Medicinal Chemistry 7th edition Test Bank| Page 1
, CHAPTER LIST
Part A: Drug Targets — Structure and Function
Chapter 1: Drugs and Drug Targets: An Overview
Chapter 2: Protein Structure and Function
Chapter 3: Enzymes — Structure and Function
Chapter 4: Receptors — Structure and Function
Chapter 5: Receptors and Signal Transduction
Chapter 6: Nucleic Acids — Structure and Function
Part B: Pharmacodynamics and Pharmacokinetics
Chapter 7: Enzymes as Drug Targets
Chapter 8: Receptors as Drug Targets
Chapter 9: Nucleic Acids as Drug Targets
Chapter 10: Miscellaneous Drug Targets
Chapter 11: Pharmacokinetics and Related Topics
Part C: Drug Discovery, Design, and Development
Chapter 12: Drug Discovery — Finding a Lead
Chapter 13: Drug Design — Optimizing Target Interactions
Chapter 14: Drug Design — Optimizing Access to the Target
Chapter 15: Getting the Drug to Market
Part D: Tools of the Trade
Chapter 16: Combinatorial and Parallel Synthesis
Chapter 17: In Silico Drug Design
Chapter 18: Quantitative Structure-Activity Relationships (QSAR)
Part E: Selected Topics in Medicinal Chemistry
Chapter 19: Antibacterial Agents
Chapter 20: Antiviral Agents
Chapter 21: Anticancer Agents
Chapter 22: Protein Kinase Inhibitors as Anticancer Agents
Chapter 23: Antibodies and Other Biologics
Chapter 24: Cholinergics, Anticholinergics, and Anticholinesterases
Chapter 25: Drugs Acting on the Adrenergic Nervous System
Chapter 26: The Opioid Analgesics
Chapter 27: Anti-Ulcer Agents
Chapter 28: Cardiovascular Drugs
Medicinal Chemistry 7th edition Test Bank| Page 2
,Chapter 1: Drugs and Drug Targets — An Overview
Q1. MCQ
A drug molecule forms a van der Waals interaction with a hydrophobic pocket in its
target protein. Which of the following best explains why this interaction, despite being
individually weak (~2 kJ/mol), is pharmacologically significant?
A. Van der Waals interactions have directional specificity that guides the drug into the
correct binding orientation.
B. Multiple van der Waals contacts across the drug–protein interface sum to provide
substantial cumulative binding energy.
C. Van der Waals interactions are strengthened by the aqueous environment
surrounding the binding site.
D. A single van der Waals contact of ~2 kJ/mol exceeds the energy of an ionic bond in a
biological system.
Answer: B
Rationale:
Patrick explains that van der Waals interactions are individually very weak (~2 kJ/mol) but
that a drug molecule makes many such contacts simultaneously with the target protein.
Their cumulative contribution to binding affinity is therefore significant. Option A is incorrect
because van der Waals interactions are non-directional induced-dipole forces, unlike
hydrogen bonds. Option C is wrong because the aqueous environment does not strengthen
hydrophobic/van der Waals interactions — it drives them (hydrophobic effect), but the water
is excluded from the pocket. Option D is incorrect; ionic bonds are far stronger (up to 40
kJ/mol in apolar environments).
Q2. MCQ
In comparing conventional hydrogen bonds with unconventional (C–H···O) hydrogen
bonds in drug–target interactions, which statement most accurately reflects the
content of Patrick's text?
A. C–H···O hydrogen bonds are stronger than conventional N–H···O bonds and are
preferred in drug design.
B. Unconventional hydrogen bonds are weaker than conventional ones but can still
contribute meaningfully to binding if present in sufficient number.
C. Unconventional hydrogen bonds are only found between drugs and nucleic acid
targets, not protein targets.
D. C–H···O interactions are considered repulsive forces that destabilise drug–target
complexes.
Answer: B
Rationale:
Medicinal Chemistry 7th edition Test Bank| Page 3
,Patrick discusses C–H···O and other unconventional hydrogen bonds as genuine, albeit
weaker, contributors to drug–target binding. They are weaker than conventional N–H···O or
O–H···O bonds but can contribute meaningfully in aggregate. Option A inverts their relative
strengths. Option C is incorrect — unconventional H-bonds occur with both protein and
nucleic acid targets. Option D is wrong; they are stabilising, not repulsive.
