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CRETE
Undergraduate Courses
You may look for individual courses offered at the Department of Chemistry as of October
2007, by browsing through the list, where they are divided by semester.
You may also download a concise list and short description of all the courses by clicking on
the link below.
Undergraduate Courses - Semester A
Principles of Chemistry
Qualitative and Quantitative Analysis
Mathematics Ι
Physics Ι
Introduction to Computer Science
English for Chemistry Foundation Course I
Undergraduate Courses - Semester B
Introduction to Biology
Organic Chemistry Ι
Mathematics ΙΙ
Physics ΙΙ
General Chemistry Lab (starts in the middle of November)
English for Chemistry Foundation Course II
Undergraduate Courses - Semester C
Analytical Chemistry I
Physical Chemistry I
Organic Chemistry II
Physical Chemistry Lab I
Organic Chemistry Lab I
Undergraduate Courses - Semester D
Analytical Chemistry ΙΙ
Physical Chemistry ΙΙ
Inorganic Chemistry Ι
Analytical Chemistry Lab Ι
Organic Chemistry Lab ΙΙ
Undergraduate Courses - Semester E
Biochemistry Ι
Chemistry of Bio-molecules
Inorganic Chemistry ΙΙ
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Inorganic Chemistry Lab Ι
Analytical Chemistry Lab ΙΙ
Undergraduate Courses - Semester F
Biochemistry ΙΙ
Environmental Chemistry
Physical Chemistry Lab ΙΙ
Inorganic Chemistry Lab ΙΙ
Biochemistry Lab
Undergraduate Courses - Semester G
Optional Course 1
Optional Course 2
Optional Course 3
Optional Course 4
Optional Course 5
Undergraduate Courses - Semester H
Optional Course 6
Optional Course 7
Optional Course 8
Optional Course 9
Optional Course 10
CH-043 Principles of Chemistry
Chemistry and Measurments
Introduction to chemistry
Natural measurments
Atoms, Molecules and Ions
Atomic theory and atomic structure
Chemical substances: Formulas and names
Chemical reactions: Equations
The gas state
The gas laws
Kinetic-Molecular theory
Thermochemistry
Enthalpy of the reaction
Use of thermal processes
Quantum theory of atom
Electromagnetic waves, photons, Bohr theory
Quantamechanic and quantum numbers
Electronic structures and pereodicity
Electronic structure of atoms
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Pereodicity of the elements
Ionic and covalent bonds
Ionic bonds
Covalent bonds
Molecular symmetry and chemical bond theory
Valence bond theory
Molecular orbital theory
States of matter: Liquids and solids
Changes of states
Liquid state
Solid state
Nuclear chemistry
Radiofrequency energy and nuclear bombardment
Energy from nuclear reactions
Chemistry of main group metals
Main group metals
Group IA: Alkali metals
Group IIA: Alkaline Earth metals
Metals of group IIIA and IVA
Chemistry of non metals
Group IVA: The group of carbon
Group VA: The group of nitrogen and phosphorous
Group VIA: The group of oxygen and sulfur
Group VIIA: The halogens
Group VIIIA: The noble gases
Transition elements and coordination compounds
Properties of transition elements
Coordination ions and compounds
CH-044 Qualitative and Quantitative Analysis
Calculations with Chemical Formulas and Equations
The mass and moles of a substance
Chemical formula determination
Stoichiometry: quantitative relationships in chemical reactions
Chemical Reactions
Ions in aqueous solution
Types of Chemical Reactions
Concentration units and solution dilution
Quantitative analysis: volumetric and gravimetric analysis
Solutions
Preparing Solutions
Colloids and their properties
Rates of Reaction
Reaction rates
Reaction mechanisms
Chemical Equilibrium
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Chemical equilibrium
Using the equilibrium constant
Le Chatelier principle
Acids and Bases
Acid – Base theory
Acid – Base strength
Water dissociation and pH
Acid-Base Equilibria
Weak acid and base containing solutions
Acid dissociation equilibrium
Polyprotic acids
Base dissociation equilibrium
Acid-base properties of salts
Solutions of weak acids or bases in the presence of another dissolved substance
Common salt effect
Buffer solutions
Titration curves
Solubility and Complex-Ion Equilibria
Solubility equilibrium - Applications
Complex-ion equilibria
Thermodynamics and Equilibrium
First law of thermodynamics – Enthalpy
Spontaneous processes and entropy: Entropy and the 2nd law of thermodynamics
Free Energy and Equilibrium constants
Principles of Qualitative Analysis
CH-201 Organic Chemistry I
1. Structure and bonds
2. Bonds and molecular properties
3. Nature of organic compounds: alkanes and cycloalkanes
4. Conformation of alkanes and cycloalkanes
5. Overview of organic reactions
6. Alkenes: structure and reactivity
7. Alkenes: preparation and reactions
8. Alkynes
9. Stereochemistry
10. Alkyl halides
