Presentation on the topic of the periodic law. Periodic law and the Periodic system of chemical elements of D.I. Mendeleev presentation for a lesson in chemistry (Grade 11) on the topic

08.05.2020

“The main interest of chemistry is in the study of the basic qualities of the elements.

Find their root properties, determine the reason for their difference and similarity,

on the basis of this, to predict the properties of the bodies formed by them - such is

path of science"

D. I. Mendeleev.

PERIODIC SYSTEM

CHEMICAL ELEMENTS

DI. MENDELEEV

OPENING

OF THE PERIODIC LAW

13 Kh.E.

WITH WITH u Au

Ag Fe S

Pb As Hg

SnBi Sb Zn

XIX in 63 c.e.

XX in 116 h.e.

XVII in the 20th century

Similar Features

Metals

non-metals

Berzelius

Transition elements

amphoteric properties

Lavoisier

Döbereiner

Johann Wolfgang

in 1817 - 1829

discovered the "law of triads"

(1780 – 1849)

John Newlands

in 1865

announced the opening

"The Law of Octaves"

(1837 – 1898)

Emile Beguier

de Chancourtois

1862

"Earth Spiral"

(1820 – 1886)

Julius Lothar Meyer

His table was

closest to

table of D.I. Mendeleev

4 val

3 val

2 val

1 val

Sn=117.6

2 val

Sb=120.6

Te=128.3

(Tl=204)

Ba=137.4

(1830 – 1895)

Difficulties

arising from the preparation of the table

1. Only 63 elements were known

2.For many chemical elements

have been incorrectly identified

atomic masses

Team 1. By whom and when was the Periodic Law discovered?

Team 3. How is the Periodic Law according to Mendeleev read?

Team 2

What was the basis for the classification of chem. elements of Mendeleev? .

Team 3.

Choose the name of the chem. elements whose etymology is associated with the name of the planets.

Team 1. Find in the PS chem. elements whose names come from the names of parts of the world.

Team 2.

Choose the name of the chem. elements whose etymology is associated with the names of great scientists.

No. 104 Rutherfordium

No. 99 Einsteinium

No. 101 Mendelevius and others

No. 34 Selenium (moon)

No. 93 Neptunium

No. 52 Tellurium (Earth)

No. 63 europium

No. 95 americium

Each period starts with an active alkali metal and ends with a noble gas.

Team 3.

Explain why the law is called

etsya periodic.

Team 1.

Team 2.

There are 8 groups in the PSCE.

How many periods are there in D.I.Mendeleev's PSHE?

How many groups are in D.I.Mendeleev's PSHE?

There are 7 periods in the PSCE. Rooms

“The future does not threaten the periodic law with destruction,

but only add-ons and

development promises"

D.I. Mendeleev

D.I. Mendeleev in his discovery relied on clearly formulated starting points:
A common invariable property of the atoms of all chemical elements is their atomic mass.
The properties of elements depend on their atomic masses.
The form of this dependence is periodic.
The birthday of the Periodic Law is March 1, 1869.
The periodic system of chemical elements is a graphical form of displaying the periodic law.

3. http://www.alhimik.ru/stroenie/gl_5.html

4. http://images.yandex.ru/yandsearch?

5. http://dic.academic.ru/dic.nsf/bse/102765/Lecoq

6. http://www.alhimikov.net/otkritie_elementov/Ge.html

7. http://www.alhimikov.net/otkritie_elementov/Sc.html

slide 1

Periodic Law and Periodic System of Chemical Elements D.I.Mendeleev “The power and strength of science is in a multitude of facts, the goal is to generalize this multitude and raise them to the beginnings… A collection of facts and hypotheses is not yet science; it is only its threshold, past which one cannot directly enter the sanctuary of science. On these thresholds there is an inscription - observations, suggestions, experience. DI. Mendeleev

slide 2

The first attempts to systematize the elements In 1829, the German chemist Johann Wolfgang Döbereiner formulated the law of triads. Cl – 35.5 Br – 80 I – 125 P – 31 As – 75 Sb – 122 S – 32 Se – 79 Te – 129 Ca – 41 Sr – 88 Ba – 137 Li – 7 Na – 23 K – 39

slide 3

Of course, Döbereiner failed to break all known elements into triads, however, the law of triads clearly indicated the existence of a relationship between the atomic mass and the properties of the elements and their compounds. All further attempts at systematization were based on the placement of elements in ascending order of their atomic weights.

