- •Introduction
- •Chapter # 1. The foundations of atomic-molecular studies. The laws and concepts of stoichiometry
- •Vocabulary
- •Subject and Tasks of Chemistry
- •General notions of atomic-molecular studies
- •Number of atoms of an element
- •Example of solution
- •Amount of substance. Mole. Avogadro’s Number. Molar mass
- •Number of moles of an element
- •Mass of an element (grams)
- •X Molar mass of element (Mm)
- •4. The laws and concepts of Stoichiometry
- •5. Types of chemical reactions
- •Chapter # 2. Atomic structure
- •Vocabulary
- •General notions
- •Theories of atomic structure
- •Figure 3. Spatial orientation of p-orbitals
- •3. Principles for distribution of electrons in atoms Distributions of electrons in atoms on energy levels and sub-levels may be presented in the form of electronic formulas.
- •Ground state
- •4. Valency and Oxidation number as function of electrons distribution
- •Practice problems
- •Chapter # 3. The periodic law and periodic table of chemical elements
- •Vocabulary
- •1. Formulation
- •2. Physical meaning of the chemical periodicity
- •3. The Periodic Table
- •Periodical table of chemical elements named by d.I. Mendeleev
- •Practice problems
- •Chapter # 4. Chemical bonding
- •Vocabulary
- •Types of Chemical Bonds
- •Ionic bond
- •Nonpolar-covalent bond
- •P olar-covalent bond
- •Figure 10. Formation of Hydrogen Bonds between water molecules
- •Figure 11. Depending of boiling-points (b.Pt) of double Hydrogen-contained compounds from nature of the second atom and presence of Hydrogen bonding
- •Why does Chemical Bond occur?
- •Practice problems
- •Сhapter # 5. Laboratory glassware, labware and rules of laboratory research
- •Vocabulary
- •Chemical glassware
- •2. Chemical reagents and their storage
- •3. Elementary operations carrying out
- •4. Safety rules during carrying out laboratory works
- •5. Rules for reagents and equipment use
- •6. Rules for work carrying out and results design
- •Chapter # 6. The main classes of inorganic compounds
- •Vocabulary
- •Classification of inorganic substances
- •Inorganic substances
- •Compounds
- •2. Relation between main classes of inorganic substances
- •3. Oxides
- •Preparation
- •Chemical properties
- •4. Bases
- •Preparation
- •Chemical properties
- •5. Acids
- •Preparation
- •Chemical properties
- •6. Amphoteric hydroxides
- •Preparation
- •7. Salts
- •Preparation
- •Chemical properties
- •Chemical properties
- •6. Thermal decomposition with medium salts formation:
- •Structural-graphic formulas of chemical compounds
- •Example of solution
- •Chapter # 7. Theory of electrolytic dissociation
- •Vocabulary
- •Solutions
- •Concentration of solutions
- •Molarity (molar concentration)
- •Theory of dissociation
- •Degree of dissociation
- •Main classes of inorganic substances from viewpoint of theory of electrolytic dissociation
- •6. Ionic equations
- •Laboratory training
- •Chapter # 8. Ionic product of water. Hydrolysis of salts
- •Vocabulary
- •Ionic product of water. Notion of pH
- •General notion of Hydrolysis
- •Different types of Hydrolysis
- •Laboratory training Experiment 1. Identification of reaction medium in solutions of salts
- •Experiment 2. Influence of temperature to hydrolysis
- •Chapter # 9. Oxidation-reduction reactions
- •Vocabulary
- •1. Oxidation of Elements
- •2. Oxidation-Reduction Reactions
- •3. Compiling Equations of Oxidation-Reduction Reactions
- •4. Most Important Oxidizing and Reducing Agents
- •Types of Redox Reactions
- •Influence of Medium to Redox Reactions
- •Electromotive Series of Metals
- •Vocabulary
- •1. General characteristics
- •Laboratory training Experiment 1. Reducing properties of metal ions of lower oxidation number
- •Chapter # 10. Complex (coordination) compounds
- •2. Nomenclature
- •3. Rules for naming of coordination compounds
- •Laboratory training
- •Chapter # 11. The halogens
- •Vocabulary
- •1. General characteristics
- •2. Chlorine
