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The course Chemical Principles provides an initial overview of chemical disciplines (such as thermodynamics, spectroscopy, kinetics, chemical structure and bonding, electrochemistry) and their relationships. In-depth understanding of
individual disciplines is left for more specialized lectures in the later stage of studies. The position of chemistry within the broader range of natural sciences is shown, focusing on the overlaps with physics and biology. Chemical Principles set the stage for follow-up courses on chemical transformations, experimental and theoretical methods in chemistry. Special attention is devoted to the connection between microscopic and macroscopic understanding of phenomena. The course is built on topical blocks according to Syllabus with each of them consisting of lecture (2h) and workshop (3h). Poslední úprava: Uhlík Filip, prof. RNDr., Ph.D. (21.12.2025)
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- P. Atkins, L. Jones, L. Laverman: Chemical Principles - the Quest for Insight, 7th edition, W. H. Freeman and Company, New York, 2016 Poslední úprava: Uhlík Filip, prof. RNDr., Ph.D. (21.12.2025)
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Final mark is based on the oral examination. Students must first obtain the credit for the accompanying workshop. Poslední úprava: Uhlík Filip, prof. RNDr., Ph.D. (21.12.2025)
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Chemical Principles Poslední úprava: Uhlík Filip, prof. RNDr., Ph.D. (06.02.2026)
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Students will be able to explain all terms listed in the Syllabus including basic equations and definitions and will develop a molecular view of the corresponding phenomena that will allow them to describe all basic processes in chemistry and in overlaps with physics and biology. In particular, 1. What is Chemistry Apply dimensional analysis to convert between units of length, time, and energy. Estimate physical quantities to compare the relative scales of atomic, molecular, meso and macroscopic systems. 2. Matter and Energy Differentiate between elementary particles (bosons and fermions) based on their spin and statistical properties. Calculate nuclear binding energies using the mass-energy equivalence principle. Predict the stability of nuclei and identify decay modes for radioactive isotopes. 3. The Quantum World Explain the failure of classical physics to describe black body radiation and the photoelectric effect. Apply the de Broglie hypothesis to calculate the wavelength of particles. Interpret the physical significance of the wave function and probability density in the Schrödinger equation. Correlate the four quantum numbers of the Hydrogen atom to electron orbitals and the organization of the Periodic Table. 4. Chemical Bond Contrast the formation of covalent, polar, and ionic bonds using electron density arguments. Interpret Potential Energy Surfaces and dissociation curves to identify bond length and bond energy. Construct Molecular Orbital diagrams for diatomic molecules to predict bond order and magnetic properties. 5. Spectroscopy Relate specific regions of the electromagnetic spectrum (MW, IR, UV/Vis, NMR) to the corresponding molecular transitions (rotational, vibrational, electronic, nuclear spin). Analyze simple spectra to deduce information about molecular structure and composition. Distinguish between absorption, emission, scattering, and diffraction phenomena. 6. Kinetic Theory of Gases Apply the Maxwell-Boltzmann distribution to determine the fraction of particles above a certain energy threshold at a given temperature. Calculate transport properties, such as mean-free path and collision frequency, for ideal gases. Relate macroscopic gas properties (pressure, temperature) to microscopic particle behavior. 7. Reaction Kinetics Determine reaction orders and rate laws from experimental data. Calculate activation energy using the Arrhenius equation. Propose plausible reaction mechanisms and identify transition states for elementary and composite reactions. 8. Thermodynamics I Distinguish between intensive and extensive properties and state versus path functions. Apply the First Law of Thermodynamics to calculate work, heat, and internal energy changes. Calculate the enthalpy of reaction using Hess’s Law and standard formation/combustion enthalpies. 9. Thermodynamics II Analyze the efficiency of heat engines using the Carnot cycle model. Apply the Second Law of Thermodynamics to predict the spontaneity of physical and chemical processes. Calculate Gibbs Free Energy (ΔG) and Entropy changes (ΔS) for isothermal and adiabatic processes. 10. Phase Equilibrium Interpret single-component phase diagrams to identify stable phases and triple points. Apply the Gibbs Phase Rule to determine the degrees of freedom in a system. Calculate vapor pressure and solubility using Raoult’s Law and Henry’s Law. 11. Chemical Equilibrium Derive the equilibrium constant expression. Predict the direction of equilibrium shift in response to external change (pressure, temperature, concentration) using Le Chatelier’s principle. Solve for equilibrium concentrations in solution utilizing the reaction quotient. 12. Electrochemistry Balance redox reactions in acidic and basic aqueous solutions. Calculate cell potentials using the Nernst equation. Design a functional electrochemical cell, battery or electrolyzer and describe the electron flow and reactions. Poslední úprava: Uhlík Filip, prof. RNDr., Ph.D. (06.02.2026)
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