* Load is given in academic hour (1 academic hour = 45 minutes)
COURSE GOALS: Systematization of basic chemical concepts about the properties of matter at the macroscopic, particles, and symbolic level. Integration of existing and new knowledge in a conceptual entity.
LEARNING OUTCOMES AT THE LEVEL OF THE PROGRAMME:
1. KNOWLEDGE AND UNDERSTANDING
1.2. demonstrate a thorough knowledge and understanding of the fundamental concepts in chemistry
1.4. demonstrate a thorough knowledge and understanding of the most important chemistry laws and theories
2. APPLYING KNOWLEDGE AND UNDERSTANDING
2.2. describe important aspects of chemical change
2.3. apply stoichiometry
5. LEARNING SKILLS
5.1.search for and use professional literature as well as any other sources of relevant information
LEARNING OUTCOMES SPECIFIC FOR THE COURSE:
1. Organize knowledge into conceptual units.
2. Formulate the problem based on the data and the set of conditions (stoichiometry).
3. Explain the physical and chemical changes in terms of scientific concepts and principles.
4. Explain the meaning of the chemical equation (qualitatively and quantitatively).
5. Distinguish three basic types of chemical bonds (ionic, covalent and metallic).
6. Predict and analyze the molecular structure and its properties.
7. Explain at the particle's level dissolving processes, and properties of the solutions.
8. Explain the influence of various factors on the chemical equilibrium.
9. Predict pH of aqueous solutions of certain substances.
10. Explain the difference between galvanic and electrolytic cell.
1st - 3rd week: The components of matter, physical and chemical properties of matter, states of matter and phase changes, the fundamental chemical laws and concepts, atomic theory and structure of atoms, types of chemical reactions, chemical equations, stoichiometry - different approaches
4th - 6th week: Gas laws, basic concepts of thermochemistry, quantum theory and atomic structure, electron configuration and chemical periodicity
7th - 10th week: Models of chemical bonding (ionic, covalent, metallic), the shapes of molecules (Lewis structures, VSEPR), theories of covalent bonding (valence bond, orbital hybridization, molecular orbital), electronegativity and bond polarity, intermolecular forces (hydrogen bond, states of mater), the relation of structure and bonding to the physical and chemical properties of matter
11th - 15th week: Properties of solutions, basic concepts of chemical kinetics and equilibrium, equilibrium in solutions of acids and bases, electrochemistry, systematization of basic concepts of the course
REQUIREMENTS FOR STUDENTS:
Regular attendance of lectures and seminars, access to the two tests, occasional homework.
GRADING AND ASSESSING THE WORK OF STUDENTS:
Successfully solved written exam (the possibility of taking over two tests) and the oral exam. The final grade form scores on written and oral exams and the points earned during class (assignments and the results of tests).
- OBAVEZNA LITERATURA:
1. S. Silberberg, Chemistry, 6. izd., McGraw-Hill, NewYork, 2006.
2. R. Chang, Chemistry, 9. izd., McGraw-Hill, NewYork, 2006.
3. I. Filipović, S. Lipanović, Opća i anorganska kemija I i II dio, IX. izd. Školska knjiga, Zagreb, 1995.
4. M. Sikirica, Stehiometrija, XX. izd. Školska knjiga, Zagreb, 2008.
- DOPUNSKA LITERATURA:
1. M. Sikirica, B. Korpar-Čolig, Praktikum iz opće kemije, II. izd. Školska knjiga, Zagreb, 2003.
2. D. Grdenić: Molekule i kristali, Školska knjiga, Zagreb, 2005.
3. T. Cvitaš, I. Planinić, N. Kallay, Rješavanje računskih zadataka u kemiji, (interna skripta), Hrvatsko kemijsko društvo, Zagreb, 2010.