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A-Level Chemistry > 3.4 Chemistry of the d-block transition metals > Flashcards

3.4 Chemistry of the d-block transition metals Flashcards

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1
Q

What is a transition metal?

A

A transition metal is a d-block element that forms one or more stable ions with partially filled d-orbitals.

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2
Q

Which two elements in the d-block of the periodic table are not technically transition metals?

A

Scandium and zinc.
They do not form ions with an incomplete d-subshell.

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3
Q

Which two elements in the periodic table are exceptions to the rule that the 4s orbital is filled before the 3p orbital?

A

Chromium and copper. The 4s orbital only fills the one electron as this gives them more stable configurations in the 3d orbital.

Chromium: [Ar] 4s1 3d5
Copper: [Ar] 4s1 3d10

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4
Q

What are some general properties of transition metals?

A
  • They have variable oxidation states.
  • They form complex ions.
  • They form coloured ions in solution.
  • They can catalyse reactions either as elements or in compounds.
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5
Q

Give examples of transition metals that have variable oxidation states

A

Fe2+ and Fe3+
Cu+ and Cu2+
Cr2+ and Cr3+

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6
Q

Why do transition metals have variable oxidation states?

A

Variable oxidation states arise because the electrons in the 4s and 3d orbitals have very similar energies. This means that a relatively similar amount of energy is required to gain or lose different numbers of electrons.

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7
Q

What are the most common oxidation states of Cr?

A

+2
+3
+6

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8
Q

What are the most common oxidation states of Mn?

A

+2
+4
+7

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9
Q

What are the most common oxidation states of Fe?

A

+2
+3

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10
Q

What are the most common oxidation states of Cu?

A

+1
+2

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11
Q

What are the most common oxidation states of Co?

A

+2
+3

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12
Q

What colour are aqueous solutions of compounds containing Cr3+ ions?

A

Green

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13
Q

What colour are aqueous solutions of compounds containing CrO4^2- ions?

A

Yellow

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14
Q

What colour are aqueous solutions of compounds containing Cr2O7^2- ions?

A

Orange

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15
Q

What colour are aqueous solutions of compounds containing MnO4^- ions?

A

Purple

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16
Q

What colour are aqueous solutions of compounds containing Co2+ ions?

A

Pink

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17
Q

What colour are aqueous solutions of compounds containing Fe2+ ions?

A

Green

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18
Q

What colour are aqueous solutions of compounds containing Fe3+ ions?

A

Brown

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19
Q

What colour are aqueous solutions of compounds containing Cu2+ ions?

A

Blue

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20
Q

What is a ligand?

A

A ligand is an ion or molecule that bonds to a central metal atom to form a complex ion.

21
Q

What type of bonding is involved in the formation of metal complex ions?

A

Coordinate bonding

22
Q

What is a complex ion?

A

A complex ion is a central metal ion surrounded by ligands

23
Q

Aqueous solutions of transition metal ions are usually ______ .
Fill in the gap

A

Coloured

24
Q

What is meant by coordination number?

A

The number of dative bonds formed with a central metal ion.

25
Q

Why do transition metals form coloured complexes?

A

When visible light hits a transition metal ion, electrons are excited to higher energy levels. Some frequencies of the visible light are absorbed when electrons jump up to higher energy orbitals. The rest of the frequencies of visible light are transmitted or reflected. These frequencies combine to make the complement of the colour of the absorbed frequencies. This creates the colour of the complex.

26
Q

What can lead to a colour change in a transition metal complex?

A
  • Change in oxidation number of the ion.
  • Change in the ligand.
  • Change in the coordination number of the complex.
27
Q

What is the shape of the [CrCl4]- complex?

A

Tetrahedral
Bond angle: 109.5

28
Q

What is the shape of the [Cr(NH3)6]3+ complex?

A

Octahedral
Bond angle: 90

29
Q

What is the shape of the [Cu(NH3)4(H2O)2]2+ complex?

A

Octahedral
Bond angle: 90

30
Q

What is a ligand exchange reaction?

