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2.06 Reactions Of Aqueous Ions > Reactions Of Inorganic Complexes > Flashcards

Reactions Of Inorganic Complexes Flashcards

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Organic Chemistry 101 flashcards
1
Q

Colour of [Cu(H2O)6]2+ as aqueous ion

A

Blue solution

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2
Q

Colour of [Co(H2O)6]2+

A

Pink

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3
Q

Colour of [Fe(H2O)6]2+

A

Green

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4
Q

Colour of [V(H2O)6]3+

A

Green

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5
Q

Colour of [V(H2O)6]2+

A

Violet

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6
Q

Colour of [Cr(H2O)6]3+

A

Violet

Usually appears as deep purple rather than violet in solution.
Note: Colour of Cr3+ is green in reactions due to substitution of other negative ions

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7
Q

Colour of [Fe(H2O)6]3+

A

Pale violet

Usually appear yellow/orange rather than violet in solution due to [Fe(H2O)5(OH)]2+ forming by hydrolysis

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8
Q

Colour of [Al(H2O)6]3+

A

Colour less

Aluminium is included but only one that isn’t a transition metal

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9
Q

Define hydrolysis

A

A reaction with a water molecule that breaks large molecules into smaller ones.

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10
Q

Why do hexaaqua complexes undergo hydrolysis

A

due to the polarising nature of the central transition metal ion.
The transition metal pulls electron density towards the metal, weakening the existing O-H bonds within the water ligands.

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11
Q

Give an equation to show the acid base reaction of
H3O+ and OH

A

H3O+ + OH- → 2H2O

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12
Q

Predict, and justify, how the addition of sodium hydroxide solution will effect the above equilibrium.

[Cu(H2O)6]2+(aq) + H2O(l) ⇌ [Cu(H2O)5(OH)]+(aq) + H3O+(aq)

A

The hydroxide ion will react with the hydroxonium ion, reducing the concentration of hydroxonium ion in the system. Equilibrium of the top reaction will shift to the right to increase the concentration of hydroxonium ion, opposing this change.

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13
Q

Give the overall equation for the reaction between hexaquacopper(II) solution and sodium hydroxide solution.

And colour

A

[Cu(H2O)6]2+(aq) + 2OH- → Cu(H2O)4(OH)2 + 2H2O(l)

Blue ppt

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14
Q

Give equations of [Fe(H2O)6]2+ + NaOH(aq) drop wise and in excess

Both colours

A

Dropwise: [Fe(H2O)6]2+ + 2OH- → Fe(H2O)4(OH)2 + 2H2O (hydrolysis)
Green ppt but goes brown on standing air

Excess: no further reaction but darkens in time on oxidation to [Fe(H2O)3(OH)3] (s)
No further change

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15
Q

Give equations for [Cu(H2O)6]2+ + NaOH(aq) drop wise and in excess

And colours

A

Dropwise: [Cu(H2O)6]2+ + 2OH- → [Cu(H2O)4(OH)2] + 2H2O (hydrolysis)
Blue ppt

Excess: no further reaction
No change

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16
Q

Give equations for [Fe(H2O)6]3+ + NaOH(aq) drop wise and in excess

A

Dropwise: [Fe(H2O)6]3+ + 3OH- → [Fe(H2O)3(OH)3] + 3H2O (hydrolysis)
Brown ppt

Excess: no further reaction
No change

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17
Q

Give equations for [Al(H2O)6]3+ + NaOH(aq) drop wise and in excess

A

Dropwise: [Al(H2O)6]3+ + 3OH- → [Al(H2O)3(OH)3] + 3H2O (hydrolysis)
Colourless

Excess: [Al(H2O)3(OH)3] + OH- → [Al(H2O)2(OH)4]- + H2O (hydrolysis)
White ppt

18
Q

General rules for aqua ions and OH-(aq)

A

• Dropwise – precipitate of neutral metal(II) hydroxide or metal(III) hydroxide forms
• Excess - [Al(H2O)3(OH)3] undergoes further hydrolysis to [Al(H2O)2(OH)4]- and so ‘re-dissolves’

19
Q

Amphoteric meaning

A

Characteristics of an acid and base

20
Q

[Fe(H2O)6]2+ + NH3(aq)
Dropwise and in excess

Colours

A

Dropwise: [Fe(H2O)6]2+ + 2NH3 → [Fe(H2O)4(OH)2] (s)+ 2NH4+ (hydrolysis)
Green pot and goes brown on standing air

Excess: no further reaction but darkens in time on oxidation to [Fe(H2O)3(OH)3]

21
Q

[Cu(H2O)6]2+ + NH3(aq)
Drop wise
In excess

And colour

A

Dropwise: [Cu(H2O)6]2+ + 2NH3 → [Cu(H2O)4(OH)2] (s)+ 2NH4+ (hydrolysis)
Blue ppt

Excess: [Cu(H2O)4(OH)2] + 4NH3 → [Cu(H2O)2(NH3)4]2+ + 2H2O + 2OH- (substitution
Deep blue solution

