COURSE OBJECTIVES:
OBJECTIVES
To familiarize students with the properties of chemical elements and their inorganic compounds by applying information on ionization energy, electron affinity, electronegativity, standard reduction potential, ionic radius, and related parameters. To introduce students to trends in the variation of the chemical and physical properties of compounds within groups and periods. To familiarize students with industrial processes for the production of technically important inorganic compounds and materials.
PREREQUISITE COURSES
Not specified.
COURSE LEARNING OUTCOMES
Upon successful completion of the course, students will be able to:
Identify stable and less stable (unstable) oxidation states based on the electron configuration of groups of elements (s, p, d, and f blocks).
Infer the stability of hydrides and oxides of elements based on their electronegativity values.
Infer the redox behavior and stability of substances in their elemental state based on ionization energy and standard reduction potential data.
Identify the type of hybridization based on the structural formula of a compound and propose the molecular geometry.
Assess the strength of an acid based on the structural formula of oxoacids.
Identify stable and less stable oxidation states based on electron-voltage diagrams and identify oxidation states susceptible to disproportionation.
Predict the products of chemical reactions of metals with oxidizing and non-oxidizing acids based on the standard reduction potential of the metal.
Relate differences in electronegativity between elements in a molecule to intermolecular interactions and the influence of these interactions on changes in the physical properties of molecules, such as melting point and boiling point.
Name a compound based on its chemical formula and write the formula of an inorganic compound based on its name.
Identify industrial processes for the production of technically important inorganic compounds and materials.
LEARNING OUTCOMES OF THE STUDY PROGRAM TO WHICH THE LEARNING OUTCOMES OF THIS COURSE CONTRIBUTE
The learning outcomes of this course contribute to the following study-program learning outcomes:
Explain the scientific foundations important for environmental engineering, particularly fundamental knowledge in chemistry, mathematics, physics, biology, and environmental engineering.
Apply basic laboratory skills and rules of laboratory practice in physical, chemical, and microbiological laboratories.
Organize effective laboratory work, independently or as part of a multidisciplinary team.
Theoretically interpret the results of experimental work.
Present the results of one's work in written and oral form.
COURSE CONTENT BY UNITS OR WEEKS
LECTURES BY WEEK
1. Periodic law and the periodic table of chemical elements
Changes in physical and chemical properties across periods and within groups; periodicity of chemical properties (electronegativity, ionization energy, electron affinity, oxidation number, standard reduction potential); periodicity of physical properties (melting point, boiling point).
2. Hydrogen
General properties and preparation. Compounds of hydrogen in positive and negative oxidation states (ionic, covalent, and metallic hydrides). Hydrogen isotopes and hydrogen bonding.
3. Group 18 elements (noble gases)
General properties and preparation. Compounds of xenon and other noble gases.
4. Group 17 elements (halogens)
Basic characteristics of the group; variation of physical and chemical properties of the elements within the group; changes in electronegativity and trends in metallic character. Properties of compounds in oxidation states ?1, 0, +1, +3, +4, +5, and +7; pseudohalides. Physical and chemical properties of the elements, chemical reactivity and trends; properties of oxoacids and their salts (halides, hypohalites, halates, and perhalates).
5. Group 16 elements (chalcogens)
General characteristics and characteristic properties of the group. Overview of compounds in oxidation states ?2, ?1, 0, +2, +3, +4, and +6. Properties and preparation of O? and O?; structure of water, hydrogen peroxide, and superoxides; oxoacids of sulfur, selenium, and tellurium; thioacids. Changes in redox properties within the group (electron-voltage equivalents).
6. Group 15 elements (nitrogen group)
General characteristics and characteristic properties of the group; changes in electronegativity and trends in properties within the group. Overview of compounds in oxidation states ?3, ?1, 0, +1, +3, and +5. Preparation and properties of ammonia, nitric acid, hydrazine, N?O, NO, NO?, N?O?, and N?O?. Preparation and properties of phosphine, arsine, stibine, and bismuthine. Preparation and properties of oxoacids of the nitrogen-group elements.
7. Group 14 elements (carbon group)
Properties of Group 14 elements; characteristic forms and compounds of carbon (diamond, graphite, graphene, fullerene); CO and CO?. Characteristics of compounds in negative oxidation states (carbides). Properties of silicon compounds in negative and positive oxidation states; silicides, silanes, and silicates. Characteristic properties of germanium, tin, and lead in oxidation states +2 and +4; lead?acid battery.
