GENERAL AND INORGANIC CHEMISTRY

Single discipline educational activity

Course Sheet

Course code:

A004478

Academic Year of enrolment:

2019/2020

Academic Year of provision:

2019/2020

Type of Course:

Basic

Degree:

5-year Single Cycle Master's Degree Programme in PHARMACY

Disciplinary Sector:

General and Inorganic Chemistry

Language:

Italian

Grouping type:

Credits:

Programme Year:

Cycle:

Single Annual Cycle

Hours of classroom activity:

Hours of individual study:

204

No advanced knowledge/skills of the subject is required but the basic scientific skills achieved at the end of the upper secondary school and required for enrollment in the Study Program are sufficient.

No specific knowledge of the subject is required but the basic scientific knowledge acquired in the upper secondary school programs and required for enrollment in the CdS.

It is imperative to follow the basic safety course in order to access the educational laboratories. If the student has not had the opportunity to follow the basic course for safety (e.g. due to enrollment in the degree program in the advanced semester), he must contact the teacher specifically to agree on the recovery of the basic course for safety.

Educational Goals

EDUCATIONAL OBJECTIVES: the course aims to provide students with the fundamentals of General and Inorganic Chemistry, that is, the set of notions essential for understanding the subsequent teachings of the Chemical Sciences of the degree course in Pharmacy. The basic concepts of the structure of matter, its properties and transformations will be illustrated and knowledge will be provided for the resolution of stoichiometry problems and simple practical problems, in agreement with the specific objectives of the CdS reported in the SUA-RAD sheet.

KNOWLEDGE AND UNDERSTANDING: At the end of the course the student will have acquired the basic theoretical and practical notions of general chemistry, such as the relationship between structure and properties of chemical compounds, the energetic aspects of chemical transformations and physical and chemical balances, with particular attention to those in aqueous systems. These skills are preparatory to the study of chemistry applied to life sciences, a topic dealt with in the other courses of the degree course.

ABILITY TO APPLY KNOWLEDGE AND UNDERSTANDING: The course helps to create the chemistry skills that are fundamental to the pharmaceutical sciences, consistently with the professional profile of the CdS and with the employment opportunities reported in the SUA-RAD sheet.

AUTONOMY OF JUDGMENT: At the end of the course the student should be able to manage the information in his possession to analyze all the processes involved in a chemical transformation and determine how to solve simple stoichiometric calculus problems that can find application in the pharmaceutical sciences.

COMMUNICATION SKILLS: At the end of the course the student should be able to clearly and completely describe the concepts addressed during the course, be able to connect the different topics of chemistry and illustrate the processes involved in a reaction.

LEARNING SKILLS: At the end of the course the student should be able to deepen independently the topics covered and connect the knowledge acquired in this course to that required in the subsequent degree course study courses.

Content

-Atomic structure and periodic properties
-Chemical bond
-Stoichiometry
-States of aggregation of matter: gas and condensed phases
-Chemical thermodynamics
-Chemical equilibria
-Solutions: properties
-Chemical equilibria in aqueous solution
-Elements of electrochemistry
-Chemical kinetics
-Elements of nuclear chemistry
-Laboratory safety course

Extended Syllabus

Topic 1 - INTRODUCTION TO CHEMISTRY. Matter, structure and classification.

Topic 2 - ATOMIC STRUCTURE AND PERIODIC PROPERTIES. Introduction to Atomic Theory. The Heisenberg uncertainty principle, the Schrödinger wave equation and the structure of the hydrogen atom. Quantum numbers. Atomic orbitals and their energy levels. The Aufbau principle. Polyelectronics atoms and their electronic configuration. Relationship between electronic configurations of the elements and their properties. Periodic table. Periodic properties of the elements: ionization energy, atomic radius, mean energy of valence electrons. The concept of mole, atomic and molecular mass. Balance of reactions. Limiting reagent.

Topic 3 - CHEMICAL BOND. The chemical bond: ionic, covalent. Valence bond theory. Hybridization and resonance. Structures of simple molecules; diatomic homonuclear and heteronuclear molecules. Description of the structure of simple polyatomic molecules of fundamental importance. Concept of oxidation number and formal charge. Length, angle and bond strength. Introduction to the theory of molecular orbitals. Metal bond (outline); examples of structure of some condensed phases (ionic, covalent, molecular solids). Intermolecular forces: ion-dipole, dipole-dipole, interactions between induced dipoles (van der Waals interactions and London dispersion forces). The hydrogen bond: nature and effect on the structure of some condensed phases.

Topic 4 - THERMODYNAMICS. Energy, work, heat and their implications in chemistry. First law of thermodynamics and enthalpy. Enthalpy (standard) of reaction, formation and bond. Hess' law. Second law of thermodynamics and spontaneity of chemical-physical transformations.

Topic 5 - GASES. The gaseous state. Pressure and pressure measurement unit. Boyle, Charles, Avogadro's law. General equation for ideal gases PV = nRT. Dalton's law. Real gases. van der Waals equation.

Topic 6 - CONDENSED STATES. Condensed phases and phase transitions. Evaporation, melting, sublimation. Normal melting point and normal boiling point. Air condensation / liquefaction. Critical phenomena. Critical temperature. State diagrams. Water state diagram. State-of-the-art thermodynamics.

