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

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 Exercises in 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.

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

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

- 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 (3 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
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. (1.5 hours)
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. . (1.5 hours)
4th week: Magnetic field. (3 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
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. (1.5 hours)
Partial assessment (1st preliminary test) related to seminars and theory addressed during the course.
6th week: Alternating currents. Electric machines. (3 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
7th week: Electromagnetic oscillating circuit and radiation. (3 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
8th week: Electromagnetic waves and nature of light. (2 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
9th week: Interaction of electromagnetic radiation and matter: absorption, refraction, reflection, polarization, scattering, photoelectric effect. Ideas of quantum physics. (4 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course. (1.5 hours)
10th week: Physical and geometric optics. (3 hours).
Seminar: Solving the numerical examples pertaining to the theoretical content addressed during the course (1.5 hours)
Partial assessment (2rd 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 fom the field of electromagnetism and optics. Additionaly, the aim is to enable the development of skills needed to conduct experiments, gather dana 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 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 occured during the measurement
- Mastering the evaluation of errors which occured 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”

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)

Format of instruction:

Student responsibilities

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

Acquiring basic basic theoretical knowledge of analytical chemistry, the role and application of analytical chemistry in various fields

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Analytical Chemistry

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
- Understand the concept of quantitative chemical reactions
- Understand the concept of gravimetric and volumetric determination
- Understand the precipitation, neutralization, complexometric and redox titrations
- Solving numerical problems from a qualitative and quantitative chemical analysis

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

First week : Description and review of curriculum. Definitions of analytical chemistry. Division of Analytical Chemistry. The concept of the analytical signal. Seminar: Solving numerical problems from theoretical lecture
Second week : The concept and definition of chemical analysis - qualitative and quantitative. Seminar: Solving numerical problems; homogeneous and heterogeneous equilibrium in analytical chemistry..
3rd week : Qualitative chemical analysis. The concept and definition of acids and bases. Consideration of acid-base balance. Seminar: Solving problems
.4th week : The concept and definition of complex ions., complexometric equilibrium . Seminar: Solving problems
5th week : The concept and definition of electrochemical reactions. Consideration of electrochemical equilibrium. Seminar: Solving problems
6th week: The concept and definition of heterogeneous equilibrium. process of dissolution and precipitation. Seminar: Solving problemsl
7th week .Recapitulation of theoretical and seminars lecture I partial exam .theoretical lecture and seminars
8th week . Quantitative chemical analysis. The concept and definition of gravimetric determination. Seminar: Solving problems,
9th week . optimization of precipitationcondition. Seminar: Solving problems.
10th week : The concept and definition of standards and standard solutions - primary and secondary. The concept and definition of the volumetric determination; Seminar: Solving problems.
11th week : The concept and definition of volumetric determinations- Argentometric titration; Seminar: Solving problems.
12 weeks The concept and definition of volumetric determinations based on neutralization reactions - acid-base titration; Seminar Solving problems
13th week . The concept and definition of volumetric determinations based on the complex - complexometric titrations; Seminar Solving problems
14th week . The concept and definition of volumetric determinations based on redox reactions. Seminar Seminar Solving problems
15th week : Recapitulation of theoretical and seminars lecture II partial exam .theoretical lecture and seminars.

Format of instruction:

Student responsibilities

Lectures attendance - at least 80% and completing exercises

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

Z. Šoljić, Računanje u analitičkoj kemiji, Zagreb, 1998.

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
- professor’s self-evaluation

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

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Analytical Chemistry

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
- Understand the concept of quantitative chemical reactions
- Understand the concept of gravimetric and volumetric determination
- Understand the precipitation, neutralization, complexometric and redox titrations
- Solving numerical problems from a qualitative and quantitative chemical analysis

