Chemistry: Reactions Of Ipns In Solutipn
This flashcard set explains how metal ions behave in aqueous solutions, emphasizing the formation of hexaaqua complexes and the color differences between main group and transition metal ions. It also explores the electronic transitions in incomplete d sub shells that cause the vivid colors of transition metal ions.
What do most metal actions exist as in aqueous solution
The hexaaqua complex ion
Key Terms
What do most metal actions exist as in aqueous solution
The hexaaqua complex ion
What kind of ions do main group metals form
Colourless
What are most transition metal ions
Coloured
Why are lost transition metal ions coloured
-incomplete d sub shell
-some wavelengths of vidible light absorbed
-d electrons ground state to excited state -
Remaining colours of visi...
Copper 2 hexaaqua ion colour
Blue
Iron 3 hexaaqua ion colour
Purple
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| Term | Definition |
|---|---|
What do most metal actions exist as in aqueous solution | The hexaaqua complex ion |
What kind of ions do main group metals form | Colourless |
What are most transition metal ions | Coloured |
Why are lost transition metal ions coloured | -incomplete d sub shell |
Copper 2 hexaaqua ion colour | Blue |
Iron 3 hexaaqua ion colour | Purple |
Aluminium 3 hexaaqua ion colour | Colourless |
What is there a hydrolysis reaction beteeen in solution | Metal aqua ion and water |
What does the charge on the metal job cause the electron density in the water ligand to do | Move closer to metal ion- water ligand polarised |
What happens if the metal ion had enough polarising power | Bonds in water weakened One of bonds breaks and proton donated to water molecule |
What is relationship between pKa and strength of acidity of hexaaqua ion | Lower pka- stronger acid- equilibrium lies further to right |
What is the difference in acidity due to in iron 2 and iron 3 | Charge/size ratios |
Why is iron 3 more acidic than iron 2 | Smaller and more highly charged and therefore able to polarise water ligands more OH bonds in water weakened more readily and protons more easily donated |
Equations for al3+ hexaaqua with water | [Al(H2O)6]3+ + H2O > [Al(H2O)5(OH)]2+ + H3O+ |
Why will al3 hexaaqua be more acidic than copper 2 hexaaqua | Al3 ions smaller and more highly charged therefore able to polarise water ligands more, weaken OH bonds therefore donate H+ ions more readily |
What does adding a base to an aqueous solution of the metal aqua ion produce | Insoluble precipitates of the metal hydroxide |
Equation for adding hydroxide to metal aqua ion | [M(H2O)6]3+ + OH- > [M(H2O)5(OH)]2+ + H2O |
What happens to the equilibrium if you add more OH- ions to metal aqua ion | Equilibrium shifts to the right to oppose the increase in [OH-] and a new equilibrium set up |
Equation for new equilibrium set up after adding more OH- ions to metal aqua ion | [M(H2O)5(OH)]2+ + OH- > [M(H2O)4(OH)2]+ + H2O |
What happens to the equivlirum if you add FURTHER OH- ions to the metal aqua ion | Equilibrium shift to the right to oppose increase in [OH-] and final equilibrium set up |
Equation for final equilibrium set up after adding further OH- ions to metal aqua ions | [M(H2O)4(OH)2] + OH- > [M(H2O)3(OH)3] + H2O |
Why does [M(H2O)3(OH)3] precipitate out | It’s neutral and insoluble |
Overall equation metal aqua ion and hydroxide | [M(H2O)6]3+ + 3OH- > [M(H2O)3(OH)3] + 3H2 |
Iron 2 hexaaqua ion colour | Green |
Colour of PPT iron 2 and NAOH | Brown |
How can reaction between iron 2 hexaaqua and sodium hydroxide be reversed | Adding acid |
What colour ppt does Al3+ hexaaqua form with hydroxide | White |
Equation for aluminium hydroxide acting as a base | [Al(H2O)3(OH)3] + 3H+ > [Al(H2O)6]3+ |
Equation for aluminium hydroxide acting as an acid | [Al(H2O)3(OH)3] + OH- > [Al(H2O)2(OH)4]- + H2O |
What does the white ppt of aluminium hydroxide dissolve to form | A colourless solution |
Overall equation for metal hexaaqua ion with NAOH | [M(H2O)6]2+ + 2OH- > [M(H2O)4(OH)2] + 2H2O |
What colour ppt is formed from reaction of iron 2 hexaaqua and NAOH | Green/grey |
Why does green/green iron 2 PPT turn green when left to stand in air | Oxidation to iron 3 hydroxide |
Equation for reaction of iron 2 oxide to iron 3 oxide | [Fe(H2O)4(OH)2] > [Fe(H2O)3(OH)3] + H+ + e- |
What colour ppt does copper 2 hexaaqua form with sodium hydroxide | Blue |
Why is ammonia able to react with metal aqua ions to produce metal hydroxides | It’s a weak base |
Reaction of iron 3 hexaaqua with aqueousammonia | [Fe(H2O)6]3+ + 3NH3 > [Fe(H2O)3(OH)3] + 3NH4+ Brown ppt |
Reaction of aluminium 3 hexaaqua with aqueous ammonia | [Al(H2O)6]3+ + 3NH3 > [Al(H2O)3(OH)3] + 3NH4+ White ppt |
Why can’t ammonia hydrolyse aluminium hydroxide further | It’s a weak base |
Reaction of iron 2 hexaaqua with aqueous ammonia | [Fe(H2O)6]2+ + 2NH3 > [Fe(H2O)4(OH)2] + 2NH4+ Green grey ppt |
Reaction of copper 2 aqueous ammonia | [Cu(H2O)6]2+ + 2NH3 > [Cu(H2O)4(OH)2] + 2NH4+ Blue ppt |
What can be formed by a ligand substitution reaction when an excess of ammonia is added to the copper 2 hydroxide precipitate | A new complex |
Equation for copper 2 hydroxide and excess ammonia | [Cu(H2O)4(OH)2] + 4NH3 > [Cu(H2O)2(NH3)4 2+ + 2H2O + 2OH- Deep blue soln |
Overall reaction between hexaaqua copper II ion and excess ammonia | [Cu(H2O)6]2+ + 4NH3 > [Cu(NH3)4(H2O)2]2+ + 2H2O |
What do 2+ metal ions react with sodium carbonate to form | Insoluble metal carbonates |
Reaction of copper 2 hexaaqua with sodium carbonate | [Cu(H2O)6]2+ + CO32- > CuCO3 + 6H2O Blue soln to blue green ppt |
Reaction iron 2 hexaaqua and aqueous sodium carbonate | [Fe(H2O)6]2+ + CO32- > FeCO3 + 6H2O Green soln to green grey ppt |
Why do 3+ metal ions form the hydroxide and release carbon dioxide gas when reacting with sodium carbonate | They’re stronger acids |
Reaction iron 3 with sodium carbonate | 2[Fe(H2O)6]3+ + 3CO32- > 2Fe(H2O)3(OH)3] + 3CO2 + 3H2O Orange soln to brown ppt |
Equation aluminium 3 with sodium carbonate | 2[Al(H2O)6]3+ + 3CO32- > 2[Al(H2O)3(OH)3] + 3CO2 + 3H2O Colourless soln Fizz |