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Course, academic year 2024/2025
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Physical Chemistry - GAF199
Title: Physical Chemistry
Guaranteed by: Department of Biophysics and Physical Chemistry (16-16110)
Faculty: Faculty of Pharmacy in Hradec Králové
Actual: from 2024
Semester: summer
Points: 0
E-Credits: 5
Examination process: summer s.:written
Hours per week, examination: summer s.:28/28, C+Ex [HS]
Capacity: unlimited / 60 (unknown)
Min. number of students: unlimited
4EU+: no
Virtual mobility / capacity: no
Key competences:  
State of the course: taught
Language: English
Teaching methods: full-time
Level:  
Explanation: (F,1.r.)
Note: deregister from the exam date if a requisite was not fulfilled
course can be enrolled in outside the study plan
enabled for web enrollment
Guarantor: Mgr. Jana Pavlíková Přecechtělová, Ph.D.
Classification: Pharmacy >
Co-requisite : GAF105
Annotation -
Physical chemistry is a multidisciplinary subject employing the knowledge of physics, chemistry, electrochemistry and quantum mechanics for the description of substances on both the molecular and the macroscopic level. This subject provides a necessary theoretical basis and enables students to acquire knowledge of principles of physical-chemical methods of measurement. This subject affords a fundamental knowledge necessary in study of follow-up subjects from the area of natural sciences as well as pharmaceutical disciplines. Topics: Interaction of electromagnetic radiation with matter, Spectroscopy - principles, Ion equilibria, Phase interface phenomena, Electrochemistry and electrochemical methods, Colloids and polymers, Reaction kinetics, Nonequilibrium systems, Biological membranes and transport of substances across membranes, Principles of sensory perception.
Last update: Pavlíková Přecechtělová Jana, Mgr., Ph.D. (15.02.2025)
Course completion requirements -

To earn the credit, students must meet the following requirements:

  1. Complete all experiments assigned in the laboratory classes. If a student misses a laboratory session for any reason (personal, medical etc.), they must perform the assigned experiment(s) on another date provided by the course teacher for this purpose. 
  2. Successfully submit laboratory protocols for all assigned experiments. A laboratory protocol counts as successfully submitted after it is approved by the course teacher.
  3. Pass the credit test that consists of two pen and paper assignments. The completion of each assignment is worth 25 points (2 x 25 points = 50 points in total). A student must earn a minimum of 20 points in total to pass the credit test.

 

Last update: Pavlíková Přecechtělová Jana, Mgr., Ph.D. (15.02.2025)
Literature -

Obligatory:

  • Kubíček, Vladimír. Physical Chemistry Calculations. : , , 82 s. ISBN .

Recommended:

  • Atkins, P. W.. Physical Chemistry. Oxford: Oxford University Press, 2022, 976 s. ISBN .

  • Sinko, Patrick J.. Martin's physical pharmacy and pharmaceutical sciences : physical chemical and biopharmaceutical principles in the pharmaceutical sciences. Philadelphia: Wolters Kluwer, 2023, s. ISBN 978-1-975174-85-9.

Last update: Pavlíková Přecechtělová Jana, Mgr., Ph.D. (15.02.2025)
Syllabus -

Interaction of electromagnetic radiation with matter


1. Electromagnetic radiation: electromagnetic wave, electromagnetic spectrum, properties of electromagnetic waves.
2. Speed of propagation of electromagnetic radiation, light beam.
3. The Huygens principle.
4. Reflection of light.
5. Refraction of light, Abbe's refractometer.
6. Bending of light, dispersion of light.
7. X-ray diffraction, Bragg's law, X-ray crystallography.
8. Geometrical (ray) optics; mirrors, lenses.
9. Young's experiment.
10. Polarized light, circular polarimeter.
11. Quantum optics, photon energy.
12. Photoelectric effect.

