Industrial pharmacy

Introductory notions. Subject of chemical research. Chemical phenomena. Fundamental laws of chemistry. Symbols and chemical notation. Amount. Atomic theory. Atoms and their properties. Mass and atomic weight. Avogadro's number. Atomic structure. Atomic spectra. Bohr model. Corpuscular and wave nature of the electron. Quantum numbers. Atomic orbitals. Electronic configuration. Chemical bond: concept of valence. The different types of bonds and their properties: order, energy, bond distance, dipolar moment. Valence bond theory and molecular orbitals. Hybrid orbitals, resonance. Structure of some typical molecules. Intermolecular bonds. States of aggregation and changes of state. Gaseous, liquid and solid state. Solutions and their colligative properties. Balance between phases and phase rules. Le Chatelier's principle. Basics of thermodynamics. Concept of balance. Principles of thermodynamics. Some thermodynamic functions. Thermochemistry. Chemical reactions and equilibria. Thermodynamic criteria for spontaneity and equilibrium in chemical transformations. Mass action law. Factors that influence the position of equilibrium. Electrolytic dissociation. Electrolytes and their properties in solution. Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Titulations. Indicators. Solubility. Solubility equilibria and factors that influence them. Partition equilibria. Electrochemical reactions. Redox reactions. Potentials, normal potentials, electromotive force, semi-elements, batteries, Nernst equation. Various types of electrolysis. Elements of kinetics. Speed, order, molecularity of a reaction, kinetic constant and its dependence on temperature. Arrhenius equation, activation energy. Basic notes on the theory of collisions and activated complexes. Catalysis. Outline of inorganic chemistry. Systematic nomenclature. Typical elements and their main compounds. Stoichiometry exercises linked to the course. Notes on calculation methods. Exponential notation of numbers and relative elementary operations. Experimental measures and significant-figures. Logarithms. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Concept of mole. Chemical formulas. Law of definite proportions, law of multiple proportions, law of combination weights. Chemical equations and their quantitative significance. Balance of chemical equations. Oxidation number. Redox reactions and their balance. Equivalent weight of combination, neutralization and redox. Quantitative relationships between substances participating in a reaction. The solutions. Concentration and its units: molarity, normality, molality, mole fraction, weight percent, volume percent. Dilution and mixing of solutions. Density. Volumetric analysis. Titled solutions. The gaseous state: units relating to volume, pressure and temperature. The laws of ideal gases: Boyle's law, Charles's law, Gay-Lussac's law. Avogadro's principle. Equation of state of ideal gases. Density. Relative density. Gas mixtures. Partial pressures. Dalton's law. Colligative properties. Colligative properties of non-electrolyte solutions: vapor pressure, Raoult's law, ebullioscope rise and cryoscopic lowering, osmotic pressure. Electrolytic dissociation.

A basic knowledge of the main concepts learned during the course of Maths. There are no prerequisites.

Per la teoria : - M. Schiavello, L. Palmisano “Fondamenti di Chimica” EdiSES - R. H. Petrucci et al. “ Chimica Generale” Piccin - F.Cacace, U. Croatto “Istituzioni di Chimica” La Sapienza Editrice - Paolo Silvestroni «Chimica generale», Quinta edizione, Zanichelli Per le esercitazioni: - F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore Roma

Course attendance is recommended.

The final evaluation consists of a written test with 3 questions which, if passed, admits to the oral test.

The course is based on lectures and stoichiometry exercises in the presence; in-depth information, clarifications, review can also be carried out in mixed mode (in person and remotely).

The course provides fundamental knowledge of general and inorganic chemistry, with particular attention to the theoretical, experimental, and quantitative aspects necessary for understanding chemical phenomena. The course is structured into a theoretical part and numerical stoichiometry exercises that are closely integrated. CONTENT ORGANIZATION: Fundamentals of chemistry and atomic structure, Chemical bonding and molecular structure, States of matter and solution properties, Chemical thermodynamics, Chemical equilibrium, Equilibria in aqueous solution, Electrochemistry, Chemical kinetics, Descriptive inorganic chemistry. Total hours of lectures and exercises: 80 hours (corresponding to 8 CFU)

