General chemistry -1Syllabus

Subject code

İF-3037y

Credits

4

Student workload

120

Semester

Autumn semester

Academic year

2025-2026

Subject type

Mandatory

Form of education

Full-time

Language of instruction

Azerbaijani

In-class hours

a) 30 saat mühazirə b) 15 saat laboratoriya

Out-of-class hours

a) 30 saat MRTSİ b) 45 saat TSİ

This subject provides students with fundamental knowledge of the basic theoretical principles of chemistry, stoichiometric laws, thermodynamic and kinetic bases of chemical processes, properties of solutions and dispersed systems, oxidation-reduction reactions, electrolysis and corrosion processes, as well as the structure, production, properties and fields of application of important inorganic compounds.

• lecture
• laboratory work
• presentations
• teamwork

1. 1

   CLO 1: It explains the basic concepts, laws and theoretical principles of chemistry.

2. 2

   CLO 2: Apply stoichiometric laws in chemical calculations.

3. 3

   CLO 3: Analyzes thermodynamic and kinetic regularities of chemical processes.

4. 4

   CLO 4: Evaluates properties of solutions, dispersed systems, oxidation-reduction reactions, electrolysis and corrosion processes.

5. 5

   CLO 5: Determines the structure, production methods and physico-chemical properties of inorganic compounds.

6. 6

   CLO 6: Apply chemical knowledge in laboratory experiments and solving engineering problems.

1. 1.
   1. primary laws of chemistry. stoichiometric lawsLecture

   In this subject, the basic laws of chemistry and the theoretical foundations of stoichiometric calculations are studied. conservation of the mass of substances during chemical reactions, the fact that compounds have a stable composition, and the combination of elements in various compounds in certain mass and volume ratios are explained. at the same time, the concept of equivalent, equivalent mass and its calculation, volume ratios of gases in reactions and the number of gas molecules under the same conditions are given.

   • It explains the basic laws of chemistry. it applies the law of conservation of mass of matter. compares the laws of composition stability and mass ratios. performs calculations using equivalent and avogadro's laws. solve stoichiometric problems.
2. 2.
   3. periodic law and periodic system. electron structure of an atom.Lecture

   The periodic law is a basic chemical law that states that the properties of chemical elements depend periodically on the charge (atomic number) of their atomic nucleus. according to modern periodic law: "the properties of the elements and their constituents change periodically with increasing charge of the atomic nucleus." the periodic law was proposed by dmitri ivanovich mendeleev in 1869. mendeleev placed the elements in order of increasing atomic mass and showed that their properties repeat at certain intervals. in modern times, elements are arranged based on increasing atomic number (number of protons). basic provisions of periodic law the properties of elements depend on their atomic structure. as the atomic number increases, the electronic structure changes in a certain order. elements located in the same group show similar chemical properties. from left to right in the periods, metallic properties decrease and non-metallic properties increase. metallic properties and atomic radius increase from top to bottom in groups. importance of periodic law

   • It explains the nature of periodic law. it characterizes the structure of the periodic system. it creates a connection between the electronic structure and the position of the elements. it explains the change of properties by period and groups. compares changes in electronegativity and atomic radius.
3. 3.
   2. general information about the structure of the atom. quantum numbers. electron orbitals.Lecture

   In this topic, general information is given about the structure of the atom, the elementary particles that make up the atom (proton, neutron and electron), their properties and their location in the atom. the structure of the atomic nucleus, the concept of isotopes and the organization of the electron shell of the atom are explained.

   • Explains the structure of the atom. distinguishes the properties of protons, neutrons and electrons. explains the physical meaning of quantum numbers. it shows the distribution of electrons in orbitals and energy levels. applying the pauli principle, he writes the electron configuration.
4. 4.
   4. chemical communication and its typesLecture

   Ionic communication. ions forming communication. ionic compounds. metal communication. orientation and saturation of metal bond. bond is an interaction that binds atoms and ions together and ensures the formation of substances. chemical bonds are formed mainly by the presence of electrons in the outer electron layers of atoms. atoms donate, accept, or share electrons to reach a more stable electron configuration (usually that of the noble gases). the main types of chemical bonds ionic communication it is caused by the transfer of electrons from one atom to another. it is mainly formed between metal and non-metal atoms. it is based on the electrostatic attraction between positively and negatively charged ions.

