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A Level Inorganic Chemistry > 2.5 Transition Metals > Flashcards

2.5 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 characteristics/physical properties of transition metals

A

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

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4
Q

Some uses of iron?

A

Bodies of vehicle,
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 so take part in many redox reactions
Coloured compounds/ ions in solution
Good catalyst
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 have Co-ordinated bonds 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 (Manganese dioxide) - 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 ligands 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 bond 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

Slide 34

Two coordinate 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

Slide 36

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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

Slide 38

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19
Q

How many Co-ordinate bonds does EDTA 4- 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, displaces 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 ion is usually formed when a transition metal compound is dissolved in water? What shape is it? Draw an example

A

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

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24
Q

If a transition metal ion has 2 ligands, what shape is it usually?

A

Linear

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25
Q

If a transition metal ion has 4 ligands, what shape is it usually?

A

Tetrahedral

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26
Q

Name an exception to the general rule that ions with 4 ligands is generally tetrahedral. What shape is it?

A

Platin is square planar —> forms cisplatin

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27
Q

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

A

Octahedral

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28
Q

How can complex ions display E-Z or cis-trans isomerism? What shapes of ion does this apply to?

A

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

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29
Q

What conditions are needed for a complex ion to display optical isomerism?

A

Octahedral molecules with 2 or more bidentate ligands, so that the mirror images are non-superimposable

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30
Q

What happens to CO2+, Cu2+ and Fe3+’s coordination numbers when Cl- ligands replace NH3 or H2O ligands?

A

Decreases from 4 to 6 as Cl- is a much larger ligand than H2O and NH3

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31
Q

What is haem - its metal ion, coordination number and ligands?

A

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

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32
Q

How does haemoglobin transport oxygen

A

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

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33
Q

Why is CO toxic

A

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

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34
Q

Why are transition metal compounds coloured

A

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

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35
Q

How do you calculate ΔE from f and/or λ?

A

ΔE = hf = hc / λ

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36
Q

What affects the colour of a transition metal compound

A

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

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37
Q

Fill in this table for vanadium species

A

Species :VO2^+, VO^2+,V^3+,V^2+
Oxidation number: 5+,4+,3+,2+
Colour: yellow,blue,green,violet

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38
Q

What can you use to reduce Vanadium

A

Zinc

39
Q

What colour is Fe2+’s aqua ion?

A

Green

40
Q

What colour is Fe3+’s aqua ion?

A

Brown

41
Q

What colour is Cr2+’s aqua ion?

A

Blue

42
Q

What colour is Cr3+’s aqua ion?

A

Red/violent

43
Q

What colour is CO2+’s aqua ion?

A

Brown

44
Q

What colour is Co3+’s aqua ion?

A

Yellow

45
Q

What does a colorimeter do?

A

Measures the absorbance of a particular wavelength of light by a solution

46
Q

How would you use colorimetry experimentally

A

Use solutions of known concentration to create a calibration graph; find unknown concentration

47
Q

What information can a colorimeter give you

A

The concentration of a certain ion in the solution

48
Q

How can transition metals have variable oxidation states

A

They have partially filled d-orbitals, so can lose 4s and 3d electrons

49
Q

Which oxidation states do all transition metals have? (Except Sc). Why?

A

+2 due to loss of electrons from 4s orbital

50
Q

When oxidation state is high, do the transition metals exist as simple ions

A

No, after oxidation state of about III, metal ions covalently bond to other species

51
Q

What is the use of the complex [Ag(NH3)2)]+ ion?

A

Tollens’ reagent to test for aldehydes/ketones (silver mirror formed with aldehydes, no visible change with ketone)

52
Q

What colour is MnO4-?

A

Deep purple

53
Q

What colour is Mn2+?

A

Pink

54
Q

Write a half equation for the reduction of MnO4- to Mn2+

A

MnO4- + 8H+ + 5e- —> Mn2+ + 4H2O

55
Q

Why are redox titrations with transition metal compounds said to be self-indicating?

A

They usually involve a colour change as the metal is changing oxidation state; sometimes an indicator is still needed/useful

56
Q

What colour is Cr2O7 2-?

A

Orange

57
Q

What colour is Cr3+?

