Metal Aqua Ions

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Last updated 4:54 PM on 4/26/26
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28 Terms

1
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Fe2+ colour in aqueous solution & compound

[Fe(H2O)6]2+(aq) pale green

2
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[Fe(H2O)6]2+(aq) + ammonia (excess and limited) colour change + compound

  • pale green solution → green ppt

  • [Fe(H2O)4(OH)2](s) formed

  • no observable change with excess

3
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[Fe(H2O)6]2+(aq) + NaOH (excess and limited) : colour change & compound

  • pale green solution → green ppt

  • [Fe(H2O)4(OH)2](s) formed

  • no observable change with excess

4
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[Fe(H2O)6]2+(aq) + sodium carbonate colour change & compound

  • pale green solution → green ppt

  • FeCO3(s) produced only no CO2

5
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why do you need to freshly prepare Fe2+?

it oxidises in air back to Fe3+

6
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Cu2+ colour in aqueous solution & compound

[Cu(H2O)6]2+(aq) blue

7
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[Cu(H2O)6]2+(aq) + NaOH (excess & limited) colour change & compound formed

  • [Cu(H2O)4(OH)2](s) formed

  • blue solution → pale blue precipitate

  • no observable change with excess

8
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[Cu(H2O)6]2+(aq) + limited NH3 colour change & compound formed

  • [Cu(H2O)4(OH)2](s) formed

  • blue solution → pale blue precipitate

9
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[Cu(H2O)6]2+(aq) + excess NH3

  • [Cu(H2O)2(NH3)4]2+ (aq) formed - partial ligand substitution

  • pale blue precipitate → deep blue solution

  • ppt dissolves because of ligand substitution

10
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[Cu(H2O)6]2+(aq) + sodium carbonate colour change + compound formed

  • CuCO3 (s) formed

  • blue solution → blue-green ppt only no CO2

11
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Fe3+ colour in solution & compound

[Fe(H2O)6]3+(aq) yellow

12
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[Fe(H2O)6]3+ (aq) + NaOH (excess & limited) colour change & compound

  • [Fe(H2O)3(OH)3] (s) formed

  • yellow solution → orange ppt.

  • no observable change with excess

13
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[Fe(H2O)6]3+(aq) + NH3 (excess & limited) colour change & compound

  • [Fe(H2O)3(OH)3] (s) formed

  • yellow solution → orange ppt.

  • no observable change with excess

14
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[Fe(H2O)6]3+(aq) + sodium carbonate colour & compound

  • [Fe(H2O)3(OH)3] (s) formed

  • yellow solution → brown ppt.

  • CO2 bubbles formed

15
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Al3+ colour in solution & compound

[Al(H2O)6]3+ (aq) colourless

16
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[Al(H2O)6]3+ (aq) + limited NaOH colour change & compound

  • [Al(H2O)3(OH)3] (s) formed

  • colourless solution → white ppt.

17
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[Al(H2O)6]3+ (aq) + NH3 (limited & excess) colour change & compound

  • [Al(H2O)3(OH)3] (s) formed

  • colourless solution → white ppt.

  • no observable change with excess

18
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[Al(H2O)6]3+ (aq) + excess NaOH colour change & compound

  • [Al(H2O)2(OH)4]-(aq) formed

  • white ppt → colourless solution

→ dissolves because it is amphoteric

19
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[Al(H2O)6]3+(aq) + sodium carbonate colour change & compound

  • [Al(H2O)3(OH)3] (s) formed

  • colourless solution → white ppt.

  • CO2 bubbles formed

20
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lewis acid definition

electron pair acceptor

21
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lewis base definition

electron pair donor

22
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Bronsted-Lowry acid definition

proton donor

23
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Bronsted-Lowry base definition

proton acceptor

24
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why are 3+ metal complexes more acidic than 2+?

  • 3+ complexes have a higher charge density & greater polarising power → more strongly attracts water

  • weakened O-H bond so it breaks more easily releasing H+ ions

25
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VO2+ colour & oxidation state

5+ yellow

26
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VO2+ colour & oxidation state

4+ blue

27
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V3+ colour & oxidation state

3+ green

28
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V2+ colour & oxidation state

2+ violet