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A LEVEL CHEM > Topic 15- Transitition Metals > Flashcards

Topic 15- Transitition Metals Flashcards

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1
Q

Where can Transition Metals be found?

A

d-block

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2
Q

Describe the electron configuration of Chromium

A

one electron in each orbital of 3d sub shell (3d5) and ONE in the 4s. This is due to greater stability having an electron in each orbital of the 3d sub shell.

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3
Q

When transition metals form positive ions which electrons from which shells are removed first?

A

outer ‘s’ electrons are removed first. Then the d electrons.

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4
Q

Which metals aren’t transition metals and WHY?

A

Scandium and Zinc. Sc only forms a positive ion (Sc 3+) which has an empty d subshell. Zn only forms Zn 2+ which results in a full d subshell

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5
Q

Define a Transition metal

A

d-block elements that can form one or more STABLE ions with incompletely filled d-orbitals.

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6
Q

What is a complex ion?

A

A metal ion surrounded by dative covalently bonded ligands.

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7
Q

What is a ligand?

A

An atom, ion or molecule that donates a lone pair of electrons to a central metal atom/ion.

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8
Q

Name the 3 types of ligand

A

Monodentate (1 lone pair)
Bidentate (2 lone pairs)
Multidentate (more than two lone pairs)

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9
Q

How can you calculate the overall charge on a complex ion?

A

work out oxidation number which is

total oxidation number - sum of charges of ligands

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10
Q

What is the coordination number?

A

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

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11
Q

What 3 shapes can complexes form?

A

Square planar-90
Tetrahedral-109.5
Octahedral-90

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12
Q

What happens to the 3d sub shell as ligands come and bond to the ions?

A

the 3d sub shell split into two different energy levels?

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13
Q

Why is Zn not a transition metal?

A

Zn can only form a +2 ion where the Zn2+ ion has a complete d orbital.

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14
Q

Why is Sc not a transition metal?

A

Sc can only form a +3 ion. In this ion Sc3+ has an empty d orbital so isn’t a transition metal.

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15
Q

Describe the successive ionization energies for the elements Sc to Zn.

A

They show a gradual increase in ionisation energy until all the 4s and 3d electrons have been removed.
Then a big jump as e-‘s removed from inner core electrons.

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16
Q

Colour changes arise from changes in…

A

Oxidation state, coordination number, ligand.

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17
Q

What is cisplatin?

A

An anti-cancer drug

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18
Q

Name properties of Transition Metals

A

Hard, Shiny, Good thermal & electrical conductors.

Multiple oxidation states, form coloured ions in solution, good catalysts, form complexes with ligands.

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19
Q

What is a heterogeneous catalyst?

A

A catalyst which is in a different phase to the reactants (e.g. solid and liquid)

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20
Q

If we increase the surface area, the rate of reaction increases. Why is this?

A

More reagents can adsorb

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21
Q

The contact process converts …. into ….. which is then converted to …… ….. using water. The catalyst is…

A

The contact process converts Sulfur dioxide into sulfur trioxide and then into sulfuric acid. The catalyst is V2O5

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22
Q

The contact process is an example of a reaction that uses a ……… ……

A

Heterogeneous catalyst

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23
Q

Catalyst poisoning can happen when …

A

Another molecule irreversibly adsorbs onto the surface of the catalyst as it stops reactants from adsorbing.

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24
Q

What is a homogeneous catalyst?

A

A catalyst which is in the same phase as the reactant e.g. two aqueous solutions

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25
Q

How do catalysts work?

A

By changing oxidation state. as they donate or accept electrons to oxidise or reduce a species.

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26
Q

What colour is Vanadium (IV) (VO2+)

A

Blue

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27
Q

What colour is Vanadium (II)

A

Violet

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28
Q

What colour is Vanadium (III)

A

Green

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29
Q

What colour is Vanadium (V) (VO+)

A

Yellow

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30
Q

Transition metals can have multiple …. …. in a number of …… states

A

Transition metals can have multiple stable ions in a number of oxidation states.

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31
Q

How can you prepare different ions of vanadium?

A

By successive reduction with zinc in acid solution.

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32
Q

What do redox potentials show you?

A

How easily a metal can be reduced.

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33
Q

Name 3 common ligands

A

H2O, NH3, Cl- (biggest)

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34
Q

The coordination number doesn’t change when substituting water for ammonia. Why?

A

Because they are of a similar size (if Cl- was substituted then it would change)

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35
Q

A ligand that can form two bonds is called….

A

Bidentate

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36
Q

A ligand that can form one bond is called….

A

Monodentate

37
Q

A ligand that can form multiple bonds is called….

A

Multidentate

38
Q

What does denticity describe?

A

The number of dative bonds that can be formed with a transition metal by one ligand.

39
Q

Name 2 factors that influence the shape of complex ions.

A
  1. Metal

2. Ligand

40
Q

What type of ligand is H₂NCH₂CH₂NH₂

A

bidentate

41
Q

What colour change would you observe in the following reaction? [Cu(H₂O)₆]²⁺ + 4Cl ⁻ ⇌ [CuCl₄]²⁻ + 6H₂O

A

pale blue solution to yellow/green solution

42
Q
  1. In which order are the third and fourth level s, p and d electrons lost? (First:Last)
A

4s, 3d, 3p, 3s

43
Q

In which order are the third and fourth level s, p and d electrons filled in? (First:Last)

A

3s, 3p, 4s, 3d

44
Q

Describe what a catalyst in catalytic converters in motor cars does.

A

It converts nitrogen oxides and carbon monoxide to nitrogen and carbon dioxide by adsorbing the reactants on its surface so weakening their bonds

45
Q

Describe Cis-platin

A

3​ )​ Pt(NH​3​ )​2​Cl​2 with ​cis geometry. An anticancer compound that binds to the two strands of DNA during cell division process. This prevents them from separating and hence stops the cell division.

