I. Watch the popular science film: “Brimstone”

Now it is impossible to establish when a person first became acquainted with sulfur and its compounds. This happened a very long time ago. It helped our ancestors get fire, or rather, sheaves of sparks when they hit a piece of pyrite with a hammer. It was used to make paints and cosmetics. The ancient Indians also knew it; it was they who gave it its name - “Sira” - meaning “yellow”. The chemical symbol comes from the Latin word "sulfur". The ancient Romans called sulfur “the bile of the god Vulcan” (the patron of fire). Painting by Karl Bryullov “The Death of Pompeii”.

Sulfur was considered the work of superhuman beings from the world of spirits or underground gods. A very long time ago, sulfur began to be used as part of various flammable mixtures for military purposes. Homer already described “sulphurous fumes,” the deadly effect of burning sulfur emissions. Sulfur was probably part of the “Greek fire”, which terrified opponents. Around the 8th century The Chinese began to use it in pyrotechnic mixtures, in particular, in mixtures such as gunpowder. The flammability of sulfur, the ease with which it combines with metals to form sulfides (for example, on the surface of pieces of metal), explains why it was considered the “principle of flammability” and an essential component of metal ores. Presbyter Theophilus (12th century) describes the method of oxidizing roasting sulfide copper ore, probably known in ancient Egypt. During the period of Arab alchemy, a composition of metals arose, according to which sulfur was revered as an essential component (father) of all metals. Later it became one of the three principles of alchemists, and later the “flammability principle” became the basis of the theory of phlogiston. The elemental nature of sulfur was established by Lavoisier in his combustion experiments. With the introduction of gunpowder in Europe, the development of natural sulfur mining began, as well as the development of a method for obtaining it from pyrites; the latter was common in ancient Rus'. It was first described in literature by Agricola. Thus, the exact time of the discovery of sulfur has not been established, but, as stated above, this element was used before our era, which means it has been familiar to people since ancient times.

II. Position of sulfur in PSCE, atomic structure

In basic condition

First excited state

+ 6

Second excited state

III. Sulfur in nature

Sulfur is the sixteenth most abundant element in the earth's crust. It is found in a free (native) state and in a bound form.

Native sulfur:

Ukraine, Volga region, Central Asia, etc.

The most important natural sulfur minerals:

• FeS 2 - iron pyrite, or pyrite(cat gold)
• ZnS - zinc blende, or sphalerite (wurtzite)
• PbS - lead gloss, or galena
• Sb 2 S 3 - stibnite

In addition, sulfur is present in oil, natural coal, natural gas and shale.

Sulfur is the sixth most abundant element in natural waters; it is found mainly in the form of sulfate ions and determines the “constant” hardness of fresh water. A vital element for higher organisms, an integral part of many proteins, it is concentrated in hair, nails, and skin. With a lack of sulfur in the body, brittle nails and bones and hair loss occur.

Peas, beans, oatmeal, wheat, meat, fish, fruits and mango juice are rich in sulfur. Sulfur compounds can serve as medicines.

Yarrow has an increased ability to extract sulfur from the soil and stimulate the absorption of this element with neighboring plants.

Garlic releases a substance - albucide, a caustic sulfur compound. This substance prevents cancer, slows down aging, and prevents heart disease.

Sulfates

• CaSO 4 x 2H 2 O - gypsum
• MgSO 4 x 7H 2 O – bitter salt (English)
• Na 2 SO 4 x 10H 2 O – Glauber's salt (mirabilite)

IV. Physical properties, allotropy

Crystalline solid yellow color, insoluble in water, not wetted by water (floats on the surface), t° kip = 445°C

Allotropy

Sulfur is characterized by several allotropic modifications:

Rhombic (a - sulfur) - S 8 t° pl. = 113°C; ρ = 2.07 g/cm3. The most stable modification.	Monoclinic (b - sulfur) - S 8 dark yellow needles, t° pl. = 119°C; ρ = 1.96 g/cm3. Stable at temperatures above 96°C; under normal conditions it turns into rhombic.	Plastic brown rubbery (amorphous) mass. Unstable, when hardening it turns into a rhombic one.

V. Sulfur production

In ancient times and in the Middle Ages, sulfur was mined by digging a large clay pot into the ground, on which another was placed, with a hole in the bottom. The latter was filled with rock containing sulfur and then heated. The sulfur melted and flowed into the lower pot. Currently, sulfur is obtained mainly by smelting native sulfur directly in places where it occurs underground. Sulfur ores are mined in different ways, depending on the conditions of occurrence. Sulfur deposits are almost always accompanied by accumulations of toxic gases - sulfur compounds. In addition, we must not forget about the possibility of its spontaneous combustion.

