Code

Course teacher

Associate teachers

Status of the course

Course objectives

To introduce students to the basic elements of calculus and linear algebra.

Course enrolment requirements and entry competences required for the course

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After finishing this course the student is expected to be able to:
- identify and sketch graphs of elementary functions, to determine the domain of the given function
- find the derivative of the given function
- apply the dervative in practice (tangents and normals, maximum, minimum and inflection points) and to interpret the shape of graphs
- solve the system of linear equations (by matrix inversion, by Gaussian elimination)

Course content broken down in detail by weekly class schedule (syllabus)

1. Sets: Notion. Algebra of sets. Sets of numbers.
2. Functions: Notion. Composite functions. Inverse function.
3. Elementary functions.
4. Functions: Limits. Continuity.
5. Derivative and application: Notion. Interpretation. Derivative techniques.
6. Differential. Higher order derivatives.
7. Theorems of differential calculus. Maximum, minimum points.
8. Inflection points. Asymptotes. Graphs sketching.
9. Sequences: Notion. Limits.
10. Series: Convergence of numeric series. Power series. Taylor series.
11. Matrices and vectors: Matrix algebra. Determinants. Inverse matrix.
12. Linear systems of equations.
13. Vector algebra.
14. Solid analityc geometry.
15. Course review. Revision.

Format of instruction:

Student responsibilities

Regular attendance of classes.

Optional literature (at the time of submission of study programme proposal)

S. Kurepa, Matematička analiza I i II dio, Školska knjiga, Zagreb, 1997.
L. Krnić, Z. Šikić, Račun diferencijalni i integralni, I dio, Školska knjiga, Zagreb, 1992.
Hughes-Hallett, Gleason et al., Calculus, John Wiley and Sons, Inc., New York, 2000.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

- Introducing students to the knowledge and principles of physics in the field of mechanics
- Forming the proper view towards the interpretation of physics phenomena and their application
- Developing the level of cognitive processing required for further studies

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Physics I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After the course, the student is expected to have mastered:
- Physical quantities, units and dimensional analysis;
- The characteristics of the exact approach to phenomena in both micro and macro world;
- The principles of the classic general mechanics;
- The basic principles of the special mechanics (mechanics of oscillations, waves and fluids);
- The use of calculus in mechanics contents;
- The application of the laws of mechanics in concrete physics examples;
- The application of the obtained knowledge in solving problem tasks;
- The application of the knowledge in professional situations.

Course content broken down in detail by weekly class schedule (syllabus)

1st week: Space, time, matter. Physical quantities, Laws of Physics. Plane and space geometry, using of vector algebra, differential and integral calculus.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course.
2nd week: Kinematics of particles
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
3rd week: Particles dynamics
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
4th week: Work and energy
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
5th week: Conservative and nonconservative forces
Partial assessment (1st preliminary test) ) related to seminars and theory addressed during the course
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
6th week: Conservation of energy law
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
7th week: Systems of particles.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
8th week: Collisions; Conservation laws
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
9th week: Rigid body mechanics. Conservation laws. Restrictions of rigid body approximations and the theory of elasticity.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course.
10th Equilibrium. Restrictions of rigid body approximations and the theory of elasticity.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
Partial assessment (2nd preliminary test) ) related to seminars and theory addressed during the course
11th week: Oscillations and waves
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
12th week: Many particle physics: gasses, liquids and solids. Internal energy, heat and heat disorder. Transport phenomena. Phase transition phenomena.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
13th week: Fluid mechanics: statics
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
14th week: Fluid mechanics: dynamics
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course
15th week: Elastic waves. Sound.
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course.
Partial assessment (3rd preliminary test ) related to seminars and theory addressed during the course

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

D. Halliday, R. Resnick, J. Walker, Fundamentals of Physics, John Wiley & Sons, New York, 1993;
Janko Herak, Osnove kemijske fizike, Farmaceutsko-biokemijski fakultet Sveučilišta u Zagrebu, 2001.
V. Lopac, P. Kulišić, M. Pavičić, Zbirka zadataka iz fizike, FGZ Zagreb, 1983.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The fundamental and the inseparable part of all physics research is the experiment. The aim of this course is to introduce the students to various techniques of conducting experiments and methods of measuring the physics quantities in the field of mechanics. Additionally, the aim is to enable the development of skills needed to conduct experiments, gather data and master various numerical problems, which are related to measuring and testing physics quantities.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Physics I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

- Obtaining basic knowledge and skills needed to conduct experiments
- The knowledge of various methods and techniques of measurement
- Mastering the calculation of errors which occurred during the measurement
- Mastering the evaluation of errors which occurred during the measurement
- The skills of graphic representation of the measured data and the method of writing reports pertaining to the experiment and the results of measuring conducted

Course content broken down in detail by weekly class schedule (syllabus)

- Measurement of length, mass and density. (3 hours)
- Numeric and graphic processing of the measurement data. (2 hours)
- Measurements of characteristic quantities: the laws of forces (friction, Hooke´s law /conservation laws (energy, momentum). (3 hours)
- Measurements of characteristic quantities: rotation (moment of inertia, torque) (2)
- Oscillations (spring oscillations, mathematical, physical and torsional pendulum). (2 hours)
- Laws of hydrostatics (Archimedes law, surface tension). (3 hours)
- Compensating exercises
- Final revision test

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

To familiarize students with the basic chemical laws and principles and to enable students to master the chemical items that follow General Chemistry. To develop students ability to think critically about the experiments performed in the laboratory and about the involvement of of chemistry in everyday life.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in General Chemistry
The condition for taking the exam: Passed the course ”Exercises in General Chemistry”

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After the the course students will be able to:
1) Understand the nature and properties of the substance differentiate elementary substances from compounds, distinguish homogeneous from heterogeneous mixtures, assume procedures for separating mixtures into pure substances.
2) Understand and applied the problem-solving approach to the balance of substances in chemical changes
3) Understand the structure of atoms and existing models of chemical bonds in such way that they can predict certain properties and reactivity of chemical elements and their ionic and covalent compounds
4) Discern the nature of certain chemical reactions.
5) Adopt the concept of pH, and assume direction of the chemical reactions on the basis of knowledge of chemical kinetics and equilibrium.
6) Independently and safely perform simple chemical experiments

Course content broken down in detail by weekly class schedule (syllabus)

Lectures:
1. Introduction - Natural sciences and chemistry. Units of measurement and measurement. Classification of matter. Pure substance. Decomposition of the substance to the pure substance.
2. Properties of pure substances, physical and chemical properties. Atom and chemical element. The chemical symbols of elements. The laws of chemical combination by weight and volume. The atomic theoryes from the early ideas to John Dalton. Avogadro’s hypothesis.
3. The discovery of the structure of atoms. The discovery of X-rays and radioactivity. Rutherford model of the atom. X-rays and crystal structure. Bragg equation. Isotopes and the structure of the atomic nucleus.
4. The structure of pure substances. The atomic structure of substances. Types of a crystal systems and crystal characteristics. Cubic crystal system. The molecular structure of substances. The nature of the gas. The nature of the fluid. The concept of temperature. The kinetic theory of gases.
5. Gas laws and the equation of state of an ideal gas. Real gases. Relative atomic and molecular weight. Methods for determining relative atomic (Dulong - Petit method, X-ray diffraction, mass spectrograph) and molecular weight (density of the gas, the method of Victor Mayer, Hoffman method). Periodic table of the elements and the periodic law.
6. Electronic structure of atoms - Bohr model of the atom, quantum numbers. Quantum theory of the electronic structure of atoms. Atomic orbitals.
7. Periodic Classification of elements and the periodic table. Periodic changes in physical properties. Atomic radius. Ionization energy. Electron affinity. Electronegativity.
8. Chemical bonding and molecular structure - Electronic valence theory, ionic and covalent compounds. Electronegativity and degree of oxidation. Writing Lewis structures and the octet rule. Formal charges. Exceptions from the octet rule. VSEPR model and geometry of the molecule.
9. Bond characteristics. Valence bond theory and theory of molecular orbitals.
10. Intermolecular forces. Dipole moment, Van der Waals and London forces, hydrogen bond.
11. The structure and properties of the liquid and solid. Physical properties of solutions. Types of solution. Expression of concentration.
12. The liquid in the liquid solution. Solutions of solids in liquids. Solutions of gases in liquids. Effect of temperature on the solubility. Effect of pressure on the solubility of gases. Colligative properties of solutions: nonelectrolyte and electrolyte solution.
13. Chemical reactions - types of chemical reactions, redox reactions, complex reactions (protolytic reactions and precipitation reactions and dissolution), complex reactions.
14. Chemical kinetics, reaction rate, reaction mechanism, the activation energy. Chemical equilibrium - term equilibrium, chemical equilibrium and chemical equilibrium constant. Factors that affect the chemical equilibrium.
15. Equilibrium in homogeneous and heterogeneous systems. Balance in the electrolyte solutions - equilibrium in solutions of acids and bases , the equilibrium of the complex in solution, the equilibrium between the solution and the insoluble crystals, redox balance
Seminars:
1. The oxidation number: definition, rules for determining in ions and molecules. Examples and training.
2. Nomenclature of Inorganic Chemistry. Names of monoatomic cations and monoatomic anions. Names of poliatomic cations and anion. The names of the ligands. Names of complex ions. Names of oxo acid and their salts.
3. Naming of inorganic compounds - training.
4. Balancing chemical equations, balancing redox equations.
5. Writing redox equations - practice.
6. The stoichiometry: Qualitative and quantitative relationships in chemical reactions. Molar method.
7. Stoichiometry: Quantitative relationships. Yield in chemical reactions and processes: the relevant reactant, the reactant in excess of the theoretical amount of reactants, the theoretical amount of product, yield and loss.
8. The stoichiometry: volume and mass in chemical reactions.
9. Electronic configuration of atoms and ions
10. Lewis structural formula
11. Electronic structural formula
12. Chemical equilibrium in homogeneous and heterogeneous systems
13. Chemical equilibrium in electrolyte solutions.

