66907 - General Chemistry (A-L)

Learning outcomes

The student acquires the fundamental knowledge on Chemistry and understands its importance as a central, useful, and creative branch of science. He also learns how to solve practical and numerical problems.

Course contents

No prerequisites but recommended skills

The course starts from the fundamentals of chemistry and does not require any specific prior knowledge of the subject. However, basic mathematical skills are recommended, particularly scientific notation, the properties of powers and logarithms, and the solution of quadratic equations.

Atomic structure and periodic properties

Atomic structure, isotopes, and atomic mass of the elements. Quantum numbers, orbital shapes, and electron configurations. Organisation of the periodic table and interpretation of the main periodic properties: ionisation energy, electron affinity, and atomic size.

Fundamental quantities of the International System of Units, amount of substance, and the mole. Application of these concepts to simple quantitative problems.

Chemical bonding and molecular structure

Covalent, polar covalent, ionic, and metallic bonding. Electronegativity and bond energy. Representation of molecules using Lewis structures. Resonance and contributing structures.

Geometry of polyatomic molecules according to VSEPR theory. Hybrid orbitals and the relationship between structure, geometry, and molecular properties.

Intermolecular interactions, with particular emphasis on hydrogen bonding and its relevance to biological systems. Fundamental principles of chemical nomenclature.

States of matter and solutions

Phase transitions and general properties of the states of matter. An introduction to the behaviour of gases and the characteristics of ionic and covalent solids.

Properties of liquids and aqueous solutions. Ways of expressing solution concentration and their use in chemical calculations. Colligative properties and their interpretation.

Chemical reactions and stoichiometric calculations

Classification and balancing of chemical reactions. Stoichiometric calculations, limiting reagents, and reaction yield.

Oxidation-reduction reactions, oxidation numbers, balancing methods, and the scale of standard electrode potentials.

Chemical equilibrium and Le Chatelier’s principle. Effects of changes in concentration, pressure, and temperature on the position of equilibrium.

Chemical equilibria in aqueous solution. Definitions of acids and bases. Ionic product of water and pH calculations. Strong and weak acids and bases, acid-base equilibria, salt hydrolysis, and buffer solutions.

Solubility equilibria, solubility product, precipitation, and the common-ion effect. An introduction to complexation equilibria.

Elements of chemical thermodynamics and kinetics

Concepts of enthalpy, entropy, and Gibbs free energy and their use in the qualitative interpretation of reaction spontaneity.

Reaction rate, activation energy, and the role of catalysts.

Practical laboratory activities

The course unit includes three practical sessions in the General Chemistry laboratory, linked to the topics covered in the lectures.

The experiments will cover:

• ·oxidation-reduction reactions;
• precipitation and complexation reactions;
• acid-base equilibria, titrations, and the preparation of buffer solutions.

During the activities, students will apply basic experimental procedures, use standard laboratory equipment, collect data, and discuss their results in written laboratory reports.

Readings/Bibliography

Teaching materials provided by the lecturer

Slides used during lectures, worked exercises, and other teaching materials will be made available on the Virtuale platform (https://virtuale.unibo.it).

Notes taken during classes, together with the materials provided by the lecturer, are a useful study aid but do not fully replace a university-level textbook in General and Inorganic Chemistry.

Recommended textbooks

Students may use any university-level General and Inorganic Chemistry textbook they already own. The books listed below are suggested as equivalent alternatives; students may choose according to personal preference, availability, and cost:

• Fusi et al., Chimica: principi generali con esercizi, Idelson-Gnocchi, ISBN 9788879476539.
• V. Balzani et al., Chimica: fondamenti e prospettive, Bononia University Press.
• J. C. Kotz, P. M. Treichel, J. R. Townsend, Chimica, 6th edition, EdiSES.
• T. L. Brown, P. M. Woodward et al., Fondamenti di chimica, 4th edition, EdiSES.
• N. J. Tro, Chimica: un approccio molecolare, 2nd edition, EdiSES.

Scientific articles

No scientific articles are compulsory. Any supplementary readings will be indicated by the lecturer during the course and made available through the Virtuale platform.

Teaching methods

The course unit is intended for first-cycle degree students and includes lectures, classroom problem-solving sessions, and practical laboratory activities.

Lectures will be supported by PowerPoint presentations and will introduce the theoretical principles, models, and applications of General and Inorganic Chemistry.

Explanations will be complemented by numerical exercises worked through by the lecturer on the board, particularly at the end of each topic. These sessions will enable students to apply theoretical concepts, assess their own understanding, and prepare for the written examination.

Active participation will be encouraged and questions, requests for clarification, and discussion of problem-solving strategies will be highly appreciated.

Attendance at lectures is not compulsory but is strongly recommended because the topics are cumulative and numerical practice is important for examination preparation.

Three practical sessions are also scheduled in the General Chemistry laboratory. Attendance at laboratory activities is not compulsory. Students who attend at least two of the three sessions may obtain the laboratory mark through participation and submission of the corresponding reports. Students who attend fewer than two sessions must be assessed on the laboratory component during the oral examination.

