Orbital - Revision history

Jmdonev: 1 revision imported

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energy>Jmdonev at 18:54, 18 February 2020

2020-02-18T18:54:43Z

← Older revision		Revision as of 18:54, 18 February 2020
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	[[Category:Done ~~2015~~-06-01]]		[[Category:Done 2020-02-29]]
	[[File:640px-F_orbital.png\|400px\|framed\|right\|Figure 1. Orbitals are ~~much more~~ complex ~~when looked at in terms of~~ quantum mechanics. Here are several orbital shapes that show where electrons are likely to be found. The numbers ~~shown below~~ are one of the quantum ~~numbers~~ used to describe these orbitals.<ref>Wikimedia Commons. (May 15, 2015). ''F Orbital'' [Online]. Available: http://commons.wikimedia.org/wiki/File:F_orbital.png#/media/File:F_orbital.png</ref>]]		[[File:640px-F_orbital.png\|400px\|framed\|right\|Figure 1. Orbitals are complex shapes that are determined using quantum mechanics. Here are several orbital shapes that show where electrons are likely to be found. The numbers are one of the [[quantum number]]s used to describe these orbitals.<ref>Wikimedia Commons. (May 15, 2015). ''F Orbital'' [Online]. Available: http://commons.wikimedia.org/wiki/File:F_orbital.png#/media/File:F_orbital.png</ref>]]
	<onlyinclude>An '''orbital''' in an atom refers to the regions within the atom where electrons have the highest probability of being found, ~~since [[electron]]s are dispersed through a large volume of~~ the [[~~atom~~]] ~~and not concentrated in one area like the [[neutron]]s and [[proton]]s~~.</onlyinclude> ~~The specifics~~ as to ''why'' electrons ~~are found more commonly in~~ certain ~~areas of the atom become~~ complex ~~very quickly, as the probabilities are based~~ in ~~principles of~~ [[quantum mechanics]].<ref>J.Kotz, J.Townsend, P.Treichel. (May 15, 2015). Chemistry and Chemical Reactivity, 8th ed. Belmont, CA, U.S.A: Brooks/Cole, 2012.</ref>		<onlyinclude>[[Electron]]s are dispersed throughout an [[atom]] rather than being in one specific place. An '''orbital''' in an atom refers to the regions within the atom where electrons have the highest probability of being found. There are also nuclear orbitals, please see the [[nuclear shell model]] to learn more.</onlyinclude> In nuclear physics these orbitals are often referred to as the ''shell model'' or ''nuclear shells''. Determining ''why'' electrons prefer certain positions is a complex calculation in [[quantum mechanics]].<ref>J.Kotz, J.Townsend, P.Treichel. (May 15, 2015). Chemistry and Chemical Reactivity, 8th ed. Belmont, CA, U.S.A: Brooks/Cole, 2012.</ref> The [[energy]] required to remove an electron from an atom depends on which orbital the electron is in.

	~~Simple understandings of~~ orbitals ~~describe the~~ areas where electrons ~~can~~ be found as "layers" in a cloud of electrons~~, spherical areas where electrons are~~ more ~~likely to be found. However,~~ quantum ~~mechanics~~ describes these orbitals quite differently, including values known as '''quantum ~~numbers~~''' to describe the size and shape of these orbitals. ~~The~~ orbital ~~that an electron lies within~~ determines the [[energy]] that the electron has~~, and orbitals~~ that result in two electrons having the same energy while ~~being~~ in a different orbital are referred to as '''degenerate'''.<ref name="RE1"/>		A simplified [[model]] for orbitals describes spherical areas where electrons are more likely to be found — as "layers" in a cloud of electrons. A more complex quantum mechanical model describes these orbitals quite differently, including values known as '''[[quantum number]]s''', to describe the size and shape of these orbitals. An electron's orbital determines the [[energy]] that the electron has. Orbitals that result in two electrons having the same energy, while each electron is in a different orbital, are referred to as '''degenerate''' orbitals.<ref name="RE1"/>

