PHYSICAL PHARMACEUTICS I

1. UNIT IV
COMPLEXATION AND PROTEIN
BINDING
By: Ms. Swati Gaikwad
Assistant Professor
Nagpur Pharmacy College ,wanadongri.Nagpur

2. Classification of complexes

3. CLASSIFICATION OF COMPLEXES
Metal ion complexes:
Metal-ion coordination complexes are also called metal ion complexes, which consist of a
central metal ion bonded to one or more Ligands.
The coordination number of the complex is the number of bonds between the metal
ion and the ligand, which can be more than one .
This number depends on the size, charge and electronic structure of the metal ion.
Coordination numbers are normally between 2 and 9 with the most common coordination
numbers being 4 and 6.

4. 1. Inorganic complexes:
 This group was first described by Werner in 1891
 There are some examples of Complex ions belonging to this groups are
[Ag(NH3)2]+, [Fe(CN)6]4-,Co(NH3)6]3+ and [Cr(H2O]6]3+
 In hexammine cobalt III chloride Co(NH3)6]3+Cl3- , ammonia molecules are known
as Ligands and are coordinated with cobalt ion.
 The number of ammonia groups coordinated with metal ions is six hence,
coordination number of cobalt ion is six.
 The metal ions which lack sufficient bonding orbital’s, Hybridization plays an
important role in coordination compounds.

5. The sp3 hybridisation of carbon Electronic configuration of d2sp3 hybridized
Hexamine cobalt III chloride
For example cobalt ion, co(III), has ground state electronic configuration. The electronic
configuration of metal ion with filled 3D levels and Thus, d2sp3 or octahedral structure is predicted
as the structure of this complex.

6.  Pauling suggested that one of the 2s electron is promoted to 2p orbital to form four
equivalent orbitals.
 This structure is known as sp3 hybrid as one S and three P orbital’s are involved.
 These bonding orbitals are directed towards the corners of a tetrahedron.
 Similarly, in a double bond, there is sp2 hybridized carbon and geometry is
triangular.
 In transition elements, such as cobalt, zinc, nickel and copper 3d, 4s and 4p orbitals
are involved in forming hybrids.
 Differently hybridized metal ions results in different geometries
H2O, NH3, CN-, or CL- like ligands donate a pair of electrons in forming a complex
with a metal ion, by filling the empty orbitals of the metal ion.

7. 2. Chelates:
 Chelation means that the anion has two or more separate sites to which the metal is
bonded.
 A molecular entity in which there is chelation is called a "chelate".
 Chelates are more stable than nonchelated compounds of comparable composition
 This phenomenon is called the chelate effect.
 The stability of a chelate is also related to the number of atoms in the chelate ring.

8.  Cis–trans isomerism occurs in octahedral and square planar complexes
 Only cis-coordinated (ligands-ligands adjacent on a molecule) were
readily replaced by reaction with a chelating agent.
 Vitamin B12 and the hemoproteins are incapable of reacting since
only the trans-coordination positions of the metal are available for
complexation.
 In contrast, the metal ion in certain enzymes, such as alcohol
dehydrogenase, which contains zinc, can undergo chelation, suggesting
that the metal is bound in such a way as to leave two cis positions
available for chelation.

9. Chelates are more stable than comparable complexes containing only one binding site.
 They are also used in formulations for increasing the shelf-life of the drug product.
Examples of such chelating agents include citric acid, tartaric acid and EDTA
(ethylenediamine tetraacetic acid).
 It can also affect the solubility and absorption of both drug and metal ion, and can lead to
either increased or decreased absorption.
 Therapeutic chelators are used in metal poisoning. For example, ethylenediamine
tetraacetic acid (EDTA) as the monocalcium disodium salt is used in the treatment of lead
poisoning. Deferiprone chelates iron.
 Tetracycline chelation with metal ions leads to decreased drug absorption:
 Polyvalent cations such as Fe2+ and Mg2+, and anions such as the trichloracetate or
phosphate interfere with absorption.
 The antibacterial action of the tetracyclines depends on their metal-binding activity, as
their main site of action is on the ribosomes, which are rich in magnesium.

10. Organic molecular complexes
 In organic molecular complexes, substrate and ligand are bonded together by weak
forces of the donor-acceptor type e.g., electrostatic interaction, charge-transfer
or hydrogen bonding.
 Substrate and ligand forming the complex can be a small molecule-small molecule,
small molecule-macromolecule, enzyme-substrate, and drug-receptor and
antigen-antibody interaction.
 The energy of attraction between them is probably less than 5 kcal/mole for most
organic complex and the bond distance is usually hence a covalent link is not
involved. greater than 3A°;

11.  One molecule polarizes the other, resulting in a type of ionic interaction or
charge transfer, and is referred to as charge transfer complexes.
 For example, the polar nitro groups of trinitrobenzene induce a dipole in
benzene molecule, and the electrostatic interaction that results in complex
formation.

Electrostatic interaction between Charge transfer complex between
Trinitrobenzene and Benzene Trinitrobenzene and Hexamethylbenzene due to
resonance.
 Resonance makes the main contribution to complexation in charge-transfer
complex, while in the donor-acceptor complex, London dispersion forces and dipole-
dipole interactions contribute more to the stability.

