GENERAL INORGANIC AND ORGANIC CHEMISTRY 3

Module GENERAL AND INORGANIC CHEMISTRY

Acquisition of key concepts in general and inorganic chemistry, and stoichiometry. The course is structured to provide a sound understanding of basic chemistry (inorganic chemistry and stoichiometry) and is divided into a theoretical section and a practical section consisting of exercises aimed at solving chemistry problems (knowledge and understanding). The aim of the course is to develop the reasoning skills required to approach the study of chemical phenomena using analytical and numerical methods (applying knowledge and understanding). By the end of the course, students should be able to exercise independent judgement: the ability to devise their own numerical exercises (making judgements) on specific topics.

In particular:

This course is primarily theoretical and includes many numerical exercises.

The specific

learning objectives

of this course are:

To understand atomic structure;

to understand the mechanisms of chemical bond formation;

to understand chemical interactions in solids and liquids and to understand the equations of state for gases; to understand the main thermodynamic and kinetic parameters involved in chemical reactions; to assess the conditions of chemical equilibrium;

to quantitatively determine equilibria in gases and aqueous solutions;

to discuss all the proposed activities using the scientific method and appropriate language.

Acquire the ability to set and correctly solve exercises on various types of chemical reactions

Furthermore, with regard to the so-called

Dublin Descriptors, this course contributes to the acquisition of the following transversal competences:

Knowledge and understanding:

Ability to reason inductively and deductively.

Ability to describe a chemical reaction in qualitative and quantitative terms.

Ability to formulate a problem using appropriate relationships between chemical and physical quantities and to solve it using analytical methods.

Ability to apply knowledge:

Ability to apply the knowledge acquired to describe chemical phenomena, rigorously applying the scientific method.

Ability to perform quantitative calculations of reactants and products in chemical reactions.

Quantitative calculations involving homogeneous solutions, their colligative properties, pH, and electrochemical phenomena.

Independence of judgement:

Ability to think critically.

Ability to identify the most appropriate solutions to chemical problems.

Ability to identify the predictions of a theory or model.

Ability to assess the level of accuracy required in stoichiometric calculations.

Communication skills:

Ability to describe a scientific topic orally, using appropriate language and precise terminology, whilst explaining its rationale and results.

Teaching methods

The course comprises 4+2 CFU, 28 hours of lectures and 24 hours of practical sessions.

Students will be actively involved in numerical exercises at the blackboard

Information for students with disabilities and / or SLD: To guarantee equal opportunities and in compliance with the laws in force, interested students can ask for a personal interview in order to plan any compensatory and / or dispensatory measures, based on the teaching objectives and specifications needs. It is also possible to contact the CInAP contact person (Center for Active and Participatory Integration - Services for Disabilities and / or SLD) of the department

You need to know:

(Essential) quantities, dimensions and units of measurement;

(Important) the basic concepts of chemistry and

chemical symbols, as well as a basic understanding of mathematics and physics.

(Useful) chemical nomenclature.

1. Composition and structure of matter: generalities, mixtures, chemical compounds, atoms, molecules and ions, molecular weight, atomic weight, concept of mole and Avogadro's number;
2. The structure of the atom: generalities, orbitals, ideal construction of atoms: Hund's principle of maximum multiplicity, the Aufbau rule, Pauli's exclusion principle, the periodic system of the elements;
3. Chemical bonding: generalities, valence bond theory, types of bonds: covalent bond (homeopolar, heteropolar), dative or coordination covalent bond, ionic bond, hydrogen bond, notes on molecular hybridization;
4. Chemical reactions: generalities, oxidation number, formation of oxides, anhydrides, acids, bases and salts, nomenclature and balancing, oxidation-reduction and balancing reactions. Moles, equivalents and stoichiometry calculations.
5. The gaseous state: pressure, volume, temperature. The laws of ideal gases (Boyle, Charles, and Gay Lussac) and the equation of state of gases. Avogadro's Law;
6. Condensed states: liquid state;
7. Electrolyte and non-electrolyte solutions: generalities, transition to solution, concentrations: percentage composition, molality, molarity, normality. General information on colligative properties. Electrolytic dissociation;
8. Chemical equilibrium: generalities, law of chemical equilibrium, equilibrium constant, factors influencing chemical equilibrium;
9. Ionic equilibria in solutions: generalities, acid and base according to Arrhenius, Bronsted and Lowy, strength of an acid and a base, ionic product of water, pH, pH indicators, hydrolysis, buffer systems, solubility product;
10. Basics of Chemical Kinetics.
11. Inorganic chemistry of the main elements of the sp.

Assessment Methods

The examination aims to assess the candidate’s overall level of knowledge, their ability to critically analyse the topics studied and to make connections between the various parts of the syllabus. The examination consists of a written paper and an oral examination. The written paper comprises 11 questions relating to the syllabus covered. This paper aims to assess the candidate’s overall level of knowledge. The time allowed for this paper is 75 minutes. The written paper will be deemed passed if the student has correctly answered at least six out of the eleven questions. During the written exam, students may use books, including exercise books, notes, tables, calculators and specific teaching materials, but not mobile phones.

There are no in-course assessments.

Any oral examination will consist of questions relating to the various parts of the syllabus, designed to assess the candidate’s overall level of knowledge.

Criteria for awarding the final mark:

The final mark will be determined in equal measure by the candidate’s demonstrated mastery of qualitative and quantitative arguments, their critical analysis of the topics covered during the course, and their ability to establish connections between the various parts of the syllabus. Finally, the average of the marks obtained in the two assessments – written and oral – will be calculated, and this will constitute the final mark.

The questions listed below are not an exhaustive list but merely a few examples

Formulas of compounds.

The Bohr/Rutherford atomic model.

Atomic orbitals. Quantum numbers.

The periodic table of elements.

Electron configuration of elements.

Periodic properties.

Ionic bonding.

Covalent bond.

Ideal gas laws.

Units of concentration.

Colligative properties.

Factors affecting chemical equilibrium.

pH.

Acid-base theories.

Ampholytes. Hydrolysis. Buffer solutions.