Stefano MILIONE | INORGANIC CHEMISTRY

cod. 0512800025

INORGANIC CHEMISTRY

	0512800025
	DEPARTMENT OF CHEMISTRY AND BIOLOGY "ADOLFO ZAMBELLI"
	EQF6
	BIOLOGICAL SCIENCES
	2019/2020

PERCORSO COMUNE

	OBBLIGATORIO
	YEAR OF COURSE 1
	YEAR OF DIDACTIC SYSTEM 2016
	PRIMO SEMESTRE

TEACHING UNITS

SSD	CFU	HOURS	ACTIVITY	TYPE OF ACTIVITY
CHIM/03	8	64	LESSONS	BASIC COMPULSORY SUBJECTS
CHIM/03	1	12	EXERCISES	BASIC COMPULSORY SUBJECTS
CHIM/03	1	12	LAB	BASIC COMPULSORY SUBJECTS

PROFESSORS

	ALFONSO GRASSI T Curriculum
	STEFANO MILIONE Curriculum

	Objectives
	THE COURSE PROVIDES THE BASIC ELEMENTS OF KNOWLEDGE ON THE STRUCTURE OF MATTER, FROM ATOMS TO MOLECULES, AND THE THERMODYNAMIC AND KINETIC PRINCIPLES WHICH GOVERN THE CHEMICAL TRANSFORMATIONS.

