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Slide text: Metals

Slide text: substances Simple Complex Composed of atoms of the same type Composed of atoms of different types

Slide text: Simple substances metals non-metals Chemical elements that form simple substances with a metal bond in a free state. Chemical elements that form substances in a free state that do not have the physical and chemical properties of metals.

Slide text: Ancient and Middle Ages – 7 metals (Au, Ag, Cu, Pb, Fe, Hg) M.V. Lomonosov - metals “a light body that can be forged” A. Lavoisier - 1789 - described 17 metals by D.I. Mendeleev - prediction of metals 19th century - discovery of platinum, alkali, alkaline earth metals. XX – discovery of transuranium elements.

Slide text: Occurrence of metals in nature In the form of compounds In the native state (Au, Pt, Ag) In the form of salts (halides, carbonates, nitrates, phosphates) In the form of oxides and sulfides

Slide text: Metals have a metallic crystal lattice. e e e e Relatively small number of electrons in the outer energy level Li 2е 1е

Slide text: They have free valence electrons. The metal bond does not have directionality or saturation. Mobile electrons compensate for the electrical repulsion between positively charged ions and thereby bind them into solids

Slide text: Physical properties of metals Solids, except mercury. (the softest is potassium, the hardest is chromium)

Slide text: Ductile Au, Ag, Cu, Sn, Pb,Zn, Fe decreases

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Slide text: Thermal conductivity of Hg, Cu, Ag, Al, Fe decreases Electrical conductivity of Ag Mn decreases

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Slide text: Melting point Low-melting refractory Hg, Ga, Cs, In, Bi W, Mo, V, Cr

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Slide text: density light heavy (Li is the lightest, (osmium is the heaviest, K, Na, Mg) Ir, Pb)

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Slide text: Have a metallic luster

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Slide text: Reasons leading to differences in the physical properties of metals Metal atoms form different types of crystal lattices

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Slide text: Reasons leading to differences in physical properties Metal atoms have different numbers of valence electrons involved in the formation of a metallic bond Atoms (ions) have different radii Metal atoms of side subgroups can also form a covalent bond with the help of unpaired d-electrons.

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Slide text: position of metals in the periodic table of D. I. Mendeleev

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Slide text: Mysterious neighbors Alkaline earth metals Transition metals Alkali metals

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Slide text: Chemical properties of metals Metals in chemical reactions are reducing agents, and they are oxidized Mo – ne = Mn+ Al, Be, Mg, Ca, Li, Na, K, Rb, Cs The reducing ability increases

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Slide text: Metals are displaced from their compounds by other metals N.N. Beketov - created a “displacement series” (prototype of the electrochemical voltage series of metals) Li, K, Ca, Na, Mg, Al, Mn, Zn, Cr, Fe, Ni, Sn, Pb, (H), Cu, Hg, Ag, Pt, Au. Slide text: Application of metals Metallurgical industry Machine tool industry Medicine Agriculture For the production of alloys Household

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Slide text: Production of metals by pyrometallurgical method - reduction with carbon, carbon monoxide (II), hydrogen at high temperature. Aluminothermic method Hydrometallurgical method - obtaining a more active metal from ore or from solutions Electrolysis - using electric current from melts or solutions

Presentation for a chemistry lesson on the topic “Metals”, grade 11. UMK Gabrielyan O.S. Basic level Municipal educational institution "Volokolamsk secondary school 2 of Volokolamsk, Moscow region Author Kolyadkina Irina Viktorovna, chemistry teacher

