“chemical engineering”

Crystallography

ĶST 305

Professor Uldis Sedmalis

Course description: 2Credit units; 32 hours (32 hours)

Control forms: Exam rakstveidā
Course content:

• 
  Conception about crystalline state of substance. Other aggregative states of substance.
  
• 
  Space lattice. Elements of space lattice. Crystall structure after principle of space lattice and its experimental evidence.
  
• 
  Crystalls and their main properties as result of composition. Anisotropy of crystalls, homogeneity, ability to form polyhedrons. Prevalence of crystalls.
  
• 
  Conception of symmetry. Symmetrical operations (transformations): rotation, reflection, inversion.
  
• 
  Symmetry of crystall polyhedrons. Symmetry axis. Symmetry plate. Centre of symmetry or inversion. Inversion axis.
  
• 
  Increasing theoremes of the main symmetry elements.
  
• 
  Conception of symmetrically-equal and the only direction.
  
• 
  Classes of crystall symmetry, their obtaining.
  
• 
  Names and designation of crystall classes.
  
• 
  Division of crystalls in categories and crystall systems.
  
• 
  Common forms and combinations.
  
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  Rationality law of parametres. Their choice depending on crystall system.
  
• 
  Face of unit, parametres, indexes and symbols of faces.
  
• 
  Bravais lattices.
  
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  Translation, axis of garlands and sliding plate of reflection. 230 spatial groups of symmetry.
  
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  Crystall as X-ray diffraction lattice.
  
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  Equation of Wolf-Breg.
  
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  Physical properties of crystalls.
  
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  Cubic and hexagonal arrangement of close-packing beads.
  
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  Radious of atoms and ions. Coordination number of atom. Isomorphism, polymorphism. Morphotrophy.
  

Literature:

1. 
   Popov G., Safranskij I. Crystallography. Moscow, Nauka, 1972, 365. (in rus.)
   
2. 
   Bokij G. Crystall chemistry. Moscow, Nauka, 1971, 400. (in rus.)
   
3. 
   Terms of Mineralogy and Crystallography. Riga, Zinatne, 1993, 226.
   

Chemistry informatics

ĶTF 302

Associētā Professor Māra Jure

Course description: 2Credit units; 32 hours (16 lectures, 16 laboratories)

Control forms: Course work, Test
Course content:

• 
  Classification of information sources. Chemistry handbooks (Beilstein “Handbuch der organischen Chemie”, Theilheimer, Houben-Weyl, etc.). Refrence literature: “Khimiya”, “Chemical Abstracts”, “Science Citation Index”. Patents. STN International data bases (Online and CD-ROM versions). Information retrieval (printed and electronic sources) - search, systematization, writing of paper.
  
• 
  Writing of paper by Microsoft Word, ISIS Draw (or other chemistry software) and Microsoft Excel software. General princips - text and drawing tools, search of text, moving, copying, formatting. Tables - creation, marking, insertion, copying, moving, formatting. Formation of large documents - styles, forms, page breaking, sections, columns, comments, headings, footnotes, page numbering, auto insertion of headings, page layout, content table. Special tools - autotext, revision, annotations, autocorrection, autoformatting. Graphics, diagrams, formulas - importation of pictures and objects, their modification, textboxes.
  
• 
  INTERNET resources for chemists.
  

Literature:

1. 
   Maizell, R.E. How to Find Chemical Information, 3rd ed. John Wiley & Sons, Inc.: New York, 1998, 515 p.
   
2. 
   Ïîòàïîâ, Â.Ì.; Êî÷åòîâà, Ý.Ê. Õèìè÷åñêàÿ èíôîðìàöèÿ. ×òî, ãäå è êàê èñêàòü õèìèêó â ëèòåðàòóðå. Ìîñêâà, “Õèìèÿ”, 1979, ñ. 304.
   
3. 
   Šlihta, G.; Šlihta, V. Pamati darbam ar personālo datoru. Apgāds “Mācību grāmata”, 1994, 160 lpp.
   