- •Laboratory training
- •Experiment 2. Halogens oxidative activity in free state
- •Experiment 5. The salts of hydrohalogen acids insoluble in water
- •Chapter # 12. The chalcogens
- •Vocabulary
- •1. General characteristics
- •Industrial Information
- •2. Oxygen
- •3. Sulfur
- •Experiment 6. Dilution of concentrated Sulfuric acid
- •Experiment 9. Instability of thiosulfuric acid
- •Chapter # 13. Nitrogen, phosphorus
- •Vocabulary
- •1. General characteristics
- •Industrial Information
- •2. Nitrogen
- •3. Phosphorus
- •Phosphorus behaves as the typical non-metal. It reacts with Oxygen, formed acid oxides:
- •Experiment 2. Oxidation and reducing power of nitrous acid and Nitrites
- •Chapter # 14. Chemistry of main biometals
- •Vocabulary
- •1. The Alkali Metals
- •Industrial Information
- •2. Other bioactive metals
Laboratory training Experiment 1. Identification of reaction medium in solutions of salts
Draw the reactions of hydrolysis for salt solutions of Na2CO3, (NH4)2SO4, ZnSO4, Cu(NO3)2, Al2(SO4)3, Na3PO4 and theoretically provide for pH of these salt solutions. Then identify reaction medium by putting the drop of solution on universal litmus paper. Draw molecular and ionic equations of hydrolysis in form of the next table:
Formula of salt |
Color of indicator |
Medium |
Reaction of hydrolysis process |
|
|
|
|
Experiment 2. Influence of temperature to hydrolysis
A) Fill each of two test tubes with 5-6 drops of 2N CH3COONa solution and one drop of phenolphthalein solution. Leave one test-tube for comparison and heat another on water bath and note color change. Draw molecular and ionic hydrolysis equations.
B) Fill test-tube with 5-6 drops of FeCl3 and 4-5 drops of CH3COONa. Note solution color change as the result Iron (III) Acetate production. Add 10 - 20 mL of distilled water and heat the mixture on water bath up to brown precipitation formation. Draw molecular and ionic equations of hydrolysis (1st and 2d steps).
Experiment 3. Hydrolysis strengthening in case of solution dilution
Put 4-5 drops of Bithmus (III) Chloride BiCl3 and by drops (15-20 drops) distilled water up to basic salt precipitation formation. Save the solution with precipitation for the next experiment. Draw hydrolysis equation taking into account that Bi(OH)2Cl is produced as the result of hydrolysis.
Experiment 4. Reversibility of hydrolysis process
Add by drops hydrochloric acid solution up to precipitation produced in previous experiment. Than add distilled water up to basic salt precipitation production. Explain the phenomenon, which occurs. Draw molecular and ionic equations.
Chapter # 9. Oxidation-reduction reactions
Vocabulary
English |
Українська назва |
English |
Українська назва |
Oxidation number (or oxidation state) |
Ступінь окислення |
Reducing agent |
Відновник |
Oxidation-reduction (redox) reactions |
Окисно-відновні реакції |
Intermolecular redox reactions |
Міжмолекулярні окисно-відновні реакції |
Reduction process |
Процес відновлення |
Intramolecular redox reactions |
Внутрішньо-молекулярні окисно-відновні реакції |
Oxidation process |
Процес окислення |
Disproporti-nation redox reactions |
Реакції самоокислення-самовідновлення (ди-спропорціонування) |
Oxidizing agent, oxidizing compound, oxidant, oxidizer |
Окисник |
Sourses:
1. Introduction in General, Organic and Biochemistry, 7th Edition, by Morris Hein, Leo R. Best, Scott Pattison and Susan Arena, Brooks/Cole Publishing Co., 2001. (Chapter 20, pp. 597-622);
2. http://antoine.frostburg.edu/chem/senese/101/redox/fag/half-reaction/
3. http://www.scince.ubc.ca/~chem/tutorials/pH/section0/index.html
http://naio.kcc.hawaii.edu/chemistry/basic_model.html
http://naio.kcc.hawaii.edu/chemistry/combination_rxn.html
http://www.shodor.org/UNChem/advanced/redox/index.html
http://www.chemtutor.com.redox.htm
http://antoine.frostburg.edu/chem/senese/101/redox/fag/how-Iron-rust/
http://www.netcomuk.co.uk/~rpeters1/auflell.htm