Ar Argon 1818 KrKr Krypton 36 Xe Xenon 54 Groups of elements IIIIIIIVVVIVIIVIII Na Sodium 11 MgMg Magnesium 12 Al Aluminum 1313 Cl Chlorine 1717 Si Silicon 14 P Phosphorus 15 S Sulfur 17 K Potassium 19 CaCa Calcium 20 H Hydrogen 1 He Helium 2 Li Lithium 3 B e Beryllium 4 F Fluorine 9 O Oxygen 8 N Nitrogen 7 C Carbon 6 B Boron 5 NеNе Neon 10 Scandium Sc 21 Titanium Ti 22 Vanadium V 2323 Chromium Cr 2424 Manganese 2525 MnMn Iron 2626 Fe Cobalt 2727 Co Nickel 2828 Ni Zinc 30 Zn Copper 2929 C uСuGe Germany 32 Ga Gallium 31 Br Bromine 35 Se Selenium 34 As Arsenic 33 Sr Strontium 38 Rb Rubidium 37 Y 39 Yttrium Ruthenium 44 Ru Rhodium 45 Rh Palladium 46 Pd Technetium 43 Tc Molybdenum 42 Mo Niobium 41 Nb Zirconium 40 Zr Cadmium 48 CdCd 47 AgIn Indium A uАu TITI Thallium 81 Rho Polonium 84 BiBi Bismuth 83 Pb Lead 82 At 85 Astatine Rn Radon 86 RaRa Radium 88 Fr Francium 87 Ac 89 Actinium ** Bohrium 107 Bh Seaborgium 106 Sg Rutherfordium 104 Rf Dubnium 105 Db Hassium 108 Hs Meitnerium 109 MtMt Peri - odes RO 4 RH R2O7R2O7 RO 3 RH 2 R2O5R2O5 RH 3 RO 2 RH 4 R2O3R2O3 ROR2OR2O Higher oxides of LVS

Metal atoms have a small number of electrons in the outer electron layer - Metal atoms give up valence electrons, turning into cations - Metal atoms are connected to each other by a metal bond - Metal atoms connected to each other by a metal bond form simple substances with a metal crystal lattice M 0 ne M n+ atom cation We know that...

Metal connection

Metal connection

Metal connection

Metal connection

Hardness From the strength of the metal bond (the number of electrons involved in the formation of the bond) W, Cr Melting point From the strength of the metal bond (the number of electrons involved in the formation of the bond) Low-melting: Cs, Na, Sn High-melting: Cu, Fe, W Physical properties of metals Than are the properties determined? Which metals have the most pronounced

Chemical properties of metals Me not Me H2OH2O Metal oxides Acids Cl 2 0 + Na 0 O 2 + Al H 2 O + Na Al + Fe 2 O 3 + ? 2Na + Cl 2 2 NaCl ?? 4Al + 3O 2 2Al 2 O 3 ? 2Na+2H 2 O2NaOH+H 2 Al + Fe 2 O 3 Al 2 O 3 + Fe Salts O2O2 Zn+HCl Fe+CuCl 2 more details?? Zn + HCL ZnCl 2 + H 2 Fe + CuCl 2 FeCl 2 + Cu

When interacting with oxygen, metals can form products of various compositions: oxides (basic and amphoteric), as well as peroxides: For example, 2Na + O 2 = Na 2 O 2 (sodium peroxide) Features of chemical reactions of metals: Interaction of metals with water, if the metal – alkaline, alkaline earth or aluminum: M + H 2 O M(OH) n + H 2 Interaction of metals with water, if the metal is in the electrochemical voltage series from manganese to lead (incl.): t M + H 2 O M x O y + H 2 Interaction of metals with water, if the metal is in the electrochemical voltage series after hydrogen: M + H 2 O

1) The metal must be in the electrochemical voltage series to the left of hydrogen. Interaction of metals with acids M + H m Ac M x Ac y + H 2 2) It is not recommended to use alkali metals for reactions, because they first react with water. 3) As a result of the reaction, a soluble salt should be formed, because otherwise, it will cover the metal with sediment and the acid will stop accessing the metal. 4) Nitric and concentrated sulfuric acids interact with metals in a special way.

1) The metal must be in the electrochemical voltage series to the left of the metal forming the salt. Interaction of metals with salt solutions M + M / x Ac y M x Ac y + M / 2) It is not recommended to use alkali metals for reactions, because they first react with water. 3) As a result of the reaction, a soluble salt should be formed, because otherwise, it will cover the metal with sediment and the access of the salt solution to the metal will stop.

General methods of obtaining metals - Pyrometallurgy - production of metals and alloys under the influence of high temperatures. - Hydrometallurgy – obtaining metals from aqueous solutions. - Electrometallurgy – production of metals under the influence of electric current.