A

A ligand exchange is a chemical reaction involving the replacement of ligands in a complex by a different set of ligands:

[Cu(H2O)6]2+ + 4NH3 —> [Cu(NH3)4(H2O)2]2+ + 4H2O

31
Q

What is the equation and observations for the ligand exchange reaction between copper hexaaqua ions and ammonia?

A

[Cu(H2O)6]2+(aq) + 2NH3(aq) —> Cu(H2O)4(OH)2 + 2NH4^+(l)

Cu(H2O)4(OH)2 + 2NH3(aq) —> [Cu(NH3)4(H2O)2]2+(aq) + 2OH- + 2H2O

The blue solution forms a light blue precipitate. This dissolves in excess ammonia to form a dark blue solution.

32
Q

What is the equation, and the observations for the ligand exchange reaction between copper hexaaqua ions and chloride ions?

A

[Cu(H2O)6]2+(aq) + 4Cl-(aq) —> [CuCl4]2-(aq) + 6H2O(l)

The blue solution forms a yellow solution.

33
Q

What is the equation, and the observations for the ligand exchange reaction between cobalt hexaaqua ions and chloride ions?

A

[Co(H2O)6]2+(aq) + 4Cl-(aq) <—> [CoCl4]2-(aq) + 6H2O(l)

The pink solution forms a dark blue solution.

34
Q

What colour are the compounds [CoCl4]2- and [CuCl4]2- ?

A

[CuCl4]2- —> Green
[CoCl4]2- —> Blue

35
Q

What colour are the compounds [Co(H2O)6]2+ and [Cu(H2O)6]2+ ?

A

[Cu(H2O)6]2+ —> Blue
[Co(H2O)6]2+ —> Pink

36
Q

What colour is the compound [Cu(NH3)4(H2O)2]2+ ?

A

Blue

37
Q

What is the difference between a homogeneous and heterogeneous catalyst?

A

A homogenous catalyst is in the same phase as the reactants and the catalysed reaction takes place via intermediate species.
A heterogeneous catalyst is in a different phase to the reactants and the reaction occurs on the surface of the catalyst.

38
Q

Why do transition metals make good homogeneous catalysts?

A

Transition metals have variable oxidation states, making them good homogeneous catalysts. The variable oxidation states mean they are able to oxidise and reduce reactants and intermediates to form the desired products.

39
Q

Why do transition metals make good heterogeneous catalysts?

A

Using the 3d and 4s electrons of the atoms on the catalyst surface, transition metals can form weak bonds with reactants, making them more reactive.

40
Q

What catalyst is used in the hydrogenation of alkenes? Is it homogeneous or heterogeneous?

A

Nickel
Heterogeneous

41
Q

What catalyst is used in the Haber process? Is it homogeneous or heterogeneous?

A

Iron
Heterogeneous

42
Q

What is the contact process?

A

An industrial process used to make sulfuric acid. It is made by oxidising sulfur dioxide in the presence of a solid catalyst. Sulfur trioxide is then reacted with water to form sulfuric acid.

43
Q

What are the conditions required for the Contact Process?

A

Temperature around 450 degrees Celsius
Vanadium oxide catalyst (V2O5)
Pressure of 2 atm

44
Q

Write the two equations showing how vanadium acts as a catalyst in the contact process

A

SO2 + V2O5 —> SO3 + V2O4
V2O4 + 1/2O2 —> V2O5

45
Q

What catalyst is used in the decomposition of hydrogen peroxide? Is it homogeneous or heterogeneous?

A

Manganese (IV) oxide
Homogeneous

46
Q

Give the reaction for the reaction of Cr(III) ions with excess NaOH

A

[Cr(H2O)6]3+ + 6OH- —> [Cr(OH)6]3- + 6H2O

47
Q

Give the equation for the reaction of Fe(II) ions with excess NaOH

A

[Fe(H2O)6]2+ + 2OH- —> Fe(H2O)4(OH)2 + 2H2O

The green solution forms a green precipitate.

48
Q

Give the equation for the reaction of Fe(III) ions with excess NaOH

A

[Fe(H2O)6]3+ + 3OH- —> Fe(H2O)3(OH)3 + 3H2O

The orange solution forms a brown precipitate.

49
Q

Give the equation for the reaction of Cu(II) ions with excess NaOH

A

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

A-Level Chemistry (9 decks)

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