Medical Chemistry
A.Y. 2024/2025
Learning objectives
At the end of the course the student will be able to:
1.know the principles underlying the behaviors of elements and compounds involved in the main biological processes
2.know how to perform simple calculations that illustrate the quantitative aspects underlying the main biological processes
3.recognize the chemical principles that govern the behavior of substances of biomedical interest
4.know the mechanisms of reactions that occur in living organisms
5.know how to carry out practical operations typical of a chemical laboratory by acquiring practice in the main methodologies.
1.know the principles underlying the behaviors of elements and compounds involved in the main biological processes
2.know how to perform simple calculations that illustrate the quantitative aspects underlying the main biological processes
3.recognize the chemical principles that govern the behavior of substances of biomedical interest
4.know the mechanisms of reactions that occur in living organisms
5.know how to carry out practical operations typical of a chemical laboratory by acquiring practice in the main methodologies.
Expected learning outcomes
At the end of the course, the student will learn:
- to describe and use in simple calculations the basic quantities and their units of measure used in chemistry (atomic and molecular mass, mole and molar mass).
- to recognize the various types of chemical reactions and balance their stoichiometric coefficients in a rational way.
- to list the various ways in which the concentration of a solution can be expressed, define the solubility and the factors that influence it.
- to understand the concept of balance of a reaction and indicate how determined parameters can modify it.
- to discuss the concept of acids and bases according to the Broensted-Lowry theory.
- to describe the concept of pH of an aqueous solution and to calculate it in the case of both strong and weak acids and bases.
- to describe the methods for the experimental determination of the pH of a solution
- to describe the composition and properties of a buffer solution.
- to know and discuss some basic concepts of electrochemistry, thermodynamics and chemical kinetics.
- to recognize the different functional groups that characterize organic compounds, with particular reference to those present in the structures of compounds of biological interest, such as amino acids, proteins, carbohydrates, lipids, nucleotides and nucleic acids.
- to describe and use in simple calculations the basic quantities and their units of measure used in chemistry (atomic and molecular mass, mole and molar mass).
- to recognize the various types of chemical reactions and balance their stoichiometric coefficients in a rational way.
- to list the various ways in which the concentration of a solution can be expressed, define the solubility and the factors that influence it.
- to understand the concept of balance of a reaction and indicate how determined parameters can modify it.
- to discuss the concept of acids and bases according to the Broensted-Lowry theory.
- to describe the concept of pH of an aqueous solution and to calculate it in the case of both strong and weak acids and bases.
- to describe the methods for the experimental determination of the pH of a solution
- to describe the composition and properties of a buffer solution.
- to know and discuss some basic concepts of electrochemistry, thermodynamics and chemical kinetics.
- to recognize the different functional groups that characterize organic compounds, with particular reference to those present in the structures of compounds of biological interest, such as amino acids, proteins, carbohydrates, lipids, nucleotides and nucleic acids.
Lesson period: First semester
Assessment methods: Esame
Assessment result: voto verbalizzato in trentesimi
Single course
This course can be attended as a single course.
Course syllabus and organization
Single session
Responsible
Course syllabus
The course syllabus includes the following topics:
- GENERAL CHEMISTRY
Matter: pure substances (elements and compounds), mixtures (homogeneous and heterogeneous). Atoms, electrons, protons and neutrons. Atomic number, mass number, isotopes. Molecules and molecular formulas. Atomic and molecular masses. Mole and molar mass.
Quantization of energy. Uncertainty principle. Wave-particle duality. Atomic models. Quantum numbers and atomic orbitals. Electron configurations of the ground state.
Periodic table of chemical elements. Groups, periods, blocks. Periodic properties of elements (ionization energy, electron affinity, electronegativity). Metals, non-metals, noble gases.
Ionic bond, ionic compounds, lattice energy in ionic solids. Covalent bond. Multiple and single bonds. Lewis structures. Resonance.
Bond energy and bond lengths. Polar covalent bond, molecular dipole. Hybridization and hybrid orbitals. Molecular orbitals (σ and π).
Metallic bonding. Oxidation number.
Weak chemical bonds: between molecules (van der Waals forces), between ions and molecules, hydrogen bonding. Solvation energy.
Real and ideal gases, the ideal gas law.
Liquids. Surface tension. Vapor pressure. Crystalline and amorphous solids. Crystal types (ionic, covalent, molecular, metallic). Phase diagram for water. Triple point.
Solutions. Concentration of solutions (molarity, molality, mole fraction, percentage). Solubility. Effect of temperature on solubility. Effect of pressure on solubility of gases (Henry's law).
Colligative properties of solutions. Boiling point elevation and freezing point depression. Osmotic pressure.
Chemical reactions and balanced equations. Chemical equilibrium and equilibrium constant. Factors that affect the chemical equilibrium. Le Chatelier's principle.
Electrochemistry. Balancing redox reactions. The standard reduction potentials. Standard hydrogen electrode. Nernst equation. Galvanic cells.