General methods for obtaining metals Hydrometallurgy Stage 1: dissolution of insoluble minerals containing metals in acid: CuS + 2HCl = CuCl 2 + H 2 S Stage 2: displacement of metals from solutions of their salts by more active metals: CuCl 2 + Fe = FeCl 2 + Cu

Chemical Electrochemical 4Fe + 6H 2 O + 3O 2 = 4Fe(OH) 3 Corrosion of iron and rust formation Corrosion of iron in contact with copper and in a solution of hydrochloric acid: Cathode 2H e = H 2 Anode Fe e = Fe 0 Corrosion of metals Spontaneous destruction of metal materials that occur under the influence of the environment is called corrosion.

List of used literature 1. O.S. Gabrielyan. Textbook for general education institutions. CHEMISTRY. A basic level of. Grade 11. – M.: Bustard, O. S. Gabrielyan, A. V. Yashukova. Chemistry. Grade 11. A basic level of. Toolkit. – M.: Bustard, O. S. Gabrielyan, I. G. Ostroumov. Chemistry 11th grade: teacher's handbook. – M.: Bustard, 2005 Internet resources used

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What you will learn (topic study plan) Physical properties of metals. Chemical properties of metals. Metals in our life. Metal connection. Corrosion of metals Methods of obtaining metals. Electrolysis. Application of metals and alloys. Properties of basic oxides and bases.

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General physical properties of metals Plasticity - the ability to change its shape upon impact, to be rolled into thin sheets, to be drawn into wire. Electrical conductivity - when heated, it decreases (vibrations of ions. Physical properties are explained by the special structure of the crystal lattice (free electrons - “electron gas”), the movement of electrons is hampered) Thermal conductivity - the pattern is the same. Due to the movement of free electrons, rapid equalization of temperature in the metal mass. Metallic luster - reflects light rays well. Density - the lightest lithium, the heaviest - osmium Melting point, C - cesium (28.6), gallium (30) - melts in the palm of the hand, tungsten (3410) Hardness - the hardest - chromium (cuts glass), the softest - potassium, rubidium, cesium (easily cut with a knife).

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General chemical properties of metals Strong reducing agents With simple substances With oxygen (oxides, peroxides, superoxides) With halogens (fluorides, chlorides, bromides, iodides) With nitrogen (nitrides) With phosphorus (phosphides) With hydrogen (hydrides) With complex substances With acids: ME + acid = salt + hydrogen (do not take nitric and sulfuric acids, metals after hydrogen in the series of metal voltages) 2. With water a) active metals - hydroxides and hydrogen b) medium active metals - oxides and hydrogen (when heated) c) inactive metals - do not react 3. With salts - a more active metal displaces a less active one from its salt

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Electrolysis Electrolysis is the redox process that occurs at the electrodes when a direct electric current passes through solutions or melts of electrolytes. On a negatively charged electrode - cathode, electrochemical reduction of particles (atoms, molecules, cations) occurs, and on a positively charged electrode - anode, electrochemical oxidation of particles (atoms, molecules, anions) occurs.

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Corrosion of metals The destruction of metals and alloys under the influence of the environment is called corrosion. Corrosion can be chemical (the interaction of metals with dry gases) and electrochemical (all cases of corrosion in the presence of water or electrolyte). The essence of corrosion Along with chemical processes (electron release), electrical processes (electron transfer) also occur. Of the two metals, the more active one corrodes. The further the metals are from each other in the electrochemical series of metal voltages, the greater the corrosion rate.

Boldyreva Anastasia

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Metals Municipal Educational Institution “Kirishi Secondary School No. 8” Completed by: 9b grade student A. Boldyreva Supervisor: chemistry teacher L.N. Babkina, Kirishi, 2007

Metals are chemical elements that, in a free state, form simple substances with metallic bonds. M.V. Lomonosov - metals “a light body that can be forged” What are metals Ba Cr K Li

The role of metals in human life and society. In ancient times, only 7 metals were known to man: Gold (Au), Silver (Ag), Copper (Cu), Tin (Sn), Lead (Pb), Iron (Fe) and Mercury (Hg). First, man became acquainted with metals that are found in native form - gold, silver and copper. The rest of the metals appeared after man learned to extract them from ores using fire. Stone Age → Copper Age → Bronze Age → Iron Age.

