CHIMICA GENERALE ED INORGANICA

EXPECTED LEARNING OUTCOMES

The aim of the course is to provide the student with the knowledge of the basics of chemistry and with theunderstanding of related subjects developed in other courses of the Degree Program.

The student acquires the disciplinary and methodological know-how necessary to the basic technical and practicalproblem solving which he/she will use in the laboratory and in the subsequent courses.

The student acquires the ability to know and understand the General and Inorganic Chemistry in order to correctlywrite the most common chemical compounds, balance chemical reactions, calculate the concentration ofsolutions, describe the concept of chemical equilibrium and the pH of a solution.

The student develops critical ability in exercises solving, ability to communicate what was learnt, ability tocontinue the study in an autonomous way and critical abilities.

The course comprises lectures and interactive stoichiometry sessions involving guided problem-solving and discussion. Lectures provide students with the fundamental principles of general and inorganic chemistry, laying the foundations for subsequent studies in pharmaceutical sciences. Problem-solving sessions enable students to apply theoretical concepts, develop calculation and reasoning skills, and assess their understanding through interaction with the lecturer.

If the course is delivered in blended or remote mode, appropriate adjustments may be made to the

REQUIRED PREREQUISITES

School knowledge of arithmetic and algebra, such as operations with rational numbers (real numbers). Solving oflinear and quadratic equations, school knowledge of physics, such as vectors, speed and energy.

ATTENDANCE OF LESSONS

Attendance is mandatory, as required by the degree programme regulations. Absences may not exceed 30% of the total teaching hours, across all modes of delivery. https://www.dsf.unict.it/it/corsi/l-29_sfa/regolamento-didattico

DETAILED COURSE CONTENT

1) Introduction - The 4 fundamental strenghts, matter and energy, states of matter* , homogeneous andheterogeneous systems, elements*, compounds* and mixtures*

.

2) Fundamental Chemical Laws -Lavoisier's law of conservation of the mass , Proust's Law of definiteproportions*, Daltom atomic theory, Dalton's Law of multiple proportions, Avogadro's Law, general knowledge onthe atom, the atomic number* and the mass number*, isotopes* , a.m.u.* , atomic mass*, molecular mass*, mole*,weight percent composition.

3) Structure of matter – Rutherford, Bohr and Sommerfeld's atomic models. Theory of atomic orbitals *, Quantum numbers*, interpretation of the atom as a wave, atomic orbitals , Pauli's principle*, Hund's rule*, Heisenberg'suncertainty principle.

4) Periodic System - Periodicity and electron configuration*, ionization potential*, electronaffinity*, electronegativity*.

5) Chemical bond* - ionic bond, covalent bond, dative bond, Lewis structures, valence, valence bond theory,orbital hybridization. Intermolecular bonds: hydrogen bond and Van der Waals forces.

6) Chemical nomenclature* -Chemical compounds, valence and oxidation number, chemical reactions and theirbalancing, redox reactions.

7) Gas phase - Partial pressures*, Dalton's Law*, Ideal gas law* , real gases.

8) Liquid phase - Properties, viscosity, surface tension, vapor pressure*

9) Phase change - Phase Diagram for H2O * and CO2.

10) Solutions*- Molarity, normality, mole fraction, molality, mass percentage, density, vapor pressure, Raoult's law, colligative properties, electrolytes, degree of dissociation, Van’t Hoff coefficient.

11) Chemical equilibrium* - Law of mass action, equilibrium constant, relation between Kp and Kc, temperaturedependence of the equilibrium constant, factors which influence the chemical equilibrium. Definition ofexothermic, endothermic reaction and enthalpy change (H), spontaneity of a chemical equilibrium and free energy change (G).

12) Acids and bases* - Definition according to Arrhenius, Bronsted and Lowry, Lewis, acids and bases strenght,dissociation constant, amphoteric electrolytes, ion product of water, acidity, alkalinity and pH calculations, pHindicators.

13) Hydrolysis of salts - Hydrolysis constant, hydrolysis pH*, buffer solutions*, titrations strong-acid strong-base*,titrations weak-acid strong-base*, solubility and solubility product*.

14) Inorganic Chemistry - Chemistry of the main elements from I° to VII° group*, general properties of groups andperiods* , chemical-physical properties of the main elements and of their most important compounds.

* fundamental topics to pass the exam.

According to Article 12 of the University Teaching Regulations (RDA), “University Credits (CFU)”, the standard workload of 25 hours of total student effort corresponding to one credit may comprise:

a) 7 hours of lectures or equivalent teaching activities, with the remaining hours devoted to independent study;

b) a minimum of 12 and a maximum of 15 hours of classroom exercises or equivalent supervised activities (laboratory sessions), with the remaining hours devoted to independent study and consolidation of learning.

