Unit PHYSICAL CHEMISTRY 1
- Course
- Chemistry
- Study-unit Code
- 55009115
- Curriculum
- In all curricula
- Teacher
- Fausto Ortica
- CFU
- 15
- Course Regulation
- Coorte 2021
- Offered
- 2022/23
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa integrata
PHYSICAL CHEMISTRY 1
| Code | 55078808 |
|---|---|
| CFU | 8 |
| Teacher | Fausto Ortica |
| Teachers |
|
| Hours |
|
| Learning activities | Base |
| Area | Discipline chimiche |
| Academic discipline | CHIM/02 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | 1) THERMODYNAMICS: Real Gases; Intermolecular Forces; State equations (van der Waals, virial). The three Principles of Thermodynamics: Work, heat; internal energy; enthalpy, heat capacities; thermochemistry; entropy, free energy, chemical potential. Equation of Gibbs-Helmholtz. Chemical equilibrium. Fundamental thermodynamic relations and thermodynamic state equations. Equations of Clapeyron and Clausius-Clapeyron. Ideal and real solutions. Raoult's and Henry's laws. Standard states. Phase diagrams, Gibbs' phase rule and applications. 2) QUANTUM MECHANICS: Principles of Quantum Mechanics. Wave-particle dualism. The De Broglie principle. Photoelectric effect. Compton effect. Quantization. Heisenberg's uncertainty principle. Operators and observables. Schrödinger equation and its application to simple systems: Particle in a box, harmonic oscillator, and rigid rotor. The Schrödinger equation for the hydrogen atom. Hydrogenoid atoms. Atomic structure and spectra. |
| Reference texts | Peter ATKINS, Julio DE PAULA, James KEELER, CHIMICA FISICA (6th Italian edition on 11th American edition), Ed. Zanichelli, Bologna (2020). |
| Educational objectives | As from program, students will acquire a detailed knowledge of the basics of equilibrium Chemical Thermodynamics, which is fundamental in many areas of Chemistry as well as in other scientific disciplines, and the first basis of Quantum Mechanics, which are fundamental in Chemistry. As far as Thermodynamics is concerned, students will have a detailed knowledge of real gases, of the Principles and applications of Thermodynamics, of phase diagrams, ideal and real solutions. As far as Quantum Mechanics is concerned, students will have clear the limitations of Classical Mechanics, the foundations of Quantum Theory, of the Schroedinger equation, of the fundamental models of the particle in the box, rigid rotor and harmonic oscillator, of the hydrogen atom and hydrogenoid atoms, of the basis of atomic structure and atomic spectroscopy. Both in Thermodynamics and Quantum Mechanics students will develop the capacity to solve a variety of numerical problems. The fundamental concepts students will become familiar with are central for continuing their studies in the course for obtaining the Bachelor degree in Chemistry. |
| Prerequisites | In order to understand the subject matter and the learning objectives it is required that the students have taken all classes of Chemistry, Mathematics and Physics given in the first year of their Bachelor studies, and it is important that they have passed all the relevant exams. |
| Teaching methods | - face-to-face lectures on all the subjects of the course, including solution of numerical problems. - as complement of the face-to-face lectures there will be, weekly, two hours of numerical exercises by the teacher or a tutor. |
| Other information | Attendance is recommended. |
| Learning verification modality | The full exam of Physical Chemistry 1 (encompassing both modules) consists in an evaluation of the written reports on the laboratory work, in a written exam and an oral exam. The written exam requires solving n. 6 problems on the various subjects of the two modules (in three and one half hour time). The written exam can be passed by also passing successfully the two progress assessments offered at regular intervals and consisting in solving n. 6 problems on parts of the program in three and one half hour time. Passing the two progress assessments or the written exam and handing the laboratory written reports allow the student to proceed to the oral exam. The written exam aims at verifying the capability of correctly applying the theoretical notions, the capability of understanding the proposed problems and the capability of written communication. The oral exam consists in a discussion of about 45 minutes finalized at verifying the level of knowledge and the capability of understanding attained by the student on the theoretical and methodological contents listed in the course program of the two modules. The oral exam will also allow to verify the communication skills of the student of using a controlled language and self-organization in the presentation on theoretical subjects. |
| Extended program | 1) THERMODYNAMICS Introduction. Thermodynamic systems, state functions, partial molar quantities. Intermolecular forces. State-equations for gaseous and condensed systems. Van der Waals equation, critical state, principle of corresponding states, compressibility factor for real gases (pure and in mixtures). Heat, work. The First Principle of Thermodynamics. Joule's experiment. Internal energy; enthalpy. Thermal capacities at constant volume and pressure. Internal pressure. Isotherm processes; reversibile and irreversibile adiabatic processes. Thermochemistry: laws, calorimetry. Enthalpy of formation, combustion, and atomization of chemical compounds. Bond and resonance enthalpy. Kirchhoff equation. Thermal balance. The Second Principle of Thermodynamics Entropy: thermodynamic and statistical approach. Carnot cycle and theorem. Disequality of Clausius. Entropy as criterion for spontaneous and equilibrium processes. Auxiliary functions: work and free energy functions. Equilibrium conditions in closed systems: equation of Gibbs-Helmholtz. Fundamental thermodynamic relations and thermodynamic state equations. Chemical potential. Equation of Gibbs-Duhem. The third Principle of Thermodynamics. Behaviour of matter close to the absolute zero. Absolute entropies and their utilization. Applications of the principles of Thermodynamics. Ideal and real gas systems: chemical potential, fugacity, fugacity coefficients. Poliphase systems: thermodynamic derivation of the Phase Rule, equations of Clapeyron and of Clausius-Clapeyron; Raoult's law and Henry's law; equation of Duhem-Margules. Chemical potential and convention about standard states for solutions. Distillation. Thermal analysis. Phase diagrams. 