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Inorganic - Transition Metals Flashcards

1
Q

What is a transition metal?

A

An element that has an incomplete d subshell in either its atoms or one of its common ions

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2
Q

What is a ligand?

A

Particle with a lone pair that forms co-ordinate bond to metal ion by donating a pair of electrons.

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3
Q

What is a complex?

A

Metal ion with ligands coordinately bonded to it

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4
Q

What is the coordinate number?

A

Number of coordinate bonds from ligand(s) to metal ions or atoms

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5
Q

What is a Lewis base?

A

Lone pair donor (ligands are Lewis bases)

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6
Q

What is a Lewis acid?

A

Lone pair acceptor

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7
Q

What are the 5 examples of ligands?

A

1) :NH3 = neutral
2) :Cl- = negative
3) H2O: = neutral
4) :OH- = negative
5) :CN- = negative

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8
Q

What are the rules when writing electronic configuration?

A

1) 4s fills before 3d
2) 4s also empties before 3d

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9
Q

What are the two exceptions when writing electronic configuration?

A

Cr is [Ar]4s^1 3d^5
Cu is [Ar]4s^1 3d^10

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10
Q

Why is Zn not actually a transition metal?

A

It does not have an incomplete d subshell.

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11
Q

What are the four properties of transition metals?

A

1) They form coloured ions.
2) They form complexes (ligands form co-ordinate bonds to the metal ion).
3) They exhibit variable oxidation states.
4) They show catalytic activity:
- Ni -> margarine
- V2O5 -> making SO3 for H2SO4
- Fe -> Haber process to make NH3
- Pt, Pd -> catalytic converters

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12
Q

What is a monodentate ligand?

A

Particle with a lone pair that forms one coordinate bond to metal ion by donating a pair of electrons

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13
Q

What is an example of a monodentate ligand?

A

H2O, NH3 and Cl-

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14
Q

What is a bidentate ligand?

A

Particle with a lone pair that forms two coordinate bonds to the metal ion by donating two pairs of electrons

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15
Q

What is an example of a bidentate ligand?

A

H2NCH2NH2 and C2O4(2-)

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16
Q

What is a multidentate ligand?

A

Particle with lone pair that forms several coordinate bonds to the metal ion by donating several pair of electrons

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17
Q

What is an example of a multidentate ligand?

A

EDTA(4-)

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18
Q

What is an example of a complex with a multidentate ligand?

A

Haem is an iron (II) complex with a multidentate ligand. Oxygen forms a coordinate bond to Fe(II) in haemoglobin, enabling oxygen to be transported in the blood.

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19
Q

How is carbon monoxide toxic?

A

Carbon monoxide is toxic because it replaces oxygen coordinately bonded to Fe(II) in haemoglobin

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20
Q

What is ligand substitution?

A

A reaction where one ligand is replaces by another ligand

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21
Q

What is the Chelate effect?

A

The replacement of monodentate ligands with bidentate and multidentate ligands in complex ions. Entropy changes are always positive in chelation because the reactions produce a net increase in the number of particles. A small enthalpy change and relative large positive entropy change generally ensures that the overall free energy change is negative.

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22
Q

What is the co-ordination number of a linear ion?

A

Coordinate number = 2

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23
Q

What is the co-ordination number of a tetrahedral ion?

A

Coordinate number = 4

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24
Q

What is the co-ordination number of a square planar ion?

