{"id":1214,"date":"2019-12-06T09:25:04","date_gmt":"2019-12-06T09:25:04","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=1214"},"modified":"2019-12-06T09:25:10","modified_gmt":"2019-12-06T09:25:10","slug":"group-2-periodic-table","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/group-2-periodic-table\/","title":{"rendered":"Group 2 Periodic Table"},"content":{"rendered":"\n

WHAT IS PERIODIC TABLE?<\/h2>\n\n\n\n

It is a tabular display of chemical elements, arranged in order of atomic number in rows so that elements with similar atomic structure and recurring chemical properties appear in vertical columns. The seven rows of the table are called a periodic table.  <\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

In the periodic table, chemical elements are present in rows\nhorizontally in order of increasing atomic number and vertically according to\nthe recurring properties of their atoms.<\/p>\n\n\n\n

Metals are on the left side and non-metal are on the right\nside of the periodic table <\/p>\n\n\n\n

GROUPING METHOD<\/h2>\n\n\n\n

In the periodic table of chemical elements, there is a group (also known as a family) is a column of elements. There are multiple ways of grouping the elements but they are commonly divided into metals, non-metals, metalloids. There are also more specific groups like alkali metals, transition metals, rare metals, alkaline earth, halogens, and noble gases.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The 18 vertical columns of the table are called Groups. The\ns-, p- and d-block elements of the periodic table are arranged into these columns\nor groups. Each group of elements having the same number of valence electrons. The\nSame group elements have similar properties and reactivity. These elements tend\nto show patterns in atomic radius, ionization energy, and electronegativity. <\/p>\n\n\n\n

GROUP 2 OF THE PERIODIC TABLE <\/h2>\n\n\n\n
\"\"<\/figure>\n\n\n\n

Group 2 elements are:<\/h3>\n\n\n\n
\n Br<\/strong>\n <\/td><\/tr>
\n Mg<\/strong><\/strong>\n <\/td><\/tr>
\n Ca<\/strong><\/strong>\n <\/td><\/tr>
\n Sr<\/strong><\/strong>\n <\/td><\/tr>
\n Ba<\/strong><\/strong>\n <\/td><\/tr>
\n Ra<\/strong><\/strong>\n <\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
  • Beryllium<\/li>
  • Magnesium<\/li>
  • Calcium<\/li>
  • Strontium<\/li>
  • Barium<\/li>
  • Radium<\/li><\/ul>\n\n\n\n

    Group 2<\/strong> elements are called alkaline metals<\/strong> because they form\nalkaline solutions, hydroxides, when reacting with water and their oxides are\nfound in the earth’s crust.<\/p>\n\n\n\n

    ALKALINE METALS<\/h2>\n\n\n\n
    • They\nhave low electron affinity.<\/li>
    • Group\n1 metals are less reactive than group 2 metals.<\/li>
    • Its\nvalence shell contains 2 electrons<\/li>
    • They\nhave low electronegativity<\/li>
    • Compounds\nof alkali metals are often insoluble in water<\/li>
    • Alkaline\nmetals are usually Shiny, silvery.<\/li>
    • They\nhave ions with a +2 charge.<\/li>
    • They\nare solid<\/li>
    • They\nare harder, denser, stronger <\/li>
    • They\n are found in the earth crust<\/li><\/ul>\n\n\n\n

      BERYLLIUM<\/h2>\n\n\n\n
      \n Group \n <\/td>\n 2\n <\/td><\/tr>
      \n Atomic number\n <\/td>\n 4\n <\/td><\/tr>
      \n Block \n <\/td>\n s\n <\/td><\/tr>
      \n State at 20\u2070\n <\/td>\n Solid\n <\/td><\/tr>
      \n Melting point\n <\/td>\n 1287C,2349F,1560K\n <\/td><\/tr>
      \n Boiling point\n <\/td>\n 2468C,4474F,2741K\n <\/td><\/tr>
      \n Density (g cm-3)<\/sup>\n <\/td>\n 1.85\n <\/td><\/tr>
      \n Key isotopes\n <\/td>\n 9<\/sup>Be\n <\/td><\/tr>
      \n Relative atomic\n mass\n <\/td>\n 9.012\n <\/td><\/tr>
      \n Electron configuration\n <\/td>\n (He)2s2<\/sup>\n <\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

