CHEMISTRY TEACHER

Efremova S.A.

Slide 2

  • 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.

Slide 3

  • 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

Slide 4

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

Slide 5

  • Interaction of metals with halogens

2Na + Cl2 → 2NaCl

2Sb + 2Cl2 → 2SbCl3

2Sb + 5Cl2 → 2SbCl5

2Fe + 3Cl2 → 2FeCl3

Table 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)

Slide 6

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↓

Slide 7

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

Slide 8

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↓

Slide 9

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 environment inhibitors are introduced.
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

  • Slide 10

    • 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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    Prepared by a 1st year student

    Groups Mts-15

    Nikolaenko Daria


    This is a group of elements, in the form of simple substances, with characteristic metallic properties, such as high thermal and electrical conductivity, positive temperature coefficient of resistance, high ductility, malleability and metallic luster.

    Metals are one of the most common materials used by civilization throughout almost its entire history.


    Of the 118 chemical elements discovered in at the moment(not all of them are officially recognized), metals include:

    6 elements in the alkali metal group:


    4 in the group of alkaline earth metals:

    and also outside certain groups


    Rest

    40 in the transition metal group:

    • - Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn;
    • - Y, Zr, Nb, Mo, Tc, Ru, Rh, Pd, Ag, Cd;
    • - La, Hf, Ta, W, Re, Os, Ir, Pt, Au, Hg;
    • - Ac, Rf, Db, Sg, Bh, Hs, Mt, Ds, Rg, Cn;

    7 in the group of light metals: Al, Ga, In, Sn, Tl, Pb, Bi

    7 in the group of semimetals: B, Si, Ge, As, Sb, Te, Po

    14 in the group lanthanides + lanthanum (La):

    Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu

    14 in the group actinides (physical properties have not been studied for all elements) + actinium (Ac):

    Th, Pa, U, Np, Pu, Am, Cm, Bk, Cf, Es, Fm, Md, No, Lr.


    Being in nature

    • Most metals are present in nature in the form of ores and compounds. They form oxides, sulfides, carbonates and other chemical compounds. To obtain pure metals and their further use, it is necessary to isolate them from ores and carry out purification. If necessary, alloying and other processing of metals is carried out. The science of metallurgy studies this. Metallurgy distinguishes ores of ferrous metals (based on iron) and non-ferrous (they do not contain iron, there are about 70 elements in total). Gold, silver and platinum are also precious (noble) metals. In addition, they are present in small quantities in sea water and in living organisms (playing an important role).
    • It is known that the human body consists of 3% metals. The body contains most calcium (in the bones) and sodium, which acts as an electrolyte in the intercellular fluid and cytoplasm. Magnesium accumulates in muscles and nervous system, copper - in the liver, iron - in the blood.

    History of the development of ideas about metals

    • Man's acquaintance with metals began with gold, silver and copper, that is, with metals found in a free state on the earth's surface; subsequently they were joined by metals that are widely distributed in nature and are easily isolated from their compounds: tin, lead, iron and mercury. These seven metals were familiar to mankind in ancient times. Among the ancient Egyptian artifacts there are gold and copper products, which, according to some data, belong to an era removed by 3000-4000 years from AD. e.

    Physical properties metals

    • All metals (except mercury and, conditionally, France) at normal conditions are in a solid state, but have different hardness. The table below shows the hardness of some metals on the Mohs scale.
    • All metals conduct electricity well; this is due to the presence in their crystal lattices of mobile electrons moving under the influence electric field. Silver, copper and aluminum have the highest electrical conductivity; for this reason, the latter two metals are most often used as wire materials.
    • The lowest thermal conductivity is found in bismuth and mercury.
    • The color of most metals is approximately the same - light gray with a bluish tint. Gold, copper and cesium are respectively yellow, red and light yellow.

    Chemical properties of metals

    At the external electronic level, most metals have a small number of electrons (1-3), so in most reactions they act as reducing agents (that is, they “donate” their electrons)

    Alloying

    This is an introduction to melt additional elements, modifying the mechanical, physical and chemical properties of the base material.


