Potassium oxide: formula, interaction. Basic oxides Potassium oxide solubility in water
The lesson is devoted to the study of the characteristics of an element by its position in the periodic table of elements. During the lesson, you will learn to determine, based on the position of an element in the periodic table, the structural features of its atom and the properties of the substances it forms; compare these properties with the properties of the element’s “neighbors” by subgroup and period.
Topic: Summarizing the material covered
Lesson: Description of a chemical element by position in the Periodic Table
1. Structure of an element’s atom
In order to determine the composition of the nucleus and the distribution of electrons among the layers in the atom of a chemical element, you need to know the atomic number of the element, period number, group number and subgroup in the Periodic System.
Let's look at a specific example. Let us determine the structure of the potassium atom. The atomic number of potassium is 19. The atomic number determines the number of protons in the nucleus and the total number of electrons in the atom. The number of neutrons in a particular atom can be determined by the difference between the mass number and the number of protons. For a potassium isotope with a mass number of 39, the number of protons is 19, the number of neutrons is 39-19=20, and the number of electrons is 19.
By the period number you can determine the number of electron layers in an atom. Potassium is a period 4 element, which means that all of its 19 electrons are located on 4 electron layers. It must be remembered that the 1st layer can have a maximum of no more than 2 electrons, the second - no more than 8. The number of electrons in the last layer is equal to the group number (for elements of the main subgroups). Potassium has only 1 outer electron, it is located in the 4th layer. The remaining electrons are in the third layer. Thus, in a potassium atom, electrons are distributed among the layers in the following quantities: 2, 8, 8, 1 (Fig. 1).
Rice. 1. Scheme of the structure of the potassium atom
The group number determines not only the number of outer electrons, but the highest valency of the element. The numerical value of the lowest valency for elements of groups V-VII is 8 - the group number. So, the highest and only valence of potassium is I.
2. Properties of a simple substance formed by an element
By the position of an element in the periodic table, one can determine whether it belongs to metals or non-metals, as well as the properties of the higher oxides and hydroxides formed by it. The elements of the main subgroups lying above the Be-At diagonal are non-metals. The remaining elements are metals. In this case, the metallic properties weaken from left to right across the period, and strengthen from top to bottom across the group.
Thus, potassium is a metal. Its metallic properties are more pronounced than those of sodium and calcium.
3. Formula and properties of the highest oxide and hydroxide of the element
If an element forms a simple metal substance, then its higher oxide and hydroxide will be basic. If it is a non-metal, then it is acidic. If it is a transition metal, then it is amphoteric (Fig. 2).
Rice. 2. Relationship between the properties of elements and the compounds formed by them
Since potassium is a metal, its higher oxide and hydroxide will exhibit basic properties.
Let's make up the formulas of higher oxide and potassium hydroxide. The highest valency of potassium is I, which means that the formula of the higher oxide is K2O, its character is basic.
The main oxide corresponds to the base - KOH.
You can confirm the basic nature of potassium oxide and hydroxide by writing down the equations for the reactions of these substances with acid:
K2O + 2HCl = 2KCl + H2O
KOH + HCl = KCl + H2O
Nonmetallic elements can form volatile hydrogen compounds. To compose the formula of a volatile hydrogen compound of a non-metal, you need to know the lowest valence of the latter. For example, the volatile hydrogen compound of nitrogen is NH3 (the lowest valency of nitrogen is III). Metals do not form volatile hydrogen compounds.
If we compare potassium with its neighboring elements in the subgroup and period, we can say that the basic properties of its oxide and hydroxide will be more pronounced than those of the oxides and hydroxides of sodium and calcium. Rubidium is a more active metal than potassium. This means that the basic properties of its oxide and hydroxide will be more pronounced than those of potassium oxide and hydroxide.