Q3. MCQ
Which of the following best describes the pharmacological basis for why most drugs
require multiple intermolecular interactions with their target rather than a single very
strong covalent bond?
A. Covalent bonds are too short-range to bridge the gap between a drug and its target
binding site.
B. Reversible binding through multiple non-covalent interactions allows the drug effect to
be terminated once the drug is eliminated, preserving normal physiological regulation. C.
Covalent bonds are too weak in biological environments due to the high dielectric
constant of water.
D. Non-covalent interactions are preferred because they allow the drug to bind
simultaneously to multiple unrelated targets.
Answer: B
Rationale:
Patrick emphasises that reversible, non-covalent drug–target binding is generally desirable
because it allows the drug effect to be switched off when the drug is metabolised or excreted,
enabling physiological control to be restored. Irreversible covalent binding (as with aspirin or
penicillin) is a deliberate exception. Option A is physically incorrect. Option C is wrong —
covalent bonds are not weakened by water's dielectric constant (that applies to
ionic/electrostatic interactions). Option D is incorrect; multi-target action of non-covalent
drugs is not the primary rationale for preferring them over covalent binding.
Q4. MCQ
Patrick describes cation–π interactions as relevant to drug binding. Which structural
feature of a drug molecule would be required to engage in a cation–π interaction with
a phenylalanine residue in the target protein?
A. A positively charged nitrogen (e.g., protonated amine) on the drug positioned above the
aromatic ring of Phe.
B. A negatively charged carboxylate on the drug interacting with the electron-rich face of
the Phe ring.
C. A halogen on the drug donating electron density to the σ-hole of Phe.
D. A polar hydroxyl group on the drug forming a water bridge with the Phe residue.
Answer: A
Rationale:
Medicinal Chemistry 7th edition Test Bank| Page 4
,Cation–π interactions, as described by Patrick, occur between a positively charged ion or
group (such as a protonated amine on the drug) and the electron-rich π system of an
aromatic ring (such as phenylalanine). The cation sits above the face of the aromatic ring,
stabilised by the negative electrostatic potential there. Option B describes an incorrect ion
polarity — it would be electrostatically repelled by the π face. Option C describes a halogen
bond (σ-hole interaction), not a cation–π interaction. Option D describes a conventional
hydrogen bond interaction, not cation–π.
Q5. MCQ
A newly developed drug has very high target affinity but shows negligible therapeutic
effect in vivo after oral administration. According to Patrick's overview of
pharmacokinetic issues, which of the following is the least likely explanation?
A. The drug is extensively metabolised to inactive products during first-pass metabolism.
B. The drug is too hydrophilic to cross intestinal epithelial membranes.
C. The drug binds irreversibly to its target, preventing normal physiological signalling. D.
The drug has poor distribution to the target tissue due to extensive plasma protein
binding.
Answer: C
Rationale:
Options A, B, and D are all well-established pharmacokinetic reasons why a drug with good
in vitro target affinity may fail in vivo — these are covered explicitly in Patrick's chapter on
pharmacokinetics. Option C describes a pharmacodynamic property (irreversible binding),
not a pharmacokinetic failure mode. Irreversible binding would, if anything, prolong rather
than reduce drug effect, and it does not explain why an orally administered drug with high
affinity fails to produce an effect — unless there is simply no drug reaching the target due to
pharmacokinetic issues. The question asks for the least likely explanation for lack of effect in
vivo, making option C the answer since irreversible binding if anything enhances duration,
not eliminates effect.
Q6. MCQ
Halogen bonds have been incorporated into modern drug design strategies. According
to Patrick, which property of a halogen atom enables it to act as a halogen bond
donor?
A. The halogen's lone pairs act as a Lewis acid to accept electrons from the target.
B. A region of positive electrostatic potential (σ-hole) at the tip of the carbon– halogen
bond interacts with an electron-rich acceptor.
C. The large atomic radius of heavier halogens enables direct orbital overlap with target
nitrogen atoms.
D. Halogens increase the dipole moment of the drug, strengthening conventional hydrogen
bonds nearby.
