GENERAL AND INORGANIC CHEMISTRY

Single discipline educational activity

Course Sheet

Course code:

00212

Academic Year of enrolment:

2022

Year of supply:

2022/2023

Type of Course:

Basic

Degree:

Course of Single Cycle Degree 5 years in MEDICINAL CHEMISTRY AND PHARMACEUTICAL TECHNOLOGY

Disciplinary Sector:

General and Inorganic Chemistry

Language:

Italian

Location:

CHIETI

Credits:

Programme Year:

Professor and Collaborators:

RE Nazzareno

Cycle:

Second semester

Obligatory attendance:

Yes

Minimum hours of attendance:

Hours of classroom activity:

Individual study hours:

149

Prerequisites:

The course of "General and Inorganic Chemistry" can also be faced by those who have no previous knowledge of chemistry, although it is useful that students have already acquired the basic notions of chemistry carried out in at least one annual high school course.
Furthermore, due to the nature of the topics that will be covered, it is important that students have mastered some basic knowledge of mathematics, in particular: the execution and properties of operations with exponential numbers and logarithms, the solution of prime equations and second degree, systems of equations.
- some basic knowledge of physics, in particular: kinetic and potential energy, work, Coulomb's law, electric charge, electric dipole, current.

Objectives

The objective of the general and inorganic chemistry course is to provide the basic concepts of chemistry necessary to tackle the chemical courses of the following years.

Expected learning outcomes
At the end of the cycle of lessons the student:
1. Knowledge and understanding
- is in possession of the basic chemical notions on the composition, structure, properties and transformations of matter;
- is in possession of fundamental knowledge on the atomic structure, on the nature of the chemical bond, and on the structure of molecules;
- is in possession of notions on the properties of the gaseous state and of the solutions;
- can balance a chemical equation and determine the quantitative relationships in a reaction;
- is in possession of useful knowledge to evaluate the concentration and dilution of aqueous solutions;
- is able to represent the formula and the predictable molecular geometry of simple binary, ternary and coordination compounds;
- will be able to interpret the behavior of a system in conditions of chemical equilibrium in the gaseous phase and in aqueous solution, also at a quantitative level;
- is in possession of in-depth knowledge to evaluate the degree of acidity (pH) of aqueous solutions and the conditions for precipitating poorly soluble compounds in the solution;
- knows the basic concepts of chemical kinetics;
- knows the energetics of chemical transformations (chemical thermodynamics) and can evaluate the spontaneity of a reaction;
- will know basic concepts of electrochemistry and its practical applications.
- knows the chemistry of the elements that will be part of his cultural background.
2. Ability to apply knowledge and understanding
- will be able to apply what he has learned theoretically to real cases.
- developed the ability to perform exact and approximate calculations by applying the laws of chemistry and stoichiometry to concrete cases (numerical exercises and laboratory activities);
3. Judgment skills
- will have to be able to solve, with scientific and logical reasoning, stoichiometry problems using their chemical and mathematical knowledge.
- they must be able to interpret experimental facts in the light of chemical theory (atomic structure, bond, equilibria, etc.).
4. Communication skills
- must be able to communicate and explain, with correct chemical terms, all the contents of the course.
5. Learning skills
- must be able, with the knowledge acquired, to follow and understand the lessons of the more specialized subsequent courses.

Contents

Introduction to Chemistry. Nomenclature of inorganic compounds. Thermodynamics and Thermochemistry. The atomic theory. Chemical bond. Gas. Staes of matter and phase transitions. Solutions. Chemical Kinetics. Chemical Equilibrium. Acid-base theories. Acid-base equilibria. Solubility equilibria. 2nd law of thermodynamics and equilibrium. Redox reactions. Electrochemistry. Brief description of the properties of the elements. Exercises in stoichiometry and on the topics covered during the lectures.

