Transition Metals Part 2 Flashcards

1
Q

How many common oxidationstates does vanadium have

A

4

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2
Q

When can the different oxidation states of vanadium be seen

A

When a solution of ammonium vanadate is reduced using zinc in acidic conditions

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3
Q

Common oxidation states of vanadium: what colour is VO2 + ion with ON +5

A

Yellow

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4
Q

Common oxidation states of vanadium: what colour is ion VO2+ with ON +4

A

Blue

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5
Q

Common oxidation states of vanadium: what colour is V3+ ion with ON +3

A

Green

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6
Q

Common oxidation states of vanadium: what colour is V2+ ion with ON +2

A

Violet

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7
Q

Half equation reduction VO2 + to VO2+

A

VO2 + 2H+ + e- > VO2+ + H2O

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8
Q

Half equation oxidation of Zn

A

Zn > Zn2+ + 2e-

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9
Q

Overall equation reduction of VO2 + to VO2+ by zinc in acidic conditions

A

2VO2 + + 4H+ + Xn> 2VO2+ + 2H2O + Zn2+

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10
Q

Half equation for reduction of VO2+ to V3+

A

VO2+ + 2H+ + e- > V3+ + H2O

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11
Q

Half equation for oxidation of Zn

A

Zn > Zn2+ + 2e-

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12
Q

Overall equation for reduction of VO2+ to V3+ in acidic conditions

A

2VO2+ + 4H+ + Zn > 2V3+ + Zn2+ + 2H2O

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13
Q

Half equation for reduction of V3+ to V2+

A

V3+ + e- > V2+

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14
Q

Half equation for oxidation of Zn

A

Zn > Zn2+ + 2e-

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15
Q

Overall equation for reduction of V3+ to V2+ by zinc in acidic conditions

A

2V3+ + Zn > 2V2+ + Zn2+

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16
Q

Formula for tollens reagent

A

[Ag(NH3)2]+

17
Q

What happens to an aldehyde when it’s warmed with tollens reagent

A

It’s oxidised to a carboxylic acid

18
Q

What happens to the silver ions when tollens is reacted with an aldehyde

A

Silver ions reduced to silver metal

19
Q

Equation for reduction of tollens reagent

A

[Ag(NH3)2]+ + e- > Ag + 2NH3

20
Q

Why do ketones give no reaction in tollens test

A

Can’t be oxidised

21
Q

What is the redox potential of an ion/atom a measure of

A

How easily it is reduced to a lower oxidation state.

22
Q

Why does a more positive redox potential mean an ion is less stable

A

More likely to be reduced

23
Q

What is the redox potential the same as standard electrode potential providing

A

It is measured unde standard conditions in aqueous solution

24
Q

Why are the ligands surrounding the metal ion water in standard electrode potential

A

Standard electrode potentials are measured in aqueous solution

25
Q

Why will changing the ligand change the value of the redox potential

A

Other ligands will bond more or less strongly to central mental ion

26
Q

Half equation for reduction of dichromate in acidic conditions

A

Cr2O72- + 14H+ > 6e- > 2Cr3+ + 2H2O

27
Q

What effect would reducing pH of dichromate have on redox potential

A

Lower pH > higher [H+] > eqm RHS > more +ve redox potential

28
Q

Half Equation for reduction of manganate

A

MnO4- + 8H+ + 5e- > Mn2+ + 4H2O