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

First week : Description and review of curriculum. Definitions of analytical chemistry. Division of Analytical Chemistry. The concept of the analytical signal. Seminar: Solving numerical problems from theoretical lecture
Second week : The concept and definition of chemical analysis - qualitative and quantitative. Seminar: Solving numerical problems; homogeneous and heterogeneous equilibrium in analytical chemistry..
3rd week : Qualitative chemical analysis. The concept and definition of acids and bases. Consideration of acid-base balance. Seminar: Solving problems
.4th week : The concept and definition of complex ions., complexometric equilibrium . Seminar: Solving problems
5th week : The concept and definition of electrochemical reactions. Consideration of electrochemical equilibrium. Seminar: Solving problems
6th week: The concept and definition of heterogeneous equilibrium. process of dissolution and precipitation. Seminar: Solving problemsl
7th week .Recapitulation of theoretical and seminars lecture I partial exam .theoretical lecture and seminars
8th week . Quantitative chemical analysis. The concept and definition of gravimetric determination. Seminar: Solving problems,
9th week . optimization of precipitationcondition. Seminar: Solving problems.
10th week : The concept and definition of standards and standard solutions - primary and secondary. The concept and definition of the volumetric determination; Seminar: Solving problems.
11th week : The concept and definition of volumetric determinations- Argentometric titration; Seminar: Solving problems.
12 weeks The concept and definition of volumetric determinations based on neutralization reactions - acid-base titration; Seminar Solving problems
13th week . The concept and definition of volumetric determinations based on the complex - complexometric titrations; Seminar Solving problems
14th week . The concept and definition of volumetric determinations based on redox reactions. Seminar Seminar Solving problems
15th week : Recapitulation of theoretical and seminars lecture II partial exam .theoretical lecture and seminars.

Format of instruction:

Student responsibilities

Lectures attendance - at least 80% and completing exercises

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

Z. Šoljić, Računanje u analitičkoj kemiji, Zagreb, 1998.

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
- professor’s self-evaluation

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

Basic knowledge in technical drawing, strength of materials, and parts of machinery in chemical industry

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)

- being capable to read and understand technical drawing
- understanding the need for dimensioning machinery parts
- recognising basic machinery parts
- recognising basic parts in chemical industry

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

Week 1: Introduction to mechanical structures. National codes. Technical drawing – basics.
Week 2: Technical drawing – cross sections, displays, dimensions.
Week 3: Technical drawing – surface finishes, tolerances
Week 4: Technical drawing – CAD, rapid prototyping, 3D scanning
Week 5: Basics of mechanics (statics, kinematics, dynamics). Materials for mechanical design. (steel alloys, cast steel materials)
Week 6: Materials for mechanical design. (copper and aluminium alloys)
Week 7: Materials for mechanical design (sinter materials, polymers). Dimensioning of structures.
Week 8: 1st colloquium. Introduction to parts of machinery.
Week 9: Bolts, springs, welding and soldering
Week 10: Shafts and clutch
Week 11: Bearings and transmissions (belt drives, friction drives)
Week 12: Gearing and chain transmissions
Week 13: Mechanical parts in chemical industry (tubes and valves)
Week 14: Vessels and seals
Week 15: 2nd colloquium

Format of instruction:

Student responsibilities

Attending 70% of courses

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

V. Hrgešić i J. Baldani, ”Mehaničke Konstrukcije”, Sveučilište u Zagrebu - Elektrotehnički Fakultet, Zagreb, 1990.
E. Hercigonja, Tehnička grafika, Školska knjiga, Zagreb, 1994.
K.-H. Decker, Elementi strojeva, Tehnička knjiga, Zagreb, 1980

Quality assurance methods that ensure the acquisition of exit competences

Student’s survey

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Acquiring a basic knowledge of basic organic chemistry that involves understanding the structure and properties of organic compounds and mechanisms of organic reactions as well as understanding identification by organic spectroscopy techniques.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Organic Chemistry

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

After completing the course, the student will become familiarized with the major concepts of organic chemistry, which includes:
- identifying and naming of organic compounds according to functional groups and compare their physico - chemical properties;
- learn about the organic compounds isomerism, stereochemical designations, features, and separation;
- learn about organic compounds structure determination by spectroscopy (MS, NMR, IR, and UV/Vis);
- analyze the reactivity of organic compounds with respect to their structure and stereochemistry;
- propose appropriate reaction mechanisms of organic molecules that include addition, substitution and elimination;
- identify and interpret division, structure and properties of natural organic compounds ( carbohydrates, nucleic acids and lipids ).