4. 
   Palīgs kursu dalībniekiem. Microsoft Word 6.0 ar lappusi Word 7.0 for Windows 95. 5.papildinātais izdevums. Rīga, RTU, 1995.
   
5. 
   Judrups, J.; Sermone, L.; Strode, M.; Tenis, U. Internet iespējas PC tipa datoru lietotājiem. Rīga, LU, 1996, 100 lpp.
   
6. 
   Murāne, I. Ar Internet uz tu. “Datortehnika”, 1996, 47 lpp.
   

Chemistry Experimental Data Analysis

ĶTF 303

Assistant Prof. Ilo Dreijers

Course description: 2Credit units; 32 hours (16 lectures, 16 laboratories)

Control forms: Test
Course description:

• 
  This course is based on interactive electronic text book /1/ lessons 1-9.
  
• 
  Data errors and uncertainty – precision, accuracy, repeatability, reproducibility.
  
• 
  Histograms, distribution of data and associated parameters.
  
• 
  Sample statistics. Correlation.
  
• 
  Regression analysis. Curve fitting. Multivariate data.
  

Literature:

1. 
   TeachMe Data Analysis.
   
2. 
   I.Dreijers. Eksperimentālās optimizācijas metodes. Mācību palīglīdzeklis.-RPI, 1978. 66 lpp.
   
3. 
   Dreijers, P. Vītols. Ķīmijas tehnoloģijas procesu teorijas pamati. - Rīga.: Zvaigzne, 1986.- 228 lpp.
   
4. 
   G.E.P.Box, W.G. Hunter, JS. Hunter, Statistics for Experimenters, John Wiley & Sons, 1978. -653 pg.
   

General Chemistry, part 1

ĶVĶ 112.1

Professor Valdis Kampars

Course description: 5Credit units; 80 hours (48 lectures, 32 laboratories)

Control forms: Exam
Course content:

• 
  Fundamental Ideas of Chemistry ;Matter and Energy. Classification of Matter. Substances, Compounds, Elements, Atoms and Mixtures. Measurements in Chemistry. Units of Measurement. Chemical stoichiometry. The mole. Molecular mass. Molecular volume. The gaseous state of matter. The ideal gas low. Gas stoichiometry. Molecular weight of a gas.
  
• 
  Compound. Empirical , molecular and structural formula: Percent composition of compounds. Determining the formula of a compound.
  
• 
  Fundamental Chemical Laws: Law of conservation of mass. Law of definite proportion. Law of multiple proportions.
  
• 
  Chemical reactions. Reaction stoichiometry: Chemical Equations. Stoichiometric calculations based on chemical equations. calculations involving a limiting reagent. Yields from chemical reactions.
  
• 
  The development ideas about nature of atoms: Dalton’s atomic theory. Cathode ray. Electrons. Thomson’s models of atom. Radioactivity. The nuclear atom. Electromagnetic radiation. Dual nature of light. The continuous spectrum. The atomic spectrum. The Bohr model. The Heisenberg uncertainty principle.
  
• 
  The modern view of atomic Structure: The Quantum Mechanical Picture of the Atom. Electron density map. Quantum numbers. Principal quantum number. Azimuthal quantum number. Magnetic quantum number. The spin. Orbital shapes and energies. The Pauli principle. Polyelectronic atoms. The electronic structures of atoms. The orbital diagram. The Hund’s rule. The valence electrons.
  
• 
  Periodicity. Periodic law: The periodic table. The groups. The periods. The metals, nonmetals, metlloids. Periodic trends in atomic properties. Atomic radius. Ionization energy. Electron affinity. Electronegativity. Information contained in periodical table.
  
• 
  Chemical bonds: Bonding – general concepts. Types of chemical bonds. Valence bond theory. Bond polarity. Dipole moments. Covalent bonding. Hybridization and localized electron model. sp³ ,sp² , sp hybridization.
  
