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Chemistry > Reactions Of Ipns In Solutipn > Flashcards

Reactions Of Ipns In Solutipn Flashcards

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1
Q

What do most metal actions exist as in aqueous solution

A

The hexaaqua complex ion

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2
Q

What kind of ions do main group metals form

A

Colourless

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3
Q

What are most transition metal ions

A

Coloured

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4
Q

Why are lost transition metal ions coloured

A

-incomplete d sub shell
-some wavelengths of vidible light absorbed
-d electrons ground state to excited state -
Remaining colours of visible light transmitted

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5
Q

Copper 2 hexaaqua ion colour

A

Blue

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6
Q

Iron 3 hexaaqua ion colour

A

Purple

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7
Q

Aluminium 3 hexaaqua ion colour

A

Colourless

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8
Q

What is there a hydrolysis reaction beteeen in solution

A

Metal aqua ion and water

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9
Q

What does the charge on the metal job cause the electron density in the water ligand to do

A

Move closer to metal ion- water ligand polarised

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10
Q

What happens if the metal ion had enough polarising power

A

Bonds in water weakened

One of bonds breaks and proton donated to water molecule

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11
Q

What is relationship between pKa and strength of acidity of hexaaqua ion

A

Lower pka- stronger acid- equilibrium lies further to right

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12
Q

What is the difference in acidity due to in iron 2 and iron 3

A

Charge/size ratios

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13
Q

Why is iron 3 more acidic than iron 2

A

Smaller and more highly charged and therefore able to polarise water ligands more

OH bonds in water weakened more readily and protons more easily donated

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14
Q

Equations for al3+ hexaaqua with water

A

[Al(H2O)6]3+ + H2O > [Al(H2O)5(OH)]2+ + H3O+

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15
Q

Why will al3 hexaaqua be more acidic than copper 2 hexaaqua

A

Al3 ions smaller and more highly charged therefore able to polarise water ligands more, weaken OH bonds therefore donate H+ ions more readily

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16
Q

What does adding a base to an aqueous solution of the metal aqua ion produce

A

Insoluble precipitates of the metal hydroxide

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17
Q

Equation for adding hydroxide to metal aqua ion

A

[M(H2O)6]3+ + OH- > [M(H2O)5(OH)]2+ + H2O

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18
Q

What happens to the equilibrium if you add more OH- ions to metal aqua ion

A

Equilibrium shifts to the right to oppose the increase in [OH-] and a new equilibrium set up

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19
Q

Equation for new equilibrium set up after adding more OH- ions to metal aqua ion

A

[M(H2O)5(OH)]2+ + OH- > [M(H2O)4(OH)2]+ + H2O

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20
Q

What happens to the equivlirum if you add FURTHER OH- ions to the metal aqua ion

A

Equilibrium shift to the right to oppose increase in [OH-] and final equilibrium set up

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21
Q

Equation for final equilibrium set up after adding further OH- ions to metal aqua ions

A

[M(H2O)4(OH)2] + OH- > [M(H2O)3(OH)3] + H2O

22
Q

Why does [M(H2O)3(OH)3] precipitate out

A

It’s neutral and insoluble

23
Q

Overall equation metal aqua ion and hydroxide

A

[M(H2O)6]3+ + 3OH- > [M(H2O)3(OH)3] + 3H2O

24
Q

Iron 2 hexaaqua ion colour

A

Green

25
Q

Colour of PPT iron 2 and NAOH

A

Brown

26
Q

How can reaction between iron 2 hexaaqua and sodium hydroxide be reversed

A

Adding acid

27
Q

What colour ppt does Al3+ hexaaqua form with hydroxide

A

White

28
Q

Equation for aluminium hydroxide acting as a base

A

[Al(H2O)3(OH)3] + 3H+ > [Al(H2O)6]3+

29
Q

Equation for aluminium hydroxide acting as an acid

A

[Al(H2O)3(OH)3] + OH- > [Al(H2O)2(OH)4]- + H2O

30
Q

What does the white ppt of aluminium hydroxide dissolve to form

A

A colourless solution

31
Q

Overall equation for metal hexaaqua ion with NAOH

A

[M(H2O)6]2+ + 2OH- > [M(H2O)4(OH)2] + 2H2O

32
Q

What colour ppt is formed from reaction of iron 2 hexaaqua and NAOH

A

Green/grey

33
Q

Why does green/green iron 2 PPT turn green when left to stand in air

A

Oxidation to iron 3 hydroxide

34
Q

Equation for reaction of iron 2 oxide to iron 3 oxide

A

[Fe(H2O)4(OH)2] > [Fe(H2O)3(OH)3] + H+ + e-

35
Q

What colour ppt does copper 2 hexaaqua form with sodium hydroxide

A

Blue

36
Q

Why is ammonia able to react with metal aqua ions to produce metal hydroxides

A

It’s a weak base

37
Q

Reaction of iron 3 hexaaqua with aqueousammonia

A

[Fe(H2O)6]3+ + 3NH3 > [Fe(H2O)3(OH)3] + 3NH4+

Brown ppt

38
Q

Reaction of aluminium 3 hexaaqua with aqueous ammonia

A

[Al(H2O)6]3+ + 3NH3 > [Al(H2O)3(OH)3] + 3NH4+

White ppt

39
Q

Why can’t ammonia hydrolyse aluminium hydroxide further

A

It’s a weak base

40
Q

Reaction of iron 2 hexaaqua with aqueous ammonia

A

[Fe(H2O)6]2+ + 2NH3 > [Fe(H2O)4(OH)2] + 2NH4+

Green grey ppt

41
Q

Reaction of copper 2 aqueous ammonia

A

[Cu(H2O)6]2+ + 2NH3 > [Cu(H2O)4(OH)2] + 2NH4+

Blue ppt

42
Q

What can be formed by a ligand substitution reaction when an excess of ammonia is added to the copper 2 hydroxide precipitate

A

A new complex

43
Q

Equation for copper 2 hydroxide and excess ammonia

A

[Cu(H2O)4(OH)2] + 4NH3 > [Cu(H2O)2(NH3)4 2+ + 2H2O + 2OH-

Deep blue soln

44
Q

Overall reaction between hexaaqua copper II ion and excess ammonia

A

[Cu(H2O)6]2+ + 4NH3 > [Cu(NH3)4(H2O)2]2+ + 2H2O

45
Q

What do 2+ metal ions react with sodium carbonate to form

A

Insoluble metal carbonates

46
Q

Reaction of copper 2 hexaaqua with sodium carbonate

A

[Cu(H2O)6]2+ + CO32- > CuCO3 + 6H2O

Blue soln to blue green ppt

47
Q

Reaction iron 2 hexaaqua and aqueous sodium carbonate

A

[Fe(H2O)6]2+ + CO32- > FeCO3 + 6H2O

Green soln to green grey ppt

48
Q

Why do 3+ metal ions form the hydroxide and release carbon dioxide gas when reacting with sodium carbonate

A

They’re stronger acids

49
Q

Reaction iron 3 with sodium carbonate

A

2[Fe(H2O)6]3+ + 3CO32- > 2Fe(H2O)3(OH)3] + 3CO2 + 3H2O

Orange soln to brown ppt

50
Q

Equation aluminium 3 with sodium carbonate

A

2[Al(H2O)6]3+ + 3CO32- > 2[Al(H2O)3(OH)3] + 3CO2 + 3H2O

Colourless soln

Fizz

Chemistry (42 decks)

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