Valence and core electrons - Revision history

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energy>Jmdonev at 22:30, 19 October 2021

2021-10-19T22:30:19Z

← Older revision		Revision as of 22:30, 19 October 2021
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	[[Category:Done ~~2018~~-06-01]]		[[Category:Done 2021-10-29]]
	[[File:Valence.png\|thumbnail\|300px\|right\|Figure 1: The two yellow electrons on the outermost oval are the '''valence electrons'''; the other 10 electrons are '''core electrons'''.<ref>This image was created by part of the [[Who_we_are\| Energy Education team]].</ref> This picture does not address the [[quantum mechanics]] of electrons around atoms.]]		[[File:Valence.png\|thumbnail\|300px\|right\|Figure 1: The two yellow electrons on the outermost oval are the '''valence electrons'''; the other 10 electrons are '''core electrons'''.<ref>This image was created by part of the [[Who_we_are\| Energy Education team]].</ref> This picture does not address the [[quantum mechanics]] of electrons around atoms.]]
	Electrons exist in [[orbital]]s around a [[nucleus]]. These orbitals and the energy needed to remove each of these electrons from the atom are set by [[quantum mechanics]]. Each of these orbitals serves to create a shell of [[electron]]s in the [[atom]].		Electrons exist in [[orbital]]s around a [[nucleus]]. These orbitals and the energy needed to remove each of these electrons from the atom are set by [[quantum mechanics]]. Each of these orbitals serves to create a shell of [[electron]]s in the [[atom]].
	<onlyinclude>'''Valence electrons''' are the electrons orbiting the nucleus in the outermost atomic shell of an atom. Electrons that are closer to the nucleus are in filled orbitals and are called '''core electrons'''.</onlyinclude> Valence electrons are the farthest from the positive [[charge]] (the [[proton]]s) and thus tend to be easier to remove than core electrons; this means that it takes them less [[energy]] to move far away from the atom. This difference comes from the [[electric force]] being an [[inverse square law]]. ~~Removing an electron~~ (~~any of them~~) ~~from a neutral atom turns~~ the ~~atom into an [[ion]]~~.		<onlyinclude>'''Valence electrons''' are the electrons orbiting the nucleus in the outermost atomic shell of an atom. Electrons that are closer to the nucleus are in filled orbitals and are called '''core electrons'''.</onlyinclude> Valence electrons are the farthest from the positive [[charge]] (the [[proton]]s) and thus tend to be easier to remove than core electrons; this means that it takes them less [[energy]] to move far away from the atom. This difference comes from the [[electric force]] being an [[inverse square law]]. In addition, core electrons in the inner shells have lower energy levels than the valence electrons occupying the outer shell. This means that electrons in the inner shells can absorb bits of energy and move (jump) to the valence electron shell.

	Valence electrons ~~also tend to be~~ the electrons ~~that specifically participate in~~ a [[~~chemical bond~~]], ~~like ionic bonds or covalent bonds~~.		===Valence electrons and [[chemical reaction]]s===
			In chemical reactions, the electrons can even break free from the valence shell. This can be to create an [[ionic bond]] or to become an [[ion]]. When an electron leaves a neutral atom, it loses a negative charge and turns into a positively charged [[ion]]. For example, sodium (Na) has one electron in it's outer shell. Thus it wants to lose a single electron and become an Na<sup>+</sup> ion. An atom can also gain an electron (usually to fill it's valence shell) and turn into a negatively charged ion. This can be seen with Chlorine, which in it's neutral state is missing one electron in it's valence electron shell. Thus, it wants to pick up an electron and become a Cl<sup>-</sup> ion.<ref name=val>"Valence electrons and open valences." Chemistry LibreTexts, 2019. [Online]. Available: https://chem.libretexts.org/@go/page/16945. [Accessed: May 15, 2021]</ref>

	~~For more information about~~ valence electrons, ~~core~~ electrons and ~~how~~ they ~~related to~~ [[~~chemical reaction~~]]~~s please see UC Davis's~~ [~~http://chemwiki.ucdavis.edu/Wikitexts/UC_Davis/UCD_Chem_124A%3A_Kauzlarich/ChemWiki_Module_Topics/Valence_and_Core_Electrons chem wiki~~].		[[Noble gas]]es are elements that have a full valence shell, meaning that the outer shell is completely filled with electrons. Noble gases neither want to gain or lose an electron, which means they tend to be chemically [[inert]] (unreactive). In general, atoms want to have full valence electron shells. This is why atoms, and also chemical compounds, lose or gain electrons to become ions, and also why they form [[ionic bond\|ionic]] and [[covalent bond]]s.