   • Differentiates types of chemical bonds. explains the formation of ionic bonds. explains the properties of metal bonding. compares the properties of substances according to the type of communication. 5. chemical kinetics
5. 5.
   7. solutions, their properties. osmotic pressure. raoult's laws.Lecture

   Vapor pressure and phase transformations of solutions. raoult's first law. freezing and boiling point of solution. raoult's second law. osmosis phenomenon. osmosis pressure and van't-hoff's law a solution is a homogeneous system consisting of two or more substances. in a solution, one substance is evenly distributed in another substance and forms a single composition. the main components of a solution are the solvent and the solute. basic concepts of solution a solvent is a component that is present in larger quantities and dissolves another substance. a solute is a component that dissolves in a solvent. a solution is a system formed by the interaction of a solvent and a solute. types of solutions according to the state of the aggregate: gas solutions (e.g. air) liquid solutions (for example, a solution of salt in water) solid solutions (eg alloys) by concentration: unsaturated solution – a solution that can still dissolve the additive. saturated solution - a solution that has dissolved the maximum amount of substance at a certain temperature. a system that stores more matter than a saturated solution - a supersaturated solution. the main properties of solutions it has a homogeneous structure. since the particles are very small, they are not separated by filtration. the properties of the solution depend on its composition and concentration. temperature, pressure, and the nature of the substances affect solubility. the importance of solutions solutions are widely used in chemistry, biology, medicine, industry and everyday life. most of the chemical reactions take place in the solution environment.

   • Explains the concept of solution. raoul applies his laws. explains the variation of freezing and boiling points. explains osmosis and osmotic pressure. it uses van't-hoff's law.
6. 6.
   5. copy of chemical reactionLecture

   The rate of chemical reactions. the rate of homogeneous reactions. the rate of heterogeneous reactions. factors affecting the rate of reaction. fruit bond is an interaction that binds atoms and ions together and ensures the formation of substances. chemical bonds are formed mainly by the presence of electrons in the outer electron layers of atoms. atoms donate, accept, or share electrons to reach a more stable electron configuration (usually that of the noble gases).

   • Explains the rate of a chemical reaction. distinguish between homogeneous and heterogeneous reactions. analyzes the factors affecting the rate of reaction. apply kinetic laws to problems
7. 7.
   8. electrochemical processes, electrode potential. hydrogen electrode. the order of abundance of metalsLecture

   Electrode potential. galvanic elements. jacobi-daniel galvanic cell. standard electrode potential and voltage order. hydrogen electrode. electromotive force of the galvanic element electrochemical processes are processes that provide mutual conversion between chemical energy and electrical energy. these processes take place on the basis of oxidation-reduction (redox) reactions and are accompanied by the transfer of electrons from one substance to another. there are two main processes in electrochemical processes: oxidation is the process of giving electrons to a substance and occurs at the anode. reduction is the process by which a substance receives an electron and occurs at the cathode.

   • Explains electrode potential. explains the importance of hydrogen electrode. explains the working principle of the galvanic element. calculates electromotive force (emf). 9. electrolysis
8. 8.
   2. determination of molecular weight of carbon dioxideLaboratory

   In this lab, the molecular weight of carbon dioxide (co₂) is determined by measuring the volume, mass, temperature, and pressure of the gas. the experiment is based on ideal gas laws. basic concepts: molar volume of gases; relative molecular mass; ideal gas law

9. 9.
   5. cr, mn, fe - their compounds and propertiesLaboratory

   Important compounds, oxidation-reduction properties and chemical reactions of chromium, manganese and iron elements are investigated in this laboratory work. topics studied: cr(iii), cr(vi) compounds; different degrees of oxidation of mn; reactions of fe(ii) and fe(iii) ions; oxidation-reduction processes

10. 10.
    1. determination of zinc equivalent.Laboratory

    In this laboratory work, the equivalent mass of zinc metal is determined experimentally. the volume of hydrogen gas released during the reaction of zinc with acid is measured and the equivalent of zinc is calculated based on the results

11. 11.
    3. chemical kinetics. dependence of reaction rate on c and tLaboratory

    In this laboratory study, the main factors that affect the rate of a chemical reaction are studied. the dependence of the reaction speed on the concentration of the substances and the temperature is investigated experimentally. studied factors: concentration of the reaction substances; effect of temperature; activation energy; reaction speed.

