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OCR Chemistry A > 5.3 - Transition Metals > Flashcards

5.3 - Transition Metals Flashcards

(61 cards)

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1
Q

Transition metals

A

Elements that can form stable ions with an incomplete d sub shell

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2
Q

Why are Sc and Zn d-block elements but not transition metals

A

Sc^3+ ions have an empty 3d sub-shell and Zn2+ have a completely full subshell

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3
Q

Properties of transition metals

A

Variable oxidation states
Catalytic action
Coloured compounds
Formation of complexes

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4
Q

Complex ion

A

Metal ion surrounded by co-ordinately bonded ligands

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5
Q

Coordinate bond

A

Covalent bond in which both electrons in the shared pair come from the same atom

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6
Q

Coordination no.

A

No. of coordinate bonds to ligands that surround a transition metal ion

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7
Q

Ligand

A

An ion/molecule that forms a coordinate bond w/ a transition metal by donating its lone pairs (acts as a base)

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8
Q

Unidentate/monodentate

A

Ligand that can only form one coordinate bond

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9
Q

Examples of unidentate ligands

A 
H2O
NH3
Cl-
OH-
CN-
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10
Q

Bidentate

A

Ligand that can form two coordinate bonds by donating two lone pairs to central metal ion

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11
Q

Multidentate

A

Ligand that can form >1 coordinate bonds

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12
Q

What does coordination no. depend on

A

Size and electronic configuration of the cation

Size and charge of the ligands

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13
Q

Common coordination no.

A

6, 4, 2

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14
Q

Octahedral complexes

A

6 coordinate bonds (90 degrees)

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15
Q

Drawing 3D octahedral complexes

A

2 on the plane
2 going back into the plane
2 coming out of the plane

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16
Q

Tetrahedral complexes

A

4 coordinate bonds (109.5 degrees)

Usually chloro complexes

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17
Q

Drawing 3D tetrahedral complexes

A

2 on the plane
1 going back into the plane
1 coming out of the plane

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18
Q

Square planar complexes

A

4 coordinate bonds (90 degrees)

Requires TM w/ a 3d8 subshell e.g. Pt

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19
Q

Drawing 3D square planar complexes

A

2 going back into the plane

2 coming out of the plane

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20
Q

Cis trans isomerism in transition metal complexes

A

Only occurs in octahedral or square planar

Need two ligands that are different to the rest

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21
Q

Optical isomerism in TM complexes

A

Occurs in octahedral complexes w/ bidentate ligands

Can also be cis/trans

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22
Q

Highest oxidation no. for Sc

A

3+

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23
Q

Highest oxidation no. for Ti

A

+5

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24
Q

highest oxidation no. for V

A

+5

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25
Highest oxidation no. for Cr
+6
26
Highest oxidation no. for Mn
+7
27
Oxidation no. for Fe - Zn
Maximum decreases from +6 to +2
28
Catalysis reactions involving iron
Haber process
29
Catalysis reaction involving V2O5
Contact process - 2 SO2 + 1/2O2 --> 2SO3 SO2 +V2O5 --> SO3 + V2O4 V2O4 +1/2 O2 --> V2O5
30
Why are transition metals good catalysts
Ability to change oxidation state ---> can be regenerated through oxidation or reduction of the intermediate Can adsorb other substances on their surface and activate them (heterogenous)
31
Why are complex ions w/ partially filled sub shells usually coloured
Electrons excited | Absorb energy from visible light spectrum
32
Transition metal complexes in the body
Haemoglobin Fe^2+
33
Transition metal complex use in medicine
Pt(NH3)2Cl 2 Cis platin (anti-cancer) Binds to DNA preventing cell-division
34
When are transition metals colourless
Filled d subshell
35
How many coordinate bonds can EDTA 4- form
6 2 lone pairs on each N 4 on -COO
36
Factors causing colour change in reactions of TM complexes
Ligand changes Oxidation no. change Coordination no. change
37
Ligand substitution
One ligand in a complex is replaced by another
38
Colour of hexaaquamanganese (II)
pale pink soln
39
Mn(OH)2 ppt
Light brown | Insoluble in XS OH- or NH3
40
Colour of Fe2+
Pale green soln.
41
Fe(OH)2 ppt
Green ppt | Insoluble in XS OH- or NH3
42
Colour of Fe 3+
Pale yelow soln.
43
Fe(OH)3 ppt
Orange-brown ppt | Insoluble in XS OH- or NH3
44
Colour of Cu2+
Blue soln
45
Cu(OH)2 ppt
Pale blue Insoluble in XS OH- Soluble in XS NH3 [Cu(H2O)6]2+ + 4NH3 --> [Cu(NH3)4(H20)2}2+ + 4 H2O (dark blue soln)
46
Colour of Cr3+
Violet soln
47
Cr(OH)3
Gray-green ppt
48
Cr3+ in XS OH-
Dark green soln | [Cr(OH)6]3-
49
[Cr(H2O)6]2+ + 6NH3
[Cr(NH3)6}3+ + 6 H2O | Purple soln
50
Ligand sub w/ HCl
[Cu(H2O)6} 2+ + 4Cl- [CuCl4]2- + 6 H2O Reversible reaction Yellow soln
51
Why does only 4 Cl- ions sub for 6 H2O's
Cl- ligands are much larger than H2O ligands and therefore less can fit around the central metal ion
52
Why do you see a green colour during ligand sub w/ Cl- in Cu2+
Blue colour from hexaaquacopper (II) mixing w/ yellow colour from [CuCl4]2-
53
Why do Fe2+. Fe3+ and Mn2+ react w/ NH3 the same way as OH-
NH3 + H2O ---> NH4+ + OH- | The OH- then react to form a ppt
54
en
H2NCH2CH2NH2
55
Ethanedioate
(C2O4)2-
56
Ligand sub in haemoglobin
Haemoglobin has one free ligand which can be used to pick up water or oxygen in oxygen-rich areas and oxygen is also easily lost in oxygen-poor areas CO and CN can also bind and isn't easily removed
57
[Fe(H2O)6]2+ ----> [Fe(H20)6]3+
Add H+/MnO4-
58
[Fe(H2O)6}3+ ------> [Fe(H2O)6]2+
Add KI
59
Oxidising Cr 3+
H2O2/ OH-
60
Reducing Cr2O7 2-
Zn/H+
61
Reducing Cu2+
I- | Cu+ readily dissociates in aq

OCR Chemistry A (16 decks)

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