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Transition Metals Flashcards

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1
Q

Define a transition element

A

An element which forms at least one stable ion with a partially full d-shell of electrons

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2
Q

Where are the transition metals located in the periodic table?

A

In the middle (block from Ti to Cu) - part of the d-block

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3
Q

What are some characteristic physical properties of transition metals?

A

Metallic, good conductors of heat and electricity, hard, strong, shiny, high m.p., high b.p., low reactivity.

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4
Q

Some uses of iron?

A

Vehicle bodies, to reinforce concrete

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5
Q

Some uses of titanium?

A

Jet engine parts

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6
Q

Some uses of copper?

A

Water pipes

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7
Q

What are the characteristic chemical properties of transition metals (4)?

A

Variable oxidation states → take part in many redox reactions Coloured compounds/ions in solution
Good catalysts
Form complex ions

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8
Q

Define the term complex ion

A

Central transition metal ion surrounded by ligands (other ions/molecules) that are co-ordinated bonded to it.

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9
Q

Give some example of transition metals catalysts and the processes/reactions they catalyse (3)?

A

Iron - Haber process
Vanadium (V) oxide - Contact process MnO2 - decomposition of H2O2

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10
Q

Which electrons do transition metals lose first when forming ions?

A

4s

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11
Q

Define the term ligand

A

An ion or molecule with at least one lone pair of electrons, that donates them to a transition metal ion to form a co-ordinate bond and thus a complex ion.

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12
Q

Define the term mono/unidentate ligands

A

A ligand that forms one co-ordinate bond to the central metal ion (one lone pair to donate)

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13
Q

Define the term bidentate ligand.

A

A ligand that forms two co-ordinate bonds to the central metal ion (2 lone pairs to donate)

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14
Q

Define the term multidentate ligand.

A

A ligand that forms three or more co-ordinate bonds to the central metal ion

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15
Q

Give some examples of common monodentate ligands (4).

A

Cl-, H2O, NH3, CN-

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16
Q

Draw ethanedioate; how many co-ordinate bonds can it form to a transition metal ion?

A

2 co-ordinate bonds

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17
Q

Draw benzene-1,2-diol; how many co-ordinate bonds can it form to a transition metal ion?

A

2 co-ordinate bonds

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18
Q

Draw ethane-1,2-diamine. What is its shortened name? How many co-ordinate bonds does it
form?

A

2 co-ordinate bonds, shortened name = en

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19
Q

How many co-ordinate bonds does EDTA4- form?

A

six

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20
Q

Define the term coordination number

A

The number of co-ordinate bonds the metal ion has formed to surrounding ligands

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21
Q

What is the Chelate effect?

A

Chelate complexes with multidentate ligands are favoured over monodentate ligands or ligands that form fewer co-ordinate bonds per molecule

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22
Q

Explain the Chelate effect in terms of entropy and the reaction that is occurring

A

Number of molecules increases when multidentate ligands, e.g. EDTA, displacee ligands that form fewer co-ordinate bonds per molecule
Significant increase in entropy → Gibbs’ free energy change < 0 → feasible reaction
A more stable complex ion is formed

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23
Q

What shape is a complex ion if it has 6 ligands?

A

Octahedral

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23
Q

What ion is usually formed when a transition metal compound is dissolved in water? What shape is it?
Draw an example

A

Aqua ion, 6 H2O ligands around the central metal ion. Octahedral complex ion is formed