11. Reactions of alkyl halides: nucleophilic substitution and elimination
12. Structural elucidation: mass spectrometry and infrared spectroscopy
13. Conjugated dienes and ultraviolet spectroscopy
CH-047 General Chemistry Lab
1)Solutions - separations
2)Chemical equilibrium
3)Electrolytes: pH, Indicators
4)Hydrolysis of salts
5)Buffer solutions
6)Volumetric methods of analysis: acid-base titration, water hardness
7)Oxidation–reduction, electrolysis
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8)UV-VIS Spectrophotometry
9)Qualitative analysis of Group I kations - known
10)Qualitative analysis of Group I kations - unknown
11)Qualitative analysis of Group III kations - known
12)Qualitative analysis of Group III kations - unknown
13)Qualitative analysis: common anions
14)Determination of Ka with potentiometric titration
15)Gravimetric determination of nickel
16)Complexometric determination of zinc
17)Photometric determination of manganese in steel
CH-301 Analytical Chemistry I
1 Introduction to Analytical Methods.
1.1 Instreuments for Analysis
1.2 Selecting an Analytical Method
2 Experimental Error
2.1 Significant Figures and Arithmetic Operations
2.2 Significant Figures and Graphs
2.3 Types of Errors
2.4 Systematic-Random Errors
2.5 Precission and Accuracy
2.6 Absolute and Relative Uncertainty
2.7 Propagation of Uncertainty to the final result
3 Statistics
3.1 Gaussian Error Curve
3.2 Student t tests
3.3 Dealing with Bad Data
3.4 Best Linear Fit to Data
4 Fundamentals of Electrochemistry
4.1 Basic Concepts
4.2 Galvanic – Electrochemical Cells
4.3 Standard Electrode Potentials
4.4 Nernst Equation
4.5 Electrochemical Potential and Equilibrium Reactions
5 Reduction Oxidation Reactions in Analysis
5.1 The shape of a Redox Titration Curve
5.2 Redox Indicators
5.3 Practical Examples of Redox Titrations for Analysis
6 Zero Current Potentiometry
6.1 The Potentials of a Cell
6.2 Reference Electrodes
6.3 Indicator Electrodes
6.4 The pH Electrode
6.5 Ion-Selective Electrodes
6.6 CHEMFETS, ISFETS and other Solid State Systems
7 Voltammetry-Amperometry
7.1 Electrolysis
7.2 Voltage Current relationship
7.3 Electrogravimetric and Coulometric Analysis
7.4 Polarography
7.5 Cyclic Voltametry
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7.6 Practical Examples of Voltametry-Amperometry
CH-048 Physical Chemistry I
(Quantum Chemistry and Spectroscopy)
1. Review of Matrices
2. Operators and the Bracket notation
3. Principles of Quantum Mechanics
4. Solutions and applications of the Schroedinger equation
5. Group Theory and Point groups
6. Rotational and Vibrational Spectroscopy
7. Molecular Orbitals
8. Electronic Structure
9. Approximation methods
10. Electronic and Photoelectron Spectroscopy
11. Spin, ESR
12. NMR
CH-202 Organic Chemistry II
1. Structural elucidation: Nuclear magnetic resonance spectroscopy
2. Benzene and aromaticity
3. Chemistry of benzene: electrophilic aromatic substitution
4. Alcohols and thiols
5. Ethers, epoxides, and sulfides
6. Aldehydes and ketones: nucleophilic addition reactions
7. Carboxylic acids
8. Carboxylic acid derivatives and nucleophilic substitution of the acyl group
9. α-Substitution reactions of carbonyl compounds
10. Condensation reactions of carbonyl compounds
11. Orbitals in organic chemistry: pericyclic reactions
CH-311 Physical Chemistry Lab I
Lectures (Classroom)
1. Lecture Introduction to Physical Chemistry laboratory
2. Lecture How to prepare the lab report.
2. Lecture Error analysis
3. Lecture Vapor pressure of a pure liquid
4. Test Vapor pressure of a pure liquid
6. Lecture Joule Thomson effect
7. Test Joule Thomson effect
8. Lecture Heat capacity of gases
9 Test Heat capacity of gases
10. Lecture Statistical Mechanics Introduction
11. Lecture Statistical Mechanics applications
a) Maxwell Boltzmann distribution
b)Heat capacity solid metals
12. Test Statistical Mechanics
13. Lecture Optics
14. Lecture Optics Applications Polarimetry Refractometry
15. Test Optics
16. Lecture Vacuum Physics, technology and application.
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Experiments Cycle A (Physical chemistry Laboratory)
1. Determination of enthalpy vaporization of a pure liquid.
2. Determination of Joule-Thomsonʼs coefficient.
3. Determination of heat capacity of gases. Determination of the adiabatic coefficient of gases
γ.
4. Velocity of gas molecules. Maxwell Boltzmann distribution
5. Heat capacity of metals
6. Saccharose inversion kinetics.
7. Optical dispersion. Determining the refractive index of glass prisms.
8. Determination of pumping speed in molecular and viscous flow area.
CH-211 Organic Chemistry Lab I
1) Laboratory safety
2) Intermolecular interactions (melting point, boiling point)
3) Solvent choice – recrystallization.
