20148 key concepts Flashcards
trend in co-ordination numbers down groups
wider range of coordination numbers for 2nd and 3rd row metals than for first row. For first row metals 4 and 6 are most common, with 6 rarely exceeded
Metal-metal bonding more common for…
2nd and 3rd row metals
Exceptions to TM 4s^2 rule
Cr and copper, both 4s^1
Why is the 4s orbital usually occupied
3d orbital lower in energy but 4s orbital occupation means less e-e repulsion, which outweighs cost of occupying higher energy orbital
Why doesnt the 4s filling apply in a compound
orbitals large so less e-e repulsion
Maximum oxidation state for Sc–>Mn
corresponds to oxidation state with all 3d and 4s electrons removed
Maximum oxidation state for Fe–>Cu
difficult to attain, still contains d electrons
Trend in +2 vs +3 oxidation state in TMs- rationalise
+3 more common than +2 in earlier transition metals
Increasing IE across the series, and increasing core-like behaviour of d orbitals across the series.
zero or negative oxidation state possible with which ligand
CO
High oxidation states possible with which ligands
fluoride and oxide
Order of stabilisation in oxidation states for halides
F-> Cl-> Br-> I-
What does reaction of V with halides (X2) give and why
VF5, VCl4 and VBr3
F best at stabilising so can maintain higher oxidation state of V
+2 oxidation states
oxides and halides form binary compounds MO MX2
All first row TMs with the exception of Ti form [M(H2O)6]2+ in aqueous solution
+3 oxidation state
Formed for all TMs, but Cu3+ is very oxidising
[M(H2O)6]3+ known for Ti–> Co
[Ti(H2O)6]3+ and [V(H2O)6]3+ both oxidised by air
+4 oxidation state
Most important oxidation state for Ti- these compounds have high covalent character and high charge density on the metal makes it very polarising
TiCl4
covalently bonded liquid
TiCl2
ionic solid
More positive value of E°
greater strength of oxidising agent on LHS of equation
Powerful oxidising agents only observed with
oxide and fluoride ligands
E° value from Latimer diagram
(n1 x E°1 + n2 x E°2) / (n1 + n2)
where n= number of electrons
1= reaction 1
2= reaction 2
Frost diagram plots
nE° against oxidation state
How can you obtain E° from a Frost diagram
gradient of the line linking 2 oxidation states
If an intermediate oxidation state lies above the line linking oxidation states, ….
the disproportionation reaction will be thermodynamically favourable
what does high pH favour in terms of oxidation states
higher oxidation states
Chromium, Molybdenum and Tungsten
CrO3 and [CrO4]2- strong oxidising agents
WO3 and [WO4]2- not readily reduced
OS: 1st row< <2nd row<3rd row
Mo(IV) and W(IV) very common, but Mo(III) and W(III) sparse
High co-ordination numbers possible eg [Mo(CN)7]5- pentagonal bipyramidal
Metal-Metal bonds more common for Mo and W than Cr
Most Mo(II) and W(II) compounds contain M-M bonds
Nickel, Palladium and Platinum
For Ni and Pd, +2 is the only important oxidation state in aqueous solution, but for Pt 4+ is also important
For Pd and Pt square planar is the most important geometry for +2
M-M bonds and low OS’s become more important down the group
Which approach can be used ton explain the SCS
LF theory, a MO based approach
4s orbital
a1g symmetry
4p orbital
t1u symmetry
3d orbitals (x2-y2 and dz2)
eg symmetry
3d orbitals (xy, xz and yz)
t2g symmetry
Additional Pi bonding in Tm complexes from…
Filled p orbitals into d orbitals- filled p lying perpendicular and can interact with d orbital not involved in sigma bond, so interacts in a Pi manner
Empty Pi* orbitals into d orbitals- have right symmetry
Draw the partial MO diagram for Pi donor ligands
Draw the partial MO diagram for Pi acceptor ligands
How do Pi donor ligands effect delta oct
reduce it
Pi donors include
O2- and N3-
Pi acceptors include
CO,CN- and C2H4
Are ligands at the top of the SCS Pi donors or acceptors
acceptors (incr delta oct, greatest splitting energy)
Nephelauxetic effect
Pairing energies lower in metal complexes than in gaseous ions, because orbitals bigger and less electron-electron repulsion in complexes
How do CO ligands co-ordinate to the metal centre
Through the less EN carbon atom
What is backbonding (CO)
Pi donation from a filled d orbital on M into empty Pi* orbital on CO
Electron density going opposite direction to sigma donation (from filled orbital on CO to empty metal d orbital)
Greater degree of backbonding = lower/higher stretching frequency
lower
stronger bonds = higher frequency
Tolman cone angle
measure of ligand size
Phosphine ligands properties
P d orbitals acceptors, P-C sigma* orbitals act as acceptors
Tertiary phosphines good sigma donors
structural role of TMs
stabilising protein structures
functional role of TMs
metal ion involved in reactivity
How many haem groups does Hb have
4
What is iron bound to in Hb and Mb to give a haem group
porphyrin ring
Mb function
storage of oxygen
What happens when oxygen binds in deoxyhaemoglobin
Electron configuration changes high to low spin t2g4 eg2 to t2g6/5. Since antibonding eg orbitals are no longer occupied the ion is smaller, so can move into the haem ring/plane
Forms oxyhaemoglobin and oxygen co-ordinated in a bent-on manner
Role of metal centre in electron transfer proteins
provide a reversible binding site for an electron
Which is iron a good metal to use in electron transfer proteins
Its has 2 OS’s readily available: Fe2+ and Fe3+
Ferrdoxins properties
iron-sulfur proteins, characterised by iron reduction potentials less than 0V. Ferredoxins contan 2,3, or 4 iron centres
Bacterial rubredoxins
contain only 1 iron centre