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24
If a transition metal ion has 2 ligands, what shape is it usually?
Linear
25
How can complex ions display E-Z or cis-trans isomerism? What shapes of ion does this apply to?
Ligands differ in the way in which they are arranged in space 2 ligands of the same type can be on the same side of the metal ion (next to each other), which forms the E or cis isomer 2 ligands of the same type can be on opposite sides of the metal ion (not next to each other), which forms the Z or trans isomer Applies to square planar and octahedral complex ions
26
If a transition metal ion has 4 ligands, what shape is it usually?
Tetrahedral
27
Name an exception to the general rule that ions with 4 ligands is generally tetrahedral. What shape is it?
Platin is square planar → forms cisplatin
28
What conditions are needed for a complex ion to display optical isomerism?
Usually applies to octahedral molecules with 2 or more bidentate ligands, so that the mirror images are non-superimposable
29
What happens to Co2+, Cu2+ and Fe3+ ‘s coordination numbers when Cl- ligands replace NH3 or H2O ligands?
Decreases from 4 to 6 as Cl- is a much larger ligand than H2O and NH3
30
What is haem - its metal ion, coordination number and ligands?
A molecule which makes up protein chains, with an Fe2+ central metal ion, which has a coordination number of 6. 4 of these bonds are to a ring system called porphyrin. 1 is to the nitrogen of a globin (protein) molecule and one is to an oxygen in an O2 molecule
31
How does haemoglobin transport oxygen?
O2 forms a weak coordinate bond to the metal ion, then is transported around the body. The bond breaks when haemoglobin reaches cells and oxygen is released
32
Why are transition metal compounds coloured?
They have partially filled d-orbitals and electrons are able to move between the d-orbitals. In compounds (when ligands coordinately bond to the ion), the d-orbitals split into different energy levels. Electrons can absorb energy in the form of photons to become excited and move to a higher energy level (excited state). Energy of photon = energy difference between levels Energy of photon is related to frequency of light by E = hf The colour corresponding to the frequency of the energy change is missing from the spectrum, so we see a combination of all the colours that aren’t absorbed
33
Why is CO toxic?
CO also coordinately bonds to the Fe2+, and is a better ligand, so bonds more strongly than O2. Stops O2 from bonding to haemoglobin, so O2 cannot be transported around the body
34
How do you calculate ΔE from f and/or λ?
ΔE=hf=hc÷λ
35
What affects the colour of a transition metal compound?
ΔE affects the frequency of absorbed photons, so determines the colour. ΔE is changed by oxidation state of the metal, number and type of ligands, shape, co-ordination number
36
Fill in this table for vanadium species:
check
37
What can you use to reduce Vanadium?
Zinc
38
What colour is Fe2+’s aqua ion?
Green
39
What colour is Co3+’s aqua ion?
Yellow
40
What colour is Fe3+’s aqua ion?
Pale brown
41
What colour is Cr2+’s aqua ion?
blue
42
What colour is Cr3+’s aqua ion?
red/violet
43
What colour is Co2+’s aqua ion?
Brown
44
What does a colorimeter do?
Measures the absorbance of a particular wavelength of light by a solution
45
How would you use colorimetry experimentally?
Use solutions of known concentration to create a calibration graph; find unknown concentration
46
What information can a colorimeter give you?
The concentration of a certain ion in the solution
47
Why can transition metals have variable oxidation states?
They have partially filled d-orbitals, so can lose 4s and 3d electrons
48
Which oxidation states do all transition metals have? (except Sc). Why?
+2 due to loss of electrons from 4s orbital
49
When oxidation state is high, do the transition metals exist as simple ions?
No, after oxidation state of about III, metal ions covalently bond to other species
50
What is the use of the complex [Ag(NH3)2)]+ ion?
Tollens’ reagent to test for aldehydes/ketones (silver mirror formed with aldehyde, no visible change with ketone)
51
What colour is MnO4-?
Deep purple
52
What colour is Mn2+?
Pink
53
Write a half equation for the reduction of MnO4- to Mn2+
check
54
Why are redox titrations with transition metal compounds said to be self-indicating?
They usually involve a colour change as the metal is changing oxidation state; sometimes an indicator is still needed/useful
55
What colour is Cr2O72-?
orange
56
What colour is Cr3+?
green
57
Write a half equation for the reduction of Cr2O72- to Cr3+
check
58
What happens to aqua metal ions in acidic conditions?
They get reduced
59
What happens to aqua metal ions in alkaline conditions?
They get oxidised
60
What happens to aqua metal ions in neutral conditions?
