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6 Cards in this Set
- Front
- Back
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When placed in water, transition metals:
1) Form? 2) Because? |
1) The form metal-aqua complexes.
2) One of the lone pairs on the Oxygen atoms in 6 water molecules co-ordinately bonds onto the central metal ions. |
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When the central metal ion is '+2': 1) The metals can be? 2) Their complexes will be? – Include their colours. |
• Fe(II) - [Fe(H2O)6]2+ - Green.
• Cu(II) - [Cu(H2O)6]2+ - Blue. • Co(II) - [Co(H2O)6]2+ - Pink. |
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When the central metal ion is '3+':
1) The metals can be? 2) Their complexes will be? – Include their colours. |
• Fe(III) - [Fe(H2O)6]3+ - Yellow.
• Cr(III) - [Cr(H2O)6]3+ - Should be ruby, but we see green due to Cl¯ impurities. • Al(III) - [Al(H2O)6]3+ - Colourless (It's not a transition metal). |
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Metal-aqua ions form:
1) What solutions? 2) Why? 3) This is known as? |
1) Acidic solutions.
2) This is when the O-H bond in one of the water ligands is broken, releasing a H+. 3) These are known as acidity/hydrolysis reactions. |
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The acidic/hydrolysis reaction:
1) At equilibrium is? |
1) [M(H2O)6]^x + H2O → [M(H2O)6]^x + H3O+
(where x is either the +2/+3 charge). |
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The metal-aqua acidic solutions:
1) For 2+? 2) For 3+? 3) Explain the difference. |
1) Weakly acidic (around pH 6).
2) Strongly acidic (around pH 3). 3) The +3 has a larger size/charge ratio which causes it to have a much greater polarising effect than the 2+ ion. It strongly attracts the electron density from the Oxygen atom on the water ligand which weakens its O-H bond, making dissociation more likely to occur. |