Coins were minted from silver, gold and copper. 1. Silver coin with the image of the goddess Athena and an owl. 2. Gold coin with the image of Alexander the Great and the god Zeus. 3. Copper coin in the shape of a dolphin. Monuments and statues are made from metals and their alloys. Tsar Cannon (bronze) Tsar Bell (bronze) Statue of the Colossus of Rhodes (Bronze)

The material from which the Cheops pyramid is built is made of stone and copper.

Being in nature

Most chemicals are metals. The boundary between metals and non-metals is conditional. B Si Nonmetals As Those Metals At

Metals Transition element Nonmetals Basic Amphoteric Acid oxide oxide oxide Base Amphoteric Acid hydroxide Na Al S Na 2 O Al 2 O 3 SO 3 NaOH Al(OH) 3 H 2 SO 4

The pattern of changes in the properties of metals in a group. The charge of the nucleus increases as the serial number increases. R increases as the number of energy levels increases. The number of electrons in the last level is constant. The ability to donate electrons increases. Reducing abilities and metallic properties are increased.

The pattern of changes in the properties of metals in a period. The charge of the nucleus increases as the serial number increases. R decreases, since the charge of the nucleus is greater, the ability to attract electrons increases, due to this the electron shells are contracted. The number of electrons in the outer level increases as the group number increases. Reducing abilities and non-metallic properties are reduced.

Physical properties of metals. All metals have common physical properties, since in all metals there is a metallic chemical bond and a metallic crystal lattice.

All metals are solids except mercury. the softest is potassium, the hardest is chromium

Ductile Au, Ag, Cu, Sn, Pb, Zn, Fe decreases

Melting point Low-melting Refractory Hg, Ga, Cs, In, Bi W, Mo, V, Cr

Density Light Heavy (Li – the lightest, (osmium – the most K, Na, Mg) heaviest Ir, Pb)

Have a metallic sheen

Alkali metals Transition metals Alkaline earth metals By chemical activity

Chemical properties of metals Metals in chemical reactions are reducing agents, and they are oxidized M o – ne =M n+ Al, Be, Mg, Ca, Li, Na, K, Rb, Cs The reducing ability increases

Metals are displaced from their compounds by other metals N.N. Beketov - created a “displacement series” (prototype of the electrochemical voltage series of metals) Li, K, Ca, Na, Mg, Al, Mn, Zn, Cr, Fe, Ni, Sn, Pb, (H), Cu, Hg, Ag, Pt, Au.

Interact with simple substances With elements of group VII (under normal conditions) 2Na + Cl 2 = 2 Na Cl - With elements of group VI (more difficult) Mg + O 2 = 2Mg O With elements of group V (under harsh conditions) 3Ca + 2P = Ca 3 P2

Interaction with complex substances With solutions of acids (metals in the voltage series up to “H”) Zn + H 2 SO 4 = Zn S O 4 + H 2 With solutions of metal salts in the voltage series to the right Zn + Pb(NO 3) 2 = Zn(NO 3) 2 + Pb C water (active) 2Na + 2H 2 O = 2Na OH + H 2 The reaction occurs if a soluble base is formed.

Application of metals Machine tool construction medicine Agriculture production of alloys In everyday life Metallurgical industry

Obtaining metals Pyrometallurgical method - reduction with carbon, carbon monoxide (II), hydrogen at high temperature. Aluminothermic method is the reduction of metals using aluminum. Hydrometallurgical method - obtaining a more active metal from ore or from solutions Electrolysis - using electric current from melts or solutions

CHEMISTRY TEACHER

Efremova S.A.

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• Metals (from Latin metallum – mine, mine):

a group of elements with characteristic metallic properties, such as high electrical and thermal conductivity, positive temperature coefficient of resistance, high ductility and metallic luster.