No change
61
What does whether reduction/oxidation occurs and the readiness of the reaction depend on?
E° values
62
Define a catalyst
A substance that increases the rate of a reaction without being chemically changed at the end of the reaction
62
What can change these E° values?
pH, ligands involved
63
How do catalysts usually work?
Provide an alternative reaction pathway with a lower activation energy
64
Why are transition metals good catalysts?
They can exist in variable oxidation states, so can provide alternative pathways easily
65
Why are group 1, 2 and 3 metals not as good catalysts?
Only exist in one oxidation state
66
What are advantages of using a catalyst for a reaction?
Allows reactions to proceed at lower temperatures and pressures → saves valuable energy and resources
67
What metals are used in a catalytic converter and which reactions do they catalyse?
Pt, Rd, Pd CatalyseCO,NO→CO2,N2andCxH2x+2 → H2O, CO2
68
Define a heterogeneous catalyst
A catalyst that is present in the reaction in a different phase to the reactants (usually a solid, with gas/liquid reactants). Catalytic activity occurs on the solid surface as the reactants pass over it
69
What is an advantage of using a heterogeneous catalyst?
No need for separation of products from catalyst
70
How do heterogeneous catalysts work?
Reactants adsorb to the catalyst’s surface at active sites. This weakens bonds within the reactants, holds reactants close together on the surface and/or in the correct orientation to react. Once the reaction has occurred, products desorb from the active sites.
71
What properties does the catalyst need to have to make it a good catalyst?
Can’t adsorb too strongly, otherwise the products will not desorb. Can’t adsorb too weakly as reactant would not be held in place for long enough and bonds would not be sufficiently weakened. Need a good balance between desorption and adsorption.
72
How can you increase the efficiency of heterogeneous catalysts?
Increase the surface area to increase the number of active sites that are present. Also spread onto an inert support medium, e.g. ceramic, to increase the surface/mass ratio. Use ceramic honeycomb matrix/mesh/sponge.
73
What is catalyst poisoning?
Unwanted impurities adsorb to the catalyst’s active sites and do not desorb. This blocks the active sites on the catalyst’s surface
74
What effect does catalyst poisoning have on catalytic activity?
Decreases the effectiveness of the catalyst over time
75
Decreases the effectiveness of the catalyst over time
76
What is the Haber process? What catalyst is used?
N2 (g) + 3H2 (g) → 2NH3 (g) Makes ammonia, uses iron (Fe) catalyst
77
What size/shape is the catalyst for the Haber process?
Pea sized lumps to increase surface area
78
How long does the catalyst last for the Haber process? What is it poisoned by?
About 5 years. Poisoned by sulfur impurities in the gas streams
79
What is the Contact Process? What is the catalyst?
Makes H2SO4. Catalysed by vanadium (V) oxide - V2O5 2SO2 (g) + O2 (g) → 2SO3 (g)
80
What are the two reactions that are involved in the contact process?
SO2 + V2O5 → SO3 + V2O4 V2O4 + 1⁄2O2 → V2O5
81
Why is V a good catalyst in the case of the contact process?
Can change oxidation state from 5+ to 4+ and back to 5+ (so can be used again)
82
Define homogeneous catalyst
A catalyst that is in the same phase as the reactants.
83
How do homogeneous catalysts work?
Form intermediates to give a different reaction pathway with lower EA
84
What is the reaction between S2O82- ions and I- ions?
S2O82- + 2I- → 2SO42- + I2 (all aq)
85
Why does the reaction between S2O82- ions and I- ions have a high EA in normal conditions?
Two negative ions are reacting. They repel each other so EA is high
86
Which transition metal ions catalyse the reaction between S2O82- ions and I- ions? Write two equations to show how.
Fe2+ S2O82- + 2Fe2+ → 2Fe3+ + 2SO42- 2Fe3+ + 2I- → 2Fe2+ + I2
87
Define the term autocatalysis
When the product of a reaction is also a catalyst for that reaction.
88
Draw a concentration of reactant against time graph for an autocatalysed reaction. Explain each stage.
Initially slow, uncatalysed as not much of catalyst has been formed Rate increases as catalyst is made; catalysed reaction is faster Slows down as reactants are used up check picture!
89
Write a half equation for the conversion of C2O42- ions into CO2
C2O42- → 2CO2 + 2e-
90
Write an equation for the reaction between C2O42- ions and MnO4- ions. How does Mn2+ autocatalyse this reaction?
2MnO4- + 16H+ + 5C2O42- → 10CO2 + 2Mn2+ + 8H2O 1st stage: MnO4- + 4Mn2+ + 8H+ → 4H2O + 5Mn3+ 2nd stage: 2Mn3+ + C2O42- → 2CO2 + 2Mn2+
91
How can you monitor the concentration of MnO4- ions?
Using a colorimeter

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