TEXTBOOK INFORMATION

General and Inorganic Chemistry

1. P. Silvestroni - Fondamenti di chimica - undicesima edizione - CEA

2. P.W. Atkins, L. Jones, L. Laverman - Fondamenti di chimica generale – Seconda edizione - Zanichelli

3. J.C. Kotz, P.M. Treichel, J.R. Townsed - Chimica - quinta edizione - Edises

4. I. Bertini, C. Luchinat, F. Mani, E. Ravera - Chimica, struttura, proprietà e trasformazioni della materia- CEA

5. P. M. Lausarot, G.A. Vaglio - Stechiometria Guida alla soluzione di problemi di chimica- Piccin Esercitazioni 

6. Slide projected at the lectures.

LEARNING ASSESSMENT PROCEDURES

Separate written and oral exam.

Students will have to take a written test and will have 2 hours to complete 7 exercises. Passing the written test(mark greater than or equal to 18/30) is binding for access to the oral exam. 

For the written and oral tests, students must bring a valid identity document.

The use of mobile phones isabsolutely NOT allowed during the tests, not even in calculation mode.

Assessment criteria

The final examination will be assessed using equally weighted indicators, consistent with the intended learning outcomes (Dublin Descriptors). The final grade therefore takes into account the following factors.

Quality of the knowledge, skills and competences acquired and/or demonstrated:

a) Appropriateness, accuracy and relevance of knowledge;
b) Appropriateness, accuracy and relevance of skills;
c) Appropriateness, accuracy and relevance of competences.

Presentation skills:

a) Ability to communicate clearly;
b) Appropriate use of subject-specific terminology;
c) Logical reasoning and coherence in connecting topics;
d) Ability to identify connections between different topics and integrate them into a coherent overall framework, ensuring a well-structured, organised and logically connected presentation;
e) Ability to summarise, including through subject-specific notation and graphical representations of concepts, such as formulae, diagrams and equations.

Interpersonal skills:

a) Willingness to engage in discussion and interact with the examiner during the oral examination.

Personal qualities:

a) Critical thinking;
b) Self-assessment skills;
c) Problem-solving skills;
d) Decision-making skills.

Based on the above criteria, performance may be assessed as follows:

Fail

Knowledge and understanding of the subject: significant gaps and inaccuracies.
Analysis and synthesis: negligible ability, with frequent generalisations.
Use of references: entirely inappropriate.

Grade: 18–20

Knowledge and understanding of the subject: very limited, with evident inaccuracies.
Analysis and synthesis: barely sufficient.
Use of references: barely appropriate.

Grade: 21–23

Knowledge and understanding of the subject: slightly above the minimum required standard.
Analysis and synthesis: satisfactory ability, with logical and coherent reasoning.
Use of references: use of standard references.

Grade: 24–26

Knowledge and understanding of the subject: good.
Analysis and synthesis: good ability, with coherent presentation of topics.
Use of references: use of standard references.

Grade: 27–29

Knowledge and understanding of the subject: very good.
Analysis and synthesis: strong ability.
Use of references: evidence of further study of the topics.

Grade: 30–30 with honours

Knowledge and understanding of the subject: excellent.
Analysis and synthesis: strong ability.
Use of references: evidence of substantial in-depth study.

Assessment may also be conducted remotely, should circumstances require it.

Exam dates are published on the degree programme website.: https://www.dsf.unict.it/it/corsi/l-
29_sfa/calendario-esami

To ensure equal opportunities and in compliance with current laws, interested students may request a
personal interview in order to plan any compensatory and/or dispensatory measures based on
educational objectives and specific needs.
Students can also contact the CInAP (Centro per l’integrazione Attiva e Partecipata — Servizi per le
Disabilità e/o i DSA, (https://www.cinap.unict.it/content/referenti) and referring teacher (prof.ssa
Santina Chiechio email: santina.chiechio@unict.it) within of department.

EXAMPLES OF FREQUENTLY ASKED QUESTIONS AND / OR EXERCISES

Written exam:

Calculation of the pH of a solution of acids and bases.

Balancing of a redox reaction.

Calculation of colligative properties.

Calculation of the concentration of the solute in a solution.

Type of chemical bond in compounds.

Electron configuration of atoms and ions.

Molecular formula and Lewis structure of chemical compounds.

Oral exam:

Theory of acids and bases.

Equilibrium in solution (acid, base, hydrolysis).

Definition of buffer solutions, buffering capacity.

Redox reactions.

Chemical equilibrium and equilibrium constant.

Factors affecting the chemical equilibrium.

Metallic and non-metallic character of the elements.

Atomic orbitals.

Quantum numbers.