1 / 63

Patrick An Introduction to Medicinal Chemistry 3/e Chapter 13

Patrick An Introduction to Medicinal Chemistry 3/e Chapter 13 QUANTITATIVE STRUCTURE-ACTIVITY RELATIONSHIPS (QSAR). Contents 1. Introduction 2. Hydrophobicity of the Molecule (4 slides) 3. Hydrophobicity of Substituents (2 slides) 4. Electronic Effects

ulysses-austin
Download Presentation

Patrick An Introduction to Medicinal Chemistry 3/e Chapter 13

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Patrick An Introduction to Medicinal Chemistry 3/e Chapter 13 QUANTITATIVE STRUCTURE-ACTIVITY RELATIONSHIPS (QSAR)

  2. Contents 1. Introduction 2. Hydrophobicity of the Molecule (4 slides) 3. Hydrophobicity of Substituents (2 slides) 4. Electronic Effects 4.1. Hammett Substituent Constant (s) (7 slides) 4.2. Electronic Factors R & F 4.3. Aliphatic electronic substituents 5. Steric Factors (3 slides) 6. Hansch Equation (4 slides) 7. Craig Plot (2 slides) 8. Topliss Scheme (5 slides) 9. Bio-isosteres 10. Free-Wilson Approach (3 slides) 11. Case Study (10 slides) 12. 3D-QSAR (10 slides) 13. 3D-QSAR Case Study(7 slides) [62 slides]

  3. Most common properties studied 1. Introduction • Aims • To relate the biological activity of a series of compounds to their physicochemical parameters in a quantitative fashion using a mathematical formula • Requirements • Quantitative measurements for biological and physicochemical properties • Physicochemical Properties • Hydrophobicity of the molecule • Hydrophobicity of substituents • Electronic properties of substituents • Steric properties of substituents

  4. [Drug in octanol] Partition Coefficient P = [Drug in water] High P High hydrophobicity 2. Hydrophobicity of the Molecule

  5. . . Log (1/C) . . . . . . . 1 æ Log ö 0.75 logP + 2.30 = C è ø 0.78 3.82 Log P 2. Hydrophobicity of the Molecule • Activity of drugs is often related to P • e.g. binding of drugs to serum albumin • (straight line - limited range of log P) • Binding increases as log P increases • Binding is greater for hydrophobic drugs

  6. Log (1/C) 1 2 æ Log ö - 0.22(logP) + 1.04 logP + 2.16 = C è ø o Log P Log P 2. Hydrophobicity of the Molecule Example 2 General anaesthetic activity of ethers (parabolic curve - larger range of log P values) Optimum value of log P for anaesthetic activity = log Po

  7. 2. Hydrophobicity of the Molecule • QSAR equations are only applicable to compounds in the same structural class (e.g. ethers) • However, log Po is similar for anaesthetics of different structural classes (ca. 2.3) • Structures with log P ca. 2.3 enter the CNS easily • (e.g. potent barbiturates have a log P of approximately 2.0) • Can alter log P value of drugs away from 2.0 to avoid CNS side effects

  8. C l C O N H 2 Benzene Chlorobenzene Benzamide (Log P = 2.13) (Log P = 2.84) (Log P = 0.64) pCl = 0.71 pCONH = -1.49 2 3. Hydrophobicity of Substituents - the substituent hydrophobicity constant (p) • A measure of a substituent’s hydrophobicity relative to hydrogen • Tabulated values exist for aliphatic and aromatic substituents • Measured experimentally by comparison of log P’s with parent structure Example : • Positive values imply substituents are more hydrophobic than H • Negative values imply substituents are less • hydrophobic than H

  9. Example : C l Log P(theory) = log P(benzene) + pCl +pCONH = 2.13 + 0.71 - 1.49 = 1.35 Log P(observed) = 1.51 2 C O N H 2 meta -Chlorobenzamide 3. Hydrophobicity of Substituents - the substituent hydrophobicity constant (p) • The value of p is only valid for parent structures • It is possible to calculate log P using p values • A QSAR equation may include both P and p. • P measures the importance of a molecule’s overall hydrophobicity (relevant to absorption, binding etc) • p identifies specific regions of the molecule which might interact with hydrophobic regions in the binding site

  10. - [PhCO ] 2 X=H K = Dissociation constant = H H] [PhCO 2 4. Electronic Effects 4.1 Hammett Substituent Constant (s) • The constant (s) a measure of the e-withdrawing or e-donating influence of substituents • It can be measured experimentally and tabulated • (e.g. s for aromatic substituents is measured by comparing the dissociation constants of substituted benzoic acids with benzoic acid)

