Chemistry and introductory biochemistry
(objectives)
The main aim of this course is to allow the students to learn the major chemical and physical principles which govern organism life. The course will further cover the study of the composition of inorganic and organic compounds as well as the reactions they undergo. These aims will be pursued through interactive frontal lectures, exercise-sessions designed to optimize learning and to maximize the student skill in recognizing and solving a given medicinal chemistry task.
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Code
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90216 |
Language
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ENG |
Type of certificate
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Profit certificate
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Credits
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6
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Scientific Disciplinary Sector Code
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BIO/10
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Contact Hours
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60
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Type of Activity
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Basic compulsory activities
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Teacher
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Tavazzi Barbara
(syllabus)
General Chemistry
INTRODUCTION REMARKS. Periodic table of elements and inorganic nomenclature. Atom: atom models, atomic particles: proton, neutron, electron. Isotopes. Electrons and atom electronic configuration. The quantum-mechanical model of the atom. Quantum numbers and orbitals. Auf-bau. Chemical bonds.
MATTER STATES. Gas: ideal gas law. Absolute temperature and its relation with mean molecular speed. Mixture of gases; Dalton law.
LIQUIDS. Vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular and metallic solids.
THERMODYNAMICS. Thermodynamic potentials; enthalpy, entropy. Free energy: relationship with enthalpy and entropy.
SOLUTIONS. Concentrations of solutions: dilution and mixing of solutions. Vapor pressure of a solution (Raoult’s law). Solubility of gases in liquids: Henry law. CHEMICAL EQUILIBRIUM. Expression of equilibrium constant. Equilibrium influencing factors. Homogeneous and heterogeneous equilibrium.
SOLUTIONS OF ELECTROLYTES. Strong and weak electrolytes: dissociation grade. Colligative properties of electrolyte solutions. Van't Hoff binomial. Acids and bases following Arrhenius, Bronsted and Lowry, Lewis definitions. Strong and weak acid and bases. pH in strong and weak acid and base solutions. Buffers. HETEROGENEOUS SYSTEMS. Equilibria of slightly soluble ionic compounds. The solubility-product constant. The effect of a common ion.
KINETICS. Introduction to kinetics, activated complex theory, activation energy. Kinetic equations and reaction order. Relationship between kinetic constants and equilibrium constants.
ELECTROCHEMISTRY. Redox reactions. Oxidation number. Redox reactions and their balance. Redox standard potentials. Nerst equation. Electromotive force potential of a cell. Half-cells. Chemical and concentration cells.
Introductory Biochemistry
HYBRIDIZATION OF THE CARBON ATOM - sp3, sp2, sp hybridizations and their geometry.
HYDROCARBONS - Saturated hydrocarbons: alkanes and cycloalkanes. Nomenclature. Unsaturated hydrocarbons: alkenes and alkynes. Nomenclature. Conformational isomerism and geometric isomerism (cis-trans). AROMATIC COMPOUNDS - Structure of benzene: the resonance model. Nomenclature of aromatic compounds. Polycyclic aromatic hydrocarbons (outline).
ALCOHOLS, PHENOLS, THIOLS - Nomenclature. Acidity and basicity of alcohols and phenols. Thiols, analogues of alcohols and phenols.
ALDEHYDES AND KETONES - Nomenclature. Preparations of aldehydes and ketones. The carbonyl group. The nucleophilic addition to the carbonyl groups; formation of semiacetals and acetals. The aldol condensation (outline).
CARBOXYLIC ACIDS AND THEIR DERIVATIVES - Nomenclature of acids. Derivatives of carboxylic acids: esters, amides. Mechanism of esterification; triesters of glycerol.
AMINES AND OTHER NITROGEN COMPOUNDS - Classification of amines and nomenclature. Basicity of amines. Comparison between the basicity of amines and amides.
STEREOISOMERY - Chirality. Enantiomers. Polarized light; the polarimeter (hints). Diastereomers. CARBOHYDRATES - Definitions and classification. The monosaccharides. Chirality in monosaccharides; Fischer's projections. Cyclic structures of monosaccharides. Anomers. Phenomenon of mutarotation. Pyranosic and furanotic structures.
AMINO ACIDS, PROTEINS - Properties of amino acids. Peptide bond
LIPIDS: Structure, nomenclature, properties
NITROGEN BASES AND NUCLEOTIDES - Structure, nomenclature.