slide 4

The first attempts to systematize the elements In 1843, Leopold Gmelin gave a table of chemically similar elements, arranged in groups in ascending order of "connective masses". Outside the groups of elements, at the top of the table, Gmelin placed three "basic" elements - oxygen, nitrogen and hydrogen. Under them were placed triads, as well as tetrads and pentads (groups of four and five elements), and under oxygen there are groups of metalloids (in the terminology of Berzelius), i.e. electronegative elements; electropositive and electronegative properties of groups of elements smoothly changed from top to bottom.

slide 5

Part of Leopold Gmelin's table H = 1 Cl = 35.5 K = 39 O = 8 N = 14 Ag = 108 S = 16 C = 6 Pb = 103.5

slide 6

The first attempts to systematize the elements John Alexander Reina Newlands in 1864 published a table of elements reflecting the law of octaves he proposed. Newlands showed that in a series of elements arranged in ascending order of atomic weights, the properties of the eighth element are similar to those of the first. Such a dependence does take place for light elements, but Newlands tries to make it universal. In the Newlands table, similar elements were arranged in horizontal rows; however, elements quite dissimilar often appeared in the same row. In addition, Newlands was forced to place two elements in some cells; finally, the Newlands table contains no empty seats.

Slide 7

Newlands table no. no. no. Zn 24 Sr 31 Cd 38 Ba V 45 Pb 52 B 4 Al 11 Cr 18 Y 25 Ce La 32 U 39 Ta 46 Th 53 C 5 Si 12 Ti 19 In 26 Zr 33 Sn 40 W 47 Hg 54 N 6 P 13 Mn 20 As 27 Di Mo 34 Sb 41 Nb 48 Bi 55 O 7 S 14 Fe 21 Se 28 Rh Ru 35 Te 42 Au 49 Os 56

Slide 8

The first attempts to systematize the elements In 1864, William Odling, having revised the systematics of the elements proposed by him in 1857, based on equivalent weights, proposed the following table, not accompanied by any explanations.

Slide 9

Odling table Triplet groups H 1 Mo 96 W 184 Au 196.5 Pd 106.5 Pt 197 Li 7 Na 23 - Ag 108 G 9 Mg 24 Zn 65 Cd 112 Hg 200 B 11 Al 27.5 - - Tl 203 C 12 Si 28 - Sn 118 Pb 207 N 14 P 31 As 75 Sb 122 Bi 210 O 16 S 32 Se 79.5 Te 129 F 19 Cl 35 Br 80 J 127 K 39 Rb 85 Cs 133 Ca 40 Sr 87.5 Ba 137 Ti 40 Zr 89.5 - Th 231 Cr 52.5 V 138 Mn 55 and others (Fe, Ni, Co, Cu)

slide 10

In 1870, Julius Lothar Meyer published his first table, which included 42 elements (out of 63), placed in six columns according to their valencies. Meyer deliberately limited the number of elements in the table in order to emphasize the regular (similar to the Döbereiner triads) change in atomic mass in the series of similar elements. The first attempts to systematize the elements

slide 11

Mayer table I II III IV V VI VII VIII IX B Al In (?) Tl C Si Ti Zr Sn Pb NPV As Nb Sb Ta Bi OS Cr Se Mo Te WF Cl Mn Fe Co Ni Br Ru Rh Pd I Os Ir Pt Li Na K Cu Rb Ag Cs Au Be Mg Ca Zn Sr Cd Ba Hg

slide 12

In March 1869, the Russian chemist Dmitry Ivanovich Mendeleev presented to the Russian Chemical Society the periodic law of chemical elements, set out in several basic provisions. In the same 1869, the first edition of the textbook "Fundamentals of Chemistry" was published, in which Mendeleev's periodic table was given.