Format of instruction:

Student responsibilities

The 80% presence at lectures and seminars, and completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Darrell D. Ebbing and Steven D. Gammon, General Chemistry, 9th edition, Houghton Mifflin Company, Boston, 2009.
Raymond Chang, Chemistry, 10th edition, McGraw-Hill, New York, 2010.

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

To introduce students to the basic elements of integral calculus, differential calculus of several variables and the basic of differential equations.

Course enrolment requirements and entry competences required for the course

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After finishing this course the student is expected to be able to:
- apply the techniques of integration (integration by substitution, integration by parts)
- use the definite integral in its geometrical applications
- solve the first-order differential equations (variables separable, homogeneous differential equations, linear differential equations, exact differential equations)
- solve the second-order linear nonhomogeneous differential equations with constant coefficients

Course content broken down in detail by weekly class schedule (syllabus)

1. Indefinite integral. Table of integrals.
2. Integration by substitution. Integration by parts.
3. Integrating rational fractions. Integrating by algebraic substitution.
4. Definite integral.
5. Improper integrals.
6. Application of definite integral.
7. Functions of several variables. Limit and continuity.
8. Partial derivatives. Differential.
9. Tangent plane and normal line. Maxima and minima.
10. Double integrals.
11. Geometric application of double integrals.
12. Ordinary differential equations.
13. First-order differential equations.
14. Second-order differential equations.
15. Course review. Revision.

Format of instruction:

Student responsibilities

Regular attendance of classes.

Optional literature (at the time of submission of study programme proposal)

S. Kurepa, Matematička analiza I i II dio, Školska knjiga, Zagreb, 1997.
Hughes-Hallett, Gleason et al., Calculus, John Wiley and Sons, Inc., New York, 2000.
McCallum, Hughes-Hallett, Gleason et al., Multivariable Calculus, John Wiley and Sons, Inc., New York, 2002.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquiring a basic knowledge of computers and computer systems. Knowledge about the use of Internet content and protect your computer from malicious programs. Basic skills about the content management (folders and files) on PCs using the Windows operating system. Basic skills using programs offered in the MS Office software.

Course enrolment requirements and entry competences required for the course

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the exam the student will be able to:
1. Manage content on PC computer (files and folders)
2. Use the MS Word in the purpose of the editing the file according to the specified requirements (defining the shape and page layout, inserting the images, finished elements, tables, graphs ...)
3. Use the MS Excel for analysis, calculation, sorting, graphical presentation and format tables.
4. Use the MS PowerPoint to create presentations
5. Set up and use MS Outlook for editing and emailing
6. Find reliable sources of information on the Internet

Course content broken down in detail by weekly class schedule (syllabus)

1. Week L General information about the course and mode of examination, Introduction to computers application, Information activity and technology, Computerization, Computer applications in Chemistry and Chemical Engineering
E
2. Week L Hardware (PC), Von Neumann’s model computers, Computer hardware, Computer types, Basic terms in the Computer Engineering and informatics, Basic parts (components) of the PC, Central processing unit (CPU), Computer memory, Motherboards and connectors, Input and Output devices
E
3. Week L Operating systems and applications, The BIOS (Basic Input / Output System), Preparing disks and drives for installation of the OS, File system (FAT, NTFS), Computer Programs, System programs, Application programs, Operating systems
E
4. Week L Basics commands for MS-DOS, GUI (Graphical User Interface), Properties GUI, History of developing the MS Windows OS, Example Installations operating systems (Windows OS), Customizing the User Interface, Library, Customize settings on PC computer, Firewall, Windows Defender, Windows Update, Action Center, Commercial antivirus programs
E
5. Week L Backup and Restore, Control Panel, Customize the computer, The Device Manager, Accounts, Network and Sharing Center, Troubleshooting, Personalization, BitLocker Drive Encryption, Region and Language, Programs and Features, Installing and uninstalling programs, Display, Devices and Printers, Default Programs, Help and Support, Accessories and system tools, Shortcuts in Window OS, Changing the language of Windows OS
E
6. Week L Malicious software (malware), Computer viruses, Computer worms, Trojan horses, Logic bombs, Spyware, Advertising Programs (Adware), INTERNET, History of the Internet, TCP / IP protocol
E
7. Week L First test
E
8. Week L Internet, Computer network and classification networks, Internet protocols: HTTP, HTTPS and FTP, Web browsers, Copyright Law
E
9. Week L MS Office, MS Word, How to start the MS Word, Layout MS Word window, The status bar, Tabs and tools, Copy and paste data, Special characters, Styles, Tabs, Sections, Creating a new document, Copy text, Headers and footers, Page numbers
E MS Word: How to insert and edit the text and its formatting. Paragraph formatting. Lists of lists. Working with documents. formatting documents
10. Week L How to insert and edit the formulas and equations, Application of the finished style characteristics, Input tables and formatting, input images in the document, the entry of bibliographic data entry page breaks and section breaks (define different sections of the document), display the contents of the document
E MS Word: Insert pictures, tables and SmartArt elements in the document. Formatting headers and footers document. Entering references and footnotes in the document. Insert the page break, Section break, Application of different style for document
11. Week L MS Excel, How to start MS Excel, Layout MS Excel windows, Toolbar for quick access, Status bar, Tabs and tools, Tabs formulas, Editing data within a worksheet, Graphic data presentation, Input data string in the table, Add the trend data, Sorting data set
E MS Excel: Working with the tables. Entering data into tables and data formatting. Entering a series of data. Entering data from different files. Displaying data graphically.
12. Week L Conditional Formatting Data, Creating and deleting equations, Addresses cells (relative, absolute, mixed), Types of functions, Logical operators, Boolean functions, Examples of application functions (IF, AND, OR, COUNTIF ..), MS PowerPoint, MS PowerPoint Startup, The appearance of windows, tabs and tools, Creating presentations, add themes, Themes Edit, Insert object (images, tables, links, media content ...)
E MS Excel: Data processing, Calculating with tables, Input and syntax for creating mathematical equations. Showing the trend curve.
13. Week L MS Outlook, MS Outlook Startup, The appearance of windows, tabs and tools, Creating a user account , Creating a new e-mail
E MS Power Point: Creating presentations. Choosing the design, How to make redesign of an existing template.
14. Week L Databases, What databases they are?, Fields in databases, How databases are developed?, Center for online databases, Bibliographic databases, Citation databases, Databases with full-text, Sciencedirect databases, Scopus databases, Web database, Bibliography
E
15. Week L Second Test
E

Format of instruction:

Student responsibilities

Class attendance in the amount of 70% to 100%, and to experimental work of 100% from total hours.

Optional literature (at the time of submission of study programme proposal)

Selected articles from journals recommended by lecturer

Quality assurance methods that ensure the acquisition of exit competences

1. Tracking suggestions and reactions of students throughout the semester
2. Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Exercising, testing and confirm knowledge from lectures. Understanding with the methods of experimental work and the acquisition of skills necessary for independent work in the lab.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course General Chemistry

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students will upon completion of the course be able to:
1. Practically through experiments verify the theoretical assumptions
2. Gain independence in performing experiments
3. Design simple experiments to illustrate the chemical properties of the substance
4. Actively exploring ways in which this discipline has consequently impact on the outside world.