8. Group 13 elements (boron group)
Properties of the group and overview of the properties of the elements within the group. Characteristic boron compounds in oxidation states +1, +2, and +3; borides and boranes. Preparation and properties of boric acid. Aluminium: properties and preparation. Amphoterism of Al(OH)?, passivation of aluminium, and aluminosilicates. Basic properties of gallium and indium.
9. Group 2 elements (alkaline earth metals)
Properties of the group. Trends in physical and chemical properties within the group. Preparation of sulfates, hydroxides, and carbonates.
10. Group 1 elements (alkali metals)
Basic properties of the group elements. Trends in physical and chemical properties within the group; reactions with water; preparation of NaOH, NaHCO?, NaCl, and gypsum.
11. Preparation and characteristic properties of metals
12. Trends in the chemical and physical properties of d- and f-block elements
Inorganic coordination compounds; ligand-field splitting.
13. Vanadium, chromium, and manganese groups of d-block elements
Basic properties of the elements; chemical reactivity and trends within the groups; oxides and the most important compounds in oxidation states +2, +3, +4, +5, and +6.
14. Iron, cobalt, and nickel groups (Groups 8, 9, and 10)
Basic properties of the elements; chemical reactivity and trends in chemical and physical properties within the triads; oxides and oxoanions. Production of iron and steel; corrosion of iron.
15. Copper and zinc groups
Basic properties, preparation, reactivity, and trends in chemical and physical properties within the groups; oxidation states +1, +2, and +3; halides, oxides, sulfides, and coordination compounds.
LABORATORY EXERCISES
Exercise 1
Preparation of hydrogen by reaction of aluminium with sodium hydroxide
Preparation of iodine by reduction of potassium iodate
Preparation and properties of oxygen
Properties of metal oxides and hydroxides
Preparation of sodium thiosulfate
Exercise 2
Preparation and decomposition of silver thiosulfate
Preparation and properties of nitrogen
Preparation of ammonia
Preparation of sodium carbonate
Exercise 3
Preparation of lead(IV) oxide; lead?acid battery
Preparation of lead(II) chloride
Preparation of boric acid
Exercise 4
Preparation of potassium aluminium sulfate dodecahydrate
Preparation of copper(I) oxide
Preparation of copper(I) chloride
Preparation of tetraamminecopper(II) sulfate monohydrate
Exercise 5
Preparation of sodium chromate
Preparation of chromium(III) oxide
Preparation of potassium chromium alum
Precipitation and properties of manganese(II) hydroxide
Preparation of potassium manganate and potassium permanganate
Exercise 6
Preparation of reducing solutions of vanadium salts using a Jones reductor
Preparation of iron(II) sulfate heptahydrate
Precipitation and properties of iron(III) hydroxide
Preparation of potassium iron(III) hexacyanoferrate(II)
Exercise 7
Preparation of Mohr's salt
Cobalt complexes
Preparation of mercury(I) iodide
Preparation of mercury(II) oxide
Exercise 8
Titration of phosphoric acid solution with sodium hydroxide solution
Titration of silver nitrate with potassium iodide solution
MODES OF INSTRUCTION
Lectures, exercises, and laboratory work.
STUDENT OBLIGATIONS
Completion of all laboratory exercises.
MONITORING OF STUDENTS' WORK
Attendance
Experimental work
Continuous assessment
Written examination
Oral examination
GRADING AND ASSESSMENT DURING CLASS AND ON THE FINAL EXAM
Entrance tests on laboratory exercises.
Two written knowledge assessments are conducted during the semester:
Test 1: maximum 100 points; minimum passing score: 50 points
Test 2: maximum 100 points; minimum passing score: 50 points
Laboratory exercises: maximum 10 points
Total: 210 points.
A minimum of 120 points is required to be exempted from the written examination.
Written examination: a minimum of 60% of the points is required to pass.
Satisfactory (2): 60?70% of points
Good (3): 70?80% of points
Very good (4): 80?90% of points
Excellent (5): 90?100% of points
Oral examination.
MANDATORY LITERATURE
I. Filipović and S. Lipanović, Opća i anorganska kemija [General and Inorganic Chemistry], Školska knjiga, Zagreb, 1995.
QUALITY ASSURANCE METHODS FOR ENSURING THE ACQUISITION OF INTENDED KNOWLEDGE, SKILLS, AND COMPETENCES
Student survey.
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