Characteristics of the element according to plan
Let us characterize the chemical element sulfur according to plan, taking into account its position in D. I. Mendeleev’s Periodic Table of Elements:
1. Chemical sign - S (“Es”)
2. Serial number - 19, VI group, A subgroup, 3rd period
3. Atomic structure:
4. Properties of a simple substance: S - non-metal
5. Highest and lowest valency: VI and II
6. Higher oxide: SO3 (acidic)
Higher hydroxide: H2SO4 (acid)
7. Formula of volatile hydrogen compound: H2S
Bibliography
Orzhekovsky P. A. Chemistry: 8th grade: textbook for general education. establishment / P. A. Orzhekovsky, L. M. Meshcheryakova, M. M. Shalashova. - M.: Astrel, 2013. (§§45) Rudzitis G. E. Chemistry: inorganic. chemistry. Organ. chemistry: textbook. for 9th grade. / G. E. Rudzitis, F. G. Feldman. - M.: Education, OJSC “Moscow Textbooks”, 2009. (§36) Khomchenko I. D. Collection of problems and exercises in chemistry for high school. - M.: RIA “New Wave”: Publisher Umerenkov, 2008. (p. 35-36) Encyclopedia for children. Volume 17. Chemistry / Chapter. ed. V. A. Volodin, leading scientific ed. I. Leenson. - M.: Avanta+, 2003.
InternetUrok. ru. Far Eastern State University of Transport.
Homework
With. 255 Nos. 1-3 from the textbook by P. A. Orzhekovsky “Chemistry: 8th grade” / P. A. Orzhekovsky, L. M. Meshcheryakova, M. M. Shalashova. - M.: Astrel, 2013. Characterize chemical element No. 20 according to the above plan.
This article will characterize potassium from the point of view of physics and chemistry. The first of these sciences studies the mechanical and external properties of substances. And the second is their interaction with each other - this is chemistry. Potassium is the nineteenth element in the periodic table. It belongs to This article will consider the electronic formula of potassium, its behavior with other substances, etc. This is one of the most active metals. The science that studies this and other elements is chemistry. Grade 8 involves studying their properties. Therefore, this article will be useful for schoolchildren. So, let's begin.
Characteristics of potassium from the point of view of physics
This is a simple substance that, under normal conditions, is in a solid state of aggregation. The melting point is sixty-three degrees Celsius. This metal boils when the temperature reaches seven hundred and sixty-one degrees Celsius. The substance in question has a silvery-white color. Has a metallic luster.
The density of potassium is eighty-six hundredths of a gram per cubic centimeter. This is a very light metal. The formula of potassium is very simple - it does not form molecules. This substance consists of atoms that are located close to each other and have a crystal lattice. The atomic mass of potassium is thirty-nine grams per mole. Its hardness is very low - it can be easily cut with a knife, like cheese.
Potassium and chemistry
Let's start with the fact that potassium is a chemical element that has very high chemical activity. You can’t even store it in the open air, as it instantly begins to react with the substances around it. Potassium is a chemical element that belongs to the first group and the fourth period of the periodic table. It has all the properties that are characteristic of metals.
Interaction with simple substances
These include: oxygen, nitrogen, sulfur, phosphorus, halogens (iodine, fluorine, chlorine, bromine). Let's consider the interaction of potassium with each of them in order. Interaction with oxygen is called oxidation. During this chemical reaction, potassium and oxygen are consumed in a molar ratio of four parts to one, resulting in the formation of an oxide of the metal in question in an amount of two parts. This interaction can be expressed using the following reaction equation: 4K + O2 = 2K2O. When potassium burns, you can observe
Therefore, this reaction is considered qualitative for the determination of potassium. Reactions with halogens are named according to the names of these chemical elements: iodination, fluorination, chlorination, bromination. These interactions can be called addition reactions, since atoms of two different substances combine into one. An example of such a process is the reaction between potassium and chlorine, which results in the formation of chloride of the metal in question. To carry out this interaction, it is necessary to take two of these components - two moles of the first and one mole of the second. The result is two moles of potassium compound. This reaction is expressed by the following equation: 2К + СІ2 = 2КІ. Potassium can form compounds with nitrogen when burned in the open air. During this reaction, the metal in question and nitrogen are consumed in a molar ratio of six parts to one; as a result of this interaction, potassium nitride is formed in an amount of two parts. This can be shown as the following equation: 6K + N2 = 2K3N. This compound appears as green-black crystals. The metal in question reacts with phosphorus according to the same principle. If we take three moles of potassium and one mole of phosphorus, we get one mole of phosphide. This chemical interaction can be written in the form of the following reaction equation: 3K + P = K3P. In addition, potassium can react with hydrogen to form a hydride. As an example, the following equation can be given: 2K + H2 = 2KN. All addition reactions occur only in the presence of high temperatures.
