PdF:CH2BP_2P6P Inorganic Chemistry 1 - Course Information
CH2BP_2P6P Inorganic Chemistry 1
Faculty of EducationSpring 2010
- Extent and Intensity
- 1/0/0. 2 credit(s). Type of Completion: k (colloquium).
- Teacher(s)
- doc. RNDr. Luděk Jančář, CSc. (lecturer)
- Guaranteed by
- doc. RNDr. Luděk Jančář, CSc.
Department of Physics, Chemistry and Vocational Education – Faculty of Education
Contact Person: Helena Pelcová - Timetable
- Tue 7:55–8:40 učebna 7
- Prerequisites
- Knowledge of inorganic chemistry on secondary school.
- Course Enrolment Limitations
- The course is also offered to the students of the fields other than those the course is directly associated with.
- fields of study / plans the course is directly associated with
- Lower Secondary School Teacher Training in Chemistry (programme PdF, B-SPE)
- Course objectives
- Main objectives can be summarised as follows:
to give a systematic overview of chosen chemical elements and their compounds;
to introduce into foundations of chemical calculations. - Syllabus
- 1. Basic nomenclature rules and norms of inorganic chemistry. Periodic system of elements – history, the present and future.
- 2. Chemisty of non-transition elememnts – general charactization. Hydrogen and its compounds.
- 3. Carbon and its inorganic compounds. Silicon and its compounds. Germanium, tin, lead and their compounds.
- 4. Oxygen, properties, preparation and production. Characteristics and properties of oxides and oxoanions.
- 5. Solutions, their types, expression of solution concentrations, electrolyte. Dissotiation step of the electrolyte, strong and weak electrolytes, dissotiation constant of the weak electrolytes. Solubility. Influence factors to matters solubility: saturated solution. Influence of temperature and pressure to the matters solubility. Henry’s law, constant of solubility.
- 6. Acid/base equilibria and reactions. Acid/base theories: Arrhenius, Brönsted. Brönsted’s theory: conjugation pair. Autoprotolyse, neutralization, ion product of water, pH of strong and weak acids and bases, amfoteric matter. Buffers – function, composition, pH (Henderson-Hasselbach‘s equation). Hydrolyses, pH of hydrolysing salts. Acid/base theories: Lewis, Pearson.
- 7. Basic chemical calculations.
- Literature
- KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1985, 591 s. info
- Teaching methods
- lectures
theoretical preparation - Assessment methods
- colloquium;
oral exam. - Language of instruction
- Czech
- Further comments (probably available only in Czech)
- Study Materials
The course is taught annually.
General note: Podmínky pro připuštění ke zkoušce: Zápočet z povinného předmětu CH2BP_1P5S a volitelného předmětu CH2BP_2W6S (pokud si ho student zapsal).
- Enrolment Statistics (Spring 2010, recent)
- Permalink: https://is.muni.cz/course/ped/spring2010/CH2BP_2P6P