22
Q

[Fe(H2O)6]3+ + NH3(aq)
Dropwise
In excess
Colours

A

Dropwise: [Fe(H2O)6]3+ + 3NH3 → [Fe(H2O)3(OH)3] (s)+ 3NH4+ (hydrolysis)
Brown ppt
Excess: no further reaction

23
Q

[Al(H2O)6]3+ + NH3(aq)
Drop wise
In excess

A

Dropwise: [Al(H2O)6]3+ + 3NH3 → [Al(H2O)3(OH)3] (s)+ 3NH4+ (hydrolysis)
White ppt
Excess: no further reaction

24
Q

General rules for metal aqua ions and NH3(aq)

A

• Dropwise – precipitate of metal(II) hydroxide or metal(III) hydroxide forms
• Excess – [Cu(H2O)4(OH)2] undergoes ligand substitution to give [Cu(H2O)2(NH3)4]2+

25
Q

[Fe(H2O)6]2+ + CO32-(aq)
Colour

A

[Fe(H2O)6]2+ + CO32- → FeCO3 (s)+ 6H2O (precipitation)
Green ppt

26
Q

[Cu(H2O)6]2+ + CO32-(aq)
Colour

A

[Cu(H2O)6]2+ + CO32- → CuCO3 (s)+ 6H2O (precipitation)
Blue - green ppt

27
Q

[Fe(H2O)6]3+ + CO32-(aq)

A

2 [Fe(H2O)6]3+ + 3CO32- → 2[Fe(H2O)3(OH)3] (s)+ 3H2O + 3CO2 (hydrolysis)

brown ppt
(ppt may look orange-brown)
and CO2 gas evolved

28
Q

[Al(H2O)6]3+ + CO32-(aq)
Colour

A

2[Al(H2O)6]3+ + 3CO32- → 2[Al(H2O)3(OH)3] (s)+ 3H2O + 3CO2 (hydrolysis)

white ppt
and CO2 gas evolved

29
Q

General rules of metal aqua ions + CO3^2-(aq)

A

• [M(H2O)6]2+ forms MCO3 as precipitate (it is not acidic enough to release CO2 from Na2CO3)
• [M(H2O)6]3+ is more acidic and undergoes hydrolysis to form [M(H2O)3(OH)3] as a precipitate and gentle fizzing as CO2 is formed

30
Q

Colour of [Cu(H2O)6]2+ with NaOH

A

Blue ppt

31
Q

You
Better
Get
Vanadium

A

Yellow [VO2(H2O)4]+
Blue [VO(H2O)5]2+
Green [V(H2O)6]3+
Violet [V(H2O)6]2+

32
Q

[V(H2O)6]2+ oxidation state

A

V(II)

33
Q

[V(H2O)6]3+ oxidation state

A

V(III)

34
Q

VO(H2O)5]2+ oxidation state

A

V(IV)

35
Q

[VO2(H2O)4]+ oxidation state

A

V(V)

36
Q

[Co(H2O)6]2+ + NH3(aq)
Dropwise
In excess
Overall
And colour change

A

Dropwise: [Co(H2O)6]2+ + 2NH3 → [Co(H2O)4(OH)2] + 2NH4+ (hydrolysis) pink to blue ppt
Excess: [Co(H2O)4(OH)2] + 6NH3 → [Co(NH3)6]2+ + 4H2O + 2OH- (substitution) blue to pale brown
Overall: [Co(H2O)6]2+ + 6NH3 → [Co(NH3)6]2+ + 6H2O (substitution) pink to pale brown

37
Q

[Cu(H2O)6]2+ + NH3(aq)
Dropwise and in excess
Overall

A

Dropwise: [Cu(H2O)6]2+ + 2NH3 → [Cu(H2O)4(OH)2] + 2NH4+ (hydrolysis) blue to blue ppt
Excess: [Cu(H2O)4(OH)2] + 4NH3 → [Cu(H2O)2(NH3)4]2+ + 2H2O + 2OH- (substitution) deep blue solution
Overall: [Cu(H2O)6]2+ + 4NH3 → [Cu(H2O)2(NH3)4]2+ + 4H2O (substitution)

38
Q

How many Cl- fit around M^n+

A

4

39
Q

[Co(H2O)6]2+ + conc HCl

A

[Co(H2O)6]2+ + 4Cl- → [CoCl4]2- + 6H2O (substitution)
Pink to blue

40
Q

[Cu(H2O)6]2+ + conc HCl

A

[Cu(H2O)6]2+ + 4Cl- → [CuCl4]2- + 6H2O (substitution)

Blue to green

2.06 Reactions Of Aqueous Ions (1 decks)

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