4) Extraction
5) Fractional distillation – vacuum distillation
6) Drying agents – purification of diethyl ether
7) Solubility of organic compounds
8) Thin layer chromatography
9) Column chromatography (oxidation of anthracene to anthraquinone followed by separation
by column chromatography)
10) Separation of mixtures
11) Caffeine isolation from tea
12) Acidic and basic character of organic compounds (new)
13) Isolation and purification of caffeine, aspirin, and acetaminophene from commercial drugs
(new)
14) Isolation of nicotine from tobacco (new)
CH-408 Analytical Chemistry II
Mass Spectrometry
Introduction to mass spectrometry
Atomic ion ionization sources
Mass analyzers (quadrupoles, magnetic analyzers, time-of-flight, etc.)
Inductively Coupled Plasma Mass Spectrometry
Sample preparation
Molecular Mass Spectrometry
Ionization sources (electron ionization EI, chemical ionization CI, fast atom bombardment
FAB, matrix assisted laser desorption ionization MALDI, and electrospray)
Applications of electrospray in proteomics and environmental analysis
Atomic Absorption Spectrometry
Physicochemical processes in atomic absorption spectrometry
Types and function of atomizers
Radiation sources
Types of atomic absorption spectrometers
Interferences: Methods for background correction
Atomic Emission Spectrometry
Physicochemical processes in atomic emission spectrometry
Types and function of atomizers (emphasis on the plasma source)
Types of atomic emission spectrometers
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Separation Methods
Introduction of separation methods
Gas chromatography
High performance liquid chromatography (HPLC)
Extractions and Supercrtical Fluid Chromatography
Capillary Zone Electrophoresis
CH-049 Physical Chemistry II
(Applied Statistical Thermodynamics)
1. Laws of Thermodynamics
2. Thermo-chemistry
3. Probability and ensembles
4. Entropy
5. The Partition Function and determination Thermodynamics Potentials
6. Gas Laws and Distributions
7. Chemical Kinetics and Rate Laws
8. Arrenhius Law
9. Molecular Collisions
10. Transition State Theory
11. RRKM Theory
12. Molecular Dynamics
13. Marcus Theory
14. Heterogeneous Chemistry
CH-401 Inorganic Chemistry I
1. Introductory concepts on transition metal complexes
VSEPR Theory-Lewis structures
Acids-Bases (Bronsted-Lowry, Lux- Flood, Lewis, Usanovich)
Steric influences
Hard-Soft concepts in acid-base chemistry (with emphasis on metal complexes)
Hydrogen bonding in Inorganic Chemistry
2. Coordination chemistry
Ligand types
Coordination number
Isomerism
Chelate effect
18-electron rule
3. Covalent compounds
Symmetry groups
Lewis structures
VSEPR structures
4. Valence bond theory
Hybridization, s, p,d bonds
Molecular orbital theory
Homo- and hetero nuclear dimeric complexes
Polyatomic complexes, clusters
Εlectron-deficient molecules, p-donor and acceptor ligands
Electronegativity
Bond energy and ionic radii
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5. Orgel and Tanabe-Sugano diagrams
6. Comparative approach to Crystal Field Theory and Molecular Orbital Theory
7. Distortions from ideal geometries
Jahn-Teller effect
Distortion from Oh geometry
8. π-Bonding
Metal carbonyls
Metal-olefin complexes and other π-type ligands
Energy diagrams
Chemical reactivity of selected π-ligands
9. Electronic spectra of transition metal complexes
Term symbols
Microstates, selection rules spectroscopic terms
Russell-Saunders coupling
10. Basic principles of magnetism and application to metal complexes
Diamagnetic and paramagnetic complexes
Magnetic moment and magnetic susceptibility
11. Structures of solids, close-packed solids, metallic bond, band theory, conductivity,
semiconductors, insulators, crystal defects, synthesis of new materials through doping,
metallurgy, alloys and related materials
CH-413 Analytical Chemistry Lab I
1. Conductivity experiment
a) Determination of cell constant
b) Titrimetric determination of BaCl2 concentration
c) Determination of CaSO4 concentration
2. Potentiometric measurement of pH
a) Determination of phosphoric acids
b) Analysis of an unknown sample.
3. Determination of potassium ions in water using potassium-selective electrode.
4. Polarographic determination of lead and cadmium
5. Wine analysis (sugar content, pH, total acidity, alcohol content, free and total sulphur
dioxide)