(reference books)
CHEMISTRY Hein M, Arena S, Foundations of College Chemistry, 14 Edition John Wiley and Sons Inc. or Peter Atkins , Loretta Jones, Leroy Laverman Chemical Principles: The Quest for Insight or Chemistry by M.S. Silderberg, McGraw-Hill International Edition
BIOCHEMISTRY Voet D, Voet JG, Pratt CW Principles of Biochemistry (international student version) IV edition – John Wiley and Sons Inc.
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Dates of beginning and end of teaching activities
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From to |
Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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Teacher
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Federici Luca
(syllabus)
General Chemistry
INTRODUCTION REMARKS. Periodic table of elements and inorganic nomenclature. Atom: atom models, atomic particles: proton, neutron, electron. Isotopes. Electrons and atom electronic configuration. The quantum-mechanical model of the atom. Quantum numbers and orbitals. Auf-bau. Chemical bonds.
MATTER STATES. Gas: ideal gas law. Absolute temperature and its relation with mean molecular speed. Mixture of gases; Dalton law.
LIQUIDS. Vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular and metallic solids.
THERMODYNAMICS. Thermodynamic potentials; enthalpy, entropy. Free energy: relationship with enthalpy and entropy.
SOLUTIONS. Concentrations of solutions: dilution and mixing of solutions. Vapor pressure of a solution (Raoult’s law). Solubility of gases in liquids: Henry law.
CHEMICAL EQUILIBRIUM. Expression of equilibrium constant. Equilibrium influencing factors. Homogeneous and heterogeneous equilibrium.
SOLUTIONS OF ELECTROLYTES. Strong and weak electrolytes: dissociation grade. Colligative properties of electrolyte solutions. Van't Hoff binomial. Acids and bases following Arrhenius, Bronsted and Lowry, Lewis definitions. Strong and weak acid and bases. pH in strong and weak acid and base solutions. Buffers.
HETEROGENEOUS SYSTEMS. Equilibria of slightly soluble ionic compounds. The solubility-product constant. The effect of a common ion.
KINETICS. Introduction to kinetics, activated complex theory, activation energy. Kinetic equations and reaction order. Relationship between kinetic constants and equilibrium constants.
ELECTROCHEMISTRY. Redox reactions. Oxidation number. Redox reactions and their balance. Redox standard potentials. Nerst equation. Electromotive force potential of a cell. Half-cells. Chemical and concentration cells.
Introductory Biochemistry
HYBRIDIZATION OF THE CARBON ATOM - sp3, sp2, sp hybridizations and their geometry.
HYDROCARBONS - Saturated hydrocarbons: alkanes and cycloalkanes. Nomenclature. Unsaturated hydrocarbons: alkenes and alkynes. Nomenclature. Conformational isomerism and geometric isomerism (cis-trans).
AROMATIC COMPOUNDS - Structure of benzene: the resonance model. Nomenclature of aromatic compounds. Polycyclic aromatic hydrocarbons (outline).
ALCOHOLS, PHENOLS, THIOLS - Nomenclature. Acidity and basicity of alcohols and phenols. Thiols, analogues of alcohols and phenols.
ALDEHYDES AND KETONES - Nomenclature. Preparations of aldehydes and ketones. The carbonyl group. The nucleophilic addition to the carbonyl groups; formation of semiacetals and acetals. The aldol condensation (outline).
CARBOXYLIC ACIDS AND THEIR DERIVATIVES - Nomenclature of acids. Derivatives of carboxylic acids: esters, amides. Mechanism of esterification; triesters of glycerol.
AMINES AND OTHER NITROGEN COMPOUNDS - Classification of amines and nomenclature. Basicity of amines. Comparison between the basicity of amines and amides.
STEREOISOMERY - Chirality. Enantiomers. Polarized light; the polarimeter (hints). Diastereomers. CARBOHYDRATES - Definitions and classification. The monosaccharides. Chirality in monosaccharides; Fischer's projections. Cyclic structures of monosaccharides. Anomers. Phenomenon of mutarotation. Pyranosic and furanotic structures.
AMINO ACIDS, PROTEINS - Properties of amino acids. Peptide bond
LIPIDS: Structure, nomenclature, properties
NITROGEN BASES AND NUCLEOTIDES - Structure, nomenclature.
(reference books)
CHEMISTRY Hein M, Arena S, Foundations of College Chemistry, 14 Edition John Wiley and Sons Inc. or Peter Atkins , Loretta Jones, Leroy Laverman Chemical Principles: The Quest for Insight or Chemistry by M.S. Silderberg, McGraw-Hill International Edition
BIOCHEMISTRY Voet D, Voet JG, Pratt CW Principles of Biochemistry (international student version) IV edition – John Wiley and Sons Inc.
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Dates of beginning and end of teaching activities
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From to |
Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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