Gallium

Jonathan Perez and Corey Dulsky

Gallium Atomic Number:31 Symbol:Ga Atomic Mass:69.723 Gallium is solid at room tempature but starts to melt slightly above room tempature

Period number:4 Group number:13 A soft silvery meta**Boiling Point:** 2403.0 °Cllic [|poor metal], elemental gallium is a brittle solid at low temperatures. As it liquifies slightly above [|room temperature], it will melt in the hand. Its melting point is used as a temperature reference point, and from its discovery in 1875 to the semiconductor era, its primary uses were in high-temperature thermometric applications and in preparation of metal alloys with unusual properties of stability, or ease of melting; some being liquid at room temperature (Ga-In eutectic, 75% Ga, 25% In, mp = 15.5°C). In semiconductors, an important application is in the compounds [|gallium nitride] and [|gallium arsenide], used most notably in [|light-emitting diodes] (LEDs). Semiconductor use is now the primary industrial market for gallium, but new uses in alloys and fuel cells continue to be discovered. Gallium is not known to be essential in biology, but because of the biological handling of gallium’s primary ionic salt Ga(III) as though it were iron(III), gallium ion localizes to and interacts with many processes in the body in which iron(III) is manipulated. As these processes include [|inflammation], which is present as a marker for many disease states, several gallium salts are used, or are in development, as both pharmaceuticals and radiopharmaceuticals in medicine. 12C Abundance is 99.89% 13C Abundance is 1.11% State of Matter is a solid at room tempature but a liquid above room tempature Gallium is bright silver Gallium is brittle Gallium is a poor conductor of electricity/heat Gallium is a metal The only way that gallium ions will form is when a gallium salt dissolves in water and dissociates into ions. Since gallium has three valence electrons, then it will form an ion with a +3 charge. Gallium is a transition metal Biological role:Gallium has no biological role but it stimulates the metabolism. Gallium compounds are not toxic Health Hazards:Inhalation-May cause a red,dry,throatand coughing,sneezingand difficulty breathing Ingestion-May cause nausea,vomiting,mettelic taste,itching,sweating,abdominal pain,Diahrrea,sleepiness,and loss of appetite Skin-May cause redness,itching and inflammation Eye- May cause red ,itching,inflammation and watering Environmental effects: Gallium is an ideal element to use in the bomb pits, but pollution is destructive to the earth and to the health of its inhabitants Abundance in Universe:10ppb Abundance in Sun : 40ppb Gallium is not found in nature Gallium is found in ores and minerals Gallium is found in minute amounts in some bodies of water
 * [[image:bohr.gif]] ||  || **Number of Energy Levels:** 4 **First Energy Level:**
 * Second Energy Level:**
 * Third Energy Level:**
 * Fourth Energy Level:** ||
 * Atomic Number:** 31
 * Atomic Mass:** 69.723 **Melting Point:** 29.78 °C (302.93 K, 85.604004 °F) **Date of Discovery:** 1875
 * Discoverer:** Paul Emile Lecoq de Boisbaudran a French Chemist
 * Name Origin:** From the Latin word //Gallia//, the old name of France
 * Uses:** semiconductor production
 * Obtained From:** bauxite, germanite, coal
 * Boiling Point:** 2403.0 °C
 * 1) of Ions:6

media type="teachertube" key="7c60d7578466a16659bd" width="400" height="350"