Interaction with complex substances
The characteristics of potassium from a chemical point of view include consideration of this topic. The types of compounds that potassium can react with include water, acids, salts, and oxides. The metal in question reacts differently with all of them.
Potassium and water
This chemical element reacts violently with it. This produces hydroxide as well as hydrogen. If we take two moles of potassium and water, we get the same amount and one mole of hydrogen. This chemical interaction can be expressed using the following equation: 2K + 2H2O = 2KOH = H2.
Reactions with acids
Since potassium is an active metal, it easily displaces hydrogen atoms from their compounds. An example would be a reaction that occurs between the substance in question and hydrochloric acid. To carry it out, you need to take two moles of potassium, as well as acid in the same amount. As a result, two moles and hydrogen are formed - one mole. This process can be written by the following equation: 2K + 2НІ = 2КІ + Н2.
Potassium and oxides
The metal in question reacts with this group of inorganic substances only upon significant heating. If the metal atom that is part of the oxide is more passive than the one we are talking about in this article, essentially an exchange reaction occurs. For example, if you take two moles of potassium and one mole of cuprum oxide, then as a result of their interaction you can get one mole of the oxide of the chemical element in question and pure cuprum. This can be shown in the form of the following equation: 2K + CuO = K2O + Cu. This is where the powerful reducing properties of potassium come into play.
Interaction with bases
Potassium is capable of reacting with metal hydroxides that are to the right of it in the electrochemical activity series. In this case, its restorative properties also appear. For example, if we take two moles of potassium and one mole of barium hydroxide, then as a result of the substitution reaction we will obtain substances such as potassium hydroxide in an amount of two moles and pure barium (one mole) - it will precipitate. The chemical interaction presented can be represented as the following equation: 2K + Ba(OH)2 = 2KOH + Ba.
Reactions with salts
In this case, potassium still exhibits its properties as a strong reducing agent. By replacing atoms of chemically more passive elements, it makes it possible to obtain pure metal. For example, if you add three moles of potassium to an amount of two moles, then as a result of this reaction we get three moles of potassium chloride and two moles of aluminum. This process can be expressed using the equation as follows: 3К + 2АІСІ3 = 3КІ2 + 2АІ.
Reactions with fats
If potassium is added to any organic substance of this group, it will also displace one of the hydrogen atoms. For example, when stearin is mixed with the metal in question, potassium stearate and hydrogen are formed. The resulting substance is used to make liquid soap. This is where the characterization of potassium and its interactions with other substances ends.
Use of potassium and its compounds
Like all metals, the one discussed in this article is necessary for many industrial processes. The main use of potassium occurs in the chemical industry. Due to its high chemical activity, pronounced alkali metal and reducing properties, it is used as a reagent for many interactions and the production of various substances. In addition, alloys containing potassium are used as coolants in nuclear reactors. The metal discussed in this article also finds its application in electrical engineering. In addition to all of the above, it is one of the main components of plant fertilizers. In addition, its compounds are used in a wide variety of industries. Thus, in gold mining, potassium cyanide is used, which serves as a reagent for separating valuable metals from ores. Phosphates of the chemical element in question are used in glass production and are components of all kinds of cleaning products and powders. Matches contain chlorate of this metal. In the manufacture of films for old cameras, bromide of the element in question was used. As you already know, it can be obtained by bromination of potassium at high temperatures. In medicine, the chloride of this chemical element is used. In soap making - stearate and other fat derivatives.