	Prerequisites
	KNOWLEDGE OF BASIC MATHS AND PHYSICS AS PROVIDED IN A REGULAR COURSE OF HIGH SCHOOL

	Contents
	A BRIEF HISTORY OF CHEMISTRY. THE GALILEO’S SCIENTIFIC METHOD. TYPES OF MATTER: HOMOGENOUS AND HETEROGENEOUS SYSTEMS AND METHODS TO SEPARATE MIXTURE. LAVOISIER’S LAW. DALTON’S AND PROUST’S LAW. ATOMIC WEIGHTS AND MOLECULAR WEIGHTS. GAY-LUSSAC’S LAW. THE AVOGADRO’S HYPOTHESIS. THE ATOMIC THEORY OF MATTER AND THE PERIODIC TABLE OF THE ELEMENTS. THOMSON’S, MILLIKAN’S AND RUTHERFORD’S EXPERIMENTS. INTERACTION BETWEEN MATTER AND ELECTROMAGNETIC RADIATION. BOHR’S ATOMIC MODEL. HYDROGENOID WAVE FUNCTIONS: THE ATOMIC ORBITALS. PAULI’S AND HUND’S PRINCIPLES. AUFBAU (ELECTRONIC CONFIGURATION OF ELEMENTS). THE PERIODIC TABLE OF THE ELEMENTS. PERIODIC PROPERTIES. STOICHIOMETRY. MOLE. CONCENTRATION UNITS. EVALUATION OF THE EMPIRICAL FORMULA FROM MASS PERCENT COMPOSITION OF A COMPOUND. CHEMICAL REACTIONS. ACID-BASE REACTION BALANCING. THE LIMITING REAGENT. OXIDATION NUMBERS. REDOX REACTIONS AND THE HALF REACTIONS AND OXIDATION NUMBER BALANCING METHODS. CHEMICAL BOND. IONIC BOND. COVALENT BOND. VALENCE BOND THEORY. MOLECULAR GEOMETRY AND VESPR RULES. IBRIDIZATION. RESONANCE. MOLECULAR ORBITAL THEORY. ELECTRONEGATIVITY AND IONICITY OF THE CHEMICAL BOND. WEAK CHEMICAL BONDS. SOLID STATE OF MATTER. AMORPHOUS AND CRYSTALLINE SOLIDS. IONIC, COVALENT AND MOLECULAR SOLIDS. ALLOTROPY AND POLYMORPHISM. METALS. GAS. BOYLE’S, CHARLES’ AND GAY-LUSSAC’S LAWS. IDEAL GAS. KINETIC THEORY OF GASES. BOLTZMANN EQUATION. DIFFUSION OF GASES. REAL GAS AND THE VAN DER WAALS’ EQUATION. LIQUIDS. VAPOUR PRESSURE OF NEAT LIQUIDS. SOLUTIONS. CONCENTRATION UNITS: MOLARITY, MOLALITY, NORMALITY. HENRY’S LAW. RAOULT’S LAW. COLLIGATIVE PROPERTIES OF SOLUTIONS: EBULLIOSCOPY, CRYOSCOPY AND OSMOTIC PRESSURE. VAPOUR-LIQUID EQUILIBRIA AND DISTILLATION. PHASE DIAGRAMS. SOLUBILITY. FREE ENERGY OF SOLUTION. STRONG AND WEAK ELECTROLYTES. DEGREE OF DISSOCIATION AND VAN'T HOFF FACTOR. SOLUBILITY OF WEAK ELECTROLYTES. COMMON ION EFFECT. ACIDS AND BASES. ARRHENIUS’ THEORY. LOWRY-BRONSTED THEORY. LEWIS THEORY. OXOACIDS. PH. WEAK ACIDS AND BASES; CALCULATING PH AND POH. BUFFER SOLUTION. HYDROLYSIS. AMINOACIDS: ISOELECTRIC PH AND IONIC MIGRATION. TITRATION AND INDICATORS. POLYPROTIC ACIDS. THERMODYNAMICS. SYSTEMS, STATES AND STATE FUNCTIONS. HEAT AND WORK. FIRST PRINCIPLE OF THERMODYNAMICS. THERMOCHEMISTRY. ENTROPY AND THE SECOND AND THIRD PRINCIPLES OF THERMODYNAMICS. FREE ENERGY AND CHEMICAL TRANSFORMATIONS. THE EQUILIBRIUM CONSTANT AND ITS DEPENDENCE FROM TEMPERATURE. KINETICS. THE REACTION RATE. FIRST ORDER KINETICS AND EXAMPLES OF SECOND ORDER KINETICS. SPECIFIC RATE CONSTANT. THE HALF LIFE RATE. REACTION MECHANISM. COLLISION THEORY. ARRHENIUS’ EQUATION. ACTIVATION ENERGY. TRANSITION STATE THEORY. HOMOGENEOUS AND HETEROGENEOUS CATALYSTS. ENZYMES. ELECTROCHEMISTRY. REDOX POTENTIALS. GALVANIC CELLS. NERST’S EQUATION. ELECTROLYSIS.

A BRIEF HISTORY OF CHEMISTRY. THE GALILEO’S SCIENTIFIC METHOD. TYPES OF MATTER: HOMOGENOUS AND HETEROGENEOUS SYSTEMS AND METHODS TO SEPARATE MIXTURE. LAVOISIER’S LAW. DALTON’S AND PROUST’S LAW. ATOMIC WEIGHTS AND MOLECULAR WEIGHTS. GAY-LUSSAC’S LAW. THE AVOGADRO’S HYPOTHESIS.

THE ATOMIC THEORY OF MATTER AND THE PERIODIC TABLE OF THE ELEMENTS. THOMSON’S, MILLIKAN’S AND RUTHERFORD’S EXPERIMENTS. INTERACTION BETWEEN MATTER AND ELECTROMAGNETIC RADIATION. BOHR’S ATOMIC MODEL. HYDROGENOID WAVE FUNCTIONS: THE ATOMIC ORBITALS. PAULI’S AND HUND’S PRINCIPLES. AUFBAU (ELECTRONIC CONFIGURATION OF ELEMENTS). THE PERIODIC TABLE OF THE ELEMENTS. PERIODIC PROPERTIES.