12. 12.
    6. reversible and irreversible reactionsLecture

    Equilibrium of homogeneous reactions. equilibrium of heterogeneous reactions. displacement of equilibrium. le chatelier's principle chemical equilibrium is a state in which the rates of forward and reverse reactions in reversible chemical reactions are equal and the concentrations of substances do not change over time. in this case, the reaction does not stop, it just continues at the same rate in both directions, and a dynamic equilibrium is established. the main characteristics of chemical equilibrium the speed of forward and reverse reactions are equal. the concentrations of reactants and products remain constant. the equilibrium state can change with changes in temperature, pressure, and density. the equilibrium constant (k) shows the relationship between the concentrations of substances involved in the reaction

    • Distinguish between reversible and irreversible reactions. explains the conditions for the formation of chemical equilibrium. it applies the principle of le chatelier. it predicts the shift of equilibrium according to various factors.
13. 13.
    9. electrolysis. laws of electrolysis. galvanic elements.Lecture

    Electrolysis process. scheme of electrolysis. anode and cathode electrodes. electrolysis of aqueous solutions of salts. laws of electrolysis: faraday's i law. faraday's second law.

    • Explains the process of electrolysis. write the anode and cathode reactions. explains the electrolysis of salt solutions. performs calculations by applying faraday's laws.
14. 14.
    10. metals. be,mg-occurrence in natureLecture

    Natural compounds. acquisition, physical and chemical properties. amphoteric property. application.

    • It explains the distribution of be and mg in nature. describes methods of acquisition. compares physical and chemical properties. explains the amphoteric property of beryllium. lists areas of application
15. 15.
    11.al, ti-light construction materialsLecture

    Finding in nature, natural compounds. physico-chemical properties and application of its preparation

    • Recognizes natural compounds of al and ti. explains methods of acquisition. compares its physical and chemical properties. justifies its application as a light construction material.
16. 16.
    12. cu, zn - found in nature, natural compounds.Lecture

    Physico-chemical properties and application of its preparation

17. 17.
    14.mn-natural compounds found in natureLecture

    Manganese (mn) is a d-block transition metal with atomic number 25, located in the 7th group of the 4th period of the periodic system. it is a silver-gray, hard and brittle metal. it is not found in free form in nature, it exists mainly in the form of ores. the electron configuration of manganese is [ar] 3d⁵4s². the semi-solid 3d⁵ underlayer gives the element high stability. manganese can exhibit various oxidation states, making it chemically versatile among the transition metals.

    • He will be able to explain the position of manganese in the periodic table (period 4, group 7, d-block element). he will be able to write the electronic structure of manganese ([ar] 3d⁵4s²) and relate it to the properties of d-metals. he will be able to explain the physical and chemical properties of manganese (hardness, oxidizability, reaction with acids, etc.). he will be able to distinguish the main oxidation states of manganese (+2, +3, +4, +6, +7) and their properties. important compounds of manganese: mno₂ (manganese(iv)-oxide) mno mnso₄ kmno₄ (potassium permanganate) will be able to recognize and explain their chemical properties. he will be able to explain the strong oxidizing properties of potassium permanganate (kmno₄) and its applications. he will be able to study the main natural sources of manganese (especially pyrolusite - mno₂) and methods of obtaining. he will be able to explain the application of manganese in steel production, batteries, catalysts and other industries. he will be able to evaluate the practical and biological importance of manganese compounds. based on chemical reactions, he will be able to determine the role of manganese compounds in oxidation-reduction processes. get smarter responses, upload files and images, a
18. 18.
    15.fe-finding in nature.Lecture

    Finding in nature, natural compounds. physico-chemical properties and application of its preparation

    • Distinguishes iron ores. explains the purchase of cast iron and steel. explains the chemical properties of iron. list the areas of application
19. 19.
    13.cr is found in nature and its compoundsLecture

    Om (cr) is a d-block transition metal with atomic number 24, located in the 6th group of the 4th period of the periodic system. it is a silver-gray, hard, strong and corrosion-resistant metal. the electron configuration [ar] is 3d⁵4s¹, which is explained by the stability of the half-filled 3d subshell. chromium mainly shows +2, +3 and +6 oxidation states. its +3 oxidation state is the most stable, while its +6 oxidation state compounds have strong oxidizing properties. chromium is not found in nature in free form, but mainly in the form of chromite (fecr₂o₄) ore. it is widely used in stainless steel production, metal coating, pigments, leather processing industry and as a catalyst.

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