Chemistry: Transition Metals Part 2
This flashcard set covers the four common oxidation states of vanadium and the conditions under which they can be observed. It also links each oxidation state to its characteristic color, helping visualize vanadium’s redox behavior during reduction reactions.
How many common oxidationstates does vanadium have
4
Key Terms
How many common oxidationstates does vanadium have
4
When can the different oxidation states of vanadium be seen
When a solution of ammonium vanadate is reduced using zinc in acidic conditions
Common oxidation states of vanadium: what colour is VO2 + ion with ON +5
Yellow
Common oxidation states of vanadium: what colour is ion VO2+ with ON +4
Blue
Common oxidation states of vanadium: what colour is V3+ ion with ON +3
Green
Common oxidation states of vanadium: what colour is V2+ ion with ON +2
Violet
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| Term | Definition |
|---|---|
How many common oxidationstates does vanadium have | 4 |
When can the different oxidation states of vanadium be seen | When a solution of ammonium vanadate is reduced using zinc in acidic conditions |
Common oxidation states of vanadium: what colour is VO2 + ion with ON +5 | Yellow |
Common oxidation states of vanadium: what colour is ion VO2+ with ON +4 | Blue |
Common oxidation states of vanadium: what colour is V3+ ion with ON +3 | Green |
Common oxidation states of vanadium: what colour is V2+ ion with ON +2 | Violet |
Half equation reduction VO2 + to VO2+ | VO2 + 2H+ + e- > VO2+ + H2O |
Half equation oxidation of Zn | Zn > Zn2+ + 2e- |
Overall equation reduction of VO2 + to VO2+ by zinc in acidic conditions | 2VO2 + + 4H+ + Xn> 2VO2+ + 2H2O + Zn2+ |
Half equation for reduction of VO2+ to V3+ | VO2+ + 2H+ + e- > V3+ + H2O |
Half equation for oxidation of Zn | Zn > Zn2+ + 2e- |
Overall equation for reduction of VO2+ to V3+ in acidic conditions | 2VO2+ + 4H+ + Zn > 2V3+ + Zn2+ + 2H2O |
Half equation for reduction of V3+ to V2+ | V3+ + e- > V2+ |
Half equation for oxidation of Zn | Zn > Zn2+ + 2e- |
Overall equation for reduction of V3+ to V2+ by zinc in acidic conditions | 2V3+ + Zn > 2V2+ + Zn2+ |
Formula for tollens reagent | [Ag(NH3)2]+ |
What happens to an aldehyde when it’s warmed with tollens reagent | It’s oxidised to a carboxylic acid |
What happens to the silver ions when tollens is reacted with an aldehyde | Silver ions reduced to silver metal |
Equation for reduction of tollens reagent | [Ag(NH3)2]+ + e- > Ag + 2NH3 |
Why do ketones give no reaction in tollens test | Can’t be oxidised |
What is the redox potential of an ion/atom a measure of | How easily it is reduced to a lower oxidation state. |
Why does a more positive redox potential mean an ion is less stable | More likely to be reduced |
What is the redox potential the same as standard electrode potential providing | It is measured unde standard conditions in aqueous solution |
Why are the ligands surrounding the metal ion water in standard electrode potential | Standard electrode potentials are measured in aqueous solution |
Why will changing the ligand change the value of the redox potential | Other ligands will bond more or less strongly to central mental ion |
Half equation for reduction of dichromate in acidic conditions | Cr2O72- + 14H+ > 6e- > 2Cr3+ + 2H2O |
What effect would reducing pH of dichromate have on redox potential | Lower pH > higher [H+] > eqm RHS > more +ve redox potential |
Half Equation for reduction of manganate | MnO4- + 8H+ + 5e- > Mn2+ + 4H2O |