Presentation on chemistry "fields of application of metals". Metals general properties and obtaining Presentation on the topic of the name of metals
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 at the moment (of which not all are officially recognized), metals include:
6 elements in the alkali metal group:
4 in the group of alkaline earth metals:
as well as 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 lanthanide + lanthanum (La) group:
Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu
14 in the group of 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 of the 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 separate them from ores and carry out purification. If necessary, alloying and other processing of metals is carried out. The study of this is the science of metallurgy. Metallurgy distinguishes between ferrous metal ores (based on iron) and non-ferrous ores (iron is not included in their composition, only about 70 elements). Gold, silver and platinum are also precious (noble) metals. Moreover, they are present in small amounts in sea water and in living organisms (while playing an important role).
- It is known that 3% of the human body consists of metals. Most of all in the body of calcium (in the bones) and sodium, which acts as an electrolyte in the intercellular fluid and cytoplasm. Magnesium is stored in muscles and nervous system, copper - in the liver, iron - in the blood.
The 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 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 items, which, according to some sources, belong to an era removed by 3000-4000 years from BC. e.
Physical properties metals
- All metals (except mercury and, conditionally, France) are in a solid state under normal conditions, but they 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 action of an electric field. Silver, copper and aluminum have the highest electrical conductivity; for this reason, the last two metals are most often used as a material for wires.
- Bismuth and mercury have the lowest thermal conductivity.
- The color of most metals is approximately the same - light gray with a bluish tint. Gold, copper and cesium, respectively, yellow, red and light yellow color.
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 “give away” their electrons)
alloying
This is the introduction of additional elements into the melt that modify 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 bond of valence electrons in metals leads to the fact that the valence band in metals turns out to be very wide, and all valence electrons are not enough to completely fill it.
- The fundamental feature of such a partially filled zone is that even at the minimum applied voltage, the rearrangement of valence electrons begins in the sample, i.e., electric current flows.
- The same high mobility of electrons leads to high thermal conductivity, as well as to the ability to mirror electromagnetic radiation (which gives metals a characteristic luster).
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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 for 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, roll into thin sheets, stretch into a wire. Electrical conductivity - decreases when heated (oscillation of ions. Physical properties are explained by the special structure of the crystal lattice (free electrons - "electronic gas"), the movement of electrons is hindered) Thermal conductivity - the same pattern. Due to the movement of free electrons, the temperature quickly equalizes in the mass of the metal. Metallic luster - light rays are well reflected. Density - the lightest lithium, the heaviest - osmium Melting point, C - cesium (28.6), gallium (30) - melt in the palm of your 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 \u003d 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) metals of medium activity - 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 a redox process that occurs on electrodes when a direct electric current passes through solutions or melts of electrolytes. Electrochemical reduction of particles (atoms, molecules, cations) occurs on a negatively charged electrode - cathode, and electrochemical oxidation of particles (atoms, molecules, anions) occurs on a positively charged electrode - anode.
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Corrosion of metals The destruction of metals and alloys under the influence of environment called corrosion. Corrosion is 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 corrodes. The corrosion rate is the greater, the farther the metals are from each other in the electrochemical series of metal voltages.
Metal
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metal elements
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Characteristics of metals
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The structure of metal atoms
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Slides: 13 Words: 391 Sounds: 0 Effects: 30Presentation on chemistry grade 9. Topic: the history of civilizations - the history of metals. Describe the discovery of metals. Perhaps the discovery of metals did not affect the development of civilizations in any way. Copper. Sometimes small nuggets of copper fell into the hearth, which 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 who smelted bronze were the Egyptians. Iron. An iron blade was found in Tutankhamun's tomb. History of aluminum. One day a stranger came to the Roman emperor Tiberius. - History of metals.ppt
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Test "Metals"
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Boldyreva Anastasia
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Metals MOU “Kirish secondary school No. 8” Completed by: 9b grade student Boldyreva A Head: chemistry teacher Babkina L.N, Kirishi 2007
Metals are chemical elements that in the free state form simple substances with a metallic bond. 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, a person got acquainted with metals that are found in native form - this is gold, silver and copper. The remaining metals appeared after a person 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 depicting the goddess Athena and an owl. 2. A gold coin depicting Alexander the Great and the god Zeus. 3. Copper coin in the form 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 pyramid of Cheops is built is made of stone and copper.
Being in nature
Most CE are metals. The boundary between metals and non-metals is arbitrary. B Si Nonmetals As Te Metals At
Metals Transition element Non-metals 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 is increased. Restorative 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 contract. The number of electrons in the outer level increases as the group number increases. Restorative 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 point Refractory Hg, Ga, Cs, In, Bi W, Mo, V, Cr
Density Light Heavy (Li - the lightest, (osmium - the most K, Na, Mg) heavy Ir, Pb)
Have a metallic luster
Alkali metals Transition metals Alkaline earth metals By reactivity
Chemical properties of metals Metals in chemical reactions are reducing agents, while they are oxidized M o - ne \u003d M n + Al, Be, Mg, Ca, Li, Na, K, Rb, Cs Reducing ability increases
Metals are displaced from their compounds by other metals N.N. Beketov - created a "displacement series" (a 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 (harder) Mg + O 2 = 2Mg O With elements of group V (under harsh conditions) 3Ca + 2P = Ca 3 P2
Interaction with complex substances With acid solutions (metals in the voltage series up to "H") Zn + H 2 SO 4 \u003d Zn S O 4 + H 2 C solutions of metal salts in the voltage series to the right of Zn + Pb (NO 3) 2 \u003d Zn (NO 3) 2 + Pb C water (active) 2Na + 2H 2 O \u003d 2Na OH + H 2 The reaction proceeds if a soluble base is formed.
The use of metals Machine tool construction Medicine Agriculture Production of alloys In the home Metallurgical industry
Obtaining metals Pyrometallurgical method - reduction with carbon, carbon monoxide (II), hydrogen at high temperature. The aluminothermic method is the reduction of metals with the help of aluminum. Hydrometallurgical method - obtaining a more active metal from ore or from solutions Electrolysis - using electric current from melts or solutions