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Advanced Higher Chemistry > Unit 1 Inorganic Chemistry: Key Area 3 - Transition Metals > Flashcards

Unit 1 Inorganic Chemistry: Key Area 3 - Transition Metals Flashcards

1
Q

What is the definition of a transition metal?

A

Elements that have an incomplete d sub-shell in at least one of their ions.

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2
Q

What principle does the filling of the d orbitals follow in transition metals?

A

The filling of the d orbitals follows the aufbau principle.

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3
Q

What is the exception of the filling of d orbitals by the Aufbau principle?

A

Copper and Chromium which are due to the special stability associated with the d subshell being half- filled or completely filled.

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4
Q

What elements do not fit the definition for transition metals and why is this?

A

Scandium and zinc as they do not show metal ion characteristics and therefore do not exhibit colour.

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5
Q

What is oxidation?

A

A loss of electrons, gain of oxygen or an increase in oxidation number.

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6
Q

What is reduction?

A

A gain of electrons, loss of oxygen or decrease in oxidation number.

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7
Q

What is the rule for checking if oxidation has occurred?

A

Eat Only Hot Curries:

  • Electrons
  • Oxygen
  • Hydrogen
  • Charge
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8
Q

When atoms from the first row of the transition elements form ions, what are lost first.

A

When atoms from the first row of the transition elements form ions, it is the 4s electrons that are lost first rather than the 3d electrons.

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9
Q

When is an element said to be in a particular oxidation state?

A

An element is said to be in a particular oxidation state when it has a specific oxidation number.

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10
Q

How can the oxidation number be determined?

A
  • Uncombined elements have an oxidation number of 0.
  • Ions containing single atoms have an oxidation number that is the same as the charge on the ion.
  • In most of its compounds, oxygen has an oxidation number of -2.
  • In most of its compounds, hydrogen has an oxidation number of +1.
  • The sum of all the oxidation numbers of all the atoms in a molecule or neutral ion must add up to zero.
  • The sum of all the oxidation numbers of all the atoms in a polyatomic ion must be equal to the charge on the ion.
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11
Q

What do transition metals have in terms of stability?

A

Transition metals have variable oxidation states in terms of differing stability.

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12
Q

What is the charge on a cyanide (CN) ion?

A

-1

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13
Q

What can compounds of the same transition metals in different oxidation states have?

A

Different colours

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14
Q

Compounds containing metals in high oxidation states are often what?

A

Oxidising agents

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15
Q

Compounds containing metals in low oxidation states are often what?

A

Reducing agents

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16
Q

What do transition metal complexes consist of?

A

A central transition metal ion surrounded by ligands.

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17
Q

What are ligands?

A

Ligands may be negative ions or molecules with non-bonding pairs of electrons that they donate to the central metal atom or ion, forming dative covalent bonds.

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18
Q

What can ligands be classified as?

A

Ligands can be classified as monodentate, bidentate, up to hexadentate.

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19
Q

What are the key features of a monodentate ligand?

A
  • Can only form 1 bond with the central metal atom/ion.
  • One binding site
  • e.g. ammonia and chlorine.
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20
Q

What are the key features of a bidentate ligand?

A
  • Can form 2 bonds with the central metal atom/ion.
  • Two binding sites.
  • e.g. diaminoethane and oxalate ion.
  • WILL ALWAYS USE BOTH BINDING SITES.
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21
Q

What are the key features of a tridentate ligand?

A
  • Can form 3 bonds with the central metal atom/ion.
  • Three binding sites.
  • e.g. 1,4,7-triazaheptane.
  • WILL ALWAYS USE ALL THEEE BINDING SITES.
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22
Q

What are the key features of a hexodentate ligand?

A
  • Can form 6 bonds with the central metal atom/ion.
  • Six binding sites.
  • e.g. Chlorophyll and haemoglobin.
  • WILL ALWAYS USE ALL SIX BINDING SITES.
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23
Q

What is a coordination number?

A

The number of lone pairs bonded to the central metal ion.

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24
Q

What is the most common coordination number?

A

6

25
Q

Tyfytutf

A

Bjhbh

26
Q

Crctrd

A

Uhunun

27
Q

Rcrdrdrd

A

Ininino

28
Q

Vgggvuyv

A

Bgcytv

29
Q

Vhghgyg

A

Ihbhinui

30
Q

What is 1st rule of naming complexes?