Acids and bases. Arrhenius and Brønsted concepts of acids and bases. Conjugate acid-base pairs. Strengths of acids and bases. Self-ionization equilibrium and ion-product constant of water. pH concept. Acid and basic ionization constants (Ka and Kb). Relationships between Ka and Kb for conjugate acid-base pairs. Buffer solutions: concept, properties, reactions. pH calculation of aqueous solutions of acids and bases (strong and weak) and of acidic or basic ions. pH calculation of buffer solutions. Experimental determination of pH using acid-base indicators or by pH meters.
Lewis definitions of acids and bases. Coordination compounds, nomenclature, constant instability.
Chemical thermodynamics. Thermodynamic systems. State functions. Standard conditions. Heat and work. First law of thermodynamics. Enthalpy. Standard molar enthalpy of formation. Enthalpy change in reactions. Exothermic and endothermic reactions.
Factors affecting the reaction's spontaneity. Entropy. Second and third law of thermodynamics. Standard molar entropy. Entropy change in reactions. Free energy and standard molar free energy of formation. Calculation of #G in non-standard conditions.
Relationship between #G° and equilibrium constant. Coupled reactions.
Chemical kinetics. Reaction rates. Rate law and order of reaction. Activation energy and Arrhenius equation. Collision theory and transition state theory. Catalysts.
- ORGANIC CHEMISTRY AND PROPAEDEUTIC BIOCHEMISTRY
Introduction to organic chemistry. Functional groups and classification of organic compounds. Ionic and radical reactions. IUPAC rules for naming organic compounds.
Nomenclature, chemical properties, and characteristic reactions of following classes of compounds: saturated and unsaturated hydrocarbons (alkanes, alkenes, alkynes, cyclic, aromatic), alcohols, phenols, ethers, sulfur analogues (thioalcohols, thiophenols, thioethers, disulfides).
Aldehydes and ketones, nomenclature, properties, reactivity.
Carboxylic acids and fatty acids, nomenclature, properties, reactivity, soaps and their amphiphilic properties. Carboxylic acid derivatives (halides, anhydrides, esters, amides), properties, acid hydrolysis and basic hydrolysis (saponification).
Amines, nomenclature, properties, tetraalkylammonium salts. Simple bifunctional compounds, classification, nomenclature.
Isomerism. Classification of various types of isomerism: constitutional (of chain, of position, of function) and stereoisomerism (conformational, configurational, geometric isomerism). Chirality of the molecules (nomenclature D and L or R and S to identify stereogenic centers). Optical activity of the stereoisomers. Racemic and meso forms.
Lipids. Simple lipids (acylglycerols and waxes) and complex lipids (glycerophospholipids and sphingolipids). Acid and basic hydrolysis of lipids.
Carbohydrates. Monosaccharides, cyclic forms, epimers and anomers. Glycosides, reducing and non-reducing disaccharides (maltose, lactose, cellobiose, sucrose). Homopolysaccharides (starch, glycogen, cellulose, chitin).
Amino acids. Definition and classification, isoionic point, isoelectric point. Predominant forms at physiological pH. Peptides and proteins, classification, peptide bond and its characteristics. Primary, secondary, tertiary and quaternary structures. Denaturation.
Nucleosides and nucleotides. Structure of nucleic acids (DNA and RNA).
- GENERAL CHEMISTRY
Matter: pure substances (elements and compounds), mixtures (homogeneous and heterogeneous). Atoms, electrons, protons and neutrons. Atomic number, mass number, isotopes. Molecules and molecular formulas. Atomic and molecular masses. Mole and molar mass.
Quantization of energy. Uncertainty principle. Wave-particle duality. Atomic models. Quantum numbers and atomic orbitals. Electron configurations of the ground state.
Periodic table of chemical elements. Groups, periods, blocks. Periodic properties of elements (ionization energy, electron affinity, electronegativity). Metals, non-metals, noble gases.
Ionic bond, ionic compounds, lattice energy in ionic solids. Covalent bond. Multiple and single bonds. Lewis structures. Resonance.
Bond energy and bond lengths. Polar covalent bond, molecular dipole. Hybridization and hybrid orbitals. Molecular orbitals (σ and π).
Metallic bonding. Oxidation number.
Weak chemical bonds: between molecules (van der Waals forces), between ions and molecules, hydrogen bonding. Solvation energy.
Real and ideal gases, the ideal gas law.
Liquids. Surface tension. Vapor pressure. Crystalline and amorphous solids. Crystal types (ionic, covalent, molecular, metallic). Phase diagram for water. Triple point.
Solutions. Concentration of solutions (molarity, molality, mole fraction, percentage). Solubility. Effect of temperature on solubility. Effect of pressure on solubility of gases (Henry's law).
Colligative properties of solutions. Boiling point elevation and freezing point depression. Osmotic pressure.
