{"id":20,"date":"2020-04-08T14:56:00","date_gmt":"2020-04-08T14:56:00","guid":{"rendered":"https:\/\/thechemicalelements.com\/?page_id=20"},"modified":"2023-08-16T11:17:20","modified_gmt":"2023-08-16T11:17:20","slug":"sodium","status":"publish","type":"post","link":"https:\/\/thechemicalelements.com\/sodium\/","title":{"rendered":"Sodium (Na)"},"content":{"rendered":"\n

Sodium is a chemical element with atomic number 11 in the periodic table. It’s the fourth most abundant element and comprises around 2.6% of Earth\u2019s crust. Being a member of the alkali metals family<\/a> of the periodic table, this monoisotopic element has one valence electron that makes it one of the most reactive elements in the periodic table.\u00a0\u00a0<\/span><\/p>\n\n\n\n

Sodium chloride (or table salt) is the most common compound of this chemical element. Being an essential nutrient responsible for the transmission of the sensory impulses between the cells of our body, high sodium levels in the blood may damage cellular metabolism, cause high blood pressure, and cardiovascular diseases.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Chemical and Physical Properties of Sodium<\/span><\/h3>\n\n\n\n
Property<\/strong><\/td>Value<\/strong><\/td><\/tr>
Symbol<\/td>Na<\/td><\/tr>
Name<\/td>Sodium<\/td><\/tr>
Atomic number<\/td>11<\/td><\/tr>
Atomic weight (mass)<\/td>22.989768 g.mol-1<\/td><\/tr>
Group<\/td>1 (Alkali Metals<\/a>)<\/td><\/tr>
Period<\/td>3<\/td><\/tr>
Color<\/td>A silvery-white alkali metal with a bright luster<\/td><\/tr>
Physical state<\/td>Solid at room temperature<\/td><\/tr>
Half-life<\/td>From 1.3(4)\u00d710\u221221 seconds to 2.605 years<\/td><\/tr>
Electronegativity<\/td>0.93<\/td><\/tr>
Density<\/td>0.971 g\/cm\u00b3<\/td><\/tr>
Melting point<\/td>370.95\u00b0C<\/td><\/tr>
Boiling point<\/td>1154.55\u00b0C<\/td><\/tr>
Ionic radius<\/td>1.02 (+1) \u00c5<\/td><\/tr>
Isotopes<\/td>21<\/td><\/tr>
Most characteristic isotope<\/td>23Na<\/td><\/tr>
Electronic shell<\/td>[Ne] 3s1<\/td><\/tr>
The energy of the first ionization<\/td>495.7 kJ.mol-1<\/td><\/tr>
Uses<\/td>Few uses for pure metal; compounds in medicine, agriculture, photography. Sodium chloride (NaCl) is table salt. Liquid sodium cools nuclear reactors.<\/td><\/tr>
Description<\/td>Lightweight, malleable, silvery-white metal. Eighth most abundant in the universe. Seventh most abundant in earth’s crust.<\/td><\/tr>
Shells<\/td>2,8,1<\/td><\/tr>
Valence<\/td>1<\/td><\/tr>
Crystal Structure<\/td>Cubic: Body centered<\/td><\/tr>
Covalent Radius<\/td>1.54 \u00c5<\/td><\/tr>
Atomic Radius<\/td>2.23 \u00c5<\/td><\/tr>
Atomic Volume<\/td>23.7 cm\u00b3\/mol<\/td><\/tr>
Name Origin<\/td>Medieval Latin: sodanum; symbol from Latin natrium.<\/td><\/tr>
Discovery date<\/td>In 1807 by Sir Humphry Davy<\/td><\/tr>
Pronunciation<\/td>SO-di-em<\/td><\/tr>
Oxidation States<\/td>1<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

With the periodic table symbol Na, atomic number 11, atomic mass of 22.990 (23) g.mol-1, and electron configuration [Ne] 3s1, sodium is soft, easily malleable, silvery-white metal with a bright luster that can be dented with any harder object. When exposed to air, sodium metal tarnishes and the substance loses its silvery luster. It also emits a brilliant yellow flame in the reaction with any of the major air components: nitrogen<\/a> (N2), oxygen<\/a> (O2), carbon<\/a> dioxide (CO2), water (H2O).<\/span><\/p>\n\n\n\n