Obtaining the metal in question
Nowadays, potassium is extracted in laboratories in two main ways. The first is its reduction from hydroxide using sodium, which is chemically even more active than potassium. And the second is to obtain it from chloride, also using sodium. If you add the same amount of sodium to one mole of potassium hydroxide, one mole of sodium alkali and pure potassium are formed. The equation for this reaction is as follows: KOH + Na = NaOH + K. To carry out the second type of reaction, you need to mix the chloride of the metal in question and sodium in equal molar proportions. As a result of this, substances such as kitchen salt and potassium are formed in the same ratio. This chemical interaction can be expressed using the following reaction equation: KCI + Na = NaCl + K.
The structure of potassium
The atom of this chemical element, like all others, consists of a nucleus that contains protons and neutrons, as well as electrons that revolve around it. The number of electrons is always equal to the number of protons that are inside the nucleus. If any electron is detached or attached to an atom, then it ceases to be neutral and turns into an ion. They come in two types: cations and anions. The former have a positive charge, while the latter have a negative charge. If an electron is added to an atom, it turns into an anion, but if any of the electrons leaves its orbit, the neutral atom becomes a cation. Since the serial number of potassium, according to the periodic table, is nineteen, there are the same number of protons in the nucleus of this chemical element. Therefore, we can conclude that there are nineteen electrons around the nucleus. The number of protons contained in the structure of an atom can be determined by subtracting the atomic number of the chemical element from the atomic mass. So we can conclude that there are twenty protons in the potassium nucleus. Since the metal considered in this article belongs to the fourth period, it has four orbits in which electrons are evenly distributed, which are constantly in motion. The diagram of potassium is as follows: the first orbit has two electrons, the second has eight; just like in the third, in the last, fourth, orbit only one electron rotates. This explains the high level of chemical activity of this metal - its last orbit is not completely filled, so it tends to combine with some other atoms, as a result of which the electrons of their last orbits will become common.
Where can this element be found in nature?
Since it has extremely high chemical activity, it is not found anywhere on the planet in its pure form. It can only be seen in various compounds. potassium in the earth's crust is 2.4 percent. The most common minerals containing potassium are salvinite and carnallite. The first has the following chemical formula: NaCl.KCl. It has a variegated color and consists of many crystals of various colors. Depending on the ratio of potassium chloride and sodium, as well as the presence of impurities, it may contain red, blue, pink, and orange components. The second mineral - carnallite - looks like transparent, soft blue, light pink or pale yellow crystals. Its chemical formula looks like this: KCl.MgCl2.6H2O. It is a crystalline hydrate.
The role of potassium in the body, symptoms of deficiency and excess
It, together with sodium, maintains the water-salt balance of the cell. It is also involved in the transmission of nerve impulses between membranes. In addition, it regulates the acid-base balance in the cell and throughout the body as a whole. It takes part in metabolic processes, counteracts the occurrence of edema, and is part of the cytoplasm - about fifty percent of it - the salt of the metal in question. The main signs that the body does not have enough potassium are swelling, the occurrence of a disease such as dropsy, irritability and disturbances in the functioning of the nervous system, slow reaction and memory impairment.
In addition, an insufficient amount of this microelement negatively affects the cardiovascular and muscular systems. A lack of potassium over a very long period of time can cause a heart attack or stroke. But due to excess potassium in the body, a small intestinal ulcer can develop. To balance your diet so that you get the normal amount of potassium, you need to know what foods contain it.
