7.50. The most important compounds of iron

Lecture

Iron(II, III) oxides and hydroxides

Iron oxide and hydroxide in the oxidation state +2 have basic properties — they react with acids:

$7.50. The most important compounds of iron$

On the other hand, iron(II) compounds take part in redox reactions, generally displaying reducing properties. Fe(II) compounds can be preserved without oxidation only in an inert medium. In air under the action of oxygen, or in aqueous solution under the action of oxidizing agents such as O2, H2O2, iron in iron(II) hydroxide is oxidized to the +3 oxidation state. In doing so, the color of the iron(II) hydroxide suspension changes from white with a grayish-green tint to brown (Fig. 118, a, b, Appendix 3):

7.50. The most important compounds of iron — Fig. 118. Iron compounds

$7.50. The most important compounds of iron$

At the same time, iron in the oxide FeO (Fig. 118, c) is reduced in reactions with hydrogen, carbon, carbon monoxide, and more active metals:

$7.50. The most important compounds of iron$ .

Iron(II) hydroxide is obtained by the action of an alkali solution on salts, for example:

$7.50. The most important compounds of iron$ ,

while the oxide can be obtained by decomposition of the hydroxide:

$7.50. The most important compounds of iron$ .

Iron(II, III) oxide Fe3O4 — magnetite — is a crystalline substance in which iron is present in two oxidation states, +2 and +3, or $7.50. The most important compounds of iron$ , and it has magnetic properties.

When it reacts with acids, two salts are formed:

$7.50. The most important compounds of iron$ .

Iron(III) oxide and hydroxide. Iron oxide and hydroxide in the +3 oxidation state are insoluble in water and display weakly pronounced amphoteric properties (Fig. 118, b, d). They readily react with acids and acidic oxides, displaying basic properties:

$7.50. The most important compounds of iron$ ,

while with alkalis and basic oxides they react only upon fusion, forming ferrites:

$7.50. The most important compounds of iron$

Iron(III) hydroxide is obtained from salt solutions by precipitation with an alkali solution:

$7.50. The most important compounds of iron$ .

Fe2O3 is formed by the thermal decomposition of Fe(OH)3:

$7.50. The most important compounds of iron$

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Lectures and tutorial on "Неорганическая химия"

Terms: Неорганическая химия

Chapter I. Introduction to Inorganic Chemistry

1.1. Chemistry. Substance, chemical element, atom

1.2. Simple and complex substances. Substances of molecular and non-molecular structure

1.3. Main classes of inorganic compounds

1.3.1. Oxides

1.3.2. Acids: Classification, Chemical Properties, Nomenclature, Methods of Obtaining Acids

1.3.3. Bases

1.3.4. Salts

1.3.5. Relationships Between Classes of Inorganic Compounds

1.4. Quantitative Characteristics of a Substance

1.5. Basic Laws of Chemistry. The Law of Constant Composition of Matter. The Law of Conservation of Mass of Substances

1.6. Avogadro's Law as One of the Fundamental Laws of Chemistry

1.6.1. Molar concentration of a gas

Chapter II. ATOMIC STRUCTURE AND THE PERIODIC LAW 2.7. Atomic Structure

2.8. The Phenomenon of Radioactivity

2.9. The State of the Electron in the Atom

2.10. The Periodic Law in the Context of Atomic Structure Theory

2.11. Periodicity of changes in the properties of the atoms of chemical elements and of the substances they form

2.12. The significance of D. I. Mendeleev's periodic law and periodic table for the development of science

Chapter III. CHEMICAL BONDING AND THE STRUCTURE OF MATTER 3.13. The nature and types of chemical bonding

3.14. Properties of chemical bonds

14.1. Hybridization of atomic orbitals

Laboratory Experiment 1. Building Models of Molecules of Inorganic and Organic Compounds

3.15. Valence and Oxidation State

3.16. Types of Crystal Structures

3.17. Intermolecular Interaction and Hydrogen Bonding

Chapter IV. CHEMICAL REACTIONS 4.18. Classification and general characteristics of chemical reactions

4.18.1. Oxidation-Reduction Reactions. The Most Important Oxidizing Agents and Reducing Agents.

4.19. Thermal Effects of Chemical Reactions

4.20. The Rate of Chemical Reactions

4.21. Factors Affecting the Rate of Chemical Reactions

Laboratory Experiment 2. Investigating the Effect of Temperature and Acid Concentration on the Rate of Reaction Between Zinc and Hydrochloric Acid

4.21.1. The law of mass action

4.22. Chemical Equilibrium

Practical work 1. Chemical reactions: the ratio of the number and composition of starting substances and reaction products, the oxidation state of atoms, the release or absorption of heat, catalysts, and phase boundaries

