Magnesium Courtney Kilgore & Shayla Edmonson

Magnesium  Chemical symbol - Mg  Atomic number - 12  Atomic mass  The group number - 2  The period number - 3

Magnesium 1.

2D

Physical properties  Magnesium has an appearance of a silvery and white shade. Among all the structural metals, magnesium is the lightest. Its boiling point is 1090 degrees Celsius or 1994 degrees Fahrenheit. The metal also displays a very good conductivity of heat and electricity. The structural metals are generally used to build massive structures and buildings. Magnesium however is rarely used in the structures in its free form due to its reactive properties. It is, in such cases, used as an alloy. This metal can be fabricated very easily. Pieces of magnesium can be welded, molded, cut and shaped according to the requirements. About 2.1 percent of the earth's crust contains magnesium. This volume makes magnesium the 6th most found element. One of the biggest deposits of magnesium is found in the sea water. It has been calculated by the scientists, that a cubic mile of seawater contains about six million tones of magnesium. As mentioned in the chemical properties, magnesium is also present in many other compounds like dolomite, magnesium carbonate that is also known as magnesite and magnesium sulfate which is also known by the name epsomite.

Chemical properties Magnesium is located among the alkaline earth metals on the periodic table. This element belongs to the group 2 and period 3 of the periodic table and has the atomic number 12. The average atomic mass of the element magnesium is It must be noted that Magnesium is a very reactive metal and does not exist in a free state in nature. It reacts with a slow pace with cold water and at a very rapid pace with hot water. The oxidation process of magnesium is very rapid and if kept in open, a layer of oxidized magnesium is formed on the surface of the metal. Magnesium also burns very rapidly, when it is at room temperature. This burning process is very furious as it produces a blinding white light. This metal also reacts with almost all the acids and alkalizes, forming a variety of different compounds and by products. Another important property of magnesium is that it actively reacts with many non-metals such as nitrogen, phosphorous, chlorine, sulfur, bromine, iodine and fluorine. Magnesium also readily reacts with some other compounds such as carbon monoxide, carbon dioxide, sulfur dioxide and nitric oxide.

The uses  Magnesium is used in pyrotechnic and incendiary devices. It is alloyed with other metals to make them lighter and more easily welded, with applications in the aerospace industry.  Magnesium is added to many propellants.  It is used as a reducing agent in the preparation of uranium and other metals that are purified from their salts.  Magnetite organic magnesium compounds have many uses.  Magnesium is essential fore plant and animal nutrition.  Chlorophyll is a magnesium-centered porphyry.

The History  Magnesium was originally named ‘magnium’ by Humphrey Davy after the element from magnesia, known now as magnesium oxide. The 1915 Nobel prize is chemistry was awarded to Richard Wills Tatter for his work with the chlorophyll and identifying magnesium was the central atom in it’s structure. Epsom salt a magnesium compound, magnesium sulfate (Mg s04). Magnesium is the 10 th most aberrant element in the human body. Magnesium will burn in pure nitrogen gas and pure carbon dioxide gas. Magnesium it’s the fifth most common element fond in sea water.

Allotropes, Isotopes, or Important Compounds  Magnesium has 21 known isotopes ranging from Mg-20 to Mg-40. Magnesium has 3 stable isotopes ; Mg-24, Mg-25 and Mg-26

The Discovery  Recognized as an element by black 1775; isolated by sir Humphrey Davy 1808 (England) 1.

Random Facts  Atomic weight  Element classification – Alkaline Earth metal  Density (g/co) – 1,738 lattice constant (a)  Atomic Radius (pm) – 160 lattice C/A Ratio –  Atomic volume (cc/mol) – 14.0 cas registry Number  Covalent radius (pm) – 136  Inaccuracies – 66 (t2e)  Specific heat mol ) –  Appears – light weight, malleable, silvery – white metal  Fusion heat (kJ/mol):  Evaporation heat (kJ/mol) –131.8  Debye temperature (k) –  Pauling negativity number – 1.31  First Ienizing energy (kJ/mol) –  Oxidation states – 2  Lattice stucture - Hexagonal 