Atom

{{Physics}}
An '''atom''' is the smallest possible physical unit of a [[chemical]] element. Atoms consist of [[proton]]s (with a single positive charge each), [[electron]]s (with a single negative charge) and  [[neutron]]s (with no charge).<ref name="britannica">[https://www.britannica.com/science/atom Atom] - ''Britannica Encyclopedia''</ref> For example, the most common isotope of [[hydrogen]] has zero neutrons and consists in its atomic form of a single proton and a single electron.<ref>{{cite book |last1=Housecroft |first=Catherine E. |last2=Sharpe |first2=Alan G. |edition=2nd |date=2005 |title=Inorganic Chemistry |publisher=Pearson Prentice-Hall |page=237 |isbn=0130-39913-2}}</ref>  All heavier nuclei require neutrons to stabilize them.<ref>[https://www.nuclear-power.com/nuclear-power/reactor-physics/atomic-nuclear-physics/nuclear-stability/ Nuclear Stability] - Nuclear Power.com</ref>

==Discovery==
{|
|-
! Fundamental particle !! Symbol !! Absolute charge !! Relative charge !! Mass !! Discovered by !! Year
|-
| Electron || e || -1.6×10<sup>-19</sup>C || -1 || 9.1×10<sup>-31</sup>kg || JJ Thompson || 1897
|-
| Proton || p || +1.6×10<sup>-19</sup>C || -1 || 1.67×10<sup>-27</sup>kg || E Goldstein || 1886
|-
| Neutron || n || 0 C || 0 || 1.67×10<sup>-27</sup>kg || J Chadwick || 1932
|}

==Isotopes==
The atoms which comprise each individual [[element]] have of a unique number of protons, known as the "atomic number".<ref>[https://www.periodic-table.org/what-is-atomic-number-definition/ What is the atomic number?] - Periodic Table Web</ref> Most elements occur in nature as several different "isotopes", each with a different number of neutrons. Combining the number of protons and the number of neutrons results in the atom's "mass number". For example, chlorine is found primarily as two stable isotopes, with mass numbers of 35 and 37, but both have 17 protons.

Often, all but one (if not all) of these isotopes will be unstable, and will [[radioactive decay|decay]] at a predictable rate to one of the lighter, more stable isotopes.  Isotopes are referred to by a number equal to the total number of protons and neutrons (i.e., U-235, U-239, etc.) which is also very close to the actual atomic mass. Elements with no stable isotopes eventually decay into other, lighter elements. The relative stability — that is, how long it takes a given percentage to decay — and initial ratios of the isotopes will determine their ratios at a subsequent point in time.<ref>[https://www.epa.gov/radiation/radioactive-decay Introduction to radioactive decay] by the [[EPA]]</ref> This is the basis for [[radiometric dating]].<ref>[https://ncse.ngo/radiometric-dating-does-work Radiometric dating does work!] - [[NCSE]]</ref>

Atoms are arranged by number and chemical behavior by the [[periodic table]].<ref>[https://history.aip.org/exhibits/curie/periodic.htm What is the periodic table?] - Marie Curie and the science of radioactivity</ref>

==Structure==
The neutrons and protons form the nucleus, a very dense core which contains virtually all the mass of the atom. Each atom also technically comes with a number of electrons equal to the number of protons, making it electrically neutral. However, in nature, the electrons can be more or less closely associated with the nucleus and its protons.{{fact}}  

While the atom is normally thought of as being like a little solar system, with the nucleus represented by the sun and the planets representing the electrons in "orbit" around it, it is really more like a tiny positively charged glob with a series of uniquely configured negatively charged force fields pulsating around it.<ref name="britannica" />

In the state of matter called ''plasma'', nuclei and their electrons are completely dissociated.  This only occurs at very high temperatures.<ref>[https://www.psfc.mit.edu/vision/what_is_plasma What is plasma?]</ref>

==References==
{{reflist}}
{{stub|physics}}
[[Category:Chemistry]]
[[Category:Physics]]

Categories: Chemistry, Physics