Course content broken down in detail by weekly class schedule (syllabus)

Exercise 1
The basic rules of laboratory work, safety precautions and protection in the lab, basic laboratory equipment. Washing, cleaning and drying of dishes. Basic laboratory operations, chemicals and dealing with them. Decomposition of the substance to the pure substance. Decomposition of heterogeneous and homogeneous mixture
Exercise 2
Decomposition of the mixture to the pure substance, Decomposition of heterogeneous substances, Sedimentation, decanting, centrifuging, filtering, Buchner funnel, distillation and fractional distillation, sublimation of iodine. Extraction of iodine from aqueous solutions
Exercise 3
Physical and chemical changes, the law of conservation of weight, Gay - Lussac’s law of connected volumes. Exercise with models of unit cells. Determining the relative atomic mass of zinc. Determination of the empirical formula of copper chloride.
Exercise 4
Gas Laws: Determination of the molar volume of oxygen, Boyle’s law, Charles Gay - Lussac’s law, the pressure dependence of the temperature in gases.
Exercise 5
Solutions and their properties. Expressing of concentration. Preparation of the solution with given concentration. Solutions of liquids in liquids. Solutions of gases in liquids. Dependence of solubility on the nature (structure) of the substance. Dependence of solubility on temperature. Dissolution of liquids in liquids. Dissolving gases in liquids. Henry’s law. Determination of molar mass by freezing point depression. Illustration of electrolytic dissociation. Illustration of ions traveling to the electrodes. Electrical conductivity of the solution. Redox - reactions of sulfur and oxygen. Redox reaction of dilute nitric acid solution and iron (II) sulfate. Decomposition and formation reactions of complexes. Ligand substitution reaction. Protolytic reactions (acid- base titration).
Exercise 6
Chemical kinetic, effect of concentration of reactants on the rate of chemical reactions. Effect of temperature on the rate of chemical reactions. The catalytic effect on the rate of chemical reactions. Balance in electrolyte solutions. Moving the chemical balance. Determination of the acid dissociation constant, Ka . Determination of pH: Approximately determination of pH using indicators. Determination of pH using pH sensors. Electrolysis - Determination of Faraday’s constant. Electromotive force of galvanic cells - Daniell cell.
Exercise 7
Protolytic reactions and titration curves obtained with the help of computers
Determination of the acid dissociation constant, Ka. Hydrolysis. Buffers.
Exercise 8
Vacuum distillation. Determination of the molar mass of easily volatile liquids.
Determination of molar mass by freezing point depression

Format of instruction:

Student responsibilities

Completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

- Introducing students to the knowledge and principles of physics in the fields of electromagnetism, optics and elementary quantum physics
- Forming the proper view towards the interpretation of physics phenomena and their application
- Developing the level of cognitive processing required for further studies

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Pysics II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After the course, the student is expected to have mastered
- The principles of electromagnetism and electromagnetic radiation
- The principles of geometrical and physical optics
- The basic principles of quantum physics
- The application of the obtained knowledge in concrete physics examples
- The application of the obtained knowledge in solving professional problem tasks
- Recognition of the application of the knowledge of physics in everyday situations

Course content broken down in detail by weekly class schedule (syllabus)

1st week: Electric charges, electrostatic force and electrostatic field. Vector field flux and Gauss’s law. Application of Gauss law. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1 hour)
2nd week: Electric potential and potential difference. Moving and storing electric charges, electric circuits. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
3rd week: Charges in motion and their interactions, electric current. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
4th week: Magnetic field. Gauss law. Ampere’s law. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
5th week: Time depending electric and magnetic fields. Faraday’s law. Inductivity. Induction generators. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
Partial assessment (1st preliminary test) related to seminars and theory addressed during the course.
6th week: Vector field circulation. Applications. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
7th week: Maxwell equations. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
8th: week: Alternating currents. Electromagnetic oscillating circuit and radiation. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
9th week: Energy of electric and magnetic fields. Electromagnetic waves and nature of light. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
10th week: Electric and magnetic field in matter. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
Partial assessment (2nd preliminary test) related to seminars and theory addressed during the course.
11th week: Physical optics (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
12th week: Geometric optics. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
13th week: Optical systems and instruments. Eye physics. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
14th week: Wave properties of matter. Concepts of quantum physics (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
15th week: Concepts of quantum physics - applications. (3 hours)
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1 hour)
Partial assessment (3rd preliminary test ) related to seminars and theory addressed during the course

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

D. Halliday, R. Resnick, Fundamentals of Physics, John Wiley, New York 2003.
Janko Herak, Osnove kemijske fizike, Farmaceutsko-biokemijski fakultet Sveučilišta u Zagrebu, 2001.
V. Lopac, P. Kulišić, M. Pavičić, Zbirka zadataka iz fizike, FGZ Zagreb, 1983.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The basic and the inseparable part of all physics research is the experiment. The aim of this course is to introduce the students to various techniques of conducting experiments and methods of measuring the physics quantities from the field of electromagnetism and optics. Additionally, the aim is to enable the development of skills needed to conduct experiments, gather data and master various numerical problems, which are related to measuring and testing physics quantities.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Pysics II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

- Obtaining the basic knowledge and skills needed to conduct experiments in the field of electromagnetism and optics
- The knowledge of various methods and techniques of measurement
- Mastering the calculation of errors which occurred during the measurement
- Mastering the evaluation of errors which occurred during the measurement
- The skills of graphic representation of the measured data and the method of writing reports pertaining to the experiment and the results of measuring conducted.

Course content broken down in detail by weekly class schedule (syllabus)

- Electric circuits: elements and instruments. (4 hours)
- Direct current ; Resistance and resistors.(4 hours )
- Alternating current; Capacitance and capacitors. (3 hours )
- Alternating current; Inductance and inductors. (3 hours )
- RLC circuits (3 hours )
- Laws of geometrical optics. (3 hours )
- Laws of physical optics. (3 hours )
- Optical instruments. (4 hours )
- Spectroscopy / quantization (3 hours )
- Compensating exercises
- Final revision test

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Introduce students to the chemical reactivity of elements along the periodic table, and with the properties and composition of common chemicals. To develop students ability to notice similarities and differences between inorganic compounds and inorganic substances. Understanding of the changes in the various physical and chemical conditions

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Inorganic Chemistry
The condition for taking the exam: Passed the course ”Exercises in Inorganic Chemistry I”

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students upon completion of the course:
1) will know the basic characteristics and producing of chemical elements for the major groups of periodic table of elements (PTE)
3) be able to identify the type and properties of chemical compounds of main group
3) be able to identify the type and properties of transition metal compounds
4) to classified compounds on the base of their characteristics
5) to predict acidic, basic and amphoteric properties of salts
6) to know common salt crystal structure
7) to predict the possible reaction mechanisms and outcomes of chemical reactions
8) to independently and safely perform simple chemical reactions

Course content broken down in detail by weekly class schedule (syllabus)

Lectures:
1. Hydrogen position in PTE, hydrogen properties and production, positive oxidation state and hydrides
2. Noble gases, properties of group, obtaining and using of xenon compounds
3. Introduction to halogens, elements properties in order to oxidation state
4. Fluorine production and properties, differences between the fluorine and the other members of the group, fluorine compounds. Chlorine producing and properties, compounds of chlorine, bromine and Iodine
5. Introduction to chalcogen elements, elements properties in order to oxidation state
6. Oxygen properties and production, the compounds of oxygen, oxides, water
7. Sulfur properties and production, oxides and sulfur acids, other sulfur compounds, compounds of selenium and tellurium,
8. A group of nitrogen, elements properties in order to oxidation state
9. Nitrogen, properties of the production, ammonia, nitric acid and other nitrogen compounds, nitrogen fixation
10. Phosphorus, properties and production, oxides and acids of phosphorus, arsenic, antimony and bismuth
11. A group of carbon, elements properties in order to oxidation state
12. Carbon allotropes, carbon properties and production, carbon oxides, carbides, carbonates and bicarbonates.
13. The compounds of silicon, germanium, tin and lead, semiconductor properties of silicon and germanium
14. A group of boron, elements properties in order to oxidation state, boranes, boric acid. Production and properties of aluminum, aluminum compounds, gallium, indium, thallium
15. Alkali and alkaline earth metals
Seminars :
1. Balancing chemical reactions, writing and balancing redox reactions in one line
2. Common reactions of hydrogen, the reducing action of hydrogen
3. Common reactions of chlorine, the disproportionation of chlorine in alkaline solutions, the oxidation activity of the halogens compounds
4. Common reactions of chalcogen elements, reaction of oxygen and ozone, the oxidizing action of oxygen,
5. The reaction of sulfur, the reactions which translate elemental sulfur to sulfuric acid, the oxidizing action of sulfuric acid, a dehydrating effect of sulfuric acid
6. Common reactions of nitrogen, the nitrogen production reactions, the reaction of ammonia oxidation to nitric acid, the oxidizing action of nitric acid.
7. Common reactions of phosphorus, oxidation reactions of phosphorus to phosphorus and phosphoric acid
8. Common reactions of carbon, oxides of carbon production, reducing effect of CO, binding of CO2 from the air, the precipitation of carbonates, cation hydrolysis
9. Common reactions of the boron group elements, reaction of boric acid production, dissolution of borax in water, production of crystalline boron acid, base properties of aluminum hydroxide,
10. Aluminum reducing action, aluminotermic reaction, common reactions of metals and metal production,
11. Common reactions of alkali and alkaline earth metals with water and their salts
12. Common reactions of transition metals, proving of peroxide with titanyl ion, oxidation states of vanadium, oxidative properties of permanganate, equilibrium between chromate and dichromate, iron compounds
13. Noble metals, zinc, cadmium and mercury
14. Sea - a mixture of inorganic substances. The chemical composition of sea water, salinity, pH and speciation
15. Mixed problems

