General and Inorganic Chemistry 1

Data

Official data in SubjectManager for the following academic year: 2022-2023

Topic

The course includes selected General Chemistry topics that are essential for pharmacy students to study the Chemistry-related subjects (eg, Pharmaceutical Chemistry, Pharmaceutical Technology) in the higher semesters.

Lectures

• 1. Classification of matter. Atomic structure. Electron configuration and periodicity. The periodic table. Periodic properties. - Dr. Kunsági-Máté Sándor
• 2. Classification of matter. Atomic structure. Electron configuration and periodicity. The periodic table. Periodic properties. - Dr. Kunsági-Máté Sándor
• 3. Structure of molecules. Chemical bonding. Chemical bonding theories. Valence bond theory. Hybrid orbitals. Molecular orbital theory. Moleculas geometry. - Dr. Kunsági-Máté Sándor
• 4. Structure of molecules. Chemical bonding. Chemical bonding theories. Valence bond theory. Hybrid orbitals. Molecular orbital theory. Moleculas geometry. - Dr. Kunsági-Máté Sándor
• 5. States of matter. The gaseous state. Gas laws. Intermolecular forces. The liquid state. The solid state. Phase transitions. Phase diagrams. - Dr. Kunsági-Máté Sándor
• 6. States of matter. The gaseous state. Gas laws. Intermolecular forces. The liquid state. The solid state. Phase transitions. Phase diagrams. - Dr. Kunsági-Máté Sándor
• 7. Water and the aqueous solutions. Dissolution of gases, liquids and solids in liquids. Types of electrolytes. Electrolytic dissociation, degree of dissociation, conductivity, and their relationships. - Dr. Kunsági-Máté Sándor
• 8. Water and the aqueous solutions. Dissolution of gases, liquids and solids in liquids. Types of electrolytes. Electrolytic dissociation, degree of dissociation, conductivity, and their relationships. - Dr. Kunsági-Máté Sándor
• 9. Chemical kinetics. Reaction rates. The collision theory. Rate laws and reaction mechanisms. - Dr. Kunsági-Máté Sándor
• 10. Chemical kinetics. Reaction rates. The collision theory. Rate laws and reaction mechanisms. - Dr. Kunsági-Máté Sándor
• 11. Chemical equilibria. LeChatelier's principle. Protolytic reactions I. Ionization of water. The pH scale. - Dr. Lóránd Tamás
• 12. Chemical equilibria. LeChatelier's principle. Protolytic reactions I. Ionization of water. The pH scale. - Dr. Lóránd Tamás
• 13. Protolytic reactions II. Acid-base concepts. Acid-base equilibria. - Dr. Lóránd Tamás
• 14. Protolytic reactions II. Acid-base concepts. Acid-base equilibria. - Dr. Lóránd Tamás
• 15. Buffers. Physiological buffer systems. Acid-base titrations. - Dr. Lóránd Tamás
• 16. Buffers. Physiological buffer systems. Acid-base titrations. - Dr. Lóránd Tamás
• 17. Heterogeneous equilibria. Thermodynamics and equilibrium. - Dr. Kunsági-Máté Sándor
• 18. Heterogeneous equilibria. Thermodynamics and equilibrium. - Dr. Kunsági-Máté Sándor
• 19. Colligative properties. Colloids. - Dr. Kunsági-Máté Sándor
• 20. Colligative properties. Colloids. - Dr. Kunsági-Máté Sándor
• 21. Thermochemistry. Basic thermodynamics. - Dr. Kunsági-Máté Sándor
• 22. Thermochemistry. Basic thermodynamics. - Dr. Kunsági-Máté Sándor
• 23. Electrochemistry I. - Dr. Kunsági-Máté Sándor
• 24. Electrochemistry I. - Dr. Kunsági-Máté Sándor
• 25. Electrochemistry II. - Dr. Kunsági-Máté Sándor
• 26. Electrochemistry II. - Dr. Kunsági-Máté Sándor
• 27. Complex ions and coordination compounds I. Structure and isomerism. - Dr. Perjési Pál
• 28. Complex ions and coordination compounds I. Structure and isomerism. - Dr. Kunsági-Máté Sándor