  11. K X s = log = logK - logK X H X K H 4.1 Hammett Substituent Constant (s) X= electron withdrawing group (e.g. NO2) Charge is stabilised by X Equilibrium shifts to right KX > KH Positive value

  12. K X s = log = logK - logK X H X K H 4.1 Hammett Substituent Constant (s) X= electron donating group (e.g. CH3) Charge destabilised Equilibrium shifts to left KX < KH Negative value

  13. 4.1 Hammett Substituent Constant (s) s value depends on inductive and resonance effects s value depends on whether the substituent is meta or para ortho values are invalid due to steric factors

  14. sm (NO2) = 0.71 meta-Substitution sp (NO2) = 0.78 para-Substitution 4.1 Hammett Substituent Constant (s) EXAMPLES: e-withdrawing (inductive effect only) e-withdrawing (inductive + resonance effects)

  15. meta-Substitution sp (OH) = -0.37 sm (OH) = 0.12 para-Substitution 4.1 Hammett Substituent Constant (s) EXAMPLES: e-withdrawing (inductive effect only) e-donating by resonance more important than inductive effect

  16. 1 æ log 2.282 - 0.348 ö = s C è ø 4.1 Hammett Substituent Constant (s) QSAR Equation: Diethylphenylphosphates (Insecticides) Conclusion : e-withdrawing substituents increase activity

  17. 4.2 Electronic Factors R & F • R - Quantifies a substituent’s resonance effects • F - Quantifies a substituent’s inductive effects

  18. X= electron donating Rate sI = -ve X= electron withdrawing Rate sI = +ve 4.3 Aliphatic electronic substituents • Defined by sI • Purely inductive effects • Obtained experimentally by measuring the rates of hydrolyses of aliphatic esters • Hydrolysis rates measured under basic and acidic conditions Basic conditions: Rate affected by steric + electronic factors Gives sI after correction for steric effect Acidic conditions: Rate affected by steric factors only (see Es)

  19. 5. Steric Factors Taft’s Steric Factor (Es) • Measured by comparing the rates of hydrolysis of substituted aliphatic esters against a standard ester under acidic conditions • Es = log kx - log ko kx represents the rate of hydrolysis of a substituted ester • ko represents the rate of hydrolysis of the parent ester • Limited to substituents which interact sterically with the tetrahedral transition state for the reaction • Cannot be used for substituents which interact with the transition state by resonance or hydrogen bonding • May undervalue the steric effect of groups in an intermolecular process (i.e. a drug binding to a receptor)

  20. 2 (n - 1) mol. wt. MR = x density 2 (n - 2) Correction factor for polarisation (n=index of refraction) Defines volume 5. Steric Factors Molar Refractivity (MR) - a measure of a substituent’s volume

  21. B4 B3 Example - Carboxylic acid B 3 B2 B1 B 4 L 5. Steric Factors Verloop Steric Parameter - calculated by software (STERIMOL) - gives dimensions of a substituent - can be used for any substituent

  22. 2 1 æ Log ö - k (logP) + k logP + k + k E + k = s s C è ø 1 2 3 4 5 6. Hansch Equation • A QSAR equation relating various physicochemical properties to the biological activity of a series of compounds • Usually includes log P, electronic and steric factors • Start with simple equations and elaborate as more structures are synthesised • Typical equation for a wide range of log P is parabolic

  23. Example: Adrenergic blocking activity of b-halo-b-arylamines 1 æ Log 1.22 - 1.59 + 7.89 ö = p s C è ø 6. Hansch Equation • Conclusions: • Activity increases if p is +ve (i.e. hydrophobic substituents) • Activity increases if s is negative (i.e. e-donating substituents)

  24. 1 2 æ ö Log - 0.015 (logP) + 0.14 logP + 0.27 + 0.40 + 0.65 + 0.88 + 2.34 = S p S p S s S s C è ø X Y X Y 6. Hansch Equation Example: Antimalarial activity of phenanthrene aminocarbinols • Conclusions: • Activity increases slightly as log P (hydrophobicity) increases (note that the constant is only 0.14) • Parabolic equation implies an optimum log Po value for activity • Activity increases for hydrophobic substituents (esp. ring Y) • Activity increases for e-withdrawing substituents (esp. ring Y)