Format of instruction:

Student responsibilities

The 80% presence at lectures and seminars and completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

F. Albert Cotton et al., Basic Inorganic Chemistry, New York, John Wiley and Sons, 1995.

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Exercising, testing and confirm knowledge from lectures. Understanding with the methods of experimental work and the acquisition of skills necessary for independent work in the lab.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Inorganic Chemistry

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students will upon completion of the course be able to:
1. Practically through experiments verify the theoretical assumptions
2. Gain independence in performing experiments
3. Design simple experiments to illustrate the chemical properties of the substance
4. Actively exploring ways in which this discipline has consequently impact on the outside world.

Course content broken down in detail by weekly class schedule (syllabus)

Exercises :
1. Exercise: HYDROGEN
2. Exercise: 17th GROUP (Halogens )
3. Exercise: 16th GROUP (Chalcogens)
4. Exercise: 15th GROUP
5. Exercise: 14th GROUP and 13th GROUP, 1st and 2nd groups (Alkali and earth alkali metals)
6. Exercise: TRANSITION ELEMENTS (groups 3 to 7)
7. Exercise: TRANSITION ELEMENTS (groups 8 to 12)
8. Exercise: Synthesis of double salts, alums and Tutton salts, Synthesis of Mohr’s salt
9. Exercise: Synthesis of nickel complexes

Format of instruction:

Student responsibilities

Completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquiring basic basic theoretical knowledge of analytical chemistry, the role and application of analytical chemistry in various fields of human activity. Being able to access the chemical analysis of the sample by applying the laws of chemistry chemical balance for identification of an analyte in a sample in order to obtain useful information.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercise of Analytical Chemistry I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After completing the course, the student will will be able to
- Define the concept of analytical chemistry
- Differentiate between the concepts of qualitative and quantitative chemical analysis
- Define the concept of analyte, the analytical signal and information.
- Understanding the basic laws of chemical analysis.
- Define the equilibrium constants of chemical reactions, the law of mass action and the principle according to Le Chatelier.
- . Implement the principle of chemical equilibrium chemical reactions for identification and separation of analytes from complex matrix.
5. Distinguish the heterogeneous from homogeneous chemical equilibrium systems.
6. Predict the behavior of a chemical reaction due to the change in pH and due to the effect of the foreign ions.
7. Capacity to apply knowledge in practice, especially in problem solving based on information from systems.

Course content broken down in detail by weekly class schedule (syllabus)

Week 1: The description and view the contents of the object. Definitions of analytical chemistry. Division of Analytical Chemistry. The concept and the formation of the analytical signal. Seminar: Solving problems.
Week 2: Definition of chemical analysis - qualitative and quantitative. Seminar: Solving problems.
Week 3: Constants homogeneous equilibrium of importance in analytical chemistry. Seminar: Solving problems.
Week 4: Constants of heterogeneous equilibrium of importance in analytical chemistry. Seminar: Solving problems.
Week 5: Qualitative chemical analysis. The concept and definition of acids and bases. Consideration of acid-base balance. Seminar: Solving problems.
Week 6: Acid-base equilibrium, acidity, pH buffers. Seminar: Solving problems
Week 7: I. Partial test (theoretical and seminar materials). Solving test
Week 8: Concept and definition of complex ions, complexometric equilibrium, kinetics of complex formation. Seminar: Solving problems
Week 9. Consideration of complexometric equilibrium. Seminar: Solving problems.
Week 10: Concept and definition of the electrochemical reaction. Consideration of equilibrium electrochemical reactions. Seminar: Solving problems
Week 11: Concept and definition of the redox reaction. Consideration of equilibrium electrochemical reactions. Seminar: Solving problems.
Week 12: Concept and definition of heterogeneous equilibrium. Consideration of the process of dissolution and precipitation. Seminar: Solving problems
Week 13: Concept and definition of extraction. Simple and complex extraction. Extraction of weak acids and metal cations from solution. Seminar: Solving problems
Week 14: Concept and definition of chromatography. Analytical separation by chromatography. Seminar: Solving problems
15th week: II. Partial test (theoretical and seminar materials). Solving test

Format of instruction:

Student responsibilities

The 80% presence at lectures and completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

1. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju I. dio, Redak, Split, 2013.
2. R. Kellner, J. M. Mermet, M. Otto, M. Valcarcel and H. M. Widmer (Urednici), Analytical Chemistry (A Modern Approach to Analytical Science, Second Edition) Wiley-VCHVerlag Gmbh & Co. KGaA, Weinheim, 2004.
3. D. A. Skoog, D. M. West, F. J. Holler and S. R. Crouch, Fundamentals of Analytical Chemistry, Eighth Edition, Thompson Brooks/Cole, Belmont, USA, 2004.
4. G. D.Christian, Analytical Chemistry, Sixth Edition, John Willey & Sons, INC, 2004.
5. D. Harvey, Modern Analytical Chemistry, McGraw-Hill Higher Education, New York, London, 2000.
6. F. W. Fifield & D. Kealey, Principles and Practice of Analytical Chemistry, Blackwell Science Ltd, Malden MA, London, 2000.
7. M. Kaštelan-Macan, Enciklopedijski rječnik analitičkog nazivlja, FKIT, Mentor, Zagreb 2014.

Quality assurance methods that ensure the acquisition of exit competences

- registration of student’s presence in class
- annual analysis of students success in this course
- student’s survey in order to evaluate the professor

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The aim is to familiarize students with the mechanisms and equilibrium of homogeneous and heterogeneous chemical reactions and their application in analytical methods and qualitative determination.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Analytical Chemistry I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Plan and conduct chemical experiments on the basis of theoretical knowledge and predictions based on calculations, Systematics cations and anions

Course content broken down in detail by weekly class schedule (syllabus)

1. Week: Introduction in laboratory work, Basic laboratory operations. (3 hours)
2. Week: Qualitative chemical analysis – determination of groups of cations. (3 hours)
3. Week: Qualitative chemical analysis – determination of cations in groups (6 hours)
4. Week: Determination of cations in the mixture. (hours)
5. Week: Qualitative chemical analysis – determination of groups of anions (3 hours)
6. Week: Qualitative chemical analysis – determination of anions in groups (6 hours)
7. Week: Determination of aniona in the mixture (6 hours)
8. Week: extraction (4 hours)
9. Week: chromatography (4 hours)
10. Week: ionic exchange (4 hours)

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

1. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju, Školska knjiga, Zagreb, 2016.

Quality assurance methods that ensure the acquisition of exit competences

- Completed all laboratory exercises
- annual analysis of students success in this course
- student’s survey in order to evaluate the professor

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Course enrolment requirements and entry competences required for the course

Introduce students to the chemistry of transition metals and to the structure and properties of their compounds. Applying important theoretical principles of atomic theory and chemical bonding in explanation of structure of complex compounds with examples of their use and importance in bioinorganic and organometallic chemistry.

