04422 - General Chemistry

Learning outcomes

L’insegnamento si propone di fornire nozioni di base di chimica, quali la composizione, la struttura e la reattività delle molecole, la stechiometria, l'equilibrio delle reazioni chimiche per sistemi omogenei ed eterogenei. Lo studente acquisirà anche la capacità di applicare tali conoscenze alla soluzione di problemi numerici e pratici

Course contents

Prerequisites

Knowledge of elementary functions: powers, roots, exponentials and logarithms. Solution of algebraic equations. Knowledge of the main physical quantities and the relationships that bind them, main units of measurement of the International System (SI) and those non-SI of common use.

 

Program and Contents

1 – Atomic structure – Atomic mass - Mole – Avogadro constant – Model of the hydrogen atom. 2 – Atomic orbitals and electron configuration - Schroedinger equation – Polyelectronic atoms. 3 – Periodic table – Periodic trends. 4 – Chemical bond – Covalent bond – Lewis structures – Molecular geometry – VSEPR theory - Metallic bond – Ionic bond. 5 – State of matter – Gas state – Ideal gas law – Molecular kinetics – Gas mixtures – Partial pressures – Non-ideal gases and Van der Waals equation. 6 – Chemical equilibrium in homogeneous phase – Equilibrium constants and their use - Le Chatelier’s principle – State change equilibria – State diagrams. 7 – Formulas and nomenclature – Chemical reactions and their balancing. 8 – Equilibria in solution – Acids, bases and pH – Buffer solution – Acid-base titrations – Heterogenous equilibria – Solubility equilibria. 9 – Thermochemistry and basics of chemical thermodynamics – Enthalpy and bond energy - Entropy and disorder – Free energy and spontaneous chemical reactions – Free energy, equilibrium constant and its dependence on temperature. 10 – Intermolecular forces and molecular solids – Covalent solids. 11 – Electrochemistry: Chemical energy and electrical work – Cells and electromotive force – Standard potentials and potential scale – Nernst equation.

The laboratory course will also include numerical exercises on the following topics: Empirical and molecular formulas – Percent composition – Chemical reactions balance – Oxidation state – Stoichiometry – Yield – Limiting reactant – Chemical equilibrium – Concentration in solution: molarity, molality, normality, mass percentage, volume percentage – Molar fraction – Heterogeneous solubility equilibria – Solution equilibria: water self-ionisation, acids and bases, pH, buffer solutions, acid-base titrations –Electrochemistry: standard reduction potential, galvanic cells, electrolytic cells, Nernst equation.

Readings/Bibliography

Weller, Overton, Rourke, Armstrong “Inorganic Chemistry 6th Edition”, ISBN 978-0-19-964182-6

Burrows, Parsons, Price, Holman, Pilling “Chemistry³: Introducing Inorganic, Organic and Physical Chemistry, 2nd edition", Oxford University Press, ISBN 978-0-19-969185-2

Teaching methods

Lectures will be complemented by tutorials consisting of exercises about the topics treated. The course is supported by activities and experiences of General Chemistry Laboratory aimed at experimenting and verifying the contents of the lessons and developing skills in basic operations in the chemical laboratory.

Laboratory activities require mandatory attendance of practical experiences. Each student is required to produce their own "laboratory notebook" in which the experiences they carried out are described and discussed. The frequency will be ascertained by signing an attendance sheet at the end of each laboratory experience. Any exceptions will be subject to evaluation by the teacher responsible for the practical laboratory activities.

To facilitate the acquisition by the student of a method of study appropriate to the characteristics of a university course and overcome any difficulties, the course offers the opportunity to perform exercises in the classroom in the presence of the teacher or a tutor, appointed by the School of Science. The role of the tutor is to balance the difficulty of the exercises, provide a clear solution and clarify the doubts that may have emerged during the student autonomous study.

Assessment methods

The knowledge examination is carried out with a final exam divided into a written and an oral part. The written test consists of solving problems, exercises and open questions, and is considered passed with a score equal to or greater than 18/30. Teaching material with exercises and problems of the same type of those included in the final test is available to students and downloadable from the Virtuale platform (https://virtuale.unibo.it/).

The oral test can be undertaken only after passing the written test. The oral exam aims to verify the acquisition of the knowledge provided according to the detailed objectives of the course and will be considered passed upon providing correct answers to the majority of the formulated questions. The passing of the latter also leads to the final grade, which results from the average of the two scores. The contents of the theory module and the laboratory module both contribute to the final grade.

The final written test can be replaced by two ongoing tests (problems, exercises and open questions). The average score obtained in the individual tests provides the final written grade.

To undertake the exam it is required to register through "Alma esami", in compliance with the deadlines indicated.

Teaching tools

Lessons are held with the help of whiteboard and PowerPoint presentations. The teaching material projected during lessons is made available in advance to students on Virtuale.

The laboratory activities are carried out at the teaching laboratories and involve the assignment of a workstation (chemical bench) and individual equipment (glassware) with which the experimental activities must be conducted.

A teaching tutor will be appointed to support learning.

Office hours

See the website of Cristina Femoni

See the website of Massimiliano Curcio