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A Level > 5.3 > Flashcards

5.3 Flashcards

1
Q

Transition metals

A

Metals that have an incomplete d subshell

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2
Q

What are the exceptions in transition metals?

A
  • Sc and Zn dont count as they have full d orbitals

- Cr and Cu have 4s1 subshell to make the 3d subshell more stable by donating an electron to it

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3
Q

What are the physical properties of transition metals?

A
  • Lustrous
  • High densities
  • High melting and boiling points
  • Conduct electricity (giant metallic lattice structure)
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4
Q

Colour of Cr2+

A

Blue

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5
Q

Colour of Mn2+

A

Light pink

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6
Q

Colour of Cr2O7 2-

A

Orange

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7
Q

Colour of MnO4-

A

dark purple

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8
Q

Colour of Fe2+

A

Pale green

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9
Q

Colour of Fe3+

A

Pale yellow

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10
Q

Colour of Co2+

A

Pink

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11
Q

Colour of Co3+

A

light green

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12
Q

Colour of Ni2+

A

green

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13
Q

Colour of Cu2+

A

Blue

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14
Q

What is an example of a disproportionation reaction?

A

Cu2O + H2SO4 —-> Cu + CuSO4 + H2O

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15
Q

What causes the colour in transition metals?

A

Caused by the incomplete d subshell

We are seeing the colour that is reflected, not the colour that is absorbed

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16
Q

How does a transition metal catalyst work?

A

Reactant adsorb onto the surface of the metal and are held in place while the reaction happens
Transition metals can change oxidation state so can act as an intermediate that has a lower activation energy

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17
Q

Transition metal catalyst for the Haber process?

A

Iron

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18
Q

Transition metal catalyst for the contact process?

A

V2O5

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19
Q

Transition metal catalyst for hydrogenation of alkenes?

A

Nickel

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20
Q

Transition metal catalyst for the decomposition of H2O2?

A

MnO2

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21
Q

Transition metal catalyst for obtaining hydrogen from zinc?

A

Copper

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22
Q

What is a complex ion?

A

A transition metal bonded to ligands with coordinate bonds

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23
Q

Coordinate bonds

A

Dative covalent bonds

24
Q

Ligand

A

Molecule that can donate a pair of electrons to a transition metal to form a coordinate bond

25
Q

Coordination number

A

Total number of coordinate bonds formed

26
Q

Lewis Base

A

An electron donor

Ligands are Lewis bases

27
Q

Bidentate ligands

A

NH2CH2CH2NH2 = ethane-1,2-diamine
shortened to ‘en’
OC=OC=OO

28
Q

Multidentate ligand

A

EDTA (+4)

29
Q

What are the benefits/risks of transition metals?

A

They reduce energy usage

They can be very toxic

30
Q

Cis/Trans isomers degrees

A

Cis- 90 degrees

Trans- 180 degrees

31
Q

Cis-platin

A

Anti-cancer drug
Binds to the DNA preventing cell division in cancer cells
But it has some unpleasant side effects such as hair loss, sickness and fatigue
Used in chemotherapy

32
Q

Optical isomers

A

Non-superimposable mirror images of each other

33
Q

[Cu(H2O)6]2+ and excess NH3

A

Ligand substitution
Pale blue to deep blue
[Cu(NH3)4(H2O)2]2+

34
Q

[Cu(H2O)6]2+ and excess Cl- (HCl)

A

Ligand substitution
Pale blue to green to yellow
[CuCl4]2-

35
Q

Why does Cl- substitute only 4 times?

A

Because it is bigger and has stronger repulsions

36
Q

[Cr(H2O)6]3+ and excess NH3

A 
Ligand substitution
Grey/green ppt
[Cr(H2O)3(OH)3]
Redissolves to a dark green solution with excess NH3
[Cr(NH3)6]3+
37
Q

How does haemoglobin work?

A

Fe2+ metal forms coordinate bonds with 4 nitrogens, a globin protein and can reversibly form one with oxygen
Carbon monoxide can take oxygens place as it forms stronger bonds, but binds irreversibly and causes oxygen starvation

38
Q

Cu2+ and NaOH dropwise

A

Precipitation reaction

Blue solution to blue gelatinous ppt

39
Q

Cu2+ and NH3 dropwise

A

Precipitation reaction
Blue solution to blue gelatinous ppt
Can redissolve

40
Q

Fe2+ and NaOH dropwise

A

Precipitation reaction
Pale green solution to green ppt
Turns rusty brown after long exposure to air

41
Q

Fe2+ and NH3 dropwise

A

Precipitation reaction

Pale green solution to dark green ppt

42
Q

Fe3+ and NaOH dropwise

A

Precipitation reaction
Pale yellow solution to rusty brown ppt
Same as with NH3

43
Q

Fe3+ and NH3 dropwise

A

Precipitation reaction
Pale yellow solution to rusty brown ppt
Same as with NaOH

44
Q

Mn2+ and NaOH dropwise

A

Precipitation reaction
Pale pink solution to brown ppt
Same as with NH3

45
Q

Mn2+ and NH3 dropwise

A

Precipitation reaction
Pale pink solution to brown ppt
Same as with NaOH

46
Q

Cr3+ and NaOH dropwise

A

Precipitation reaction
Green solution to green ppt
Can redissolve
Same as with NH3

47
Q

Cr3+ and NH3 dropwise

A

Precipitation reaction
Green solution to grey-green ppt
Can redissolve
Same as with NaOH

48
Q

Using transition metals as indicators in titrations, what is the endpoint colour change for MnO4- to Mn2+?

A

Purple to very pale pink/colourless

49
Q

Using transition metals as indicators in titrations, what is the endpoint colour change for Cr2O7 2- oxidising Fe2+?

A

Redox indicator is used

Violet/blue endpoint

50
Q

Using transition metals as indicators in titrations, what is the endpoint colour change for iodine and thiosulphate?

A

When the mixture becomes a pale yellow colour, iodine is added
Endpoint is from blue/black to colourless

51
Q

What is the test for transition metal ions?

A

React with NaOH or NH3 dropwise, and look for the colour change

52
Q

What is the test for the ammonium ion?

A

React with OH- to produce ammonia gas and H2O

It will turn damp red litmus paper blue

53
Q

What is the test for carbonate ions?

A

React with acid to give off CO2 gas

Bubble gas through limewater, it will turn cloudy

54
Q

What is the test for sulphate ions?

A

React with barium chloride, it will turn cloudy with a white precipitate

55
Q

What is the test for halide ions?

A

React with silver nitrate and dilute nitric acid

It will make white/cream/yellow ppt depending on halogen

56
Q

What order do you do the tests for ions?

A

Carbonate
Sulphate
Halide

A Level (25 decks)

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