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

At the end of the course students will:
- know the characteristic properties and reactions of transition metal
- be able to predict physical and chemical properties of transition metals compounds based on the knowledge of their structure
- be able to determine the structure and predict the properties of complex ions and their compounds
- be able to predict the influence of ligands on the properties of complex ions and their compounds
- understand the basic problems in bioinorganic and organometallic chemistry

Course content broken down in detail by weekly class schedule (syllabus)

1. lecture: Introduction to the Chemistry of transition elements
2. lecture: Group III PSE, lanthanides and actinides
3. lecture: IV and V groups PSE
4. lecture VI and VII of the PSE Group
5. lecture: VIII and IX of the PSE Group
6. lecture: X, XI and XII PSE group
7. lecture: Complex compounds, types of ligands, isomerism, the application of valence bond theory
8. lecture: Theory of crystal field
9. lecture: Theory of molecular orbitals (LCAO) and photoelectron spectroscopy, symmetrical operations
10. lecture: ligand field theory.
11. lecture: The stability of complex compounds, thermodynamic and kinetic
12. lecture: Spectroscopic and magnetokemijsko behavior of complex compounds.
13. lecture: Organometallic compounds.
14. lecture: Bioinorganic Chemistry.
1. seminar: Transition elements,
2. seminar: Elements of 4th-5th PSE group
3. seminar: Elements 5th-6th PSE group
4. seminar: Elements of 7th-8th PSE group
5. seminar: Elements of 9th-10th PSE group
6. seminar: Elements of 11th-12th PSE group
7. seminar: Coordination nomenclature
8. seminar: isomerion complex compounds
9. seminar: The structure of complex ions, magnetic properties
10. seminar: Forecasting the colors of the complex based on the type of ligand and cleavage d orbitals of the metal ion
11. seminar: Determining the structure of a complex compound on the basis of experimental results
12. seminar: Identifying stable complexes
13. seminar: Organometallic Compounds
14. seminar: Bioinorganic Chemistry

Format of instruction:

Student responsibilities

The 80% presence at lectures and seminars, and completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Filipović, I., Lipanović, S., Opća i anorganska kemija I i II dio, Školska knjiga, Zagreb, 1995

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Exercising, testing and confirm knowledge from lectures. Understanding with the methods of experimental work and the acquisition of skills necessary for independent work in the lab.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Inorganic Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students will upon completion of the course be able to:
1. Practically through experiments verify the theoretical assumptions
2. Gain independence in performing experiments
3. Design simple experiments to illustrate the chemical properties of the substance
4. Actively exploring ways in which this discipline has consequently impact on the outside world.

Course content broken down in detail by weekly class schedule (syllabus)

In the frame of laboratory exercises students will perform exercises independently from the content of these topics:
Exercises :
Exercise 1
Changing the coordination number of compounds - Complexes of nickel
Exercise 2
Preparation of potassium trioxalatoferrate(III) trihydrate and preparation of potassium tetraperoxochromate(V)
Exercise 3
Determination of composition of the potassium trioxalatoferrate(III) trihydrate and potassium tetraperoxochromate(V).
Exercise 4
Preparation of ammonium manganese(II) phosphate monohydrate; Preparation of ferric(III) chloride; Preparation of chromium (III) oxide
Exercise 5
Preparation of [CoCl(NH3)5]2+ complex.
Exercise 6
Hydration of [CoCl(NH3)5]2+ complex.

Format of instruction:

Student responsibilities

Completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Course enrolment requirements and entry competences required for the course

The goal of course is to familiarize students with the mechanisms and equilibrium of homogenous and heterogeneous chemical reactions and their applications in analytical methods for determining process. Theoretical basis of kinetic methods of analysis will be explained.

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

1. Calculate and predict the acid-base titration curve. Apply acid-base titration based on theoretical predictions.
2. Explain the method of calculating pM values different parts of the EDTA titration curves, based on the application of knowledge of the equilibrium of complex formation.
3. Construct the redox titration curve and anticipate the possibility of using visual redox indicators based on theoretical predictions.
4. Define and apply the precipitation requirements.
5. Calculate and predict the precipitation titration curve.
6. Compare kinetic methods of analysis and classical analytical methods based on thermodynamic equilibrium, in terms of selectivity and application options.
7. Solve numerically analytical problems.

Course content broken down in detail by weekly class schedule (syllabus)

1st week
Lectures: Gravimetric analysis.
Seminars: Gravimetric analysis (numerical examples).
2nd week
Lectures: Precipitation gravimetry, properties of precipitate and precipitation requirements.
Seminars: Gravimetric analysis (numerical examples).
3rd week
Lectures: Quantitative determination, titrations, standard preparation.
Seminars: Quantitative determination, titrations, standard preparation (numerical examples).
4th week
Lectures: Precipitation titrations.
Seminars: Precipitation titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
5th week
Lectures: Precipitation titration, End –point detection.
Seminars: Precipitation titrations (numerical examples, titration curve construction, using of the Excel spreadsheet)
6th week
Lectures: Acid-base titrations, titration of the strong acid with strong base and strong base with strong acid. Titration of the weak acid with strong base and weak base with strong acid.
Seminars: Acid-base titrations (numerical examples, titration curve construction, using of the Excel spreadsheet)..
7th week
Lectures: Titrations in polyprotic systems. Finding the end point with pH electrode.
Seminars: Acid-base titrations (numerical examples, titration curve construction, using of the Excel spreadsheet)..
8th week
Lectures: Finding the end point with visual indicators. Titration in nonaqueous solvents.
Seminars: Acid-base titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
9th week
Lectures: EDTA titrations. The impact of conditional formation constants on the inflection of the EDTA titration curves.
Seminars: EDTA titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
10th week
Lectures: Auxilary complexing agents. Metal ion indicators.
Seminars: EDTA titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
11th week
Lectures: Redox titrations. Redox titration based on the simple stochiometry redox reaction.
Seminars: Redox titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
12th week
Lectures: Redox titration based on the complex stochiometry redox reaction, the effect of pH value.
Seminars: Redox titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
13th week
Lectures: Analysis of a mixture. Finding the end point of redox titrations.
Seminars: Redox titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
14th week
Lectures: Adjustment of analyte oxidation state. Preparation and standardization of titration standards.
Seminars: Redox titrations (numerical examples, titration curve construction, using of the Excel spreadsheet).
15th week
Lectures: Kinetic method analysis.
Seminars: Kinetic method analysis (numerical examples).

Format of instruction:

Student responsibilities

The 70% presence at lectures and seminars

Optional literature (at the time of submission of study programme proposal)

1. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju I. dio, Redak, Split, 2013.
2. R. Kellner, J. M. Mermet, M. Otto, M. Valcarcel and H. M. Widmer (Urednici), Analytical Chemistry (A Modern Approach to Analytical Science, Second Edition) Wiley-VCHVerlag Gmbh & Co. KGaA, Weinheim, 2004.
3. D. A. Skoog, D. M. West, F. J. Holler and S. R. Crouch, Fundamentals of Analytical Chemistry, Eighth Edition, Thompson Brooks/Cole, Belmont, USA, 2004.
4. G. D.Christian, Analytical Chemistry, Sixth Edition, John Willey & Sons, INC, 2004.
5. D. Harvey, Modern Analytical Chemistry, McGraw-Hill Higher Education, New York, London, 2000.
6. F. W. Fifield & D. Kealey, Principles and Practice of Analytical Chemistry, Blackwell Science Ltd, Malden MA, London, 2000.
7. M. Kaštelan-Macan, Enciklopedijski rječnik analitičkog nazivlja, FKIT, Mentor, Zagreb 2014.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Students gain basic knowledge of working in the analytical laboratory, the proper approach to chemical analysis of samples, the possibility of critical reasoning based on knowledge, the chemical changes in the experimental work , correct writing lab reports in accordance with good laboratory practices.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Analytical Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

1. Apply standard laboratory procedures in gravimetric analysis.
2. Apply titration based on homogenous or heterogeneous equilibrium with previous theoretical predictions.
4. Apply the principles of good laboratory practice.
5. Properly collect and process numerical data.
6. Write the appropriate laboratory report.

Course content broken down in detail by weekly class schedule (syllabus)

1. (6 hours) Determinations based on heterogeneous equilibrium. Argentometric titration.
2. (6 hours) Potentiometric titration.
3. (6 hours) Gravimetric determination of sulphate ion.
4. (6 hours) Gravimetric determination of nickel ion.
5. (4 hours) Preparing standard solution, acid-base titration.
6. (6 hours) Acid-base titration, determination of H2C2O4.
7. (6 hours) Finding the end point with pH electrode.
8. (4 hours) Preparing standard solution, EDTA titration.
9. (6 hours) EDTA titration, determination of Fe3+.
10. (4 hours) Preparing standard solution, redox titration.
11. (6 hours) Redox titration, determination of Cu2+.

Format of instruction:

Student responsibilities

Students must attend classes regularly and do all laboratory exercises in planned program.