Chapter V. CHEMISTRY OF SOLUTIONS 5.23. Dissolution as a Physicochemical Process

5.24. Preparation of Solutions

5.25. Electrolytic dissociation of substances in solutions

5.26. The Concept of the Hydrogen Index (pH) of a Solution. Acidity, Alkalinity

Laboratory Experiment 3. Determining the acidic or basic character of a solution using indicators

5.27. Chemical Properties of Acids, Bases, and Salts in Light of the Theory of Electrolytic Dissociation

Laboratory Experiment 3.1*. Ion Exchange Reactions

5.27.1. Hydrolysis of Salts

Laboratory Experiment 3.2*. Hydrolysis of salts (determining the pH of salt solutions)

Practical Work 2. Studying the Properties of Acids, Bases, and Salts in Light of the Theory of Electrolytic Dissociation

Practical Work 2.1*. Solving experimental problems on the topic "Solution Chemistry"

Chapter VI. NONMETALS. 6.28. General Characteristics of Nonmetals

6.29. Hydrogen as a chemical element

Laboratory Experiment 4. Testing solutions of hydrogen compounds of nonmetals with an indicator

6.29.1. Hydrogen Compounds of Nonmetals and Metals

6.29.2. Hydrogen Peroxide

6.30. Halogens as Chemical Elements

6.31. Compounds of the Halogens

6.32. Group VIA Elements. Oxygen and Sulfur

6.32.1. Ozone

6.33. Hydrogen Compounds of Oxygen and Sulfur

6.34. Oxygen compounds of sulfur

6.35. Sulfuric Acid

Laboratory Experiment 5. Investigating the Chemical Properties of a Dilute Sulfuric Acid Solution

6.36. Group VA Elements. Nitrogen and Phosphorus

6.37. Ammonia: Structure, Physical Properties, Preparation and Uses

Laboratory Experiment 6. Detecting ammonium ions in solution

6.37.1. Nitrogen Oxides NO and NO2

6.38. Nitric acid

6.39. Oxygen-Containing Compounds of Phosphorus

Laboratory Experiment 6.1*. Detecting phosphate ions in solution

6.40. The Most Important Mineral Fertilizers

6.41. Group IVA Elements. Carbon and Silicon

6.42. Carbonic and Silicic Acids, Their Salts

Practical Work 3. Solving Experimental Problems on the Topic "Non-Metals"

Practical work 3.1. Identification of mineral fertilizers

Chapter VII. METALS 7.43. Metals. General Characteristics

7.44. General chemical properties of metals

Laboratory Experiment 7. Reaction of Metals with Acid Solutions

7.45. General methods of obtaining metals

45.1. Obtaining Metals by Electrolysis of Aqueous Salt Solutions

7.46. Alkali Metals

7.47. Group IIA metals of the periodic system

Laboratory Experiment 8. Detection of Calcium Ions in Solution

Aluminum and Its Compounds

Laboratory Experiment 9. Amphoteric Properties of Aluminum Hydroxide

7.48.1. General Characteristics of Group B Metals

7.48.2. General Characteristics of the Acid-Base Properties of Oxides and Hydroxides of Group B Metals

49. Iron and Its Compounds

7.50. The most important compounds of iron

7.50.1. Chromium Compounds in Various Oxidation States

7.50.2. Compounds of Manganese in Various Oxidation States

7.50.3. Applications and Biological Role of Group B Metals and Their Compounds

Laboratory experiment 9.1*. Detection of iron(II) and iron(III) ions in solutions

Practical work 4. Solving experimental problems on the topic "Metals"

Practical work 4.1*. Solving experimental problems on the topic "Metals"

Chapter VIII. Chemical Substances in Human Life and Activity. 8.51. The Role of Chemistry in the Development of Civilization

8.51.1. Chemistry and agriculture

8.51.2 Medicinal Chemistry

8.51.2 Food Chemistry. Food Preparation Techniques, Food Industry

8.52. The Chemical Industry and Chemical Synthesis in the Service of Human Development

53. Ecology. Protecting the Environment from the Harmful Effects of Chemical Substances. "Green Chemistry"

Practical Work 7*. Solving Experimental Problems on the Topic "Preparation and Properties of Inorganic Compounds"

Appendix 1. Electronic Structure of Atoms of Chemical Elements of the Small Periods (I–III)

Appendix 2. Minerals and Their Hardness on the Mohs Scale

Appendix 3. Qualitative reactions

Appendix 4. Solubility table of acids, bases, and salts in water

Answers to Calculation Problems and Tests in Inorganic Chemistry