	Although orbitals are complex, their structure ~~can explain~~ properties of ~~some~~ matter. For example, ~~by knowing whether or not~~ an orbital ~~is full (each has room for two electrons),half full or empty~~ determines ~~the stability of an~~ [[~~element~~]] since the orbitals "want" to be ~~full or half~~ full. For example, an element like [[~~copper~~]] is a ~~stable element~~.<ref name="RE1">UC Davis Chemwiki. (May 15, 2015). ''Electronic Orbitals'' [Online]. Available: http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals</ref> ~~In addition to this, many~~ of the periodic properties of certain elements and the properties that families of elements have is caused by how these orbitals are filled with electrons.<ref>HyperPhysics. (May 15, 2015). ''Visualizing Electron Orbitals'' [Online]. Available: http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html</ref>		Although orbitals are complex, their structure explains many properties of [[matter]]. For example, the fullness of an orbital determines how that atom will [[chemical reaction\|chemically react]], since the orbitals "want" to be full. For example, an [[element]] like [[helium]] is chemically unreactive, being a noble gas, its orbitals are full.<ref name="RE1">UC Davis Chemwiki. (May 15, 2015). ''Electronic Orbitals'' [Online]. Available: http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals</ref> Many of the periodic properties of certain elements, and the properties that families of elements have, is caused by how these orbitals are filled with electrons.<ref>HyperPhysics. (May 15, 2015). ''Visualizing Electron Orbitals'' [Online]. Available: http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html</ref>

	To learn more about orbitals from a chemistry perspective, see [http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals UC Davis' Chemwiki].		To learn more about orbitals from a chemistry perspective, see [http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals UC Davis' Chemwiki].

	To learn more about orbitals from a physics perspective, see [http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html Hyperphysics].		To learn more about orbitals from a physics perspective, see [http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html Hyperphysics]. The [[nuclear shell model]] describes how orbitals of [[proton]]s and [[neutron]]s inside of a [[nucleus]] determine nuclear properties in a similar way.

			==For Further Reading==

			*[[Electron]]
			*[[Valence and core electrons]]
			*[[Valence band]]
			*[[Nucleus]]
			*Or explore a [[Special:Random\|random page]]

	==References==		==References==
	{{reflist}}		{{reflist}}
	[[Category:Uploaded]]		[[Category:Uploaded]]

J.williams: 1 revision imported

2015-08-26T21:31:28Z

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J.williams at 16:57, 12 August 2015

2015-08-12T16:57:17Z

New page

[[Category:Done 2015-06-01]]
[[File:640px-F_orbital.png|400px|framed|right|Figure 1. Orbitals are much more complex when looked at in terms of quantum mechanics. Here are several orbital shapes that show where electrons are likely to be found. The numbers shown below are one of the quantum numbers used to describe these orbitals.<ref>Wikimedia Commons. (May 15, 2015). ''F Orbital'' [Online]. Available: http://commons.wikimedia.org/wiki/File:F_orbital.png#/media/File:F_orbital.png</ref>]]
<onlyinclude>An '''orbital''' in an atom refers to the regions within the atom where electrons have the highest probability of being found, since [[electron]]s are dispersed through a large volume of the [[atom]] and not concentrated in one area like the [[neutron]]s and [[proton]]s.</onlyinclude> The specifics as to ''why'' electrons are found more commonly in certain areas of the atom become complex very quickly, as the probabilities are based in principles of [[quantum mechanics]].<ref>J.Kotz, J.Townsend, P.Treichel. (May 15, 2015). Chemistry and Chemical Reactivity, 8th ed. Belmont, CA, U.S.A: Brooks/Cole, 2012.</ref>

Simple understandings of orbitals describe the areas where electrons can be found as "layers" in a cloud of electrons, spherical areas where electrons are more likely to be found. However, quantum mechanics describes these orbitals quite differently, including values known as '''quantum numbers''' to describe the size and shape of these orbitals. The orbital that an electron lies within determines the [[energy]] that the electron has, and orbitals that result in two electrons having the same energy while being in a different orbital are referred to as '''degenerate'''.<ref name="RE1"/>

Although orbitals are complex, their structure can explain properties of some matter. For example, by knowing whether or not an orbital is full (each has room for two electrons),half full or empty determines the stability of an [[element]] since the orbitals "want" to be full or half full. For example, an element like [[copper]] is a stable element.<ref name="RE1">UC Davis Chemwiki. (May 15, 2015). ''Electronic Orbitals'' [Online]. Available: http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals</ref> In addition to this, many of the periodic properties of certain elements and the properties that families of elements have is caused by how these orbitals are filled with electrons.<ref>HyperPhysics. (May 15, 2015). ''Visualizing Electron Orbitals'' [Online]. Available: http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html</ref>

To learn more about orbitals from a chemistry perspective, see [http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals UC Davis' Chemwiki].

To learn more about orbitals from a physics perspective, see [http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/eleorb.html Hyperphysics].

==References==
{{reflist}}
[[Category:Uploaded]]