STOICHIOMETRY. MOLE. CONCENTRATION UNITS. EVALUATION OF THE EMPIRICAL FORMULA FROM MASS PERCENT COMPOSITION OF A COMPOUND. CHEMICAL REACTIONS. ACID-BASE REACTION BALANCING. THE LIMITING REAGENT. OXIDATION NUMBERS. REDOX REACTIONS AND THE HALF REACTIONS AND OXIDATION NUMBER BALANCING METHODS.

CHEMICAL BOND. IONIC BOND. COVALENT BOND. VALENCE BOND THEORY. MOLECULAR GEOMETRY AND VESPR RULES. IBRIDIZATION. RESONANCE. MOLECULAR ORBITAL THEORY. ELECTRONEGATIVITY AND IONICITY OF THE CHEMICAL BOND. WEAK CHEMICAL BONDS.

SOLID STATE OF MATTER. AMORPHOUS AND CRYSTALLINE SOLIDS. IONIC, COVALENT AND MOLECULAR SOLIDS. ALLOTROPY AND POLYMORPHISM. METALS.

GAS. BOYLE’S, CHARLES’ AND GAY-LUSSAC’S LAWS. IDEAL GAS. KINETIC THEORY OF GASES. BOLTZMANN EQUATION. DIFFUSION OF GASES. REAL GAS AND THE VAN DER WAALS’ EQUATION.

LIQUIDS. VAPOUR PRESSURE OF NEAT LIQUIDS. SOLUTIONS. CONCENTRATION UNITS: MOLARITY, MOLALITY, NORMALITY. HENRY’S LAW. RAOULT’S LAW. COLLIGATIVE PROPERTIES OF SOLUTIONS: EBULLIOSCOPY, CRYOSCOPY AND OSMOTIC PRESSURE. VAPOUR-LIQUID EQUILIBRIA AND DISTILLATION. PHASE DIAGRAMS.

SOLUBILITY. FREE ENERGY OF SOLUTION. STRONG AND WEAK ELECTROLYTES. DEGREE OF DISSOCIATION AND VAN'T HOFF FACTOR. SOLUBILITY OF WEAK ELECTROLYTES. COMMON ION EFFECT.

ACIDS AND BASES. ARRHENIUS’ THEORY. LOWRY-BRONSTED THEORY. LEWIS THEORY. OXOACIDS. PH. WEAK ACIDS AND BASES; CALCULATING PH AND POH. BUFFER SOLUTION. HYDROLYSIS. AMINOACIDS: ISOELECTRIC PH AND IONIC MIGRATION. TITRATION AND INDICATORS. POLYPROTIC ACIDS.

THERMODYNAMICS. SYSTEMS, STATES AND STATE FUNCTIONS. HEAT AND WORK. FIRST PRINCIPLE OF THERMODYNAMICS. THERMOCHEMISTRY. ENTROPY AND THE SECOND AND THIRD PRINCIPLES OF THERMODYNAMICS. FREE ENERGY AND CHEMICAL TRANSFORMATIONS. THE EQUILIBRIUM CONSTANT AND ITS DEPENDENCE FROM TEMPERATURE.

KINETICS. THE REACTION RATE. FIRST ORDER KINETICS AND EXAMPLES OF SECOND ORDER KINETICS. SPECIFIC RATE CONSTANT. THE HALF LIFE RATE. REACTION MECHANISM. COLLISION THEORY. ARRHENIUS’ EQUATION. ACTIVATION ENERGY. TRANSITION STATE THEORY. HOMOGENEOUS AND HETEROGENEOUS CATALYSTS. ENZYMES.

ELECTROCHEMISTRY. REDOX POTENTIALS. GALVANIC CELLS. NERST’S EQUATION. ELECTROLYSIS.

