651-2018/02 – General and Inorganic Chemistry (OACH)
| Gurantor department | Department of Chemistry and Physico-Chemical Processes | Credits | 6 |
| Subject guarantor | Ing. Silvie Vallová, Ph.D. | Subject version guarantor | Ing. Silvie Vallová, Ph.D. |
| Study level | undergraduate or graduate | Requirement | Choice-compulsory type B |
| Year | 1 | Semester | winter |
| | Study language | English |
| Year of introduction | 2022/2023 | Year of cancellation | |
| Intended for the faculties | USP, FS | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
- Acquirement of the basic terms in the field of the atomic structure and chemical bonding
- Knowledge of the relationship between the properties of elements and periodicity of the electron shell build-up
- Knowledge of the patterns of the chemical reactions course
- Arrangement and enumeration of chemical equations, performing stoichiometric calculations
- Knowledge of the properties and application of the most important elements and their compounds
- Basic operations in the laboratory, preparation of inorganic compounds
Teaching methods
Lectures
Tutorials
Experimental work in labs
Summary
Compulsory literature:
Recommended literature:
1. http://www.highered.mcgraw-hill.com/sites/0073656011/
Way of continuous check of knowledge in the course of semester
Credit: tests - chemical calculations.
Final written and oral exam.
E-learning
Other requirements
There are no additional requirements for students.
Prerequisities
Subject has no prerequisities.
Co-requisities
Subject has no co-requisities.
Subject syllabus:
Lectures:
1. Basic terms. Composition of systems, substance quantity, electronegativity, oxidation number.
2. Structure of atoms - atomic nucleus, radioactivity, mononuclear, binuclear nuclear reactions.
3. Structure of atoms - electron shell. Construction principle, electronic configurations.
4. Types of ties. The formation of a chemical bond from the point of view of quantum mechanics. Hybridization and structure of molecules.
5. Periodic table. Metallic character, atomic radii, ionization energy, density, melting points.
6. Group states of substances. Phase diagram of a single-component system. Laws of ideal gases.
7. Dispersion systems. Solutions, Raoult's law, Henry's law. Atomic, metallic, ionic, molecular substances.
8. Division of chemical reactions. Chemical kinetics. Factors influencing the rate of chemical reactions.
9. Energy changes during chemical reactions. Internal energy, enthalpy, entropy, Gibbs energy.
10. Chemical equilibrium. Effect of temperature, pressure and concentration on the composition of the equilibrium mixture.
11. Electrolytic dissociation, ionic equations. Neutralization, precipitation reactions, hydrolysis, displacement of acids and bases.
12. Acid-base reactions. Scales of acidity and basicity in aqueous solutions and ionic melts.
13. Oxidation-reduction reactions, electrode potential. Electrochemical voltage series of metals.
14. Galvanic cells primary, secondary. Electrolysis of aqueous solutions and melts.
15. Hydrogen, oxygen, water.
16. s1 and s2 elements – general properties. Sodium, potassium, magnesium, calcium.
17. p1, p2, p3 elements - general properties. Aluminium, carbon, silica, tin, lead, nitrogen, phosphorus.
18. p4, p5, p6 elements - general properties. Sulphur, fluorine, chlorine.
19. d elements. Transition metals complexes, structure, bonding, spectroscopic and magnetic properties. Coordination equilibria and reaction mechanisms.
20. Titanium, zirconium, chromium, molybdenum, tungsten, manganese, iron, zinc, mercury, copper, silver, gold.
computational exercise:
• Inorganic nomenclature (binary and pseudobinary compounds, acids).
• Inorganic nomenclature (salts, crystal hydrates, complex compounds).
• Basic concepts (quantity of substances, molar quantities).
• Composition of multicomponent systems (mass, molar and volume fraction, molar concentration).
• Stoichiometric calculations according to the chemical formula (determination of empirical composition, calculation of element mass).
• Laws of ideal gases (Calculations from the equation of state of an ideal gas).
• Stoichiometric calculations from the chemical equation (solids, gases under normal conditions).
• Stoichiometric calculations from the chemical equation (substances in solution, gases under general conditions).
• Preparation of solutions by dilution and mixing (balance in solutions, mixing equations).
• Electrolyte solutions (electrolytic dissociation, calculation of concentration of ions in solutions, calculation of pH).
• Ionic reactions and equations (neutralization, precipitation, hydrolysis, dissolution, displacement).
• Oxidation-reduction reactions (calculation of oxidation-reduction equations, oxidizing and reducing agent).
practical excercises:
• Work safety and organization in the laboratory.
• Basic laboratory techniques. Separation of a heterogeneous mixture.
• Determination of the molar mass of carbonates. Sublimation of benzoic acid.
• Determination of the crystal hydrate formula. Acid-base (neutralization) titration.
• Electrochemical voltage series of metals. Properties of transition metal hydroxides.
• Determination of the molar mass of oxygen. Determination of CaCO3 in technical limestone.
• Preparation of chrome green. Preparation of chrome yellow.
• Preparation of insoluble carbonates by precipitation. Determination of the molar mass of metals.
• Preparation and dilution of solutions. Preparation of sodium chloride by neutralization.
• Acid-base nature of solutions. Strength of acids and bases.
• Precipitation reactions. Preparation of emerald (Guinet) green.
• Oxidation and reduction.
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction
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