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Physical Pharmacy II - GF427
Title: Fyzikální farmacie II
Guaranteed by: Department of Biophysics and Physical Chemistry (16-16110)
Faculty: Faculty of Pharmacy in Hradec Králové
Actual: from 2025 to 2025
Semester: summer
Points: 0
E-Credits: 5
Examination process: summer s.:written
Hours per week, examination: summer s.:28/28, C+Ex [HS]
Capacity: unknown / unknown (unknown)
Min. number of students: unlimited
4EU+: no
Virtual mobility / capacity: no
Key competences:  
State of the course: taught
Language: Czech
Teaching methods: full-time
Level:  
Guarantor: doc. Mgr. Petra Pullmannová, Ph.D.
Co-requisite : GF408, GF425
Incompatibility : GF199
Interchangeability : GF199
Annotation -
Physical Pharmacy II is an interdisciplinary subject that uses the knowledge of physics, chemistry, electrochemistry and quantum mechanics to describe the properties of compounds at the molecular level. This subject follows the subject of Physical Pharmacy I. It provides students with the necessary theoretical and practical (within laboratories) background in the field and knowledge of the principles of physico-chemical measurement methodologies. It is a preparatory course, which aims to prepare students for related disciplines of a general scientific basis and purely pharmaceutical disciplines. Topics: Interaction of electromagnetic radiation with matter, Spectroscopy - principles, Ionic equilibria, Interfacial phenomena, Electrochemistry and electrochemical methods, Dispersion and polymers, Chemical kinetics, Non-equilibrium systems, Biological membranes and transport of substances across membranes, Principles of sensory perception.
Last update: GF427\5056461 (12.09.2025)
Course completion requirements -

Following conditions need to be fulfilled to gain the course credit:

  1. Completing all the tasks in the practical classes. Tasks missed for any reason need to be replaced in specified terms.
  2. Successful submission of protocols from completed tasks.
  3. Passing the credit test. The credit test consists of 2 computational tasks. To pass the test, a student needs to obtain at least 40% of the points.

The exam from Physical Pharmacy II takes the form of a written test. At least 60% of the points is required to pass the exam.

Last update: GF427\5056461 (12.09.2025)
Literature - Czech

Povinná:

  • Vacík, J. Obecná chemie. : Přírodovědecká fakulta Univerzity Karlovy, 2017, s. ISBN 978-80-7444-050-2.

Last update: Pullmannová Petra, doc. Mgr., Ph.D. (12.09.2025)
Syllabus -

Interaction of electromagnetic radiation with matter

1. Electromagnetic radiation: electromagnetic wave, electromagnetic spectrum, properties of electromagnetic radiation.
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. Young's experiment.
8. Diffraction of electromagnetic radiation. Bragg's law, principles of X-ray diffraction.
9. Geometrical (ray) optics; mirrors, lenses.
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 an 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 I and II

1. Activity, activity coefficient, ionic strength of solutions, Debye-Hückel theory. Formula for activity coefficients calculation.
2. Characteristics of electrolytes, degree of dissociation, Arrhenius theory. Arrhenius equation for the degree of dissociation.
3. Conductivity of electrolytes, its concentration dependence, Kohlrausch's law of independent ion travel. Mobility of ions in an electric field.
4. Measurement of conductivity, use of conductivity measurements.
5. Solubility product, solubility of precipitates.
6. Autoprotolysis of water, pH, acid-base theory (Arrhenius, Bronsted-Lowry, Lewis).
7. Dissociation of weak acids and bases, calculation of their pH, Ostwald's dilution law.
8. Hydrolysis of salts, hydrolytic constant, calculation of pH of salts.
9. Buffers, mechanism of action, Henderson - Hasselbalch equations.
10. Amphoteric electrolytes, isoelectric point.   
11. Acid-base indicators.  

