90931 - General and Inorganic Chemistry

Course Unit Page

  • Teacher Marco Montalti

  • Learning modules Marco Montalti (Modulo 3)
    Francesco Musiani (Modulo 2)
    Simona Fermani (Modulo 1)

  • Credits 10

  • SSD CHIM/03

  • Teaching Mode Traditional lectures (Modulo 3)
    Traditional lectures (Modulo 2)
    Traditional lectures (Modulo 1)

  • Language English

  • Campus of Rimini

  • Degree Programme Single cycle degree programme (LMCU) in Pharmacy (cod. 9078)

Academic Year 2022/2023

Learning outcomes

The General Chemistry course provides the basic knowledge of the atomic structure of chemical species, chemical bonds, general properties of solutions, general features of the reactions (stoichiometry, spontaneity, completeness, rate) and the main parameters which affect these properties, elements of thermodynamics and kinetic. The student is able to identify the structure, geometry and nomenclature of inorganic compounds and the student is able to balance chemical reaction starting from reagents and to predict if they are or not spontaneous reactions.

Course contents

Course contents

The course is divided in three parts that will be teached by two different professors:

Prof.ssa Simona Fermani, first part 4 credits, Fundamentals of Chemistry

Prof. Francesco Musiani, second part 3 credits, Chemistry in solution

Prof. Marco Montalti, third part 3 credits, Stoichiometry

The professors will follow in a homogeneous way the program reported here after.

Introduction to the Inorganic Chemistry

The atom

The atomic theory; atomic composition; atomic and mass numbers. Isotopes and atomic weight. Bohr's atomic theory; energy quantization. Atomic structure and quantum theories; orbitals, quantum numbers and spin. Orbitals in polyelectronic atoms, electronic configurations of elements. Periodic Table and relation with electronic configuration. Ionization energy, electron affinity, atomic and ionic radii.

Compounds

Minimum and molecular formula. Valence and oxidation degrees. Nomenclature. Lewis structures of molecule and polyatomic ions. Molecular geometry. Resonance, isomers, PM and PF. The mole and NA. Molar mass and numbers of moles.

Chemical bond

General concepts. Ionic bond: lattice energy, stoichiometry and geometry of ionic compounds. Covalent bonds: electronegativity and bond polarity; bond energy and distance. Valence bond theory and molecular orbital theory. Ibridization. Metallic bond. Intermolecular forces: Van der Waals, London and hydrogen bond.

Solid, liquid and gaseous states

Solid, liquid and gaseous states: general properties. Gas theoretic model. Equation of state for gases. Gas mixtures: partial pressure. Changes of state and phase diagrams.

Solutions

General properties of solutions. Concentration. Solubility. Solutions of electrolytes. Ideal diluted or concentrated solutions. Changes of state in liquid solutions. Raoult and Henry laws. Osmosis. Colligative properties and determination of molecular weight.

Chemical reactions

Chemical reactions and equations; mass conservation law. Equation balancing. Redox reactions and their balancing. Reactions in solution and ionic equations; redox half-reactions. Mass relation in the reactions; equivalent weight.

Thermodynamics

Generalities of thermodynamics; reactions and heat (internal energy, enthalpy), spontaneous reactions (entropy, free energy), study of the free energy variation during a chemical reaction.

Kinetic

Rate of reaction, kinetic equation. Reaction mechanism. Activated complex and activation energy. Catalysis.

Chemical equilibrium

Complete and uncompleted reactions. The equilibrium constants: Kc and Kp. Homogeneous and heterogeneous equilibria. Le Chatelier's principle. Solubility and Kps. Complex ion equilibria. Effects of P,V,T, concentrations of reagents and products on the position of the equilibria. Simultaneous equilibria. Stoichiometric calculations on equilibria.

Acids and bases

Protonic theory of acid and bases. Autoionization; Kw. Ka and Kb. Polyprotic acids and bases. Molecular structure and acid/base properties. Acidity of solutions: pH. Acid-base reactions. Buffers. pH and solubility.

Electrochemistry

Galvanic cells. Reduction potentials and cell e.m.f. Electrolysis.

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Readings/Bibliography

General Chemistry is a base science so any book on the subject for UNIVERSITY students is suitable for the preparation of the exam. Two titles of the many that are available are suggested:

- P. Atkins, L. Jones, L. Laverman. “Chemical Principles: The Quest for Insight”. W.H. Freeman and Company

- N. J. Tro. “Introductory chemistry essentials”. Prentice Hall (Pearson)


Teaching methods

Class lessons and exercises discussed in class with the teacher, power point presentations.


Assessment methods

The students have to take a written test (compulsory), composed by multiple choice questions and problems. They have 2 hours to complete the test. The students with an evaluation equal or higher than 18/30 have the possibility to take an oral exam (optional).

For the written test students have to bring a valid identity document with picture, the periodic table of the elements and a scientific calculator. The use of mobile phones as calculators is forbidden.


Teaching tools

Teaching tools

PC connected projector, overhead projector for class lessons.

Distribution of copies of extra-materials when needed and possibility to download the files of the lessons from websites of the professors and Insegnamenti On line (https://iol.unibo.it/).

Office hours

See the website of Marco Montalti

See the website of Francesco Musiani

See the website of Simona Fermani