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A- Level Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

1
Q

colour of V^(2+) (oxidation state 2)

A

purple

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2
Q

colour of V^(3+) (oxidation state 3)

A

blue

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3
Q

colour of VO^(2+) (oxidation state 4)

A

green

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4
Q

colour of VO2^(+) (oxidation state 5)

A

yellow

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5
Q

[Cu(H2O)6]^(2+) +2OH-/2NH3 —–>

products, type of reaction and colour change

A

[Cu(H2O)4(OH)2] + 2H2O/2NH4+
acid base reaction
pale blue sol——> blue ppt

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6
Q

[Cu(H2O)4(OH)2] + 4NH3(conc)———>

products, type of reaction and colour change

A

[Cu(NH3)4(H2O)2]^(2+) +2OH- and 2H2O
ligand substitution
blue ppt——-> deep blue solution

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7
Q

[Cu(H2O)6]^(2+) + 4Cl- ———–>

(products, type of reaction and colour change)

A

[CuCl4]^(2-) + 6H2O
coordination no. change
blue sol——> yellow sol (when there a mixture of the two it is green sol

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8
Q

Fe(H2O)6 + 2OH-/NH3——->

A

[Fe(H2O)4(OH-)2] + 2h2O/2nh4+

green sol—–> green ppt

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9
Q

[Fe(H2O)4(OH)2] when left in air —>

A

[Fe(H2O)3(OH)3]

green ppt—-> brown ppt

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10
Q

Co(H2O)6 +2OH-/2NH3—->

A

[Co(H2O)4(OH)2] +2H2O/2NH4-

pink sol—-> blue ppt

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11
Q

[Co(H2O)4(OH)2] + conc 6NH3—->

A

[Co(NH3)6]2+

blue ppt—–> yellow/light brown solution

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12
Q

[Co(NH3)6]2+ left in air——->

A

[Co(NH3)6]3+ (It oxidises in air)

yellow/brown solution—–> brown sol

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13
Q

[Co(OH)2(H2O)4] when left in air—>

A

[Co(OH)3(H2O)3]

blue ppt——>brown ppt

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14
Q

[Cr(h2o)6]^(3+) + 3OH-/3NH3——->

A

Cr(OH)3(H2O)3

violet sol—-> green ppt

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15
Q

Cr(OH)3(H2O)3 + 3NH3 (conc) ——>

A

{Cr(NH3)6]^3+

green ppt—–>violet sol

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16
Q

Cr(OH)3(H2O)3 +3OH- (conc)—->

A

[Cr(OH)6]^3-

green ppt—–> green sol

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17
Q

[Cr(OH)6] ^3- + H2o2 in alkaline conditions—->

A

CrO4 ^(2-)

green sol—–yellow sol

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18
Q

CrO4 ^(2-) + H+——>

A

Cr2O7^(2-)

yellow sol—–>orange sol

19
Q

Ionic equations for production of Fe3+ catalyst

A

S2O8(2-) + Fe(2+)—-> 2S2O4 + Fe3+

Fe3+ + 2I(-) ——> Fe2+ + I2

20
Q

Describe the mechanism of catalysis

A
  1. Adsorption- reactants stock to surface of catalyst
  2. Reaction- bonds of the reactants are weakened
  3. desorption- products come off the surface of the catalyst
21
Q

Reactions of catalyst of the Contact Proces

A

V2O5 + SO2—> V2O4 + SO3

V2O4 + 0.5O2 ——> V2O5

22
Q

Define heterogenous catalysts

A

When the catalyst is in a different phase to the reactants

23
Q

Why are Zn and Sc not a transition metals?

A

Zn can only form a +2 ion and Sc3+. In these ions they have a completed orbital and so does not meet the criteria of having an incomplete d orbital in one of its compounds.

24
Q

define ‘complex’

A

central atom surrounded by ligands

25
Q

define ‘ligand’

A

a species which can donate a lone pair of electrons

26
Q

how do coloured metal ions form?

A

Colour arises from electronic transitions from the ground state to excited states: between different d orbitals
A portion of visible light of specific frequencies is absorbed to promote d electrons to higher energy levels.
The light that is not absorbed is transmitted to give the substance colour.

27
Q

where do colour changes arise from

A
  1. oxidation state
  2. coordination number
  3. ligand
28
Q

define ‘unidentate ligands’

A

have one atom which can donate one lone pair of electrons- forms one coordinate bond

29
Q

define ‘bidentate ligands’

A

have two atoms which can each donate one lone pair electrons- form two coordinate bonds

30
Q

define ‘multidentate ligands’

A

can form several coordinate bonds

31
Q

examples of bidentate ligands

A

1,2-diaminoethane (en)

ethanedioate ligand C2O4^2-

32
Q

example of multidentate ligands

A

EDTA^4-

33
Q

shape of [CuCl4]^2- and why

A

tetrahedral

Cl- ligands are too large for more than 4 to fit around

34
Q

Cr2O7 + Zn in acidic conditions——>

A

[Cr(H2O)6]3+

orange to green

35
Q

catalysed reaction between iodide and persulfate ions

A

stage 1 S2O82- + 2Fe2——-> 2SO42- + 2Fe3+

stage2 2I- + 2Fe3+——-> 2Fe2+ + I2

36
Q

autocatalytic reaction between ethanedioate and manganate ions

A

Step 1: 4Mn(2+) + MnO4- + 8 H+———>5Mn (3+) + 4 H2O

Step 2: 2Mn(3+) + C2O4(2-) ——–>2Mn (2+ )+ 2CO2

37
Q

what is autocatalysis?

A

when a product of a reactions acts as a reagent

38
Q

Features of transition metals

A

shows variable oxidation states

can form complex ions

39
Q

why might one ion have a different colour to another ion?

A

different ligands would split the d orbitals to different extents
so different frequencies of light are absorbed

40
Q

Why does Cr has a unexpected electron configuration?

A

Half filled d orbital are more stable

Paired electrons easily removed due to repulsion

41
Q

why is cisplatin an effective cancer treatment?

A

The Cl- ligands are on the left side of the complex, these can both be displaced and bind to DNA preventing the cell division of cancerous cells

42
Q

Why can transition metals form variable oxidation states

A

This is because the ions contain partially filled sub-shells of d electrons that can easily lose or gain electrons. The energy differences between the oxidation states are small

43
Q

what makes something a good homogenous catalyst

A

needs to have its electrode potential in between the two half equations so it can oxidise one reagent and reduce the other

44
Q

why is a solid catalyst a good thing?

A

it can be filtered off

A- Level Chemistry (13 decks)

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