Electron-Deficient Compounds
| Formula / Notation | Incomplete octet: e.g., BF₃, AlCl₃, B₂H₆ |
|---|---|
| Also Known As | Lewis acid; incomplete octet compound; electron-poor compound; BF₃-type compound; boron compounds |
What is Electron-Deficient Compounds?
Electron-deficient compounds are molecules or ions that have fewer than the expected number of electrons for a complete octet around the central atom. They act as Lewis acids (electron pair acceptors) and form adducts with electron-donating species (Lewis bases). Classic examples are boron trifluoride (BF₃), aluminium chloride (AlCl₃), and diborane (B₂H₆).
Formula & Notation
Other Names / Synonyms: Lewis acid; incomplete octet compound; electron-poor compound; BF₃-type compound; boron compounds
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
Electron-deficient compounds are molecules or ions that have fewer than the expected number of electrons for a complete octet around the central atom. They act as Lewis acids (electron pair acceptors) and form adducts with electron-donating species (Lewis bases). Classic examples are boron trifluoride (BF₃), aluminium chloride (AlCl₃), and diborane (B₂H₆).
Friedel-Crafts catalysts (AlCl₃, BF₃); Lewis acid catalysts in organic synthesis; hydroboration reactions (B₂H₆, borane); synthesis of organoboron compounds; polymerisation catalysts
Boron trifluoride is toxic and corrosive; aluminium chloride reacts violently with water producing HCl. Diborane is flammable, toxic, and spontaneously ignites in moist air. Handle with extreme caution in dry, inert conditions with appropriate PPE.
The formula or notation for Electron-Deficient Compounds is: Incomplete octet: e.g., BF₃, AlCl₃, B₂H₆