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Chemistry Inorganic > Transition metals > Flashcards

Transition metals Flashcards

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1
Q

Define transition metals

A

Metals that can form 1/more stable ions w/ partially filled d sub-shells

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2
Q

What causes the special chemical properties of T-metals?

A

Incomplete d sub-shell

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3
Q

Why is scandium not a t-metal?

A
  • Only forms 1 ion: Sc3+
  • Empty d sub-level
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4
Q

Why is zinc not a t-metal?

A
  • Only forms 1 ion: Zn2+
  • Has full d sub-level
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5
Q

When ions are formed which e- are removed first?

A

S then D

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6
Q

State the physical properties of t-metals

A
  • High density
  • High MP + BP
  • Ionic radii = same
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7
Q

State the chemical properties of t-metals

A
  • Form complex ions
  • Form coloured ions
  • Good catalyst
  • Variable oxidation state
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8
Q

Why do t-metals show variable oxidation states?

A
  • Energy level of 4s + 3d sub-level are v close to one another
  • So diff. no. e- gained or lost using similar amounts of energy
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9
Q

Cu2+

A

Blue

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10
Q

Ni2+

A

Green

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11
Q

Co2+

A

Pink

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12
Q

Fe2+

A

Pale green

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13
Q

Mn2+

A

Pink

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14
Q

V2+

A

Violet

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15
Q

Fe3+

A

Yellow

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16
Q

Cr3+

A

Green/violet

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17
Q

V3+

A

Green

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18
Q

VO2+

A

Blue

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19
Q

VO2+

A

Yellow

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20
Q

Cr2O72+

A

Orange

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21
Q

MnO4-

A

Purple

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22
Q

Define complex

A

Central metal atom/ion surrounded by co-ordinately bonded ligands

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23
Q

Define co-ordinate bond

A

Covelant bond where both e- in shared pair come from same atom/ligand

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24
Q

Define ligand

A

Atom, ion or molecule that donates pair of e- to central t-metal to form co-ordinate bond

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25
Q

Define co-ordinate no.

A

No. of co-ordinate bonds formed w/ central metal ion

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26
Q

Which ligands do t-metals form octahedral complexes w/?

A
  • Small ligands
  • Eg. H2O, NH3
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27
Q

Which ligands do t-metals form tetrahedral complexes w/?

A
  • Larger ligands
  • eg. Cl-
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28
Q

What shape does 6 co-ordinate bonds form + what is the bond angle?

A
  • Octahedral
  • 90º
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29
Q

What shapes do 4 co-ordinate bonds form + what is the bond angle?

A
  • Tetrahedral: 109.5º
  • Square planar: 90º (cisplatin)
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30
Q

What shape does some silver complexes w/ 2 co-ordinate bonds form + what is the bond angle?

A
  • Linear
  • 180º
31
Q

What is the overall charge on the complex ion?

A

Total oxidation state

32
Q

Oxidation state of metal ion equation

A

Oxidation state of metal ion = total oxidation state - sum of oxidation states of ligands

33
Q

Give an example of a linear complex + what it’s used for

A
  • [Ag(NH3)2]+
  • Tollen’s reagent
34
Q

Define monodentate

Give examples

A

Ligand that can only form 1 co-ordinate bond

H2O, NH3, Cl-

35
Q

Define multidentate

Give examples

A

Ligand that can form more than 1 co-ordinate bond

EDTA4-

36
Q

What does EDTA4- stand for?

A

ethane diomine tetra acetate

37
Q

Define bidentate

Give examples

A

Multidentate ligands that form 2 co-ordinate bonds

  • ethane-1,2-diamine (H2NCH2CH2NH2)
  • ethandioate (C2O42-)
38
Q

What is haem?

A

Iron (II) complex w/ multidentate ligand

39
Q

Why is haemoglobin important?

A

O2 co-ordinately bonds to Fe2+ to form oxyhaemoglobin + is carries O2 round body in blood

40
Q

Why is CO dangerous?

A
  • Co-ordinately bonds to Fe2+ instead of O2, forming carboxyhaemoglobin
  • CO is a strong ligand + doesn’t readily exchange w/ H2O/O2 ligands
  • Unable to transport O2 round body
  • Causes: headaches, dizziness + death
41
Q

Define optical isomerism

A

Ions can exist in 2 forms that are non-superimposable mirror images

42
Q

Which complexes show optical isomerism?

A

Octahedral complexes w/ bidentate ligands

43
Q

Which complexes form + display cis-trans isomerism?

A
  • Octahedral complexes (monodentate ligand)
  • Square planar
44
Q

What is the cis isomer of cisplatin used for?

