GENERAL AND INORGANIC CHEMISTRY I AND LAB EXPERIENCES M - Z

Module Module 1

The course aims to transfer the basic knowledge of general chemistry to the student. 
In particular, the student will be directed to understand the atomic and molecular structure, 
the periodic properties of the elements, the chemical bonds, the chemical reactions, 
the properties of gases and solutions as well as the quantitative aspects of general chemistry.

• First module

  Lectures, excercises

Information for students with disabilities and/or DSA.

As a guarantee of equal opportunities and in compliance with current laws, interested students can ask for a personal interview in order to plan any compensatory and/or dispensatory measures, based on their specific needs and on teaching objectives of the discipline. It is also possible to ask the departmental contacts of CInAP (Center for Active and Participatory Inclusion- Services for Disabilities and/or DSAs).

Basic knowledge of mathematics, physics and chemistry

• First module

  • The composition of matter: molecules and molecular compounds, ions and chemical compounds, chemical nomenclature, constitution of the atom, atomic weight and molecular weight, periodic table of elements, groups and periods, periodic properties of the elements, diagonal relationships.
  • Fundamental laws of chemistry: Dalton's atomic theory, Avogadro's principle, combination laws, discovery of electrons, protons and neutrons.
  • Chemical reactions: the concept of mole, chemical equations, balancing simple reactions, definition of oxidant and reducing agent, oxidation number and redox reactions, definition of acid and base, acid-base reactions, quantitative meaning of chemical reactions, at equilibrium and irreversible.
  • Structure of the atom: Electromagnetic radiation, hints of quantum mechanics: Planck, photoelectric effect, atomic spectra, Bohr, de Broglie, Heisenberg model, Schrödinger equation, monoelectronic atoms, polyelectronic atoms: spin and quantum number of spin, orbital energies of polyelectronic atoms, Pauli, Aufbau's exclusion principle and Hund's rule.
  • The chemical bond: covalent bond according to Lewis, Molecular geometry and VSEPR theory, Valence bond theory, Molecular geometry and hybridization, Multiple bonds, Outline of molecular orbital theory, electronic configuration of homopolar diatomic molecules of the second period, non- covalent, ionic bond, hydrogen bond, metal bond.
  • The gaseous state: laws of gases, equation of state for ideal gases, molar volume, density of gases, diffusion law of gases, real gases, van der Waals equation for real gases, molecular meaning of pressure and temperature, hints of kinetic theory of gases.
  • State transitions: Gas-Vapor-Liquid, critical pressure and temperature, state diagrams, equilibria between phases.
  • Notes on the solid state: metallic and ionic solids, molecular solids and covalent lattice solids, lattice energy, Born-Haber cycle.
  • The liquid state and solutions: role of non-covalent interactions, vapor pressure of liquids and boiling temperature, solvation of solutes, concentration of solutions, Raoult's law, deviations from Raoult's law, notes on the distillation of liquids, properties colligative, cryoscopy and ebullioscopy, osmotic pressure, strong and weak electrolytes, degree of dissociation, solubility of gases in liquids.
  • Kinetics and chemical equilibrium: equilibrium reactions, speed of a chemical reaction, order of a reaction, activation energy and Arrhenius equation, kinetic deduction of the chemical equilibrium, equilibrium constant, influence of concentration, pressure and temperature on chemical equilibria, catalysis, homogeneous and heterogeneous catalysts.
  • Hints of thermodynamics and thermochemistry: definitions and system-environment relations, state functions, I principle of Thermodynamics, molar thermal capacities, measurement of heat, Hess's law and reaction enthalpies, II principle of Thermodynamics, III principle of Thermodynamics and entropies of reaction, free energy, relationship between free energy and the equilibrium constant.

• First module

  R.H. Petrucci, W.S.Harwood, F.G. Herring, CHIMICA GENERALE (Principi e moderne applicazioni), Piccin

  Kotz-Treichel-Townsend (ed edizioni precedenti) - Chimica- EdiSeS M. Speranza-Chimica Generale ed Inorganica-Edi-Ermes
  P. W Atkins, J. Loretta - Chimica Generale - Zanichelli
  M Schiavello, L. Palmisano - Fondamenti di Chimica - EdiSes

  N. J. Tro - Chimica Un approccio molecolare - Zanichelli

  P. Silvestroni- Fondamenti di Chimica- CEA

  M. Speranza-Chimica Generale ed Inorganica-Edi-Ermes

The final exam consists of a written test (the day of the exam will be as indicated on 
the official calendar), based on exercises similar to those developed in the classroom during 
the course and in an oral interview (date and place will be indicated by the teacher) based 
on all topics of the program and on laboratory experiences.
The exam tends to ascertain the level of overall knowledge acquired by the candidate, 
his ability to critically address the topics studied and to relate the various parts of the 
program. The exam consists of a written test and an oral exam. The written exam consists 
in solving simple stoichiometry problems related to nomenclature, chemical reactions, 
gas transformations and the study of chemical phenomena in aqueous solution, thermochemistry. 
This test tends to verify the possession of the basic notions of the discipline. The written 
test will be considered passed if the student has solved exactly more than half of the assigned 
exercises. During the written exam, students will be able to use the periodic table and 
calculator, but not cell phones.
Passing the written exam is a necessary but not sufficient condition to pass the final exam.
The oral exam will consist of questions relating to the various parts of the program to ascertain 
the overall level of knowledge acquired by the candidate.
Criteria for awarding the final grade:
The mastery shown in the qualitative and quantitative arguments, the critical vision of 
the topics addressed during the course and the ability to correlate the various parts of 
the program will contribute in equal measure to the formulation of the final grade.