Foods high in the micronutrient in question
First of all, these are nuts such as cashews, walnuts, hazelnuts, peanuts, almonds. Also, a large amount of it is found in potatoes. In addition, potassium is found in dried fruits such as raisins, dried apricots, and prunes. Pine nuts are also rich in this element. Its high concentration is also observed in legumes: beans, peas, lentils. Sea kale is also rich in this chemical element. Other products that contain this element in large quantities are green tea and cocoa. In addition, it is found in high concentrations in many fruits, such as avocados, bananas, peaches, oranges, grapefruits, and apples. Many cereals are rich in this microelement. This is primarily pearl barley, as well as wheat and buckwheat. Parsley and Brussels sprouts also have a lot of potassium. In addition, it is found in carrots and melon. Onions and garlic contain a considerable amount of the chemical element in question. Chicken eggs, milk and cheese are also high in potassium. The daily norm of this chemical element for the average person is from three to five grams.
Conclusion
After reading this article, we can conclude that potassium is an extremely important chemical element. It is necessary for the synthesis of many compounds in the chemical industry. In addition, it is used in many other industries. It is also very important for the human body, so it must be supplied there regularly and in the required quantity with food.
Potassium oxide is an inorganic substance with the chemical formula K 2 O.
Brief characteristics of potassium oxide:
Potassium oxide– an inorganic substance of colorless or pale yellow color.
3. reaction of potassium oxide with carbon monoxide (carbon dioxide):
K 2 O + CO 2 → K 2 CO 3.
Potassium oxide reacts in air with carbon dioxide(which is an acidic oxide), forming a salt - potassium carbonate.
4. reaction of potassium oxide with sulfur oxide:
K 2 O + SO 2 → K 2 SO 3;
K 2 O + SO 3 → K 2 SO 4.
K 2 O + ZnO → K 2 ZnO 2.
K 2 O + NO 2 → KNO 3 + KNO 2.
As a result of the reaction, salts are formed - potassium nitrate and potassium nitrite, respectively.
8. reaction of potassium oxide with hydrofluoric acid:
K 2 O + 2HF → 2KF + H 2 O.
As a result of a chemical reaction, salt is obtained - potassium fluoride and water.
9. reaction of potassium oxide with nitric acid:
K 2 O + 2HNO 3 → 2KNO 3 + H 2 O.
As a result of a chemical reaction, salt is obtained - potassium nitrate and water.
The reactions of potassium oxide with other acids proceed similarly.
10. reaction of potassium oxide with hydrogen bromide (hydrogen bromide):
K 2 O + 2HBr → 2KBr + H 2 O.
As a result of a chemical reaction, a salt is obtained - potassium bromide and
Among the chemical elements, potassium stands out for a number of its unique physical and chemical properties. It is of interest to chemists for its high activity. This substance instantly reacts with oxygen, heating in air leads to its combustion, the product of this reaction is potassium superoxide. Interaction with water and acid solutions leads to violent ignition and even explosion. Potassium is capable of reducing sulfuric acid to hydrogen sulfide, sulfur dioxide and sulfur, and is reduced to molecular nitrogen.
In the periodic table, potassium occupies cell number nineteen. Its belonging to the alkali metals explains the silvery-white color and high ductility of this substance; it is easily cut with a knife and exhibits high chemical activity. This explains the fact that pure potassium does not occur in nature. Among the substances in which potassium is included as a constituent element, the most common is sea water; it can also be found in various minerals. The rapid oxidation of this substance leads to the fact that potassium oxide (formula K2O) quickly turns into the peroxide state (K2O4).
Potassium can be produced by heating the metal to 180 °C in an oxygen-depleted environment or by heating a mixture of superoxide and potassium metal. As a constituent, potassium oxide is found in cement and some types of fertilizers.
Potassium is of great importance for the plant world; it is one of the three main building materials of organic compounds, along with nitrogen and phosphorus. Fruiting and further preservation of fruits and tubers are associated with the level of potassium. Potassium plays an important role in the transport of sugar and in the formation of plant reserves, this is manifested in an increase in starch in tubers, rhizomes and roots. Potassium has a beneficial effect on increasing the density of plant tissues and their stems. The lack of potassium results in the plant being unable to properly absorb nitrogen. Plants use potassium hydroxide. It interacts with a number of substances, ensuring the normal functioning of the plant organism.
