65931 - Inorganic and General Chemistry

Learning outcomes

At the end of the course, the student has a qualitative but rigorous knowledge of the principles of interpretation of general and inorganic chemistry. In particular, it is able to: - understand and describe the composition, structure and reactivity of molecules - using the periodic law as a basis for rationalization of the variety and complexity of chemical phenomena; - perform simple laboratory manipulations. The student also has knowledge of the chemical elements of more widespread in the environment, with particular attention to their importance in natural and industrial processes.

Course contents

Prerequisites. Basic mathematical functions: roots, power of and logarithms. Solutions of algebraic equations, Knowledge of the principal physical tenets, their correlation with each other and their measure units.

Introduction. Chemical and physical properties of matter. States of aggregation and phases.

Atoms. The fundamental laws of chemistry. Subatomic particles. Atomic number and mass number. Isotopes. Mole. Wave-particle dualism and quantum-mechanical model of atom; quantum numbers and their meaning, orbital shells and sub-shells, electronic configurations.

The Periodic Table. Periodic properties. Dimensions of atoms and ions, ionization energy, electronic affinity and interpretation of their periodic behavior.

Name of inorganic compounds. Chemical compounds. Oxidation numbers. Name of inorganic compounds.

Stoichiometry. Chemical reactions, chemical equations and their balancing. Reactions in solution. Concentration in solution and dilution. Acid-base reactions. Redox reactions and their balancing. Combustion reactions. Titrations. Limiting reagent and reaction yield.

Chemical bond. Electronegativity. Compounds characteristics as a function of chemical bonds. Ionic bond: reticular energy, Born-Haber cycle. Covalent bond: octet rule, Lewis structures, multiple bonds, resonance, partial and formal charges, molecules geometry, valence bond model, hybrid orbitals. Metallic bond. Intermolecular bonds and hydrogen bond.

Gases. Properties of gases, laws of gases, ideal gas law, Dalton law on partial pressures. Ideal and real gases.

The solid state. Physical properties of solids. Crystal structures. Ionic, covalent, molecular and metallic solids. Polymorphism and isomorphism.

Chemical equilibrium. Haber process. Law of mass action. Relation between Kp and Kc. Principle of Le Chatelier. Homogeneous and eterogeneous equilibria.

Equilibria in solution. Dissociation of water and pH. Properties and strength of acids and bases. pH calculations for strong and weak acids and bases, salts and pH of their solutions. Buffer solutions. Solubility and solubility product. The common ion effect. Titration curves; pH indicators.

Phase diagrams. Phase diagrams of pure substances: equilibrium curves, triple point, critic point.

Liquids and solutions. Vapor pressure and liquid properties. Colligative properties. Osmotic pressure.

Fundamentals of Inorganic Chemistry. Overview on the chemical properties of the principal elements as a function of their position in the Periodic Table. Elements and compounds of high environmental relevance.

Readings/Bibliography

Course contents can be found in any university book of General Chemistry. Suggested books

- Palmisano, Schiavello "ELEMENTI DI CHIMICA", EDISES

- Petrucci, Herring, Madura, Bissonnette "CHIMICA GENERALE, Principi ed applicazioni moderne”, Ed. PICCIN

- Del Zotto "Esercizi di Chimica Generale" - EDISES

Materials from lectures are available through username and password in IOL Insegnamenti online - Supporto online alla didattica. https://iol.unibo.it/ - Università di Bologna. The use of this material does NOT substitute the use of text book.

Teaching methods

The course consists of 8 CFU: 6CFU of Lectures,1CFU of numerical exercises and 1CFU of laboratory experiments.

Numerical exercises and laboratory activity are focused to acquire practical skills.

Assessment methods

Written and oral tests.

The assessment of knowledge includes a written test consisting of 10 numerical exercises related to the course program, to be completed in 3 hours. Passing the written test requires a grade greater than or equal to 18/30 and allows access to an oral interview in which the level of depth of the subject achieved by the student will be ascertained. The oral exam will start from the discussion of the exercises not completed or performed incorrectly during the written test. You will be asked to draw the Lewis structure of a simple inorganic compound, discussing its geometry and hybridization.

There will be 2 partial written tests in progress, each with 5 exercises, only for students of the present Academic Year. Passing the first test with at least 18/30 allows access to the second test. The grade for admission to the oral test will be the average of the two grades of the tests in progress, which must be equal to or greater than 18/30.


The final grade does not correspond to the mathematical average of the grade of the written and oral tests, but is mainly influenced by the performance of the oral test

On written tests only pen, scientific calculator and periodic table of elements are admitted. Books are not permitted.

Elements of judgment used for the attribution of the grade
Written exam: the ability to correctly solve stoichiometry exercises and rework the concepts acquired in the classroom in the General Chemistry Course, the correct use of units of measurement, attention to the order of magnitude of the results and the demonstration of a logical and formally correct approach to the execution of the exercises will be assessed.
Oral exam: the ability to critically correct and/or discuss the written exam will be assessed, starting from the exercises not solved or solved badly. Particular attention will be given to the expository order and formal correctness. Synthesis, clarity and coherence are additional elements taken into consideration for the evaluation of the oral exam.
All evaluations, both positive and negative, are accompanied by comments provided by the teachers in order to ensure the acceptability of the grade by the student.

Students with learning disorders and\or temporary or permanent disabilities: please, contact the office responsible (https://site.unibo.it/studenti-con-disabilita-e-dsa/en/for-students ) as soon as possible so that they can propose acceptable adjustments. The request for adaptation must be submitted in advance (15 days before the exam date) to the lecturer, who will assess the appropriateness of the adjustments, taking into account the teaching objectives.

 

Teaching tools

Blackboard and video projector. Chemical laboratory activity.

Lessons in classroom accompanied by suitable exercises and practical experiences in laboratory.

Links to further information

https://iol.unibo.it/

Office hours

See the website of Francesca Soavi