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chemistry > Reactions of Transition Metal Ions in Solution > Flashcards

Reactions of Transition Metal Ions in Solution Flashcards

1
Q

Iron(II) Aqueous ion

A

[Fe(H2O)6]2+(aq)
green solution

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2
Q

Iron(II) Action of NaOH

A

Fe(H2O)4(OH)2(s)
green ppt goes brown on standing in air

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3
Q

Iron(II) Action of an excess of
NaOH(aq)

A

No further change

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4
Q

Iron(II) Action of NH3(aq)

A

Fe(H2O)4(OH)2(s)
green ppt goes brown
on standing in air

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5
Q

Iron(II) Action of an excess
of NH3(aq)

A

No further change

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6
Q

Iron(II) Action of Na2CO3(aq)

A

FeCO3(s)
green ppt

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7
Q

Copper(II) Aqueous ion

A

[Cu(H2O)6]2+(aq)
blue solution

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8
Q

Copper(II) Action of NaOH

A

Cu(H2O)4(OH)2(s)
blue ppt

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9
Q

Copper(II) Action of an excess of NaOH(aq)

A

No further change

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10
Q

Copper(II) Action of NH3(aq)

A

Cu(H2O)4(OH)2(s)
blue ppt

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11
Q

Copper(II) Action of an excess of NH3(aq)

A

[Cu(H2O)2(NH3)4]2+(aq)
deep blue solution

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12
Q

Copper(II) Action of
Na2CO3(aq)

A

CuCO3(s)
blue-green ppt

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13
Q

Iron(III) Aqueous ion

A

[Fe(H2O)6]3+(aq)
purple solution may look yellow-brown due to some [Fe(H2O)5(OH)]2+(aq)

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14
Q

Iron(III) Action of NaOH

A

Fe(H2O)3(OH)3(s)
brown ppt
(ppt may look orange-brown)

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15
Q

Iron(III) Action of an excess of NaOH(aq)

A

No further change

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16
Q

Iron(III) Action of NH3(aq)

A

Fe(H2O)3(OH)3(s)
brown ppt
(ppt may look orangebrown)

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17
Q

Iron(III) Action of an excess of NH3(aq)

A

No further change

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18
Q

Iron(III) Action of Na2CO3(aq)

A

Fe(H2O)3(OH)3(s)
brown ppt
(ppt may look orange-brown)
and CO2 gas evolved

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19
Q

Aluminium(III) Aqueous ion

A

[Al(H2O)6]3+(aq)
colourless solution

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20
Q

Aluminium(III) Action of NaOH

A

Al(H2O)3(OH)3(s)
white ppt

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21
Q

Aluminium(III) Action of an
excess of NaOH(aq)

A

[Al(OH)4]–(aq)
colourless solution

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22
Q

Aluminium(III) Action of NH3(aq)

A

Al(H2O)3(OH)3(s)
white ppt

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23
Q

Aluminium(III) Action of an excess of NH3(aq)

A

No further change

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24
Q

Aluminium(III) Action of
Na2CO3(aq)

A

Al(H2O)3(OH)3(s)
white ppt and CO2 gas evolved

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25
Q

V(V) Species in acidic solution and colour of solution

A

[VO2(H2O)4]+
yellow

26
Q

V(IV) Species in acidic solution and colour of solution

A

[VO(H2O)5]2+
blue

27
Q

V(III) Species in acidic solution and colour of solution

A

[V(H2O)6]3+
green

28
Q

V(II) Species in acidic solution and colour of solution

A

[V(H2O)6]2+
purple

29
Q

what are transition metals and its properties

A

metals that form one or more stable ions with a partially filled d subshell
-form complexes
-form coloured ions
-have variable oxidation states
-are good catalysts

30
Q

what is a complex

A

central metal atom or ion surrounded by ligands

31
Q

what is a ligand

A

molecule or ion that joins to a central transition metal atom or ion via a co ordinate bond by donating a pair of electrons