The lack of potassium in some soils is compensated by the use of a wide range. Their production is based on the use of natural deposits of potassium salts; the minerals are called sylvinite and carnallite; potassium sulphate salts include shenite, kainite and langbeinite. The use of minerals makes it possible to obtain fertilizers with a high concentration of potassium.
The most common fertilizer, which includes potassium oxide, is This mixture is a composition of finely ground mineral of natural origin sylvinite, and potassium oxide reaches 40%.
A substance with pronounced basic properties is capable of reacting violently not only with acids, acid oxides and even water. The property of this compound to exchange carbon dioxide for oxygen is widely used in gas masks of the insulating principle of action, as well as on submarines. The absorbent in this case is an equimolar mixture of sodium peroxide and potassium superoxide. If the mixture is not equimolar and there is an excess of sodium peroxide, more gas is absorbed than is released. For two volumes of carbon dioxide, one volume of oxygen is released. At the same time, in a confined space the pressure drops. Excess potassium superoxide has the effect of absorbing two volumes and releasing three volumes of oxygen, and the pressure will increase. Equimolarity of the mixture makes it possible to achieve equalization of the volumes of absorbed and released gases.
Being a strong oxidizing agent, peroxides are used in the textile industry to bleach fabrics.
There are three main classes of compounds. These are acids, alkalis and oxides. An acid consists of a hydrogen cation and an acidic anion. Alkali - made from a metal cation and a hydroxyl group. We will talk about oxides in more detail later.
What is an oxide?
This is a compound consisting of two different chemical elements, one of which is oxygen. The second one can be metal or non-metal. The number of oxygen atoms depends on the valence of the second chemical element included in the compound. So, for example, the valency of potassium is one, so potassium oxide will contain one oxygen atom and two potassium atoms. The valency of calcium is two, so its oxide will consist of one oxygen atom and one calcium atom. The valency of phosphorus is five, so its oxide consists of two phosphorus atoms and five oxygen atoms.
In this article we will talk in more detail about potassium oxide. Namely - about its physical and chemical properties, about its application in various fields of industry.
Potassium oxide: formula
Since the valency of this metal is one, and the valence of oxygen is two, this chemical compound will consist of two metal atoms and one oxygen atom. So, potassium oxide: formula - K 2 O.
Physical properties
The oxide in question has a pale yellow color. Sometimes it can be colorless. At room temperature it has a solid state of aggregation.
The melting point of this substance is 740 degrees Celsius.
The density is 2.32 g/cm 3 .
The thermal decomposition of this oxide produces peroxide of the same metal and pure potassium.
Soluble in organic solvents.
It does not dissolve in water, but reacts with it.
It is highly hygroscopic.
Chemical properties of K 2 O
This substance has chemical properties typical of all basic oxides. Let us consider the chemical reactions of this oxide with various substances in order.
Reaction with water
First of all, it is capable of reacting with water to form the hydroxide of this metal.
The equation for such a reaction is as follows:
- K 2 O + H 2 O = 2 KON
Knowing the molar mass of each substance, the following conclusion can be drawn from the equation: from 94 grams of the oxide in question and 18 grams of water, 112 grams of potassium hydroxide can be obtained.
With other oxides
In addition, the oxide in question is capable of reacting with carbon dioxide (carbon dioxide). In this case, a salt is formed - potassium carbonate.
The reaction equation for potassium oxide and carbon oxide can be written as follows:
- K 2 O + CO 2 = K 2 CO 3
So, we can conclude that from 94 grams of the oxide in question and 44 grams of carbon dioxide, 138 grams of potassium carbonate are obtained.
Also, the oxide in question can react with sulfur oxide. In this case, another salt is formed - potassium sulfate.
The interaction of potassium oxide with sulfur oxide can be expressed by the following equation:
- K 2 O + SO 3 = K 2 SO 4
It shows that by taking 94 grams of the oxide in question and 80 grams of sulfur oxide, you can get 174 grams of potassium sulfate.
In the same way, K 2 O can react with other oxides.