Practices

• 1. Laboratory safety. Introduction and handover of laboratory equipment. Basic principles. Classification of matter. Naming simple compounds: Acids, bases and salts. Weighing.
• 2. Laboratory safety. Introduction and handover of laboratory equipment. Basic principles. Classification of matter. Naming simple compounds: Acids, bases and salts. Weighing.
• 3. Laboratory safety. Introduction and handover of laboratory equipment. Basic principles. Classification of matter. Naming simple compounds: Acids, bases and salts. Weighing.
• 4. Basic principles of calculations I: Concentrations. Delivering liquids. Preparation of solutions. Measuring density.
• 5. Basic principles of calculations I: Concentrations. Delivering liquids. Preparation of solutions. Measuring density.
• 6. Basic principles of calculations I: Concentrations. Delivering liquids. Preparation of solutions. Measuring density.
• 7. Basic principles of calculations II: Concentrations. Purification of inorganic compounds I.: Decantation, Filtration. Recrystallisation. Purification of alum by recrystallisation I, Dilution of solutions.
• 8. Basic principles of calculations II: Concentrations. Purification of inorganic compounds I.: Decantation, Filtration. Recrystallisation. Purification of alum by recrystallisation I, Dilution of solutions.
• 9. Basic principles of calculations II: Concentrations. Purification of inorganic compounds I.: Decantation, Filtration. Recrystallisation. Purification of alum by recrystallisation I, Dilution of solutions.
• 10. Basic principles of calculations III: Concentrations. Purification of inorganic compounds II.: Destillation, Sublimation.
• 11. Basic principles of calculations III: Concentrations. Purification of inorganic compounds II.: Destillation, Sublimation.
• 12. Basic principles of calculations III: Concentrations. Purification of inorganic compounds II.: Destillation, Sublimation.
• 13. Basic principles of calculations III: Stochiometry. Purification of inorganic compounds III. Desalination of water. Extraction.
• 14. Basic principles of calculations III: Stochiometry. Purification of inorganic compounds III. Desalination of water. Extraction.
• 15. Basic principles of calculations III: Stochiometry. Purification of inorganic compounds III. Desalination of water. Extraction.
• 16. Basic principles of calculations IV. Stochiometry. Basic thermodynamics. Hess?s law. Observation of thermal decompositions. Determination of melting point. Determination
• 17. Basic principles of calculations IV. Stochiometry. Basic thermodynamics. Hess?s law. Observation of thermal decompositions. Determination of melting point. Determination
• 18. Basic principles of calculations IV. Stochiometry. Basic thermodynamics. Hess?s law. Observation of thermal decompositions. Determination of melting point. Determination
• 19. Basic principles of chemical kinetics. Observation of reaction rates. Landolt-reaction. Oscillating reactions.
• 20. Basic principles of chemical kinetics. Observation of reaction rates. Landolt-reaction. Oscillating reactions.
• 21. Basic principles of chemical kinetics. Observation of reaction rates. Landolt-reaction. Oscillating reactions.
• 22. Electrolytic dissociation. Weak and strong electrolytes. Preparation of boric acid from borax I., Preparation of potassium dihydrogenphosphate I.
• 23. Electrolytic dissociation. Weak and strong electrolytes. Preparation of boric acid from borax I., Preparation of potassium dihydrogenphosphate I.
• 24. Electrolytic dissociation. Weak and strong electrolytes. Preparation of boric acid from borax I., Preparation of potassium dihydrogenphosphate I.
• 25. Acid-base equilibrium I. Arrhenius concept, Brönsted-Lowry concept, Lewis concept.
• 26. Acid-base equilibrium I. Arrhenius concept, Brönsted-Lowry concept, Lewis concept.
• 27. Acid-base equilibrium I. Arrhenius concept, Brönsted-Lowry concept, Lewis concept.
• 28. Acid-base equilibrium II. Hydrolysis of ions. Buffers. Observation of hydrolysis of salts Demonstration of buffer capacity.
• 29. Acid-base equilibrium II. Hydrolysis of ions. Buffers. Observation of hydrolysis of salts Demonstration of buffer capacity.
• 30. Acid-base equilibrium II. Hydrolysis of ions. Buffers. Observation of hydrolysis of salts Demonstration of buffer capacity.
• 31. Acid-base equilibrium III. Acid-base titrations Determination of concentration of monoprotic acid solutions (hydrochloric acid, acetic acid) by titration.
• 32. Acid-base equilibrium III. Acid-base titrations Determination of concentration of monoprotic acid solutions (hydrochloric acid, acetic acid) by titration.
• 33. Acid-base equilibrium III. Acid-base titrations Determination of concentration of monoprotic acid solutions (hydrochloric acid, acetic acid) by titration.
• 34. Heterogenous equilibrium. Solubility calculations. Qualitative comparison of solubility products.
• 35. Heterogenous equilibrium. Solubility calculations. Qualitative comparison of solubility products.
• 36. Heterogenous equilibrium. Solubility calculations. Qualitative comparison of solubility products.
• 37. Redox reactions I. Oxidation state. Important oxidizing and reducing agents. Observation of oxidation-reduction reactions. Preparation of copper(I) oxide through copper(I) chloride
• 38. Redox reactions I. Oxidation state. Important oxidizing and reducing agents. Observation of oxidation-reduction reactions. Preparation of copper(I) oxide through copper(I) chloride
• 39. Redox reactions I. Oxidation state. Important oxidizing and reducing agents. Observation of oxidation-reduction reactions. Preparation of copper(I) oxide through copper(I) chloride
• 40. Redox reactions II. Electrodes, electrochemical cells, electrolysis. Redox titrations
• 41. Redox reactions II. Electrodes, electrochemical cells, electrolysis. Redox titrations
• 42. Redox reactions II. Electrodes, electrochemical cells, electrolysis. Redox titrations

