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:

Professor and Collaborators:

POMARICO Giuseppe Professor

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.

Educational Goals

LEARNING OUTCOMES: the aims of the course is to provide students with the fundamentals of General and Inorganic Chemistry, that is the set of essential concepts for understanding the subsequent teachings of the degree course in Pharmacy. The basic concepts of the structure of matter, its properties and transformations will be illustrated; these topics for the applications of chemistry in pharmaceutical sciences will be explained also using examples taken from everyday experience. The knowledge for solving stoichiometry problems and simple practical problems will also be provided.

KNOWLEDGE AND UNDERSTANDING: at the end of the course the student must have acquired the basic notions on the relationship between structure and properties of chemical compounds, on the energetic aspects of chemical transformations and on physical and chemical equilibria, with particular attention to equilibria in aqueous systems. The student must also be able to apply the knowledge acquired in this course to other courses of the degree in Pharmacy.

APPLYING KNOWLEDGE AND UNDERSTANDING: at the end of the course the student should be able to apply the acquired knowledge to predict the properties of an element based on its position in the periodic table, to correlate the structure of simple chemical compounds to their properties, to analyze the energy contributions involved in a chemical reaction and to be able to solve stoichiometry problems with a different level of difficulty inherent in the study of general chemistry applied to pharmaceutical sciences.

MAKING JUDGEMENTS: at the end of the course the student should be able to manage the information in his / her possession to analyze all the processes involved in a chemical transformation and to determine how to solve simple stoichiometric calculation problems that can find application in 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, to be able to link the different topics of chemistry and to illustrate all the processes involved in a reaction.

LEARNING SKILLS: at the end of the course the student should be able to study the topics covered in an autonomous way and to link the knowledge acquired in this course to those required in the subsequent degree courses.

Content

ATOMIC STRUCTURE, PERIODIC PROPERTIES, AND CHEMICAL BONDING
BULK MATTER
THERMODYNAMICS
STOCHIOMETRY
PHYSICAL EQUILIBRIUM
EQUILIBRIUM IN AQUEOUS SOLUTION
KINETICS
ELETROCHEMISTRY
FUNDAMENTALS OF NUCLEAR CHEMISTRY
MAIN GROUP ELEMENTS
INORGANIC CHEMISTRY APPLIED TO MEDiCINE AND PHARMACEUTIC

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.

Argomento 4-I GAS. Lo stato gassoso. Pressione e unità di misura della pressione. Leggi di Boyle, Charles, Avogadro. Equazione generale per i gas ideali PV=nRT. Legge di Dalton. Gas reali. Equazione di van der Waals.

Argomento 5-TERMODINAMICA CHIMICA. Energia, lavoro, calore e loro risvolti in chimica. Primo principio della termodinamica e entalpia. Entalpia (standard) di reazione, di formazione e di legame. Legge di Hess. Secondo principio della termodinamica e spontaneità̀ delle trasformazioni chimico-fisiche.

Argomento 6-STATI AGGREGATI. Fasi condensate e transizioni di fase. Evaporazione, fusione, sublimazione. Punto di fusione normale e punto di ebollizione normale. Condensazione/liquefazione degli aeriformi. Fenomeni critici. Temperatura critica. Diagrammi di stato. Diagramma di stato dell’acqua. Termodinamica dei passaggi di stato.

Topic 4-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 5 - 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 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 - 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 8 - 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 9-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 10-CHEMICAL KINETICS. The reaction rate. Concentration and time. Reaction mechanisms. Models of reactions.

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 - MAIN GROUP ELEMENTS CHEMISTRY AND INORGANIC CHEMISTRY IN MEDICAL AND PHARMACEUTICAL FIELD. Hydrogen, alkaline metals (sodium and potassium), alkaline earth metals (calcium and magnesium), nitrogen, chalcogens (oxygen and sulfur), halogens (fluorine and chlorine).

Recommended Bibliography

To support the lectures and the material provided by the teacher, 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 stoichiometry numerical exercises, all given by lectures.

Assessment Methods

The exam is made by by a written test mainly concerning the concepts of stoichiometry which, if passed (minimum mark required: 18/30), gives access to the oral test (more focused on theoretical concepts).
There are also midterm tests (in number 2 or 3) that will be made during the course to replace the written test; also these tests are considered to be passed if a mark of at least 18/30 is obtained in each test. For the midterm tests, the average grade is considered as the final grade of the written test.
The written test consists of 4-6 numerical exercises to solve and multiple choice theoretical questions.
Oral exam consists of theoretical questions (for example: structure of molecules, chemical equilibrium, energetic aspects of chemical reactions) and how to solve numerical problems.
The final grade, expressed in thirtieths, is assigned according to the result obtained in the written test (60% of the final grade) and the oral one (40% of the final grade). The completeness and correctness of the information, the ability to represent the structures of molecules, graphs and formulas to describe chemical and physical transformations are evaluated.
The oral exam must be taken in the same session as the written exam.
Textbook and notes are not allowed.

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

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