Ateneo - UPO

The module will deal with stoichiometry calculations strategies and problem solving related to the basic concepts illustrated the General and Inorganic Chemistry module: chemical nomenclature of inorganic compounds, balancing of chemical equations, chemistry laws calculations, solutions and their properties, chemical equilibria, acids and bases, electrochemistry.

R. Breschi e A. Massagli, “Stechiometria”, Edizioni ETS; M. Bruschi, “Stechiometria e Laboratorio di Chimica Generale”, Pearson; P. Michelin Lausarot e G. A. Vaglio, “Fondamenti di Stechiometria”, Piccin; Caselli, Rizzato, Tessore, Stechiometria dal testo di M. Freni e A. Sacco, EDISES; R. Morassi, G.P. Speroni, “Il laboratorio Chimico”, Piccin; Slowinski, Wolsey, Masterton, “Laboratorio di Chimica”, Piccin.

Background and skills: the main objective of the module is to provide the student with the necessary basic knowledge and tools to develop an appropriate problem-solving ability applied to stoichiometry problems related to General and Inorganic Chemistry. In particular, the module intends to guide the student toward a fully independent critical attitude in problem-solving, starting from the recognition of the dependent and independent variables, the design of the resolution strategy and finally, in the critical discussion and validation of the results. These skills and competences will be the basis for the successive laboratory course. The module will be developed by slowly increasing the degree of complexity of the proposed stoichiometry problems to include multi-level calculations on different topics, in order to stimulate the development of the capacity to identify the chemical system as a whole. Communications skills: the module will guide the student toward the acquisition and mastering of an appropriate chemical/scientific vocabulary.

No particular prerequisites are expected, save for the basic competences of the TCI test, with particular reference to basic mathematics. 

Classroom lectures, slide shows and guided exercises with open discussion. Students will be encouraged to supplement in-class work with individual homework for a successful fruition of the course.

Students will be encouraged to actively participate to classes and guided through individual or collaborative problem-solving activity in order to stimulate preparation progresses and regularly test them. This approach will also favor the development of the expected specific communication skills. Students with physical disabilities, Learning Disabilities or Special Education Needs can request specific services and tools via the Staff Sviluppo e Coordinamento Carriere e Servizi alle Studentesse e agli Studenti, consulting the University webpage: https://www.uniupo.it/en/services/services-students-physical-or-learning-disabilities Students with disabilities, learning disabilities or special education needs, once they have contacted the University Staff, can refer to the tutor in charge of the course to define the examination modalities, concerning academic aspects.

The final exam will consist in a written test to be performed in 3 h (max). The test will contain 5-8 questions (problems) which will include numerical exercises. Each question (problem) will correspond to a score of 1 to 3 points depending on the complexity. The maximum score attainable is 10 and the minimum score requested to gain access to the General and Inorganic Chemistry module is 6/10. The evaluation and scoring of the test will be primarily based on the capacity of the student to identify the unknown variables of the problem, implement a rational and justified resolution strategy and use the appropriate vocabulary and rigorous chemical symbolism.

The Stoichiometry module is conducted within the framework of the General and Inorganic Chemistry courses and therefore consists of solving, including numerically, basic problems related to topics covered in the theoretical course. The scientific method. Measurements and SI units of measurement. Main units of measurement of interest in chemistry. Conversion factors and exercises. Measurement uncertainty, mean, true value. Accuracy and precision. Significant figures. Classification of compounds, ionic compounds, and nomenclature of ionic compounds. Oxidation number. Molecular compounds, traditional, IUPAC, and Stock nomenclature. Classification and nomenclature of the main inorganic compounds. Mineral acids and bases and their formation reactions. Main salt formation reactions. Empirical formula and molecular formula. Percentage calculations. Balancing non-redox reactions. Reaction yield. Introduction to green chemistry metrics and atom economy calculations. Limiting reactant. Classification of chemical reactions and predicting reaction products for simple reactions. Gas laws: Boyle, Charles, Gay-Lussac, Avogadro. Ideal gas law. Use of the respective equations in stoichiometric calculations. Gas density. Gas mixtures: average molar mass and mole fraction. Dalton's and Amagat's laws. Weight, volume, and mole percentages. The molar volume in stoichiometric calculations. Concentration of solutions. Weight percentage, weight-by-volume percentage, volume percentage. Molarity, molality. Concept of equivalent and normality. Preparation of solutions by weighing and by dilution. Calculating the concentration of solution mixtures. Colligative properties. Boiling point elevation and freezing point depression. Raoult's law and its application to liquid mixtures and solutions of solid solutes. Osmosis and calculation of the osmotic pressure of different solutions in contact. Chemical equilibrium. Law of mass action and its significance. Kc and Kp and their relationship. Reaction quotient. Calculation of K and equilibrium composition. Comparison of Q and K. Properties of the K expression, reverse reactions, stoichiometric multiples, multi-step reactions. Complex equilibria. Validity of approximations. Le Chatelier's principle. Modification of the equilibrium composition by adding a species. Acids and bases. Self-ionization of water and Kw. Calculation of pH and the pH of strong acid and strong base solutions. pH of highly dilute strong acids and bases. Strong acid-strong base titrations and related calculations. Weak acids, acid and base dissociation constants. Calculation of pH, Ka, and Kb. Calculation of the pH of polyprotic acids with one or two partial dissociations. pH of weak acid mixtures. Degree of acid dissociation. Acid and base hydrolysis and pH calculation. Buffer solutions and pH calculation. Henderson-Hasselbalch equation. Calculation of pH for successive additions of acid or base. Heterogeneous equilibria, solubility product, and ionic product. Predicting supersaturation or unsaturation of solutions. Solubility calculation. Solubility and pH. Common-ion effect on salt solubility. Sequestering agents. Redox reactions and their balancing. Balancing in acidic and basic media. Disproportionation reactions. Galvanic cells. Relationship between free energy and potential. Derivation of the Nernst equation. Standard reduction potentials. Electrode potentials under non-standard conditions. Cell diagram. Calculation of cell potential under non-standard conditions. Concentration cells, diagram, and potential calculation under non-equilibrium conditions. Conditions for cell operational termination.

Background knowledge: basic knowledge of general chemistry necessary for the resolution of stoichiometry problems. Competences and skills: ability to apply the acquired knowledge to the correct assignment of chemical nomenclature, balancing of chemical equations, stoichiometry calculations, resolution of problems on gases, solutions, chemical equilibrium, acids and bases and electrochemistry. Independent judgment ability: capability to independently implement the correct resolution strategies, analyze and validate data correctly and draw reliable conclusions. Communication skills: mastering of the appropriate scientific vocabulary and capability to realize a scholar presentation in a concise and clear manner.