write down the silent of physical properties of metal
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Answer:
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Explanation:
Metals have different physical and chemical properties. They have different surface appearance, density, hardness, melting point, boiling point, Young Modulus, breaking stress/strain, shear modulus, heat and electrical conductivity, malleability, ductility and magnetic properties.
They also all have many different isotopes. The isotopes of a particular metal all have the same atomic number, Z, but they have different mass numbers, A, because they are atoms/ nuclei with different numbers of neutrons. Many of a metals isotopes are radioactive, but the metal usually has one most abundant isotope, which is stable. As Z increases, metals tend to have more isotopes.
All metals are solids at room temperature, except for Mercury, which is a very dense liquid. The least dense metal is Lithium ( 0.543 g/cm^3), and the most dense is Osmium ( 22.59 g/cm^3). The hardest metal is Chromium, and the softest is Caesium. The metal with the highest melting point is Tungsten, 3422 degC. It is also the strongest metal. The best conductor is silver, followed by copper and gold. Gold is also the most malleable and ductile metal. Potassium and sodium are the least ductile metals. If a metal is strongly attracted to a permanent magnet, then it is called ferromagnetic; the three strongest are Iron, Nickel and Cobalt. Some of the others, such as Aluminium, Copper, Uranium and Platinum, are only very weakly attracted, and are called paramagnetic. A few are even weakly repelled and are called diamagnetic - examples include Bismuth.
Metals have similar chemical reactions and form similar compounds. All metals have 1, 2 or 3 unpaired electrons in their outer shell, and they easily lose these electrons, so as to produce a full outer shell and a +1, +2 or +3 ion, which is more stable than the neutral arrangement.
Metals differ in how reactive they are. The Group 1 Alkali metals are the most reactive group, and they get more reactive as you go down the group. Francium doesn’t have any stable isotopes, so the most reactive metal is Caesium. Nearly all metals form oxides, by reacting with Oxygen, and the Group 1 metals, in their pure form, react with the Oxygen in the air, so they have to be kept under oil. They all react spontaneously, and vigorously with water, giving off H2 gas, and forming the metal hydroxide, which is basic or alkaline, in solution. Hydroxides will react with acids to form salts, like Sodium Chloride ( NaCl), KCl etc etc, or carbonates, like Calcium Carbonate (CaCO3), and sulphates, like Copper Sulphate (CuSO4).
Magnesium burns in air, with a very hot, white, bright flame, to produce Magnesium Oxide, in the form of a white powder. Pure Aluminium reacts with the Oxygen in the air to form a surface layer of Aluminium Oxide (Al2O3). Even iron, which is not all that reactive, reacts with oxygen in the air, in the presence of water and salt, to produce red Iron Oxide or rust (Fe2O3). Iron is a rather odd metal because its ion can be either Fe2+ or Fe3+. Several other metals are also like this, and these tend to fall amongst the transition metals.
Transition metal compounds tend to be coloured, unlike those of Groups 1,2 and 3. Copper Sulphate, which is a strong blue colour, is a good, common example. Transition metal chemistry is complex because the atoms of these metals can exist in a large number of different oxidation states, like Iron in the weird compound Potassium Ferrate, with a formula K2FeO4. Here, the iron atom is in an oxidation state of +6 (6 electrons have been lost from the atom) and the tetrahedral FeO4 group is an anion of charge 2-. It is a stable, very strong oxidizing agent, purple solid at room temperature, but breaks down in water producing O2 gas, Iron(111) oxide (Fe2O3) and Potassium Hydroxide (KOH) in solution. The products are just more stable, when in water. There are several similar compounds, such as Potassium Permanganate, K2MnO4, and Potassium Chromate K2CrO4 (this is a yellow solid at room temperature, and is also a strong oxidizing agent).
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