How does aluminium form [AlF6]-3?

Asked by Thoms | 8th Jan, 2014, 06:57: PM

Expert Answer:

When aluminium and fluoride are together in aqueous solution, they readily form complex ions such as [AlF6]3-.

Electronic configuration of Aluminum is: [Ne] 3s23p1

Al has vacant 'd' orbitals and can expand its octet in [AlF6]. It has six ligands.

Aluminium can accommodate six F atoms. [AlF6]3- is octahedral and has 3-center, 4-electron bonding.

 

Al3+ + 6 F-  <----------> [AlF6]3-

[AlF6]3- is the most stable complex. This is explained by the fact that alumimium and fluoride, which are both very compact ions, fit together just right to form the octahedral aluminium hexafluoride complex. When aluminum and fluoride are together in water in a 1:6 molar ratio, [AlF6]3- is the most common form, even in rather low concentrations.

 

Answered by Hanisha Vyas | 14th Jan, 2014, 11:50: AM

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