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

 LECTURES AND SEMINARS:
1. Introduction: What is organic chemistry? History of organic chemistry and its modern role. The main concepts of organic chemistry (functional groups, stereochemistry, curly arrows) (2 hours)
2. The nature of chemical bonds: Electronegativity. Bonds polarity, dipol, and formal charge. Lewis structure. Atomic orbitals. Molecular orbitals. Hybridization (sp3, sp2, sp). Length and energy of the bonds. The molecular geometry. The modified hybrid orbitals. VSEPR theory. (4 hours)
3. Physical properties and intermolecular connections: Van der Waals forces. Dipole - dipole. ”Hydrogen bond”. Solubility in solvents. (2+1 hours)
4. Nomenclature and classes of organic compounds. Hydrocarbons (alkanes, cycloalkanes). Functional groups and acronyms. The nomenclature of hydrocarbons (alkenes, alkynes). Nomenclature organohalogenated compounds, alcohols, amines. Nomenclature of aldehydes and ketones, carboxylic acids, acid derivatives. Systematic (IUPAC) nomenclature. Examples. (7+2 hours)
5. Structure of molecules and isomerism. Constitutional isomers. Alkanes. Isomers. Shapes of molecules and IHD. Stereochemistry. Conformations of alkanes (ethane, butane) and rings (C3, C4, C5, cyclohexane). Mono-substituted cycloalkanes. (3+1 hours)
I. PARTIAL EXAM (written, 1hour and 10 min)
6. Configuration of the cis / trans and E / Z; CIP rule. Conformations of disubstituted cycloalkanes. Alkenes. Chirality and the plane of symmetry. Molecules with one stereocenter. Enantiomers and racemic mixtures. The properties of the enantiomers. Optical activity. Polarimeter. Determination of tetrahedral stereogenic center. Fischer projections. Relative configuration. Molecules with two stereocenter. The properties of enantiomers, diastereomers and meso compounds. The separation of the racemate. Chiral molecules without stereocenter. (9+2 hours)
7. Determining organic structures. Introduction. Mass spectrometry (MS). Resolution. 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 IR, and NMR spectra. (6+3 hours)
8. Organic reactions. Definitions of basic terms. The division of reactions to the change of structure and to the reaction type. Acidity, basicity, and pKa. Factors that enhance the acidity (the size of atoms, electronegativity, resonance, hybridization, inductive effects, charge, solvation, steric effects). Acid - base reactions. The rules for determining the oxidation state of carbon. Oxidation - reduction reactions. Usage of the curly arrows in the reaction mechanism. Intermediates. Nucleophiles and electrophiles. (4 hours)
II. PARTIAL EXAM (written, 1hour and 10 min)
9. Alkanes and cycloalkanes. Oxidation. Halogenation. Alkyl halides. Nucleophilic substitution at the saturated carbon (SN1 and SN2 mechanism). Elimination reactions (E1, E2 mechanisms). Alkenes and alkynes. Electrophilic additions and free radical, polymerization. Conjugated unsaturated compounds. 1,2 - and 1,4 - addition. Aromatic compounds. Electrophilic and nucleophilic aromatic substitution. Phenols. Alcohols and ethers. Organometallic compounds. Aldehydes and ketones. Nucleophilic addition to the carbonyl group. Carboxylic acids and derivatives. Nucleophilic substitution at the carbonyl group. Amines. Heterocyclic compounds. (18+5 hours)
10. Carbohydrates. Amino acids. Nucleic acid. Lipids. (5+1 hours)
III. PARTIAL EXAM (written, 1hour and 10 min)
IV. PARTIAL EXAM (oral, 30 min)

Format of instruction:

Student responsibilities

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

V.Rapić: Nomenklatura organskih spojeva, Školska knjiga , Zagreb, 2004.
S. E. Meislich, H. Meislich & J. Scharefkin, 3000 Solved Problems in Organic Chemistry, The McGraw-Hill, 1994.

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 basic organic chemistry that involves mastering practical laboratory techniques used in the synthesis, isolation, purification and identification of organic compounds.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Organic Chemistry

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

After completing the course, the student will be able to use laboratory techniques (such as recrystallization, distillation, extraction, reflux, chromatography, infrared spectroscopy, etc.), for
(i) purification,
(ii) isolation,
(iii) synthesis, and
(iv) identification of the organic compounds.

