Chemistry and Introductory Biochemistry
A.Y. 2023/2024
Learning objectives
The course aims to provide students with the basics of chemistry that make it possible to understand the behavior of the compounds involved in the main biological processes and the knowledge necessary to understand the quantitative aspects involved, with particular reference to some topics preparatory to next courses, such as the structures and chemical properties of carbohydrates, lipids, amino acids, proteins, nucleotides and nucleic acids.
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 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 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. 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, atomic radius). 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 and
Metallic bonding. Oxidation number.
Weak chemical bonds: between molecules (van der Waals forces), hydrogen bonding, between ions and molecules. Solvation energy. Real and ideal gases, the ideal gas law.
Liquids. Surface tension. Vapor pressure. Crystalline solids: 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. Osmotic pressure.
Chemical reactions and balanced equations. Chemical equilibrium and equilibrium constant. Factors that affect the chemical equilibrium. Le-Chatelier's principle.
Electrochemistry. The standard reduction potentials. Standard hydrogen electrode. Nernst equation. Galvanic cells.
Acids and bases. Arrhenius, Bronsted-Lowry and Lewis 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) pH calculation of buffer solutions.
Chemical thermodynamics. Thermodynamic systems. State functions. Standard conditions. Heat and work. Enthalpy. Exothermic and endothermic reactions.
Factors affecting the reaction's spontaneity. Entropy. Free energy and standard molar free energy of formation. Calculation of ΔG in non-standard conditions. Relationship between ΔG° 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 TO BIOCHEMISTRY
Introduction to organic chemistry. Functional groups and classification of organic compounds. Ionic and radical reactions. 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.
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, tetra alkylammonium 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. Characteristics and functions of simple lipids (triglycerides) and complex lipids (sphingolipids and glyceropholipids). Carbohydrates. Characteristics and functions of monosaccharides, cyclic forms and polysaccharides (homo polysaccharides: starch, glycogen, cellulose, chitin and hetero polysaccharides: (peptidoglycans)
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. Nucleic Acid. Nucleosides and nucleotides. Structure, characteristics and functions 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. 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, atomic radius). 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 and
Metallic bonding. Oxidation number.
Weak chemical bonds: between molecules (van der Waals forces), hydrogen bonding, between ions and molecules. Solvation energy. Real and ideal gases, the ideal gas law.
Liquids. Surface tension. Vapor pressure. Crystalline solids: 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. Osmotic pressure.
Chemical reactions and balanced equations. Chemical equilibrium and equilibrium constant. Factors that affect the chemical equilibrium. Le-Chatelier's principle.
Electrochemistry. The standard reduction potentials. Standard hydrogen electrode. Nernst equation. Galvanic cells.
Acids and bases. Arrhenius, Bronsted-Lowry and Lewis 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) pH calculation of buffer solutions.
Chemical thermodynamics. Thermodynamic systems. State functions. Standard conditions. Heat and work. Enthalpy. Exothermic and endothermic reactions.
Factors affecting the reaction's spontaneity. Entropy. Free energy and standard molar free energy of formation. Calculation of ΔG in non-standard conditions. Relationship between ΔG° 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 TO BIOCHEMISTRY
Introduction to organic chemistry. Functional groups and classification of organic compounds. Ionic and radical reactions. 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.
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, tetra alkylammonium 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. Characteristics and functions of simple lipids (triglycerides) and complex lipids (sphingolipids and glyceropholipids). Carbohydrates. Characteristics and functions of monosaccharides, cyclic forms and polysaccharides (homo polysaccharides: starch, glycogen, cellulose, chitin and hetero polysaccharides: (peptidoglycans)
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. Nucleic Acid. Nucleosides and nucleotides. Structure, characteristics and functions of nucleic acids (DNA and RNA).
Prerequisites for admission
No particular preliminary knowledge are required
Teaching methods
The assessment method is a written test with a duration of 90 minutes and consists of 10 open-ended questions, five concerning general chemistry topics and five topics in organic chemistry and in propedeutic to biochemistry.
In the evaluation, to every single answer is given a score from 0 to 3 and the sum of the points assigned to the answers represents the vote expressed in thirtieths
In the evaluation, to every single answer is given a score from 0 to 3 and the sum of the points assigned to the answers represents the vote expressed in thirtieths
Teaching Resources
"Chimica medica e propedeutica biochimica", Bellini T., Zanichelli "Chimica e propedeutica biochimica", II ed., Bettelheim F.A. et al, EdiSES
Assessment methods and Criteria
The assessment method is a written test with a duration of 90 minutes and consists of 10 open-ended questions, five concerning general chemistry topics and five topics in organic chemistry and in propaedeutic to biochemistry.
In the evaluation, to every single answer is given a score from 0 to 3 and the sum of the points assigned to the answers represents the vote expressed in thirtieths
In the evaluation, to every single answer is given a score from 0 to 3 and the sum of the points assigned to the answers represents the vote expressed in thirtieths
Educational website(s)
Professor(s)
Reception:
To be defined via e-mail
c/o Osp. San Paolo, Via A. di Rudinì 8, Laboratorio di Biochimica, 9 piano, Blocco C,