00088 - Chemistry

Learning outcomes

At the end of the course, the student will have acquired an understanding of the structure of matter and of the thermodynamic and kinetic principles governing its transformation, and will be able to interpret the structural and functional properties of molecules involved in elemental cycles within the agro‑environmental biosphere.

Course contents

The course programme* begins with a description of atomic structure, and then addresses the properties of systems of increasing complexity: molecules, substances, homogeneous and heterogeneous systems, and their transformations.

Introduction. The importance of chemistry as a fundamental science. Problem‑solving and the improvement of quality of life. The relevance of chemistry within the degree programme.

Chemical Classification of Matter. Substances and mixtures – elements and compounds – homogeneous and heterogeneous systems. Atoms, atomic symbols and formulas, atomic number and mass number, isotopes, ions. Considerations on the limitations of experimental measurements.

Atomic Weight, Chemical Formulas, Mole. Atomic mass, atomic weight, formula weight and molecular weight; the mole.

Structure of the Atom. The hydrogen atom and multielectron atoms. Orbitals, quantum numbers and electronic configurations. The periodic table and periodic properties.

Compounds and Chemical Bonding. The covalent bond: Lewis structures, electronegativity, molecular geometry and polarity; valence bond theory, hybrid orbitals, multiple bonds. Introduction to molecular orbital theory. Ionic bonding and ionic lattices. Metallic bonding (overview). Intermolecular forces, hydrogen bonding. Empirical and molecular formulas, VSEPR theory and molecular geometry. Nomenclature of simple molecules and polyatomic ions.

Gases, Liquids, Solids. Properties of ideal gases, partial pressures; introduction to kinetic molecular theory. Liquids: vapour pressure, melting and boiling points. Structure and physical properties of solids (overview). Allotropy and polymorphism. Allotropic forms of major elements. Phase diagrams and phase transitions.

Solutions. Molarity and other concentration units. Dilutions. Colligative properties, osmotic pressure. Solubility.

Chemical Reactions. Chemical reactions and equations; law of conservation of mass and balancing. Redox reactions and their balancing. Mass relationships in chemical reactions. Stoichiometric calculations.

Thermodynamics. Introduction to heat exchange in reactions (internal energy, enthalpy), entropy and its meaning. Introduction to the concepts of entropy and free energy. Spontaneity of reactions as a function of temperature and major thermodynamic parameters.

Chemical Equilibria. Complete and incomplete reactions. Chemical equilibria. Reaction quotient and law of mass action, equilibrium constant. Homogeneous and heterogeneous equilibria. Effect of major experimental parameters on equilibria. Le Chatelier’s principle. Simultaneous equilibria. Stoichiometric calculations.

Solubility Equilibria. Behaviour of sparingly soluble salts. Solubility and solubility product. Common‑ion effect.

Acids and Bases. Properties of acids and bases (Brønsted–Lowry model), conjugate acid–base pairs, amphoteric compounds. Autodissociation of water. pH: definition and calculation for strong and weak acids and bases, degree of dissociation. Salt hydrolysis and its effect on pH. Buffer solutions, acid–base titrations.

Fundamentals of Organic Chemistry. Representation of organic structures. Hybridisation of the carbon atom.

Acids and bases according to Lewis, nucleophiles and electrophiles.

The main classes of organic compounds and functional groups will be briefly described, with introductory notes on their nomenclature: hydrocarbons (alkanes, alkenes, alkynes, arenes), alcohols and phenols, amines, aldehydes, ketones, carboxylic acids and their derivatives (esters, amides, anhydrides, acyl halides).

Polarity and acid–base properties of major functional groups. Relationship between polarity and acid–base behaviour of simple organic molecules.

Introduction to Biomolecules: fundamental units, structure and properties of selected biomolecules: amino acids, peptide bond and proteins, enzymes and their function. Lipids: fats, oils, soaps. Phospholipids. Steroids. Biological membranes. Overview of Wood and Humic Acids

*Students may request a more detailed programme from the instructor via email.

