![]() It is used in solvent extraction, organic catalysis reaction, in Al dual-ion batteries.Due to its thermal stability, low melting point and low vapor pressure, it is widely used as an ionic electrolyte for redox reactions and chemical reactions.Note: A polyatomic anion with a metal cation yields an ionic compound. It is a polyatomic anion where a chloride ion shares two electrons by a covalently coordinate bond to AlCl 3 (covalent ). Tetrachloroaluminate is a covalent molecule. They are also observed as an intermediate species during many organic reactions like Friedel Crafts alkylation, acylation etc. Note : Formation of AlCl 4 – – As AlCl 3 has empty p orbital that can accept another electron to complete its octet, it reacts with a chloride ion easily to form a more stable ionic molecule. It has its octet complete making it a stable compound. It has high thermal stability, high conductivity, low melting point which make it an excellent choice for further study and investigation. ![]() Molecule Tetrachloroaluminate, AlCl 4 – Type Polyatomic ion Hybridisation sp 3 Shape Tetrahedral Bond angle 109’5” Bond and Lone Pairs 4, 12 Is AlCl 4 – stable ? It has 4 single bonds with bond length of Al-Cl at around 2.06-2.08 armstrong. It has sp 3 hybridisation with tetrahedral geometry and bond angle of 109 ’5 ”. It is a tetrahedral structure and not square planar as alkaline earth metals do not necessarily exhibit square planar complexes formation since they do not contribute to the overall CFSE value. Hybridisation of a molecule = ( Valence electrons of the central atom + Number of monovalent atoms attached to the central atom + Negative charge on the molecule – Positive charge on the molecule )/2 There is a simple rule or equation to be followed to find out the hybridization of molecules real quick. Hybridisation, Shape and Angle of AlCl 4 – : Note: In actual sense of chemistry, there is a coordinate bond formation between AlCl 3 and Cl – ( electron pairs shared completely by chloride ion, a type of covalent bond). It has 4 bond pairs ( that is formed by a single covalent bond here) and 12 total lone pairs of electrons ( that did not participate in bond formation). ĪlCl 4 – valence electrons, bond pairs and lone pairs of electrons : Note: Elements having expanded valence shells like 3d elements, it can exceed the octet rule like SF 6, PF 5 or elements with fewer valence electrons can have incomplete octet like H 2.
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