Transition metals Flashcards
Fe 2+ in aqueous solution
[Fe(H2O)6]2+ green solution
Cu 2+ in aqueous solution
[Cu(H2O)6]2+ blue solution
Fe 3+ in aqueous solution
[Fe(H2O)6]3+. pale violet solution but appears orange due to hydrolysis to some [Fe(H2O)5(OH)]2+
Al 3+ in aqueous solution
[Al(H2O)6]3+ colourless solution
Add aqueous NaOH dropwise to Fe2+
[Fe(H2O)4(OH)2] green precipitate (darkens on standing due to oxidation to [Fe(H2O)3(OH)3]
Add aqueous NaOH dropwise to Cu 2+
[Cu(H2O)4(OH)2] blue precipitate
Add aqueous NaOH dropwise to Fe3+
[Fe(H2O)3(OH)3] brown precipitate
Add aqueous NaOH dropwise to Al3+
[Al(H2O)3(OH)3] white precipitate
addition of excess aqueous NaOH to Fe2+
no further reaction form when was added dropwise
addition of excess aqueous NaOH to Cu2+
no further reaction form when was added dropwise
addition of excess aqueous NaOH to Fe3+
no further reaction form when was added dropwise
addition of excess aqueous NaOH to Al3+
[Al(H2O)2(OH)4]- re-dissolved to give colourless solution
adding aqueous NH3 dropwise to Fe2+
[Fe(H2O)4(OH)2] green precipitate which darkens on standing due to oxidation causing [Fe(H2O)3(OH)3]
adding aqueous NH3 dropwise to Cu2+
[Cu(H2O)4(OH)2] blue precipitate
adding aqueous NH3 dropwise to Fe3+
[Fe(H2O)3(OH)3] brown precipitate
adding aqueous NH3 dropwise to Al3+
[Al(H2O)3(OH)3] white precipitate
Adding excess aqueous NH3 to Fe2+
no further reaction form when it was added dropwise
Adding excess aqueous NH3 to Cu2+
[Cu(H2O)2(NH3)4]2+ deep blue solution
Adding excess aqueous NH3 to Fe3+
no further reaction form when it was added dropwise
Adding excess aqueous NH3 to Al3+
no further reaction form when it was added dropwise
adding aqueous Na2CO3 to Fe2+
FeCO3 green precipitate
adding aqueous Na2CO3 to Cu2+
CuCO3 blue-green precipitate
adding aqueous Na2CO3 to Fe3+
[Fe(H2O)3(OH)3] brown precipitate and bubbles of CO2 gas
adding aqueous Na2CO3 to Al3+
[Al(H2O)3(OH)3] white precipitate and bubbles of CO2 gas
adding concentrated HCl to Fe2+
[FeCl4]2- yellow solution
adding concentrated HCl to Cu2+
[CuCl4]2-green solution
adding concentrated HCl to Fe3+
[FeCl4]-yellow solution
adding concentrated HCl to Al3+
[AlCl4]- colourless solution
reaction between iodide ions and S2O8 2- catalysed by Fe
S2O8 2- + 2e- –> 2 SO4 2-
Fe3+ + e- –> Fe2+
I2 + 2e- –> 2 I-
all arrows are reversible
reactions can occur either way round which is why Fe2+ or Fe3+ can be the catalyst
overall:
2 I- + S2O8 2- –> I2 + 2 SO4 2-
contact process
-catalysed by V2O5
V2O5 + SO2 –> V2O4 + SO3
V2O4 = 0.5O2 –> V2O5
overall:
2 SO2 + O2 –> 2 SO3
colours of vanadium ions oxidation state = +5
VO2 + yellow
colours of vanadium ions oxidation state = +4
VO 2+ blue
colours of vanadium ions oxidation state = 3+
V 3+ green
colours of vanadium ions oxidation state = 2+
V 2+ violet
haber process
3 H2 + N2 –> 2 NH3
reversible reaction arrow
reaction of ethanedioate ions and manganate ions
2 MnO4- + 16H+ + 5C2O42- –> 2 Mn2+ + 8 H20 + 10 CO2
catalysed by Mn2+ ions
reaction of manganate ions and iron ions
MnO4- + 8 H+ + 5 Fe 2+ –> Mn2+ + 4 H2O + 5 Fe 3+