Acquire the fundamental experimental and theoretical concepts of general chemistry
teacher profile teaching materials
2. CHEMICAL BONDS. Ionic bond. Covalent bond: and bonds. Polyatomic molecules: molecular structure. Hybridization and resonance. Molecular orbital. Metallic bond. Intermolecular forces.
3. NOMENCLATURE AND CHEMICAL REACTIONS. Oxides, hydroxides, acids, salts, ions. Balancing chemical reactions: redox reactions.
4. STATES OF AGGREGATION. Gas state, ideal gas law. Solid state: ionic, covalent, molecular and metallic solids. Conductors, semiconductors, insulators. Liquid and amorphous states. Phase transitions and phase diagrams.
5. SOLUTIONS. Concentration, colligative properties; electrolyte solutions.
6. THERMODYNAMICS. Matter, energy, heat, first and second principles; enthalpy, entropy, free energy.
7. CHEMICAL EQUILIBRIUM. Equilibrium constant and free energy. Gas-phase and heterogeneous equilibria. Le Chatelier’s principle. Van’t Hoff equation.
8. EQUILIBRIA IN SOLUTION. Acid-base equilibria: acids and bases, pH, dissociation constant, polyprotic acids, hydrolysis, buffers. Acid-base titrations and pH indicators. Solubility equilibria: solubility product, common ion effect.
9. ELECTROCHEMISTRY. Batteries, electrode potentials, Nernst’s equation. Electrolysis.
10. CHEMICAL KINETICS. Reaction speed, speed constant. Influence of the temperature on the reaction speed: Arrhenius equation. Catalysts.
Numerical exercises on all the listed subjects.
Programme
1. ATOMIC THEORY AND ATOMIC STRUCTURE. Atoms, molecules, moles; atomic and molecular weight. Atomic models: Rutheford, Bohr. Quantum theory, quantum numbers and energy levels. Polyelectronic atoms; periodic system.2. CHEMICAL BONDS. Ionic bond. Covalent bond: and bonds. Polyatomic molecules: molecular structure. Hybridization and resonance. Molecular orbital. Metallic bond. Intermolecular forces.
3. NOMENCLATURE AND CHEMICAL REACTIONS. Oxides, hydroxides, acids, salts, ions. Balancing chemical reactions: redox reactions.
4. STATES OF AGGREGATION. Gas state, ideal gas law. Solid state: ionic, covalent, molecular and metallic solids. Conductors, semiconductors, insulators. Liquid and amorphous states. Phase transitions and phase diagrams.
5. SOLUTIONS. Concentration, colligative properties; electrolyte solutions.
6. THERMODYNAMICS. Matter, energy, heat, first and second principles; enthalpy, entropy, free energy.
7. CHEMICAL EQUILIBRIUM. Equilibrium constant and free energy. Gas-phase and heterogeneous equilibria. Le Chatelier’s principle. Van’t Hoff equation.
8. EQUILIBRIA IN SOLUTION. Acid-base equilibria: acids and bases, pH, dissociation constant, polyprotic acids, hydrolysis, buffers. Acid-base titrations and pH indicators. Solubility equilibria: solubility product, common ion effect.
9. ELECTROCHEMISTRY. Batteries, electrode potentials, Nernst’s equation. Electrolysis.
10. CHEMICAL KINETICS. Reaction speed, speed constant. Influence of the temperature on the reaction speed: Arrhenius equation. Catalysts.
Numerical exercises on all the listed subjects.
Core Documentation
P.W.Atkins, L. Jones; CHEMISTRY: MOLECULES, MATTER, AND CHANGEType of delivery of the course
Frontal lessons and numerical exercises. Lessons will not be recorded. Two laboratory exercises are plannedAttendance
Attendance of lessons in class or via teams depending on the situation related to the health emergency from COVID-19Type of evaluation
The exam consists of a written test followed by an oral exam. The written test consists of 5 exercises; 6 points are awarded for each year. The written test is valid for two oral exams; subsequently it expires. Students who attend the lessons can participate to two written tests during the course