6. Spectrophotometric determination of the pKa of a pH indicator (bromothymol blue)
7. Analysis of olive oil.
a) Determination peroxide value
b) Determination of spectrophotometric K-value
8. Spectrophotometric determination of phosphate in soft drinks
CH-212 Organic Chemistry Lab II
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1) Cannizzaro reaction
2) Esterification reaction
3) Ester hydrolysis – measurement of saponification number of fatty acids
4) Production of soap and detergents
5) Nucleophilic substitution reaction (SN2)
6) Friedel-Crafts reaction
7) Diels-Alder cycloaddition
8) Oxidation of benzylic alcohol
9) Aldol condensation
10) Aloformic reaction
11) Aromatic sulfonylation reaction
12) Grignard reaction (two experiments)
13) Enzymatic reduction: Preparation of optically active alcohol (new)
14) Preparation of chemilluminescent compounds (new)
15) Horner-Emmous-Wittig reaction (new)
CH-028 Biochemistry I
1. Introduction
2. Protein structure and function
3. DNA and RNA: Molecules of heredity
4. Myoglobin and hemoglobin
5. Introduction to enzymes
6. Mechanisms of enzyme action
7. Control of enzymatic action
8. Introduction to biological membranes
9. Metabolism: Basic concepts and design
10. Glycolysis
11. Citric acid cycle
12. Oxidative phosphorylation
13. Pentose phosphate pathway and gluconeogenesis
14. Photosynthesis
CH-050 Biomolecular Chemistry
1. Carbohydrates
2. Amino acids, peptides, proteins, and enzymes
3. Lipids, terpenes, and steroids
4. Heterocyclic compounds, and nucleic acids
5. DNA and RNA
6. Organic chemistry of metabolic processes
7. Electrolyte chemistry in vivo
8. Coordination compounds in vivo (Iron Molybdenum, Zinc, Copper, Chromium, and
Vanadium)
CH-402 Inorganic Chemistry II
Transition Elements and Coordination Compounds.
• Introduction to mechanisms, kinetics and rate laws.
• Classification of inorganic reactions: i) exchange of ligands, ii) rearrangement of the
coordination sphere, iii) redox processes and iv) reactions on the ligands themselves.
• Reactions of the central atom: Redox reactions, inner sphere and outer sphere
mechanisms.
• Ligand substitution reactions: dissociative, associative, interchange mechanisms and their
general characteristics.
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• Important factors determining the mechanisms of substitution reactions: Lability-Inertness
and Nucleophilicity.
• Ligand substitution in square-planar complexes. Rate laws and mechanisms. Factors
affecting reactivity: cis and trans effect, trans influence, leaving and entering group effect.
Stereochemistry.
• Ligand substitution reactions in octahedral (Oh) complexes: rate laws and mechanisms,
importance of CFSE (CFAE), water exchange, base hydrolysis.
• Reactions of coordinated ligands.
• Oxidative addition and reductive elimination reactions.
• Insertion reactions.
• Catalysis and transition metal complexes.
Main Group Elements.
• Structure, physical properties, acid-base character, and reactivities of their compounds.
Lewis adducts and coordination compounds; organo derivatives, simple anions, oxoacids and
their salts; periodic trends, e.g., metallic character of the elements, properties of the oxides,
halides, hydrides, coordinative saturation and unsaturation; bond strengths and energies.
CH-411 Inorganic Chemistry Lab I
Preparation of coordination complexes
Synthesis of square planar copper derivatives
Synthesis of tetrahedral and octahedral cobalt(II) complexes
FT-IR spectra of coordination derivatives
Introduction to IR spectroscopy
Recording techniques to record IR spectra
Elucidation of coordination modes by IR
Elucidation of isomer forms, coordination modes and symmetry.
Electronic spectra of coordination complexes
Recording technique for electronic spectra
Square plana and octahedral copper derivatives
Octahedral complexes with chromium(III)
Tetrahedral and octahedral cobalt(II) complexes
Magnetic properties of coordination derivatives
Basic principles of magnetochemistry
Experimental methods for magnetic susceptibility
Experimental part
Calculations-questions
Conductivity
Conductivity study of coordination complexes
CH-414 Analytical Chemistry Lab II
1. Metal determination using atomic absorption spectrometry
a) Determination of calcium in water samples
b) Determination of magnesium in water samples
2. Determination of the basic parameters of gas chromatography
a) Column efficiency, Van-Deemter plot, optimum flow rate
b) Determination of organic compounds using gas chromatography – analysis of unknowns.
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3. Determination of the basic parameters in high performance liquid chromatography (HPLC)
Study of the partition method in the reverse phase liquid chromatography, analysis of
unknown samples.
4. Quantitative determination of acetylsalicylic acid in aspirin tablets using HPLC with UV
detection
5. Quantitative analysis using gas chromatography with flame ionization detection
6. Determination of anions and cations in drinking water using ion chromatography
7. SDS electrophoresis of proteins. Determination of relative molecular mass of unknown
proteins
8. Demonstration exercise: Determining the relative molecular mass of proteins using mass
spectrometry
CH-030 Biochemistry II
1. Glycogen metabolism
2. Fatty acids metabolism
3. Amino acids catabolism and the circle of urea
4. Biosynthesis of amino acids
5. Nucleotide biosynthesis
6. Biosynthesis membrane lipids and steroids
7. Connective tissue proteins
8. Integration of metabolism
9. DNA replication recombination and repair, antibodies
10. RNA synthesis and splicing
11. Protein synthesis
12. Control of gene expression
CH-405 Environmental Chemistry
INTRODUCTION
The purpose of this course is the presentation of the chemical processes, which define the
composition of the fresh waters. The course offers basic knowledge of a) physicochemical
features and principles, which determine the chemical substances in the environment (relation
of structure and chemical activity) b) Chemical transformations (biological and non biological),
which occur in the aquatic environment, and c) chemical equilibria that determine the
biogeochemical cycles of the elements (e.g. carbon cycle). Emphasis will be given on
quantification of Chemical and Physicochemical processes in the water.
The course includes two main sections: Aquatic Chemistry of Natural Waters and Organic
Environmental Chemistry of Aquatic Systems.
