Chemical properties of sulfur. Characterization and boiling point of sulfur

Sulfur is a chemical element that is in the sixth group and the third period of the periodic table. In this article, we will take a closer look at its chemical and physical properties, obtaining, using, and so on. The physical characteristic includes such features as color, the level of electrical conductivity, the boiling point of sulfur, etc. Chemical, however, describes its interaction with other substances.

Sulfur in terms of physics

It's a fragile substance. Under normal conditions, it stays in a solid aggregate state. The sulfur has a lemon-yellow color. And for the most part all its compounds have yellow shades. It does not dissolve in water. It has low heat and electrical conductivity. These characteristics characterize it as a typical non-metal. Despite the fact that the chemical composition of sulfur is not at all complicated, this substance can have several variations. Everything depends on the structure of the crystal lattice, with which atoms are connected, they do not form molecules.

So, the first option is rhombic sulfur. It is the most stable. The boiling point of sulfur of this type is four hundred forty-five degrees Celsius. But in order for this substance to pass into a gaseous aggregate state, it must first pass through the liquid. So, the melting of sulfur occurs at a temperature that is one hundred and thirteen degrees Celsius.

The second option is monoclinic sulfur. It is a needle-shaped crystal with a dark yellow color. Melting of sulfur of the first type, and then its slow cooling leads to the formation of this species. This variety has almost the same physical characteristics. For example, the boiling point of sulfur of this type is the same four hundred and forty-five degrees. In addition, there is a variety of this substance, such as plastic. It is obtained by pouring into a cold water a boiling rhombic almost to boiling point. The boiling point of sulfur of this kind is the same. But the substance has the property of stretching, like rubber.

Another component of the physical characteristics, which I would like to say, is the sulfur ignition temperature. This indicator may vary depending on the type of material and its origin. For example, the technical sulfur ignition temperature is one hundred and ninety degrees. This is a fairly low rate. In other cases, the flash point of sulfur may be two hundred and forty-eight degrees and even two hundred and fifty-six. It all depends on what material it was extracted from, what density it has. But we can conclude that the combustion temperature of sulfur is quite low, compared to other chemical elements, it is a flammable substance. In addition, sometimes sulfur can be combined into molecules consisting of eight, six, four or two atoms. Now, having examined sulfur from the point of view of physics, we proceed to the next section.

Chemical characterization of sulfur

This element has a relatively low atomic mass, it is equal to thirty-two grams per mole. The characteristic of the element of sulfur includes such a feature of this substance as the ability to possess a different degree of oxidation. This is different from, say, hydrogen or oxygen. Considering the question of what is the chemical characteristic of the element of sulfur, it is impossible not to mention that, depending on the conditions, it exhibits both reducing and oxidizing properties. So, in order consider interaction of a given substance with various chemical compounds.

Sulfur and simple substances

Simple substances are substances that have only one chemical element in their composition. Its atoms can be combined into molecules, as, for example, in the case of oxygen, or they may not combine, as is the case for metals. Thus, sulfur can react with metals, other non-metals and halogens.

Interaction with metals

To carry out this kind of process, a high temperature is necessary. Under these conditions, an addition reaction occurs. That is, the metal atoms combine with the sulfur atoms, forming sulfides at the same time. For example, if you heat two moles of potassium, mixing them with one mole of sulfur, we get one mole of the sulphide of a given metal. The equation can be written in the following form: 2K + S = K ₂ S.

Reaction with oxygen

This is the burning of sulfur. As a result of this process, its oxide forms. The latter can be of two kinds. Therefore, the combustion of sulfur can occur in two stages. The first is when one mole of sulfur dioxide is formed from one mole of sulfur and one mole of oxygen. The equation for this chemical reaction can be written as follows: S + O ₂ = SO ₂ . The second stage is the addition of one more oxygen atom to the dioxide. This occurs if one mole of oxygen is added to two moles of sulfur dioxide under high-temperature conditions. As a result, we obtain two moles of sulfuric trioxide. The equation of this chemical interaction looks like this: 2SO ₂ + O ₂ = 2SO ₃ . As a result of this reaction, sulfuric acid is formed. Thus, after carrying out the two described processes, it is possible to pass the resulting trioxide through a jet of water vapor. And we get sulphate acid. The equation for such a reaction is written as follows: SO ₃ + H ₂ O = H ₂ SO ₄ .

Interaction with halogens

The chemical properties of sulfur, like other non-metals, allow it to react with this group of substances. It includes compounds such as fluorine, bromine, chlorine, iodine. Sulfur reacts with any of them, except for the latter. As an example, we can cite the fluoridation process of the element of the Mendeleyev table under consideration. By heating the said non-metal with halogen, two variations of fluoride can be obtained. The first case: if we take one mole of sulfur and three moles of fluorine, we get one mole of fluoride, the formula of which is SF ₆ . The equation is as follows: S + 3F ₂ = SF ₆ . In addition, there is a second option: if we take one mole of sulfur and two moles of fluorine, we get one mole of fluoride with the chemical formula SF ₄ . The equation can be written in the following form: S + 2F ₂ = SF ₄ . As you can see, it all depends on the proportions in which to mix the components. In exactly the same way, it is possible to carry out the process of sulfur chlorination (two different substances can also be formed) or bromination.

Interaction with other simple substances

On this, the characteristic of the sulfur element does not end. The substance can also react chemically with hydrogen, phosphorus and carbon. Due to the interaction with hydrogen, sulfide acid is formed. As a result of its reaction with metals, it is possible to obtain their sulfides, which, in turn, are also obtained directly by the interaction of sulfur with the same metal. The addition of hydrogen atoms to sulfur atoms occurs only at very high temperature. In the reaction of sulfur with phosphorus, its phosphide forms. It has the following formula: P ₂ S _3. In order to obtain one mole of this substance, it is necessary to take two moles of phosphorus and three moles of sulfur. In the interaction of sulfur with carbon, the carbide of the non-metal under consideration is formed. Its chemical formula looks like this: CS ₂ . In order to get one mole of this substance, you need to take one mole of carbon and two moles of sulfur. All of the addition reactions described above occur only when the reagents are heated to high temperatures. We have considered the interaction of sulfur with simple substances, now proceed to the next point.

