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Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

Define a transition metal as opposed to a d block element

A

TM: exists with partially filled d-block sub-shell in at least one of its compounds
D block: ground state has outer e- in d sub-shell

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2
Q

Name two characteristics of TM electron configuration

A

Lose 4s before 3d
Cu/Cr: 4s1 ground state (sub shells very energetically similar)

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3
Q

Which elements are excluded from transition metals

A

Exclude Sc down
(Include Zn down)
Sc3+ = 4s03d0
Zn2+ = 4s03d10

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4
Q

Name 4 general TM properties

A

Complex ions
Often coloured compounds
Often catalytic behaviour
Range of oxidation states

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5
Q

How are complex ions formed

A

Metal accepts e- from ligand lp
Dative cov bonds

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6
Q

Ligand

A

Donates lp to TM

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7
Q

Coordination number

A

No. Bonds to lps

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8
Q

1-5 prefixes

A

Mono
Di
Tri
Tetra
Penta
Hexa

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9
Q

H2O suffix

A

Aqua

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10
Q

NH3 suffix

A

Ammine

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11
Q

Cl- suffix

A

Chloro

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12
Q

OH- suffix

A

Hydroxy

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13
Q

CN- suffix

A

Cyano

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14
Q

Naming complex ions order

A

No. Ligands
Type of ligand
Metal
Oxidation no. Of metal

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15
Q

Name 4 possible complex ion shapes

A

6 octahedral
2 linear
4 tetrahedral
4 planar

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16
Q

Monodentate ligand

A

Attach to metal ion via one lp

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17
Q

Polydentate ions

A

Attach to metal ion with more than one lp
Di/tri/tetra
Usually organic diamines/dioates

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18
Q

Isolated atom subshell arrangement

A

Equal 5 d sub shells
e-s bound with same NRG
Same diagram NRG level

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19
Q

Complex ion subshell arrangements

A

Orbitals de/stabilised by ligands
Unequal orbitals

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20
Q

How is colour created by complex ions

A

e- in bottom group
e- vacancy in top group
Absorbs visible light of a specific frequency
e- excited
Reflects the rest of white light as photons

21
Q

Describe octahedral vs tetrahedral subshell structure

A

Octahedral: 2 top, 3 bottom
Tetrahedral: 3 top, 2 bottom

22
Q

What does the light frequency needed to excite an e- depend on

A

Orbital groups energy gap
Octahedral (usually) > tetrahedral

Metal oxidation state
Ligand nature

23
Q

Industrial dyes

A

Use e- excitation
Gap can be made without d orbital splitting

24
Q

Why does deprotination occur

A

Some metal +ve offset by e- ligand donation
Aqua: spread +ve to H
Increase +ve H compared to pure water
More likely H+ dissociation
Acidic behaviour
Especially in 3+ metals

25
Q

Forced deprotination using a base

A

Continue until ion has no charge
Insoluble ppte
OH in product is not the added base
Base removes H+ from H2O

26
Q

Acid strength

A

Polyprotic weak acids
Weaker with successive deprotinations
Some amphoteric
Uncharged ppte acidic enough to deprotination —> -ve charged

27
Q

Hexaaquaccopper (II) excess NH3 colour change

A

Pale blue solution to dark blue solution

28
Q

Hexaaquaccobalt (II) excess NH3 colour change

A

Pink solution to brown solution

29
Q

Hexaaquacchromate (III) excess NH3 colour change

A

Green solution to purple solution

30
Q

Hexaaquacchromate (III) excess OH- colour change

A

Green solution to dark green solution

31
Q

Hexaaquacchromate (III) limited NH3/OH- colour change

A

Green solution to grey-green ppte

32
Q

Hexaaquacferrate (II) limited NH3/OH- colour change

A

Pale green solution to dark green ppte
(Oxidised to brown Fe3+ when left)