• 
  The molecular orbital model: σ- and π- bonding molecular orbital and antibonding molecular orbital. Bond order. Bonding in homonuclear and heteronuclear diatomic molecules. The delocalized π- bonding.
  
• 
  Ionic bond: Binary ionic compounds.
  
• 
  Intermolecular forces: Dipole-dipole forces. Hydrogen bonding. London dispersion forces.
  
• 
  An introduction to structures and types of solids: Crystalline and amorphous solids. The lattice. The unit cell. Types of crystalline solids. Ionic, molecular and atomic solids. Structure and Bonding in Crystalline Solids.
  
• 
  Chemical Thermodynamics: The nature of energy. Chemical energy. Energy changes that accompany chemical changes. The thermodynamic state of a system. State functions. The internal energy. Changes in internal energy. The enthalpy change. Thermochemical equations. Standard molar enthalpies of formation. Law of heat summation (Hess’ law). Spontaneity. Entropy. Second law of thermodynamics. Entropy change. Free energy change. A criterion for spontaneity. Free energy and chemical equilibrium.
  
• 
  Chemical kinetics: Rates of a chemical reactions. Factors affecting reaction rates. Nature of reactants. The effect of concentration on reaction rate. The rate law. The rate constant. Determining reaction orders. The integrated rate equation. Reaction mechanisms. Collision theory and transition theory. The activation energy. The activated complex. Temperature affecting reaction rates. Catalysts.
  
• 
  Chemical equilibrium: The equilibrium condition. The equilibrium constant. Heterogeneous equilibrium. Factors that affect equilibrium. Le Chatelier’s principle. The effect of change in concentration. The effect of change in pressure. The effect of change in temperature.
  
• 
  Properties of solutions: Various types of solutions. Colloids. The dissolving process. Solution composition. Colligative properties of solutions. Osmotic pressure. Lowering of vapour pressure and Raoult’s law. Boiling point elevation. Freezing point depression. Colligative properties of electrolyte solutions.
  
• 
  Acids and bases: The nature of acids and bases. Water as an acid and base. The ion-product constant. The pH scale. Acid-base indicators. Equilibrium of dissociation strong acid or base and weak acid or base. Acid (base) dissociation constant. Calculation the pH of strong or weak acid solutions. Acid-base properties of salts. Solutions of acids or base containing a common ion. Buffered solutions. Solubility equilibrium and the solubility product. Precipitation. The Lewis Theory.
  
• 
  Oxidation-Reduction: The Characteristics of oxidation-reduction reactions. Oxidation states. Oxidation. Reduction. Oxidizing agent. Reducing agent. Balancing Oxidation-Reduction equations. The oxidation state method. The half-reaction method. Oxidation-Reduction potential.
  
• 
  Metals: General classification. General process of obtaining a metal from its ore. Structure and bonding in metals. General properties of metals. Chemical reactions of metals with water, acids, bases, water solutions of salts. Metal alloys.
  
• 
  Coordination compounds: Terms in coordination chemistry. Coordination number. Ligands. Bonding in Coordination compounds. Nomenclature. Chemical properties of coordination compounds.
  
• 
  Electrochemistry. Galvanic cells: Electrodes. Electrode potentials. The construction of simple galvanic cells. The standard hydrogen electrode. Standard electrode potentials. Dependence of cell potential on concentration. The Nernst equation.
  
• 
  Electrolysis: Electrolytic cell. The electrolysis of molten salts. The electrolysis of water solutions. Cathode reaction. Anode reaction. Faraday’s law of electrolysis. Commercial electrolytic processes. Electrolytic refining and electroplating of metals.
  
• 
  Primary and secondary voltaic cells. Batteries: The dry cell. The lead storage battery.
  
• 
  Corrosion of metals: The electrochemical nature of corrosion. Anodic regins. Chodic regions. Corrosion of iron.
  
• 
  Prevention of corrosion: Methods for protection of metals against corrosion. Application of a coating. Paint and metal plating. Cathodic protection. Anodic protection.
  

General Chemistry (Introductory Chemistry), part 2

ĶVĶ112.2.