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A Level Inorganic Chemistry > Section 4 - Transition Metals > Flashcards

Section 4 - Transition Metals Flashcards

1
Q

Define transition metal:

A

A metal that can form one or more stable ions with a partially filled sub-shell.

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2
Q

Which period 4, d-block elements are not transition metals?

A

Scandium and Zinc

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3
Q

What are the 3 physical properties of transition metals?

A
  • high density
  • high mpts and bpts
  • similar ionic radii
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4
Q

What is the oxidation state/colour of:

MnO4-

A

+7 - purple

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5
Q

What is the oxidation state/colour of:

Cr2O72-

A

+6 - Orange

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6
Q

What is the oxidation state/colour of:

VO2+

A

+5 - Yellow

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7
Q

What is the oxidation state/colour of:

VO2+

A

+4 - Blue

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8
Q

What is the oxidation state/colour of:

V3+

A

+3 - Green

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9
Q

What is the oxidation state/colour of:

Cr3+

A

+3 - Green/Violet

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10
Q

What is the oxidation state/colour of:

Fe3+

A

+3 - Yellow

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11
Q

What is the oxidation state/colour of:

V2+

A

+2 - Violet

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12
Q

What is the oxidation state/colour of:

Mn2+

A

+2 - Pale Pink

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13
Q

What is the oxidation state/colour of:

Fe2+

A

+2 - Pale Green

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14
Q

What is the oxidation state/colour of:

Co2+

A

+2 - Pink

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15
Q

What is the oxidation state/colour of:

Ni2+

A

+2 - Green

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16
Q

What is the oxidation state/colour of:

Cu2+

A

+2 - Blue

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17
Q

Define Complex Ion

A

A central metal atom/ion surrounded by co-ordinately bonded ligands.

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18
Q

What is the coordination number?

A

The number of coordinate bonds formed with the central metal ion

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19
Q

What are the usual coordination numbers?

A

6 for small ligands eg. water, ammonia

4 for large ligands eg. Cl-

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20
Q

What are the bond angles in a tetrahedral compex ion shape?

A

109.5

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21
Q

How do you calculate the oxidation state of a metal ion?

A

total oxidation state - sum of oxidation states of ligands

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22
Q

What are the bond angles in a square planar complex ion?

A

90

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23
Q

What complex ion forms a linear shape with bond angle 180?

A

[Ag(NH3)2]+

24
Q

What is a monodentate ligand?

A

One which can form only one bond

25
Q

What is a multidentate ligand?

A

One which can form more than one bond

26
Q

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

A
  • form complex ions
  • form coloured ions
  • good catalysts
  • variable oxidation states
27
Q

What is Haem?

A

Fe2+ ions with multidentate ligands

28
Q

How does Haem transport oxygen?

A

Oxygen forms a co-ordinate bond to Fe(II) in haemoglobin , enabling oxygen to be transported in the blood.

29
Q

Why is CO toxic?

A

Carbon monoxide is toxic because it replaces oxygen co-ordinately bonded to Fe(II) in haemoglobin.

30
Q

What type of isomerism do some complex ions show?

A

Optical - when a complex metal ion has 3 bidentate ligands coordinately bonded to it

31
Q

In which case can complex ions show E-Z isomerism?

A

When octahedral/square planar complex ions have monodentate ligands of various types

32
Q

What is the chelate effect?

A

When bidentate and multidentate ligands replace monodentate ligands from complexes.

33
Q

How do transition metals display colour?

A

Colour arises when some of the wavelengths of visible light are absorbed when electrons jump to the higher energy level and the remaining wavelengths of light are transmitted or reflected.

34
Q

What colour will you see if the 3d sub shell is full or empty?

A

White/colourless

35
Q

What happens to d electrons when light is absorbed?

A

They move from a ground state to an excited state

36
Q

The energy difference between the ground state and the excited state of the d electrons is given by:

A

∆E = hν = hc/λ

37
Q

What can cause a change of colour?

A

Changes in oxidation state, co-ordination number and ligand alter ∆E and this leads to a change in colour.

38
Q

How can spectroscopy be used to find concentrations of transition metal ions?

A

The absorption of visible light is used in spectroscopy. A simple colorimeter can be used to determine the concentration of coloured ions in solution.

39
Q

Why are complex ions with multidentate ligands more stable than with monodentate ligands?

A

The number of particles in the solution increases so there is a greater entropy and therefore it is more stable.

40
Q

What is redox potential dependent on?

A
  • ligands attached
  • pH
41
Q

How do you reduce Vanadium ions?

A

Vanadium species in oxidation states IV, III and II are formed by the reduction of vanadate(V) ions by zinc in acidic solution.

42
Q

Give the equation for the redox titration of Fe2+ with MnO4-

A

MnO4- + 8H+ + 5Fe2+ —> Mn2+ + 5Fe3+ + 4H2O

43
Q

Give the equation for the redox titration of C2O42- with MnO4-

A

2MnO4- + 16H+ + 5C2O42- –> 2Mn2+ + 8H2O + 10CO2

44
Q

What is a heterogenous catalyst?

A

A heterogeneous catalyst is in a different phase from the reactants and the reaction occurs at active sites on the surface.

45
Q

What are support mediums used for?

A

They are used to increase the surface area of the catalyst while minimising cost - the cayalyst is coated onto it

46
Q

Give the equation for the Iron catalyst in the Haber Process

A

N2 + 3H2 ——Fe——–> 2NH3

47
Q

Give the equation for the Vanadium Oxide catalyst in the Contact Process for making sulfuric acid

A

SO2 + 1/2O2 ——-V2O5 ——-> SO3

48
Q

Give the equations for the Vanadium catalyst regenerating itself

A

V2O5 + SO2 —> V2O4 + SO3

V2O4 + 1/2O2 —> V2O5

49
Q

How is the iron catalyst poisoned in the Haber Process>

A

The methane which provides the hydrogen contains impurities (sulfur compounds) which adsorb onto the iron, stopping the catalyst from working effectively.

50
Q

What is a homogenous catalyst?

A

Catalysts in the same state as the reactants.

51
Q

How do homogenous catalysts provide a more effective route?

A

They combine with the reactants to form an intermediate species. The Ea to form this and then to form the products is lower than to form the products directly.

52
Q

Why are variable oxidation states important in catalysts?

A

Transition mtals can transfer electrons to speed up reactions.

53
Q

Why does the reaction between iodide ions and peroxodisulfate ions require a catalyst?

A

They are both negatively charged so repel each other meaning its unlikely they’ll collide and react.

54
Q

Give the equation for the reaction of S2O82- and I- with an iron (II) catalyst and explain why it works.

A

S2O82- + I- –> I2 + 2SO42- Overall equation

S2O82- + 2Fe2+ —> 2Fe3+ + 2SO42- Iron ions are oxidised

2Fe3+ + 2I- —> I2 + 2Fe2+ Iron ions oxidise iodine ions and catalyst is regenerated

55
Q

What is autocatalysis?

A

When a product catalyses a reaction

56
Q

Give the equations for the reaction of the reaction of C2O42- and MnO4- with a Mn2+ catalyst

A

2MnO4- + 16H+ + 5C2O42- —> 2Mn2+ + 8H2O + 10CO2 Overall equation

MnO4- + 4Mn2+ + 8H+ —> 5Mn3+ + 4H2O

2Mn3+ + C2O42- —> 2Mn2+ + 2CO2

A Level Inorganic Chemistry (4 decks)

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