Optional literature (at the time of submission of study programme proposal)

1. D.A. Skoog, D.M. West, F.J. Holler, Osnove analitičke kemije, šesto izdanje (englesko), prvo izdanje (hrvatsko), Školska knjiga, Zagreb, 1999.
2. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju, Zagreb, 2016.
3. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju I. dio, Redak, Split, 2013..
4. M. Kaštelan-Macan, Kemijska analiza u sustavu kvalitete, Školska knjiga, Zagreb 2003.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Students gain basic knowledge of working in the analytical laboratory, the proper approach to chemical analysis of samples, the possibility of critical reasoning based on knowledge, the chemical changes in the experimental work , correct writing lab reports in accordance with good laboratory practices.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Analytical Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

1. Apply standard laboratory procedures in gravimetric analysis.
2. Apply titration based on homogenous or heterogeneous equilibrium with previous theoretical predictions.
4. Apply the principles of good laboratory practice.
5. Properly collect and process numerical data.
6. Write the appropriate laboratory report.

Course content broken down in detail by weekly class schedule (syllabus)

1. (6 hours) Determinations based on heterogeneous equilibrium. Argentometric titration.
2. (6 hours) Potentiometric titration.
3. (6 hours) Gravimetric determination of sulphate ion.
4. (6 hours) Gravimetric determination of nickel ion.
5. (4 hours) Preparing standard solution, acid-base titration.
6. (6 hours) Acid-base titration, determination of H2C2O4.
7. (6 hours) Finding the end point with pH electrode.
8. (4 hours) Preparing standard solution, EDTA titration.
9. (6 hours) EDTA titration, determination of Fe3+.
10. (4 hours) Preparing standard solution, redox titration.
11. (6 hours) Redox titration, determination of Cu2+.

Format of instruction:

Student responsibilities

Students must attend classes regularly and do all laboratory exercises in planned program.

Optional literature (at the time of submission of study programme proposal)

1. D.A. Skoog, D.M. West, F.J. Holler, Osnove analitičke kemije, šesto izdanje (englesko), prvo izdanje (hrvatsko), Školska knjiga, Zagreb, 1999.
2. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju, Zagreb, 2016.
3. Nj. Radić i L. Kukoč Modun, Uvod u analitičku kemiju I. dio, Redak, Split, 2013..
4. M. Kaštelan-Macan, Kemijska analiza u sustavu kvalitete, Školska knjiga, Zagreb 2003.

Quality assurance methods that ensure the acquisition of exit competences

Quality assurance will be performed at three levels:
(1) University Level; (2) Faculty Level by Quality Control Committee; (3) Lecturer’s Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquisition of basic knowledge of modern organic chemistry, understanding the structure and properties of organic compounds, nomenclature of organic compounds, the types of isomers, spectroscopic techniques in determining organic structures, understanding the mechanisms of organic reactions of addition, substitution, elimination and rearrangement.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Laboratory exercises in organic chemistry I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the course, students will be able to:
- describe the basic concepts, nomenclature of organic compounds, stereochemistry, and typical organic reactions of addition, elimination, substitution and rearrangement
- illustrate modes of applying the nomenclature, isomerism, stereochemistry and mechanisms of organic reactions (ion type and radical type)
- determine the structure of simple organic compounds on the basis of spectroscopic methods
- propose mechanisms for nucleophilic substitution reactions at saturated carbon and elimination reactions, additions to the unsaturated carbon and electrophilic aromatic substitution, taking into account the regio-selectivity / specificity and stereo-selectivity / specificity
- choose the correct chemical approach to solving problems in the field of organic chemistry, starting from the acquired knowledge in general, analytical and physical chemistry

Course content broken down in detail by weekly class schedule (syllabus)

Introduction. A short historical overview. The modern organic chemistry. The binding in organic molecules. Electronegativity and bond types. Quantum mechanics and atomic orbitals. Electronic configuration. Lengths and bond energies. (3 hours); Hybrid atomic orbitals (sp3, sp2 and sp). Molecular orbitals (σ- and π-bonds), polar and non-polar covalent bond. Bonding angles. Examples of organic molecules (orbital images) with single, double and triple bond. (3 hours); Physical properties, molecular structure and intermolecular bonds (dipole-dipole, van der Waals and hydrogen bonding). Solubility in organic solvent. Examples. Presentation of organic structures. (3 hours)
Classification and nomenclature of organic compounds. Functional groups and priority order. Alkanes. Alkenes. Alkynes. Aromatic hydrocarbons. Examples of the nomenclature of branched acyclic and cyclic and aromatic hydrocarbons. Alcohols. Phenols. Thiols. (3 hours); Ethers. Thioethers. Amines. Organohalogen compounds. Aldehydes. Ketones. Carboxylic acids. Carboxylic acid derivatives (acyl halides, anhydrides, esters, amides and nitriles). (3 hours); Examples of the nomenclature of various functional groups. (3 hours)
Isomers. Constitutional isomers. Index of hydrogen deficiency (IHD). The conformation and configuration. Stereoisomers. Conformations of acyclic alkanes (conformational analysis). (3 hours); Conformations of cycloalkanes (angle tension and heat of combustion). Substituted cycloalkanes. Geometric isomers of alkenes, aldoximes, ketoximes and azo compounds (cis, trans, E, Z, sin, anti). CIP rule sequence. (3 hours); Examples of geometric isomers of molecules with multiple double bonds. Geometric isomers of cyclic compounds (cis, trans isomers conformational structure). Symmetry, chirality and achirality. Stereogenic center (chiral center). Enantiomers. Diastereomers. (3 hours); The absolute configuration. CIP system - rule sequences. Fischer projection formula. The properties of the enantiomers. Optical activity. The racemic mixture. Enantiomeric excess. The optical purity. The biological significance of chirality. Examples of chiral biologically active substances. (3 hours); The separation of the racemate (direct crystallization, converting into diastereomers, chromatographic methods and kinetic resolution). Molecules having multiple stereogenic centers. Relative configuration erythro- and threo. Meso compounds. Stereoisomers of cyclic compounds. Chiral molecules without tetrahedral atoms. Examples of different kinds of stereoisomers. (3 hours)
Determination of organic structures. Introduction. Mass spectrometry (MS). Resolution. The molecular ion. Isotopes. Fragmentation. Examples of mass spectra. Electromagnetic radiation. Ultraviolet and visible spectroscopy (UV / Vis). Infrared spectroscopy (IR). Nuclear magnetic resonance (NMR). 13C NMR. 1H NMR. Chemical shift. Spin-spin coupling. Examples of the IR and NMR spectra. (11 hours)
Types of organic reactions. Mechanisms. Acid-base reactions. Nucleophiles and electrophiles. Redox reactions. Energy and reaction kinetics. (4 hours)
Nucleophilic substitution at saturated carbon. SN2-mechanism. SN1-mechanism. Energy diagrams. The stereochemistry of the nucleophilic substitution. (3 hours); Variables in the nucleophilic substitution of (leaving group, nucleophile, position of substitution and solvent). Conditions of SN2 and SN1-reaction. Competitive reactions. (3 hours); Nucleophilic substitution possibilities, conventional nucleophiles and their products. Examples. Elimination reactions. E1 and E2 mechanism. Conditions of E1 and E2 reactions. Orientation of elimination. The stereochemistry of the elimination (anti- or sin-) (3 hours); Competition elimination and substitution (reaction process conditions and examples). Examples of elimination reactions: dehydrogen-halogenation, dehalogenation of vicinal dihalogenalkanes, double dehydrogenation, dehydratation of alcohols (E1 and E2 mechanism, energy diagrams). (3 hours)
Electrophilic Addition. Orientation and additions (regioselectivity). The stereochemistry of the addition (anti- or sin-). Addition of free radicals. The addition of hydrogen. The addition of halogen. Halohydrin reaction. The addition of hydrogen halide. Conditions of Markovnikov and anti-Markovnikov addition. (3 hours); Hydration. Oxymercuration / demercuration. Hydroboration. Epoxidation - hydroxylation. Oxidation of alkenes with KMnO4 and OsO4. The ozonolysis of alkenes. The addition of alkenes (alkylation). (3 hours); Polymerization (radicals type and ions type). Examples of typical polymers. The additions to alkynes. Examples. Summary of the reaction of alkanes, alkenes, alkynes and halogenoalkanes. (3 hours)
Aromatic compounds and antiaromatics. The structure of benzene. Examples. Mechanism of electrophilic aromatic substitution. The impact on the groups on electrophilic aromatic substitution. (3 hours); Multiple substitutions of substituted aromatic compounds. Arenes. Phenols. Aromatic amines. Examples. (3 hours)

Format of instruction:

Student responsibilities

Students are required to attend classes (lectures and seminars) and actively participate in the teaching process, which will be evaluated in the final assessment by the weight coefficient of 5%.