    Electronic structure

    • For a more correct description of the electronic properties of metals, it is necessary to use quantum mechanics. In all solids with sufficient symmetry, the energy levels of the electrons of individual atoms overlap and form allowed bands, and the band formed by valence electrons is called the valence band. The weak connection of valence electrons in metals leads to the fact that the valence band in metals is very wide, and all the valence electrons are not enough to completely fill it.
    • The fundamental feature of such a partially filled zone is that even at a minimum applied voltage, a rearrangement of valence electrons begins in the sample, that is, an electric current flows.
    • The same high mobility of electrons leads to high thermal conductivity, as well as the ability to specularly reflect electromagnetic radiation (which gives metals their characteristic shine).

    Metal

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    Position of metals in P.S. The largest typical elements are metals placed on the beginning of periods (starting from 2). Thus, out of 113 elements, 85 are metals. Periodic system D. I. Mendelev. Budova of metal atoms. Budova atoms. Physical power. Silver and copper have the highest electrical conductivity. Electric flow is the process of directing the flow of charging particles. Chemical power. Zagalny chemical power. The most active ones were to react with simple substances (non-metals): halogens and acids. Ca - daily. Mg - daily. Na - day-to-day. 4) Metals, hydroxides and amphotenes, usually interact with acids and compounds. - Metal.ppt

    Metal elements

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    Copper, Bronze, Iron Age. Sodium. Natrium), a soft alkali metal silver- white. For example, soda (natron), found naturally in the waters of soda lakes in Egypt. Tin. Tin (lat. Tin was known to man already in the 4th millennium BC. Iron. Ferrum), one of the most common metals in the earth’s crust. Gold. Gold is the 79th element of the periodic table of elements, a noble metal of yellow color. Pure gold is a soft yellow metal. In thin films, gold shows through green. Gold has exceptionally high thermal conductivity and low electrical resistance. - Metals.ppt

    Metal world

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    Metals lesson

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    Integration of chemistry with other subjects. Organization and conduct of integrated lessons. TO international day water. Interesting facts about water. Geography. Chemistry. Physics. Biology. "City Ecology". Integrated lesson "Metals". Integrated lesson in chemistry, geography, biology. Metals in nature. The most common metal on Earth is aluminum (more than 8% of the earth's crust). Metals. Black 90%. Colored 10%. Iron, steel, cast iron. Methods for obtaining metals. 3. Electrometallurgy is a method of producing metal using electric current(electrolysis). Metallurgical bases of Russia. - Lesson Metals.ppt

    City of Metal

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    Journey through the city of metals. Travel plan. Preliminary task. Institute for Nuclear Research. Physical street. Geological Lane. Dead end of the Red Devil. Name the methods of protection against corrosion. Which iron product will last longer: galvanized or tinned. Chemical embankment. Oxidation-reduction prospectus. Metallurgical station. River of Transformations. Mathematical park. Theater Illusion. Palace of the Wise. Write down the reaction equations in short ionic form. Reaction equations. - City of Metal.ppt

    Chemistry metals

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    Position of metals in the Periodic Table Structure of atoms Crystal lattices General physical properties Metals in nature Methods of obtaining metals Chemical properties of metals. Metals include simple substances that form: Me – ne- Men+. All solids except mercury Metallic luster Plasticity, malleability Electrical conductivity Thermal conductivity High melting points. The most common metal in nature is aluminum - more than 8% of the earth's crust. Reducing agents: Obtaining metals by electrolysis: Obtaining metals by reduction from salt solutions: Metals are reducing agents. - Chemistry Metals.ppt

    Metals in chemistry

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    Metals. Characteristic properties of metals. Metallic luster (except for iodine. Despite its metallic luster, crystalline iodine is a non-metal). Physical properties of metals. All metals (except mercury) are solid under normal conditions. Melting points range from -39 °C (mercury) to 3410 °C (tungsten). Mechanical properties of metals. Soldering Turning Drilling Sawing Planing Machining, etc. General chemical properties of metals. Electrochemical voltage series of metals: Interaction with simple non-metal substances. 1. With oxygen 2. With halogens 3. With hydrogen 4. With sulfur 5. With nitrogen. - Metals in chemistry.ppt

