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OCR Chemistry > 5.3 TRANSITION METALS > Flashcards

5.3 TRANSITION METALS Flashcards

1
Q

State the two types of precipitation reactions transition metals can undergo

A

1) Sodium hydroxide + transition metal
2) Ammonia + transition metal

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2
Q

State the colour of Cu2+ / Copper solution

A
  • Blue
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3
Q

State the colour of Fe2+ / Iron(II) solution

A
  • Green
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4
Q

State the colour of Fe3+ / Iron(III) solution

A
  • Yellow
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5
Q

State the colour of Mn2+ / Manganese solution

A
  • Pink
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6
Q

State the colour of Co2+ / Cobalt solution

A
  • Pink
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7
Q

State the colour of Cr3+ / Chronium solution

A
  • Green
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8
Q

State the observation of Cu2+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Blue precipitate forms
  • no change with excess NaOH
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9
Q

State the observation of Fe2+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Green precipitate forms
  • No change with excess NaOH
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10
Q

State the observation of Fe3+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Brown precipitate forms
  • No change with excess NaOH
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11
Q

State the observation of Mn2+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Brown precipitate forms
  • No change with excess NaOH
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12
Q

State the observation of Co2+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Blue precipitate forms
  • No change with excess NaOH
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13
Q

State the observation of Cr3+ with dropwise then excess aqueous NaOH/ Sodium hydroxide

A
  • Green precipitate forms
  • Precipitate dissolves in excess NaOH
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14
Q

State the observation of Cu2+ with dropwise then excess aqueous NH3/Ammonia

A
  • Blue precipitate forms
  • Deep blue solution forms with excess NH3
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15
Q

State the observation of Fe2+ with dropwise then excess aqueous NH3/Ammonia

A
  • Green precipitate forms
  • No change with excess NH3
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16
Q

State the observation of Fe3+ with dropwise then excess aqueous NH3/Ammonia

A
  • Brown precipitate forms
  • No change with excess NH3
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17
Q

State the observation of Mn2+ with dropwise then excess aqueous NH3/Ammonia

A
  • Brown precipitate forms
  • No change with excess NH3
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18
Q

State the observation of Co2+ with dropwise then excess aqueous NH3/Ammonia

A
  • Blue precipitate forms
  • No change with excess NH3
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19
Q

State the observation of Cr3+ with dropwise then excess aqueous NH3/Ammonia

A
  • Green precipitate forms
  • Purple solution forms with excess NH3
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20
Q

Define transition element

A
  • A d-block element that has an incomplete d-sub-shell when a stable ion
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21
Q

State the two elements are not classed as a transition element/metal

A
  • Zinc Zn2+
  • Scandium Sc3+
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22
Q

State the electron configuration to explain why scandium 3+ is not a transition element/metal

A
  • Scandium’s d-orbital is empty
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23
Q

State the electron configuration to explain why zinc 2+ is not a transition element/metal

A
  • Zinc’s d-orbital is full/complete
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24
Q

Give two examples of transition metals as catalysts

A

1) MnO2 catalyses the decompostion of H202
2) Cu2+ catalyses the reaction of Zn with acids

25
Q

Give two examples of transition elements with variable oxidation states

A

1) Fe2+ and Fe3+
2) Cr2+ and Cr3+ and Cr6+

26
Q

State an advantage and disadvantage of using transition metals as catalysts

A
  • Reduces energy usage which improves profits
  • However, they are toxic
27
Q

Define complex

A
  • A central metal ion surrounded by ligands
28
Q

Define ligand

A
  • An atom, ion or molecule which can donate a lone pair of electrons
29
Q

State the type of bonding used in complex formation

A
  • Co-ordinate/dative covalent
30
Q

Define co-ordination number

A
  • The number of co-ordinate bonds formed to a central metal ion
31
Q

Define bidentate ligand

A
  • A ligand that donates two electron pairs to a metal ion to form two co-ordinate bonds with the metal ion
32
Q

