Molecular Biology, Medicinal Chemistry and Computer Science for Pharmaceutical Applications

Activity type

Discipline chimiche

SSD

CHEM-03/A

Year

1st year

Semester

1st semester

CFU

3

Hours distribution

24 classroom hours

Lecturers

MARIA ELISA CRESTONI
CHIARA SALVITTI

Activity type

Discipline chimiche

SSD

CHEM-03/A

Year

1st year

Semester

1st semester

CFU

3

Hours distribution

24 classroom hours

Lecturers

CHIARA SALVITTI

The student will be able to:
- Understand and apply the fundamental laws of chemistry, such as the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.
- Describe the fundamental properties of atoms (atomic number, mass number, isotopes, atomic/molar mass), molecules, and ionic compounds.
- Correctly use the concepts of mole, Avogadro's number, and molecular weight in stoichiometric calculations.
- Balance chemical equations and determine the limiting reagent in a chemical reaction.
- Explain atomic structure in terms of quantum numbers and electron configuration, and predict periodic trends (ionization energy, electron affinity, atomic radius).
- Interpret and describe different types of chemical bonds (ionic, covalent, coordinate), the concept of resonance, and hybrid orbitals.
- Predict molecular geometry and discuss intermolecular forces affecting the physical properties of substances.
- Apply IUPAC nomenclature to correctly name basic chemical compounds.
- Describe the different states of matter and the related phase changes in terms of energy and intermolecular interactions.
- Understand the basic concepts of chemical thermodynamics, including the main state functions and the laws of thermodynamics.
- Analyze chemical equilibrium with reference to the law of mass action and the factors that influence equilibrium (Le Châtelier’s principle).
- Interpret the rate of a chemical reaction, determine its order, and explain the effect of temperature on the rate constant.
- Provide examples of catalyzed reactions and explain the role of catalysts.
- Understand and apply fundamental concepts related to solutions;
- Analyze and balance redox reactions.
- Describe the behavior of acids and bases.
- Perform acid-base titrations.
- Understand the principles of solubility.

1. Knowledge and Understanding
By the end of the course, the student will have acquired:
- Knowledge of the fundamental concepts of general and inorganic chemistry, including atomic structure, chemical bonding, the periodic table, states of matter, chemical thermodynamics, kinetics, and chemical equilibria.
- An understanding of the chemical behavior of elements and compounds, both at a theoretical level and through experimental or practical examples.

2. Applying Knowledge and Understanding
The student will be able to:
- Apply theoretical concepts to solve both quantitative and qualitative problems, such as stoichiometric calculations, pH determination, predictions of reaction spontaneity, equilibrium, and solubility.
- Use basic laboratory tools to interpret chemical data and relate them to theoretical principles.
- Integrate chemical knowledge with related disciplines (e.g., biology, physics, geosciences).

3. Making Judgements
The student will be able to:
- Critically analyze data, problems, and results related to chemical phenomena.
- Assess the validity of theoretical models and experimental outcomes.
- Formulate hypotheses about chemical phenomena and verify them using calculations or fundamental chemical concepts.

4. Communication Skills
The student will be able to:
- Communicate clearly and effectively, both orally and in writing, using appropriate scientific language.
- Describe fundamental chemical concepts, experimental procedures, and the results of exercises or problems logically and coherently.
- Interact with instructors and peers in collaborative learning settings or scientific discussions.

5. Learning Skills
The student will be able to:

- Independently organize the study of chemical content, using textbooks, multimedia materials, and scientific sources.
- Successfully engage with advanced courses in chemistry or related scientific fields, thanks to a solid theoretical and methodological foundation.
- Develop effective study methods for the continuous updating of knowledge in the field of chemical sciences.

Essential: The student must have a basic knowledge of algebra (first- and second-degree equations, properties of logarithms and exponents).
Important: Basic concepts of physics.
Useful: Basic rules of integrals and derivatives.

Module I:
Fundamental laws of chemistry. Mass number and atomic number, isotopes, atomic mass, atomic weight, molecules, molecular weight. The mole. Avogadro’s number. Ionic compounds. Chemical equations. The concept of limiting reagent.
Atomic structure. Quantum numbers. Electronic configuration. Ionization energy, electron affinity, and atomic radius. Periodic table of the elements.
Chemical bonding: bond order, bond energy, bond length. Ionic bond, covalent bond (nonpolar and polar), dipole moment, coordinate (dative) bond. Hybrid orbitals, resonance.
Structure of molecules and ions. Intermolecular forces. Systematic nomenclature.
States of matter and phase changes. Gaseous, liquid, and solid states.
Introduction to thermodynamics. Selected thermodynamic functions. The laws of thermodynamics. Chemical reactions and equilibria. Law of mass action. Factors affecting equilibrium.
Basic principles of chemical kinetics. Reaction rate and reaction order, rate constant and its temperature dependence. Examples of catalysis.
Stoichiometric calculations.

Module II:
Solutions, units of concentration, dilution, mixing, and colligative properties. Electrolytes and their properties in solution, van’t Hoff coefficient.
Oxidation number, redox reactions, and their balance.

Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Buffer solutions.
Titrations. Indicators.
Solubility. Solubility equilibria and influencing factors. Common ion effect.
Numerical exercises of Stoichiometry.

Chemistry,
Zumdahl/Zumdahl (Houghton Mifflin Company)
Any other General Chemistry textbook, provided it is at the university level.

Module: PRINCIPLES OF GENERAL AND INORGANIC CHEMISTRY I
N/D
Module: PRINCIPLES OF GENERAL AND INORGANIC CHEMISTRY II
N/D

The Principles of General and Inorganic Chemistry course consists of in-person lectures, structured as follows:
Module: Principles of General and Inorganic Chemistry I
- 18 hours of lectures
- 6 hours of numerical problem-solving sessions
Module: Principles of General and Inorganic Chemistry II
- 18 hours of lectures
- 6 hours of numerical problem-solving sessions

Teaching materials (lecture slides, stoichiometry exercises, archive of past exam papers) are made available on the course’s e-learning and Classroom platforms, where students can also find course information, the exam syllabus, and the list of recommended textbooks.

Attendance is not mandatory but is strongly recommended.

The exam consists of a written test lasting 120 minutes, comprising 30 multiple-choice and/or open-ended questions covering the topics discussed in class and listed in the course syllabus. The test may include numerical exercises in stoichiometry and/or questions on theoretical concepts. The aim is to assess the students’ basic knowledge of General and Inorganic Chemistry, as well as their ability to apply theoretical concepts to solve problems involving stoichiometric calculations. The exam is considered passed with a score of no less than 18 out of 30.
There are five written exams per year, held in January, February, June, July, and September, plus two additional extraordinary sessions in April and November. The latter two are reserved exclusively for graduating students, students who are behind schedule, and working students.

Multiple-choice and/or open-ended questions covering topics discussed during lectures and detailed in the course syllabus.
Numerical exercises involving stoichiometric calculations, used to assess the student's ability to apply theoretical concepts to problem-solving.
Throughout the course, sample questions and exercises will be provided during lectures, and exam simulations will be conducted at the end of each module.
An archive of past exam papers is available to students on the course’s e-learning page and via the Classroom platform.

• Lecture 1: Fundamental laws of chemistry. Mass number and atomic number, isotopes, atomic mass, atomic weight, molecules, molecular weight. The mole. Avogadro’s number. Ionic compounds. Chemical equations. The concept of limiting reagent. Stoichiometric calculations (numerical exercises).
  • Books: Teaching and didactic materials: Unit 1- Introduction to Chemistry


• Lecture 2:Atomic structure. Quantum numbers. Electronic configuration. Ionization energy, electron affinity, atomic radius. Periodic table of the elements. Stoichiometric calculations (numerical exercises).
  • Books: Teaching and didactic materials: Unit 2- Atomic structure and orbital model; Unit 3- Periodic table.


• Lecture 3:Chemical bonding: bond order, bond energy, bond length. Ionic bond, covalent bond (nonpolar and polar), dipole moment, coordinate (dative) bond. Hybrid orbitals, resonance. Structure of molecules and ions. Intermolecular forces.
  • Books: Teaching and didactic materials: Unit 4- Chemical bond; Unit 5- Molecular structures


• Lecture 4:Systematic nomenclature. States of matter: gaseous, liquid, and solid. Stoichiometric calculations (numerical exercises).
  • Books: Teaching and didactic materials: Unit 6- Nomenclature; Unit 7- Gaseous state; Unit 8- Solid and liquid states


• Lecture 5:Introduction to thermodynamics. Selected thermodynamic functions. The laws of thermodynamics. Introduction to chemical kinetics: reaction rate and order, rate constant and its temperature dependence. Examples of catalysis.
  • Books: Teaching and didactic materials: Unit 9- Thermochemistry; Unit 10- Kinetics


• Lecture 6:Chemical reactions and equilibria. Law of mass action. Factors affecting equilibrium. Phase transitions. Stoichiometric calculations (numerical exercises).
  • Books: Teaching and didactic materials: Unit 11- Chemical equilibrium; Unit 12- Phase transition


• Lecture 7: Solutions, units of concentration, dilution and mixing, colligative properties. Electrolytes and their properties in solution, van’t Hoff coefficient.
  • Books: Teaching and didactic materials: Unit 13 - Oxidation-reduction reactions


• Lecture 8: Oxidation number, redox reactions and their balance.
  • Books: Teaching and didactic materials: Unit 14 - Solutions and their properties; Unit 15 - Units of concentration, colligative properties


• Lecture 9: Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Buffer solutions.
  • Books: Teaching and didactic materials: Unit 16 – Aqueous Equilibria: Acids and Bases; Unit 17 – Salts; Unit 18 – Buffer Solutions; 


• Lecture 10: Titrations. Indicators.
  • Books: Teaching and didactic materials: Unit 19 – Titrations, Indicators


• Lecture 11: Solubility. Solubility equilibria and influencing factors. Common ion effect.
  • Books: Teaching and didactic materials:  Unit 20 – Solubility 


• Lecture 12: Numerical exercises of Stoichiometry.
  • Books: Teaching and didactic materials:  Stoichiometric exercises