GENERAL AND INORGANIC CHEMISTRY
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- Versione italiana
- Academic year
- 2022/2023
- Teacher
- ALESSANDRA MOLINARI
- Credits
- 9
- Didactic period
- Primo Semestre
- SSD
- CHIM/03
Training objectives
- Knowledge goals: acquire knowledge and skills in chemical discipline and language.
Skill goals: Students are expected to learn how to apply general concepts to problem solving and to perform calculations related with simple general chemistry problems and simple laboratory operations (weighting, volumetric glassware, pHmeters). Acquisition of awareness to safety, to respect for the environment, to resources saving and to responsible management of lab waste.
Expected results: after attending lectures and the laboratory and having studied the subject independently, the student will be able to represent the substances through symbols and formulas, to predict the geometry of molecules and some their properties. He/she will be able to deduce information from the Periodic Table of the elements. He/she will have acquired the ability to represent a chemical transformation through a balanced reaction equation and to use it quantitatively. He/she will be able to solve fundamental stoichiometric calculations and to perform simple laboratory operations (weighing, making volume, measuring of pH) with attention to safety and waste management. Prerequisites
- Basic physics concepts usually learned in high school, use of the most common measure units. Fundamentals of mathematics (e.g. first and second grade equations, logarithms properties, exponential notation, use of a bidimensional diagram).
Fundamentals of general chemistry usually learned in high school. No rules are present, since this course is the first course in Chemistry. Course programme
- PART ONE: the structure of matter (24 hours, 3 credits).
- The language of chemistry: matter, elements, compounds, mixtures. Homogeneous and heterogeneous systems. Matter constituents (atoms, molecules, ions) and their representation (symbols, formulae, names, chemical equations).
- Absolute and relative atomic masses, molecular mass, formula weight. Avogadro number. Mole concept, quantitative meaning of formulae and chemical equations.
- Inorganic nomenclature – from the formula to the name and from the name to the formula.
- Atomic structure. Atom constituents: electrons, protons, neutrons. The nucleus. Atomic number and mass number. Isotopes.
- Recent models for the hydrogen atom. Orbitals and quantic numbers. Polyelectronic atoms. Aufbau. Electronic configuration and position in the Periodic Table, periodic properties.
- Chemical bond: Valence bond theory. Ionic and covalent character, electronegativity. Bond order: simple, double and triple bonds. Bond polarity, bond length, bond energy. Lewis structure, hybridization, VSEPR, resonance. Representation of common molecules, molecular geometry and properties. Fundamentals of molecular orbitals theory, some examples. Dative bond and coordination compounds. Metallic bond. Intermolecular interactions. Hydrogen bond and its influence on the properties of some substances.
- Physical states of the matter. Gases, laws of gases, state equation of ideal gases, Avogadro principle. Mixture of gases. Partial pressures and Dalton law. Real gases. Basics on solid and liquid state. Phases equilibria, state diagrams.
- Solutions – Kind of solutions, solubility. Concentration and various ways to express concentration. Aqueous solutions, electrolytes properties. Preparation of solutions and dilution problems. Colligative properties.
PART TWO: how matter transforms (32 hours - 4 credits)
- Reactions – chemical and physical transformations.
- Chemical reactions: qualitative aspects: acid-base reactions, redox. Ionic equations.
- Quantitative aspects – balancing, stoichiometric ratios, excess-defect of reagent, limiting reagent, yield.
- Reactions in gas phase. Reactions in solutions. Equivalent and normality. Titrations.
- Introductory notes on energy in reactions and spontaneity - first principle, enthalpy, entropy, second principle, free energy.
- Introductory notes on Kinetics. Rate of reaction. Reaction order and its determination. Reaction rate control. Catalysis.
- Chemical equilibrium: definition, equilibrium constant, mass law, Le Chatelier principle. Homogeneous equilibria in gas phase. Equilibria and temperature. Free energy and equilibrium.
- Acids, bases and equilibria in aqueous solution. Ionic dissociation of water. Ionic product of water, pH. Acids and bases: various definitions, strength, dissociation constants and their use, dissociation grade.
- Polyprotic acid, salt hydrolysis, amphoterism, buffer solutions.
- Heterogeneous equilibria. Solubility product constants. Precipitation reactions.
- Electrochemistry, electrochemical cells. Nernst equation. Spontaneous and non-spontaneous redox reactions.
- Redox equilibrium constants determination.
- Electrolysis, Faraday law, some applications.
PART THREE: INORGANIC CHEMISTRY (8 hours – 1 credit)
- The Periodic Table and the information therein.
- For some elements of the representative groups: natural state, industrial and lab preparation of the elemental state, properties; main compounds and their preparation and properties. Notes on inorganic pollutants chemistry.
- Chemistry of d-block elements: some examples mainly related to coordination chemistry and organometallic derivatives.
PRACTICAL WORK IN LAB: 4 sessions, 3 hours each (each student attends to 12 hours of practice in lab. 12 hours are equivalent to 1 CFU). The arguments of the 4 sessions are listed below:
SESSION 1: the lab, chemicals, mole, density.
SESSION 2: chemical reactions
SESSION 3: solutions
SESSION 4: acids, bases, pH Didactic methods
- Teaching will be delivered exclusively in PRESENCE in the classroom and laboratory. NO form of synchronous or non-synchronous (i.e., videotaped) distance learning will be available. The hands-on laboratory portion will take place approximately in November. Access to the laboratory is conditional on obtaining a "low risk" safety certificate.
The Classroom will be used as a virtual environment in which to exchange teaching materials and organizational information. The student must therefore register for the Classroom using the code gjdz7jt Learning assessment procedures
- The final examination consists of a written and an oral test.
The written consists of two sections: section 1 consists of 5 questions on Part One of the content (excluding chemical bonding). Each question done correctly is worth 2 points. Section 1 is passed with scores greater than or equal to 6.
Section 2 also consists of 5 numerical exercises on Part Two of the contents. Each exercise done correctly is worth 4 points. Section 2 is passed with a score greater than or equal to 12.
The paper is approved ONLY if both Sections are passed. Overall, the written test is passed with a score greater than or equal to 18. The time allotted for the written is 90 minutes. Use of the periodic table is encouraged, reference of texts and tables and use of calculator are allowed.
An approved written is essential for admission to the oral.
The written is valid for not more than 6 months. By the deadline, the student must take and pass the oral interview.
The oral will focus on chemical bonding, Part III content, and practical work done in the laboratory.
The final evaluation is based on the oral interview, which must be graded favorably in itself (with a grade of 18 to 30Lode), and on the grade obtained in the written assignment.
In order to obtain the maximum score in the exam, the written paper must also be perfect (5 correct answers out of 5 exercises/questions in each Section).
6/7 appeals will be scheduled during the calendar year. Reference texts
- J. C Kotz, P. M. Treichel, J. R. Townsend - CHIMICA - Edises VI or VII Edition
and
I. Bertini, F.Mani - Stechiometria - Ambrosiana, Milano
