GENERAL AND INORGANIC CHEMISTRY
CHIMICA GENERALE ED INORGANICA
| A.Y. | Credits |
|---|---|
| 2019/2020 | 8 |
| Lecturer | Office hours for students | |
|---|---|---|
| Mauro Formica | Friday 09.00-12.00 by by previous appointment (email or phone) |
| Teaching in foreign languages |
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Course with optional materials in a foreign language
English
This course is entirely taught in Italian. Study materials can be provided in the foreign language and the final exam can be taken in the foreign language. |
Assigned to the Degree Course
| Date | Time | Classroom / Location |
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| Date | Time | Classroom / Location |
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Learning Objectives
The course has the purpose to provide the student of the general and inorganic chemistry foundations taking into account the theoretical and applicative aspects. The main goal is to supply the student of the knowledge to can understand and to analyze the matter, its properties as well as its transformations under the chemical point of view, mainly considering the biological field. In particular, the student will be able to use the chemical language, to understand and to use correctly the molecular formula and to foresee the chemical-physical characteristics of a compound as its reactivity, on the base of its structure and its elemental composition. This will be pursued, paying particular attention to the chemical bonds, to the chemical reactions, to the main interactions in the molecular systems as well as to the aqueous solution chemistry.
Program
01 - The matter. Atoms and chemical elements. Molecule and ionic compounds. Isotopes.
02 – Aggregation states of the matter. Atomic structure: protons, neutrons and electrons.
03 - Atomic mass, atomic and molecular weights. Mole and molar mass. Percentage composition, minima and molecular formula.
04 - Energy. Electromagnetic radiations. Photoelectric effects.
05 - The hydrogen atom and its energetic levels. Atomic orbitals. Quantum numbers. Energetic levels in polyelectronic atoms. The spin quantum number. Rules for the filling orbitals. Electron configuration of the elements.
06 - Periodic systems. Ionization energy, electron affinity, electronegativity.
07 - Covalent bond. σ and π bonds. Valence bond and molecular orbital theory. Polar bond. Hybrid orbitals.
08 - Structural formula and molecular geometry.
09 - Ionic bond.
10 - Metal bond.
11 - Chemical bond and physical properties of the matter.
12 – Polar and apolar molecules. Intramolecular forces. Van der Walls forces. Hydrogen bond.
13 - Chemical properties and periodicity. Nomenclature of the chemical compounds. Oxides hydrides. Oxidation number. General characteristics and reactivity of groups and of main elements. Main compounds.
14 - Acid-base theory of BrØnsted-Lowry and of Lewis. Levelling effect of the solvent.
15 - Chemical reactions. Redox reaction. Acid-base reactions. The balance of a chemical reaction.
16 - Gas-state. Ideal gas. Kinetic theory of gas. Real gas.
17 - Solutions. The concentration of solutions. Vapor tension. Ebullioscopy and cryoscopy of solutions. Osmotic pressure. Solubility.
18 - Coordination compounds.
19 - Chemical equilibrium. Reversibility of chemical reactions. Law of mass action. Le Chatelier-Braun’s principle. Equilibrium of heterogenic systems. The solubility-product constant.
20 - Equilibrium for acid-base reactions. Ionic product of water. Buffer solutions. Salt hydrolysis. The pH. Determination of pH. The glass electrode. Titrations. Indicators of pH.
21 - Chemical Kinetics; rate of reaction, activation energy, catalysts.
22 - Thermodynamic in chemistry: work and heat; Thermodynamics’ laws. Enthalpy and entropy, Gibbs free energy. Equilibrium and free energy; equilibrium constant and temperature.
23 - Electrochemistry. The battery, electromotive force. Standard potentials. The electrolysis.
Bridging Courses
Bridging courses do not foreseen
Learning Achievements (Dublin Descriptors)
D1 – Knowledge and ability of comprehension.
The student will have the ability to analyze the properties of the matter, highlighting the relation among formula, geometries and molecular properties. He will have to know the principles at the chemical bond, the nomenclature of the inorganic chemical compounds, foresee and understand the acid-base and redox behavior of the main compounds, the principles of the chemical equilibria and of the chemical reactions as the acid-base and redox reactions, the atomic and molecular structure, the foundations of the periodic tables with its periodic properties, the main properties of gases, liquids and solids, the intermolecular forces, the main foundations of the thermodynamic, of the chemical kinetic and of the electrochemistry. He will have the skill with the concepts of the mole, the concentration of the solutions, the pH and the solubility. In addition, he will have to know the numerical techniques to describe the equilibria, the reactions. These knowledges will be checked by oral questions.
D2 – Ability to apply knowledge and comprehension.
Student will have to be able to utilize the correct chemistry language, and to apply the stoichiometric calculation in order to determine the equilibrium state of a chemical system (yield of a reaction, pH of a solution, solubility of an insoluble electrolyte). The achievement of these abilities will be tested through a written examination.