slide 13

The first table of D.I. Mendeleev, 1869 H = 1 Ti = 50 V = 51 Cr = 52 Mn = 55 Fe = 56 Co = Ni = 59 Cu = 63.4 Zr = 90 Nb = 94 Mo = 96 Rh = 104.4 Ru = 104.4 Pd = 106.6 Ag = 108 = 180 Ta = 182 W = 186 Pt = 197.4 Ir = 198 Os = 199 Hg = 200 Be = 9.4 Mg = 24 Zn = 65.2 Cd = 112 B = 11 Al = 27.4 ? = 68 Ur = 116 Au = 197 C = 12 Si = 28 ? = 70 Sn = 118 N = 14 P = 31 As = 75 Sb = 122 Bi = 210 O = 16 S = 32 Se = 79.4 Te = 128? F = 19 Cl = 35.5 Br = 80 J = 127 Li = 7 Na = 23 K = 39 Ca = 40 = 45 ?Er = 56 ?Yt = 60 ?In = 75.6 Rb = 85.4 Sr = 87.6 Ce = 92 La = 94 Di = 95 Cs = 133 Ba = 137 Tl = 204 Pb = 207

slide 14

At the end of 1870, Mendeleev reported to the RCS an article " natural system elements and its application to indicating the properties of undiscovered elements", in which he predicted the properties of yet undiscovered elements - analogues of boron, aluminum and silicon (respectively, ekabor, ekaaluminum and ekasilicon). Location in the periodic table of elements known in 1870. Cells are shown in green, corresponding to the elements whose properties were predicted by D. I. Mendeleev

slide 15

In 1871, Mendeleev, in his final article "The Periodic Law of Chemical Elements", formulated the Periodic Law: "The properties of the elements, and therefore the properties of the simple and complex bodies formed by them, are in a periodic dependence on the atomic weight." At the same time, Mendeleev gave his periodic table a classical look.

slide 16

More common than others are 3 forms of the periodic table: “short” (short-period) “long” (long-period) “extra-long”. In the "extra-long" version, each period occupies exactly one line. In the "long" version, the lanthanides and actinides are removed from the general table, making it more compact. In the "short" form of entry, in addition to this, the fourth and subsequent periods occupy 2 lines; the symbols of the elements of the main and secondary subgroups are aligned relative to different edges of the cells.

slide 17

Periodic system of elements IA IIA IIIB IVB VB VIB VIIB ---- VIIIB ---- IB IIB IIIA IVA VA VIA VIIA VIIIA 1 1 H 2 He 2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 3 11 Na 12 Mg 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 4 19 K 20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 5 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo (43) Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 6 55 Cs 56 Ba * 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po (85) At 86 Rn 7 87 Fr 88 Ra ** (104) Rf (105) Db (106) Sg ( 107) Bh (108) Hs (109) Mt (110) Ds (111) Rg (112) Cp (113) Uut (114) Uuq (115) Uup (116) Uuh (117) Uus (118) Uuo 8 (119) ) Uue (120) Ubn Lanthanides * 57 La 58 Ce 59 Pr 60 Nd (61) Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu Actinides ** 89 Ac 90 Th 91 Pa 92 U (93) Np (94) Pu (95) Am (96) Cm (97) Bk (98) Cf (99) Es (100) Fm (101) Md (102) No (103) Lr

slide 18

slide 19

The second formulation of the Periodic Law The properties of chemical elements and the substances formed by them are in a periodic dependence on their charges. atomic nuclei.

slide 20

The third formulation of the Periodic Law The properties of chemical elements and the substances formed by them are in a periodic dependence on the periodicity in the change in the configurations of the external electronic words of the atoms of chemical elements.

