00088 - Chemistry (A-L)

Learning outcomes

Upon completion of the course, the student will have acquired fundamental knowledge of chemistry and will be able to apply this knowledge to the resolution of numerical problems. Furthermore, the student will recognize chemistry as an interdisciplinary, useful, and innovative science.

Course contents

Prerequisites and recommended skills

There are no formal prerequisites. The course starts from the foundations of chemistry and does not require prior subject-specific knowledge. Basic mathematical skills are nevertheless recommended, particularly scientific notation, powers and logarithms, and the solution of quadratic equations.

Introduction

Introduction to chemistry and its impact on everyday life. Experimental measurements, uncertainty and measurement limits. Homogeneous and heterogeneous systems. Elements and compounds.

The atom and electronic structure

Atomic theory and atomic composition: protons, neutrons and electrons; atomic number and mass number. Isotopes and calculation of average atomic mass. The Bohr model, quantised energy levels and limitations of the model. The uncertainty principle and wave-particle duality. Quantum-mechanical model of the hydrogen atom: orbitals, quantum numbers n, l and m, spin, and representation of the main orbital types. Multi-electron atoms, filling order, Pauli exclusion principle, Hund's rule and ground-state electronic configurations.

The periodic table and periodic properties

Groups, periods and blocks. Relationship between position in the periodic table and electronic configuration. Periodic trends in ionisation energy, electron affinity, atomic radii and ionic radii. Relationship between periodic position, chemical behaviour and metallic or non-metallic character.

Chemical bonding

General concepts of chemical bonding. Covalent bonding within valence bond theory: electron sharing, bond order, polarity, electronegativity, bond energy and bond length. Electronic promotion in main-group elements. Lewis structures of molecules and polyatomic ions. Coordinate bonding, donors and acceptors. Molecular geometry, electron-pair repulsions, hybridisation and the relationship between hybridisation and molecular shape. Resonance and electron delocalisation. Fundamentals of molecular orbital theory. Ionic bonding, lattice energy and stoichiometry of ionic compounds. Metallic bonding, electrical conductivity and semiconductors. Intermolecular forces: van der Waals forces, London forces and hydrogen bonding. Effects of temperature and pressure on bonds and material properties.

Chemical formulae, the mole and nomenclature

Empirical and molecular formulae; isomerism, polymorphism and allotropy. Molecular and formula mass. The mole, Avogadro's number and molar mass. Relationships among mass, molar mass and amount of substance. Determination of empirical and molecular formulae. Oxidation number and coordination number. Classification, properties and nomenclature of oxides, hydrides, binary compounds and salts.

States of matter

General properties of solids, liquids and gases. Pressure-temperature-volume relationships; ideal gas model, equation of state and limitations. Introduction to real gases. Ideal gas mixtures and partial pressures. Phase changes and interpretation of phase diagrams.

Solutions

General properties of solutions and concentration units: mass and volume percentage, mole fraction, molality, molarity and normality. Solubility, saturated solutions, strong and weak electrolytes. Ideal, dilute and concentrated solutions. Raoult's and Henry's laws; systems with volatile components and with a non-volatile solute. Osmosis and osmotic pressure. Colligative properties of molecular and electrolyte solutions and their use in molar-mass determination. Quantitative applications and stoichiometric calculations.

Chemical reactions and stoichiometry

Chemical reactions and equations. Conservation of mass and balancing. Redox reactions and balancing methods. Molecular and ionic equations in solution. Mass relationships, limiting and excess reagents, and yield. Equivalent masses of oxidising agents, reducing agents, acids and bases. Stoichiometric problem solving.

Thermochemistry and thermodynamics

Internal energy, reaction enthalpy and Hess's law. Entropy, Gibbs free energy and spontaneity. Calculation and interpretation of changes in thermodynamic quantities. Complete and incomplete reactions, useful work and non-spontaneous processes.

Chemical kinetics

Reaction rate, rate laws, reaction order and rate constants. Radioactive decay and selected medical applications. Reaction mechanisms, elementary steps, activated complex and activation energy. Factors affecting reaction rate. Homogeneous and heterogeneous catalysis and chain reactions.

Chemical equilibria

Complete and incomplete reactions. Reaction quotient, law of mass action and equilibrium constant. Homogeneous and heterogeneous equilibria. Solubility and solubility product. Effects of pressure, volume, concentration and temperature. Le Chatelier's principle and simultaneous equilibria. Set-up of stoichiometric calculations for equilibria, with worked classroom examples.

Acids and bases

Brønsted-Lowry theory, conjugate acid-base pairs, autoprotolysis and the ionic product of water. Ka and Kb values and classification of acids and bases, including polyprotic systems. Relationship between molecular structure and acid-base properties. pH and pOH. Neutralisation reactions and salt formation. Acidity and basicity of salt solutions. Calculations involving acid-base equilibria and buffer solutions.