Spectroscopy - principles


1. Spectroscopy. Spectrum.
2. Lambert-Beer's law, absorbance, transmittance.
3. Atomic spectroscopy: interpretation using Bohr's model of the atom, absorption spectra, emission spectra.
4. Introduction to molecular spectroscopy: electron, vibrational and rotational energy levels. Areas of the electromagnetic spectrum and spectroscopic techniques that use them.
5. UV-VIS spectroscopy: molecular orbitals, diagram of molecular orbitals in a hydrogen molecule, electron transitions, effects of substituents, conjugation and solvents, complementary colors.
6. Introduction to vibrational spectroscopy: potential and energy levels of harmonic and anharmonic oscillators.
7. Infrared spectroscopy (IR): selection rule for infrared transitions, normal modes of polyatomic molecules, characteristic vibration region and thumbprint region in infrared spectrum.
8. Raman spectroscopy: selection rule for Raman transitions, Stokes and anti-Stokes shift, selection rule for Raman transitions.
9. Luminescence spectroscopy: fluorescence, phosphorescence, Jablonski diagram, multiplicity of state.
10. NMR spectroscopy in the context of other spectroscopic methods - how is NMR different?

Ionic equilibria


1. Characteristics of electrolytes, degree of dissociation, Arrhenius theory. Arrhenius relation for the degree of dissociation.
2. Activity, activity coefficient, ionic strength of solutions, Debye-Hückel theory. Relations for calculating activity coefficients.
3. Dissociation of weak acids and bases, calculation of their pH, Ostwald's dilution law.
4. Hydrolysis of salts, hydrolytic constant, calculation of pH of salts.
5. Buffers, mechanism of action, Henderson - Hasselbalch equations.
6. Autoprotolysis of water, pH, acid-base theory (Arrhenius, Bronsted-Lowry, Lewis).
7. Amphoteric electrolytes, isoelectric point.
8. Acid-base indicators.
9. Solubility product, solubility of precipitates.

Phase interface phenomena


1. Solid and liquid phase interfaces.
2. Surface tension.
3. Adsorption in liquid interphase, surfactants, hydrophilic-lipophilic system.
4. Particle phase interface phenomena, influence of electrolytes, principles of chromatographic methods.
5. Positive and negative adsorption on liquid surfaces.
6. Interfacial tension.
7. Tension applied at the point of contact of the three phases.
8. Contact angle.
9. Expansion coefficient.

Electrochemistry, electrochemical methods


1. Conductivity of electrolytes, its concentration dependence, Kohlrausch's law of independent ion travel. Mobility of ions in an electric field.
2. Measurement of conductivity, use of conductivity measurements.
3. Formation of electrode potential. Nernst equation. Tabulation of electrode potentials.
4. Potentiometry and its applications.
5. Types of electrodes, Donnan potential.  
6. Galvanic cells and EMN measurements. Relationship between EMN° and Gibbs energy.
7. Electrolysis, Faraday's laws.
8. Flux of substances, diffusion (Fick's law).
9. Other transport processes in solutions, Nernst-Planck equation.

Colloidics, polymers


1. Types of dispersions and characterization of colloidal systems.
2. Lyophilic, lyophobic and associative colloids.
3. Optical, kinetic, and electrical properties of colloids.
4. Suspensions, interfacial properties, suspension formation, sedimentation.
5. Emulsions, types of emulsions, theory of their formation and stability.
8. Micelles, critical micellar concentration.
9. Sedimentation of particles.
10. Monomeric composition of polymers.
11. Structure of polymers and copolymers.
12. Crystalline and amorphous regions of polymers.
13. Physical properties of polymers.
14. Glass transition of polymers.
15. Solubility of polymers.

Non-equilibrium systems


1. Non-equilibrium, stationary and equilibrium systems.
2. Flow of a quantity, flux of a quantity, gradient of a quantity.
3. Transport processes.
4. Cross effects in systems where there is more than one gradient.
5. Diffusion in a liquid medium.
6. 1. Fick's law.
7. Stokes-Einstein equation.
8. 2. Fick's law.
9. Diffusion in non-liquid media.
10. Dissolution of a solid.
11. Thermodynamically unstable systems.

Biological membranes and the transport of substances across membranes


1. Membranes - structure, function.
2. Lipid bilayer.
3. Lipids in biological membranes.
4. Liposomes.
5. Lipid peroxidation.
6. Proteins in biological membranes.
7. Active and passive transport of substances across the membrane.
8. Simple diffusion across the membrane, diffusion of charged particles.
9. Partition coefficient.
10. Osmosis.
11. Donnan equilibrium.
12. Active and vesicular transport.
13. Secondary active transport.
14. Compartment system.

