C9364 - CHIMICA GENERALE ED INORGANICA

Learning outcomes

The course aims to provide students with the basic concepts of chemistry and the ability to apply this knowledge to the solution of numerical and practical problems. In particular, students will be able to: understand and describe the composition, structure and reactivity of molecules; use the Periodic Table as a basis for rationalising chemical phenomena; carry out stoichiometric calculations using the concepts of mole, concentration, pH and solubility; apply the general principles governing the equilibrium of chemical reactions to homogeneous and heterogeneous systems; apply the concepts of electrochemistry to chemical processes; recognise inorganic compounds.

Course contents

Introduction to Chemistry: the importance of chemistry as a basic science. Introduction to the scientific method and critical thinking.

Chemical classification of matter: substances and mixtures; elements and compounds; homogeneous and heterogeneous systems. Considerations on the limitations of experimental measurements.

The atom: atomic theory; composition of atoms, atomic number and mass number; isotopes and atomic weight; atomic structure and an outline of quantum theories; atomic orbitals, quantum numbers and spin; orbitals in polyelectronic atoms and filling order; electronic configurations of the elements.

Periodic Table: relationship with electronic configurations; ionisation energies; electron affinities; atomic dimensions and their periodic trends.

Compounds: empirical and molecular formulae; valence; oxidation state and its determination; nomenclature; mole, Avogadro’s number and number of moles; binary compounds with oxygen, oxides, and their nomenclature; classification of their hydrolysis products; binary compounds with hydrogen.

Chemical bonding: general concepts; sharing of electron pairs; number of bonds, molecules and infinite structures; Lewis structures of molecules and polyatomic ions, including formal charges and expansion of the octet; molecular geometry in relation to structural formulae, using the VSEPR method; predictions of molecular polarity as a function of geometry and electronegativity; resonance; isomerism; molecular weight and formula weight.

Ionic bonding: lattice energy and crystal lattice; stoichiometry of ionic compounds.

Covalent bonds: outline of valence bond theory and electronic configuration; outline of molecular orbital theory; coordinate bond: acceptors and donors.

Type of bond and position within the Periodic Table. Valence, oxidation state and coordination number.

Non-covalent molecular interactions: Van der Waals interactions, London dispersion forces and hydrogen bonds. Metals and non-metals; outline of metallic bonding.

Elements of inorganic chemistry: review of periodic properties, including electronic configuration, main oxidation states and electronegativity. Acid-base and redox properties of the main elements. Introduction to coordination compounds.

States of matter: states of aggregation of matter; general properties of solids, liquids and gases; polymorphism and allotropy; relationship between pressure, temperature and volume in gases; theoretical model of gases; equation of state; ideal gas mixtures; partial pressures; changes of state; phase diagrams.

Solutions: general concepts; methods for expressing the concentration of a species: percentage by weight and volume, mole fraction, molality and molarity; conversions between concentration units; solubility and saturated solutions; electrolyte solutions: strong and weak electrolytes, degree of dissociation and van’t Hoff factor; characteristics of ideal, dilute and concentrated solutions.

Chemical reactions: reactions and chemical equations; law of conservation of mass and balancing of equations; redox reactions and their balancing; reactions in solution and ionic form of their equations; mass relationships in chemical reactions; stoichiometric calculations.

Chemical equilibria: complete and incomplete reactions; spontaneity of a reaction; reaction quotient; law of mass action; equilibrium constant; homogeneous and heterogeneous equilibria; solubility and solubility product; effects of pressure, volume, and amounts of reactants and products on equilibria; effects of heat and temperature on equilibria; Le Chatelier’s principle; simultaneous equilibria; stoichiometric calculations.

Acids and bases: proton theory of acids and bases; conjugate acids and bases; autoprotolysis reactions; ionic product of water; determination of the strength of acids and bases: Ka and Kb and classification; polyprotic acids and bases; relationship between molecular structure and acid-base properties; acid-base properties of ions; acidity and basicity of aqueous solutions: pH and pOH; reactions between acids and bases; acidity and basicity of salt solutions; reactions between acids and salts or bases and salts; properties of buffer solutions; stoichiometric calculations.