1. Industrial method - smelting ore using steam.

2. Incomplete oxidation of hydrogen sulfide (with a lack of oxygen): 2H 2 S + O 2 = 2S + 2H 2 O

3. Wackenroeder reaction: 2H 2 S + SO 2 = 3S + 2H 2 O

VI. Chemical properties of sulfur

VII. Application

Approximately half of the sulfur produced is used in the production of sulfuric acid.

Sulfur is used for vulcanization of rubber, as a fungicide in agriculture and as colloidal sulfur - a medicinal product. Also, sulfur in sulfur bitumen compositions is used to produce sulfur asphalt, and as a substitute for Portland cement to produce sulfur concrete. Sulfur is used for the production of pyrotechnic compositions, was previously used in the production of gunpowder, and is used for the production of matches.

Obtaining ebonite, production of gunpowder, in the fight against agricultural pests, for medical purposes (sulfur ointments for the treatment of skin diseases). Sulfur is the basis of an ointment for the treatment of fungal skin diseases and to combat scabies. Sodium thiosulfate Na 2 S 2 O 3 is used to combat it.

Many sulfuric acid salts contain water of crystallization: ZnSO 4 × 7H 2 O and CuSO 4 × 5H 2 O. They are used as antiseptics for spraying plants and treating grain in the fight against agricultural pests.

Iron sulfate FeSO 4 × 7H 2 O is used for anemia.

BaSO 4 is used for radiographic examination of the stomach and intestines.

Potassium aluminum alum KAI(SO 4) 2 ×12H 2 O is a hemostatic agent for cuts.

The mineral Na 2 SO 4 × 10H 2 O is called “Glauber’s salt” in honor of the German chemist I.R. Glauber who discovered it in the 8th century. Glauber suddenly fell ill during his journey. He could not eat anything, his stomach refused to accept food. One of the local residents directed him to the source. As soon as he drank the bitter salt water, he immediately began to eat. Glauber examined this water, and the salt Na 2 SO 4 × 10H 2 O crystallized out of it. Now it is used as a laxative in medicine, when dyeing cotton fabrics. Salt also finds use in glass production.

VIII. Exercise equipment

IX. Tasks

№1. Complete the reaction equations:

S + O 2 =
S+Na=
S+H2=
Arrange the coefficients using the electronic balance method, indicate the oxidizing agent and reducing agent.

№2. Carry out transformations according to the scheme:
H 2 S → S → Al 2 S 3 → Al(OH) 3

№3. Complete the reaction equations, indicate what properties sulfur exhibits (an oxidizing agent or a reducing agent).

Introduction

Sulfur is one of the few substances with which the first “chemists” operated several thousand years ago. She began to serve humanity long before she occupied cell No. 16 in the periodic table. Substances containing sulfur can be both beneficial and harmful to humans.

Origin of sulfur

Sulfur occurs in nature in a free (native) state, so it was known to man already in ancient times. Sulfur attracted attention due to its characteristic color, blue flame and specific smell that occurs during combustion (the smell of sulfur dioxide). It was believed that burning sulfur drove away evil spirits. The Bible talks about the use of sulfur to cleanse sinners. For medieval people, the smell of “sulfur” was associated with the underworld. The use of burning sulfur for disinfection is mentioned by Homer. In ancient Rome, fabrics were bleached using sulfur dioxide. Sulfur has long been used in medicine - patients were fumigated with its flame, it was included in various ointments for the treatment of skin diseases. In the 11th century Avicenna (Ibn Sina), and then European alchemists, believed that metals, including gold and silver, consist of sulfur and mercury in varying proportions. Therefore, sulfur played an important role in alchemists' attempts to find the "philosopher's stone" and transform base metals into precious ones.

Structure of the sulfur atom

This element has a relatively low atomic mass, equal to thirty-two grams per mole. The characteristics of the element sulfur include such a feature of this substance as the ability to have different degrees of oxidation. That is, it can exhibit both oxidizing and reducing properties.

Located in the main subgroup of the sixth group. Since the serial number of sulfur in the periodic table is sixteen, we can conclude that its nucleus contains exactly this number of protons. Based on this, we can say that there are also sixteen electrons rotating around. The number of neutrons can be found by subtracting the serial number of the chemical element from the molar mass: 32 - 16 = 16. Each electron does not rotate chaotically, but in a specific orbit. Since sulfur is a chemical element that belongs to the third period of the periodic table, there are three orbits around the nucleus. The first of them has two electrons, the second has eight, and the third has six. The electronic formula of the sulfur atom is written as follows: 1s 2 2s 2 2p 6 3s 2 3p 4.