Optional literature (at the time of submission of study programme proposal)

Clayden, Greeves, Warren and Wothers, Organic Chemistry, Oxford University Press, 2001.
S. Borčić, O. Kronja, Praktikum preparativne organske kemije, Školska knjiga Zagreb, 1991.

Quality assurance methods that ensure the acquisition of exit competences

Monitoring of quality assurance will be performed at three levels:
(1) University; (2) Faculty Level by Quality Control Committee; (3) Academic Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquisition of basic knowledge of practical work in organic-chemical laboratory in line with modern trends in organic chemistry.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Organic chemistry I

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the course, students will be able to:
- describe basic laboratory procedures in organic-chemistry laboratory
- demonstrate fundamental processes in organic-chemical laboratory, the simple methods of synthesis of organic compounds and determination the functional groups
- determine the structure of simple organic compounds using spectroscopic methods
- propose basic laboratory procedures in accordance with set-up objectives (synthesis or isolation)

Course content broken down in detail by weekly class schedule (syllabus)

Preparing for laboratory work, conducting laboratory diary and account of reaction yields. Isolation and purification of organic compounds. Recrystallization. Sublimation. Extraction. Distillation. Chromatography. (5 hours) Qualitative element analysis of organic compounds. The solubility of organic compounds. Detection of functional groups of organic compounds. Spectroscopic methods of organic analysis. (10 hours) Organic reactions and preparation of compounds. Oxido-reduction reactions. Nucleophilic substitution and elimination reactions at saturated carbon Electrophilic aromatic substitution. (15 hours)

Format of instruction:

Student responsibilities

Optional literature (at the time of submission of study programme proposal)

I. Borčić, O. Kronja, Praktikum iz preparativne organske kemije, Školska knjiga Zagreb, 1991.

Quality assurance methods that ensure the acquisition of exit competences

Monitoring of quality assurance will be performed at three levels:
(1) University; (2) Faculty Level by Quality Control Committee; (3) Academic Level.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquisition of basic knowledge about chemistry of carbonyl compounds, carboxylic acid and derivatives, heterocycles and carbohydrates.
This course is basis for understanding other courses, such as Natural products, Organic synthesis, Organic analysis, Biochemistry.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Experimental Organic Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the exam students will be able to:
- recognize and give the IUPAC name to carbonyl compounds, carboxylic acids and derivatives, heterocycles and carbohydrates, and draw the corresponding structural formula based on systematic name (apply basic rules of organic compounds nomenclature)
- connect organic compounds molecular structure with their physico - chemical
properties and reactivity
- differentiate, describe and compare reaction mechanisms of nucleophilic addition and nucleophilic substitution at carbonyl group
- specify the most important reactions of carbonyl and carboxylic compounds
- describe heterocycles and carbohydrates reaction mechanisms, specify the most important reactions of these compounds
- solving problems regarding carbonyl compounds, carboxylic acid and derivatives, heterocycles and carbohydrates

Course content broken down in detail by weekly class schedule (syllabus)

Lectures (2 hours weekly):
1st week: Introduction to course (course content, students responsibilities, terms and conditions for passing exam). Nucleophilic aromatic substitution. Addition-elimination mechanism. Elimination-addition mechanism. Aryl cation mechanism.
2nd week: Polycyclic aromatic compounds - sources. Polycyclic aromatic compounds reactions. Nucleophilic addition to carbonyl group - introduction. Cyanide as a nucleophile (cyanohydrin formation).
3th week: Oxygen and sulphur as nucleophiles. Addition of alcohols (hemiacetals and acetals formation). Addition of water (hydrates formation). Addition of thiols (hemithioacetals and thioacetals formation). Hydride as a nucleophile - reduction. Reduction by complex metal hydrides. Cannizzaro reaction -disproportionation.
4th week: Carbon as a nucleophile - organometallic compounds. Organometallic reagents synthesis. Grignard reaction. Syntheses using Grignard reagents.
5th week: Nitrogen as a nucleophile. Imines. Enamines. Nucleophilic addition to carbonyl related compounds. Nucleophilic addition to imines. Nucleophilic addition to enamines. Nucleophilic addition to nitriles.
6th week: Nucleophilic acyl substitution - introduction. Carboxylic acids and derivatives reactivity. Oxygen and sulfur as nucleophiles. Substitution with alcohols - esterification. Lactonization. Transesterification. Substitution with water - hydrolysis.
7th week: Substitution with thiols. Nitrogen as a nucleophile. Acyl halides and anhydrides. Acyl halide synthesis. Anhydride synthesis.
8th week: Hydride as a nucleophile - reduction. Carbon as a nucleophile - organometallic reagents. Reactions with esters. Reactions with acyl halides. Reactions with carboxylic acids.
9th week: Nucleophilic substitution on derivatives of sulfuric and phosphoric acid. Nucleophilic reactions involving enolate anions. Enols and enolate anions. Enolization (keto-enol tautomerism). The aldol reaction.
10th week: Mixed aldol reaction. Dehydration of aldol products. Ester condensation – Claisen condensation.
11th week: Mixed Claisen condensation. -dicarbonyl compounds splitting. Reverse Claisen reaction. Decarboxylation.
12th week: Alkylation of enolate anions. Active methylene compounds.
Conjugate addition reactions. Electrophilic conjugate addition - conjugated dienes.
13th week: Nucleophilic conjugate addition - ,-unsaturated carbonyl compounds. Michael reaction. Diels-Alder cycloaddition.
14th week: Carbohydrates – definition and classification. Cyclic forms of monosaccharides and their representation. Reactions of monosaccharides. Oxidation. Reduction. Monosaccharides in aqueous solution (mutarotation). Monosaccharides in alkaline or acidic solution.
15th week: Glycosides. Typical disaccharides and polysaccharides.
Heterocyclic compounds (five-membered and six-membered heterocycles). Structures and stability of aromatic heterocycles. Electrophilic and nucleophilic aromatic substitution reactions.
Seminars (1 hour weekly):
Solving problems in organic chemistry.

Format of instruction:

Student responsibilities

Students are required to attend lectures and seminars in the amount of at least 80% of the times scheduled and complete all laboratory exercises (100% attendance). Active participation in teaching process will be also evaluated in the final score.

Optional literature (at the time of submission of study programme proposal)

T. W. Solomons & C. B. Fryhle, Organic Chemistry, John Wiley & Sons, Inc., New York, 2004.
J. Clayden, N. Greeves, S. Warren, P. Wothers, Organic Chemistry, Oxford University Press, Oxford, 2005.

Quality assurance methods that ensure the acquisition of exit competences

Monitoring of quality assurance will be performed at three levels:
(1) University Level, conducting surveys of students on teaching quality;
(2) Faculty Level, by Quality Control Committee;
(3) Lecturer’s Level, monitoring and accepting suggestions of students and colleagues

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquisition of basic knowledge and working skills in organic laboratory, application of laboratory methods and techniques for laboratory synthesis, isolation, characterization and purification of organic compounds.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Organic Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the course students will be able to:
- perform independently laboratory exercises according to laboratory procedures
- apply basic laboratory procedures and techniques for synthesis, isolation and purification of organic compounds as well as their characterization and identification
- connect theoretical knowledge gained throughout lectures in organic chemistry with experimental work
- propose basic laboratory procedures in accordance with set-up objectives (organic compound synthesis or isolation)

Course content broken down in detail by weekly class schedule (syllabus)

Exercises (3 hours weekly joined together in 7 lab periods):
1. Nucleophilic substitution at acyl carbon. Acetanilide synthesis. (1 lab period)
2. Electrophilic aromatic substitution. p-Nitroacetanilide synthesis. p-Nitroaniline synthesis. (2 lab periods)
3. Nucleophilic aromatic substitution. Diazotation. Phenol synthesis. (2 lab periods)
4. Nucleophilic addition at carbonyl group. The Cannizzaro reaction – benzyl alcohol and benzoic acid synthesis. (1 lab period)
5. Organic compounds characterization. Determination of physical constants and spectroscopic analysis (UV/VIS and FT-IR spectra recording and interpretation). (1 lab period)

Format of instruction:

Student responsibilities

Students have to complete all planned laboratory exercises (100% of the times scheduled) and active participate in laboratory work.

Optional literature (at the time of submission of study programme proposal)

S. Borčić, O. Kronja, Praktikum preparativne organske kemije, Školska knjiga, Zagreb, 1991.
V. Rapić, Postupci priprave i izolacije organskih spojeva, Školska knjiga, Zagreb, 1994.