Another type of interaction is reactions not with acidic, but with amphoteric oxides. In this case, it is not an acid that is formed, but a salt. An example of such a chemical process is the interaction of the oxide in question with zinc oxide.
This reaction can be expressed by the following equation:
- K 2 O + ZnO = K 2 ZnO 2
It shows that when the oxide in question interacts with zinc oxide, a salt called potassium zincate is formed. If you know the molar mass of all substances, then you can calculate that from 94 grams of K 2 O and 81 grams of zinc oxide you can get 175 grams of potassium zincate.
K2O is also capable of interacting with nitric oxide. In this case, a mixture of two salts is formed: potassium nitrate and nitrite. The equation for this reaction looks like this:
- K 2 O + 2NO 2 = KNO 3 + KNO 2
If you know the molar masses of substances, we can say that from 94 grams of the oxide in question and 92 grams of nitrogen oxide, you can get 101 grams of nitrate and 85 grams of nitrite.
Interaction with acids
The most common case is potassium oxide + sulfuric acid = potassium sulfate + water. The reaction equation looks like this:
- K 2 O + H 2 SO 4 = K 2 SO 4 + H 2 O
From the equation we can conclude that to obtain 174 grams of potassium sulfate and 18 grams of water, it is necessary to take 94 grams of the oxide in question and 98 grams of sulfuric acid.
In a similar way, a chemical interaction occurs between the oxide in question and nitric acid. This produces potassium nitrate and water. The equation for this reaction can be written as follows:
- 2K 2 O + 4HNO 3 = 4KNO 3 + 2H 2 O
Thus, from 188 grams of the oxide in question and 252 grams of nitric acid, 404 grams of potassium nitrate and 36 grams of water can be obtained.
By the same principle, the oxide in question can react with other acids. During this process, other salts and water will be formed. So, for example, when this oxide reacts with phosphoric acid, phosphate and water are obtained, with chloride acid - chloride and water, and so on.
K 2 O and halogens
The chemical compound in question is capable of reacting with substances of this group. Halogens are simple compounds consisting of several atoms of the same chemical element. These are, for example, chlorine, bromine, iodine and some others.
So, chlorine and potassium oxide: equation:
- K 2 O + CI 2 = KSI + KSIO
As a result of this interaction, two salts are formed: potassium chloride and potassium hypochlorite. From 94 grams of the oxide in question and 70 grams of chlorine, 74 grams of potassium chloride and 90 grams of potassium hypochlorite are obtained.
Interaction with ammonia
K 2 O is able to react with this substance. As a result of this chemical interaction, potassium hydroxide and amide are formed. The equation for this reaction is as follows:
- K 2 O + NH 3 = KOH + KNH 2
Knowing the molar masses of all substances, you can calculate the proportions of reactants and reaction products. From 94 grams of the oxide in question and 17 grams of ammonia, you can get 56 grams of potassium hydroxide and 55 grams of potassium amide.
Interaction with organic substances
Among organic chemicals, potassium oxide reacts with ethers and alcohols. However, these reactions are slow and require special conditions.
Obtaining K 2 O
This chemical can be obtained in several ways. Here are the most common ones:
- From potassium nitrate and potassium metal. These two reactants are heated, resulting in the formation of K 2 O and nitrogen. The reaction equation is as follows: 2KNO 3 + 10K = N 2 + 6K 2 O.
- The second method occurs in two stages. First, a reaction occurs between potassium and oxygen, resulting in the formation of potassium peroxide. The reaction equation looks like this: 2K + O 2 = K 2 O 2. Next, the peroxide is enriched with potassium, resulting in potassium oxide. The reaction equation can be written as follows: K 2 O 2 + 2K = 2K 2 O.
Use of K2O in industry
The substance in question is most commonly used in the agricultural industry. This oxide is one of the components of mineral fertilizers. Potassium is very important for plants, as it increases their resistance to various diseases. The substance in question is also used in construction, as it may be present in some types of cement. In addition, it is used in the chemical industry to produce other potassium compounds.
