Drug Receptor Interactions PDF

Drug Receptor Interactions Course: Pharmaceutical Chemistry Course code: PMY 2230 H O H H O N O2C Me...

Drug Receptor Interactions Course: Pharmaceutical Chemistry Course code: PMY 2230 H O H H O N O2C Me H H Binding site Organised by Mwiinga A.  Learning Outcomes At the end of this lesson students will be able to Define and describe the drug targets and drug binding. Explain various drug-receptor interactions such as ❑ Covalent bonding ❑ Ionic (electrostatic) interaction ❑ Dipole-dipole interaction ❑ H-bonding ❑ Hydrophobic interaction ❑ Van der Waals forces. Define and describe agonists and antagonists for receptors. Applications of Bonding Intermolecular Forces Set of attractive and repulsive forces. Present between two molecules Weak forces Play important role in determining the physical properties of a substance. States of substances is determined by these forces. The stronger the intermolecular forces are, the more energy it will require to pull the molecules apart. Molecules that have strong intermolecular forces also have high melting points and boiling points.  Intramolecular Attraction: much weaker than ionic or covalent bonds. They become weaker as distance between molecules increases. Examples Dipole-to-Dipole forces Dipole-induced dipole forces London dispersion forces Hydrogen bonding Bonding  Dipole-to-Dipole intermolecular attraction due to molecular polarity.  Hydrogen Bond is a special type of very strong dipole-to-dipole intermolecular attraction. Water has very strong H-bonds. London Dispersion Forces are intermolecular attractions between non-polar molecules. Intramolecular bonding forces exist between the atoms in a molecule and hold the molecule together Intermolecular forces exist between molecules H- O ….H- O Dipole-to-Dipole Attractions Size of permanent dipole depends on the bonded atoms and shapes of molecules. Individually, dipole-to-dipole attraction is stronger than induced dipole-to-induced dipole attraction. ✓ But for larger molecules the London Dispersion forces become more important for predicting the physical properties a) The interaction of two polar molecules. b) The interaction of many dipoles in a liquid Hydrogen Bonding Molecules that have –OH or –NH groups have particularly large intermolecular attractions - Also the HF molecules  How body do its jobs Main systems of the body are:  CNS: - Sympathetic - Parasympathetic - Signals move through [polarization-depolarization] mechanism.  Liver: - Detoxification process - Storage device.  Hormones: - From where they produced - How they work, to understand all this you have to understand the molecular level of body organization. CELL  Drugs Targets ❑ Macromolecules such as: 1. Proteins (mainly enzymes, receptors and transport proteins) 2. Lipids 3. Carbohydrates 4. Nucleic acids (DNA and RNA) are the main molecular targets for drugs. ❑For a drug to have an action, it should interact [bind] with one of these molecules. ❑ The area of the macromolecule where the interaction takes place is called the binding site; which is a pocket or canyon at the surface of the macromolecule. ❑ Drug-target interactions can be grouped into two types: 1- Permanent (Irreversible) - covalent bonding (strength of 200-400KJ/mol). 2- Reversible – by different types of interactions How Binding Takes Place  Binding occur through points of attachment, for a chemical compound they are the functional groups.  Functional groups use their electronic & shape characters in the binding process.  Bonds could be inter-molecular or intramolecular.  If we talk about reversible binding, binding of drug to receptor should be in equilibrium state. Example The protein The active site The drug Receptor-drug interaction  Receptors are mostly membrane-bound proteins that selectively bind small molecules called ligands which results in physiological response.  They are difficult to isolate because they exist in tiny amount and if isolated it will be difficult to purify. Overall Process of Receptor/ Messenger Interaction M M M RE RE R Signal transduction ✓ Binding interactions must be strong enough to hold the messenger sufficiently long for signal transduction to take place. ✓ Interactions must be weak enough to allow the messenger to depart. ✓ Implies a fine balance. Receptor-drug interaction  The driving force for drug-receptor interaction is the low energy state of the drug-receptor complex.  The biological activity is related to the drug affinity for the receptor, i.e the stability of the complex.  Dissociation constant of the drug-receptor complex gives an idea a bout how potent is the drug.  The protein surface contains an area which has the correct shape to accept the incoming messenger. This area is known as the binding site and is analogous to the active site of an enzyme. But unlike enzymes, chemical messenger does not undergo a chemical reaction. It fits into the binding site of the receptor protein, passes on its message and then leaves unchanged. Ligand receptor interaction involves the same bonding types that are for drug-enzyme interaction.  Receptor-Drug interactions  Includes: Covalent bonds  Strong, irreversible bonds (-40 to -110 Kcal/mol stability).  Rarely seen in drug-receptor interaction.  More prevalent in drug-enzyme and drug-DNA interaction. Covalent bonds  For covalent bond formation, there should be two poles; the electrophile and the nucleophile.  Nucleophiles in biology have the following functional groups:  Thiol in the amino acid cysteine  Hydroxyl in the amino acid serine  Amine in the amino acid lysine  Carboxylate in the amino acid glutamic acid.  Electrophiles  Epoxide ring  Alkyl group attached to halogen  Positively charged centre Ionic or electrostatic interactions  This type of bond is weaker than covalent bond (-5 Kcal/mol).  At the same time, it is one of the most prevalent bonds in drug-receptor interaction.  The drug molecule must have opposite charge compared to the ionized amino acids found in the receptor or enzyme.  Extent of ionization affects the occurrence of this bond.  The distance between opposite charges has a role as well. Example  In biological systems, it happens between residues having carboxylate group such as aspartic acid & glutamic acid (acidic amino acids), and aminium ions such as Histidine, Lysine and Arginine (basic amino acids). Antidepressant drug pivagabine ION-DIPOLE AND DIPOLE-DIPOLE INTERACTIONS  Electronic dipole is formed when we have polarized bond due to electronegativity of atoms.  