33
Q

Hexaaquacferrate (III) limited NH3/OH- colour change

A

Yellow solution to red-brown ppte

34
Q

Hexaaquaccobalt (II) limited NH3/OH- colour change

A

Pink solution to blue ppte

35
Q

Hexaaquaccopper (II) limited NH3/OH- colour change

A

Light blue solution to blue ppte

36
Q

What structure/colour do chlorocopper/cobalt ligand exchanges form

A

Tetrahedral
Charged ligands produce greater colour changes
Copper: light blue to lime green
Cobalt: Pink to dark blue

37
Q

Ligand exchange equilibrium

A

Step wise process
Each step is reversible
Each step has an associated k value
New ligand metal bonds > old = exo
More exo, increase k

38
Q

Entropy multidentate vs monodentate ligands

A

Replace mutiple mono with fewer multi
More free product particles
+ve Ssys, increase k
Unfavourable exchange with excess = still get some exchange

39
Q

EDTA

A

Fully deprotinated
6 lps
Displace 6 monodentate ligands
Very +ve Ssys
Used as a cleaning agent for metal poisoning and soil/river metal pollution

40
Q

CO ligand exchange in haemaglobin

A

Strong monodentate ligand
Bind strongly to Fe2+
Detach oxygen
Practically irreversible
Toxic

41
Q

Haemaglobin structure

A

4 polypetide chains
4 haem groups
Fe2+ at each centre
Each dative cov bonded to 4 N lps (porphyrin ring)
Each dative cov bonded to one other globin
6th octahedral position binds to oxygen (oxyhaemaglobin) or water (deoxyhaemaglobin)
O2 and H2O easily switch

42
Q

TM redox reactions

A

Many oxidation states so many redox reactions
Use electrode potential data to determine spontaneity/acid or alkali conditions
Use ACW method

43
Q

Vanadium 4 oxidation states and colours

A

+5, yellow, VO2(+)
+4, blue, VO2+
+3, green, V3+
+2, purple, V2+

44
Q

Vanadium 3 half equations

A

V3+ + e- —> V2+
VO2+ + 2H+ + e- —> V3+ + H2O
VO2(+) + 2H+ + e- —> VO2+ + H2O

45
Q

4 chromium oxidation states and the conditions they’re produced under

A

+5, Cr2O7-2, acidic, yellow
+5, CrO4-2, alkali from Cr2O7-2 (H2O2 from Cr3+) orange
+3, Cr3+ acidic (H2O2/Zn from Cr2O7-2, O2 from Cr2+)
+2, Cr2+, acidic (anaerobic Zn from Cr3+)

46
Q

Heterogenous catalysts

A

Different state/phase to reactants
Continuous processes
No separation
Reactant molecules adsorb to surface
Weakened reactant bonds
Reactant molecules meet/react on surface
Product molecules desorb

47
Q

Heterogenous catalyst examples (4)

A

Ni alkene to alkane
Fe ammonia industrial production
Pt/Rh catalytic converters
- 2NO(g) + 2CO(g) —> N2(g) + CO2(g)
V2O5 H2SO4 production
- S(s) + O2(g) —> SO2(g)
- SO2(g) + 1/2O2(g) —> SO3(g)
— SO2(g) + V2O5(s) —> V2O4(s) + SO3(g)
— V2O4(s) + 1/2O2(g) —> V2O5(s)
- SO3(g) + H2O(l) —> H2SO4(aq)

48
Q

Homogenous catalysts

A

Same state/phase as reactants
Batch processes
Separate after mixing
TM aq ions = intermediates

49
Q

Homogenous catalyst examples (2)

A

Mn2+
- 2MnO4-(aq) + 16H+(aq) + 5C2O42-(aq) —> 2Mn2+(aq) + 8H2O(l) + 10CO2(g)
- Autocatalyst, product of the reaction
- Start slow, speed up
Fe3+
- 2I-(aq) + S2O8-2(aq) —> I2(aq) + 2SO4-2(aq)
- opp charged species react faster than 2 -ve charged species
— I2 + 2e- —> 2I-
— Fe3+ + e- —> Fe2+
— S2O8-2 + 2e- —> 2SO4-2

Chemistry (24 decks)

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