Readings/Bibliography

It is recommended to use the teaching material and lecture notes. As a supplement to the study any UNIVERSITY text dedicated to General and Inorganic Chemistry courses of the first level is suitable.

Students who already have a book are invited to verify with the teacher its contents.

Teaching methods

Teaching Methods: lectures: delivery of theoretical course content through classroom lectures supported by PowerPoint presentations. Use of simple animations and visual materials to aid the understanding of molecular geometry.

Exercises: problem‑solving sessions at the blackboard covering the main topics of the course, with emphasis on examples relevant to the final examination.

Subject to compatibility with the course schedule, the use of short videos and/or simple in‑class experimental demonstrations may be considered.

Regular attendance and consultation of the teaching materials are essential for successful completion of the final assessment.

Assessment methods

The final assessment consists of a written examination aimed at verifying the acquisition of knowledge and skills developed throughout the course.

Students have 2 hours to complete the exam and may NOT use:

• handouts or textbooks

• any electronic device other than a calculator

Students must bring the following materials to the exam:

1. a valid photo ID: identity card, driver’s license, or university badge with a high‑quality photo that allows personal identification

2. a scientific calculator

3. a black or blue pen

4. a periodic table of the elements NOT containing information on compound nomenclature (a suitable version will be provided by the instructor among the teaching materials)

The written examination includes:

• seven multiple‑choice theory questions covering all topics addressed during the course. Scoring: 2 points for a correct answer; 0 points for no answer; −1 point for an incorrect answer.

• three numerical exercises on the following topics: atomic weight and the mole; balancing chemical reactions (including redox reactions); stoichiometric calculations (including limiting reagent problems); concentration calculations and solution preparation; acid–base reactions and equilibria in solution (pH calculation, hydrolysis reactions, acid–base reactions, buffer solutions); colligative properties; solubility equilibria. The maximum score for each numerical exercise is 6 points.

The final score of the written exam is obtained by summing the points earned in all questions and problems.

The maximum achievable score is 32 points, corresponding to 30 cum laude. The exam is passed with a minimum score of 18 points.

During the written examination, students are allowed to use:

• a periodic table of the elements that does NOT include nomenclature information

• a scientific calculator

• writing materials

• one A4 sheet (front/back) on which definitions, schemes, formulas, examples, or any information deemed useful for the exam may be written

Students with DSA certification are allowed to use four A4 sheets (front/back), which may not be subject to instructor verification.

During the exam, the use of ANY electronic device other than a calculator is strictly prohibited. Examples include: tablets, smartphones, personal computers, smart glasses equipped with cameras or AI functions, earphones.

The evaluation of the final written exam determines the course grade; no midterm tests or extraordinary exam sessions are scheduled for regularly enrolled students.

Students may choose to take an optional oral examination to improve the grade obtained in the written test, provided the written score is 18 or higher.

Both the written and the optional oral examination may be taken in English. Students who wish to take the exam in English must notify the instructor by email no later than one week before the examination.

Students with DSA certification or temporary/permanent disabilities must contact the instructor and the responsible University office  (https://site.unibo.it/studenti-con-disabilita-e-dsa/it ) at least 15 days before the exam date.

If the default compensatory tools described above are not sufficient, students are strongly encouraged to contact the University office responsible (https://site.unibo.it/studenti-con-disabilita-e-dsa/it ) well in advance. The office will propose additional compensatory and/or dispensatory measures, which must be submitted—at least 15 days before the exam—to the teacher for approval, who will evaluate their appropriateness in relation to the learning objectives of the course.

Teaching tools

Classrooms are equipped with video projectors, interactive whiteboards and traditional blackboards.

Teaching materials used during lectures can be downloaded from the course page on the University online platform (https://virtuale.unibo.it/).

The online teaching materials provided include detailed information on participation requirements, exam procedures and grade acceptance.

 

Office hours

See the website of Enrico Rampazzo