The section of Aquatic Chemistry of Natural Waters includes the chemical equilibria in natural
waters and the phenomena that affect them. The Organic Environmental Chemistry of Aquatic
Systems section includes mainly the physicochemical processes which rule the
transportation, the changes and residence time of the organic substances in the aquatic
environment.
An introduction to the “design” of models, based on Aquatic Chemistry concepts, which help
us to predict the fate of chemical substances (e.g. pollutants) in aquatic environment.
The evaluation of graduate student performance is based on written examination.
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I. Aquatic Chemistry of Natural Waters
1.Introduction
2.Properties of the water
a.Quality and quantity of waters
b.Sources and uses of water and hydrological cycle
c.Properties of water
d.Characteristics of aquatic systems - aquatic life
e.Composition of natural waters (acidity, alkalinity, hardness, etc.)
3.Elements Aquatic Chemistry of Natural Waters
a.The carbon dioxide cycle in aquatic systems
b.Metals and the chemical equilibrium (precipitations, complexations)
c.Polyphosphates, humic and fulvic compounds
4.Oxidation – reduction reactions in natural waters
a.The pE of the water
b.pE/pH diagrams
5.Phase interactions in natural waters
a.Chemical and physicochemical processes between solids, gases and water
b.Formation of sediments
c.Solubility
d.Colloids
e.Aggregation of particles
f.Adsorption of chemical substances on solids - Adsorption models
g.Ion exchange
II. Organic Environmental Chemistry of Aquatic Systems
6.Introduction to Ecotoxicology
a.Introduction to aquatic microbiology and biochemistry
b.Methodological approach to the estimation of the fate of organic compounds in the aquatic
environment: Structure activity relationships
7.Definition of physicochemical parameters that determine the partition of organic compounds
in the environment
a.Coefficient of lipophilicity (Kow)
b.Solubility of organic compounds in water
c.Adsorption coefficient of organic compounds in sediments and soils
d.Bioaccumulation factor of organic compounds in living organisms
e.Henry law and exchange organic compounds between atmosphere and water
f.Molecular transformation of organic compounds in the environment
g.Structural changes through microbiological processes
h.Hydrolysis of organic compounds
i.Photochemical reactions
8.Uses of models in aquatic environmental chemistry
a.Process models
b.Integrated models
CH-312 Physical Chemistry Lab II
1. Basic techniques in Calorimetry: Determining of the enthalpy dialysis.
2. Electrochemisty
a) Determination of Faradayʼs constant.
b) Determination of electrochemical equivalent.
3. Determination of potential diffusion. Nernst equation
4.Viscometry: Determination of the activation energy of viscous
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5. Deterimnation of the Molecular weight of a polymer from intrinsic viscisity measurements
6. Atomic spectroscopy
7.Absorption spectrum of a conjugated dye
8. Laser fundamentals: Malus law with a He-Ne Laser.
9. Partial molecular volume.
10. Boiling point diagram of a binary mixture
CH-412 Inorganic Chemistry Lab II
Security rules and behavior in the laboratory
Material Safety Data and Use of the Gases
Halogens chemistry. Interhalogens and oxidations states. Preparation and study of ICl 3
Silicon polymers, synthesis of Bouncing Putty
Oxidation states for Tin: Synthesis and study of SnI4, SnI2
Constant stability for Tin (IV) and Plomb (IV), synthesis and study of (NH 4)2[SnCl6],
(NH4)2[PbCl6]
Preparation of trialkoxyborates
A) preparation of Tri-n-propylborate
B) preparation of a poly(vinylalcoohol)-borate coopolymer.
Porphyrin ring
Α) Synthesis
Β) Metallation reaction, study and characterization.
Preparation of Rhodium metallocarbonyls
CH-051 Biochemistry Lab
1. Isolation and characterization of bovine milk α-lactalbumin (4 lab periods).
-Preparation of milk whey
-Affinity chromatography
-Bradford protein assay
-SDS-PAGE of α-lactalbumin
2. Identification of α-lactalbumin by SDS-PAGE and western blotting (2 lab
periods).
-Electroblotting
-Detection of blotted proteins
3. Catechol oxidase: Action-inhibition-selectivity.
Oxidation-reduction reactions modeling biochemical systems.