 

Principles of sensory perception

1. Sense perception, the general structure of the receptive system, senses.
2. Weber-Fechner law and Stevens law.
3. Sight. Ocular light refractive apparatus, accommodation, visual acuity.
4. Trichromatic theory of vision.
5. Molecular mechanism of vision, photochemical reaction.
6. Eye defects.
7. Sound, hearing, and theories of hearing.
8. Acoustic impedance.
9. Structure of the outer, middle, and inner ear.
10. Corti's organ.
11. Hearing defects.

 

Practical training

  1. Determination of the partition coefficient of a substance between two immiscible liquids.
  2. Potentiometric determination of the dissociation constant of a weak acid.
  3. Conductimetric determination of the dissociation constant of a weak acid or a weak base.
  4. Spectrophotometry: determination of the molar absorption coefficient.
  5. Optical measurement methods: refractometry and polarimetry.
Last update: Pavlíková Přecechtělová Jana, Mgr., Ph.D. (16.02.2025)
Learning outcomes -

The subject Physical chemistry builds on the knowledge and skills acquired in the courses General and Bioinorganic Chemistry and Physical Pharmacy I.

After completing the course, the learner will be able to use the following terms in the correct context: Electromagnetic radiation, wavelength, frequency, photon energy, Snell's law, refractometry, geometrical (beam optics), scattering and diffraction of radiation, polarized light, polarimetry, absorption, Lambert-Beer’s law, UV-VIS spectroscopy, atomic, infrared, Raman, and luminescence spectroscopy, surface tension, phase interface, adsorption, surfactant, interfacial tension, contact angle, spreading coefficient, degree of electrolyte dissociation, conductivity (specific, molar, limiting molar), conductometry, Arrhenius law for conductivity of weak electrolytes, Kohlrausch equation, activity, Ostwald's dilution law, Debye-Hückel limiting relation, ionic strength, autoprotolysis of water, dissociation of weak acids and bases, dissociation constant, pH, acid-base indicator, solubility, Henderson-Hasselbach equation, buffer solution, hydrolysis of salts, ampholyte, amphion, isoelectric point, reaction rate, reaction order, kinetics of the 0. , 1st and 2nd order, reaction rate constant, Arrhenius equation, activation energy, current, flux, and gradient of functions, diffusion, 1st and 2nd Fick's law, dissolution rate, thermodynamic instability, electrode action, electrode potential, Nernst’s equation, standard hydrogen electrode, standard reduction potential, spontaneous redox reactions, galvanic cell, potentiometry, electrode, membrane electrode, Donnan’s potential, flux to electrode, Nernst-Planck equation, electric double layer, colloidal system, specific surface, micelle, critical micellar concentration, zeta potential, sedimentation rate, polymer, copolymer, crystalline and amorphous substance, vitreous transition, cell membrane, lipid bilayer, liposome, lipid peroxidation, passive and active transport, partition coefficient, osmosis, exocytosis, endocytosis, compartment, receptor, sensory organs, light refractive apparatus of the eye, accommodative width, visual acuity, trichromatic theory of vision, photochemical reaction of rhodopsin, myopia, hyperopia, astigmatism, sound, transverse and longitudinal waves, sound intensity, sound intensity level, acoustic wave, acoustic impedance, structure of ear, organ of Corti, theory of hearing, hearing defects.

Learning outcomes:

Students based on the knowledge and skills acquired can:

Ø  define basic terms in physical pharmacy;

Ø  explain the principles of basic physicochemical measurement methods;

Ø  orient themselves in the complex systems and phenomena;

Ø  calculate and prepare a solution of a given concentration;

Ø  perform refractometry, polarimetry, UV-VIS spectrophotometry, conductometry, potentiometry (pH measurement), and determine the Nernst partition coefficient according to instructions;

Ø  calculate, in examples, the concentration of a substance, molar absorption coefficient, molar conductivity, dissociation degree, dissociation constant, pH using the Henderson-Hasselbach equation, Nernst’s partition coefficient;

Ø  evaluate, plot and interpret experimental data obtained using the methods described above;

Ø  design an appropriate method for determining the refractive index, specific optical rotation, concentration of a substance, conductivity of a solution, dissociation constant, pH of a solution, and partition coefficient of a substance.

 

Last update: Pavlíková Přecechtělová Jana, Mgr., Ph.D. (31.03.2025)
 
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