Menù principale
B025339 - Biochemistry
Main information
Teaching Language
Course Content
Suggested readings
Learning Objectives
Prerequisites
Teaching Methods
Type of Assessment
Course program
Academic Year 2018-19
Coorte 2018 - 3-years First Cycle Degree (DM 270/04) in ENVIRONMENT AND WORKPLACE PREVENTION TECHNIQUES
Course year
First year - First Semester
Belonging Department
Experimantal and Clinical Medicine
Modulo di sola Frequenza of
Scientific Area
BIO/10 - BIOCHEMISTRY
Credits
5
Teaching Hours
60
Teaching Term
01/10/2018 ⇒ 30/04/2020
Attendance required
No
Type of Evaluation
Giudizio Finale
Course Content
show
Course program
show
Lectureship
Teaching Language
italian
Course Content
general chemistry, organic chemistry and biochemistry
Suggested readings (Search our library's catalogue)
For general and organic chemistry:
M. Stefani & N. Taddei, "Chimica, Biochimica e biologia applicata", Ed. Zanichelli, third edition
For Biochemistry:
Lehninger - PRINCIPLES OF BIOCHEMISTRY
Fourth Edition
David L. Nelson (University of Wisconsin–Madison)
Michael M. Cox (University of Wisconsin–Madison)
M. Stefani & N. Taddei, "Chimica, Biochimica e biologia applicata", Ed. Zanichelli, third edition
For Biochemistry:
Lehninger - PRINCIPLES OF BIOCHEMISTRY
Fourth Edition
David L. Nelson (University of Wisconsin–Madison)
Michael M. Cox (University of Wisconsin–Madison)
Learning Objectives
At the end of the lessons, the student must possess the knowledge necessary to manage the chemical and biological risks in the professional activity, in production processes, in the environment and in the workplace.
Prerequisites
none
Teaching Methods
frontal lessons
Type of Assessment
Final written tests, one for chemistry and one for biochemistry
Course program
Program of general chemistry:
ATOMS, ORBITALS, PERIODIC SYSTEM OF ELEMENTS: Structure of the atom, neutrons, protons and electrons - Atomic -number and mass number - Isotopes - Atomic weight - Orbitals: name, shape and energy - Aufbau principle for electron configuration of the orbitals – Examples of electron configuration for some atoms - Periodic system of elements - Mole
ELECTRONEGATIVITY, IONIC BOND, COVALENT BOND: Ionization energy and electron affinity – Electronegativity -Ionic bond - Covalent bond as overlap of atomic orbitals - Covalent bonds and Examples of diatomic and polyatomic molecules.
HYBRIDIZATION OF ORBITALS, STRUCTURAL FORMULAS: Geometry of molecules. Principle of repulsion of electronic pairs - Molecular formulas and structural formulas - Rules for writing structural formulas - Examples of structural formulas.
WEAK BONDS, STATE OF MATTER AGGREGATION: Molecular weight and formula weight - Van der Waals forces - Hydrogen bond - The three states of matter aggregation: solid, liquid and gaseous.
SOLUTIONS, CHEMICAL EQUATION, THERMODYNAMICS Definition of solution, solvent and solute - Examples of solutions - Solubility, solvation, saturated and unsaturated solutions - Concentrations of solutions. Molarity, molality, mole fraction and percentage - Osmotic pressure of a solution - Chemical equation. Reactants, products and stoichiometric coefficients – Open, closed and isolated systems. - First law of thermodynamics. Internal energy, heat and work - Definition and meaning of enthalpy - Exothermic and endothermic reactions - Second law of thermodynamics. Entropy and disorder - Gibbs free energy and spontaneity of a reaction – Changes of enthalpy, entropy and free energy in standard conditions.
KINETIC, CHEMICAL EQUILIBRIUM, LAW OF MASS ACTION: Chemical kinetic. Reversible and irreversible reactions – Kinetic law and rate constant. Arrhenius equation - Factors influencing the rate of a reaction: kinetic energy and orientation of molecules - Activation energy and activated complex. Reaction diagram - Kinetic and thermodynamic criteria for determining if a reaction can occur - Effects of temperature and catalysts in increasing the rate of a reaction - Chemical equilibrium. Speed of direct and reverse reaction - Law of mass action. Equilibrium constant - Equilibrium constant in a heterogeneous system - Reversible and irreversible reactions - Relation between equilibrium constant and ΔG°.