Extended Syllabus

Introduction: Principles of Chemistry. Molecules and molecular compounds. Aggregation States of the Matter. Atomic number, mass number and isotopes. Molecular mass and formula mass. The mole. Molecular formula, empirical formula, ions and ionic compounds.
IUPAC rules for the nomenclature of the most common inorganic compounds
Thermodynamics and Thermochemistry: Energy and its units. Temperature, heat and thermal capacity. The System and Surroundings. Heat and work. Internal Energy. First law of thermodynamics. Enthalpy. Reaction heat and enthalpy. Thermochemical equation. Hess law.
The atomic theory: structure of the atom, nuclear model of the atom. The proton and the nucleus. Radioactivity. Quantum theory, quantization of energy. Photons and photoelectric effect. Bohr's theory of the hydrogen atom. The Schroedinger equation. Quantum numbers. Atomic orbitals, electron configuration. The periodic table. Periodic trends in chemical properties of the main group elements.
Chemical bond: Ionic bond. Covalent bond. Electronegativity and polarity. The Lewis approach. Molecular geometry and the VSEPR model. Valence bond theory. Multiple and single bonds: s and p bonds. Hybridization and hybrid orbitals. Hybrid orbitals and molecular geometries. Molecular orbital theory. Metallic bond.
Gas: Properties of gases. The kinetic molecular theory of gases.
States of matter: Equilibrium between the phases. Phase changes. Vapor pressure. Clausius-Clapeyron equation. Phase diagram. Intermolecular forces. Hydrogen Bond. Properties of solids. Crystal structures and unit cells. The liquid state.
Solutions: Types of solutions. Concentration units. Solutions of gases in liquids and Henry law. Colligative properties of solutions. Raoult's law.
Chemical kinetics: Reaction rate. Reaction order. First-order reactions: concentration dependence vs. time. Half-life, Arrhenius law.
Chemical equilibruium: The concept of equilibrium and the equilibrium constant. Le Chatelier's principle. Heterogeneous equilibria. Aqueous equilibria. Arrhenius, Bronsted-Lowry and Lewis acids and bases. The acid-base properties water. The pH scale. Strong and weak acids and bases. Polyprotic acids. Amphoteric substances. Acid-base properties of salt solutions: hydrolysis. Buffer solutions. Solubility product and common ion effect.
Thermodynamics and equilibrium: Spontaneous reactions. Entropy and second law of thermodynamics. Third law of thermodynamics and standard entropies. Free energy and equilibrium constant. Van’t Hoff equation.
Electrochemistry: Redox reactions. Galvanic cells. Standard reduction potentials. Nernst equation. Concentration cells. Electrolysis. Faraday's laws.
Properties of the elements: Properties of the main groups of the Periodic Table, including transition metals and their complexes.

Exercises on the following subjects:

- mole, empirical and molecular formulas, percent by mass,
- stoichiometry, the limiting reactant;
- gas laws;
- concentration and composition of the solutions;
- equilibria in the gas phase (Kc, Kp);
- equilibria in solution: acid/base equilibria, hydrolysis, buffer solutions, heterogeneous equilibria;
- balancing redox reactions;
- electrochemistry.

Recommended Bibliography

Autori vari; Chimica Generale ed Inorganica , Edi.Ermes - Milano 2013
Kotz, Treichel, Weaver; Chimica, Edises – Napoli 2013

Methods of Provision

Conventional

Teaching Methods

The course consists of lectures in the classroom (scheduled for 64 hours) and exercises in stoichiometry (scheduled for 12 hours).
Frontal lessons.
Teaching is mainly of a conventional type, with oral presentation, supported by slide projections and writing on the blackboard. The teacher illustrates the relevance of the topics by giving concrete examples of their application in the context of numerical applications and subsequent courses of the Degree Course. The aim of the lectures is to convey the notions of theory relevant to the topics discussed.
Stoichiometry exercises.
The exercises are carried out in parallel with the lectures, at the end of a cycle of lessons with coherent contents. The purposes of the exercises are:
- the practical application of the theoretical notions proposed (acquisition of practical skills)
- stimulate the ability to analyze and identify a strategy aimed at solving the problem (acquisition of processing skills)

Evaluation methods

Verification of learning:

The exam consists of a written test and an oral test. The written exam consists of a multiple choice test of 16 questions including 8 theoretical questions and 8 exercises. With the questions we intend to evaluate both the understanding of the fundamental principles of chemistry and the student's ability to apply what is described in theory to real cases. Stoichiometry problems, on the other hand, are aimed at verifying the student's ability to use the concepts acquired by carrying out numerical exercises. Those who pass the written test with a mark of at least 18/30 are allowed to sit the oral in the same section.
The oral exam consists of a discussion lasting about 20-30 minutes in which questions will be asked relating to theoretical aspects related to the topics addressed in the teaching and reported in the detailed program of the course, and is aimed at ascertaining the level of knowledge and skills of understanding achieved by the student on the theoretical and methodological contents indicated in the program. It will also make it possible to verify the student's communication skills with language properties and autonomous organization of the exposition of the topics, as well as verify the student's ability to apply the skills acquired to more complex systems, however, attributable to the teaching program.
The final mark of the exam will be expressed out of thirty and will take into account overall the evaluations obtained in the written and oral tests.

Contacts/More Information

During the course two partial tasks will be carried out, the overcoming of which, with an average grade of at least 16/30 and a minimum of 12/30 on each task , exempts the candidate from taking the written exam in the June and July sessions
The teacher recommends regular attendance and participation in the lessons.
The teaching material (slides, exercises proposed during numerical exercises, texts of previous exemptions and written tests) are made available to students on the Moodle e-learning platform after registration.

Università degli Studi
"G. d'Annunzio"

Chieti - Pescara

Aree