      Occurrence<\/h3>\n\n\n\n

      It is a rare element in-universe. Beryllium was discovered in\n1798 <\/strong>by French chemist Nicolas-Louis Vauquelin<\/strong>. The name was\nderived from the Greek name beryl,\n\u2018beryllo\u2019<\/strong>. Friedrich Wohler at berlin in 1828 isolated the beryllium metal.\nBeryllium generally occurs in the earth’s crust to the extent of 0.0002\npercent. Beryllium is a steel-gray metal. It is quite brittle. Its chemical\nproperties resemble aluminum. Emerald is known to be a variety of beryl.<\/p>\n\n\n\n

      Physical properties<\/h3>\n\n\n\n

      It has a close-packed hexagonal crystal structure.it has a\nvery high melting point which makes beryllium metal the best heat dissipation\ncharacteristics per unit weight.it has a low coefficient of linear thermal\nexpansion. These characteristics make unique stability under thermal loading.\nIn the air, beryllium resists oxidation and corrosion.it is extracted by the\nmineral beryl.<\/p>\n\n\n\n

      Chemical properties<\/h3>\n\n\n\n

      While bonding with the other atoms, it has a very high ionization\npotential and strong polarization. Beryllium has a +2 oxidation state.it allows\nforming many covalent bonds.it dissolves in non- oxidizing acids. Binary compounds\nare formed by the combination of beryllium with non-metals such as Beryllium\noxide (BeO). It is white solid and has a very high melting point. Emerald and\naquamarine contain Beryllium. <\/p>\n\n\n\n

      Uses<\/h3>\n\n\n\n
      • It\nis used to make semiconductor devices.<\/li>
      • It\nis useful in making radio equipment and engines.<\/li>
      • It\nis used in making windows for X-rays tubes.<\/li>
      • Useful\nfor mirrors and camera shutters.<\/li>
      • It\nis fabricated into gyroscopes, computer parts, and accelerometers.<\/li><\/ul>\n\n\n\n

        MAGNESIUM<\/h2>\n\n\n\n
        \n Symbol\n <\/td>\n Mg\n <\/td><\/tr>
        \n Atomic number\n <\/td>\n 12\n <\/td><\/tr>
        \n Atomic mass\n <\/td>\n 24.305\n <\/td><\/tr>
        \n Electron configuration\n <\/td>\n 1s2<\/sup>,2s2<\/sup>,2p6<\/sup>,3s2<\/sup>\n <\/td><\/tr>
        \n Oxidation state\n <\/td>\n +2\n <\/td><\/tr>
        \n Specific gravity\n <\/td>\n 1.74 at 20,68\n <\/td><\/tr>
        \n Melting point\n <\/td>\n 650(1202\n <\/td><\/tr>
        \n Boiling point\n <\/td>\n 1090(1994)\n <\/td><\/tr>
        \n Thermal\n conductivity\n <\/td>\n 156 W m-1<\/sup>K-1<\/sup>\n <\/td><\/tr>
        \n Atomic Radius\n <\/td>\n 150pm\n <\/td><\/tr>
        \n Electrical\n conductivity\n <\/td>\n 22.4 x 106<\/sup>\n Sm-1<\/sup>\n <\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

        Occurrence <\/h3>\n\n\n\n

        It was first isolated in 1808<\/strong>\nby Sir\nHumphrey Davy<\/em><\/strong> by the process of mercury evaporation from the magnesium\namalgam which is made by the electrolyzing a mixture of moist magnesia and\nmercuric oxide. By heating, mercury was removed from the amalgam and leave the\nmercury metal. He isolated many other alkalies and alkali earth metals. <\/p>\n\n\n\n

        In June 1808 he described how he obtained magnesium by\nremoving mercury. He observed that in the air the metal turned into white\npowder and gains weight, reacts with oxygen and returned to its oxide form.<\/p>\n\n\n\n

        In the earth’s crust, it is the eighth-most abundant\nelement.it is found in more than 60 minerals.it is found in large deposits of\ndolomite, magnesite, brucite, and carnallite and in mineral water where\nmagnesium is soluble.<\/p>\n\n\n\n

        Production of magnesium<\/h3>\n\n\n\n

        The double carbonate of calcium and magnesium, dolomite is\nfar more widely distributed and seawater provides an inexhaustible source of\nthe chloride in the dilute form, while certain concentrated solutions of\nmagnesium salts are present in the Dead sea. <\/p>\n\n\n\n

        There are two methods for the production of magnesium<\/p>\n\n\n\n