Answer: B
Medicinal Chemistry 7th edition Test Bank| Page 5
,Rationale:
Patrick explains that halogen bonds arise from the σ-hole — a region of positive electrostatic
potential at the tip of the C–X bond (opposite the carbon) — which can interact with
electronrich groups (lone pairs on O, N, S) in the target. This is counterintuitive since
halogens are electronegative but develop a positive cap due to anisotropy of electron
distribution. Option A reverses the roles: the σ-hole acts as a Lewis acid acceptor of electron
density, not the lone pairs of the halogen. Option C is incorrect; direct orbital overlap is not
the mechanism. Option D conflates the electronic effect with a different type of
intermolecular interaction.
Q7. MCQ
According to Patrick's classification of drugs, which of the following groupings would
place morphine (an opioid analgesic acting on μ-opioid receptors in the CNS) and
atenolol (a β1-selective adrenergic receptor blocker) in the same class?
A. Classification by pharmacological effect
B. Classification by target molecule (receptor type)
C. Classification by target system
D. Classification by chemical structure
Answer: C
Rationale:
Patrick describes classification by target system as grouping drugs that act on the same
physiological/pharmacological system. Both morphine (CNS, opioid receptors) and atenolol
(adrenergic receptors, cardiovascular system) are drugs acting on receptor-mediated
signalling systems within the nervous system — though different receptors, they share the
same broad target system category (G-protein–coupled receptors or receptor-based targets of
the nervous system). Classification by pharmacological effect (A) would separate them
(analgesic vs antihypertensive). Classification by target molecule (B) would also separate
them (μ-opioid vs β1-adrenergic receptor). Classification by chemical structure (D) would also
separate them (phenanthrene alkaloid vs aryloxypropanolamine).
Q8. MCQ
Patrick discusses repulsive interactions as relevant to drug design. In which scenario
would a repulsive steric interaction between a drug and its target protein be
deliberately exploited in a beneficial way?
A. To increase the binding affinity of an agonist by forcing the binding site into an active
conformation.
B. To confer selectivity by ensuring the drug binds one receptor subtype but is sterically
excluded from a closely related subtype.
C. To facilitate covalent bond formation between the drug and a catalytic residue in the
active site.
Medicinal Chemistry 7th edition Test Bank| Page 6
, D. To enhance membrane permeability by reducing the drug's polarity at physiological
pH.
Answer: B
Rationale:
Patrick notes that repulsive steric interactions, while generally unfavourable for binding, can
be deliberately engineered into drug molecules to exploit differences between related receptor
or enzyme subtypes. If a bulky group is added to a drug that is tolerated at one subtype but
sterically clashes with a residue unique to another subtype, selectivity is achieved. Option A
is incorrect because repulsive interactions reduce, not increase, agonist binding affinity.
Option C is incorrect; repulsion does not facilitate covalent bonding. Option D confuses steric
bulk with lipophilicity.
Q9. FILL-IN-THE-BLANK
The ________ interaction is responsible for the tendency of hydrophobic drug
molecules to associate with the hydrophobic core of a lipid bilayer or a protein's
hydrophobic binding pocket, driven primarily by an increase in the entropy of the
surrounding water molecules rather than a direct attractive force between the
nonpolar groups.
A. Van der Waals
B. Hydrophobic
C. π–π stacking
D. Dipole–dipole
Answer: B
Rationale:
Patrick explicitly explains the hydrophobic interaction as an entropy-driven phenomenon:
when nonpolar molecules associate together, the ordered water cage (clathrate) surrounding
each molecule is disrupted and water molecules are rel eased into bulk solvent, increasing
the overall entropy. This is the thermodynamic driving force, not a direct attractive force
between hydrophobic groups per se (though van der Waals forces also contribute). Option A
(van der Waals) represents the direct attractive force that accompanies hydrophobic contact
but is not the primary driver of the hydrophobic effect. Options C and D are specific
electronic interactions, not the general entropy-driven hydrophobic effect.
Q10. FILL-IN-THE-BLANK
When two aromatic rings in a drug–protein complex adopt a face-to-face or edge-
toface geometry, the stabilising interaction between them is classified as a ________
interaction.