Interfacial phenomena


1. Solid and liquid phase interfaces.
2. Surface tension.
3. Surface properties of the solid phase.
4. Adsorption/desorption of compounds in phase interphase, chemisorption, physical adsorption.
5. Linear, Freundlich, and Langmuir adsorption isotherm.
6. Surfactants, hydrophilic-lipophilic system.
7. Particle phase interface phenomena, influence of electrolytes, principles of chromatographic methods. 
8. Positive and negative adsorption on liquid surfaces.
9. Interfacial tension.
10. Tension applied at the point of contact of the three phases.
11. Contact angle. 
12. Expansion coefficient.

Electrochemistry I and II


1. Methods based on the electrode process: electrolysis, Faraday's laws, practical usage.
2. Formation of electrode potential. Nernst equation. Tabulation of electrode potentials. 
3. Galvanic cells and electromotive force (EMF) measurements. Relationship between EMF° and Gibbs energy. 
4. Methods based on the electrode process: Potentiometry and its applications. 
5. Types of electrodes, Donnan potential.
6. Flux of substances, diffusion (Fick's law), application in voltammetry.
7. Other transport processes in solutions (migration in an electric field, convection), Nernst-Planck equation. 

Dispersions, polymers

1. Classification of dispersion systems according to the number of phases, state of matter, particle size, and type of interaction (lyophilic, lyophobic, and associative).
2. Characterization of dispersion systems.
3. Types of particles forming dispersions.
4. Properties of dispersions (optical, kinetic, sedimentation, osmotic, viscosity, electrical, and electrokinetic properties).
5. Methods of characterizing dispersions (microscopy, interaction with electromagnetic radiation).
6. Sedimentation rate of particles in gravitational and centrifugal fields.
7. Micelles, critical micelle concentration.
8. Types of micelles.
9. Nernst potential, zeta potential.
10. Dispersion separation techniques (filtration, dialysis, size exclusion chromatography).
11. Definition of terms: monomer, polymer, oligomer, homopolymer, copolymer, and types of copolymers.
12. Structure and shape of polymers and copolymers.
13. Crystalline and amorphous state of polymers and copolymers.
14. Physical properties of polymers and copolymers.
15. Thermotropic behaviour, melting and glass transition.
16. Solubility of polymers and copolymers.

Chemical kinetics

1. Average and instantaneous rate of chemical reaction, units of rate, rate constant and its units, partial and overall order of reaction.
2. Zero-order reaction: differential and integrated form of the rate equation, graph of instantaneous concentration and rate versus time, graphical determination of the rate constant, calculation and graphical determination of the reaction half-life.
3. First-order reaction: differential and integrated form of the rate equation, graph of the dependence of instantaneous concentration, instantaneous rate, and logarithm of instantaneous concentration on time, graphical determination of the rate constant, calculation and graphical determination of the reaction half-life.  
4. Second-order reaction: differential and integrated form of the rate equation, graph of the dependence of instantaneous concentration, instantaneous rate, and reciprocal instantaneous concentration on time, graphical determination of the rate constant, calculation and graphical determination of the reaction half-life.
5. Dependence of reaction rate on temperature, Arrhenius equation for rate constant: exponential and linearized form, activation energy, reaction coordinate, rate-determining step.
6. Kinetically and thermodynamically controlled reactions.

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. 1st Fick's law.
7. Stokes-Einstein equation.
8. 2nd Fick's law.
9. Factors affecting the rate of dissusion.
10. Diffusion in non-liquid media.
11. Dissolution of a solid. Solvation.
12. 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.

 

Laboratory 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. Conductometric 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: GF427\5056461 (12.09.2025)
Learning resources - Czech

https://intranet.faf.cuni.cz/Studijni-materialy/KBFCH/?path=fyzik%c3%a1ln%c3%ad+chemie

E-learning Moodle: Fyzikální chemie

https://dl1.cuni.cz/course/view.php?id=3610

Vacík, J. Obecná chemie; Přírodovědecká fakulta Univerzity Karlovy, 2017.

Last update: GF427\5056461 (12.09.2025)
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 for rate constant, 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: GF427\5056461 (12.09.2025)
 
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