To successfully undertake the General and Inorganic Chemistry course, it is essential that students possess: • Basic knowledge of mathematics: ability to manipulate algebraic equations, solve systems of linear equations, use logarithms and exponentials, work with proportions and percentages • Basic knowledge of physics: fundamental concepts of mechanics (energy, work, force), elementary thermodynamics (temperature, heat, energy), basic electromagnetism (electric charge, electric field) • Logical-deductive reasoning skills and systematic quantitative problem-solving abilities • Knowledge of the International System of Units and ability to perform conversions between different units It is advisable to possess: • Familiarity with scientific notation and significant figures • Elementary knowledge of the structure of matter acquired in secondary school Notes on prerequisites: No prerequisites are required

- M. Speranza, A. Filippi “Le basi della Chimica” - Edizioni A.L.E. - Roma - M. Aschi, A. Filippi “Stechiometria - Chimica Generale Attraverso gli Esercizi” - Edizioni A.L.E. - Roma - M. Speranza, A. Filippi, M. Crucianelli "L’esame di Chimica Generale" - Edizioni A.L.E. – Roma

The course has the following organization: • resolution of numerical problems in the classroom The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher.

Attendance requirements Attendance at lectures and exercises of the General and Inorganic Chemistry course is not mandatory. However, attendance is strongly recommended because: • It facilitates better understanding of topics through direct explanation by the instructor and classroom interaction • It allows participation in guided numerical exercises, fundamental for acquiring the skills necessary to solve stoichiometric problems • It enables students to benefit from active learning activities and discussions with peers • It allows direct comparison with the instructor for immediate clarification of doubts and difficulties • It helps maintain a constant rhythm in study and learning

Learning assessment methods The final examination aims to verify the achievement of the expected learning outcomes, assessing the acquisition of fundamental theoretical knowledge of general and inorganic chemistry and the ability to apply it in solving quantitative problems. Type of examination: The learning assessment includes a written exam followed by an oral interview. 1. Written examination (mandatory) Objective: To verify the student's ability to apply acquired knowledge in solving quantitative stoichiometry problems and to answer theoretical questions. Exam composition: • Numerical stoichiometry exercises (3 exercises): stoichiometric calculations, reaction balancing, solution calculations, ideal gases, chemical equilibria, pH, electrochemistry, colligative properties Administration method: Written exam in person Duration: 1.5 hours Grading: The written exam is graded out of thirty. Passing the written exam is a necessary condition to access the oral exam. Written exam evaluation criteria: • Correctness of the solution procedure and numerical result (exercises) • Correct application of formulas and units of measurement • Appropriate use of significant figures • Clarity of exposition and logical organization of the answer (theoretical questions) • Correctness and completeness of theoretical content • Appropriate use of scientific language and chemical symbols 2. Oral examination (mandatory) Objective: To deepen and integrate the verification of theoretical knowledge, evaluate critical reasoning ability, scientific language proficiency, and ability to connect different program topics. Administration method: Oral interview in person Duration: Approximately 40-50 minutes Content: The oral interview covers all program topics. The student is asked questions designed to verify: • In-depth understanding of theoretical principles of general chemistry • Ability to describe and explain chemical phenomena • Ability to correlate molecular structure and physicochemical properties • Ability to apply thermodynamic and kinetic principles • Knowledge of chemical nomenclature • Ability to connect different topics critically and thoughtfully Oral exam evaluation criteria: • In-depth knowledge and understanding of topics • Ability to connect different program topics • Language proficiency and correct use of scientific terminology • Critical reasoning and analytical ability • Clarity of exposition Final grade The final grade (expressed out of thirty) takes into account both examinations and is determined considering: • Written exam result (weight: 40%) • Oral exam result (weight: 60%) The final grade may vary from the written exam grade based on the quality of the oral performance. The final grade is communicated at the end of the oral exam. Honors (cum laude) are awarded to students who have demonstrated: • Excellent mastery of all program topics • Capacity for critical and independent connection between different concepts • Particular clarity of exposition and rigor in the use of scientific language • Excellence in both written and oral examinations Students with learning disabilities Students with a diagnosis of Specific Learning Disorder (SLD) or certified disability may request the use of compensatory tools and/or dispensatory measures during examinations, upon presentation of necessary documentation to the instructor and the University Inclusion Service (SASD). International incoming mobility students International incoming mobility students may take the exam in English, upon notification to the instructor at least 15 days before the exam date. The program and assessment methods remain unchanged. Notes: • Non-attending students follow the same assessment methods as attending students • For exam session dates, refer to the calendar published on the Study Program website • Exam registration is mandatory and must be done through the Infostud system Rationale for assessment choices with respect to expected learning outcomes: The combination of written and oral examinations allows for a complete and integrated verification of all Dublin Descriptors: • The written exam primarily verifies the ability to apply knowledge (DD2) through solving quantitative problems and the ability to communicate in written form (DD4) • The oral exam verifies knowledge and understanding (DD1), making judgments (DD3), oral communication skills (DD4), and learning ability (DD5) through questions requiring connections, critical analysis, and synthesis of content