Define monodetate ligand

A
  • A ligand that donates one electron pair to a metal ion to form one co-ordinate bond with the metal ion
33
Q

Draw the two optical isomers of the complex ion ethandioate and state the co-ordinate number

34
Q

Draw the two optical isomers of the complex ion and state the co-ordinate number

35
Q

State what is required for cis-trans isomerism in square planar complexes

A
  • Four ligands where two are the same and the other two are the same
36
Q

State what is required for cis-trans isomerism in octahedral complexes

A
  • Six ligands where four are the same and the other two are the same
37
Q

State what is required for optical isomerism in octahedral complexes

A
  • Three bidentate ligands
38
Q

Describe the advantages and disadvantages of the use of cisplatin

A
  • Anti-cancer drug used in chemotherapy
  • Binds to the DNA in cancer cells to prevent division and stop cancer
  • However can cause hairloss, sickness and fatigue if it binds to healthy cells
39
Q

Define ligand substitution

A
  • A reaction where one ligand is substituted for another ligand in a complex ion
40
Q

Explain the importance of iron in haemoglobin in terms of ligand substitution

A
  • O₂ is a ligand that datively/co-ordinately bonds with Fe²⁺ so that oxygen can be carried in the blood
  • When required, O₂ is released
41
Q

Explain why carbon monoxide is toxic in terms of ligand substitution

A
  • CO is a ligand that datively/co-ordinately bonds with Fe²⁺ in haemoglobin
  • These are stronger than the ones O₂ forms with Fe²⁺ in haemoglobin
  • This prevents O₂ from bonding to it
42
Q

State the three typical reaction of transition metals

A

1) Percipitation
2) Ligand substitution
3) Redox

43
Q

Draw out all the reactions of iron as a transition metal

44
Q

Draw out all the reactions of copper as a transition metal

45
Q

Draw out all the reactions of chronium as a transition metal

46
Q

Draw out all the reactions of cobalt as a transition metal

47
Q

Draw out all the reactions of manganese as a transition metal

48
Q

Test for Cu²⁺ ions

A
  • Cu²⁺ is a blue solution
  • Dropwise NH₃ or OH⁻ produces a blue percipitate
  • Excess NH₃ dissolves the blue percipitate to form a blue solution
  • No change with excess OH⁻
49
Q

Test for Fe²⁺ ions

A
  • Fe²⁺ is a green solution
  • Dropwise NH₃ or OH⁻ produces a green percipitate
  • No change with excess NH₃
  • No change with excess OH⁻
50
Q

Test for Fe³⁺ ions

A
  • Fe³⁺ is a yellow solution
  • Dropwise NH₃ or OH⁻ produces a brown percipitate
  • No change with excess NH₃
  • No change with excess OH⁻
51
Q

Test for Mn²⁺ ions

A
  • Mn²⁺ is a pink solution
  • Dropwise NH₃ or OH⁻ produces a brown percipitate
  • No change with excess NH₃
  • No change with excess OH⁻
52
Q

Test for Cr³⁺ ions

A
  • Cr³⁺ is a green solution
  • Dropwise NH₃ or OH⁻ produces a green percipitate
  • Excess NH₃ dissolves the green percipitate to form a purple solution
  • Excess OH⁻ dissolves the green percipitate to form a green solution
53
Q

Test for NH₄⁺

A
  • Add NaOH and gentle warming
  • Distinctive ammonia gas smell will turn red litmus paper into blue
54
Q

Test for CO₃²⁻

A
  • Add strong acid
  • Produces carbon dioxide gas which turns limewater cloudy
55
Q

Test for SO₄²⁻

A
  • Add barium chloride
  • A white percipitate of barium sulfate forms
56
Q

Test for Cl⁻,Br⁻,I⁻ ions

57
Q

State in which order 4s electrons are added and removed

A
  • added first and removed first

OCR Chemistry (13 decks)

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