2.6 Reactions of ions in solution

• The type of complex formed can be identified by testing with carbonate, ammonia, and sodium hydroxide.
• The carbonate ion reacts with the complex, producing metal with OH- and H2O.
• Carbonate ion reacts with free hydroxo ions instead of displacing water ligands.
• To test for methylene solutions, these reactions can be used to identify them.
• Three plus ions are more acidic than two plus ions, resulting in more hydroxo ions in solution.
• When a three plus reactant is used, a hydroxide complex is formed with carbon dioxide and water.
• Metal aqua ions form the six water ligands that were around them and detach from the complex, forming a precipitate.
• Ammonia is not a strong base.
• Adding an excess amount of ammonia can lead to a ligand exchange reaction.
• Metal aqua ions have six water molecules ligands surrounding them.
• Metal aqua ions can react with a carbonate instead of ammonia or hydroxide to form a precipitate.
• Metal aqua ions react with carbonates to form an insoluble methyl carbonate.
• When metal aqua ions react with ammonia, they can use OHS- or use hydrolysis.
• When a 3 plus metal ion reacts with a carbonate, it forms a metal carbonate precipitate.
• When ammonia doesn't have a negative charge itself, it needs water to form the OH-minuses which makes it basic.
• A complete substitution of all of the water ligands occurs when an excess amount of ammonia is added to some metal hexa aqua complexes.
• When ammonia is added to metal acridine, it produces the same metal hydroxides as if hydroxide was added.
• Xide precipitates as well as giving up or accepting protons.
• When excess ammonia is added to some metal hexa aqua complexes, some of the ligands are displaced and a charged soluble complex is formed.
• When a 2 plus metal ion reacts with a carbonate, it forms a metal carbonate precipitate.
• Aluminium hydroxide is an example of an amphoteric compound.
• Transition metal ions react within water and have specific properties.
• Transition metal ions form hydrated metal aqua complexes when added to water.
• Hydrated metal aqua complexes are surrounded by six water ligands which form coordinate bonds around the metal ion.
• Amphoteric metal hydroxides can act as both an acid and a base.
• Further reactions of metal aqua ions with ammonia can form metal hydroxides.
• When an acid is added to aluminium hydroxide, it acts as a bronsted-lowry base and accepts a proton to dissolve the complex.
• When a base is added to aluminium hydroxide, it acts as a bronsted-lowry acid and donates a proton to form a new complex.
• Aluminium hydroxide is an example of an amphoteric metal hydroxide.
• All of the metal ions mentioned (iron, copper, aluminum, iron 3) will react with ammonia to form precipitates, except for copper hydroxide which dissolves when excess ammonia is added due to ligand substitution.
• All of the metal ions mentioned (iron, copper, aluminum, iron 3) will react with sodium hydroxide to form precipitates, except for aluminum hydroxide which dissolves when excess sodium hydroxide is added due to its amphoteric nature.
• All of the metal ions mentioned (iron, copper, aluminum, iron 3) will react with sodium carbonate to form precipitates, with aluminum and iron 3 forming bubbles of carbon dioxide in addition to the precipitate.
• Fe 2 plus ions oxidize readily with air, so the iron 2 plus solution should be made fresh to avoid oxidation to Fe 3 plus.
• Iron(III) is insoluble in excess hydroxide or ammonia.
• Copper(II) reacts with hydroxide or ammonia to form a pale blue precipitate.
• Iron(II) is insoluble in excess hydroxide or ammonia.
• Iron(III) reacts with sodium carbonate to form a brown precipitate.
• Iron(III) is yellow-orange.
• Aluminium is amphoteric and forms a colorless solution with excess hydroxide.
• Iron(II) is pale green and oxidizes readily to iron(III).