46
Q

Ligand exchange?

A

​ A reaction in which a ligand is substituted by another ligand.

47
Q

Adsorption

A

​The process of forming weak bonds by reactants to a surface of a solid catalyst

48
Q

Desorption

A

The reverse process to adsorption. Adsorbed molecules leave the surface

49
Q

Autocatalysis

A

When a product of a reaction catalyses the reaction, e.g. Mn​ 2+ in oxidation of c2o4 (2-) with Mno4- under acidic conditions.

50
Q

Colour of Cr3+?

A

Green

51
Q

Colour of Fe3+

A

yellow

52
Q

Colour of Fe2+

A

Pale green

53
Q

Colour of Co2+

A

pink

54
Q

Colour of Cu2+

A

pale blue

55
Q

Colour of Cr2O7 ^2-

A

Orange

56
Q

How does the fact that transition metals have partially filled d-orbitals help it act as a heterogenous catalyst?

A

The orbitals allow reactant molecules to make weak bonds to the catalyst

57
Q

Explain how adsorption helps to catalyse the reaction.

A

The surface of the catalyst activates the molecules, weakening the bonds between the atoms in the reactants, making them easier to break and reform as products

58
Q

What is a dative covalent bond?

A

A covalent bond in which both electrons in the shared pair come from the same atom

59
Q

What shape molecule is cis-platin?

A

Square Planar

60
Q

What colour is the ion of a CrO4-?

A

Yellow

61
Q

What colour is the ion of a Cr3+?

A

Violet is surrounded by 6 water ligands

Green if substituted with impurities ie Cl-

62
Q

What colour is the ion Cr2+

A

Blue

63
Q

Chromium Hydroxide is Amphoteric. What does this mean?

A

Reacts with both acids and bases

64
Q

If you add excess ammonia to chromium hydroxide precipitate a …… ….. …. occurs

A

If you add excess ammonia to chromium hydroxide precipitate a ligand exchange reaction(substitution) occurs

65
Q

Transition metal ions form tetrahedral complexes with …….. ligands such as …

A

Transition metal ions form tetrahedral complexes with LARGE ligands such as Cl-

66
Q

What type of ligand is NH2CH2CH2NH2 ?

A

Bidentate

67
Q

What type of ligand is EDTA 4- ?

A

Multidentate

68
Q

The catalysed reaction with a homogeneous catalyst proceeds via an ………. …….

A

Homogeneous catalysts proceed via an intermediate species

69
Q

Why do transition metals show multiple oxidation numbers?

A

able to donate and receive electrons and are
able to oxidize and reduce because partially filled sub-shells of d electrons easily lose or gain electrons. Energy differences between the oxidation states are small

70
Q

What is the reason behind a CHANGE in colour of an ion?

A

Changing a ligand or changing the coordination number as it alters energy split therefore the frequency of light absorbed

71
Q

Which transition metal ion can form LINEAR complexes?

A

Ag+ , e.g. [Ag(NH3)2]+,[Ag(S2O3)2]3- and

[Ag(CN)2]- (all colourless)

72
Q

Why does Cisplatin have to have cis geometry?

A

The cisplatin version only works as two chloride ions are displaced and the molecule joins on to the DNA.
Transplatin IS TOXIC

73
Q

Is there an overall change in oxidation number during a catalysed heterogeneous reaction?

A

NO

74
Q

Copper(II) Sulfate solution is blue. This is because…

A

electrons absorb light in the red region of the spectrum and the residual frequencies are observed.

75
Q

What can result in the change in colour of transition metal ions?

A

Change in ligand
Change in oxidation state
Change in coordination number

76
Q

How does Carbon monoxide poisoning occur?

A

CO replaces an oxygen/H2O molecule which forms a STRONGER bond with the iron so won’t readily exchange with oxygen so Haemoglobin can’t transport oxygen anymore.

77
Q

………. ligands will almost always displace ……… ligands at a metal centre

A

multidentate ligands will almost always displace monodentate ligands at a metal centre

78
Q

Which 3 metal ions form linear complexes?

A

Cu, Ag, Au

79
Q

How do variable oxidation states arise?

A

Arises from the similar energies required for removal of 3d and 4s electrons.

80
Q

What is the colour change of [CuCl4] 2- —-> [Cu(H2O)6] 2+

A

Yellow to blue

81
Q

What is the colour change of [Cu(NH3)4(H2O)2) 2+ —-> [Cu(H2O)6] 2+

A

Deep blue to pale blue

82
Q

What is the colour change of [CoCl4] 2- —–> [Co(H2O)6] 2+

A

Blue to Red

83
Q

Which two metal hydroxides undergo a ligand exchange reaction in excess ammonia?

A

[Co(OH)2(H2O)4] + 6NH3 -> [Co(NH3)6] 2+
blue precipitate dissolves to form a yellow-brown sol
[Cu(OH)2(H2O)4] + 4NH3 -> [Cu(NH3)4(H2O)2] 2+
blue precipitate goes to deep blue solution

84
Q

Colour change of

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

A

Pale blue solution turns to blue precipitate.

85
Q

Colour change of

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

A

Pale green solution turns to green precipitate which darkens on standing

86
Q

Colour change of

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

A

Yellow solution to orange precipitate and darkens on standing

87
Q

Colour change of

[Co(H2O)6]2+ +2OH- –> [Co(OH)2(H2O)4] +2H2O

A

Pale pink solution to a blue precipitate which turns brown on standing.

88
Q

To form a compound or complex containing an ion the energy given out needs to…… than the energy taken to remove the outer electrons.

A

Energy given out should be greater than energy taken to remove outer electrons

A LEVEL CHEM (34 decks)

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