Organization of teaching activities The course consists of 8 CFU divided into theoretical lessons and numerical exercises that are closely integrated. Delivery mode: In-person teaching Teaching methodologies adopted: The course adopts a combination of different teaching methodologies aimed at achieving the expected learning outcomes: 1. Lectures Lectures are dedicated to the systematic presentation of the theoretical contents of the course. During lectures: • The fundamental principles of general and inorganic chemistry are illustrated • Models and theories are presented with multimedia support (presentations, animations, videos) • Applied examples are discussed to connect theory and practice • Critical reflection points on chemical phenomena are proposed • Moments of interaction with students are fostered through questions and guided discussions 2. Numerical stoichiometry exercises Exercises are closely integrated with theoretical lessons and aim to develop the ability to apply knowledge through guided resolution of quantitative problems. During exercises: • Systematic problem-solving methods are illustrated • Exercises of increasing difficulty are solved with detailed explanation of the procedure • Students are encouraged to actively participate by proposing solution strategies • Guidance is provided on common errors and strategies to avoid them • Specific moments are dedicated to clarifying doubts and difficulties 3. Active learning During lessons, active learning techniques are integrated such as: • Problem-based learning: presentation of real chemical problems to be solved by applying studied concepts • Peer instruction: moments of peer discussion on questions posed by the instructor • Just-in-time teaching: use of brief tests or preliminary questions to identify student difficulties and adapt the lesson accordingly 4. Use of online support tools The course uses the Moodle platform to: • Share teaching materials (lecture slides, solved exercises, supplementary material) • Provide self-assessment exercises with automatic feedback • Communicate with students (notices, schedule changes, additional materials) • Promote interaction by receiving students for questions and clarifications 5. Support materials Students are provided with: • Lecture slides in PDF format • Collection of solved and commented exercises • Proposed exercises with solutions for self-assessment • Links to online resources (simulations, educational videos, interactive applets) Consistency between teaching methodologies and expected learning outcomes: The teaching methodologies adopted are designed to facilitate the achievement of learning outcomes through: • Lectures develop knowledge and understanding (DD1) by providing a systematic and in-depth presentation of theoretical content • Numerical exercises develop the ability to apply knowledge (DD2) through systematic practice of solving quantitative problems • Active learning techniques foster making judgments (DD3) by stimulating critical thinking and problem analysis • Classroom discussion and use of guided questions develop communication skills (DD4) by encouraging students to express scientific concepts with appropriate language • Use of the Moodle platform and self-assessment materials support autonomous learning ability (DD5) by providing tools for individual study and progress monitoring Time organization: Lessons are held according to the Study Program's academic calendar. The distribution of topics throughout the semester is organized to ensure: • Logical and gradual progression of content • Alternation between theoretical topics and practical exercises • Review and consolidation moments before intermediate assessments • Adequate time for assimilation of more complex concepts The detailed program with topics and reference text is available in Field 9 - Programming. Activities for non-attending students: Non-attending students have access to all teaching materials through the Moodle platform and can contact the instructor via email for clarifications. The exam program and assessment methods are identical for attending and non-attending students. However, attendance at lessons is recommended, particularly at numerical exercises, to acquire better mastery of problem-solving techniques. Student office hours: The instructor receives students by appointment (to be arranged via email).