Alfonso GRASSI | INORGANIC CHEMISTRY

cod. 0512800025

INORGANIC CHEMISTRY

	0512800025
	DEPARTMENT OF CHEMISTRY AND BIOLOGY "ADOLFO ZAMBELLI"
	EQF6
	BIOLOGICAL SCIENCES
	2016/2017

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
	MARINA LAMBERTI Curriculum

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

	Prerequisites
	NO CONNECTIONS

	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. EMISSION AND ADSORPTION SPECTRA OF THE ATOMS. BOHR’S 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: IONIZATION ENERGY, ELECTRON AFFINITY, ATOMIC AND IONIC RADII. STOICHIOMETRY. MOLE. CONCENTRATION UNITS: MOLE FRACTION, WEIGHT FRACTION, VOLUME FRACTION. EVALUATION OF THE EMPIRICAL FORMULA FROM PERCENT COMPOSITION BY MASS OF A COMPOUND. CHEMICAL REACTIONS. BALANCING OF THE ACID-BASE REACTIONS. THE LIMITING REAGENT. THE OXIDATION NUMBERS. BALANCING OF THE REDOX REACTIONS WITH THE HALF REACTIONS AND OXIDATION NUMBER 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. METALLIC BONDING. WEAK CHEMICAL BONDS. SOLID STATE OF MATTER. AMORPHOUS AND CRYSTALLINE SOLIDS. IONIC, COVALENT AND MOLECULAR SOLIDS. ALLOTROPY AND POLYMORPHISM. METALS. GAS STATE OF MATTER. BOYLE’S LAW; CHARLES’ LAW; GAY-LUSSAC’S LAW. IDEAL GAS LAW. KINETIC THEORY OF GASES. BOLTZMAN EQUATION. DIFFUSION OF GASES. REAL GASES. VAN DER WAALS’ EQUATION. LIQUID STATE OF MATTER. LIQUIDS. VAPOUR PRESSURE OF NEAT LIQUIDS. SOLUTIONS. CONCENTRATION UNITS: MOLARITY, MOLALITY, NORMALITY. HENRY’S LAW. RAOULT’S LAW. COLLIGATIVE PROPERTIES OF SOLUTIONS: EBULLIOSCOPY, CRIOSCOPY AND OSMOTIC PRESSURE. VAPOUR LIQUID EQUILIBRIA AND DISTILLATION. PHASE DIAGRAMS. SOLUBILITY. FREE ENERGY OF SOLUTION. STRONG AND WEAK ELECTROLITES. DEGREE OF DISSOCIATION AND VAN'T HOFF FACTOR. SOLUBILITY OF WEAK ELECTROLITES. 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. EMISSION AND ADSORPTION SPECTRA OF THE ATOMS. BOHR’S 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: IONIZATION ENERGY, ELECTRON AFFINITY, ATOMIC AND IONIC RADII.
STOICHIOMETRY. MOLE. CONCENTRATION UNITS: MOLE FRACTION, WEIGHT FRACTION, VOLUME FRACTION. EVALUATION OF THE EMPIRICAL FORMULA FROM PERCENT COMPOSITION BY MASS OF A COMPOUND. CHEMICAL REACTIONS. BALANCING OF THE ACID-BASE REACTIONS. THE LIMITING REAGENT. THE OXIDATION NUMBERS. BALANCING OF THE REDOX REACTIONS WITH THE HALF REACTIONS AND OXIDATION NUMBER 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. METALLIC BONDING. WEAK CHEMICAL BONDS.
SOLID STATE OF MATTER. AMORPHOUS AND CRYSTALLINE SOLIDS. IONIC, COVALENT AND MOLECULAR SOLIDS. ALLOTROPY AND POLYMORPHISM. METALS.
GAS STATE OF MATTER. BOYLE’S LAW; CHARLES’ LAW; GAY-LUSSAC’S LAW. IDEAL GAS LAW. KINETIC THEORY OF GASES. BOLTZMAN EQUATION. DIFFUSION OF GASES. REAL GASES. VAN DER WAALS’ EQUATION.
LIQUID STATE OF MATTER. LIQUIDS. VAPOUR PRESSURE OF NEAT LIQUIDS. SOLUTIONS. CONCENTRATION UNITS: MOLARITY, MOLALITY, NORMALITY. HENRY’S LAW. RAOULT’S LAW. COLLIGATIVE PROPERTIES OF SOLUTIONS: EBULLIOSCOPY, CRIOSCOPY AND OSMOTIC PRESSURE. VAPOUR LIQUID EQUILIBRIA AND DISTILLATION. PHASE DIAGRAMS.
SOLUBILITY. FREE ENERGY OF SOLUTION. STRONG AND WEAK ELECTROLITES. DEGREE OF DISSOCIATION AND VAN'T HOFF FACTOR. SOLUBILITY OF WEAK ELECTROLITES. 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). EXERCISES (1CFU). LAB PRACTICE (1CFU).

	Verification of learning
	THE ASSESSMENT INCLUDES A WRITTEN TEST AND ORAL EXAM WHERE THE POSITIVE EVALUATION OF THE FORMER IS MANDATORY TO ENDS OF THE ADMISSION TO THE ORAL EXAM. THE WRITTEN TEST CONSISTS IN SOLVING NUMERICAL PROBLEMS DEALING WITH THE SUBJECT PRESENTED IN THE LESSONS (SEE THE PROGRAM ATTACHED); TYPICALLY THE TEST IS EVALUATED POSITIVELY IF AT LEAST THREE OVER SIX PROBLEMS HAVE BEEN SOLVED CORRECTLY. THE ORAL EXAM CONSISTS OF A DISCUSSION ON THE MAIN SUBJECTS OF THE PROGRAM AND AIMS TO ASSESS THE DEGREE OF KNOWLEDGE OF THE STUDENT 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

Verification of learning

THE ASSESSMENT INCLUDES A WRITTEN TEST AND ORAL EXAM WHERE THE POSITIVE EVALUATION OF THE FORMER IS MANDATORY TO ENDS OF THE ADMISSION TO THE ORAL EXAM. THE WRITTEN TEST CONSISTS IN SOLVING NUMERICAL PROBLEMS DEALING WITH THE SUBJECT PRESENTED IN THE LESSONS (SEE THE PROGRAM ATTACHED); TYPICALLY THE TEST IS EVALUATED POSITIVELY IF AT LEAST THREE OVER SIX PROBLEMS HAVE BEEN SOLVED CORRECTLY. THE ORAL EXAM CONSISTS OF A DISCUSSION ON THE MAIN SUBJECTS OF THE PROGRAM AND AIMS TO ASSESS THE DEGREE OF KNOWLEDGE OF THE STUDENT 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

	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

	More Information
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Alfonso GRASSI | INORGANIC CHEMISTRY