Electrochemistry

Relationship between redox reactions and electricity. Galvanic cells, electromotive force, standard reduction potentials and their dependence on concentration and pH. Use of potentials to predict reaction direction. Relationship between Gibbs free energy and electrical work. Electrolysis.

Applications and problem-solving sessions

Whenever possible, the topics will be connected with examples from everyday life and with scientific, technological and biomedical applications. Worked problems will be presented for every topic involving quantitative treatment. At the end of the syllabus, before the first written examination, a classroom mock examination and a guided board-based solution session will be held.

Readings/Bibliography

Teaching materials provided by the lecturer

All materials used during classes, worked numerical exercises and selected examples of past written examinations will be made available on the Virtuale platform.

Recommended textbooks

Any university-level General and Inorganic Chemistry textbook, including an older edition already owned by the student, may be used. The following are non-binding suggestions and may be selected according to personal preference, availability and cost:

• V. Balzani, M. Moggi, L. Prodi, M. Venturi, Chimica: fondamenti e prospettive, Bononia University Press.
• P. W. Atkins, L. Jones, Principi di chimica, Zanichelli.

Scientific articles

No compulsory scientific articles are assigned. Any supplementary readings will be indicated during the course.

Teaching methods

The course is delivered through lectures and board-based problem-solving sessions. No laboratory activities are included.

Lectures introduce and develop the theoretical principles, models and terminology of General and Inorganic Chemistry. Whenever possible, the lecturer connects the content with practical applications and everyday phenomena, in order to highlight the interdisciplinary nature of chemistry.

Problem-solving sessions focus on the set-up and solution of numerical problems involving formulae, stoichiometry, gases, solutions, colligative properties, equilibria, acids and bases, thermodynamics and electrochemistry. Guided discussion of solution methods helps students assess their understanding, recognise common errors and develop autonomy in selecting appropriate strategies.

Before the first written examination, a mock examination will be held, followed by a guided correction and discussion at the board.

There are no formal prerequisites. The basic mathematical skills listed in the Course contents section are nevertheless recommended.

Assessment methods

Assessment consists of a compulsory written examination. After passing it, students may either request direct registration of the mark or take an optional oral examination.

The use of artificial intelligence is prohibited in both the written and oral examinations. Any use constitutes a breach of academic integrity.

Written examination

The written examination lasts two hours and consists of eight exercises covering the entire syllabus. The first six exercises are mainly numerical and are worth up to 4 points each; partial credit is awarded according to the correctness of the set-up, working, calculations and final result. The final two exercises are more strongly focused on theoretical understanding and are worth up to 3 points each.

The examination assesses knowledge of fundamental principles, the ability to select and apply suitable models and equations, calculation accuracy, correct use of units, justification of methodological choices and the physical-chemical consistency of results.

Students may not leave the examination room before handing in their paper. A scientific calculator is required; mobile phones may not be used, even as calculators, and must remain switched off. A periodic table may be used and, if necessary, will be provided by the lecturer.

Students may also bring one double-sided A4 sheet containing equations from the syllabus that they consider useful, prepared in accordance with the guidelines published on Virtuale.

The examination is passed with a mark of at least 18/30. Students who pass may accept the written mark and request its registration or take an optional oral examination.

Students may reject the written mark and retake the written examination at a later session. Sitting a new written examination automatically cancels the previous result. The valid mark is always that obtained in the most recent written examination, even when it is lower than the previous mark or below the pass threshold.

Optional oral examination

The oral examination normally consists of three questions. Where appropriate, it starts from topics in which difficulties emerged in the written examination, without necessarily requiring repetition of the same exercise, and may cover the entire syllabus.

The oral examination assesses understanding of principles, the ability to establish connections, appropriate scientific language, critical thinking and autonomy in argumentation.

The oral mark is averaged arithmetically with the written mark and may therefore raise or lower the final mark. By attending the oral examination, the student accepts the written mark and may no longer retake the written examination. If the resulting oral mark is rejected, the written examination remains valid for the academic year and the student may take another oral examination, but may no longer request registration of the written mark alone.

Grading criteria

30 cum laude-30: Complete and in-depth knowledge; correct and autonomous solution of complex problems; excellent ability to connect concepts and evaluate them critically; precise scientific language; full autonomy in reasoning.

Fail: Fragmentary or seriously incomplete knowledge; inability to set up or complete fundamental procedures; poor conceptual understanding; 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 interpret processes, diagrams and data, the quality of critical connections, the appropriateness of scientific language, and the degree of autonomy shown during the examination.

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

All materials used during classes will be made available on the Virtuale platform: https://virtuale.unibo.it.

The material will be organised by topic and will include presentations, worked numerical exercises, guidelines for preparing the A4 formula sheet permitted in the examination, and examples of previous examination papers illustrating the structure of the written test.

All students enrolled in the relevant year are invited to join the course page on Virtuale, which will also be used for announcements, notices and notifications to the whole cohort.

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

Office hours

Please consult Professor Nelsi Zaccheroni's webpage.

Office hours

See the website of Nelsi Zaccheroni