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Aqueous Ions
AQA A Level Chemistry
| Question | Answer |
|---|---|
| Define Lewis acid and Lewis base | Lewis acid- electron pair acceptor, Lewis base-electron pair donor |
| Give the formula of metal-aqua ions formed when iron(II), copper(II), iron (III) and aluminium ions in aqueous solution. | [Fe(H2O)6]2+, [Cu(H2O)6]2+,, [Fe(H2O)6]3+,[Al(H2O)6]3+, |
| Explain why [Fe(H2O)6]3+, is more acidic than [Fe(H2O)6]2+, | Fe3+ is more charge dense than Fe2+ , because it is smaller and has a higher charge. This means it has a bigger polarising effect on its water ligands. This weakens the 0—H bond in the water ligand and makes it more likely to hydrolyse in the presence of |
| Describe what you would observe and give an equation for the reaction between [Fe(H20)6]2+ and a few drops of sodium hydroxide. | Green solution forms a green precipitate [Fe(H2O)6]2+ + 20H- ---> [Fe(H20)4(OH)2 + 2H2O |
| "Describe what you would observe and give an equation for the reaction between [Fe(H20)6]2+ and a few drops of ammonia | Green solution forms a green precipitate [Fe(H20)6]2+ + 2NH3 ------> [Fe(H20)4(OH)2] + 2NH4+ |
| State and explain what happens to the transition metal containing product of the above reaction if the reaction mixture is left to stand in air. | The green precipitate turns brown as the iron (II) is oxidised to iron (Ill) by the oxygen in air |
| Describe what you would observe and give an equation for the reaction between [Fe(H20)6]2+ and a few drops of sodium carbonate. | Green solution forms a green precipitate [Fe(H20)6]2+ + CO32 - ------.> FeCO3 + 6H20 |
| Describe what you would observe and give an equation for the reaction between [Cu(H20)6]2+ and a few drops of sodium hydroxide. | Blue solution forms a Blue precipitate [Cu(H2O)6]2+ + 20H- ---> [Cu(H20)4(OH)2] + 2H2O |
| "Describe what you would observe and give an equation for the reaction between [Cu(H20)6]2+ and a few drops of ammonia | Blue solution forms a Blue precipitate [Cu(H20)6]2+ + 2NH3 ------> [Cu(H20)4(OH)2] + 2NH4+ |
| "Describe what you would observe and give an equation for the reaction between [Cu(H20)4(OH)2] and excess aqueous ammonia | Blue precipitate to dark blue solution [Cu(H2O)4(OH)2] + 4NH3 → [Cu(H2O)2(NH3)4]2+ + 2H2O + 2OH- |
| Describe what you would observe and give an equation for the reaction between [Cu(H20)6]2+ and a few drops of sodium carbonate. | Blue solution forms a Blue precipitate [Cu(H20)6]2+ + CO32 - ------.> CuCO3 + 6H20 |
| Describe what you would observe and give an equation for the reaction between [Al(H20)6]3+ and a few drops of sodium hydroxide. | Colourless solution forms a white precipitate [Al(H2O)6]3+ + 30H- ---> [Al(H20)3(OH)3] + 3H2O |
| "Describe what you would observe and give an equation for the reaction between [Al(H20)3(OH)3 and excess Sodium Hydroxide | White precipitate re-dissolved to form a colourless solution [Al(H2O)3(OH)3] + OH- → [Al(H2O)2(OH)4]- + H2O |
| Describe what you would observe and give an equation for the reaction between [Al(H20)6]33+ and a few drops of sodium carbonate. | Colourless solution forms a white precipitate effervescence 2[Al(H20)6]3+ + 3CO32 - ------.> 2[Al(H20)3(OH)3] + 3CO2 + H2O |
| "Describe what you would observe and give an equation for the reaction between [Al(H20)6]3+ and a few drops of ammonia | Colourless solution forms a White precipitate [Al(H20)6]3+ + 3NH3 ------> [Al(H20)3(OH)3] + 3NH4+ |
| Describe what you would observe and give an equation for the reaction between [Fe(H20)6]3+ and a few drops of sodium hydroxide. | Orange solution forms a brown precipitate [Fe(H2O)6]3+ + 30H- ---> [Fe(H20)3(OH)3] + 3H2O |
| "Describe what you would observe and give an equation for the reaction between [Fe(H20)6]3+ and a few drops of ammonia | Orange solution forms a brown precipitate [Fe(H20)6]3+ + 3NH3 ------> [Fe(H20)3(OH)3] + 3NH4+ |
| Describe what you would observe and give an equation for the reaction between [Fe(H20)6]33+ and a few drops of sodium carbonate. | Orange solution forms a brown precipitate effervescence 2[Fe(H20)6]3+ + 3CO32 - ------.> 2[Fe(H20)3(OH)3] + 3CO2 + H2O |
| Write equations to demonstrate the amphoteric nature of [Al(H20)3(OH)3] | [Al(H20)3(OH)3] + OH- ------> [Al(OH)4]- + 3H2O [Al(H20)3(OH)3] + H3O+ ------> [Al(H2O)6]3+ + 3H2O |
Created by:
JBearfield
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