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

1. Laboratory safety and rules. Isolation and purification of organic compounds. Crystallization and melting point determination. Distillation. Extraction. Test. (4 hours)
Organic compounds synthesis.
2. Nucleophilic aromatic substitution. The preparation of phenol (diazotation). Test. (9 hours)
3. Nucleophilic addition. The preparation of benzyl-alcohol and benzoic acid (Cannizzaro reaction). Test. (4 hours)
4. Nucleophilic substitution. The preparation of acetanilide (acylation). Test. (4 hours)
5. Electrophylic aromatic substitution. The preparation of p-nitroacetanilide and p-nitroaniline (nitration and hydrolysis). Test. (5 hours)
6. Oxidation-reduction reaction. The preparation of 2-butanone. Test. (4 hours)
Chromatography.
7. Thin-layer chromatography. Column chromatography. Test. (5 hours)
Organic compounds characterization.
8. Characteristic reactions of functional groups. Test. (5 hours)
9. Methods of spectroscopic analysis. (UV/Vis, FTIR). Test. (4 hours)

Format of instruction:

Student responsibilities

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

V. Rapić: Postupci priprave i izolacije prirodnih spojeva, Školska knjiga, Zagreb, 1994.
S. Borčić, O. Kronja, Praktikum preparativne organske kemije, Školska knjiga Zagreb, 1991.
D. Kolbah, Priručnik za kemičare, Kemija u industriji, Zagreb,1986.

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

Student will acquire knowledge about principles of the thermodynamic and kinetic approach to physical and chemical changes.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Physical chemistry

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

After successful completion of the course students will know the basic principles of physical chemistry, which include: 1) physical properties and structure of substances, 2) thermodynamics of mixing, 3) chemical equilibrium, 4) the rates of chemical reactions, 5) molecular motion in gases and the motion of molecules and ions in liquids, 6) electric and magnetic properties of molecules

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

Lectures
1st week: Introduction. Properties of gases. The perfect gas. The states of gases. The gas laws. Real gases. Van der Waals equation. The First Law of thermodynamics. The basic concepts. Work, heat and energy. The formal statment of the First Law
2nd week: Expansion work. Heat and enthalpy. Heat capacity. Thermochemistry. Standard enthalpy changes. Enthalpies of formation. The temperature dependence of reaction enthalpies.
3rd week: Work of adiabatic expansion. Perfect gas adiabats. The Second Law. The dispersal of energy. Entropy. Entropy change during the isothermal expansion of a perfect gas.
4th week: The entropy as a state function. The entropy of irreversible change. Entropy changes accompanying specific processes. The variation of entropy with temperature. The Third Law.
5th week: Third-Law entropies. The Helmholtz and Gibbs energies. Standard molar Gibbs energies. Combining the First and Second Laws. Properties of the internal energy. Properties of the Gibbs energy.
6th week: The chemical potential. Real gases – the fugacity. Standard states of real gases. The relation between fugacity and pressure. Physical transformations of pure substances. Phase boundaries. The dependence of stability on the conditions. The location of phase boundaries.
7th week: The first partial exam. The properties of simple mixtures. Partial molar quantities. The thermodynamics of mixing. The chemical potentials of liquids.
8th week: Liquid mixtures. Colligative properties. The sovent activity. The solute activity. The phase rule. Phase diagrams.
9th week: Two-component systems. Vapour pressure diagrams. Temperature-composition diagrams. Liquid-liquid phase diagrams. Liquid-solid phase diagrams. Three-component systems. Chemical equilibrium. The Gibbs energy minimum. The extent of reaction.
10th week: The reaction Gibbs energy. Exergonic and endergonic reactions. The composition of reactions at equilibrium - the thermodynamic equilibrium constant. Perfect gas equilibria. The general case of a reaction. Le Chatelier’s principle.
11th week: The second partial exam. The rates of chemical reactions. Rate laws and rate constants. Reaction order. The determination of the rate law. Integrated rate laws. First-order reactions. Half-lives. Second-order reactions.
12th week: Reactions approaching equilibrium. The temperature dependence of reaction rates. Elementary reactions. Consecutive elementary reactions. The rate-determing step. The steady-state approximation. Pre-equilibria. Third-order reactions. Unimolecular reactions. Molecules and ions in motion. Molecular motion in gases.
13th week: Viscosity. The conductivity of electrolyte solutions. Strong electrolytes. Weak electrolytes. The drift speed. Ion mobilities. Mobility and conductivity.
14th week: The measurement of transport numbers. Conductivities and ion-ion interactions. Spectroscopy. The electric and magnetic properties of molecules. Permanent and induced electric dipole moments. Polarization at high frequencies. The relative permittivity. Refractive index. Optical activity. Beer-Lambert law.
15th week: Atomic spectra. Molecular spectra. Infrared spectroscopy. Rotational and vibrational spectra. Measurement of IR spectra. Visible and ultraviolet spectroscopy. The Franck-Condon principle. Charge-transfer transitions.
Seminars
Solving numerical problems.