    9th grade metals

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    Metals. Metals Black non-ferrous noble Alkaline alkaline earth. Metal crystal lattice. A metal atom is a metal cation, an electron that moves freely. THE MOST, THE MOST, THE MOST. . . The shiniest metal... ? The hardest metal... ? The most refractory metal... ? The most fusible metal... ? The most ductile metal... ? The most electrically conductive metal... ? The heaviest metal... ? The lightest metal...? Liquid metal... ? Noble metal... ? One of the main metals...? - 9th grade Metals.ppt

    Metals concept

    Slides: 24 Words: 743 Sounds: 1 Effects: 105

    Inorganic chemistry. Metals. Basic concepts. Main characteristic. Which of these elements is redundant? Which of these metals does not react with water. Guess what natural compound we are talking about. Gypsum. Write an equation for the reaction. With which of these salts will zinc not react? Find all metals. Sodium oxide. Characteristic. Sodium hydroxide. Insert missing concepts. Find the third extra substance. Find matches. Find the picture. Answer the questions. Feldspars. What characteristics are suitable for aluminum. Write down reaction equations. Solve the problem. - Concept of metals.ppt

    Chemistry theme Metals

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    The topic of the educational project: “Metals”. "Metals in the service of man." Fundamental question: Academic subjects: chemistry, biology, geography. Project participants: 9th grade students. as a result develops critical thinking, Project abstract: Topics of independent research: Stages and timing: - Chemistry topic Metals.ppt

    Metal Features

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    Systematize and deepen knowledge about elements - metals. Develop a concept about the structure of simple substances. General characteristics of metals. Definitions. Iron easily oxidizes in air and becomes rusty. The structure of atoms. Position in the periodic table. Typical metals: S-elements (1-2? at the external E level) D-elements (1-2? at the external E level) P-elements - less often. A small number of electrons in the outer energy level. Ме0 + Еi Ме+n + n? Еi – ionization energy М0 – n? Ме+n oxidation process Metal is a reducing agent. The chemical bond is metallic. Chem. properties. Phys. properties. - Features of metal.ppt

    Characteristics of metals

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    Metals. General characteristics of metals. Variety of metals. Properties of metals. Finding metals in nature. The use of metals in human life. Contents of the work: Metals include approximately 70% of all chemical elements. General characteristics. Metallic shine. Good electrical conductivity. Many metals are widely distributed in nature. Large quantity sodium and magnesium contained in sea water: - 1.05%, - 0.12%. From medicinal products containing noble metals, the most common are lapis, protargol, etc. Iron. Metals form one of the foundations of civilization on planet Earth. - Characteristics of metals.ppt

    "Metals" chemistry grade 10

    Slides: 18 Words: 588 Sounds: 0 Effects: 50

    Metals. What are metals? The role of metals in the development of civilization. Copper. Sometimes small nuggets of copper fell into the hearth and softened in the fire. Then people learned to smelt copper from ore. Molten copper was poured into a mold and a copper product of the desired type was obtained. Bronze. The first people from the ancient world to smelt bronze were the Egyptians. Iron. An iron blade was discovered in the tomb of Tutankhamun. Being in nature. The pattern of changes in the properties of metals in a group. The nuclear charge increases as the atomic number increases. R increases as the number of energy levels. - “Metals” chemistry grade 10.ppt

    General characteristics of metals

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    The amazing world of metals. Kaleidoscope. Operating with knowledge. Students' knowledge of chemistry. Level of knowledge mastery. Thinking mind. Story. Physics. Chemistry. Biology. - General characteristics of metals.ppt

    Metals and electrons

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    Metals. Plan: Metals in the service of humanity. Metals in nature. Questions to reinforce the material. Light created seven metals according to the number of seven planets. N.A. Morozov. Cu. Fe. Ag. Au. Sn. Pb. Hg. The most common metal on Earth is aluminum (more than 8% of the earth's crust). Methods for obtaining metals. 3. Electrometallurgy - a method of producing metal using electric current (electrolysis). The position of metals in D.I. Mendeleev’s psche, structural features. Metals in PS make up 80% of all elements. Features of some metals. Ag pt - the most brilliant. Ag cu au al are the best guides. - Structure.ppt