OXIDATION AND REDUCTION REACTIONS , BALANCING: Definition of oxidation number - Reactions of oxidation-reduction (redox). Oxidizing and reducing agents - Balancing of non-redox reactions - Balancing of redox reactions - Standard electrode potential.
ACIDS AND BASES, PH, BUFFER SOLUTIONS: Definition of acid and base - Reactions acid-water and base-water - Polyprotic acids and polyacid bases. Amphoteric substances. Salts - Ionic water product. Concentration of hydrogen and hydroxide ions - pH and pOH. Neutral, acid and basic solutions. - Acid and base dissociation constants - Weak and strong acids and bases - Buffer solutions: composition and use.
Program of organic chemistry
ORGANIC COMPOUNDS: Functional groups, nomenclature, properties and main reactions - Saturated and unsaturated, aliphatic and aromatic hydrocarbons - Alicyclic compounds - Structural isomers - Stereoisomers - Alcohols - Phenols - Aldehydes and Ketones - Amines - Carboxylic acids and their derivatives
Program of biochemistry
Structure and function of biomolecules:
Monosaccharides, disaccharides and polysaccharides.
- Sucrose, lactose, maltose, starch, glycogen and cellulose
- Lipids. Fatty acids, triacylglycerides, phosphoglycerides. Cholesterol and its derivatives
- Amino acids of proteins, classification of 20 amino acids of the protein.
peptide bond. Proteins, biological importance.
- Structure of proteins, conjugated proteins, lipoproteins, glycoproteins and glycosaminoglycans.
- Hemoglobin and Myoglobin: structure and function, regulation by external factors: pH, 2.3 phosphoglycerate, saturation curves
Fundamentals of enzymology:
- Enzymes: biological importance factors affecting the activity (pH, temperature, substrate concentration, and Menten equation Mechaelis. Enzyme catalysis.
- Coenzymes. water-soluble and fat-soluble vitamins.
- Allosterismo: Adjusting enzyme activity.
- Inhibition of the enzymes. Overview of medical and pharmacological importance of enzymes
Metabolism:
- Forms of energy used by living things
- General principles of metabolism
- Sugar metabolism: glycolysis and fermentation. Via the pentose-phosphate. Gluconeogensi. Glycogen metabolism.
- Lipid metabolism: transport in the mitochondria synthesis and degradation fatty acids (beta oxidation, ACP). Synthesis and utilization of ketone bodies. I note on the biosynthesis of cholesterol.
- Metabolism of amino acids. Deamininazioni and transaminazioni. Carbamoyl phosphate, Ureogenesi (urea cycle). Notes on metabolism nitrogen bases (uric acid production).
- Terminal Metabolism: citric acid cycle, respiratory chain and oxidative phosphorylation.
Hormones and metabolic control:
- - Control of metabolism. Fundamentals of signal transduction: cell signaling pathways: hormones and growth factors, classification of hormones.
ATOMS, ORBITALS, PERIODIC SYSTEM OF ELEMENTS: Structure of the atom, neutrons, protons and electrons - Atomic -number and mass number - Isotopes - Atomic weight - Orbitals: name, shape and energy - Aufbau principle for electron configuration of the orbitals – Examples of electron configuration for some atoms - Periodic system of elements - Mole
ELECTRONEGATIVITY, IONIC BOND, COVALENT BOND: Ionization energy and electron affinity – Electronegativity -Ionic bond - Covalent bond as overlap of atomic orbitals - Covalent bonds and Examples of diatomic and polyatomic molecules.
HYBRIDIZATION OF ORBITALS, STRUCTURAL FORMULAS: Geometry of molecules. Principle of repulsion of electronic pairs - Molecular formulas and structural formulas - Rules for writing structural formulas - Examples of structural formulas.
WEAK BONDS, STATE OF MATTER AGGREGATION: Molecular weight and formula weight - Van der Waals forces - Hydrogen bond - The three states of matter aggregation: solid, liquid and gaseous.