Format of instruction:

Student responsibilities

Students are required to attend classes (lectures and seminars 80%) and actively participate in the teaching process. This will be recorded and evaluated in making a final assessment.

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

I. Tominić, Fizikalna kemija II, Kemijsko-tehnološki fakultet, Split, 2010.

Quality assurance methods that ensure the acquisition of exit competences

Quality of the teaching and learning, monitored at the level of the (1) teachers, accepting suggestions of students and colleagues, and (2) faculty, conducting surveys of students on teaching quality.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

The aim of the course is to train students to work independently in the laboratory of physical chemistry, processing experimental data and presenting the results of data processing in written form.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Physical Chemistry

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

After successful completion of the course students will:
1) be acquainted with the fundamental operating procedures in the laboratory of physical chemistry 2) learn the principles of various laboratory instruments and devices 3) be able to independently perform measurements in the laboratory 4) know about how to process and present the collected data and measurement results using the computer 5) know to identify and independently solve engineering problems

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

1st week: Vapour pressure of pure liquid.
2nd week: Refractometric determination of composition of two-component mixture. 3rd week: Viscosity.
4th week: Colligative properties.
5th week: Equilibrium constant of homogeneous reaction.
6th week: Phase diagram for three-component system.
7th week: Transport numbers by Hittorf method.
8th week: Conductometry and conductometric titration.
9th week: Rate constant of inversion of sucrose by polarimetric method.

Format of instruction:

Student responsibilities

Students are required to carry out all laboratory exercises. Before each exercise, students should take the oral partial exam. After each exercise, students should submit a report on the completed exercise. This will be recorded and evaluated in making a final assessment.

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

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

Quality assurance methods that ensure the acquisition of exit competences

Quality of the teaching and learning, monitored at the level of the (1) teachers, accepting suggestions of students and colleagues, and (2) faculty, conducting surveys of students on teaching quality.

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Gain knowledge of application of principles of conservation of mass and energy to chemical process systems. To acquire a basic knowledge of the systematic problem solving related to the quantity and composition of process input and outputs.

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 is expected to know:
- explain the law of conservation of mass and write general material balance equation on (continuous) steady-state and (batch) unsteady-state processes,
- write material balances on unreactive and reactive processes,
- write a flowchart of single and multiple-unit processes and solve the system of mass balance equations in order to define amount and composition of material of each process stream,
- apply the law of conservation of energy and write energy balances for chemical processes,
- write energy balances on opened and closed steady-states systems,
- apply simultaneous material and energy balances.

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

1st week: Introductions to engineering calculations.
2nd week: Processes and process variables
3th week: General material balance equation.
4th week: Material balances on continuous steady-states processes without chemical reaction.
5th week: Material balances on batch unsteady-states processes without chemical reaction.
6th week: Material balances on process with recycle and bypass.
7th week: Material balances on multiple-unit processes.
8th week: Material balances on reactive processes.
9th week: Balances on atomic and molecular species.
10th week: Balances on combustion processes.
11th week: Energy and energy balances. Instructional objectives.
12 th week: Energy balances on closed systems at steady-states.
13th week: Energy balances on opened systems at steady-states.
14th week: Energy balances on reactive processes.
15th week: Simultaneous material and energy balances.