2) QUANTUM MECHANICS AND ATOMIC STRUCTURE Introduction. Wave-particle dualism of matter and radiation. The black body radiation. Photoelectric effect. Compton effect. Davisson and Germer experiment. Dynamics of microscopic systems and principles of quantum mechanics. Schrödinger's equation. Quantization. Operators and observables. Uncertainty principle. Treatment of model systems. Particle in the box; harmonic oscillator; bi-dimensional and tri-dimensional rigid rotor. Atomic spectra and atomic structure. Absorption, emission, transition probability. Quantum-mechanical treatment of the hydrogen atom and spectrum of atomic hydrogen. Vector model for mono- and poli-electronic systems; L, S and J quantum numbers; LS and jj couplings. Space quantization: Zeeman effect. Deduction of the terms for ground and excited states of atoms using Pauli's principle and Hund's rules. |
PHYSICAL CHEMISTRY LABORATORY 1
| Code | 55078807 |
|---|---|
| CFU | 7 |
| Teacher | Paola Sassi |
| Teachers |
|
| Hours |
|
| Learning activities | Caratterizzante |
| Area | Discipline chimiche inorganiche e chimico-fisiche |
| Academic discipline | CHIM/02 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | The course is meant to supply with student the knowledge for understanding chemical and electrochemical equilibrium. Laboratory practices on thermochemistry, equilibria, solution properties and electrochemistry are also planned. |
| Reference texts | P.W. ATKINS, Chimica Fisica, Ed. Zanichelli, Bologna; W.J. MOORE, Chimica fisica, Piccin, Padova; SILLEN, LANGE, GABRIELSON, Problemi di Chimica Fisica, Piccin, Padova; lesson notes. |
| Educational objectives | The student will learn thermodynamic basic knowledge concerning chemical equilibrium and electrochemistry. The main competence to be developed will concern the ability to apply the knowledge acquired in the solution of various problems of both conceptual and numerical nature, related to those subjects. |
| Prerequisites | In order to understand the subject matter and the learning objectives it is required that the students have taken all classes of Chemistry, Mathematics and Physics given in the first year of their Bachelor studies, and it is important that they have passed all the relevant exams. |
| Teaching methods | The course consists in face-to-face lessons and laboratory practise on the following subjects: thermochemistry (combustion heats determination); solution properties (binary partial volumes determination) and electrochemistry (transference number determination and Onsager equation verification). For laboratory practise, the students will be divided into groups of 2 or 3 units each at most. |
| Other information | Attendance is recommended and is mandatory for laboratory activities. |
| Learning verification modality | The full exam of Physical Chemistry 1 (encompassing both modules) consists in an evaluation of the written reports on the laboratory work, in a written exam and an oral exam. The written exam requires solving n. 6 problems on the various subjects of the two modules (in three and one half hour time). The written exam can be passed by also passing successfully the two progress assessments offered at regular intervals and consisting in solving n. 6 problems on parts of the program in three and one half hour time. Passing the two progress assessments or the written exam and handing the laboratory written reports allow the student to proceed to the oral exam. The written exam aims at verifying the capability of correctly applying the theoretical notions, the capability of understanding the proposed problems and the capability of written communication. The oral exam consists in a discussion of about 45 minutes finalized at verifying the level of knowledge and the capability of understanding attained by the student on the theoretical and methodological contents listed in the course program of the two modules. The oral exam will also allow to verify the communication skills of the student of using a controlled language and self-organization in the presentation on theoretical subjects. |
| Extended program | Chemical equilibrium and its thermodynamic meaning. Chemical equilibrium in gas phase: equilibrium constant and its expressions. Temperature dependence of equilibrium constant. Principle of Le Chatelier and its analytical expression. Chemical yield. Equilibrium in heterogenous phase. Electrochemistry (ionic solutions). Transport properties in liquids. Equilibrium in solution. Chemical potential and activity of the ions in solution. Ionic conductivity, transference number and their experimental determination. Debye-Hückel theory and its application for activity coefficient and solution conductivity determination. Electroch emistry (electrochemical cells).Types of potential: electrical, chemical and electrochemical. Electrochemical cells and their classification. Reversibility and irreversibility: basic concepts of liquid-solid interphase. Nernst equation. Thermodynamics of the electrochemical cells. Types of electrodes. Application of f.e.m. measurements. Experimental data treatments. Data presentation, error determination and its propagation in the experimental measures. Laboratory practices. Four experiences will be performed on the following subjects by each student: thermochemistry (combustion heats determination); solution properties (binary partial volumes determination); electrochemistry (transference number determination and Onsager equation verification). |