In the polarized bond one of the pole will be partially positive and the other partially negative.  These partially positive or negative charges might form an electrostatic bond with either partially charged atoms or ionized elements. Ion-dipole occur when an ionic group on one molecule interacts with a permanent dipole on a second molecule. It is stronger than dipole-dipole interactions (decreases relative to the square of separation). This type of interaction has the energy -1 to -7 Kcal/mol). Example of Drug: Zaleplon (treat insomnia). H-bonding  Should have H-Bond acceptor (the electron rich atom, slightly negative) and H-Bond donor (electron-deficient hydrogen, slightly positive).  Stability of this bond is -1 to -7 kcal/mol  H-bonds are between 1.5-2.2 Å.  Increase electron density, better H-Bond acceptor, so anions are better than uncharged compounds e.g. carboxylate anion.  If the lone pair on nitrogen atom are delocalized, this will weaken the HBD capacity H-Bond donors are better if the H is more electron deficient by attachment to more electron deficient atom such as quaternary ammonium compounds. Two types of H-bonding:  Intramolecular H-bonding: which occur within the same molecule.  Intermolecular H-bonding: occurs between two nearby molecules  The occurrence of intramolecular H-bonding could affect the pharmacological action of a drug:  P-hydroxybenzoate has more potent antibacterial action compared to methyl salicylate, it is normally used as food additive as preservative. CHARGE-TRANSFER INTERACTIONS  Occurs between an electron donor group in one molecule and an electron acceptor in another.  Electron donors such as alkenes, alkynes and aromatic ring bearing an electron donating group, and atoms having pairs of non-bonded electrons such as O, N and S  Electron acceptors such as aromatic ring bearing an electron withdrawing group,  These groups might exist in the receptor binding sites:  Electron donor such as aromatic ring of tyrosine and carboxylate group of aspartate.  Electron acceptor: cysteine  Having both: Histidine, tryptophan and Asparagine. Charge-Transfer bonds  HYDROPHOBIC INTERACTIONS ❑ When two nonpolar groups (lipophilic group on a drug and a nonpolar receptor group, each surrounded by ordered water molecules which become disordered in an attempt to associate with each other. ❑ This increase in entropy, therefore, results in a decrease in the free energy (ΔG = ΔH − TΔS), which stabilizes the drug–receptor complex. ❑ This stabilization is known as a hydrophobic interaction. HYDROPHOBIC INTERACTIONS Example of hydrophobic interactions Hydrophobic interactions are responsible for non- covalent intermolecular interactions in aqueous solution.  HYDROPHOBIC INTERACTIONS ❑ Another type of hydrophobic interactions is called as π-π interaction. ❑ This involve a parallel arrangement of aromatic rings in which the π-electrons interact in a face-to-face arrangement. Example: Anticonvulsant drug Lacosamide has phenyl ring (π electrons) The receptor has phenyl alanine contains the phenyl ring (π electrons)  Van der Waals forces  Occurs due to temporary non-symmetrical distribution of electron density, this will form temporary dipole that will interact with nearby dipole.  Stability accounts for only -0.5 kcal/mole, this means that this type of bonds are much weaker than other bonds. EXAMPLE OF POTENTIAL MULTIPLE DRUG–RECEPTOR INTERACTIONS Dibucaine, the local anaesthetic drug exhibits variety of interactions.  Receptor’s agonist  Agonists mimic the natural messenger of a receptor.  Agonists bind reversibly to the binding site and produce the same induced fit as the natural messenger - receptor is activated.  Similar intermolecular bonds formed as with natural messenger.  Agonists are often similar in structure to the natural messenger.  Receptor’s agonist  To design an agonist you have to know:  The geometry and topography of the active site and /or.  The chemical structure (preferably the 3D structure) of the normal substrate that act upon.  Requirements for agonist design:  The agonist must have the correct binding groups.  The binding groups must be correctly positioned to interact with complementary binding regions.  The drug must have the correct shape and size to fit the binding site The agonist must have the correct binding groups. The binding groups must be correctly positioned to interact with complementary binding regions. The drug must have the correct shape and size to fit the binding site  Receptor’s antagonist  Strategies to design an antagonists:  is to design a drug that has the right shape to bind to the receptor site, but which would fail to change the shape of the receptor  Receptor’s antagonist  Strategies to design an antagonists:  Allosteric antagonists  Receptor’s antagonist  Strategies to design an antagonists:  Antagonism by the 'umbrella’ effect: Here the drug will bind to a region close to binding site, once bound, part of its structure (tail) will cover the opening of the binding site....preventing the normal messenger from accessing the binding site  Competitive Antagonists: Compete with agonist for receptor binding => Agonist appears less potent, but can still achieve 100% effect but at higher concentrations. Non-competitive  Antagonists: Bind to receptor at different site and either prevent agonist binding or the agonist effect => maximal achievable response reduced.  affinity, efficacy, and potency  Affinity: how strongly the drug binds to the receptor; depends on the molecular complementarily of drug and receptor.  Efficacy: the maximum biological effect the drug can produce. A compound with high affinity does not necessarily have high efficacy (e.g. antagonists).  Potency: the amount of drug needed to achieve a defined biological effect. The smaller the dose required, the more potent the drug. It is possible to have potent drugs with low efficacy. Potency depends in part on the affinity of the receptor for binding the drug, and in part on the efficiency with which the drug-receptor interactions is coupled to response.  Recommended Books 1. The organic chemistry of drug design by Richard B. Silverman. Second edition, Elsevier, 2004. 2. An introduction to Medicinal Chemistry by Graham L. Patrick. Fourth edition, Oxford, 2009. 45 END LECTURE NOTES!