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Slides captions:

Kartashova L.A., Chemistry teacher, MBOU "Secondary School No. 27 with UIOP", Balakovo Periodic law and periodic system elements D.I. Mendeleev

The discovery of the periodic law was preceded by the accumulation of knowledge about substances and properties. As new chemical elements were discovered, the composition and properties of their compounds were studied, the first attempts to classify elements according to some criteria appeared. In total, up to D.I. Mendeleev, more than 50 attempts were made to classify chemical elements. None of the attempts led to the creation of a system that reflects the relationship of elements, reveals the nature of their similarities and differences, and has a predictive character. Discovery of the Periodic Law

The basis of his work on the classification of chemical elements D.I. Mendeleev put two of their main and constant features: the magnitude of the atomic mass and the properties of substances formed by chemical elements. He wrote down on the cards all the known information about the chemical elements discovered and studied at that time and their compounds. Comparing this information, the scientist compiled natural groups of elements similar in properties. At the same time, he discovered that the properties of elements within certain limits change linearly (monotonically increase or decrease), then after a sharp jump they repeat periodically, i.e. after a certain number of elements, similar ones occur. Discovery of the Periodic Law

In the transition from lithium to fluorine, there is a regular weakening of the metallic properties and an increase in non-metallic ones. When moving from fluorine to the next element in terms of atomic mass, sodium, there is a jump in the change in properties (Na repeats the properties of Li) Na is followed by Mg, which is similar to Be - they exhibit metallic properties. A1, following Mg, resembles B. As close relatives, Si and C are similar; P and N; S and O; C1 and F. When passing to the element K following C1, there is again a jump in change and chemical properties. What was discovered?

If we write the rows one under the other so that sodium is under lithium, and argon is under neon, then we get the following arrangement of elements: Li Be B C N O F Ne Na Mg Al Si P S Cl Ar Periodic law D.I. Mendeleev

Li Be B C N O F Ne Na Mg Al Si P S Cl Ar In this arrangement, elements with similar properties fall into the vertical columns. Periodic law D.I. Mendeleev

Based on his observations on March 1, 1869, D.I. Mendeleev formulated the periodic law, which in its initial formulation sounded like this: the properties of simple bodies, as well as the shapes and properties of compounds of elements, are periodically dependent on the values of the atomic weights of elements. The first version of the Periodic Table

The vulnerable moment of the periodic law immediately after its discovery was the explanation of the reason for the periodic repetition of the properties of elements with an increase in the relative atomic mass of their atoms. Moreover, several pairs of elements are located in the Periodic Table in violation of the increase in atomic mass. For example, argon, with a relative atomic mass of 39.948, is ranked 18th, and potassium, with a relative atomic mass of 39.102, is atomic number 19. Periodic table DI. Mendeleev Ar argon 18 K 19 potassium 39.102 39.948

Only with the discovery of the structure of the atomic nucleus and the establishment physical sense the serial number of the element, it became clear that in the Periodic system they are arranged in order of increasing positive charge of their atomic nuclei. From this point of view, there is no violation in the sequence of elements 18 Ar - 19 K, 27 Co - 28 Ni, 52 Te - 53 I, 90 Th - 91 Pa. Consequently, the modern interpretation of the Periodic Law is as follows: The properties of chemical elements and the compounds they form are in a periodic dependence on the magnitude of the charge of their atomic nuclei. Periodic law D.I. Mendeleev

The law discovered by D. I. Mendeleev and the periodic system of elements built on the basis of the law is the most important achievement chemical science. Periodic table of chemical elements

Periodic table of chemical elements Periods - horizontal rows of chemical elements, 7 periods in total. Periods are divided into small (I, II, III) and large (IV, V, VI), VII - unfinished. Each period (with the exception of the first) begins with a typical metal (Li, Na, K, Rb, Cs, Fr) and ends with a noble gas (He, Ne, Ar, Kr, Xe, Rn), which is preceded by a typical non-metal.

Periodic table of chemical elements Groups - vertical columns of elements with the same number of electrons on the outer electronic level equal to the group number. There are main (A) and secondary subgroups (B). The main subgroups consist of elements of small and large periods. Secondary subgroups consist of elements of only large periods.