A

Green

58
Q

Write a half equation for the reduction of Cr2O72- to Cr3+

A

Cr2O72- + 14H+ + 6e- ——> 2Cr3+ + 7H2O

59
Q

What happens to aqua metal ions in acidic conditions

A

They get reduced

60
Q

What happens to aqua metal ions in alkaline conditions

A

They get oxidised

61
Q

What happens to aqua metal ions in neutral conditions

A

No change

62
Q

What does whether reduction/oxidation occurs and the readiness of the reaction depend om

A

E^0 values

63
Q

What can change these E^0 values

A

pH, ligands involved

64
Q

Define catalyst

A

A substance that increases the rate of a reaction without being chemically changed at the end of the reaction

65
Q

How do catalysts usually work

A

Provide an alternative reaction pathway with a lower activation energy

66
Q

Why are transition metals good catalysts

A

They can exist in variable oxidation states, so can provide alternative pathways easily

67
Q

Why are group 1,2 and 3 metals not as good catalysts

A

Only exist in one oxidation state

68
Q

What are advantages of using a catalyst for a reaction

A

Allows reactions to proceed at lower temperatures and pressures —> saves valuable energy and resources

69
Q

What metals are used in a catalytic converter and which reaction do they catalyse

A

Pt,Rd,Pd

Catalyse CO, NO —> CO2, N2 and CxH2x+2 —> H2O,CO2

70
Q

Define a heterogenous catalyst

A

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

71
Q

What is an advantage of using a heterogenous catalyst?

A

No need for separation of products from catalyst

72
Q

How do heterogenous catalysts work?

A

Reactants adsorb to the catalyst’s surface at active sites. This weakens bonds within the reactants, hold 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

73
Q

What properties does the catalyst need to have to make it a good catalyst

A

Can’t adsorb too strongly, otherwise products will not desorb. Can’t adsorb too weakly as reactants would not be held in place for long enough and bonds would not be sufficiently weakened. Need a good balance between desorption and adsorption

74
Q

How can you increase the efficiency of heterogenous catalysts

A

Increase the surface area to increase the number of active site 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

75
Q

What is catalyst poisoning?

A

Unwanted impurities adsorb to the catalyst’s active sites and do not desorb. This blocks the active sites on the catalyst’s surface

76
Q

What effect does catalyst poisoning have on catalytic activity?

A

Decrease the effectiveness of the catalyst over time

77
Q

How else can a catalyst be degraded

A

Finely divided catalysts can be gradually lost from their support medium

78
Q

What is the haber process? What catalyst is used?

A

N2(g) + 3H2(g) —> 2NH3(g) Makes ammonia, uses iron (Fe) catalyst

79
Q

What size/shape is the catalyst for the Haber process

A

Pea sized lumps to increase surface area

80
Q

How long does the catalyst last for the Haber process? What is it poisoned by?

A

About 5 years. Poisoned by sulfer impurities in the gas streams

81
Q

What is the contact process? What is the catalyst?

A

Makes H2SO4. Catalysed by vanadium (V) oxidise -V2O5

2SO2(g) + O2(g) —> 2SO3(g)

82
Q

What are the two reactions that are involved in the contact process?

A

SO2 + V2O5 —> SO3 + V2O4

V2O4 + 1/2O2 —> V2O5

83
Q

Why is V a good catalyst in the case of the contact process?

A

Can change oxidation state from 5+ to 4+ and back to 5+ (so can be used again)

84
Q

Define homogenous catalyst

A

A catalyst that is in the same phase as the reactants

85
Q

How do homogeneous catalysts work

A

Forms intermediates to give a different reaction pathway with a lower Ea

86
Q

What is the reaction between S2O82- ions and I- ions

A

S2O8 2- + 2I- —> 2SO4 2- + I2 (all aq)

87
Q

Why does the reaction between S2O8 2- ions and I- ions have a high Ea in normal conditions

A

Two negative ions are reacting. They repel each other so Ea is high

88
Q

Which transition metal ions catalyse the reaction between S2O8 2- ions and I- ions? Write two equations to show how

A

Fe2+

S2O8 2- + 2Fe2+ —> 2Fe3+ + 2SO4 2-

2Fe3+ + 2I- —> 2Fe2+ + I2

89
Q

Define the term autocatalysis

A

When the product of a reaction is also a catalyst for that reaction

90
Q

Draw a concentration of reactant against time graph for an autocatalysed reaction. Explain each stage

A

Slide 182

91
Q

Write a half equation for the conversion of C2O4 2- ions into CO2

A

C2O4 2- —> 2CO2 + 2e-

92
Q

Write an equation for the reaction between C2O4 2- ions and MnO4- ions. How does Mn2+ autocatalyse this reaction

A

2MnO4- + 16H+ +5C2O4 2- —> 10CO2 + 2Mn2+ + 8H2O

1st stage: MnO4- + 4Mn2+ + 8H+ —> 4H2O + 5Mn3+
2nd stage: 2Mn3+ + C2O4 2- —> 2CO2 + 2Mn2+

93
Q

How can you monitor the concentration of MnO4- ions?

A

Using a colorimeter

A Level Inorganic Chemistry (6 decks)

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