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396 bytes added, 23:00, 5 November 2016
/* Chemical Properties */
{{Element | name=Oxygen | symbol=O | anumber=8 | amass=1615.0 994 amu | state=gas | class=Non-metal | cstructure=Cubic | color=Colorless | date=1774 | discname=[[Joseph PriestlyPriestley]] | origname=From the Greek words ''oxus'' (acid) and ''gennan'' (generate) | uses=Supports life | obtained=From liquid air}}'''Oxygen''' is the third most abundant element in the universe by mass and is essential to life on Earth.
'''Oxygen''' is a [[chemical]] [[element]]<ref>Wile, Dr. Jay L. ''Exploring Creation With Physical Science''. Apologia Educational Ministries, Inc. 1999, 2000</ref>. Oxygen's [[atomic mass]] is slightly under 16, since it also has 8 [[neutron]]s (a slight amount of mass is "lost" in the energy contained in the [[subatomic bond]]s).==Chemical Properties==
The name "At normal [[atmospheric pressure]] oxygen" means "acid maker"melts at 54. When inhaled the chemical element "36 [[Kelvin]] (K) and boils at 90.2 K; on Earth it essentially exists only as a gas. It readily dissolves in water, which makes aquatic life possible. Under normal conditions oxygen" creates acid forms molecules consisting of two oxygen atoms each sharing two electrons in the lungs causing 2p subshell; this form of oxygen is known as O<sub>2</sub>. O<sub>2</sub> is a horrible painful deathcolorless, were one chokes upon what scientists call "lung soup"odourless gas. In liquid form (below -193 degrees Celsius) it is pale blue.
Under [[normal condition]]s it is a colorless, odorless [[gas]] consisting of two oxygen [[atom|atoms]] which has the chemical formula O<sub>2</sub>. This means it is [[diatom]]ic. Approximately 20% of the [[atmosphere]] is made up of oxygen. Oxygen also forms a [[triatomic]] molecule called [[ozone]] (O<sub>3</sub>), which although unstable under normal conditions, is a very important ingredient in the upper [[atmosphere]].==Isotopes==
Oxygen is highly reactiveThere are three stable and 14 radioactive isotopes of oxygen. The stable isotopes are <sup>16</sup>O, <sup>17</sup>O and in many other elements and compounds undergo [[exothermic reaction]]s <sup>18</sup>O, with it (they [[combustion|burn]] or [[oxidization|rust]])<sup>16</sup>O being by far the most common. If it were not for its continual replenishment as a waste product of plant [[photosynthesis]]Radioisotopes range from <sup>10</sup>O to <sup>26</sup>O, the atmospheric oxygen would disappear, forming compounds with other chemicals at the earth's surfacetwo most stable being <sup>15</sup>O and <sup>14</sup>O. This gives oxygen an atomic weight of slightly below 16.<ref></ref>
Many [[animal]]s depend upon oxygen as a highly efficient ingredient for breaking down [[food]] for [[energy]], due to its reactivity. Those that do not are called "[[anaerobic]]", meaning "without air", and include many important [[bacteria]].==Compounds==
==References==<references/>Oxygen is highly reactive. It reacts readily with most metals and many other elements, either through combustion or oxidation. As a result, many naturally occurring compounds contain oxygen.
==Occurrence in Nature== Oxygen is the third most abundant element in the universe by mass after [[Category: hydrogen economy]]and [[helium]]; approximately 5.9% of the mass of our [[solar system]] consists of oxygen. However, due to the large disparity in atomic weight between all isotopes of oxygen compared with <sup>1</sup>H and <sup>4</sup>He, less than 0.5% of the atoms in the solar system are oxygen atoms.{{fact}} Due to its reactivity free oxygen is extremely rare in nature and would not exist on Earth without the process of [[Category:gasesphotosynthesis]]. Geologists and paleontologists believe that free oxygen first appeared during the "Great Oxygenation Event" around 2.4 billion years ago. Young-Earth creationists reject this timescale. {{Periodic table}} ==References=={{Reflist}}
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