4. Photoinduced proton transport through chloroplast membranes.
5. Extaction and characterization of bacterial DNA.
New Undergraduate Program of the Department of
Chemistry, 2007
First year
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– 15 –
A Semester
Principles of Chemistry
Qualitative and Quantitative Analysis
Mathematics Ι
Physics Ι
Introduction to the Computers Science
Β Semester
Introduction to Biology
Organic Chemistry Ι
Mathematics ΙΙ
Physics ΙΙ
General Chemistry Lab (starts in the
middle of November)
Second year
C Semester
Analytical Chemistry Ι
Physical Chemistry Ι
Organic Chemistry ΙΙ
Physical Chemistry Lab Ι
Organic Chemistry Lab Ι
D Semester
Analytical Chemistry ΙΙ
Physical Chemistry ΙΙ
Inorganic Chemistry Ι
Analytical Chemistry Lab Ι
Organic Chemistry Lab ΙΙ
Third year
E Semester
Biochemistry Ι
Chemistry of Bio-molecules
Inorganic Chemistry ΙΙ
Inorganic Chemistry Lab Ι
Analytical Chemistry Lab ΙΙ
F Semester
Biochemistry ΙΙ
Environmental Chemistry
Physical Chemistry Lab ΙΙ
Inorganic Chemistry Lab ΙΙ
Biochemistry Lab
Fourth year
G Semester
Choice 1
Choice 2
Choice 3
Choice 4
Choice 5
H Semester
Choice 6
Choice 7
Choice 8
Choice 9
Choice 10
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First Year
16
Principles of Chemistry [XHM-043]
Chemistry and Measurments
Introduction to chemistry
Natural measurments
Atoms, Molecules and Ions
Atomic theory and atomic structure
Chemical substances: Formulas and names
Chemical reactions: Equations
The gas state
The gas laws
Kinetic-Molecular theory
Thermochemistry
Enthalpy of the reaction
Use of thermal processes
Quantum theory of atom
Electromagnetic waves, photons, Bohr theory
Quantamechanic and quantum numbers
Electronic structures and pereodicity
Electronic structure of atoms
Pereodicity of the elements
Ionic and covalent bonds
Ionic bonds
Covalent bonds
Molecular symmetry and chemical bond theory.
Valence bond theory
Molecular orbital theory
States of matter: Liquids and solids
Changes of states
Liquid state
Solid state
Nuclear chemistry
Radiofrequency energy and nuclear bombardment
Energy from nuclear reactions
Chemistry of main group metals
Main group metals
Group IA: Alkali metals
Group IIA: Alkaline Earth metals
Metals of group IIIA and IVA
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Chemistry of non metals
Group IVA: The group of carbon
Group VA: The group of nitrogen and phosphorous
Group VIA: The group of oxygen and sulfur
Group VIIA: The halogens
Group VIIIA: The noble gases
Transition elements and coordination compounds.
Properties of transition elements
Coordination ions and compounds
Introduction to Biology [XHM-046]
1. Elements in the living organism, categories of biological macromolecules Origin of life - RNA
- catalytic RNA chemical frame of life prokaryotic, eukaryotic, and viruses
2. Cell: architecture – structure cell of prokaryotic and eukaryotic evolutionary relation of cells
3. Cell: cytoplasm, ribosome, cytoskeleton, membranes, flagella
4. Molecular biology, DNA - rules of Mendel, term of genes, genetic code, transcription and
translation
5. Biology of reproduction circle. Change of generations
6. Growth, differentiation and development of cells
7. Signals pathways, receptors
8. Physiology of cell, physiology of animals
9. Models of research - genetics, proteomics, chemical biology - transformation (vectors)
10. Microbial populations - ecosystems - environment - parasitism (generally not only in plant
cells)
11. Virology. Bacteriophages and viruses, pictures of illnesses, construction (morphology).
Organic Chemistry I [XHM-201]
1. Structure and bonds
2. Bonds and molecular properties
3. Nature of organic compounds: alkanes and cycloalkanes
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4. Conformation of alkanes and cycloalkanes
5. Overview of organic reactions
6. Alkenes: structure and reactivity
7. Alkenes: preparation and reactions
8. Alkynes
9. Stereochemistry
10. Alkyl halides
11. Reactions of alkyl halides: nucleophilic substitution and elimination
12. Structural elucidation: mass spectrometry and infrared spectroscopy
13. Conjugated dienes and ultraviolet spectroscopy
Physical Chemistry I [XHM-048]
(Quantum Chemistry and Spectroscopy)
1. Review of Matrices
2. Operators and the Bracket notation
3. Principles of Quantum Mechanics
4. Solutions and applications of the Schroedinger equation
5. Group Theory and Point groups
6. Rotational and Vibrational Spectroscopy
7. Molecular Orbitals
8. Electronic Structure
9. Approximation methods
10. Electronic and Photoelectron Spectroscopy
11. Spin, ESR
12. NMR
Physical Chemsitry IΙ [XHM-049]
(Applied Statistical Thermodynamics)
1. Laws of Thermodynamics
2. Thermo-chemistry
3. Probability and ensembles
4. Entropy