D3 – Autonomy of judgement.
Student will have to be able to estimate the role played by the substances composing a chemical system in determining its physical-chemical properties. This knowledge will be essential in order to interpret the behavior of more complex systems tackled in the next teaching. The achievement of these abilities will be tested through the written examination and oral questions aimed at estimate them.
D4 – Application skill.
Student will have to be able to clearly describe the physical-chemical phenomena learned in the course with appropriate language and examples.
D5 – Learning skill.
Student will have to be able to grow autonomously and critically their scientific knowledges by using the teaching material provided by the teacher and any other book or scientific article provided by themselves. These abilities will be stimulated by the teacher proposing and resolving numeric problems.
Teaching Material
The teaching material prepared by the lecturer in addition to recommended textbooks (such as for instance slides, lecture notes, exercises, bibliography) and communications from the lecturer specific to the course can be found inside the Moodle platform › blended.uniurb.it
Supporting Activities
The course foresees some hours of facultative stoichiometric exercitations in addition to the 56 foreseen.
Teaching, Attendance, Course Books and Assessment
- Teaching
The course consists in lecturers and stoichiometry together with practical experiences to favor the comprehension.
Students can attend the lectures asking explanations to the teacher.
- Attendance
The frequency is not obligatory. Basic knowledges of mathematic and physic are requested.
- Course books
Fusi, Giorgi, Lippolis, Zaccheroni Chimica: principi generali con esercizi. Idelson Gnocchi editore; ISBN: 9788879476539
- Assessment
The assessment of the learning provides a written and an oral examination
The aim of the written examination is to verify the student skills with respect to the balance of a chemical reaction, to the stoichiometric calculus, to the calculus of the concentration of a solution and its related properties, the quantification of reagents and products in a chemical equilibrium, paying particular attention to the acid-base reactions and to the pH. The written examination consists of eight exercises: one related to design a molecular structure of a species and the indication of the geometry of the species; one related to the balance of a redox reaction; two nomenclature exercises in which must be indicated the molecular formula of three species knowing the systematic name and viceversa; two stoichiometric exercises with the calculus of the concentration of the solutions; one related to the stoichiometry of the chemical reactions; one related to the pH of a solution. The written examination will be judged by a qualitative result (scarcely sufficient, sufficient, good, very good, optimum)
The aim of the oral examination is to verify the student preparation with respect to the writing of a chemical formula, to the prevision of the chemico-physical properties of the main inorganic compounds (oxides, hydrides, acids, bases, salts) as well as of the theoretical concepts, explained during the course. The student must be able to furnish appropriate examples concerning each argument to demonstrate the full comprehension of it.
The oral examination will be judge with a thirtieth vote in which the written examination will be taken into account
- Disability and Specific Learning Disorders (SLD)
Students who have registered their disability certification or SLD certification with the Inclusion and Right to Study Office can request to use conceptual maps (for keywords) during exams.
To this end, it is necessary to send the maps, two weeks before the exam date, to the course instructor, who will verify their compliance with the university guidelines and may request modifications.
Additional Information for Non-Attending Students
- Teaching
It is custom of the teacher to send the done program each week to the students with the aim help them in studying organization.
- Attendance
Basic knowledges of mathematic and physic are requested
- Course books
Fusi, Giorgi, Lippolis, Zaccheroni Chimica: principi generali con esercizi. Idelson Gnocchi editore; ISBN: 9788879476539
- Assessment
The assessment of the learning provides a written and an oral examination.
The aim of the written examination is to verify the student skills with respect to the balance of a chemical reaction, to the stoichiometric calculus, to the calculus of the concentration of a solution and its related properties, the quantification of reagents and products in a chemical equilibrium, paying particular attention to the acid-base reactions and to the pH. The written examination consists of eight exercises: one related to design a molecular structure of a species and the indication of the geometry of the species; one related to the balance of a redox reaction; two nomenclature exercises in which must be indicated the molecular formula of three species knowing the systematic name and viceversa; two stoichiometric exercises with the calculus of the concentration of the solutions; one related to the stoichiometry of the chemical reactions; one related to the pH of a solution. The written examination will be judged by a qualitative result (scarcely sufficient, sufficient, good, very good, optimum)
The aim of the oral examination is to verify the student preparation with respect to the writing of a chemical formula, to the prevision of the chemico-physical properties of the main inorganic compounds (oxides, hydrides, acids, bases, salts) as well as of the theoretical concepts, explained during the course. The student must be able to furnish appropriate examples concerning each argument to demonstrate the full comprehension of it. The oral examination will be judge with a thirtieth vote in which the written examination will be taken into account
- Disability and Specific Learning Disorders (SLD)
Students who have registered their disability certification or SLD certification with the Inclusion and Right to Study Office can request to use conceptual maps (for keywords) during exams.
To this end, it is necessary to send the maps, two weeks before the exam date, to the course instructor, who will verify their compliance with the university guidelines and may request modifications.
Notes
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