Sulfur and complex compounds

Complex are called those substances, the molecules of which consist of two (or more) different elements. The chemical properties of sulfur allow it to react with compounds such as alkalis, as well as concentrated sulfate acid. Its reactions with these substances are rather peculiar. First, let's consider what happens when mixing the non-metal in question with alkali. For example, if we take six moles of potassium hydroxide and add three moles of sulfur to them, we get two moles of potassium sulphide, one mole of the sulphite of the metal and three moles of water. This kind of reaction can be expressed by the following equation: 6KOH + 3S = 2K ₂ S + K2SO ₃ + 3H ₂ O. By the same principle, interaction occurs if sodium hydroxide is added . Next, consider the behavior of sulfur when adding to it a concentrated solution of sulfate acid. If we take one mole of the first and two moles of the second substance, we obtain the following products: sulfur trioxide in an amount of three moles, and also water - two moles. This chemical reaction can only be carried out by heating the reagents to a high temperature.

Preparation of the non-metal under consideration

There are several basic ways by which you can extract sulfur from a variety of substances. The first method is to isolate it from pyrite. The chemical formula of the latter is FeS ₂ . When this substance is heated to a high temperature without access to oxygen, another iron sulfide, FeS and sulfur, can be obtained. The reaction equation is written in the following form: FeS ₂ = FeS + S. The second method of obtaining sulfur, which is often used in industry, is the burning of sulfur sulfide under the condition of a small amount of oxygen. In this case, it is possible to obtain the considered non-metal and water. To carry out the reaction, it is necessary to take the components in a molar ratio of two to one. As a result, we get the final products in proportions of two to two. The equation of this chemical reaction can be written as follows: 2H ₂ S + O ₂ = 2S + 2H ₂ O. In addition, sulfur can be obtained in a variety of metallurgical processes, for example, in the production of metals such as nickel, copper and others.

Use in industry

The broadest application of the nonmetal we are considering is found in the chemical industry. As already mentioned above, here it is used to obtain from it sulfate acid. In addition, sulfur is used as a component for making matches, due to the fact that it is a flammable material. It is indispensable in the production of explosives, gunpowder, Bengal lights, etc. In addition, sulfur is used as one of the ingredients of pest control. In medicine, it is used as a component in the manufacture of drugs for skin diseases. Also, the substance in question is used in the manufacture of a variety of dyes. In addition, it is used in the manufacture of phosphors.

Electronic structure of sulfur

As is known, all atoms consist of a nucleus in which the protons are located - positively charged particles - and neutrons, ie, particles having zero charge. Around the nucleus, electrons rotate, the charge of which is negative. For an atom to be neutral, its structure should have the same number of protons and electrons. If the latter is larger, it is already a negative ion - anion. If on the contrary - the number of protons is greater than the number of electrons - this is a positive ion, or cation. The sulfur anion can act as an acid residue. It is part of the molecules of substances such as sulfide acid (hydrogen sulphide) and metal sulphides. Anion is formed during electrolytic dissociation, which occurs when the substance is dissolved in water. In this case, the molecule decomposes into a cation, which can be represented as a metal ion or hydrogen, as well as a cation-ion of the acid residue or hydroxyl group (OH-). Since the serial number of sulfur in the periodic table is sixteen, it can be concluded that there is exactly such a number of protons in its core. Proceeding from this, we can say that there are also sixteen electrons rotating around. The number of neutrons can be determined by subtracting the order number of the chemical element from the molar mass: 32-16 = 16. Each electron rotates not chaotically but in a certain orbit. Since sulfur is a chemical element that belongs to the third period of the periodic table, there are three orbits around the nucleus. On the first of them two electrons are located, on the second - eight, on the third - six. The electronic formula of the sulfur atom is written as follows: 1s2 2s2 2p6 3s2 3p4.

Prevalence in nature

In general, the chemical element in question is found in minerals, which are sulphides of various metals. First of all, this pyrite is the salt of iron; Also it is lead, silver, copper shine, zinc blende, cinnabar - mercury sulphide. In addition, sulfur can also enter into the composition of minerals, the structure of which is represented by three or more chemical elements. For example, chalcopyrite, mirabilite, kieserite, gypsum. You can consider each of them in more detail. Pyrite is a sulphide of ferrum, or FeS ₂ . It has a light yellow color with a golden sheen. This mineral can often be found as an impurity in lapis lazuli, which is widely used for making jewelry. This is due to the fact that these two minerals often have a common deposit. Copper shine - chalcocite, or chalcosine - is a bluish-gray substance, similar to metal. Lead gloss (galena) and silver shine (argentite) have similar properties: they both resemble metals in appearance, they have a gray color. Cinnabar is a brownish-red dull mineral with gray impregnations. Chalcopyrite, whose chemical formula CuFeS ₂ , is golden yellow, it is also called golden blend. Zinc blende (sphalerite) can have a color from amber to fiery orange. Mirabilite - Na ₂ SO ₄ x10H ₂ O - transparent or white crystals. It is also called glauber's salt, used in medicine. The chemical formula of kieserite is MgSO ₄ xH ₂ O. It looks like a white or colorless powder. The chemical formula of gypsum is CaSO ₄ x2H ₂ O. In addition, this chemical element is part of the cells of living organisms and is an important microelement.