Giuliana GORRASI | CHIMICA
Giuliana GORRASI CHIMICA
cod. 0612300003
CHIMICA
| 0612300003 | |
| DIPARTIMENTO DI INGEGNERIA INDUSTRIALE | |
| EQF6 | |
| MECHANICAL ENGINEERING | |
| 2016/2017 |
| OBBLIGATORIO | |
| YEAR OF COURSE 1 | |
| YEAR OF DIDACTIC SYSTEM 2016 | |
| PRIMO SEMESTRE |
| SSD | CFU | HOURS | ACTIVITY | |
|---|---|---|---|---|
| CHIM/07 | 6 | 60 | LESSONS |
| Objectives | |
|---|---|
| CRITICAL KNOWLEDGE OF CHEMICALS AND CHEMICAL FUNDAMENTALS - PHYSICAL NEEDED TO INTERPRET THE BEHAVIOR AND TRANSFORMATIONS OF MATTER IN RELATION TO KEY TECHNOLOGIES AND TO ENGINEERING PROBLEMS. INTERPRETATION OF MATTER TRANSFORMATIONS BY PROVIDING A SUMMARY OF THE PRINCIPLES COMMON TO THE VARIOUS PHENOMENA AND TO THE DIFFERENT CATEGORIES OF SUBSTANCES. IT WILL BE ACQUIRED THE ABILITY TO RELATE THE MACROSCOPIC PROPERTIES OF A COMPOUND WITH ITS MICROSTRUCTURE TO INCLUDE THE CRITERIA THAT GOVERN THE DESIGN AND SYNTHESIS OF SUBSTANCES AND MATERIALS IN RELATION TO POSSIBLE APPLICATIONS. |
| Prerequisites | |
|---|---|
| FUNDAMENTALS OF MATHEMATICS AND PHYSICS WHICH MAY BE ACQUIRED LEVEL OF SECONDARY SCHOOL |
| Contents | |
|---|---|
| MATTER AND ENERGY. NATURE OF MATTER. PHYSICAL AND CHEMICAL. LAW OF DEFINITE PROPORTIONS. LAW OF MULTIPLE PROPORTIONS. THEORY OF ATOMIC DALTON. LAW OF CONSERVATION OF MASS. ATOMS AND MOLECULES. RELATIVE ATOMIC MASS. CONCEPT OF MOLE. AVOGADRO NUMBER. MOLECULAR MASS. FORMULA MINIMUM AND MOLECULAR. PERCENTAGE COMPOSITION OF ELEMENTS IN THE FORMULA. ATOM: ATOMIC NUMBER AND MASS NUMBER. ISOTOPES. THOMSON MODEL. MODEL OF RUTHERFORD. BOHR MODEL. THE PHOTOELECTRIC EFFECT. PLANCK THEORY. NATURE WAVE ELECTRON. THE PRINCIPLE HEISENBERG UNCERTAINTY. QUANTUM VISION ATOM. MODEL AND FUNCTIONS OF SCHRODINGER WAVE. QUANTUM NUMBERS. ORBITAL ATOMIC. PRINCIPLE OF PAULI EXCLUSION. RULE OF HUND. ELECTRONIC STRUCTURES. PERIODIC SYSTEM. PERIODIC SYSTEM OF ELEMENTS AND ELECTRONIC STRUCTURE. DIMENSIONS OF ATOMS. IONIZATION ENERGY. AFFINITY ELECTRONICS. ELECTRONEGATIVITY. CHEMICAL BOND. IONIC BOND. LEWIS MODEL TIE COVALENT. BOND ENERGY. BONDING LENGTH. FORMULAS LEWIS. STRUCTURES RESONANCE LIMIT. MOLECULAR GEOMETRY ACCORDING TO THE THEORY VSEPR. THEORY OF VALENCE BOND. TIE PI SIGMA AND GREEK. TIES DOUBLE AND TRIPLE. ORBITAL HYBRIDIZATION OF ATOMIC. HYBRIDIZATION. MOLECULAR ORBITAL THEORY FOR H2 AND HE2. BOND METAL. POLES OF MOLECULES. WEAK INTERACTIONS: INTERACTIONS HYDROGEN, DIPOLE-DIPOLE, VAN DER WAALS FORCES. CHEMICAL REACTIONS. ASPECTS OF QUALITY AND QUANTITY. CLASSIFICATION OF CHEMICAL REACTIONS. REDOX REACTIONS. ION BALANCE IN ENVIRONMENT (ACID AND BASIC). STOICHIOMETRIC CALCULATIONS. DETERMINATION OF LIMITING REAGENT. SOLID STATE. PROPERTIES OF SOLID. CLASSIFICATION OF SOLID: COVALENT, IONIC, MOLECULAR, METAL. PHYSICAL PROPERTIES OF SOLID. MECHANICAL PROPERTIES. THE GASEOUS STATE. PROPERTIES OF GAS. IDEAL GAS. LAW ISOTHERM, ISOBARIC, ISOCHORIC. EQUATION OF STATE OF PERFECT GASES. IDEAL GAS MIX. OF