis Dot Structures:
For Phosphorus Trichloride (PCl₃):
- Phosphorus (P) has 5 valence electrons.
- Chlorine (Cl) has 7 valence electrons.
Lewis Dot Structure for PCl₃:
- The central atom, phosphorus, is surrounded by three chlorine atoms.
- Each chlorine atom forms a single bond with phosphorus, utilizing one of phosphorus's valence electrons for bonding.
- Each chlorine atom has three lone pairs of electrons remaining (6 electrons) after the bond is formed.
Here’s a simple representation of the Lewis structure:
Cl: Cl:
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:Cl — P — Cl:
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Cl: ...
In this structure:
- "Cl" represents chlorine.
- ":" represents the lone pairs of electrons on the chlorine atoms.
- The lines represent the bonds formed between phosphorus and chlorine.
For Phosphorus Pentachloride (PCl₅):
When phosphorus forms phosphorus pentachloride, it utilizes all five of its valence electrons.
Lewis Dot Structure for PCl₅:
- Phosphorus forms five single bonds with five chlorine atoms.
- Each chlorine atom will have three lone pairs of electrons remaining.
Here’s a simple representation:
Cl: Cl:
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Cl:— P —Cl:
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Cl: Cl:
In this diagram:
- The central phosphorus atom is bonded to five chlorine atoms, using all five of its valence electrons.
- Each chlorine atom has three lone pairs (the ":" symbols) remaining.
Summary
- PCl₃ and PCl₅ are both products of the reaction between phosphorus and chlorine, and their Lewis dot structures reflect how the valence electrons are utilized in bonding.
- The structure shows the bonds between phosphorus and chlorine, and the arrangement of lone pairs on the chlorine atoms.