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Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Aluminium forms covalent compound with chloride because lonisation enthalpy (∆iH= +5137 kJ/mole) of Aluminium is very high due to small size and chlorine is unable to convert  Al into Al+3 ions. 

However, when anhydrous AlCl3 (which is covalent in character) is dissolved in water, it undergoes hydration as follow:  

                                   AI2CI6 + H2O  ---> 2[Al(H2O)6]+3 + Hydration  Energy (∆H)  

Hydration of anhydrous aIuminium chloride is highly exothermic in nature. The hydration enthalpy is more than ionisation enthalpy of aluminium.This hydration enthalpy removes all the three valence electrons of the aluminium leading to the formation of Al3+ more easly.This AI3+ is hydrated with water and form a complex ion. Thus in water Al exist as [Al(H2O)6]+3 . The three electrons of aluminum is accepted by CI of AlCl3. Thus hydrated AlCl3  represented [Al(H2O)6]Cl3   and it is ionic in nature.

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Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

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Four-center two-electron bond (4C-2e Bond): Structure of AlCl3:

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Titration of Borax: Tincal : Suhaga :

Structure of Borax: Tincal or Suhaga:

Titration of Boric Acid:

DIBORANE-HYDRIDE OF BORONE-(B2H6):

CHEMICAL PROPERTIES OF DIBORANE:

STRUCTURE OF BORON NITRIDE:

STRUCTURE OF BORAZINE OR BORAZOLE:

STRUCTURE OF DIBORANE :

BORIC ACID (H3BO3) :

BORAX BEAD TEST:

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