A. Cation–π
B. Halogen bond
C. π–π (pi–pi stacking)
Medicinal Chemistry 7th edition Test Bank| Page 7
, CHAPTER LIST
Part A: Drug Targets — Structure and Function
Chapter 1: Drugs and Drug Targets: An Overview
Chapter 2: Protein Structure and Function
Chapter 3: Enzymes — Structure and Function
Chapter 4: Receptors — Structure and Function
Chapter 5: Receptors and Signal Transduction
Chapter 6: Nucleic Acids — Structure and Function
Part B: Pharmacodynamics and Pharmacokinetics
Chapter 7: Enzymes as Drug Targets
Chapter 8: Receptors as Drug Targets
Chapter 9: Nucleic Acids as Drug Targets
Chapter 10: Miscellaneous Drug Targets
Chapter 11: Pharmacokinetics and Related Topics
Part C: Drug Discovery, Design, and Development
Chapter 12: Drug Discovery — Finding a Lead
Chapter 13: Drug Design — Optimizing Target Interactions
Chapter 14: Drug Design — Optimizing Access to the Target
Chapter 15: Getting the Drug to Market
Part D: Tools of the Trade
Chapter 16: Combinatorial and Parallel Synthesis
Chapter 17: In Silico Drug Design
Chapter 18: Quantitative Structure-Activity Relationships (QSAR)
Part E: Selected Topics in Medicinal Chemistry
Chapter 19: Antibacterial Agents
Chapter 20: Antiviral Agents
Chapter 21: Anticancer Agents
Chapter 22: Protein Kinase Inhibitors as Anticancer Agents
Chapter 23: Antibodies and Other Biologics
Chapter 24: Cholinergics, Anticholinergics, and Anticholinesterases
Chapter 25: Drugs Acting on the Adrenergic Nervous System
Chapter 26: The Opioid Analgesics
Chapter 27: Anti-Ulcer Agents
Chapter 28: Cardiovascular Drugs
Medicinal Chemistry 7th edition Test Bank| Page 2
,Chapter 1: Drugs and Drug Targets — An Overview
Q1. MCQ
A drug molecule forms a van der Waals interaction with a hydrophobic pocket in its
target protein. Which of the following best explains why this interaction, despite being
individually weak (~2 kJ/mol), is pharmacologically significant?
A. Van der Waals interactions have directional specificity that guides the drug into the
correct binding orientation.
B. Multiple van der Waals contacts across the drug–protein interface sum to provide
substantial cumulative binding energy.
C. Van der Waals interactions are strengthened by the aqueous environment
surrounding the binding site.
D. A single van der Waals contact of ~2 kJ/mol exceeds the energy of an ionic bond in a
biological system.
Answer: B
Rationale:
Patrick explains that van der Waals interactions are individually very weak (~2 kJ/mol) but
that a drug molecule makes many such contacts simultaneously with the target protein.
Their cumulative contribution to binding affinity is therefore significant. Option A is incorrect
because van der Waals interactions are non-directional induced-dipole forces, unlike
hydrogen bonds. Option C is wrong because the aqueous environment does not strengthen
hydrophobic/van der Waals interactions — it drives them (hydrophobic effect), but the water
is excluded from the pocket. Option D is incorrect; ionic bonds are far stronger (up to 40
kJ/mol in apolar environments).
Q2. MCQ
In comparing conventional hydrogen bonds with unconventional (C–H···O) hydrogen
bonds in drug–target interactions, which statement most accurately reflects the
content of Patrick's text?
A. C–H···O hydrogen bonds are stronger than conventional N–H···O bonds and are
preferred in drug design.
B. Unconventional hydrogen bonds are weaker than conventional ones but can still
contribute meaningfully to binding if present in sufficient number.
C. Unconventional hydrogen bonds are only found between drugs and nucleic acid
targets, not protein targets.
D. C–H···O interactions are considered repulsive forces that destabilise drug–target
complexes.
Answer: B
Rationale:
Medicinal Chemistry 7th edition Test Bank| Page 3
,Patrick discusses C–H···O and other unconventional hydrogen bonds as genuine, albeit
weaker, contributors to drug–target binding. They are weaker than conventional N–H···O or
O–H···O bonds but can contribute meaningfully in aggregate. Option A inverts their relative
strengths. Option C is incorrect — unconventional H-bonds occur with both protein and
nucleic acid targets. Option D is wrong; they are stabilising, not repulsive.
