Theme 5 Lecture 16 Optimization of drug targets Flashcards
Lead optimisation (theme 3)
target selection-hit identification-lead identification- lead optimisation- candidate drug nomination -pre clinical development
LO process and identification of clinical candidates
Iterative process
In vitro assays then secondary as well as in vivo animal models.
Aims to identify clinical candidates with optimal potency, selectivity, efficacy, physical and pharmaceutical properties, and safety profile.
This process covers 3 main activities, what are they?
1)Optimisation of drug-target interactions via testing the bio activity of compounds in the assays(prim and sec)
2)Of drug like properties
3)In vivo testing for toxicity and safety= pre clinical studies (PHARMACEUTICAL TYPE PROPERTIES)
Importance of binding
In order for biological activity, the ligand needs to bind to its target.
High affinity and potency for the drugs=lower conc
High affinity for on target sites/low for off target=lower side effect
Understanding specific ligand- target interaction is essential for affinity
Binding as an equilibrium process, what is the equation?
Kd=(B)(P)/(BP)
The top is unbound and bottom is bound
Smaller Kd= higher affinity
The direction of the equation is solely relied on the Kd( moves right=unbound and left etc)
Energetics Of binding
Binding can only occur if it is energetically favourable
Enthalpy and entropy
Enthalpy is what you want for the reaction to be favourable which is deltaH, deltaS is entropy
Enthalpy which is deltaH needs to be more negative in order to be favourable.
∆𝐆 =∆𝐇−𝐓∆𝐒
Enthalpic consideration
Formation of the binding interactions between D and P=favourable interactions between h-bonding, dipoles(placements of F groups) and weaker VdW(good size and shape complementary)
Ligand(D) desolvation= increased water-water H-bonding enthalpic gains
Binding pocket (P)= Water-water interactions h bonding=enthalpic gains
Entropic considerations
Reduced rotational and translational freedom in DP compared to D+P
Water is in disordered state for desolvation and binding pocket
When its in the disordered state it can make more interactions with itself rather than interacting with the ligand
How does the equilibrium dissociation constant of a drug-target interaction relate to the Gibbs free energy of binding
∆𝑮 = −𝑹𝑻 𝒍𝒏 𝑲𝒅
∆𝑮= GIBBS FREE ENERGY OF BINDING
R=gas constant
T=temperature
Typical non-covalent drug target intercations
Ion-ion: Electrostatic interaction between two opposite formal charges
H-bonding: Electrostatic interaction between an electron-deficient hydrogen bonded to an electronegative atom (e.g. N, O, F) and the lone pair of electrons on an electronegative atom (e.g. N, O)
Dipole-dipole: Electrostatic interaction between permanent dipoles
Ion-dipole: Electrostatic interaction between a formal ion and a fixed dipole
Cation-𝜋: Electrostatic interaction between a cation and a delocalised 𝜋-system (i.e. an area of high electron density)
𝜋-𝜋: Orbital interaction between two 𝜋-systems
VdW: hydrophobic interactions
What do hydrophobic aliphatic interactions cause?
These cause desolvation at the binding site so can be entropically or enthalpic favourable
Some drugs bind through a covalent mechanism
Strongest type of interaction
Attack on the electrophilic centre by a nucleophilic protein residue.
Drug binding can compromise interactions (shape of drug)
The better the shape and fit of the drug in the binding pocket with good placement of the functional groups leads to higher affinity of the drugs.
This due to more favourable reactions with the proteins.
Drug stereochemistry is important, look at the photo on slide 14.
3 point contact model
R and S enantiomer
R has the 3 point contact with Pi-Pi, ionic and H bond-=more optimal
Whereas S has Pi-Pi and ionic but lacks H-bond.
3 types of enantiomers
eutomer- active
distomer- less
Eudismic- ratio of both=more stereoselectivity