32
Q

what is a coordintation number

A

the number of coordinate bonds to the central metal atom or ion

33
Q

monodentate, bidentate, polydentate ligand

A

mono- ligand donates one pair
poly- 2 or more pairs
bi- 2 pairs

34
Q

examples of monodentate ligands

A

Cl-, CN-
NH3 and H2O

35
Q

examples of bidentate ligands

A

C2O4^2-
NH2CH2CH2NH2

36
Q

example of a hexadentate ligand

A

EDTA^4-

37
Q

what is coordination number affected by

A

-size of metal ion and ligands
-electronic configuration of metal ion

38
Q

why do transition metal ions appear coloured

A

they absorb certain frequencies of light causing electrons in d sub-shell to become excited
the colour observed is the light not absorbed/the light transmitted

39
Q

what factors affect the size of the energy gap between d block compounds

A

-transition metal ion
-oxidation state
-ligands
-shape

40
Q

how to calculate energy difference

A

energy= planck x frequency
velocity of light= wavelength x frequency
therefore, energy= (planck x velocity) / wavelength

41
Q

how to find conc of unknown solution

A

-make up standard solutions of coloured compounds
-choose suitable filter
-zero the colorimeter with tube of pure solvent
-measure absorbance of standard solutions and plot calibration curve
-measure absorbance of unknown solution and read off conc from calibration curve

42
Q

redox of MnO4^-, Fe^2+ and C2O4^2-

A

MnO4^- –> Mn^2+
Fe^2+ –> Fe^3+
C2O4^2- –> CO2

43
Q

what is a homogenous catalyst

A

-catalyst in the same phase as the reactants
-forms an intermediate compound
-intermediate breaks down to form product and catalyst reforms

44
Q

show how Fe2+ acts as a catalyst for S2O8^2- to SO4^2-

A

slow reaction because negative ions repel
S2O8^2- + 2Fe^2+ –> 2SO4^2- + 2Fe^3+ (intermediate)

2Fe^3+ + 2I- –> I2 + 2Fe2+

45
Q

what is a heterogenous catalyst and how does it work

A

catalyst in a different phase from the reactants
-reactants adsorb onto surface of catalyst
-the bonds in the reactant are weakened
-products desorb from catalyst surface

46
Q

what is catalyst poisoning

A

-if the bonds are too strong, the products may remain fixed to the catalyst
-active sites blocked

47
Q

what are the stages of the contact process used to make sulfuric acid

A

S + O2 –> SO2
2SO2 + O2 <–> 2SO3
SO3 + H2O –> H2SO4

48
Q

what are the equations for the contact process with a vanadium oxide catalyst

A

V2O5 + SO2 –> V2O4 + SO3
2V2O4 + O2 –> 2V2O5

49
Q

what does the graph for autocatalysis look like

A

-starts slowly as not much catalyst product has formed
-slope increases as catalyst forms
-slope decreases as reactants are being used up

50
Q

why are aqua ions with a 3+ charge more acidic than those with a 2+ charge

A

3+ ions have a higher charge density so the OH bond is weakened
tendency to donate a H+ ions increases making the solution acidic

51
Q

overall equation of reacting [M(H2O)6]3+ with XS OH-

A

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

52
Q

overall equation of reacting [M(H2O)6]2+ with XS OH-

A

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

53
Q

[M(H2O)6]3+ with NH3

A

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

54
Q

[M(H2O)6]2+ with NH3

A

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

55
Q

reaction of Cu(H2O)4(OH)2 with XS NH3

A

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

56
Q

[M(H2O)6]3+ with CO3^2-

A

2[M(H2O)6]3+ + 3CO3^2- –> 2M(H2O)3(OH)3 + 3CO2 + 3H2O

57
Q

[M(H2O)6]2+ with CO3^2-

A

[M(H2O)6]2+ + CO3^2- –> MCO3 + 6H2O

58
Q

reactions of Al(H2O)3(OH)3 with acid and base

A

Al(H2O)3(OH)3 + H+ –> [Al(H2O)6]3+
Al(H2O)3(OH)3 + OH- –> [Al(OH)4]- + 3H2O

59
Q

[M(H2O)6]2+ with H2O

A

[M(H2O)6]3+ + H2O –>
[M(OH)(H2O)5]+ + H3O+

60
Q

[M(H2O)6]3+ + H2O

A

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

chemistry (15 decks)

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