Bases of chemistry 2 WF-OB-PCH2
Classical chemical concepts and laws. Stoichiometry of chemical reactions. Models of atoms. Perfect gas model versus real gases. Chemical reactions with elements of thermodynamics. Chemical equilibrium. Acids and bases according to different theories. Redox reactions and electrochemical cells. Quantum numbers, atomic orbitals. Molecular orbitals as linear combinations of atomic orbitals. Structure of the periodic table and consequent properties of elements, e.g. electronegativity of elements, polarity of chemical bonds. Hybridisation as an effective tool for describing the structure of multi-atomic molecules. Examples of the structure of molecules for basic types of hybridisation : sp3, sp, sp2, d2sp3. Types of chemical bonds. Ways of expressing concentrations of solutions: molar fraction, weight fraction, percentage concentration, molar concentration, conversion of concentrations, example tasks.
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Term 2021/22_Z:
None |
Term 2022/23_Z:
None |
Term 2023/24_Z:
General and physical chemistry: principles of classification and nomenclature in inorganic chemistry. Structure of matter - Elementary particles and their structure, atomic nucleus. Electron structure of the atom. Chemical bonding - Atomic bonds and intermolecular forces. Chemical thermodynamics and thermochemistry. Chemical kinetics. Chemical statics. Chemical equilibrium. Gases - perfect and real gases. Gas laws. Liquids - Division and properties. Solution theory: non-electrolyte solutions. Electrolytes. Theory of acids and bases. Electrochemistry. Inorganic chemistry: periodicity in the behaviour of elements, periodicity law. Groups and periods. Group properties. Occurrence, basic properties and reactions of selected elements. Basic stoichiometry. Chemical equations. Expression of concentrations. Oxidation and reduction reactions. |
Term 2024/25_Z:
General and physical chemistry: principles of classification and nomenclature in inorganic chemistry. Structure of matter - Elementary particles and their structure, atomic nucleus. Electron structure of the atom. Chemical bonding - Atomic bonds and intermolecular forces. Chemical thermodynamics and thermochemistry. Chemical kinetics. Chemical statics. Chemical equilibrium. Gases - perfect and real gases. Gas laws. Liquids - Division and properties. Solution theory: non-electrolyte solutions. Electrolytes. Theory of acids and bases. Electrochemistry. Inorganic chemistry: periodicity in the behaviour of elements, periodicity law. Groups and periods. Group properties. Occurrence, basic properties and reactions of selected elements. Basic stoichiometry. Chemical equations. Expression of concentrations. Oxidation and reduction reactions. |
(in Polish) E-Learning
(in Polish) Grupa przedmiotów ogólnouczenianych
Subject level
Learning outcome code/codes
Type of subject
Course coordinators
Learning outcomes
KNOWLEDGE: The student knows and understands the basic patterns of chemical, physical, and knows their application. Describes the physical phenomena occurring chemical in nature. Demonstrates knowledge of basic conceptual categories and terminology in the area of life sciences and the development of these disciplines are used in their research methods. The student knows the hazards that can occur in the chemical laboratory. He knows and understands the basic techniques of analytical chemistry.
SKILLS: Students can apply basic chemical formulas accounting tasks. Interpret the observations and measurements, and on the basis of draw correct conclusions. Puts the correct hypothesis about the reasons for the situation / threat based on logical grounds. Student is able to keep you in the chemical laboratory, know how to use basic laboratory glass, can build a basic set of markings / analysis.
COMPETENCE: Able to work independently demonstrating initiative and independence in activities and interact effectively in teamwork, performing in her various roles. He is responsible for entrusted equipment and other own work. Student is prepared for practical activities in the field of chemistry in the laboratory.
ECTS [1 ECTS = 30(25) h]:
participating in lecture: 30 h
participating in auditorium classes: 30 h
preparing for exams: 30 h
suma godzin: 90 [90/30(25)=3]
number of ECTS: 3
Assessment criteria
Written examination covering general topics and calculation tasks. A prerequisite for admission to the examination is the successful completion of laboratory exercises.
Bibliography
1. Loretta Jones, Peter W. Atkins: „Chemia ogólna. Cząsteczki, materia, reakcje”, Wyd. PWN, 2009.
2. P. A. Cox: „Krótkie wykłady, Chemia nieorganiczna” Wydawnictwo Naukowe PWN, Warszawa 2003;
3. A.G. Whittaker, A. R. Mount, M. R. Heal: „Krótkie wykłady, Chemia fizyczna” Wydawnictwo Naukowe PWN, Warszawa 2003;
4. D. Kealey, P.J. Haines: „ Krótkie wykłady - Chemia analityczna” Wydawnictwo Naukowe PWN, Warszawa 2005;
5. Adam Bielański: „Podstawy chemii nieorganicznej” Wydawnictwo Naukowe PWN, Warszawa, 1997, 2002;
6. J. D. Lee: „Zwięzła chemia nieorganiczna” Wydawnictwo Naukowe PWN, Warszawa, 1997;
7. Peter Wiliam Atkins: „Chemia fizyczna” Wydawnictwo Naukowe PWN, Warszawa, 2002;
8. Jerzy Minczewski, Zygmunt Marczenko „Chemia analityczna”, PWNchemiczne”
|
Term 2021/22_Z:
None |
Term 2022/23_Z:
None |
Term 2023/24_Z:
1. Loretta Jones, Peter W. Atkins: „Chemia ogólna. Cząsteczki, materia, reakcje”, Wyd. PWN, 2009. |
Term 2024/25_Z:
1. Loretta Jones, Peter W. Atkins: „Chemia ogólna. Cząsteczki, materia, reakcje”, Wyd. PWN, 2009. |
Notes
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Term 2021/22_Z:
None |
Term 2022/23_Z:
None |
Term 2023/24_Z:
Knowledge of basic chemistry |
Term 2024/25_Z:
Knowledge of basic chemistry |
Additional information
Information on level of this course, year of study and semester when the course unit is delivered, types and amount of class hours - can be found in course structure diagrams of apropriate study programmes. This course is related to the following study programmes:
Additional information (registration calendar, class conductors, localization and schedules of classes), might be available in the USOSweb system: