CH2BP_2P6P Inorganic Chemistry 1

Faculty of Education
Spring 2014
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. Petr Sládek, CSc.
Department of Physics, Chemistry and Vocational Education – Faculty of Education
Contact Person: Mgr. Bc. Lucie Viková
Supplier department: Department of Physics, Chemistry and Vocational Education – Faculty of Education
Timetable
Mon 15:45–16:30 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
Course objectives
At the end of this course, student should be able to: understand and be able to explains structure and reactivity basic relationships of inorganic chemistry; use data to inorganic chemistry problem solutions independently; make reasoned decisions about reactivity of inorganic compounds; formulate a reasoned differential diagnosis for products deduction of similar reactions; interpret inorganic compounds characteristics.
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.
  • 8. Atom, its composition, elementary particles.
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;
colloquium - written part (test from calculations - 60 % of correct calculations) and oral part (70 % of correct answers is needed to pass).
Language of instruction
Czech
Further Comments
Study Materials
The course is taught annually.
The course is also listed under the following terms Spring 2004, Spring 2005, Spring 2006, Spring 2007, Spring 2008, Spring 2009, Spring 2010, Spring 2011, Spring 2012, Spring 2013, Spring 2015, Spring 2016, Spring 2017, Spring 2018.
  • Enrolment Statistics (Spring 2014, recent)
  • Permalink: https://is.muni.cz/course/ped/spring2014/CH2BP_2P6P