    Metal composition

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    Alkaline earth metals. Light gray, refractory. A unique combination of hardness and lightness. Pure is plastic. Highly toxic. Covered with an oxide film. The opposite of beryllium. Soft and flexible. Melts at lower temperatures. Covered with an oxide film. Lightweight malleable metal of silver-white color. Malleable, silver-white metal. A soft, slightly ductile metal with a silvery-white color. Radioactive shiny metal of silvery-white color. Beryllium minerals. Emerald in Rus' was considered a stone of wisdom, bringing happiness and joy. Aquamarine has positive energy and improves mood. - Metal composition.ppt

    Structure of metal atoms

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    Structure of metal atoms. Metals are elements whose atoms have weak bonds. Filling with electrons. Find matches. Make up electronic formulas. How will the process of iron corrosion change? Chemical properties of metals. Give two examples of reaction equations. Sodium tetrahydroxozincate. Arrange the coefficients using the electronic balance method. 4Zn0 + 5H2S+6O4 = 4Zn+2SO4 + H2S-2+4H2O Zn0 – 2e Zn+2 4 S+6 + 8e S-2. - Structure of metal atoms.ppt

    Metal Age

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    I am hard, malleable and plastic, brilliant, needed by everyone, practical. I already gave you a hint, so who am I?...... metal. “Man cannot do without metals... Without metals the level of earthly civilization is unthinkable. Country of metals. Al. Cr. Na. K. Fe. Welcome. CLUSTER (English Cluster. Me. Occurrence in nature. Biological role. Chemical properties. Physical properties. Application. History of metals. Preparation. Position in PSCEM. Structure of the atom. Stone Age. At the end of the Stone Age, the use of pottery. Stone tools were made from various types stone - Age of Metals.ppt

    History of metals

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    Presentation on 9th grade chemistry. Topic: history of civilizations - history of metals. Talk about the discovery of metals. Perhaps the discovery of metals had no impact on the development of civilizations. Copper. Sometimes small nuggets of copper fell into the fireplace and softened in the fire. Then people learned to smelt copper from ore. Molten copper was poured into a mold and a copper product of the desired type was obtained. Bronze. The first people from the ancient world to smelt bronze were the Egyptians. Iron. An iron blade was discovered in the tomb of Tutankhamun. History of aluminum. One day a stranger came to the Roman Emperor Tiberius. - History of metals.ppt

    Antiquity metals

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    Copper, Bronze, Iron Age

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    Copper, Bronze, Iron Age. Iron Age. The period of distribution of copper tools. Only small tools were made from copper. Casting. Bronze. Bronze is used to make sculptures. Third and final period primitive era. The first iron. Iron alloys. Position of metals in the Periodic Table. - Copper, Bronze, Iron Age.ppt

    Stone, copper, bronze, iron age

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    Copper, Bronze, Iron Age. History clock. Stone Age. Stone tools. Copper. Copper products. Native copper. The largest copper nugget ever found. Bronze. Colossus of Rhodes. The king is a cannon. The king is a bell. Bronze Horseman. Meteoric iron. The history of iron goes back 4 – 4.5 thousand years. Iron. The Bronze Age gave way to the Iron Age. Cast iron. Steel. The use of iron made it possible to dramatically increase the area under cultivation. Products containing steel. Gold. Silver. - Stone, copper, bronze, iron ages.ppt

    Test "Metals"

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    Materials Science. Choose a topic. Cast iron. Steel. White cast iron. Cat in a poke. Hardness of cast iron. With increasing carbon content, the hardness of cast iron increases. The hardness of cast iron increases. Specify the grade of cast iron. Tensile strength. High strength cast iron. Is it possible to forge a horseshoe from malleable cast iron, for example, KCh 60-3? Cast iron cannot be forged. You cannot forge a horseshoe. Name the grade of steel. Steel grade U13. 1.3% carbon. Name the grade of carbon tool steel. Grade of carbon tool steel. Brand. Name the grade of alloy structural steel. Grade of alloy structural steel. -

    Boldyreva Anastasia

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    Slide captions:

    Metals MOU “Kirishi average” 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 nuclear charge 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 metal 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 that are in the voltage series up to “H”) Zn + H 2 SO 4 = Zn S O 4 + H 2 With solutions of metal salts that are 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

    Production of 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