A

Coordinate number = 4

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25
What is the co-ordination number of an octahedral ion?
Coordinate number = 6
26
What is the bond angle of a linear ion?
180 degrees
27
What is the bond angle of a tetrahedral ion?
109.5 degrees
28
What is the bond angle of a square planar ion?
90 degrees
29
What is the bond angle of an octahedral ion?
90 degrees
30
What is the occurance of a linear ion?
Ag+ complexes
31
What is the occurance of a tetradhedral ion?
Large ligands e.g. Cl-
32
What is the occurance of a sqaure planar ion?
Pt2+ complexes
33
What is the occurance of an octahedral ion?
Commonest
34
What is an example of a linear ion?
[Ag(NH3)2]+
35
What is an example of a tetrahedral ion?
[CuCl4]2-
36
What is an example of a square planar ion?
[PtCl4]2-
37
What is an example of an octahedral ion?
[Cu(H2O)6]2+
38
What is a stereoisomer?
Same formula but different 3D arrangement of atoms in space
39
What are the two types of stereoisomerism?
1) E-Z Isomerism 2) Optical Isomerism
40
What is an optical isomer?
Non-superimposable mirror images of eachother
41
What is cis-platin?
- Very effective drug in chemotherapy - Binds to guanine in DNA and stops replication - cis isomer (Z)
42
What are some examples of molecules that show E-Z isomerism?
[PtCl2(NH3)2] [CoCl2(NH3)4]+
43
How is the colour of a transition metal ion formed?
When visible light hits a transition metal ion, some frequencies are absorbed when electrons jump up to the higher orbitals. The frequences absorbed depends on the size of the energy gap. The rest of the frequencies are transmitted or reflected, these frequencies combine to form the complement of the colour of the absorbed frequencies (the colour you see)
44
What is an example of coloured ions?
Hydrated [Cu(H2O)6]2+ ions absorb light from the red end of the spectrum. The remaining frequencies combine to produce the complementary colour blue, so the [Cu(H2O)6]2+ ion appears blue.
45
What is the colour of an ion affected by?
The size of the energy gap between the d-orbitals and so the colour is affacted by changes in: 1) The metal ion 2) The oxidation state 3) The ligands present 4) The coordination number
46
How can the energy absorbed when electrons jump up from the ground state to an excited state be worked out?
Using the formula: ΔE = hc/λ v=frequency of light absorbed (Hz) h=Planck's constant (6.63 x 10^-34 Js) c=speed of light (3.00 x 10^8 m/s) λ=wavelength of light absorbed (m)
47
How can the concentration of coloured ion be found?
Spectroscopy can be used to determine the concentration of a solution by measuring how much light it absorbs. The more concentrated a coloured solution is, the more light it will absorb.
48
How can a calibartion curve for measuring the concentration of ions be produced?
You can produce a calibration curve by measuring the absorbanceof known concentrations of solutions and plotting the results on a graph.
49
What is the oxidation state of the Dioxovanadium (V) Ion?
+5
50
What is the formula of the Dioxovanadium (V) Ion?
VO2(+)
51
What is the colour of the Dioxovanadium (V) Ion?
Yellow
52
What is the oxidation state of the Vanadate (V) Ion?
+5
53
What is the formula of the Vanadate (V) Ion?
VO3(-)
54
What is the colour of the Vanadate (V) Ion?
Yellow
55
What is the oxidation state of the Oxovanadium (IV) Ion?
+4
56
What is the formula of the Oxovanadium (IV) Ion?
VO(2+)
57
What is the colour of the Oxovanadium (IV) Ion?
Blue
58
What is the oxidation state of the Vanadium (III) Ion?
+3
59
What is the formula of the Vanadium (III) Ion?
V(3+)
60
What is the colour of the Vanadium (III) Ion?
Green
61
What is the oxidation state of the Vanadium (II) Ion?