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• Chemical properties of metals
• All metals exhibit only reducing properties
• Metal atoms easily give up electrons from the outer (and some from the outer) electron layer, turning into positive ions.
• Metals have a large atomic radius and a small number of electrons (from 1 to 3) in the outer layer.
• Exception:

Ge, Sn, Pb ─ 4 electrons;

Sb, Bi ─ 5 electrons;

Po ─ 6 electrons

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Interaction of metals with oxygen

• Active metals

4Li + O2 → 2Li2O

2Na + O2 → Na2O2

Na2O2 + O2 → 2Na2O

2Na2O2 + 2CO2 = 2Na2CO3 + O2

(In submarines it regenerates O2)

• Low-active metals

4Al + O2 → 2Al2O3

3Fe + 2O2 = Fe3O4

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• Interaction of metals with halogens

2Na + Cl2 → 2NaCl

2Sb + 2Cl2 → 2SbCl3

2Sb + 5Cl2 → 2SbCl5

2Fe + 3Cl2 → 2FeCl3

Salt

• Interaction of metals with sulfur

2Al + 3S → Al2S3

• Interaction of metals with water

2Me + 2H2O = 2MeOH + H2

(Alkali and alkaline earth metals)

3Fe + 4H2O → Fe3O4 + 4H2

(low-active)

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Zn + 2HCl → ZnCl2 + H2

• Interaction of metals with acids

Zn + 2H → Zn + H2

2CH3COOH + Zn → (CH3COO)2Zn + H2

Zn + 2H → Zn + H2

2C2H5OH + 2Na → 2C2H5ONa + H2

2C6H5OH + 2Na → 2C6H5ONa + H2

• Interaction of metals with salts

Fe + CuSO4 → Cu↓ +FeSO4

Fe + Cu → Cu + Fe

(redox reaction)

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag↓

Cu + 2Ag → Cu + Ag↓

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Metallothermy

• Some active metals - lithium, magnesium, calcium, aluminum - are capable of displacing other metals from their oxides. This property is used to obtain certain metals, as well as to prepare thermite mixtures.

2Al + Cr2O3 = Al2O3 + 2Cr

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Metal corrosion

• Spontaneous destruction of metals and alloys under the influence of the environment.
• (from Latin corrosio - to corrode)
• Electrochemical corrosion
• Destruction of metal under the influence of galvanic elements arising in a corrosive environment

Fe – 2e → Fe

Fe + 2H → Fe + H2

(on hardware)

Chemical corrosion

• Interaction of a metal surface with a corrosive environment, not accompanied by the occurrence of electrochemical processes at the phase boundary

4Fe + 3O2 + 6H2O = 4Fe(OH)3↓

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Corrosion protection
Depending on the causes of corrosion, the following protection methods are distinguished:
Protective coatings. To isolate the metal from the environment, various types of coatings are applied to it: varnishes, paints, enamels.
Treatment of the external environment in which corrosion occurs. To slow down the corrosion process as much as possible, inhibitors are introduced into the environment.
Electrochemical protection – sacrificial and cathodic. Protective – a product protected from corrosion is connected to scrap metal made of a more electronegative metal (protective). Cathode - the protected structure, located in the electrolyte (soil water), is connected to the cathode of an external current source.
Coating with a layer of another metal (Au, Ag, Cr, Ni, Zn. Sn- or Pb-tinning).
Use of stainless alloys (chrome, nickel, titanium).
(Fe +H2SO4– add HNO3)
Monument to Yu.A. Gagarin in Moscow, made of titanium

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• We must not allow people to direct to their own destruction those forces of nature that they were able to discover and conquer.

F. Joliot-Curie

• The benefits and harms of metals for humans
  • Cadmium - accumulating in the kidneys, leads to hypertension, decreased immunity, and dementia. Contained in tobacco smoke, drinking water, polluted air
  • Aluminum – senile dementia, impaired vasomotor reactions, anemia, kidney and liver disease. Food foil, dishes, beer cans.
  • Lead - impaired brain activity, cancer, impaired fertility in women. Polluted air - car exhaust gases
  • Calcium is the basis of structural bone tissue in the human body. The most essential mineral for humans.
  • Copper - plays an important role in providing immune protection, including anti-radiation and anti-cancer, participates in energy metabolism and hematopoiesis, in the formation of the protective skin pigment melanin
  • Iron - necessary for life, for the formation of hemoglobin (red blood cells), myoglobin (red pigment in muscles) and some enzymes

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