DALTON LAW. LIQUID. PROPERTIES OF LIQUID. VISCOSITY. VAPOR PRESSURE. CONCEPT OF BOILING POINT. PATTERNS OF STATE. STEPS OF PHASE EQUILIBRIUM AND PHYSICAL. PATTERNS OF STATE OF WATER AND CARBON DIOXIDE. TRIPLE POINT AND CRITICAL POINT. VARIANCE. RULE OF THE PHASES OR GIBBS. SOLUTIONS. SYSTEMS MISSING. SOLVENT AND SOLUTE. METHODS TO EXPRESS THE CONCENTRATION OF A SOLUTION. MOLARITY. MOLALITY. MOLAR FRACTION. IDEAL SOLUTIONS. COLLIGATIVE PROPERTIES SOLUTIONS OF NON-ELECTROLYTES: LOWERING THE STEAM SUPPLY, CRYOSCOPIC, RAISING EBULLIOSCOPIC, OSMOTIC PRESSURE. CHEMICAL BALANCE. OF CHEMICAL BALANCE CONCEPT. CONSTANT BALANCE AND THEIR MEANING. MASS ACTION LAW. QUOTIENT OF REACTION. HOMOGENEOUS EQUILIBRIUM IN GAS PHASE. THERMAL SEPARATION OF GASEOUS MOLECULES. ALTERATION OF AN EQUILIBRIUM: PRINCIPLE OF THE CHATELIER. BALANCE ION SOLUTION. ACIDS AND BASES. DEFINITIONS OF ARRHENIUS AND BRONSTED-LOWRY. SUBSTANCES AMPHOTERIC. AUTOPROTOLYSIS AND KW. SCALES AND PH POH. NEUTRALISATION MONOPROTIC ACID FORTE FORTE-BASIC. WEAK ACIDS MONOPROTIC. WEAK BASES. KA. KB. RELATIONSHIP BETWEEN KA AND KB OF ACID-BASE MARRIED COUPLES. BALANCE OF WEAK ACID IN WATER AND WEAK BASES IN WATER. DETERMINATION OF PH. ELECTROCHEMISTRY. WORKING PRINCIPLE OF A BATTERY. POTENTIAL ELECTRODE. STANDARD ELECTRODE POTENTIAL AND HYDROGEN. BATTERIES STANDARD CONDITIONS. BATTERY IN STANDARD CONDITIONS. BATTERIES NOT STANDARD. NERNST EQUATION. |
| Teaching Methods | |
|---|---|
| TEACHING PROVIDES LESSONS THEORY AND EXERCISES IN CLASSROOM. EXERCISES IN CLASSROOM IS PROPOSED TO STUDENTS SOLVING CHEMICALS THAT ARE EXPRESSION IN CONCRETE FORM AND QUANTITATIVE CONCEPTS COMING FROM TIME TO TIME PROVIDED IN THEORETICAL LESSONS. THE METHOD OF PROBLEM RESOLUTION YOU CHOSEN TO BE ATTENTION TO THE REASONING AND IS BASED ON A PROCEEDING STAGES; FIRST STEP TO UNDERSTANDING OF THE PROBLEM FOLLOWING THE STAGE OF PLANNING AND TERMINATION. THE STAGE OF PLANNING NEED TO REFLECT ON HOW TO SOLVE THE PROBLEM BEFORE YOU HANDLE THE VALUES NUMBER. THE LAST STAGE, THAT VERIFICATION, PROMOTES THE HABIT TO EVALUATE THE REASONABLE RESPONSE AND ENSURES CONSISTENCY WITH THE FUNDAMENTAL PRINCIPLES OF CHEMISTRY. |
| Verification of learning | |
|---|---|
| ASSESSMENT WILL ACHIEVE YOUR INTENDED BY A TEST OF WRITTEN WITH QUESTIONS IN STOICHIOMETRY AND THEORY, INTRODUCTORY TALK TO A HEARING. TO OVERCOME THE EXAM STUDENT MUST SHOW THAT YOU UNDERSTAND AND KNOW HOW TO APPLY THE MAIN CONCEPTS EXPOSED DURING. THE VOTE, OUT OF THIRTY WITH ANY PRAISE, BY MATURITY ACQUIRED WILL DEPEND ON THE CONTENT OF THE COURSE, EVEN TAKING ACCOUNT OF THE QUALITY OF AUTONOMY AND JUDGING DEMONSTRATED. |
| Texts | |
|---|---|
| 1) BRAIN B. LAIRD. CHIMICA GENERALE (MCGRAW-HILL) 2) BROWN-LEMAY. FONDAMENTI DI CHIMICA (EDISES) 3) ANY UNIVERSITY TEXT OF INORGANIC CHEMISTRY |
| More Information | |
|---|---|
| EXERCISES FRONT COVER ABOUT 40% OF THE COURSE |
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