Learning objectives
At the end of the course the students are expected to have acquired knowledge and understanding of General and Inorganic Chemistry concepts that will allow them to interpret the biological phenomena at molecular level.
In particular, with reference to the Dublin Indicators, the student at the end of the course will have pursued and obtained the underreported targets.
Knowledge and understanding: the student will know the fundamental concepts of chemistry necessary to interpret at molecular level the biological phenomena.
Application of knowledge and understanding: the student will be able to apply the techniques learned during the lectures in calculations and will be able to tackle the most common chemical problems.
Communication skills: the student will be able to express using a correct formal language, verbally and in writing, chemical concepts and ideas.
Making judgements: with the intellectual tools provided in the course, the student will be able to use the principles of mass and charge conservation, to predict the molecular shape and the properties of molecules, and to analyse chemical reactions based on thermodynamic and kinetic considerations.
Learning skills: at the end of the course the students should have acquired the basic concepts of chemistry and should be able to study by themselves without problems on advanced level chemistry texts and be able to expand, with a good level of independence, their knoweldge in the field.
Prerequisites
No prior knowledge of chemistry is required.
Basic mathematics prerequisites are expected, such as the use of significant figures, exponential notation, and the ability to solve first- and second-degree equations. Operations involving exponents and logarithms, as well as the ability to read and interpret graphs, are also required.
The mathematical aspects required are reviewed in the appendices of the recommended textbook.
Course unit content
The course is made up of 9 ECTS, 7 of which devoted to the theoretical part and 2 to stoichiometry.
The lectures are divided into four Units:
Unit 1: Atomic-molecular Theory
The chemical tools. Atoms and elements. Compounds and molecules. Chemical reactions: an introduction. Reactions in water solutions. Thermochemistry.
Unit 2: Atomic structure and the chemical bondAtomic and molecular structure. Structure of the atom. Electronic configuration of atoms and periodic properties. Basic concepts on the chemical bond and on the molecular structure. – Further concepts on the chemical bond: orbital hybridization, molecular orbital theory and metallic bond.
Unit 3: Thermodynamics
The states of aggregation: gases and their behaviour. Intermolecular forces: liquids and solids. Solutions and their behaviour. The control of chemical reactions: thermodynamic and kinetic aspects. The principles of thermodynamics and their implications in a chemical context. Spontaneity of the chemical reactions. Enthropy and free energy. Chemical equilibrium. The chemistry of acids and bases. Buffer systems. Precipitation reactions. Thermodynamics of redox reactions. Electrochemistry.
Unit 4: Kinetics
Rates and mechanisms of chemical reactions – Chemistry of the elements and of their compounds: the s and p blocks and the transition elements of biological relevance.
The stoichiometry part includes:
Writing a chemical formula from the name of a compound and vice versa.
Balancing chemical reactions.
The concept of mole and its use.
Redox reactions. Equivalent weight. Normality.
Principles of volumetric analysis.
Equilibria in solution: calculation of the pH of various kinds of solutions.
Buffer solutions.
Hydrolysis.
Full programme
Atomic theory
Atoms and elements - Compounds and molecules - Nomenclature of Inorganic Compounds - Chemical reactions: an overview - Reactions in aqueous solution
Atomic and molecular structure
The structure of the atom - Electronic configuration of atoms and periodicity - Basics on molecular structure and chemical bonding: Lewis and VSEPR theory, VB theory (hybridization) and MO theory (application with homo- and heteronuclear diatomic molecules)
Thermodynamics
States of matter - Gases and their behaviour - Intermolecular forces - Thermodynamics: the principles of thermodynamics and their implications in chemistry - Thermochemistry - The spontaneity of chemical reactions: entropy and Gibbs free energy - Equilibrium: general concepts - The chemistry of weak acids and bases - Buffer solutions - Solubility
Kinetics
Reaction rate - kinetic equations - Reaction order - Arrhenius equation - Activated complex theory - Mechanisms in Chemical Reactions -
Tutorials
Stoichiometry. Balancing chemical reactions. Limiting reagent. Principles of volumetric analysis. Equilibria in solution. Calculation of pH in solutions of weak acids and bases. Buffer solutions. Calculations of solubility.
Bibliography
Title: Chimica di Base
Authors: F. Arnesano, G. Bandoli, F. Bisceglie, A. Dolmella, D. Maggioni, F. Musiani, G. Natile, M.M. Natile, D. Tesauro
Editor: Edises
ISBN: 9788836231843
Edition: III
Pubblication year: 2024
Students who have problems with stoichiometry are advised to refer to the following text:
Maurizio Bruschi Stechiometria e laboratorio di chimica generale. Eserciziario 2/Ed. Pearson, 2018
Teaching methods
The course is made up of lectures, supplemented by material accessible online on the site https://elly2024.didattica.unipr.it/. Impromptu tests will be taken during the year to check the students’ level of comprehension. The stoichiometry part will be carried out by presenting a series of examples at the blackboard followed by problems to be solved individually or in group, in the classroom or at home.
During the lectures questions concerning the subject under discussion will be posed and students are incouraged to intervene or ask further questions.
Assessment methods and criteria
Possibility to take an intermediate test (approximately in the second half of November) lasting 45 minutes.
Students who pass the intermediate test with a score of at least 9/14 will be allowed to take the remaining part of the program during an exam in the first session (January-February), with one hour available. The test will be considered passed with a score of at least 9/16.
Note: The partial test will only be valid during the first session of the following calendar year, and when registering for the exam on the ESSE3 platform, it is mandatory to indicate in the notes that the partial test was passed.
No exceptions to these rules will be allowed.
The final grade will be the sum of the score obtained in the intermediate test and the score obtained in the second test, provided that both are greater than or equal to 9. The final grade can either be accepted or rejected.
Alternatively:
The learning outcomes are assessed through a final written exam (1.5 hours) consisting of a series of 13 open-ended questions, distributed as follows:
Four questions on the concepts of atomic and molecular theory (11 points)
Three questions on chemical bonding theory (6 points)
Four questions on chemical thermodynamics (10 points)
Two questions on chemical kinetics (3 points)
To pass the exam, it is not enough to accumulate 18 points; the student must obtain at least half of the points assigned to each of the four teaching units. If, in addition to answering all the questions, the written exam is well-organized and the student demonstrates a strong command of language, honors will be awarded.
Other information
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2030 agenda goals for sustainable development
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