Chemical reactions and balanced equations. Chemical equilibrium and equilibrium constant. Factors that affect the chemical equilibrium. Le Chatelier's principle.
Electrochemistry. Balancing redox reactions. The standard reduction potentials. Standard hydrogen electrode. Nernst equation. Galvanic cells.
Acids and bases. Arrhenius and Brønsted concepts of acids and bases. Conjugate acid-base pairs. Strengths of acids and bases. Self-ionization equilibrium and ion-product constant of water. pH concept. Acid and basic ionization constants (Ka and Kb). Relationships between Ka and Kb for conjugate acid-base pairs. Buffer solutions: concept, properties, reactions. pH calculation of aqueous solutions of acids and bases (strong and weak) and of acidic or basic ions. pH calculation of buffer solutions. Experimental determination of pH using acid-base indicators or by pH meters.
Lewis definitions of acids and bases. Coordination compounds, nomenclature, constant instability.
Chemical thermodynamics. Thermodynamic systems. State functions. Standard conditions. Heat and work. First law of thermodynamics. Enthalpy. Standard molar enthalpy of formation. Enthalpy change in reactions. Exothermic and endothermic reactions.
Factors affecting the reaction's spontaneity. Entropy. Second and third law of thermodynamics. Standard molar entropy. Entropy change in reactions. Free energy and standard molar free energy of formation. Calculation of #G in non-standard conditions.
Relationship between #G° and equilibrium constant. Coupled reactions.
Chemical kinetics. Reaction rates. Rate law and order of reaction. Activation energy and Arrhenius equation. Collision theory and transition state theory. Catalysts.
- ORGANIC CHEMISTRY AND PROPAEDEUTIC BIOCHEMISTRY
Introduction to organic chemistry. Functional groups and classification of organic compounds. Ionic and radical reactions. IUPAC rules for naming organic compounds.
Nomenclature, chemical properties, and characteristic reactions of following classes of compounds: saturated and unsaturated hydrocarbons (alkanes, alkenes, alkynes, cyclic, aromatic), alcohols, phenols, ethers, sulfur analogues (thioalcohols, thiophenols, thioethers, disulfides).
Aldehydes and ketones, nomenclature, properties, reactivity.
Carboxylic acids and fatty acids, nomenclature, properties, reactivity, soaps and their amphiphilic properties. Carboxylic acid derivatives (halides, anhydrides, esters, amides), properties, acid hydrolysis and basic hydrolysis (saponification).
Amines, nomenclature, properties, tetraalkylammonium salts. Simple bifunctional compounds, classification, nomenclature.
Isomerism. Classification of various types of isomerism: constitutional (of chain, of position, of function) and stereoisomerism (conformational, configurational, geometric isomerism). Chirality of the molecules (nomenclature D and L or R and S to identify stereogenic centers). Optical activity of the stereoisomers. Racemic and meso forms.
Lipids. Simple lipids (acylglycerols and waxes) and complex lipids (glycerophospholipids and sphingolipids). Acid and basic hydrolysis of lipids.
Carbohydrates. Monosaccharides, cyclic forms, epimers and anomers. Glycosides, reducing and non-reducing disaccharides (maltose, lactose, cellobiose, sucrose). Homopolysaccharides (starch, glycogen, cellulose, chitin).
Amino acids. Definition and classification, isoionic point, isoelectric point. Predominant forms at physiological pH. Peptides and proteins, classification, peptide bond and its characteristics. Primary, secondary, tertiary and quaternary structures. Denaturation.
Nucleosides and nucleotides. Structure of nucleic acids (DNA and RNA).
Prerequisites for admission
No prior knowledge of Chemistry is required, as the course is designed to be accessible to students who have not previously studied chemistry topics.
Teaching methods
The course will be delivered through lectures (frontal lessons) using slides, which will be made available in PDF format on the myAriel educational platform for Medical Chemistry.
Teaching Resources
Anastasia - Chimica di Base per le Scienze della Vita, 2ª ed. (Vol I e II), Antonio Delfino Editore.
Bellini T. - Chimica medica e propedeutica biochimica, Zanichelli.
Bellini T. - Chimica medica e propedeutica biochimica, Zanichelli.
Assessment methods and Criteria
The assessment method is a written test with a duration of 90 minutes and consists of 10 open-ended questions. Using a calculator is allowed for the exam.
In the evaluation, each individual answer is given a score from 0 to 3, and the sum of the points assigned to the answers represents the grade expressed out of thirty.
On a day following the written exam, an oral interview is scheduled, which essentially involves discussing with the student the evaluation given to their response to each single question of the written test.
In the evaluation, each individual answer is given a score from 0 to 3, and the sum of the points assigned to the answers represents the grade expressed out of thirty.
On a day following the written exam, an oral interview is scheduled, which essentially involves discussing with the student the evaluation given to their response to each single question of the written test.
BIO/10 - BIOCHEMISTRY - University credits: 4
Lessons: 40 hours
Professor:
Morelli Laura
Educational website(s)