The pure, elemental form of sodium reaches its boiling point at 882.940\u00b0C, 1621.292\u00b0F, and 1156.090 K, while the melting point is achieved at 97.794\u00b0C, 208.029\u00b0F, and 370.944 K. Even though the density of alkali metals increases with the increase of the atomic number, sodium has a higher density in comparison to potassium<\/a>. This member of the alkali metals family of elements has an electronegativity of 0.9 according to Pauling, whereas the atomic radius according to van der Waals is 0.196 nm.\u00a0<\/span><\/p>\n\n\n\n

In contact with water, sodium creates an extremely volatile reaction that results in an explosion that releases a large amount of heat. This chemical reaction also produces sodium hydroxide and hydrogen<\/a> gas. Sodium metals float in water due to their extremely low density.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Was Sodium Discovered?<\/span><\/h2>\n\n\n\n

In 1807, the English chemist Sir Humphry Davy (1778 \u2013 1829) became the first scientist who succeeded in preparing elemental sodium. Intrigued by his discovery of the electrical nature of the chemical bonding, Sir Davy came up with the idea that he could use this electricity for isolating the chemical elements from the compounds. For this, he conducted electrolysis of caustic soda which resulted in the pure form of sodium for the first time in science. The electrolysis was powered by three batteries made by this Cornish inventor.<\/span><\/p>\n\n\n\n

During the experiment, Sir Davy observed a liquid substance at the wire electrode immersed in sodium hydroxide which turned into a solid and silvery-lustrous metal when exposed to room temperature. The great English chemist also succeeded in obtaining scientific evidence for the sodium\u2019s reaction with water that produced hydrogen as a result.\u00a0<\/span><\/p>\n\n\n\n

Despite the lower density in comparison to the other metal elements<\/a>, Sir Davy held his opinion that it should be also classified as a metal, pointing out the fact that the platinum<\/a> is nearly four times as heavy as tellurium<\/a>, as well as the great differences of the chemical properties among the metal elements.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Did Sodium Get Its Name?<\/span><\/h2>\n\n\n\n

The name of element 11 comes from the Latin word \u2018<\/span>natrium<\/span><\/i>\u2019, which refers to one of the most common sodium compounds. Sir Humphry Davy himself gave the name sodium to the new metal he had discovered, for he isolated the pure form of it from caustic soda.\u00a0<\/span><\/p>\n\n\n\n

On the other hand, the German word for soda is \u2018<\/span>natronlauge<\/span><\/i>\u2019, so the name \u2018<\/span>natronium<\/span><\/i>\u2019 was also suggested by the German physicist and chemist L. W. Gilbert (1769 \u2013 1824).\u00a0<\/span><\/p>\n\n\n\n

The Swedish chemist, Baron J\u00f6ns Jacob Berzelius, preferred the shorter form of the aforementioned term – <\/span>natrium<\/span><\/i>, which served as a source of the chemical symbol for sodium (Na).<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Where Can You Find Sodium?<\/span><\/h2>\n\n\n\n

Copious quantities of sodium can be found in the heavy stars, the Sun, as well as in the region between the stars, made up of gaseous clouds and solid particles. Sodium has been traced in the aforementioned celestial objects in both its atomic and ionic form. It\u2019s formed when atoms of neon gain a proton. Before this process, the atoms of neon<\/a> are formed by the carbon atoms consolidated during nuclear fusion reactions.\u00a0<\/span><\/p>\n\n\n\n

On our planet, oceans are one of the richest sources of sodium. It also occurs in spring water and alkaline and salty lakes. Sodium is one of the most reactive elements of the periodic table. As a result, it can rarely be found in nature in its pure, elemental form. Hence, element 11 is often found in many mineral ores, such as soda niter, amphibole, rock salt, feldspars, zeolite, cryolite, and sodalite. Among these mineral compounds, halite (sodium chloride salt) is the mineral from which sodium is most often obtained by mining.\u00a0<\/span><\/p>\n\n\n\n

The first commercial quantities of sodium were produced by the <\/span>Deville process<\/span><\/a> that includes thermal reduction of sodium carbonate with carbon at 1,100 degrees Celsius. Also, the pure form of sodium can be obtained by electrolysis of molten sodium chloride or thermal decomposition of sodium azide.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Sodium in Everyday Life<\/span><\/h2>\n\n\n\n

Sodium is used in a wide array of industries where it\u2019s used to prepare sodium compounds such as common salt, baking soda, borax, sodium nitrate, etc. Furthermore, this chemical finds application in the following instances:<\/span><\/p>\n\n\n\n