Format of instruction:

Student responsibilities

Students are required to attend at least 80% of lectures and seminars.

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

Luyben, W. L., Wenzel, L. A.: Chemical Process Analysis: Mass and Energy Balances, Prentice-Hall Inc., New Jersey, 1998.
T. Bradić, R. Roki, J. Pečarić, M. Strunje: Matematika za tehnološke fakultete, Sveučilište u Zagrebu, Multigraf – Zagreb, Zagreb, 1994..

Quality assurance methods that ensure the acquisition of exit competences

- monitoring of students suggestions and reactions during semester
- students evaluation organized by University

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Gaining knowledge about the principles of transfer of momentum, heat and mass transfer on the principle of a unified approach to transport phenomena. This knowledge forms the basis of chemical engineering unit operations, and they are therefore essential for a fuller understanding of process engineering.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Transport Phenomena

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

After passing the exam the student is expected to know:
- how to apply the laws of conservation of the fluid flow
- about molecular and convective mechanisms of transport of momentum, energy and mass
- how to recognize the major resistance at transport phenomena and how to intensifying the observed transfer
- how to gain insight into the functional dependence of the characteristics of a given system by the use of similarity theory and dimensional analysis
- the analogy of transfer of momentum, energy and mass

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

1st week: Introduction to physical transport phenomena. Conservation law. Molecular and convective transport mechanisms.
2nd week: Stationary and non-stationary processes. Rate of transport processes. Momentum, heat and mass fluxes. Fluid characteristics (density, relative density, specific weight...)
3rd week: Momentum transfer. Newton’s low of viscosity. Momentum flux. Application of momentum and mass balances in fluid mechanics.
4th week: Application of heat balance in fluid mechanics: Bernoulli equation and its application in process engineering.
5th week: Theories of similarity. Dimensional analysis. Flow phenomena. Laminar flow. Stationary laminar flow between two flat horizontal plates.
6th week: Stationary laminar flow through a horizontal circular tube. Hagen-Poiseuille law. Turbulent flow. Pressure drop in straight channels and in pipe systems. Moody diagram.
7th week: Flow around obstacles. Rate of sedimentation.
8th week: Flow through beds of particles. Fluidization.
9th week: Fundamental principles of heat transfer. Stationary heat conduction. Heat conduction through walls and through cylindrical walls.
10th week: Heat transfer by forced convection. Thermal boundary layer. Partial and overall heat transfer coefficients. Heat transfer during laminar and turbulent flows in pipes. Heat transfer during condensation.
11th week: Heat transfer during boiling. Heat transfer around obstacles. Heat transfer during natural convection.
12th week: Heat transport by radiation.
13th week: Fundamental principles of mass transfer. Stationary diffusion. Equimolar counterdiffusion and one-component diffusion.
14th week: Mass transfer with forced convection. Mass transfer by natural convection.
15th week: Interphase mass transfer. Analogy between heat and mass transfer.

Format of instruction:

Student responsibilities

Lecture attendance: 80 %. Laboratory exercises attendance: 100 %.

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

E. Mitrović-Kessler: Prijenos tvari i energije, Tehnološki fakultet Split, Split, 1991.

Quality assurance methods that ensure the acquisition of exit competences

- monitoring of students suggestions and reactions during semester
- students evaluation organized by University

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Gaining knowledge in application of basic measurements in process engineering, conducting measurements of fluid flow, pressure and temperature, analysis of experimental data and writing final reports, basic use of Microsoft Office Excel in data processing.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Transport Phenomena

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

After finishing the laboratory exercises, student is expected to know:
- how to determine and measure fluid flow
- how to calibrate an orifice plate and rotameter in order to use them as a flow meter in a pipeline
- how to measure a pressure drop in a pipeline and determine pipe roughness and friction coefficients
- how to conduct appropriate measurements needed to calculate particle sedimentation rate
- how fluidization is conducted and where can it be applied
- what are the major resistances in heat and transfer and know the basics in how to reduce them