  25. Correlated values. Are any differences due to p or MR? No correlation in values Valid for analysing effects of p and MR. 6. Hansch Equation Choosing suitable substituents • Substituents must be chosen to satisfy the following criteria: • A range of values for each physicochemical property studied • values must not be correlated for different properties (i.e. they must be orthogonal in value) • at least 5 structures are required for each parameter studied Substituent H Me Et n-Pr n-Bu p 0.00 0.56 1.02 1.50 2.13 MR 0.10 0.56 1.03 1.55 1.96 Substituent H Me OMe NHCONH2 I CN p 0.00 0.56 -0.02 -1.30 1.12 -0.57 MR 0.10 0.56 0.79 1.37 1.39 0.63

  26. +s -p +s +p -p +p -s -p -s +p 7. Craig Plot Craig plot shows values for 2 different physicochemical properties for various substituents Example:

  27. 7. Craig Plot • Allows an easy identification of suitable substituents for a QSAR analysis which includes both relevant properties • Choose a substituent from each quadrant to ensure orthogonality • Choose substituents with a range of values for each property

  28. 8. Topliss Scheme Used to decide which substituents to use if optimising compounds one by one (where synthesis is complex and slow) Example: Aromatic substituents

  29. Act. Act. Little change add second Cl to increase p and s further replace with OMe (-p and -s) replace with Me (+p and -s) 8. Topliss Scheme Rationale Replace H with para-Cl (+p and +s) +p and/or +s advantageous favourable p unfavourable s +p and/or +s disadvantageous Further changes suggested based on arguments of p, s and steric strain

  30. 8. Topliss Scheme Aliphatic substituents

  31. 8. Topliss Scheme Example

  32. 8. Topliss Scheme Example

  33. p -0.55 0.40 -1.58 -1.63 -1.82 -1.51 sp 0.50 0.84 0.49 0.72 0.57 0.36 sm 0.38 0.66 0.52 0.60 0.46 0.35 MR 11.2 21.5 13.7 13.5 16.9 19.2 9. Bio-isosteres • Choose substituents with similar physicochemical properties (e.g. CN, NO2 and COMe could be bio-isosteres) • Choose bio-isosteres based on most important physicochemical property • (e.g. COMe & SOMe are similar in sp; SOMe and SO2Me are similar in p)

  34. 10. Free-Wilson Approach Method • The biological activity of the parent structure is measured and compared with the activity of analogues bearing different substituents • An equation is derived relating biological activity to the presence or absence of particular substituents Activity = k1X1 + k2X2 +.…knXn + Z • Xn is an indicator variable which is given the value 0 or 1 depending on whether the substituent (n) is present or not • The contribution of each substituent (n) to activity is determined by the value of kn • Z is a constant representing the overall activity of the structures studied

  35. 10. Free-Wilson Approach Advantages • No need for physicochemical constants or tables • Useful for structures with unusual substituents • Useful for quantifying the biological effects of molecular features that cannot be quantified or tabulated by the Hansch method Disadvantages • A large number of analogues need to be synthesised to represent each different substituent and each different position of a substituent • It is difficult to rationalise why specific substituents are good or bad for activity • The effects of different substituents may not be additive • (e.g. intramolecular interactions)

  36. 10. Free-Wilson / Hansch Approach Advantages • It is possible to use indicator variables as part of a Hansch equation - see following Case Study

  37. 11. Case Study QSAR analysis of pyranenamines (SK & F) (Anti-allergy compounds)

  38. 1 2 æ ö Log - 0.14 - 1.35( ) 0.72 = S p S s - C è ø Sp and Ss = total values for p and s for all substituents 11. Case Study Stage 1 19 structures were synthesised to study p and s • Conclusions: • Activity drops as p increases • Hydrophobic substituents are bad for activity - unusual • Any value of s results in a drop in activity • Substituents should not be e-donating or e-withdrawing (activity falls if s is +ve or -ve)

  39. 11. Case Study Stage 2 61 structures were synthesised, concentrating on hydrophilic substituents to test the first equation Anomalies a) 3-NHCOMe, 3-NHCOEt, 3-NHCOPr. Activity should drop as alkyl group becomes bigger and more hydrophobic, but the activity is similar for all three substituents b) OH, SH, NH2 and NHCOR at position 5 : Activity is greater than expected c) NHSO2R : Activity is worse than expected d) 3,5-(CF3)2 and 3,5(NHMe)2 : Activity is greater than expected e) 4-Acyloxy : Activity is 5 x greater than expected

  40. 11. Case Study Theories a) 3-NHCOMe, 3-NHCOEt, 3-NHCOPr. Possible steric factor at work. Increasing the size of R may be good for activity and balances out the detrimental effect of increasing hydrophobicity b) OH, SH, NH2, and NHCOR at position 5 Possibly involved in H-bonding c) NHSO2R Exception to H-bonding theory - perhaps bad for steric or electronic reasons d) 3,5-(CF3)2 and 3,5-(NHMe)2 The only disubstituted structures where a substituent at position 5 was electron withdrawing e) 4-Acyloxy Presumably acts as a prodrug allowing easier crossing of cell membranes. The group is hydrolysed once across the membrane.