In view of the types of activities and teaching methods adopted, participation in this course unit requires all students to complete Modules 1 and 2 in e-learning mode at https://www.unibo.it/en/services-and-opportunities/health-and-assistance/health-and-safety/safety-and-health-in-places-of-study-and-internship and to attend Module 3 of the specific training on health and safety in study environments. Information on the dates and procedures for attending Module 3 is available in the dedicated section of the degree programme website.

The course is a prerequisite for Biochemistry and Molecular Biology. In addition, several third-year courses require students to have passed the main first-year examinations, including General Chemistry, as part of their overall prerequisite requirements.

Assessment methods

 

Assessment consists of a written test, a compulsory oral examination, and assessment of the laboratory component.

Written test

The written test lasts two hours and thirty minutes and normally consists of approximately ten exercises on the main topics of the syllabus, including:

• pH calculations;
• stoichiometry and limiting reagents;
• ·oxidation-reduction reactions;
• colligative properties;
• solubility equilibria;
• ·nomenclature;
• acid-base reactions;
• buffer solutions.

  Exercises carry different marks, generally from 1 to 8 points depending on their difficulty. The mark assigned to each exercise is explicitly stated in the examination paper. An oxidation-reduction exercise is normally worth 3 points, whereas exercises on acid-base equilibria may be worth from 6 to 8 points.

  The written test assesses students’ ability to apply theoretical principles, set up calculations correctly, use appropriate units of measurement, interpret results, and use chemical terminology accurately.

  During the test, students may use only a periodic table and a scientific calculator. Books, notes, and mobile phones used in place of a calculator are not permitted.

  A mark of at least 18/30 in the written test is required for admission to the oral examination.

  The written test may be retaken at any subsequent examination session regardless of the previous result. Retaking the test automatically cancels the previous mark.

  A passed written test remains valid for examination sessions within the same academic year.

  Oral examination

  Registration for the oral examination is compulsory. The examination normally consists of three or four questions and may cover any topic in the syllabus.

  The oral examination assesses understanding of theoretical principles, the ability to connect different topics, independent reasoning, and appropriate use of scientific language.

  Simple numerical applications may be required. A calculator is neither permitted nor necessary.

  Failure to pass the oral examination or rejection of the proposed mark does not invalidate the written-test result, which remains valid within the same academic year.

  The mark for the theoretical component is normally calculated as the average of the written-test mark and the oral-examination mark. The overall evaluation also considers clarity of exposition, reasoning ability, and the level of autonomy demonstrated during the oral examination.

  Assessment of the laboratory component

  The laboratory component includes three in-person experiments on oxidation-reduction, precipitation, complexation, and acid-base equilibria, including titrations and buffer solutions.

  A written report is required for each experiment.

  Attendance is not compulsory. Students who attend at least two of the three sessions may obtain the laboratory mark according to the following criteria:

• 5 points for each laboratory session attended;
• up to 5 points for each report submitted.

  A mark of at least 18/30 is required to pass the laboratory component.

  Students who attend fewer than two of the three sessions, or who do not obtain the minimum laboratory mark, will be asked additional questions during the oral examination on the principles, procedures, data, and interpretation of the laboratory experiments.

  Calculation of the final mark

  The final mark is calculated as a weighted average of:

• the mark for the theoretical component, consisting of the written and oral examinations and corresponding to 7 ECTS credits;
• the mark for the laboratory component, corresponding to 1 ECTS credit.

Grading criteria

30 with honours-30: complete and in-depth knowledge; correct and independent solution of problems, including complex ones; excellent ability to make connections and evaluate critically; precise scientific language; full autonomy in argumentation and interpretation of results.

Fail: fragmentary or seriously incomplete knowledge; inability to set up or complete fundamental procedures; poor understanding of concepts; inappropriate language; lack of autonomy in analysis and argumentation.

Intermediate grades: marks from 18 to 29 will be awarded proportionally, based on the level of knowledge demonstrated, the correctness and completeness of the answers, the ability to establish connections and perform critical analysis, the appropriate use of scientific language, and the degree of autonomy shown during the examination.

With regard to assessment, the use of AI is prohibited. Any use constitutes a breach of academic integrity.

Teaching tools

Teaching activities will use:

• personal computer and projector;
• PowerPoint presentations;
• whiteboard or blackboard for worked exercises;
• equipment and materials available in the teaching laboratory;
• the Virtuale platform for sharing slides, exercises, and any supplementary materials: https://virtuale.unibo.it.

Students with specific learning disabilities or temporary or permanent disabilities are advised to contact the University office responsible in good time (https://site.unibo.it/studenti-con-disabilita-e-dsa/en). The office will propose any appropriate adjustments, which must in all cases 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 unit.

Office hours

Please consult Professor Nelsi Zaccheroni’s faculty webpage.

Office hours

See the website of Nelsi Zaccheroni