5. The Partition Function and determination Thermodynamics Potentials
6. Gas Laws and Distributions
7. Chemical Kinetics and Rate Laws
8. Arrenhius Law
9. Molecular Collisions
10. Transition State Theory
11. RRKM Theory
12. Molecular Dynamics
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13. Marcus Theory
14. Heterogeneous Chemistry
Organic Chemistry II [XHM-202]
1. Structural elucidation: Nuclear magnetic resonance spectroscopy
2. Benzene and aromaticity
3. Chemistry of benzene: electrophilic aromatic substitution
4. Alcohols and thiols
5. Ethers, epoxides, and sulfides
6. Aldehydes and ketones: nucleophilic addition reactions
7. Carboxylic acids
8. Carboxylic acid derivatives and nucleophilic substitution of the acyl group
9. α-Substitution reactions of carbonyl compounds
10. Condensation reactions of carbonyl compounds
11. Orbitals in organic chemistry: pericyclic reactions
Inorganic Chemistry Ι [XHM-401]
1. Introductory concepts on transition metal complexes
VSEPR Theory-Lewis structures
Acids-Bases (Bronsted-Lowry, Lux- Flood, Lewis, Usanovich)
Steric influences
Hard-Soft concepts in acid-base chemistry (with emphasis on metal complexes)
Hydrogen bonding in Inorganic Chemistry
2. Coordination chemistry
Ligand types
Coordination number
Isomerism
Chelate effect
18-electron rule
3. Covalent compounds
Symmetry groups
Lewis structures
VSEPR structures
4. Valence bond theory
Hybridization, s, p,d bonds
Molecular orbital theory
Homo- and hetero nuclear dimeric complexes
20
Polyatomic complexes, clusters
Εlectron-deficient molecules, p-donor and acceptor ligands
Electronegativity
Bond energy and ionic radii
5. Orgel and Tanabe-Sugano diagrams
6. Comparative approach to Crystal Field Theory and Molecular Orbital Theory
7. Distortions from ideal geometries
Jahn-Teller effect
Distortion from Oh geometry
8. π-Bonding
Metal carbonyls
Metal-olefin complexes and other π-type ligands
Energy diagrams
Chemical reactivity of selected π-ligands
9. Electronic spectra of transition metal complexes
Term symbols
Microstates, selection rules spectroscopic terms
Russell-Saunders coupling
10. Basic principles of magnetism and application to metal complexes
Diamagnetic and paramagnetic complexes
Magnetic moment and magnetic susceptibility
11. Structures of solids, close-packed solids, metallic bond, band theory, conductivity,
semiconductors, insulators, crystal defects, synthesis of new materials through doping,
metallurgy, alloys and related materials
Physical Chemistry Laboratory I [XHM-311]
Lectures (Classroom)
1. Lecture Introduction to Physical Chemistry laboratory
2. Lecture How to prepare the lab report.
2. Lecture Error analysis
3. Lecture Vapor pressure of a pure liquid
4. Test Vapor pressure of a pure liquid
6. Lecture Joule Thomson effect
7. Test Joule Thomson effect
8. Lecture Heat capacity of gases
9 Test Heat capacity of gases
10. Lecture Statistical Mechanics Introduction
11. Lecture Statistical Mechanics applications
a) Maxwell Boltzmann distribution
b)Heat capacity solid metals
12. Test Statistical Mechanics
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13. Lecture Optics
14. Lecture Optics Applications Polarimetry Refractometry
15. Test Optics
16. Lecture Vacuum Physics, technology and application.
Experiments Cycle A (Physical chemistry Laboratory)
1. Determination of enthalpy vaporization of a pure liquid.
2. Determination of Joule-Thomson’s coefficient.
3. Determination of heat capacity of gases. Determination of the adiabatic coefficient
gases γ.
4. Velocity of gas molecules. Maxwell Boltzmann distribution
5. Heat capacity of metals
6. Saccharose inversion kinetics.
7. Optical dispersion. Determining the refractive index of glass prisms.
8. Determination of pumping speed in molecular and viscous flow area.
of
Analytical Chemistry Laboratory I [XHM-413]
1. Conductivity experiment
a) Determination of cell constant
b) Titrimetric determination of BaCl2 concentration
c) Determination of CaSO4 concentration
2. Potentiometric measurement of pH
a) Determination of phosphoric acids
b) Analysis of an unknown sample.
3. Determination of potassium ions in water using potassium-selective electrode.
4. Polarographic determination of lead and cadmium
5. Wine analysis (sugar content, pH, total acidity, alcohol content, free and total sulphur dioxide)
6. Spectrophotometric determination of the pKa of a pH indicator (bromothymol blue)
7. Analysis of olive oil.
a) Determination peroxide value
b) Determination of spectrophotometric K-value
8. Spectrophotometric determination of phosphate in soft drinks
Organic chemistry laboratory I [XHM-211]
1)
Laboratory safety
2)
Intermolecular interactions (melting point, boiling point)
3)
Solvent choice – recrystallization.