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

Laboratory exercises:
Exercise 1: Determination of fluid flow type and the critical Reynolds number (1 hour)
Exercise 2: Applying the Bernoulli’s theorem: Dynamic and Surface Flow Meters - Calibration of orifice plate and rotameter (2 hours)
Exercise 3: Determination of pressure drop in the pipeline (2 hours)
Exercise 4: Determination of particle sedimentation rate in a stationary fluid (2 hours)
Exercise 5: Determination of fluidized bed characteristics (2 hours)
Exercise 6: Determination of partial and overall heat transfer coefficients (2 hours)
Exercise 7: Complex heat transfer by radiation and convection (2 hours)
Exercise 8: Interphase mass transfer. (2 hours)

Format of instruction:

Student responsibilities

Laboratory exercises attendance: 100 %.

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

E. Mitrović-Kessler: Prijenos tvari i energije, Tehnološki fakultet Split, Split, 1991.

Quality assurance methods that ensure the acquisition of exit competences

- monitoring of students suggestions and reactions during semester
- students evaluation organized by University

Other (as the proposer wishes to add)

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Students will learn the basic laws of electrolysis and electrochemical kinetics which play an important role in materials science and materials engineering, corrosion protection of materials, electroorganic and inorganic synthesis processes and also in modern and sustainable technologies.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course Exercises in Electrochemistry
The condition for taking the exam: Completed the course ”Exercises in Electrochemistry”

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

After the successfully passed exam student is able to:
- explain the difference between chemical and electrochemical reactions
- describe the components and processes in the electrochemical reactor
- identify the types of conductors and conductivity
- define the concept of electrode potential
- explain the structure of electrified phase boundary
- differentiate between the concepts of polarization and overvoltage
- explain the causes of different overvoltage types
- recognize the important electrochemical processes
- introduce electrochemical aspects of environmental protection
- apply the acquired knowledge in solving numerical problems in electrochemistry.

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

1st week: Introduction. Overview of the main problems in electrochemistry. Chemical and electrochemical reactions. Electrochemical systems. Basic concepts in electrochemistry. Types of conductivity. Electrochemical stoichiometry – Faraday law.
2nd week: Ionics. Ion-solvent interaction. Electrolyte definition. Solvent and dissolution process. Ion hydration. Ion-ion interaction. Concept of ionic atmosphere.
3rd week: Non-stationary phenomena in electrolyte solutions. Current flow through electrolyte solutions.
4th week: The modern theory of electronic conductors.
5th week: First test. Electrochemical thermodynamics. Equilibrium cell voltage. Redox reactions and electrochemical systems. Reversibility of electrochemical processes.
6th week: Electrode potentials. Absolute electrode potential. Volta potential, real potential and relative electrode potential. Electrode potential measurement. Nernst relation. Definition of standard electrode potential. Reference electrodes. Standard hydrogen potential scale.
7th week: Phase boundary. Ideally polarizable electrode and electrocapillarity. Adsorption. Nonspecific and specific adsorption. Double layer structure and models. Helmholtz model. Gouy-Chapman model. Stern model. Stern-Gram model.
8th week: Electrokinetic phenomena and zeta-potential. Electrooosmosis. Strearming potential. Electrophoresis. Dorn effect. Electrode kinetics. Electrochemical systems in non-equilibrium conditions.
9th week: Anodic and chatodic processes. Electrochemical reaction mechanism and rate determining step. Polarization and overpotential. Overvoltage types. Second test.
10th week: Electrochemical overpotential. Buttler-Volmer and Tafel equations. Diagnostic criteria.
11th week: Diffusion overpotential. Diffusion in stationary and non-stationary condition.
12th week: Reaction ovrepotential. Crystallization overpotential. Electrochemical measurement methods - stationary and non-stationary.
13th week: Analysis of mechanism selected electrode processes. Electrocatalysis - evolution and reduction of hydrogen and oxygen. Deposition and dissolution of metals. Corrosion of metals.
14th week: Nucleation and new phase formation. Passivity phenomena. Conversion and storage of energy.
15th week: Environmentally oriented electrochemistry. Third test.
Seminars (one hour weekly): Solving numerical problems in electrochemistry.

Format of instruction:

Student responsibilities