Seminars

Reading material

Obligatory literature

Ebbing D.D., Gammon S.D.: General Chemistry, Houghton Miffilin Co., Boston, 2009

Literature developed by the Department

Almási A., Kuzma M., Perjési P.: General and Inorganic Chemistry - Laboratory Techniques and Practices, Electronic educational material, University of Pécs, 2014

Notes

Recommended literature

en.wikibooks.org/wiki/General_Chemistry

Conditions for acceptance of the semester

Acknowledgement of the course is in accord with the Code of Studies and Examinations. Participation is both the lectures and the practices is obligatory. Maximum three absences can be accepted both from lectures and practices. Two compulsory midterm tests (on the topics of the lectures and practices) will be written during the semester on the 7th and the 12th weeks. One of the test result should be above 60%. One re-take chance is allowed at the 14th weak of the semester. Students have to write at least four mini-tests on the practices. The average of the results must be at least 50%. The practical work (results of the written tests and the experimental work) is evaluated by a practical grade. Satisfactory (2) evaluation is the minimum requirement of acknowledgement of the semester.

Mid-term exams

Making up for missed classes

There is no oppurtunity to make up missed classes (lectures and practices).

Exam topics/questions

Written test covering the topics of the lectures and the laboratory practices. Written exam covering the topics of the lectures and the laboratory practices. The result of the first part of the written exam (Minimum Written Test) should be at least 80%. In the case of the third (“C”) exam the written exam is evaluated regardless the result of the Minimum Written Test. The list of the possible questions of the Minimum Written Test is announced on the Neptun system. The result of the written exam must be above 60%. The final grade is based on results of the midterm tests and the written exam. Maximum contribution of the results of the midterm tests to the total score of the written exam is 25%. Participation on the first exam is compulsory. The result of the written test must be above 60%. The final grade is based on results of the midterm tests and the written test. Maximum contribution of the results of the midterm tests to to the total score of the written test can be 25%. Participation on the first exam is compulsory.

Examiners

• Dr. Kunsági-Máté Sándor
• Dr. Perjési Pál

Instructor / tutor of practices and seminars

• Dr. Kiss László
• Dr. Kulcsár Győző Kornél
• Dr. Kunsági-Máté Sándor