Quality assurance methods that ensure the acquisition of exit competences

Monitoring of quality assurance will be performed at three levels:
(1) University Level, conducting surveys of students on teaching quality;
(2) Faculty Level, by Quality Control Committee;
(3) Lecturer’s Level, monitoring and accepting suggestions of students and colleagues

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The aims of the course are to enable students to:
- understand chemical and electrochemical kinetics which is raised at a higher level,
- understand processes and equilibriums in electrolyte solutions, and understand of surface dynamics,
- resolve different physicochemical problems,
- apply acquired knowledge and skills in professional and specialist courses.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Physical Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Upon successful completion of the program, students will be able to:
1. Describe and explain mechanism and kinetics of complexs reactions.
2. Describe and explain various equilibriums in the electrolyte solutions.
3. Describe and explain equilibrium and dynamics of processes on solid and liquid surfaces.
4. Calculate physicochemical parameters using thermodynamic and kinetic equations.
5. Interpret experimental and numerical data.

Course content broken down in detail by weekly class schedule (syllabus)

Lectures (2 hours weekly):
1st, 2nd and 3rd week: Ionic equilibria: The solute activity in molality scale. Mean activity coefficient of electrolyte. Debye-Hückel theory. Colligative properties of electrolyte solutions. Acid-base equilibria in water medium. Solubility of slightly soluble salts. The solubility constant. The common-ion efect. The activity coefficient from measurement of solubility.
4th, 5th, and 6th and 7th week: Equilibrium electrochemistry: Thermodynamic functions of the ion formation. Electrochemical cells. Galvanic cells. Half-reactions and electrodes. Reactions at electrodes. The cell reaction. The potential difference of the cell. Standard electrode potentials. Cells at equilibrium. Types of electrode. Types of galvanic cells. The liquid junction potential and transference number. The solobility constant from potential difference mesurements of the cell. The determination of pH. The determination of thermodynamic functions. Diffusion potential.
8th, 9th and 10th week: The kinetics of complex reactions: Chain reactions. The structure of chain reactions. The rate laws of chain reactions. The explosion. Polymerization kinetics. Chain polymerization. Stepwise polymerization. Photochemical reactions and their quantum yields. Molecular reaction dynamics. Reactive encounters. Activated complex theory. Catalysis. Kinetics in the liquid phase. Primary kinetic salt efect.
11th, 12th and 13th week: The properties of surfaces (Surface dynamics): Types of disperse systems. Colloidal systems. The properties of liquid surfaces. Solid surfaces: surfaces growth and surface composition and structure. Physisorption and chemisorption. Adsorption isotherms. Langmuir isotherm. Catalytic activity at surfaces. Mechanisms af heterogeneous catalysis. Use of adsorption measurements to determine surface area: Low-energy electron diffraction. Electron emission from surfaces (photoelectron spectroscopy).
14th and 15th week: Dynamic electrochemistry: Processes at electrodes. The electrical double layer. The rate of charge transfer. Polarization. Electrochemical processes. Electrolysis. The characteristics of working cells. Fuel cells and secondary cells. Corrosion. The rate of corrosion. The inhibition of corrosion.
Seminars (one hour weekly):
Solving numerical problems in physical chemistry.

Format of instruction:

Student responsibilities

Lecture and seminar attendance and active participation of at least 70 percent of the planned schedule.
The exam can be taken continuously (cumulatively) through colloquiums (partial tests) combining theoretical and practical tasks or as one comprehensive exam (written and oral).

Optional literature (at the time of submission of study programme proposal)

I. Mekjavić, Fizikalna kemija 2, Golden marketing, Zagreb, 1999.
P. Atkins, J. de Paula, Atkins’ Physical Chemistry, 8th Edition, Oxford University Press, Oxford, 2006.

Quality assurance methods that ensure the acquisition of exit competences

- monitoring suggestions and reactions of participants during the semester
- student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The aims of the course are to enable students to:
- perform measurements in the laboratory individually or in a team, present and process measurement data.
- apply acquired knowledge and skills in professional and specialist courses.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Physical Chemistry II

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Upon successful completion of the program, students will be able to:
1. Perform experiments and measurements in the laboratory.
2. Explain different physicochemical dependencies of the examined systems.
3. Calculate physicochemical parameters using thermodynamic and kinetic equations.
4. Interpret experimental and numerical data.

Course content broken down in detail by weekly class schedule (syllabus)

Exercises in Laboratory for Physical Chemistry (5 hours weekly):
1. week: Vapour pressure of pure liquid.
2. week: Surface tension and refractometric determination of composition of two-component mixture.
3. week: Viscosity.
4. week: Colligative properties.
5. week: Adsorption from aqueous solution.
6. week: Equilibrium constant of homogeneous reaction.
7. week: Phase diagram for three-component system.
8. week: Transference numbers by Hittorf method.
9. week: Conductometry and conductometric titrations.
10. week: Galvanic cell and electrode potentials.
11. week: Rate constant of inversion of sucrose by polarimetric method.
12. week: Conductometric determination of the rate constant of hydrolysis of ethyl acetate.

Format of instruction:

Student responsibilities

Completed all laboratory exercises (100 %).
Student must show theoretical knowledge before each practical work or experiments (12 partial oral exams).
Student must write 12 reports with complete experimental and calculated data: All reports should contains tables and graphical dependencies. At the end of report put conslusion.

Optional literature (at the time of submission of study programme proposal)

A. M. Halpern, Experimental Physical Chemistry, A Laboratory Textbook, 2nd Edition, Prentice Hall, New Jersey, 1997.

Quality assurance methods that ensure the acquisition of exit competences

- monitoring suggestions and reactions of participants during the semester
- student survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

- acquiring knowledge about the role of catalysts in chemical reaction
- identify the key variables for the preparation of better catalysts
- overview of the processes of catalysts preparation
- understanding the importance of catalysts in industry and sustainable development through the improvement of existing or development of new chemical, petrochemical and related processes

Course enrolment requirements and entry competences required for the course

None.

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

After passing the exam, the student is expected to be able to:
- list and describe types of catalysts
- explain the principle of operation of the catalyst in a chemical reaction
- know the role of each component in catalyst system
- explain the processes of catalysts preparation
- explain deactivation, reactivation and regeneration of catalyst
- give examples of the catalyst application in real systems
- to argue the importance of a catalyst for industry and sustainable development

Course content broken down in detail by weekly class schedule (syllabus)

1st week: General concept of catalysis: the definition of catalysis and catalysts, the historical development of catalytic processes, the economic importance of the catalyst.
2nd week: Distribution of catalysis and katalizatora. Comparison of homogeneous and heterogeneous catalysts and the industrial značaj. General theory of catalysis. Effect of catalyst on reaction rates and the position of the chemical equilibrium. The activation energies.
3rd week: The mechanism of catalysis, inhibition, initiation. Basic features of the catalyst: activity, selectivity and stability.
4th week: Homogeneous catalysis in the gaseous and in the liquid phase. Homogeneous catalysis by acids and bases, by ions and transition metal compounds.
5th week: Coordination complexes as catalysts. Metallocenes.
6th week: Heterogeneous catalysis: the basic stages of heterogeneous catalytic reactions. Physical and chemical adsorption and their comparison. The heat of adsorption (Lennard-Jones diagram).
7th week: Types of adsorption isotherms. The basic laws of adsorption. Mechanisms and kinetics of heterogeneous catalytic reactions in the gas phase: Langmuir Hinshelwood mechanism. Eley-Rideal mechanism.
8th week: Theories of the catalytic activity of heterogeneous catalysts: the theory of unstable intermediates, the theory of active centers, the theory of geometric factors.
9th week: Theory of electronic factors. The selectivity of catalysts.
10th week: Durability (stability) and resistance to deactivation. Poisoning and selectivity coefficient of toxicity. Deactivation of the catalyst layers on the surface. Deactivation by sintering and phase transformation. Loss of catalyst by evaporation. Mechanical disintegration of the catalyst. Prevention of deactivation. Reactivation and regeneration of the catalyst.
11th week: Zeolites: properties, catalytic properties, selectivity. Zeolite modification processes.
12th week: Design of heterogeneous catalysts: active components, carriers, promoters, moderators, inhibitors, activators.
13th week: Characterization of heterogeneous catalysts. Determination of physical properties of the catalyst: the volume and the pore size, the total area of the catalyst. Mechanical properties of the catalyst.
14th week: Methods of heterogeneous catalysis: the precipitated catalysts impregnated catalysts, skeletal catalysts, catalysts with active coating. Monolithic catalysts.
15th week: Biocatalysts. Final comments, discussion, conclusions.

Format of instruction:

Student responsibilities

Attending lectures and seminars in the 80% amount of the total number of lessons.