A

Anti-cancer drugs

45
Q

When does the 3d orbital split into 2 diff energy levels?

A

Ligands bond to ions + causes orbitals to gain energy

46
Q

Which orbitals do e- tend to occupy?

A

Lower orbitals

47
Q

Where does e- get energy from to jump up to the higher orbitals?

A

Visible light

48
Q

What happens when visible light hits a t-metal ion?

A

d e- move from ground state to excited state

49
Q

How does colour arise in t-metals?

A
  • Some wavelengths of visible light are absorbed
  • Rest of freq. transmitted/reflected
50
Q

What does the freq. absorbed depend on?

A

Size of the energy gap ΔE

51
Q

What happens when the frequencies are reflected/transmitted?

A

Freq combines to make compliment of colour of absorbed freq - colour you see

52
Q

What is the colour when there are no 3d e- or 3d sub-level is full?

A
  • Colourless
  • Bc no e- will jump so no energy absorbed
53
Q

The larger the gap the___ the feq. of light that is absorbed

A

Higher

54
Q

How can the colour of a complex be altered?

A

By change size of energy gap

  • Change in:
  • Oxidation state
  • Co-ordination no.
  • Ligand
55
Q

What can be used to find the conc of t-metal ions?

A
  • Spectroscopy
  • White light shone through filter, chosen to only let colour of light absorbed by sample
  • Light passes through sample to colorimeter - calculates how much light is absorbed
  • More conc = more light absorbed
56
Q

What must be produced before finding the unknown conc of a sample?

A
  • Calibration curve - measuring absorbance of known conc of solutions + plot on graph
  • Measure absorbance of sample + read off graph
57
Q

Define ligand substitution

What does it usually result in?

A
  • Ligands changing places w/ another
  • Colour change
58
Q

What happens to the co-ordination no. + shape of a complex ion if the ligands are similar size + same charge?

A

Nothing

59
Q

Why is substitution btw H2O + NH3 easy?

A
  • Similar size
  • Both uncharged
60
Q

What happens to the co-ordination no. + shape of a complex ion if the ligands are diff. size?

A

Changes

61
Q

Why is the enthalpy change for a ligand exchange reaction v small?

A

Strength of bonds being broken is v similar to bonds formed

62
Q

What is the chelate effect?

A

When monodentate ligands are substituted w/ bidentate + multidentate ligands, inc in stability, no. particles inc, so greater entropy - more likely to occur

63
Q

What is used to reduce vanadium ions?

A

Zinc metal in acidic solution

64
Q

How is the stability of an ion affected the larger the redox potential?

A

Less stable, more likely to be reduced

65
Q

How is the redox potential affected in an acidic solution?

A

Larger redox potential, easier to reduce

66
Q

Outline how to carry out a titration to find out how much oxidising agent is needed to react w/ a quantity of reducing agent

A
  • Measure out reducing agent using pipette + put into CF
  • Using measuring cylinder, add dliute sulfuric acid to flask
  • Add oxidising agent (aqueous potassium manganate) to reducing agent using burette
  • Add until the mixture changes colour to purple
67
Q

How do transition metals work as catalysts?

A

Changing oxidation states

68
Q

Outline heterogeneous catalyst

A
  • Diff phase to reactants
  • Reaction happens at active site on surface of catalyst
  • Support mediums used to max. SA + minimise cost
69
Q

Give examples when heterogenous catalysts are used

A
  • Iron in haber process to make ammonia
  • Vanadium oxide in contact process to make sulfuric acid
70
Q

What is the problem in using hetrogenous catalysts?

Give example

A
  • Impurities bind to catalyst surface + block reactants from being adsorbed - catalyst poisoning
  • Reduces SA, slowing down reaction
  • Inc cost
  • Sulfur poisons iron catalyst in haber process, H produced from methane, sulfur reacts w/ iron to produce iron sulfide
71
Q

Outline the process of heterogenous catalyst

A
  • Diffusion
  • Adsorption
  • React (bonds broken/formed)
  • Desorption
  • Diffusion
72
Q

Outline homogneous catalyst

A
  • Same phase as reactants
  • Work by forming intermediate species which react to form products + re-form catalyst
73
Q

Why is the reaction btw iodide ions + peroxidisulfate slow?

How can you over come this problem?

A
  • Both ions -ve charged so repel, less likely to collide
  • Add Fe2+ ions bc +ve ion so no repulsion
74
Q

Define autocatalyst

A

Product of reaction catalyses reaction

Chemistry Inorganic (7 decks)

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