transition metals (a level chemistry)(help me)
When [Al(H20)6]3+ reacts with Na2CO3, it forms Al(H20)3(OH)3
But when [Cu(H20)6]2+ reacts with Na2CO3, it forms CuCO3 despite the conditions being the same
Why is this the case?
But when [Cu(H20)6]2+ reacts with Na2CO3, it forms CuCO3 despite the conditions being the same
Why is this the case?
The charge on the transition metal ion affects its acidity, and that determines what products you get.
3+ ions are sufficiently acidic to form the metal hydroxide ppt.
2+ ions are not as acidic and form the metal carbonate ppt.
There's a nice explanation here: https://www.chemguide.co.uk/inorganic/complexions/aquaco3.html
As for why there is a difference in acidity, it's due to the charge density on the metal ion and how that affects the strength of the O-H bonds in its water ligands
Again there's a nice explanation here: https://www.chemguide.co.uk/inorganic/complexions/acidity.html
3+ ions are sufficiently acidic to form the metal hydroxide ppt.
2+ ions are not as acidic and form the metal carbonate ppt.
There's a nice explanation here: https://www.chemguide.co.uk/inorganic/complexions/aquaco3.html
As for why there is a difference in acidity, it's due to the charge density on the metal ion and how that affects the strength of the O-H bonds in its water ligands
Again there's a nice explanation here: https://www.chemguide.co.uk/inorganic/complexions/acidity.html
Reply 2
aluminium is amphoteric. this means it has the ability to act as both an acid and a base. in this case, it is acting as an acid because it is donating 3 protons, to gain a neutral charge. the second reaction is a displacement reaction, and it is with copper which isnt amphoteric
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