Q3. MCQ
Which of the following best describes the pharmacological basis for why most drugs
require multiple intermolecular interactions with their target rather than a single very
strong covalent bond?
A. Covalent bonds are too short-range to bridge the gap between a drug and its target
binding site.
B. Reversible binding through multiple non-covalent interactions allows the drug effect to
be terminated once the drug is eliminated, preserving normal physiological regulation. C.
Covalent bonds are too weak in biological environments due to the high dielectric
constant of water.
D. Non-covalent interactions are preferred because they allow the drug to bind
simultaneously to multiple unrelated targets.
Answer: B
Rationale:
Patrick emphasises that reversible, non-covalent drug–target binding is generally desirable
because it allows the drug effect to be switched off when the drug is metabolised or excreted,
enabling physiological control to be restored. Irreversible covalent binding (as with aspirin or
penicillin) is a deliberate exception. Option A is physically incorrect. Option C is wrong —
covalent bonds are not weakened by water's dielectric constant (that applies to
ionic/electrostatic interactions). Option D is incorrect; multi-target action of non-covalent
drugs is not the primary rationale for preferring them over covalent binding.
Q4. MCQ
Patrick describes cation–π interactions as relevant to drug binding. Which structural
feature of a drug molecule would be required to engage in a cation–π interaction with
a phenylalanine residue in the target protein?
A. A positively charged nitrogen (e.g., protonated amine) on the drug positioned above the
aromatic ring of Phe.
B. A negatively charged carboxylate on the drug interacting with the electron-rich face of
the Phe ring.
C. A halogen on the drug donating electron density to the σ-hole of Phe.
D. A polar hydroxyl group on the drug forming a water bridge with the Phe residue.
Answer: A
Rationale:
Medicinal Chemistry 7th edition Test Bank| Page 4
,Cation–π interactions, as described by Patrick, occur between a positively charged ion or
group (such as a protonated amine on the drug) and the electron-rich π system of an
aromatic ring (such as phenylalanine). The cation sits above the face of the aromatic ring,
stabilised by the negative electrostatic potential there. Option B describes an incorrect ion
polarity — it would be electrostatically repelled by the π face. Option C describes a halogen
bond (σ-hole interaction), not a cation–π interaction. Option D describes a conventional
hydrogen bond interaction, not cation–π.
Q5. MCQ
A newly developed drug has very high target affinity but shows negligible therapeutic
effect in vivo after oral administration. According to Patrick's overview of
pharmacokinetic issues, which of the following is the least likely explanation?
A. The drug is extensively metabolised to inactive products during first-pass metabolism.
B. The drug is too hydrophilic to cross intestinal epithelial membranes.
C. The drug binds irreversibly to its target, preventing normal physiological signalling. D.
The drug has poor distribution to the target tissue due to extensive plasma protein
binding.
Answer: C
Rationale:
Options A, B, and D are all well-established pharmacokinetic reasons why a drug with good
in vitro target affinity may fail in vivo — these are covered explicitly in Patrick's chapter on
pharmacokinetics. Option C describes a pharmacodynamic property (irreversible binding),
not a pharmacokinetic failure mode. Irreversible binding would, if anything, prolong rather
than reduce drug effect, and it does not explain why an orally administered drug with high
affinity fails to produce an effect — unless there is simply no drug reaching the target due to
pharmacokinetic issues. The question asks for the least likely explanation for lack of effect in
vivo, making option C the answer since irreversible binding if anything enhances duration,
not eliminates effect.
Q6. MCQ
Halogen bonds have been incorporated into modern drug design strategies. According
to Patrick, which property of a halogen atom enables it to act as a halogen bond
donor?
A. The halogen's lone pairs act as a Lewis acid to accept electrons from the target.
B. A region of positive electrostatic potential (σ-hole) at the tip of the carbon– halogen
bond interacts with an electron-rich acceptor.
C. The large atomic radius of heavier halogens enables direct orbital overlap with target
nitrogen atoms.
D. Halogens increase the dipole moment of the drug, strengthening conventional hydrogen
bonds nearby.
