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Core Chemistry 1A - Paper 2 > Coordination > Flashcards

Coordination Flashcards

(52 cards)

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1
Q

Transition metal definition

A

An element with an unfilled d- or f-orbital in at least one common oxidation state

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2
Q

Definition of complex

A

Positively charged central ion (possibly neutral), an acceptor, surrounded in a symmetrical manner by a shell of ions or molecules call ligands

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3
Q

Ligands are held to metal via…

A

dative bonds

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4
Q

Monodentate ligand definition and examples

A

Has one donor atom

eg OH2, Cl-, CN-

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5
Q

Bidentate ligand definition and examples

A

Has two donor atoms

eg bipy, acac-, en, dppe

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6
Q

Tridentate ligand definition and examples

A

Has three donor atoms

eg dien, terpy

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7
Q

Tetradenate ligand definition and examples

A

Has four donor atoms

eg tren, trien

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8
Q

Hexandentate ligand deifnition and examples

A

Has six donor atoms

eg [EDTA]4-

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9
Q

What is chelation?

A

Formation of complexes by chelate ligands

Simultaneous bonding of multiple donor atoms by forming rings around the central atom

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10
Q

Definition and examples of ambidentate ligands

A

Can bond with different atoms depending on metal and conditions
eg SCN- (thiocyanate) and NCS- (isothiocyanate)
NO2- (nitro) and ONO- (nitrito)
Special case CN- in prussion blue:
links through Fe(II) - C - N - Fe(III)

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11
Q

Possible shapes of complexes of metals with coordination number 4

A

Tetrahedral, square planar

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12
Q

Possible shapes of complexes of metals with coordination number 6

A

Octahedral

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13
Q

Possible shapes of complexes of metals with coordination number 5

A

Trigonal bipyramid, square-based pyramid

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14
Q

Order to put things in when writing metal complex formula

A

In square brackets, [ ], cation then anion
Metal ion first
Anionic ligands next (alphabetical)
Neutral ligands (alphabetical)

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15
Q

Types of isomerism

A 
Ligand
Linkage
Ionisation
Hydrate
Coordination
Polymerisation
Geometric
Optical
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16
Q

What is ligand isomerism?

A

Confined to organic ligands

- isomers of the ligand e.g. ortho, para,meta

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17
Q

What is linkage isomerism?

A

For ambidentate ligands only

- bonding with different atoms to central ion

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18
Q

What is ionisation isomerism?

A

Possible in compounds with a complex ion and counter-ion (also a ligand)
eg [PtCl2(NH3)4]Br2 and [PtBr2(NH3)4]CL2

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19
Q

What is hydrate isomerism?

A

Possible with water in or out of coordination sphere

eg [Cr(OH2)6]Cl3 and [CrCl(OH2)5]Cl2·H2O and [CrCl2(OH2)4]Cl·2H2O

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20
Q

What is coordination isomerism?

A

Possible for compounds made up of both cationic and anionic complex ions
Neutral species NOT allowed
eg Cr(NH3)6Cr(CN6)
and [Cr(CN)2(NH3)4]+[Cr(CN)4(NH3)2]-

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21
Q

What is polymerisation isomerism?

Study These Flashcards
A 
Multiply the molecular formula by 2, 3 etc
If oxidation number is +2, up to 3x
If +3, up to 5x
If +4, up to 7x
Only works if all ligands are on metal
22
Q

What is geometric isomerism?

Study These Flashcards
A

Ligands bonded in a different order to the central metal ion

eg cis and trans

23
Q

What is optical isomerism?

Study These Flashcards
A

non-superimposable mirror images

24
Q

Describe stability of complexes for reaction

M-L + L* M-L* + L

Study These Flashcards
A

If reaction goes to RHS, L* makes a more stable complex with M than L

25
What are hard acids?
``` Most metals in normal oxidation states H+ All electropositive metals Have small atomic radius High effective nuclear charge High charge-to-radius ratio High energy LUMO ```
26
What are soft acids?
Cu(I), Rh(I), Ag(I), Au(I) Pd(II), Pt(II), Cd(II), Hg(III), Au(III) Have lower charge-to-radius ratio
27
What are hard bases?
Have low energy HOMO F-, OH-, NH3, OH2, N NO3-, SO4(2-) ox(2-), CO3(2-)
28
What are soft bases?
Br-, I-, S, P | H-, C2H4, CN-
29
Most stable complexes formed are...
A hard acid with a hard base | A soft acid with a soft base
30
Assumptions made in Crystal Field Theory
Central metal ion = point positive charge Ligands regarded as dipoles or anions Ligands = point negative charges Ionic lattice built from point positive and negative charges Ionic bonding = electrostatic forces
31
d^n configuration =
No of electrons for 'framework' | = group no. - oxidation state
32
Rules for electron filling
Electrons prefer to occupy orbital of lowest energy Hund's rule - if there is more than one degenerate orbital, electrons first occupy separate orbitals with parallel spins Pauli Exclusion Principle - no more than 2 electrons can occupy a single orbital. If 2 electrons occupy a single orbital the spins must be paired Energy is required to pair 2 electrons in a single orbital, the energy penalty for pairing 2 electrons = pairing energy, P
33
What is Δo and what factors affect its size?
As charge on metal increases, Δo gets larger Δo(1st row) >∆o(2nd row) > ∆o(3rd row) Stronger field ligands --> larger ∆o
34
Strongest field ligands
CN-, CO, PR3, NO2-
35
Weakest field ligands
I-, Br-, SCN-, Cl-
36
Describe octahedral crystal field splitting energy, ∆o
The energy between the lower dxy, dyz, dxz and higher d(z^2), d(x^2-y^2) When ligands bond to the metal ion, the orbitals have different energies
37
Name of ligand: OH2
Aqua
38
Name of ligand: N2
Dinitrogen
39
Name of ligand: O2
Dioxygen
40
Name of ligand: NH3
Ammine
41
Name of ligand: CO
Carbonyl
42
Name of ligand: NO
Nitrosyl
43
Name of ligand: Cl-
Chloro
44
Name of ligand: Br-
Bromo
45
Name of ligand: OH-
Hydroxo
46
Name of ligand: CN-
Cyano
47
Naming complexes: if ligand already has prefix but there are more than 1 of them e.g. (dioxygen)2 use...
bis, tris, etc
48
Order of ions when naming complexes
Cation, then anion Ligands are listen alphabetically before the metal (excluding prefixes) Include oxidation number of metal For anionic complexes add 'ate' to name
49
Name of ligand: PPh3
Triphenylphosphine
50
When is an octahedral complex low spin and high spin?
∆o high --> low spin | ∆o low --> high spin
51
First row of d-block
Proton numbers 21-30 | groups 3 - 12
52
How to work out group from top element
If in d-block: +18 for second element, +32 for third | Rest of table: +8 for second element, +18 for third, +18 for fourth, +32 for fifth

Core Chemistry 1A - Paper 2 (6 decks)

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