Topic 7-SOLUTIONS - PROPERTIES. Solutions. Solubility. Ways of expressing concentration: molarity, molality, weight / volume percentage, weight / weight percentage, parts per million. Dilution law. Solubility of gases; Henry's law. Colligative properties of the solutions: vapor pressure lowering, ebullioscopic elevation, cryoscopic lowering, osmosis and osmotic pressure. Effect of electrolyte upon colligative properties.

Topic 8 - CHEMICAL EQUILIBRIUM. Homogeneous mixtures. Solutions. Solubility. Concentration measurement. Molarity, molality. Dilution. Raoult's laws for the non-volatile and volatile solute. Solubility of gases; Henry's law. Dependence of solubility on the nature of solute, solvent and temperature. Colligative properties of solutions. Osmosis and osmotic pressure. Fractional distillation. Law of mass action. Equilibrium constant. Reaction quotient. Effect of temperature on equilibrium. Le Chatelier's principle. Relationship between free energy and equilibrium constants (Kp, Kc). Chemical equilibrium in homogeneous and heterogeneous gas phase.

Topic 9 - CHEMICAL EQUILIBRIUM IN AQUEOUS SOLUTION. Homogeneous equilibria in aqueous solution. Acid-base theories and applications. Definition of pH. Autoionization of water and Kw. Strength of acids and bases. pH, pOH and pK scales. pH calculation. Relationship between structure and acidic or basic strength. Saline hydrolysis. Buffer solutions. Solubility product and solubility equilibria. Enthalpy of solution and ions hydration, their relationship with the solubility of ionic compounds.

Topic 10-ELECTROCHEMISTRY. Oxidation-reduction reactions. Balancing of redox reactions. Electrode potentials and electromotive force of an electrochemical cell. Standard potentials. Standard electromotive force of a galvanic cell. Nernst's law and its thermodynamic meaning. Some examples of batteries. Electrolysis. Stoichiometry of electrolysis: Faraday's law.

Topic 11-ELEMENTS OF NUCLEAR CHEMISTRY. Mass defect. Radionuclides and nuclear stability. Natural decay. Radioactive activity. Dating with the C14. Nuclear Fission. Radioactivity in everyday life and biomedical aspects.

Topic 12-CHEMICAL KINETICS. The reaction rate. Concentration and time. Reaction mechanisms. Models of reactions.

Recommended Bibliography

To support the lectures and the material provided by the teacher (by Moodle), any text of General Chemistry at university level in Italian or English is suitable.

For the theory one of the following texts is suggested:
- Fondamenti di Chimica, IV edizione; Brown, LeMay, Bursten, Murphy, Woodward, Stoltzfus; EdiSES; 2018
- Chimica, VI edizione; Kotz, Trichel, Townsend, Treichel; EdiSES; 2018
- Fondamenti di Chimica Generale, II edizione; Atkins, Jones, Laverman; Zanichelli; 2018

As exercise book:
- Esercizi di Chimica Generale; Alessandro Del Zotto; EdiSES; 2019

Methods of Provision

Conventional

Teaching Methods

The course is structured in theoretical lessons and numerical exercises in stoichiometry (at least 20% of the total hours), all delivered with frontal lessons.
In general, the teaching methods comply with the indications of the PQA guidelines.

Assessment Methods

The overall score of the exam of the integrated course is given by a mark expressed in thirtieths
The exam is divided into a written test which, if passed (minimum mark required: 18/30), gives access to the oral test.
In place of the written test, two ongoing tests are scheduled during the course; even the exemptions are considered outdated if a vote of at least 18/30 is obtained in each. For on-going tests, the arithmetic average of the marks is considered as the final mark of the written test.
The written tests consist of 4-6 numerical exercises to be carried out and possibly multiple choice theoretical questions. The oral exam, which starts from the discussion of the written tests, consists of questions on theoretical topics (example: the structure of molecules, energetic aspects of chemical processes, equilibria ...) and the approach to solve numerical problems.
The final mark expressed in thirtieths is the weighted average of the marks of the written test (60% of the final mark) and the oral one (40% of the final mark). The completeness and correctness of information, the ability to represent the structures of molecules, graphs and formulas to describe chemical and physical transformations are assessed.
The oral exam must be taken in the same session as the written one or in the following one.
Textbooks or notes are not allowed.

The examination of the laboratory safety course is independent from that of General and Inorganic Chemistry.

If the health emergency due to Covid-19 prevents the taking of exams in the presence with the written and oral test, the exam will be carried out remotely only by means of an oral test, following the guidelines established by the University.
For students who have passed the first partial written test, the topics already dealt with and the marks obtained will be taken into account.

Assessment:

Final Mark

Programme of Educational Activities

Start date of teaching period:

Monday, October 21, 2019

End date of teaching period:

Friday, June 5, 2020

Other Information

Information on the teacher and office hours can be found on the teacher page on the university portal.

Within the general chemistry course, a course (12 hours total, professor Flora Boroni) on laboratory safety will be held. At the end of this course there will be an exam to check eligibility.
These are the topics:
- lesson 1: regulations and sic procedures
- lesson 2: part 2 procedures in case of emergency in the lab and part 1 chemical risk
- lesson 3: 2nd part chemical risk and DPC
- lesson 4: biological risk and DPC
- lesson 5: dpi
- lesson 6: final test

Attendance to the course is mandatory as per the CdS regulation

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