12. Quinhydrone obtained from Salicylic acid

13. •Picric acid complexes
 When 2,4,6 trinitro phenol(Picric acid), reacts with weak bases it forms molecular
complexes where as when it reacts with strong bases to form salts.
 For example Butesin picrate which is 2:1 complex is a molecular complex formed with
picric.
 Eg. In Picric acid complex Butesin picrate, Butesin act as anaesthetic and picrate as
antiseptic and is used as a 1% ointment for burns and pain.
 Carcinogen+ picric=carcinogenic activity
 Substitution carcinogenic + picric=interfere with complex
 Reduce carcinogenicity of carcinogen
 It was observed that the stability of the complexes formed between carcinogenic agents
and picric acid leads to carcinogenic activity
 and any substitution on the carcinogen molecule that interfere with Picrate
complexation also reduces carcinogenicity.
Butesin picrate (2:1 complex)

14. •Caffeine & other drug complexes
Complexation of caffeine with number of acidic drugs was studied by Higuchi and his associates.
According to them interaction between caffeine and acidic drug is due to the Dipole-Dipole force
or hydrogen bonding between the carbonyl group of caffeine and hydrogen atom of acid.
Secondary interaction may occur between the nonpolar parts of the molecules.
Many important drugs belong to ester class and many complexes formed between esters and
Amines, phenols, ethers and ketones is due to hydrogen bonding between carbonyl oxygen and
active hydrogen.
But it does not explain complexation of caffeine with Benzocain, Procaine and Tetracaine as there
is no active hydrogen on caffeine and hydrogen at 8 position is very weak to form a complex.
Formula I- Numbering in caffiene molecule.
Formula II-Strongly electrophilic nature of nitrogen at 2 position due to withdrawal of electrons by oxygen at 1 and 3 position.
Formula III-In benzocaine, carboxyl oxygen is nucleophilic which interacts with electophilic nitrogen of caffeine.

15. Polymer complexes
 Polymers containing nucleophilic oxygen can form complexes with various drugs,
polymers like Polystyrene, PEG, carboxymethyl cellulose.
 Some of them are incompatible with several drugs due to these interactions
 Eg. Certain polyethers, such as carbowaxes, pluronics and tweens with tannic acid,
salicylic acid & phenol are incompatible.
 This incompatibility may be due to undesirable physical, chemical or pharmacological
effects, like precipitation, flocculation, loss of preservative action, delayed biological
absorption etc.
 Fromming et.al. Studied interaction of Crosspovidone with acetaminophen, benzocaine,
caffeine, tannic acid & Papavaine HCl.etc.
 Crosspovidone is used as a disintegrant in pharmaceutical granules & tablets, does not
interfere with gastrointestinal absorption because the binding to drug is reversible.
 Drug polymer interaction may used to modify biopharmaceutical parameters of drug
eg. dissolution rate of ajmaline is increased by complexation with PVP.
 This interaction is due to amide group of PVP & aromatic ring of ajmaline to yield a
dipole-dipole induced complex.

16. Inclusion complexes
 There are the compounds which are formed, as one constituent of complex get trapped in
the open lattice or cage like structure of the other to yield stable arrangement .
 These complexes generally do not have any adhesive forces working between their
molecules and are therefore also known as no-bond complexes.
Deoxycholeic Acid, which forms channel lattice type complex.
1. Channel lattice type:
• The deoxycholeic acids (bile acids) can form complexes with paraffins, organic acids,
esters, ketones and aromatic compounds, and with solvents like ether, alcohol and
dioxanes.
• The crystals of deoxychloleic acid arrange to form a channel into which complexing
molecule can fit.

17. 2. Layer type:
In this type of complex, complexing agent trap the compounds between the layers of their
lattices.
Such as clay montmorillonite, the principle constituent of bentonite, trap hydrocarbon,
alcohol & graphites between its layers.
Similarly, graphites can also trap compounds between its layers.
Layer type complex

18. 3. Clathrates:
Some complexing agents have ability to crystallize as a cage like lattice, and coordinating
compound get entrapped inside this cage.
Molecular size of entrapped component is important and no chemical bonds are involved.
The stability of the complex formed is because higher amount of energy is required to
decompose the compound, due to strong structure.
Whereas Powell and Palin made a detailed study of clathrate, he showed that highly toxic
agent hydroquinone (quinol) crystallize in a cage like hydrogen-bonded structure.
These quinol molecules allow entrapment of one small molecule between two quinol
molecules .
These holes have diameter of 4.2 A therefore, very small molecules like H2 and large
molecules like ethanol cannot be accommodated in the cavity but small molecules like
methyl alcohol,CO2 & HCL may be trapped
Another example is official drug warfarin sodium USP is a clathrate of water and isopropyl
alcohol .

19. Structure of clathrates.

20. • Monomolecular complexes.
Cyclodextrins: According to Davis and Brewstar, Cyclocdextrins are cyclic oligomers of glucose that can form
water soluble inclusion complexes with small molecules and portions of large compound monomolecular inclusion
compound involve the entrapment of single guest molecule in the cavity of one host molecule.
β-Cyclodextrin

21. • Cyclodextrins are cyclic oligosaccharides consisting of (α-1,4)-linked D-glucopyranose units, with a
hydrophilic outer surface and a hydrophobic central cavity.
• The cavity entrance is hydrophilic due to presence of primary and secondary hydroxyl groups,
whereas interior of the cavity is relatively hydrophobic due to CH2 groups.
• The natural -cyclodextrin, β-cyclodextrin and -cyclodextrins consist of six, seven, and eight units of
glucose and diameters of the central cavities are about 5, 6, and 8 Å for α-, β-, and γ-cyclodextrin,
respectively.
• Ability to form inclusion compounds is due to typical arrangement of the glucose units.
• The molecule actually exists as a truncated cone and can accommodate drug molecule to form
inclusion compounds.

22. Macro molecular inclusion compounds
 Macromolecular inclusion compounds are commonly called as molecular sieves.
 They include zeolites, dextrins, silicagels and related substances.
 The arrangement of these compounds is three dimensional and produces cages and channel like
structures.
 Synthetic zeolites are made to have a definite pore size so as to separate molecules of different
dimensions and these are also capable of ion exchange.