ligand substitution reactions

what would happen if one similarly sized ligand is substituted for another? give an example:

• no change in coordination number

• no change in shape

• change in colour

• e.g. [Co(H₂O)]²⁺ + 6NH₃ → 6H₂O + [Co(NH₃)₆]²⁺

what would happen if one different sized ligand is substituted for another? give an example:

• change in coordination number

• change in shape

• change in colour

• e.g. [Cu(H₂O)₆]²⁺ + 4Cl^- → 6H₂O + [CuCl₄]^2- - Cl^- ligands are bigger than H₂O and NH₃ ligands so the shape changes from octahedral to tetrahedral upon substitution (i.e. coordination number changes from 6 to 4)

what is partial substitution? give an example:

where not all ligands can be substituted e.g. [Cu(H₂O)₆]²⁺ _(aq) + 4NH_{3 (aq)} → [Cu(NH₃)₄(H₂O)₂]²⁺ _(aq) + 4H₂O _(l):

• here, not all water ligands can be replaced by NH₃ ligands :(

• shape changes from octahedral → elongated octahedral, w/ 2 H₂O ligands occupying the trans positions

describe the structure of haemoglobin w/ reference to it as a transition metal complex:

• one haem group contains Fe²⁺ at its centre which accepts 6 lone pairs from ligands, w/ 4 being from H atoms which form a circle around the molecule - the haem

• a globin (type of protein) and either an oxygen atom or water molecule can bind, forming an octahedral structure

describe the role of haemoglobin in the body with reference to the ligand substitution reactions which could occur:

• haemoglobin transports oxygen around the body and substitutes it for water where needed

• if CO is inhaled, then haemoglobin can substitute the water or oxygen ligands, forming carboxyhaemoglobin

• but CO binds more strongly to haemoglobin and doesn’t exchange for water or oxygen ligands

• this may therefore starve the body of oxygen, causing headaches/dizziness/death

why is CO toxic?

replaces oxygen co-ordinately bonded to Fe (II) in haemoglobin

are ligand substitution reactions reversible? in what case may this change?

• yes - ligand substitution reactions are reversible

• unless the new complex is much more stable than the old one

why are EDTA^4- and ethylenediamine reactions usually irreversible?

• multidentate ligands (such as the above) form much more stable complexes than monodentate ligands

• it is difficult to reverse the substitution of a monodentate ligand for a multidentate ligand, as doing so would result in a decrease in entropy

describe and justify the typical enthalpy change for a ligand substitution reaction:

typically low - enthalpy of breaking old coordinate bonds and forming new bonds is fairly similar

explain the chelate effect:

• when bidentate/multidentate ligands replace monodentate ligands to form a more stable complex

• because there is an increase in entropy or more particles formed

why is it difficult to reverse the substitution of a monodentate ligand for a multidentate ligand?

doing so would result in a decrease in entropy

give an example of the chelate effect:

reactions replacing monodentate ligands w/ EDTA are very difficult to reverse:

• ([Cr(NH₃)₆]³⁺ + EDTA^4- → [Cr(EDTA)]^- + 6NH₃

• 2 particles → 7 particles ∴ entropy increases and so stability of complex increases

the figure shows the structure of the EDTA^4- ion. atoms of 2 diff elements in EDTA^4- can form coordinate bonds w/ an aluminium ion - on the figure above, draw circles around the atoms of 2 diff elements that would llink to an aluminium ion by a coordinate bond (2)