00088 - Chemistry

Learning outcomes

The course is aimed to provide to the students a basic understanding of the structure of matter and of the thermodynamic and kinetic principles that rule its transformation. The students will also acquire the basic knowledge to understand the connections among the structure, the properties and the reactivity of the organic molecules with particular emphasis on their acid-base characteristics. The student will be able to critically analyze, from a molecular point of view, the chemical reactions that take place in the agro-environmental ecosphere.

Course contents

MOD. 1 (Prof. Enrico Rampazzo, 3 CFU - 30h)

Introduction

What Chemistry Is.

Chemical Classification of Matter

Elements and compounds, pure substances and mixtures. Atomic symbols, atomic number and mass number, isotopes, ions.

Atomic weight, chemical formulas, mole.

Atomic mass, atomic weight, formula weight and molecular weight; mole.

Atomic structure

Hydrogen atom and multielectronic atoms. Orbitals, quantum numbers and electron configurations. The periodic table and periodic properties.

Chemical Bonding

The covalent bond: Lewis structures, electronegativity, molecular geometry and polarity; valence bond theory, hybrid orbitals, multiple bonds. Molecular orbital theory (overview). Ionic bonding, 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: vapor pressure, melting point and boiling point. Structure and physical properties of solids (overview). Allotropy and polymorphism. Allotropic forms of major elements. Phase diagrams, phase transitions.

Solutions

Molarity and other ways of expressing concentration. Dilutions. Colligative properties, osmotic pressure. Solubility.

 

MOD. 2 (Prof. Massimo Baroncini, 3 CFU - 30h)

Chemical Equations and Main Categories of Compounds

Balancing chemical equations, stoichiometric calculations, limiting reagent. Oxidation number; redox reactions: principles and balancing. Overview of the main families of inorganic compounds: oxides, hydrides, acids, bases, salts.

Introduction to Chemical Thermodynamics

Heat, work and energy; first law of thermodynamics, state functions, reaction and formation enthalpy, standard states, Hess’s law. Spontaneous processes: entropy. Second and third law of thermodynamics. Gibbs free energy.

Chemical Equilibrium

Equilibria in the gas phase. Complete and incomplete reactions; equilibrium constant, reaction quotient, effect of temperature, Le Châtelier’s principle; meaning and use of the equilibrium constant.

Equilibria in Aqueous Solution. Acids and Bases

Properties of acids and bases (Brønsted–Lowry model), conjugate acid–base pairs, amphoteric compounds. Autoionization 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.

Solubility Equilibria

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

Chemical Kinetics

Introduction to chemical kinetics: reaction rate; rate equations; reaction order; rate constants and factors influencing them. Reaction mechanisms and elementary steps. Activated complex, activation energy. Homogeneous and heterogeneous catalysis.

Overview of the Chemical Properties of Main Elements

The periodic table and periodic chemical trends; outline of the properties of the main elements belonging to the s‑block and p‑block (groups 1 to 3 and 14 to 18). The carbon cycle, oxygen cycle, nitrogen cycle, sulfur cycle, and phosphorus cycle.

Elements of Organic Chemistry

Aliphatic hydrocarbons: alkanes, cycloalkanes, alkenes, alkynes; structure, nomenclature, conformations, geometric isomerism. Chirality. Aromatic hydrocarbons: benzene and derivatives; heterocyclic compounds. Aliphatic and aromatic halides, alcohols, ethers, amines. Carbonyl derivatives: aldehydes, ketones, carboxylic acids, acyl halides, esters, amides. Macromolecules and polymers. Fatty acids, surfactants.

Classes of Biologically Relevant Molecules

Carbohydrates, lipids, amino acids and proteins, nucleic acids.

Readings/Bibliography

It is mainly 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 other study texts are invited to discuss with the teacher to verify the contents.

Teaching methods

Classroom lectures with power point presentations concerning the theoretical aspects of the course.

Practical lectures dealing with chemistry numerical problems, with particular reference to final exam examples.

Compatibly with time, the possibility of using small videos and / or simple experimental demonstrations in the classroom will be evaluated.

The attendance to the lectures and the study of the teaching material is essential to passing the final exam.

Assessment methods

The final assessment consists of a written examination designed to verify the acquisition of the knowledge and skills developed throughout the course. Students have 1.5 hours to complete the test and may not use notes, handouts, textbooks or any electronic device other than a scientific calculator. Students must bring a valid photo ID, a scientific calculator, a blue or black pen, and a periodic table (provided by the instructor in the teaching materials).

The written exam includes:

• Seven multiple‑choice theory questions covering all topics addressed during the course (scoring: +2 for a correct answer; 0 for no answer; –1 for an incorrect answer).

• Three numerical exercises, each on a different topic selected from: atomic weight and mole, stoichiometry, colligative properties, chemical equilibrium, acid–base equilibria, pH, hydrolysis, buffer solutions, acid–base titrations, solubility equilibria (each exercise worth up to 6 points).

The final score is obtained by summing the points from all questions and problems. The maximum achievable score is 32, corresponding to 30 with honours. The exam is passed with a minimum score of 18.

Permitted materials during the written exam

• a periodic table without nomenclature

• a scientific calculator

• writing materials

• one A4 sheet (double‑sided) containing definitions, schemes, formulas, examples or any information considered useful

Students with certified specific learning disorders (DSA) may use up to four A4 sheets (double‑sided); no prior authorization from the instructor is required.

The use of any electronic device other than the calculator is strictly prohibited (e.g., tablets, smartphones, personal computers, smart glasses with camera or AI functions, earphones).

The final written exam determines the course grade; no mid‑term tests are scheduled. Students may request an optional oral examination to improve the grade obtained in the written test.

Both the written and the optional oral exam may be taken in English. Students wishing to take the exam in English must notify the instructor by email at least one week before the examination.

Detailed information on exam procedures is available in the file “0 – Info Corso di Chimica PA” on the course page of the online teaching platform (https://virtuale.unibo.it/).

Students with DSA or disabilities

Students with certified DSA or temporary/permanent disabilities are advised to contact the University support office (https://site.unibo.it/studenti-con-disabilita-e-dsa/it). The office will propose any necessary accommodations, which must be submitted to the instructor at least 15 days in advance for approval, in accordance with the learning objectives of the course.

Additional Requirements for Students from the “Semestre Filtro”

Students entering the Produzioni Animali degree programme from the “semestre filtro” must complete an additional 2 CFU of Chemistry. Recognition of these credits requires passing a written exam on the following supplementary topics:

• construction of Lewis structures for simple molecules and polyatomic ions; determination of molecular geometry using VSEPR

• calculation of moles from mass

• definitions and calculations of concentration units: mass and volume percent, mole fraction, molality, molarity, normality

• electrolytic solutions: strong and weak electrolytes; degree of dissociation; van’t Hoff factor

• calculations involving colligative properties and determination of solute molar mass

• balancing chemical reactions (including redox) and related stoichiometric calculations

• stoichiometric calculations involving solubility equilibria (solubility, common‑ion effect, saturation conditions)

• stoichiometric calculations and pH determination in acid–base solutions (strong and weak acids/bases, buffer solutions)

Se vuoi, posso armonizzare tutte le sezioni già tradotte in un syllabus completo e impaginato oppure produrre una versione più sintetica per brochure o guide rapide.

Teaching tools

Projectors, interactive whiteboards and classroom whiteboards.
Possibility to download (https://virtuale.unibo.it/) the lectures teaching material given by the teacher.

A section of the teaching material will be dedicated to the information related to the participation of the course and for undertake of the final exam.

Office hours

See the website of Enrico Rampazzo

See the website of Massimo Baroncini