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attaches. These processes are inextricably linked. Compounds containing

elements with the highest oxidation state may only be oxidizing agents during

redox. Compounds containing elements with the lowest oxidation state may only

be reducing agents during redox. Connections, which include elements with an

intermediate oxidation stete, can be both oxidizing and reducing agents.

To balance the equations of redox the method of electronic balance is used.

The scheme of the method is as follows:

- the equation of reaction is written down;

- the oxidation determine of the atoms of all elements is determined;

- the atoms of elements that have changed the oxidation state are determined (for

both the oxidant (s) and the reducing agent (s));

- electronic equations for an oxidizer and reducing agent are made up;

- the main coefficients of the equation are determined;
- metals are equalized;

- non-metals (except Hydrogen and Oxygen) are equalized;
- the Hydrogen atoms are equalized;

- the balance of oxygen atoms is determined.
Example 1:

K 2Cr 2O 7 + HCl → CrCl 3 + Cl 2 + KCl + H 2O.

Let us determine the oxidation state of elements in this equation:

6.3. Oxidants and reducing agents

From the chemical point of view reduction-oxidation processes are specific.

To a certain extent their specificity depends on the nature of the oxidizer and

reducing agent. Let us consider in detail the substance which includes elements

that can change the oxidation state. Oxidants include substances that have a

pronounced tendency to attach electrons. For example, oxidizing agents are

oxygen, free halogens, compounds of some metals with higher oxidation levels (

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