Because oxidative restorative properties atoms affect the properties simple substances and their compounds, then the metallic properties of simple substances of the elements of the main subgroups increase, decrease in periods, and non-metallic properties, respectively, on the contrary, decrease in the main subgroups, and increase in periods. redox properties

The reducing properties of atoms (the ability to lose electrons during the formation chemical bond) increase in the main subgroups, and decrease in periods. Oxidizing (the ability to accept electrons), on the contrary, - in the main subgroups they decrease, in periods - they increase. Redox properties

The electronegativity in a period increases with the increase in the charge of the nucleus of a chemical element, that is, from left to right. In a group, with an increase in the number of electron layers, electronegativity decreases, that is, from top to bottom. This means that the most electronegative element is fluorine (F), and the least electronegative is francium (Fr). Electronegativity

The radius of an atom with an increase in the charges of the nuclei of atoms in the period decreases, because. the attraction of the electron shells by the nucleus increases. At the beginning of the period, there are elements with a small number of electrons in the outer electron layer and a large atomic radius. Electrons that are farther from the nucleus easily break away from it, which is typical for metal elements Change in the radius of an atom in a period

In the same group, as the period number increases, the atomic radii increase. Metal atoms donate electrons relatively easily and cannot add them to complete the construction of their outer electronic layer. Changing the radius of an atom in a group

O.S. Gabrielyan, I.G. Ostroumov Chemistry. Final exam M. Drofa, 2008. P.A. Orzhekovsky Preparation for the exam. Chemistry. Collection of tasks. M. Eksmo, 2011 Sources of information

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In the transition from lithium to fluorine, there is a regular weakening of the metallic properties and an increase in non-metallic ones. When moving from fluorine to the next element in terms of atomic mass, sodium, there is a jump in the change in properties (Na repeats the properties of Li) Na is followed by Mg, which is similar to Be - they exhibit metallic properties. A1, following Mg, resembles B. As close relatives, Si and C are similar; P and N; S and O; C1 and F. When moving to the next element K after C1, there is again a jump in the change in chemical properties. What was discovered?

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Li Be B C N O F Ne Na Mg Al Si P S Cl Ar In this arrangement, elements with similar properties fall into the vertical columns. Periodic law D.I. Mendeleev

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The vulnerable moment of the periodic law immediately after its discovery was the explanation of the reason for the periodic repetition of the properties of elements with an increase in the relative atomic mass of their atoms. Moreover, several pairs of elements are located in the Periodic Table in violation of the increase in atomic mass. For example, argon with a relative atomic mass of 39.948 is ranked 18th, and potassium with a relative atomic mass of 39.102 has serial number 19. D.I. Mendeleev Ar argon 18 K 19 potassium 39.102 39.948

9 slide

Description of the slide:

Only with the discovery of the structure of the atomic nucleus and the establishment of the physical meaning of the serial number of the element, it became clear that in the Periodic system they are arranged in order of increasing positive charge of their atomic nuclei. From this point of view, there is no violation in the sequence of elements 18Ar - 19K, 27Co - 28Ni, 52Te - 53I, 90Th - 91Pa. Consequently, the modern interpretation of the Periodic Law is as follows: The properties of chemical elements and the compounds they form are in a periodic dependence on the magnitude of the charge of their atomic nuclei. Periodic law D.I. Mendeleev

10 slide

Description of the slide:

The law discovered by D. I. Mendeleev and the periodic system of elements built on the basis of the law is the most important achievement of chemical science. Periodic table of chemical elements

11 slide

Description of the slide:

Periodic table of chemical elements Periods - horizontal rows of chemical elements, 7 periods in total. Periods are divided into small (I, II, III) and large (IV, V, VI), VII-unfinished. Each period (except the first) begins with a typical metal (Li, Na, K, Rb, Cs, Fr) and ends with a noble gas (He, Ne, Ar, Kr, Xe, Rn), preceded by a typical non-metal.

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Description of the slide:

Periodic table of chemical elements Groups - vertical columns of elements with the same number of electrons in the outer electronic level, equal to the group number. There are main (A) and secondary subgroups (B). The main subgroups consist of elements of small and large periods. Secondary subgroups consist of elements of only large periods.

13 slide

Description of the slide:

Since the redox properties of atoms affect the properties of simple substances and their compounds, the metallic properties of simple substances of the elements of the main subgroups increase, decrease in periods, and non-metallic properties, respectively, on the contrary, decrease in the main subgroups, and increase in periods. redox properties

14 slide