SOLUTIONS, CHEMICAL EQUATION, THERMODYNAMICS Definition of solution, solvent and solute - Examples of solutions - Solubility, solvation, saturated and unsaturated solutions - Concentrations of solutions. Molarity, molality, mole fraction and percentage - Osmotic pressure of a solution - Chemical equation. Reactants, products and stoichiometric coefficients – Open, closed and isolated systems. - First law of thermodynamics. Internal energy, heat and work - Definition and meaning of enthalpy - Exothermic and endothermic reactions - Second law of thermodynamics. Entropy and disorder - Gibbs free energy and spontaneity of a reaction – Changes of enthalpy, entropy and free energy in standard conditions.
KINETIC, CHEMICAL EQUILIBRIUM, LAW OF MASS ACTION: Chemical kinetic. Reversible and irreversible reactions – Kinetic law and rate constant. Arrhenius equation - Factors influencing the rate of a reaction: kinetic energy and orientation of molecules - Activation energy and activated complex. Reaction diagram - Kinetic and thermodynamic criteria for determining if a reaction can occur - Effects of temperature and catalysts in increasing the rate of a reaction - Chemical equilibrium. Speed of direct and reverse reaction - Law of mass action. Equilibrium constant - Equilibrium constant in a heterogeneous system - Reversible and irreversible reactions - Relation between equilibrium constant and ΔG°.
OXIDATION AND REDUCTION REACTIONS , BALANCING: Definition of oxidation number - Reactions of oxidation-reduction (redox). Oxidizing and reducing agents - Balancing of non-redox reactions - Balancing of redox reactions - Standard electrode potential.
ACIDS AND BASES, PH, BUFFER SOLUTIONS: Definition of acid and base - Reactions acid-water and base-water - Polyprotic acids and polyacid bases. Amphoteric substances. Salts - Ionic water product. Concentration of hydrogen and hydroxide ions - pH and pOH. Neutral, acid and basic solutions. - Acid and base dissociation constants - Weak and strong acids and bases - Buffer solutions: composition and use.
Program of organic chemistry
ORGANIC COMPOUNDS: Functional groups, nomenclature, properties and main reactions - Saturated and unsaturated, aliphatic and aromatic hydrocarbons - Alicyclic compounds - Structural isomers - Stereoisomers - Alcohols - Phenols - Aldehydes and Ketones - Amines - Carboxylic acids and their derivatives
Program of biochemistry
Structure and function of biomolecules:
Monosaccharides, disaccharides and polysaccharides.
- Sucrose, lactose, maltose, starch, glycogen and cellulose
- Lipids. Fatty acids, triacylglycerides, phosphoglycerides. Cholesterol and its derivatives
- Amino acids of proteins, classification of 20 amino acids of the protein.
peptide bond. Proteins, biological importance.
- Structure of proteins, conjugated proteins, lipoproteins, glycoproteins and glycosaminoglycans.
- Hemoglobin and Myoglobin: structure and function, regulation by external factors: pH, 2.3 phosphoglycerate, saturation curves
Fundamentals of enzymology:
- Enzymes: biological importance factors affecting the activity (pH, temperature, substrate concentration, and Menten equation Mechaelis. Enzyme catalysis.
- Coenzymes. water-soluble and fat-soluble vitamins.
- Allosterismo: Adjusting enzyme activity.
- Inhibition of the enzymes. Overview of medical and pharmacological importance of enzymes
Metabolism:
- Forms of energy used by living things
- General principles of metabolism
- Sugar metabolism: glycolysis and fermentation. Via the pentose-phosphate. Gluconeogensi. Glycogen metabolism.
- Lipid metabolism: transport in the mitochondria synthesis and degradation fatty acids (beta oxidation, ACP). Synthesis and utilization of ketone bodies. I note on the biosynthesis of cholesterol.
- Metabolism of amino acids. Deamininazioni and transaminazioni. Carbamoyl phosphate, Ureogenesi (urea cycle). Notes on metabolism nitrogen bases (uric acid production).
- Terminal Metabolism: citric acid cycle, respiratory chain and oxidative phosphorylation.
Hormones and metabolic control:
- - Control of metabolism. Fundamentals of signal transduction: cell signaling pathways: hormones and growth factors, classification of hormones.