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Chemistry: Transition Metals Part 2

Chemistry28 CardsCreated 2 months ago

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

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Key Terms

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

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TermDefinition

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