As already mentioned, sulfur can exhibit different states of oxidation. This is due to the structure of its atom. A sulfur atom can accept two electrons and will have a charge of -2. Sulfur can also donate two electrons and then it will take on an oxidation state of +2. In order for sulfur to have an oxidation state of +4 or +6, it is necessary to use a d-orbital to which electrons will transfer. Sulfur has valencies II, IV, VI. Valence IV corresponds to the oxidation state +4, valency VI - +6. With valence IV, one electron will transfer from the p-orbital to the d-orbital, with valence VI - one electron from the p-orbital and one from the s-orbital to the d-orbital.

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Slide captions:

SULFUR. Atomic structure, allotropy, properties and applications of sulfur Completed by the teacher of the Municipal Educational Institution “Secondary School No. 17” Svetlana Valentinovna Malishevskaya

What elements are included in the VI-A subgroup, structural features of atoms? O, S, Se , Te , Po 8 O 1 s 2 2 s 2 2 p 4 16 S ….. 3 s 2 3 p 4 34 Se …. 4 s 2 4 p 4 52 Te…. 5 s 2 5 p 4 84 Po ….. 6 s 2 6 p 4 What is common and what is the difference in the structure of the atoms of the elements of the VI-A subgroup? General: the number of electrons in the outer energy level. Difference: number of energy levels.

How do the properties of elements in a group change from top to bottom? Explain your reasons

When and by whom was oxygen discovered?

Name the basic physical properties of oxygen

Name the basic chemical properties of oxygen

What allotropic modifications of oxygen do you know, the differences?

Valence possibilities of the sulfur atom

Native sulfur

Sulfide sulfur PbS - lead luster Fe S - copper luster

Sulfide sulfur ZnS - zinc blende HgS - cinnabar

Sulfated sulfur Gypsum (CaSO 4 * 2H 2 O) Bitter salt (MgSO 4 * 7H 2 O)

Sulfur production 1. Industrial method - smelting from ore using water steam. 2. Incomplete oxidation of hydrogen sulfide (with a lack of oxygen). 2 H 2 S + O 2 = 2 S + 2 H 2 O 3. Wackenroder reaction 2 H 2 S + SO 2 = 3 S + 2 H 2 O

Chemical properties of sulfur 1) The interaction of sulfur with simple substances: A) with metals, forming sulfides. - Write down the reaction equation, create an electron balance equation. 2 Na + S -> Na 2 S with other metals (except Au, Pt) - at elevated t °: 2Al + 3S – t ° -> Al 2 S 3 Zn + S – t ° -> ZnS Cu + S – t °-> CuS

Chemical properties of sulfur B) Interaction of sulfur with non-metals. For example: The interaction of sulfur and hydrogen. H 2 + S -> H 2 S 2 P + 3 S -> P 2 S 3 C + 2 S -> CS 2 B) The interaction of sulfur and oxygen. S + O 2 – t° -> S +4 O 2 2S + 3O 2 – t°;pt -> 2S +6 O 3

On the topic: methodological developments, presentations and notes

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SULFUR- SULFUR, Sulfur, chemical. element VI gr. Mendeleev system, symbol S, serial number 16, at. V. 32.07. Known since ancient times. In nature, it occurs in the form of water (neptunian) and volcanic deposits. origin. Also found in… Great Medical Encyclopedia

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- (denoted S), a chemical element of group VI of the PERIODIC TABLE, a non-metal, known since antiquity. Occurs in nature both as a separate element and in the form of sulfide minerals such as GALENITE and PYRITE, and sulfate minerals,... ... Scientific and technical encyclopedic dictionary

In the mythology of the Irish Celts, Sera is the father of Parthalon (see chapter 6). According to some sources, it was Sera, and not Parthalon, who was Dilgneid's husband. (

DEFINITION

Sulfur located in the third period of group VI of the main (A) subgroup of the Periodic table.

Belongs to elements of the p-family. Non-metal. The nonmetallic elements included in this group are collectively called chalcogens. Designation - S. Serial number - 16. Relative atomic mass - 32.064 amu.

Electronic structure of the sulfur atom

A sulfur atom consists of a positively charged nucleus (+16), consisting of 16 protons and 16 neutrons, around which 16 electrons move in 3 orbits.

Fig.1. Schematic structure of the sulfur atom.

The distribution of electrons among orbitals is as follows:

1s 2 2s 2 2p 6 3s 2 3p 4 .

The outer energy level of the sulfur atom contains six electrons, all of which are considered valence electrons. The energy diagram takes the following form:

The presence of two unpaired electrons indicates that sulfur is capable of exhibiting the +2 oxidation state. Several excited states are also possible due to the presence of vacant 3 d-orbitals. First, electrons 3 are steamed p-sublevel and occupy free d-orbitals, and then - electrons 3 s-sublevel:

This explains the presence of two more oxidation states in sulfur: +4 and +6.