A

If the complex is a salt, the name of the positive ion (cation) precedes the name of the negative ion (anion).

31
Q

What is 2nd rule of naming complexes?

A

The name of the complex part (ion or neutral) consists of two parts written as one word. The ligand is named first and the central metal ion second.

32
Q

What is 3rd rule of naming complexes?

A

The ligand name is preceded by a greek prefix showing the number of ligands (di, tri etc.).

33
Q

What are common ligand names?

A
  • Chloride - Chlorido
  • Oxide - Oxido
  • Cyanide - Cyanido
  • Hydroxide - Hydroxido
  • Ammonia - Ammine
  • Water - Aqua
  • Carbon Monoxide - Carbonyl
34
Q

What do negative ions end in?

A

‘O‘.

35
Q

What is 4th rule of naming complexes?

A

The metal name is followed by the oxidation number in brackets.

36
Q

What is 5th rule of naming complexes?

A

If the complex ion, is negative, the metal name is followed by the suffix - ate.

37
Q

What are common negative complex ion names?

A
  • Vanadium - Vanadate
  • Chromium - Chromate
  • Manganese - Manganate
  • Iron - Ferrate
  • Cobalt - Cobaltate
  • Nickel - Nickelate
  • Copper - Cuprate
  • Silver - Argentate
  • Gold - Aurarate
  • Lead - Plumbate
38
Q

When a colour change occurs in a transition metal reaction, what is there a change in at least one of?

A

1) The nature of the TM element
2) Oxidation state
3) Co-ordination number
4) Type of ligand

39
Q

Why are TM complexes coloured?

A

The 5d orbitals in an isolated TM atom are degenerate. In complexes, the d sub-level splits into two sets of orbitals of different energy and the electron transitions that take place between them are responsible for their colours.

40
Q

What is the difference in energy between the two sets of orbitals called

A

Crystal field strength (Δ).

41
Q

What does the crystal field strength depend on?

A

The position of the ligand in the spectrochemical series.

42
Q

What is the order of the spectrochemical series?

A

Strongest ligand first (ligand that gives the largestvalue of Δ).

43
Q

What is the value of Δ and λ for a stronger Crystal field strength?

A

Larger Δ and shorter λ.

44
Q

What is the value of Δ and λ for a weaker Crystal field strength?

A

Smaller Δ and longer λ.

45
Q

How can the colours of many transition metals complexes be explained?

A

Colours of many transition metal complexes can be explained in terms of d-d transitions.

46
Q

When do d-d transistions occur?

A

When electrons are promoted from the lower energy d orbital to higher levels. This can be the result of radiation of the correct enefgy being absorbed by the electron.

47
Q

What is the colour of many transistion metal complexes due to?

A

d-d transistions

48
Q

What is the equation for the origin of colour?

A

ΔE = hf

49
Q

If light of one colour is absorbed then what will be observed.

A

If light of one colour is absorbed, then the complementary colour will be observed.

50
Q

When can visible spectroscopy used?

A

If energy is absorbed in the visible region of the EM spectrum a coloured compound is produced therefore visible spectroscopy can be used.

51
Q

When can UV spectroscopy be used?

A

If enefgy is absorbed in the UV region of the EM spectrum the compound will appear colourless therefore UV spectroscopy can be used.

52
Q

What can transistion metals and their compounds act as?

A

Catalysts

53
Q

What are hetrogeneous catalysts?

A

Catalysts that are in a different state to the reactants.

54
Q

What are homogeneous catalysts?

A

Catalysts that are in the same state as the reactants.

55
Q

What happens in Stage 1 (absorption) of catalysts by transistion metals?

A

Reactant lands on an active site and forms bonds with the catalysts.

56
Q

What happens in stage 2 + 3 (reaction) of catalyst by transistion metals?

A

Absorbed substance may be held on the surface in just the right orientation for a reaction to occur. This increaces the chances of favourable collisions taking place.

57
Q

What happens in stage 4 (desorption) of catalysts by transistion metals?

A

Products are then released from the active sites.

58
Q

What happens in catalysts by transistion metals.

A

The presence of unpaired d electrons or unfilled d orbitals allows intermediate complexes to form. This weakens the covalent bonds within reactant molecules.
This provides a reaction pathway of lower activation energy.

59
Q

What type of oxidation states do transistion metals have and what can this provide.

A

Transition metals also have variable oxidation states, which can provide alternative pathways.

Advanced Higher Chemistry (6 decks)

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