  41. 1 2 æ Log - 0.30 - 1.35( ) + 2.0(F - 5) + 0.39(345 - HBD) - 0.63(NHSO ) ö = S p S s 2 C è ø + 0.78(M - V) + 0.72(4 - OCO) - 0.75 11. Case Study Stage 3 Alter the QSAR equation to take account of new results Conclusions (F-5) e-withdrawing group at position 5 increases activity (based on only 2 compounds though) (3,4,5-HBD) H-bond donor group at positions 3, 4,or 5 is good for activity Term = 1 if a HBD group is at any of these positions Term = 2 if HBD groups are at two of these positions Term = 0 if no HBD group is present at these positions Each HBD group increases activity by 0.39 (NHSO2) Equals 1 if NHSO2 is present (bad for activity by -0.63). Equals zero if group is absent. (M-V) Volume of any meta substituent. Large substituents at meta position increase activity 4-O-CO Equals 1 if acyloxy group is present (activity increases by 0.72). Equals 0 if group absent

  42. 1 2 æ Log - 0.30 - 1.35( ) + 2.0(F - 5) + 0.39(345 - HBD) - 0.63(NHSO ) ö = S p S s 2 C è ø + 0.78(M - V) + 0.72(4 - OCO) - 0.75 11. Case Study Stage 3 Alter the QSAR equation to take account of new results The terms (3,4,5-HBD), (NHSO2), and 4-O-CO are examples of indicator variables used in the free-Wilson approach and included in a Hansch equation

  43. 11. Case Study Stage 4 37 Structures were synthesised to test steric and F-5 parameters, as well as the effects of hydrophilic, H-bonding groups Anomalies Two H-bonding groups are bad if they are ortho to each other Explanation Possibly groups at the ortho position bond with each other rather than with the receptor - an intramolecular interaction

  44. 1 2 2 æ Log - 0.034( ) - 0.33 + 4.3(F - 5) + 1.3 (R - 5) - 1.7( ) + 0.73(345 - HBD) ö = S p S p S s C è ø - 0.86 (HB - INTRA) - 0.69(NHSO ) + 0.72(4 - OCO) - 0.59 2 11. Case Study Stage 5 Revise Equation a) Increasing the hydrophilicity of substituents allows the identification of an optimum value for p (Sp = -5). The equation is now parabolic (-0.034 (Sp)2) b) The optimum value of Sp is very low and implies a hydrophilic binding site c) R-5 implies that resonance effects are important at position 5 d) HB-INTRA equals 1 for H-bonding groups ortho to each other (act. drops -086) equals 0 if H-bonding groups are not ortho to each other e) The steric parameter is no longer significant and is not present

  45. XH X X X NH3 11. Case Study Stage 6 Optimum Structure and binding theory

  46. 11. Case Study NOTES on the optimum structure • It has unusual NHCOCH(OH)CH2OH groups at positions 3 and 5 • It is 1000 times more active than the lead compound • The substituents at positions 3 and 5 • are highly polar, • are capable of H-bonding, • are at the meta positions and are not ortho to each other • allow a favourable F-5 parameter for the substituent at position 5 • The structure has a negligible (Ss)2 value

  47. 12. 3D-QSAR • Physical properties are measured for the molecule as a whole • Properties are calculated using computer software • No experimental constants or measurements are involved • Properties are known as ‘Fields’ • Steric field - defines the size and shape of the molecule • Electrostatic field - defines electron rich/poor regions of • molecule • Hydrophobic properties are relatively unimportant Advantages over QSAR • No reliance on experimental values • Can be applied to molecules with unusual substituents • Not restricted to molecules of the same structural class • Predictive capability

  48. Build 3D model Active conformation Define pharmacophore 12. 3D-QSAR Method • Comparative molecular field analysis (CoMFA) - Tripos • Build each molecule using modelling software • Identify the active conformation for each molecule • Identify the pharmacophore

  49. Build 3D model 12. 3D-QSAR Method • Comparative molecular field analysis (CoMFA) - Tripos • Build each molecule using modelling software • Identify the active conformation for each molecule • Identify the pharmacophore Active conformation Define pharmacophore

  50. . . . . . Grid points 12. 3D-QSAR Method • Place the pharmacophore into a lattice of grid points • Each grid point defines a point in space

More Related