	Teaching Methods
	LESSONS (8CFU; 64H) SUPPORTED BY SLIDE SHOW; PROBLEM SOLVING (1CFU; 12H); LAB PRACTICE (1CFU; 12H) CONSISTING OF THREE EXPERIMENTS (4H/EACH). THE CLASS FOR THE LAB PRACTICE CONSISTS OF 18 TEAMS, EACH ONE COMPOSED BY TWO STUDENTS. ELABORATION OF AN INDIVIDUAL SCIENTIFIC REPORT FOR EACH EXPERIMENT. THE ATTENDANCE TO THE LAB PRACTICE IS MANDATORY.

	Verification of learning
	THE ASSESSMENT INCLUDES A WRITTEN TEST AND ORAL EXAM WHERE THE POSITIVE EVALUATION OF THE TEST IS MANDATORY FOR THE ADMISSION TO THE ORAL EXAM. THE WRITTEN TEST CONSISTS IN NUMERICAL PROBLEM SOLVING RELATED TO THE SUBJECTS DISCUSSED IN THE LESSONS (SEE THE PROGRAM); TYPICALLY THE TEST IS EVALUATED POSITIVELY IF AT LEAST THREE OVER SIX PROBLEMS HAVE BEEN SOLVED CORRECTLY IN 3H. THE ORAL EXAM CONSISTS OF A DISCUSSION (20 MIN) ON THE MAIN SUBJECTS OF THE PROGRAM AND AIMS TO ASSESS THE KNOWLEDGE ABOUT THE PROPERTIES OF MATTER AND THE LAWS GOVERNING THE CHEMICAL TRANSFORMATIONS. THE ORAL EXAM ALSO INCLUDES A DISCUSSION ON THE SCIENTIFIC REPORTS ELABORATED BY THE STUDENT AT THE END OF THE LAB PRACTICE. THE FINAL EVALUATION IS EXPRESSED WITH MARKS (18- 30 PTS) AND TAKES INTO ACCOUNT OF THE WRITTEN TEST, ORAL EXAM AND LAB PRACTICE.

Verification of learning

THE ASSESSMENT INCLUDES A WRITTEN TEST AND ORAL EXAM WHERE THE POSITIVE EVALUATION OF THE TEST IS MANDATORY FOR THE ADMISSION TO THE ORAL EXAM. THE WRITTEN TEST CONSISTS IN NUMERICAL PROBLEM SOLVING RELATED TO THE SUBJECTS DISCUSSED IN THE LESSONS (SEE THE PROGRAM); TYPICALLY THE TEST IS EVALUATED POSITIVELY IF AT LEAST THREE OVER SIX PROBLEMS HAVE BEEN SOLVED CORRECTLY IN 3H. THE ORAL EXAM CONSISTS OF A DISCUSSION (20 MIN) ON THE MAIN SUBJECTS OF THE PROGRAM AND AIMS TO ASSESS THE KNOWLEDGE ABOUT THE PROPERTIES OF MATTER AND THE LAWS GOVERNING THE CHEMICAL TRANSFORMATIONS. THE ORAL EXAM ALSO INCLUDES A DISCUSSION ON THE SCIENTIFIC REPORTS ELABORATED BY THE STUDENT AT THE END OF THE LAB PRACTICE. THE FINAL EVALUATION IS EXPRESSED WITH MARKS (18- 30 PTS) AND TAKES INTO ACCOUNT OF THE WRITTEN TEST, ORAL EXAM AND LAB PRACTICE.

	Texts
	A TEXTBOOK OF GENERAL CHEMISTRY FOR BACHELOR DEGREE. EXAMPLES: 1) KELTER, MOSHER, SCOTT “CHIMICA: LA SCIENZA DELLA VITA” - EDISES 2) BROWN, LEMAY, BURSTEN, MURPHY, WOODWARD “FONDAMENTI DI CHIMICA” – EDISES. FOR SOLVING NUMERICAL PROBLEMS: BERTINI, LUCHINAT, MANI “STECHIOMETRIA”- CASA EDITRICE AMBROSIANA

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Stefano MILIONE | INORGANIC CHEMISTRY