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Distribution of elements in nature and their significance for chemical technology.
Hydrogen. A structure of atom, oxidation state, peculiarities of position in the periodic table. Isotopes. Industrial and laboratory methods of hydrogen obtaining. Physical and chemical properties. An atomic hydrogen, its properties. Types of hydrogen compounds with metals and nonmetals.
Oxygen. A structure of atom, oxidation state. Occurrence of oxygen in nature, methods of obtaining. A structure of molecule, physical and chemical properties of oxygen. Oxygen as an oxidising agent. Ozone, its obtaining, structure of molecule and properties.
Types of elements compounds with oxygen: oxides, peroxides, superperoxides, ozonides. Classes of inorganic compounds.
Water. A structure of molecule, physical and chemical properties. Water as a solvent. Crystallohydrates. Reactions of hydration and hydrolysis. Hydrogen peroxide. A structure of molecule. Acid-base, oxidising and reducing properties of hydrogen peroxide.
Questions and tasks
1. What are the methods of hydrogen obtaining in industry and in laboratory? Write down the equations of the relevant reactions.
2. Indicate the peculiarities of hydrogen position in the periodic table. How can it be explained by the structure of hydrogen atom?
3. What oxidation states are characteristic for hydrogen compounds? Give the relevant examples.
4. Indicate reactions that prove oxidising and reducing properties of free hydrogen.
5. What compounds react with hydrogen? What oxide of metals can it reduce?
6. Explain, whether H+ ion can exist?
7. Formulate the base principles, which testify advancement of use of hydrogen as fuel for jet engine.
8. How is oxygen obtained in industry and laboratories? Write down the equations of the reactions and indicate the conditions of their proceeding.
9.What is an electronic configuration of oxygen atom? How are paramagnetic properties of a molecule О2 explained by means of the molecular orbital method? Do ions O 
, O 
, O 
exist? What ion is the most stable and why?
10. Give the description of reactivity of oxygen in relation to the simple substances and the chemical compounds. Indicate elements that don’t react with oxygen directly?
11. What structure has a molecule of ozone? Why is ozone a stronger oxidising agent, than oxygen? Confirm this with the help of the relevant reactions.
12. What are peculiarities of oxidation-reduction reactions with ozone? What substance is an obligatory product of all such reactions? Give examples.
13. Indicate similarity and difference in structure and properties of water and hydrogen peroxide.
14. Describe oxidation-reduction (redox) properties of hydrogen peroxide. Give examples of the relevant reactions.
Make up the equations of the reactions:
С + N2О =
СN4 + N2О =
Fe + HCl =
H2 + O2 =
H2 + CuO =
NaH + H2O =
O3 + KI + H2SO4 =
BaO2 + H2SO4 =
H2O2 + Ba(OH)2 =
H2O2 + KI + H2SO4 =
H2O2 + PbS =
H2O2 + KMnO4 + H2SO4 =
H2O2 + O3 =
KClO3 
KMnO4
O3 + KI + H2SO4 =
BaO2 + H2SO4 =
H2O2 + Ba(OH)2 =
H2O2 + KI + H2SO4 =
H2O2 + PbS =
H2O2 + KMnO4 + H2SO4 =
H2O2 + O3 =
KClO3
KMnO4
Experimental section
Materials and equipment: sulfur, metallic aluminium and zinc, copper (II) and manganese (ІV) oxides, crystalline potassium permanganate, potassium chlorate, solutions of neutral litmus, hydrochloric acid, sulfuric acid, hydrogen peroxide, sodium hydroxide, potassium iodide, potassium permanganate, Kipp gas generator, 100 mls beakers, test tubes, glass rods.
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