Answer: B
Medicinal Chemistry 7th edition Test Bank| Page 5
,Rationale:
Patrick explains that halogen bonds arise from the σ-hole — a region of positive electrostatic
potential at the tip of the C–X bond (opposite the carbon) — which can interact with
electronrich groups (lone pairs on O, N, S) in the target. This is counterintuitive since
halogens are electronegative but develop a positive cap due to anisotropy of electron
distribution. Option A reverses the roles: the σ-hole acts as a Lewis acid acceptor of electron
density, not the lone pairs of the halogen. Option C is incorrect; direct orbital overlap is not
the mechanism. Option D conflates the electronic effect with a different type of
intermolecular interaction.
Q7. MCQ
According to Patrick's classification of drugs, which of the following groupings would
place morphine (an opioid analgesic acting on μ-opioid receptors in the CNS) and
atenolol (a β1-selective adrenergic receptor blocker) in the same class?
A. Classification by pharmacological effect
B. Classification by target molecule (receptor type)
C. Classification by target system
D. Classification by chemical structure
Answer: C
Rationale:
Patrick describes classification by target system as grouping drugs that act on the same
physiological/pharmacological system. Both morphine (CNS, opioid receptors) and atenolol
(adrenergic receptors, cardiovascular system) are drugs acting on receptor-mediated
signalling systems within the nervous system — though different receptors, they share the
same broad target system category (G-protein–coupled receptors or receptor-based targets of
the nervous system). Classification by pharmacological effect (A) would separate them
(analgesic vs antihypertensive). Classification by target molecule (B) would also separate
them (μ-opioid vs β1-adrenergic receptor). Classification by chemical structure (D) would also
separate them (phenanthrene alkaloid vs aryloxypropanolamine).
Q8. MCQ
Patrick discusses repulsive interactions as relevant to drug design. In which scenario
would a repulsive steric interaction between a drug and its target protein be
deliberately exploited in a beneficial way?
A. To increase the binding affinity of an agonist by forcing the binding site into an active
conformation.
B. To confer selectivity by ensuring the drug binds one receptor subtype but is sterically
excluded from a closely related subtype.
C. To facilitate covalent bond formation between the drug and a catalytic residue in the
active site.
Medicinal Chemistry 7th edition Test Bank| Page 6
, D. To enhance membrane permeability by reducing the drug's polarity at physiological
pH.
Answer: B
Rationale:
Patrick notes that repulsive steric interactions, while generally unfavourable for binding, can
be deliberately engineered into drug molecules to exploit differences between related receptor
or enzyme subtypes. If a bulky group is added to a drug that is tolerated at one subtype but
sterically clashes with a residue unique to another subtype, selectivity is achieved. Option A
is incorrect because repulsive interactions reduce, not increase, agonist binding affinity.
Option C is incorrect; repulsion does not facilitate covalent bonding. Option D confuses steric
bulk with lipophilicity.
Q9. FILL-IN-THE-BLANK
The ________ interaction is responsible for the tendency of hydrophobic drug
molecules to associate with the hydrophobic core of a lipid bilayer or a protein's
hydrophobic binding pocket, driven primarily by an increase in the entropy of the
surrounding water molecules rather than a direct attractive force between the
nonpolar groups.
A. Van der Waals
B. Hydrophobic
C. π–π stacking
D. Dipole–dipole
Answer: B
Rationale:
Patrick explicitly explains the hydrophobic interaction as an entropy-driven phenomenon:
when nonpolar molecules associate together, the ordered water cage (clathrate) surrounding
each molecule is disrupted and water molecules are rel eased into bulk solvent, increasing
the overall entropy. This is the thermodynamic driving force, not a direct attractive force
between hydrophobic groups per se (though van der Waals forces also contribute). Option A
(van der Waals) represents the direct attractive force that accompanies hydrophobic contact
but is not the primary driver of the hydrophobic effect. Options C and D are specific
electronic interactions, not the general entropy-driven hydrophobic effect.
Q10. FILL-IN-THE-BLANK
When two aromatic rings in a drug–protein complex adopt a face-to-face or edge-
toface geometry, the stabilising interaction between them is classified as a ________
interaction.
A. Cation–π
B. Halogen bond
C. π–π (pi–pi stacking)
Medicinal Chemistry 7th edition Test Bank| Page 7