Electrochemistry and galvanic cells: galvanic cells; electromotive force and reduction potentials; use of potentials; Nernst equation; concentration cells, corrosion and electrolysis.

Readings/Bibliography

It is essential to use the teaching materials provided, including slides, worked examples and exercises, self-assessment exercises available on Virtuale (https://virtuale.unibo.it/ ), together with lecture notes.

Students are advised to supplement their study with a university-level textbook for introductory courses in General and Inorganic Chemistry.

Among the many possible options, the following are suggested:

• Balzani, Moggi, Prodi, Venturi, CHIMICA: FONDAMENTI E PROSPETTIVE, Bononia University Press, 2021
• R.H. Petrucci, F.G. Herring, J.D. Madura, C. Bissonnette, Chimica Generale, Piccin

Students who already have other textbooks are invited to contact the lecturer in order to verify their suitability and contents.

Teaching methods

The course adopts an active, student-centred teaching approach, integrating short lectures, guided exercises, problem-solving activities, inquiry-based learning activities and self-assessment opportunities. Topics are introduced through problem-based questions and applied cases, in order to foster understanding of the fundamental principles of chemistry and their application to the solution of numerical and conceptual problems. During the course, students are engaged in individual and collaborative activities, formative quizzes and guided discussions, with the aim of developing progressive autonomy, chemical reasoning skills and awareness of their own learning process.

Assessment methods

Assessment consists of a short written test and an oral examination, both aimed at verifying the achievement of the course learning outcomes.

The short written test has an indicative duration of 60 minutes and consists of numerical exercises related to the main topics of the course. The test is designed to assess the student’s ability to apply the fundamental concepts of general chemistry to the solution of structured problems, such as stoichiometric calculations, concentrations, chemical equilibria, pH, solubility, redox reactions and electrochemistry. The assessment of the written test will take into account the correctness of the procedure, the appropriate use of units of measurement, the coherence of the logical steps and the ability to interpret the result obtained. Admission to the oral examination is conditional upon achieving a passing grade in the written test.

During the written test, students are allowed to use:

• a Periodic Table of the elements;

• a scientific calculator.

The use of textbooks, notes or handouts is NOT permitted.

During the examination, the use of ANY electronic device other than the calculator is NOT permitted.

The oral examination is aimed at assessing the understanding of theoretical concepts, the ability to connect the different topics of the course and the correct use of chemical terminology. During the oral examination, the exercises completed in the written test may also be discussed, in order to verify the student’s awareness of the procedure adopted, the ability to identify and correct any errors, and the mastery of the chemical principles involved.

The final grade is expressed out of 30 and takes into account the overall outcome of the two tests. The written test contributes 40% to the final grade, while the oral examination contributes 60%. In order to pass the examination, students must demonstrate sufficient preparation both in the solution of applied problems and in the understanding and discussion of the fundamental concepts of the discipline. Students must also have obtained the pass/fail assessment for the General Chemistry laboratory component.

In addition to the correctness of the answers, the assessment considers the ability to apply knowledge to chemical problems, to justify the procedures used, to critically interpret the results and to communicate clearly and appropriately. The use of digital tools or generative Artificial Intelligence is not permitted during the examination, unless explicitly indicated otherwise by the lecturer.

Students with specific learning disorders, temporary or permanent disabilities are recommended to contact the relevant University office in good time (https://site.unibo.it/studenti-con-disabilita-e-dsa/it ). The office will propose any necessary adjustments to the students concerned; these adjustments must in any case be submitted to the lecturer for approval at least 15 days in advance. The lecturer will assess their suitability also in relation to the learning outcomes of the course.

Teaching tools

Video projectors, interactive whiteboards and classroom boards.

Teaching materials distributed by the lecturer can be downloaded from the course section on the online learning platform (https://virtuale.unibo.it/ ). Subject to prior request by email to the lecturer, recordings of the lectures held in class may also be made available.

Office hours

See the website of Lucia Maini