+2
62
What is the formula of the Vanadium (II) Ion?
V(2+)
63
What is the colour of the Vanadium (II) Ion?
Violet
64
What metal is used to reduce vanadium?
Zinc (Zn)
65
What are the equations for the reduction of VO2(+) to V(2+)?
2VO2(+) + Zn +4H+ -> 2VO(2+) + Zn(2+) + 2H2O 2VO(2+) + Zn + 4H+ -> 2V(3+) + Zn(2+) + 2H2O 2V(3+) + Zn -> 2V(2+) + Zn(2+)
66
What is redox potential?
The redox potential of an ion or atoms tells you how easily it is reduced to a lower oxidation state (same as electrode potentials). The larger the redox potential, the less stable the ion will be and so the more likely it is to be reduced.
67
What is the redox potential of a transition metal infleunced by?
The redox potential for a transition metal ion changing from a higher to a lower oxidation state is influenced by pH and by the ligand. pH = change in OS usually involves hydrogen ions ligand = can affect the potential due to the strength of the ligand
68
Reduction of Tollen's Reagent
- Contains [Ag(NH3)2]+ - Distinguishes between aldehydes and ketone - Ag+ reduced to Ag - Aldehyde is oxidised to carboxylic acid
69
What is the equation for the reduction of Tollen's Reagent?
[Ag(NH3)2]+ + e- -> Ag + 2NH3
70
What happens in a REDOX titration?
- Involves an oxidising agent being titrated against a reducing agent - Electrons are transferred from one species to another - 'self-indicating' - Manganate (VII) Ions and Dichromate (VI) Ions
71
Manganate (VII) Titrations
- Potassium manganate (VII) is an oxidising agent and a deep purple colour - Reduction of manganate ions: MnO4(-) + 8H+ + 5e- -> Mn(2+) + 4H2O Example: Oxidation: Fe(2+) -> Fe(3+) + e- Reduction: MnO4(-) + 8H+ + 5e- -> Mn(2+) + 4H2O Overall: MnO4(-) + 8H+ + 5Fe(2+) -> Mn(2+) + 4H2O + 5Fe(3+) Colour change = deep purple to colourless
72
Dichromate (VI) Titrations
- Potassium dichromate (VI) -> K2Cr2O7 - Oxidation state of chromium changes from +6 to +3: Cr2O7(2-) + 14H+ + 6e- -> 2Cr(3+) + 7H2O - To enchance the endpoint an indicator called diphenylaminesulfonate is used which turns from colourless to purple at the endpoint Colour change = orange to green (purple with indicator) Example: Oxidation: Fe(2+) -> Fe(3+) + e- Reduction: Cr2O7(2-) + 14H+ + 6e- -> 2Cr(3+) + 7H2O Overall: 6Fe(2+) + Cr2O7(2-) + 14H+ + 6e- -> 2Cr(3+) + 7H2O
73
What is a catalyst?
Speeds up a reaction, without being used up, by providing an alternative reaction pathway, with a lower activation energy.
74
What are the two types of catalyst?
Heterogeneous and Homogeneous
75
What is a heterogeneous catalyst?
A catalyst that is in a different state from the reactants e.g Fe in the Haber process
76
What is a homogeneous catalyst?
A catalyst that is in the same state an the reactants e.g. Fe(2+) in the reaction between I(-) and S2O8(2-)
77
The Contact Process
V2O5 + SO2 -> V2O4 + SO3 V2O4 + 1/2O2 -> V2O5 Overall: SO2 + 1/2O2 -> SO3 Can be used as a catalyst because its OS can change
78
Fe(2+) can catalyse the reaction between I(-) and S2O8(2-)
- Example of Fe(2+) being a homogeneous catalyst - Overall equation for the reaction: S2O8(2-) + 2I(-) -> 2SO4(2-) + I2 - The reaction is slow to begin with because the two negative ions repel each other Fe(2+) ions catalyse the reaction: 2Fe(2+) + S2O8(2-) -> 2Fe(3+) + 2SO4(2-) 2Fe(3+) + 2I -> 2Fe(2+) + I2
79
Mn(2+) can autocatalyse the reaction between C2O4(2-) and MnO4(-)
- The products in a reaction acts as a catalyst for the reaction 5C2O4(2-) + 2MnO4- + 16H+ -> 10CO2 + 2Mn(2+) + 8H2O Mn(2+) ions catalyse the reaction in two reactions: 4Mn(2+) + MnO4(-) + 8H+ -> 5Mn(3+) + 4H2O 2Mn(3+) + C2O4 -> 2Mn(2+) + 2CO2

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