Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

(49 cards)

Start Studying
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Name two characteristics of TM electron configuration

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Which elements are excluded from transition metals

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Name 4 general TM properties

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How are complex ions formed

A

Metal accepts e- from ligand lp
Dative cov bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Ligand

A

Donates lp to TM

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Coordination number

A

No. Bonds to lps

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

1-5 prefixes

A

Mono
Di
Tri
Tetra
Penta
Hexa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

H2O suffix

A

Aqua

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

NH3 suffix

A

Ammine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Cl- suffix

A

Chloro

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

OH- suffix

A

Hydroxy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

CN- suffix

A

Cyano

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Naming complex ions order

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Name 4 possible complex ion shapes

A

6 octahedral
2 linear
4 tetrahedral
4 planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Monodentate ligand

A

Attach to metal ion via one lp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Polydentate ions

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Isolated atom subshell arrangement

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Complex ion subshell arrangements

A

Orbitals de/stabilised by ligands
Unequal orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How is colour created by complex ions

Study These Flashcards
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

Study These Flashcards
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

Study These Flashcards
A

Orbital groups energy gap
Octahedral (usually) > tetrahedral

Metal oxidation state
Ligand nature

23
Q

Industrial dyes

Study These Flashcards
A

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

24
Q

Why does deprotination occur

Study These Flashcards
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
Forced deprotination using a base
Continue until ion has no charge Insoluble ppte OH in product is not the added base Base removes H+ from H2O
26
Acid strength
Polyprotic weak acids Weaker with successive deprotinations Some amphoteric Uncharged ppte acidic enough to deprotination —> -ve charged
27
Hexaaquaccopper (II) excess NH3 colour change
Pale blue solution to dark blue solution
28
Hexaaquaccobalt (II) excess NH3 colour change
Pink solution to brown solution
29
Hexaaquacchromate (III) excess NH3 colour change
Green solution to purple solution
30
Hexaaquacchromate (III) excess OH- colour change
Green solution to dark green solution
31
Hexaaquacchromate (III) limited NH3/OH- colour change
Green solution to grey-green ppte
32
Hexaaquacferrate (II) limited NH3/OH- colour change
Pale green solution to dark green ppte (Oxidised to brown Fe3+ when left)
33
Hexaaquacferrate (III) limited NH3/OH- colour change
Yellow solution to red-brown ppte
34
Hexaaquaccobalt (II) limited NH3/OH- colour change
Pink solution to blue ppte
35
Hexaaquaccopper (II) limited NH3/OH- colour change
Light blue solution to blue ppte
36
What structure/colour do chlorocopper/cobalt ligand exchanges form
Tetrahedral Charged ligands produce greater colour changes Copper: light blue to lime green Cobalt: Pink to dark blue
37
Ligand exchange equilibrium
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
Entropy multidentate vs monodentate ligands
Replace mutiple mono with fewer multi More free product particles +ve Ssys, increase k Unfavourable exchange with excess = still get some exchange
39
EDTA
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
CO ligand exchange in haemaglobin
Strong monodentate ligand Bind strongly to Fe2+ Detach oxygen Practically irreversible Toxic
41
Haemaglobin structure
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
TM redox reactions
Many oxidation states so many redox reactions Use electrode potential data to determine spontaneity/acid or alkali conditions Use ACW method
43
Vanadium 4 oxidation states and colours
+5, yellow, VO2(+) +4, blue, VO2+ +3, green, V3+ +2, purple, V2+
44
Vanadium 3 half equations
V3+ + e- —> V2+ VO2+ + 2H+ + e- —> V3+ + H2O VO2(+) + 2H+ + e- —> VO2+ + H2O
45
4 chromium oxidation states and the conditions they’re produced under
+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
Heterogenous catalysts
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
Heterogenous catalyst examples (4)
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
Homogenous catalysts
Same state/phase as reactants Batch processes Separate after mixing TM aq ions = intermediates
49
Homogenous catalyst examples (2)
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions