Transition Metals

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oxidation states of vanadium
+5, +4, +3, +2
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Oxidation State: +5. Ion:
[VO2]+
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Oxidation State: +4. Ion:
[VO]2+
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Oxidation State: +3. Ion:
[V]3+
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Oxidation State: +2. Ion:
[V]2+
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Colour of [VO2]+
Yellow
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Colour of [VO]2+
Blue
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Colour of [V]3+
Green
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Colour of [V]2+
Violet
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Most common oxidation state of Silver
Ag+ (+1)
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Reduction of Ag+
Ag+ + e- --> Ag
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Tollens reagent
[Ag(NH3)2]+
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Tollens and aldehyde reaction
RCHO + 2[Ag(NH3)2]+ + 3OH- --> RCOO- + 2Ag + 4NH3 + 2H2O
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Titration of Fe2+ and MnO4- equation
MnO4- + 8H+ + 5Fe2+ --> Mn2+ + 4H2O + 5Fe3+
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Titration of [C2O4]2- and MnO4- equation
2MnO4- + 16H+ + 5(C2O4)2- ----> 2Mn2+ + 8H2O + 10CO2
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[Cu(H2O)6]2+ (blue solution) with OH- or NH3
Cu(H2O)4(OH)2, a blue ppt is formed
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[Cu(H2O)6]2+ (blue solution) with excess OH-
no change
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[Cu(H2O)6]2+ (blue solution) with excess NH3
[Cu(NH3)4(H2O)2]2+, a deep blue solution, is formed
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[Cu(H2O)6]2+ (blue solution) with Na2CO3
a green blue ppt formed -- CuCO3
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[Fe(H2O)6]2+ (green solution) with OH- or NH3
Fe(OH)2(H2O4), a green ppt formed
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[Fe(H2O)6]2+ (green solution) with excess OH-
no change
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[Fe(H2O)6]2+ (green solution) with excess NH3
no change
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[Fe(H2O)6]2+ (green solution) with Na2CO3
FeCO3, a green ppt is formed
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[Al(H2O)6]3+ (colourless solution) with OH- / NH3
Al(OH)3(H2O)3 white ppt formed
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[Al(H2O)6]3+ (colourless solution) with excess OH-
[Al(OH)4(H2O)2]- colourless solution formed
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[Al(H2O)6]3+ (colourless solution) with excess NH3
no change
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[Al(H2O)6]3+ (colourless solution) with Na2CO3
Al(OH)3(H2O)3 white ppt formed and bubbles
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[Fe(H2O)6]3+ (yellow solution) with excess OH-/NH3
Fe(OH)3(H2O)3 brown ppt formed
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[Fe(H2O)6]3+ (yellow solution) with excess OH-
no change
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[Fe(H2O)6]3+ (yellow solution) with excess NH3
no change
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[Fe(H2O)6]3+ (yellow solution) with Na2CO3
Fe(OH)3(H2O)3 brown ppt and bubbles
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How do we get Vanadium to its various ox states?
Vanadium in oxidation states: 4,3,2 are formed by the reduction of +5 ions by zinc in acidic solution
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redox potential changing from a higher to lower ox state is influenced by...
pH and ligand
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redox potent. will be more ______ in more acidic solutions
positive because the ion is more easily reduced
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Other cards in this set

Card 2

Front

Oxidation State: +5. Ion:

Back

[VO2]+

Card 3

Front

Oxidation State: +4. Ion:

Back

Preview of the front of card 3

Card 4

Front

Oxidation State: +3. Ion:

Back

Preview of the front of card 4

Card 5

Front

Oxidation State: +2. Ion:

Back

Preview of the front of card 5
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