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4)
Extraction
5)
Fractional distillation – vacuum distillation
6)
Drying agents – purification of diethyl ether
7)
Solubility of organic compounds
8)
Thin layer chromatography
9)
Column chromatography (oxidation of anthracene to anthraquinone followed by
separation by column chromatography)
10)
Separation of mixtures
11)
Caffeine isolation from tea
12)
Acidic and basic character of organic compounds (new)
13)
Isolation and purification of caffeine, aspirin, and acetaminophene from commercial
drugs (new)
14)
Isolation of nicotine from tobacco (new)
Organic chemistry lab ΙΙ
1)
Cannizzaro reaction
2)
Esterification reaction
3)
Ester hydrolysis – measurement of saponification number of fatty acids
4)
Production of soap and detergents
5)
Nucleophilic substitution reaction (SN2)
6)
Friedel-Crafts reaction
7)
Diels-Alder cycloaddition
8)
Oxidation of benzylic alcohol
9)
Aldol condensation
10)
Aloformic reaction
11)
Aromatic sulfonylation reaction
12)
Grignard reaction (two experiments)
13)
Enzymatic reduction: Preparation of optically active alcohol (new)
14)
Preparation of chemilluminescent compounds (new)
15)
Horner-Emmous-Wittig reaction (new)
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Biochemistry I [XHM-028]
1. Introduction
2. Protein structure and function
3. DNA and RNA: Molecules of heredity
4. Myoglobin and hemoglobin
5. Introduction to enzymes
6. Mechanisms of enzyme action
7. Control of enzymatic action
8. Introduction to biological membranes
9. Metabolism: Basic concepts and design
10. Glycolysis
11. Citric acid cycle
12. Oxidative phosphorylation
13. Pentose phosphate pathway and gluconeogenesis
14. Photosynthesis
Biochemistry II [XHM-030]
1. Glycogen metabolism
2. Fatty acids metabolism
3. Amino acids catabolism and the circle of urea
4. Biosynthesis of amino acids
5. Nucleotide biosynthesis
6. Biosynthesis membrane lipids and steroids
7. Connective tissue proteins
8. Integration of metabolism
9. DNA replication recombination and repair, antibodies
10. RNA synthesis and splicing
11. Protein synthesis
12. Control of gene expression
Chemistry of Biomolecules [XHM-50]
1. Carbohydrates
2. Amino acids, peptides, proteins, and enzymes
3. Lipids, terpenes, and steroids
4. Heterocyclic compounds, and nucleic acids
5. DNA and RNA
6. Organic chemistry of metabolic processes
7. Electrolyte chemistry in vivo
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8. Coordination compounds in vivo (Iron Molybdenum, Zinc, Copper, Chromium, and
Vanadium)
Inorganic chemistry II [XHM-402]
Transition Elements and Coordination Compounds.
 Introduction to mechanisms, kinetics and rate laws.
 Classification of inorganic reactions: i) exchange of ligands, ii) rearrangement of the
coordination sphere, iii) redox processes and iv) reactions on the ligands themselves.
 Reactions of the central atom: Redox reactions, inner sphere and outer sphere
mechanisms.
 Ligand substitution reactions: dissociative, associative, interchange mechanisms and their
general characteristics.
 Important factors determining the mechanisms of substitution reactions: LabilityInertness and Nucleophilicity.
 Ligand substitution in square-planar complexes. Rate laws and mechanisms. Factors
affecting reactivity: cis and trans effect, trans influence, leaving and entering group
effect. Stereochemistry.
 Ligand substitution reactions in octahedral (Oh) complexes: rate laws and mechanisms,
importance of CFSE (CFAE), water exchange, base hydrolysis.
 Reactions of coordinated ligands.
 Oxidative addition and reductive elimination reactions.
 Insertion reactions.
 Catalysis and transition metal complexes.
Main Group Elements.
 Structure, physical properties, acid-base character, and reactivities of their compounds.
 Lewis adducts and coordination compounds; organo derivatives, simple anions, oxoacids
and their salts; periodic trends, e.g., metallic character of the elements, properties of the
oxides, halides, hydrides, coordinative saturation and unsaturation; bond strengths and
energies.
Biochemistry Lab [XHM-051]
1. Isolation and characterization of bovine milk α-lactalbumin (4 lab periods).
-Preparation of milk whey
-Affinity chromatography
-Bradford protein assay
-SDS-PAGE of α-lactalbumin
2. Identification of α-lactalbumin by SDS-PAGE and western blotting (2 lab
periods).
-Electroblotting
-Detection of blotted proteins
3. Catechol oxidase: Action-inhibition-selectivity.
Oxidation-reduction reactions modeling biochemical systems.
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4. Photoinduced proton transport through chloroplast membranes.
5. Extaction and characterization of bacterial DNA.
Physical Chemistry Laboratory II [XHM-312]
1. Basic techniques in Calorimetry: Determining of the enthalpy dialysis.
2. Electrochemisty
a) Determination of Faraday’s constant.
b) Determination of electrochemical equivalent.
3. Determination of potential diffusion. Nernst equation
4.Viscometry: Determination of the activation energy of viscous
5. Deterimnation of the Molecular weight of a polymer from intrinsic viscisity measurements
6. Atomic spectroscopy
7.Absorption spectrum of a conjugated dye
8. Laser fundamentals: Malus law with a He-Ne Laser.
9. Partial molecular volume.
10. Boiling point diagram of a binary mixture
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Analytical Chemistry Laboratory II [XHM-414]
1. Metal determination using atomic absorption spectrometry
a) Determination of calcium in water samples
b) Determination of magnesium in water samples
2. Determination of the basic parameters of gas chromatography
a) Column efficiency, Van-Deemter plot, optimum flow rate
b) Determination of organic compounds using gas chromatography – analysis of
unknowns.
3. Determination of the basic parameters in high performance liquid chromatography (HPLC)
Study of the partition method in the reverse phase liquid chromatography, analysis of unknown
samples.
4. Quantitative determination of acetylsalicylic acid in aspirin tablets using HPLC with UV
detection
5. Quantitative analysis using gas chromatography with flame ionization detection
6. Determination of anions and cations in drinking water using ion chromatography
7. SDS electrophoresis of proteins. Determination of relative molecular mass of unknown
proteins
8. Demonstration exercise: Determining the relative molecular mass of proteins using mass
spectrometry
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