			===Valence electrons and [[chemical bond\|chemical bonding]]===
			[[File:sigma_bond.png\|300px\|thumb\|framed\|Figure 2: Depiction of the covalent sigma bonds in [[Ethane]]. Valence electron pairs are being shared between the carbon atoms to create a single carbon-carbon bond.<ref>"Illustrated Glossary of Organic Chemistry." UCLA College. Online. Available: http://www.chem.ucla.edu/~harding/IGOC/S/sigma_bond.html.</ref>]]
			In both ionic and covalent bonding, it is the valence electrons that participate these [[chemical bond]]s.<ref name=val/> In single [[covalent bond]]s, typically both atoms in the bond contribute one valence electron each in order to form a shared [[electron pair]]. An example is seen in figure 2 where a strong sigma bond (σ bond) is formed. Valence electrons are also used to form double and triple bonds, which have valence electrons configured in pi bonds (π bonds).<ref name=bond/>

			In [[ionic bond\|ionic bonding]], valence electrons are completely transferred between [[atom]]s. It is a type of chemical bond that generates two oppositely charged ions, one [[anion]] and one [[cation]]. Ionic bonding is observed because [[metal]]s have few electrons in their valence [[orbital]]s and [[nonmetal]]s almost have 8 electrons in their valence shells. Metals lose their valence electrons and become more stable by satisfying the octet rule. Similarly, nonmetals will readily accept electrons to achieve a [[noble gas]] configuration.<ref name=bond>"Ionic and Covalent Bonds," Chemistry LibreTexts, 2020. Online. Available: https://chem.libretexts.org/@go/page/839.</ref>

			For more information about valence electrons, core electrons and how they related to [[chemical reaction]]s please see UC Davis's [https://chem.libretexts.org/@go/page/2606 chem wiki].

			==For Further Reading==
			*[[Atom]]
			*[[Electron]]
			*[[Ion]]
			*[[Nucleus]]
			*Or explore a [[Special:Random\|random page]]
	==References==		==References==
	{{reflist}}		{{reflist}}
	[[Category:Uploaded]]		[[Category:Uploaded]]

Jmdonev: 1 revision imported: Doing upload, largely of old redirects.

2018-06-04T16:52:33Z

1 revision imported: Doing upload, largely of old redirects.

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Jmdonev at 22:22, 1 June 2018

2018-06-01T22:22:54Z

← Older revision		Revision as of 22:22, 1 June 2018
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	[[Category:Done ~~2015~~-06-01]]		[[Category:Done 2018-06-01]]
	[[File:Valence.png\|thumbnail\|300px\|right\|Figure 1: The two yellow electrons on the outermost oval are the '''valence electrons'''; the other 10 electrons are '''core electrons'''.<ref>This image was created by part of the [[Who_we_are\| Energy Education team]].</ref> This picture does not address the [[quantum mechanics]] of electrons around atoms.]]		[[File:Valence.png\|thumbnail\|300px\|right\|Figure 1: The two yellow electrons on the outermost oval are the '''valence electrons'''; the other 10 electrons are '''core electrons'''.<ref>This image was created by part of the [[Who_we_are\| Energy Education team]].</ref> This picture does not address the [[quantum mechanics]] of electrons around atoms.]]
	Electrons exist in [[orbital]]s around a [[nucleus]]. These orbitals and the ~~associated~~ energy needed to remove each of these electrons are set by [[quantum mechanics]]. Each of these orbitals serves to create a shell of [[electron]]s in the [[atom]].		Electrons exist in [[orbital]]s around a [[nucleus]]. These orbitals and the energy needed to remove each of these electrons from the atom are set by [[quantum mechanics]]. Each of these orbitals serves to create a shell of [[electron]]s in the [[atom]].
	<onlyinclude>'''Valence electrons''' are the electrons orbiting the nucleus in the outermost atomic shell of an atom. Electrons that are closer to the nucleus are in filled orbitals and are called '''core electrons'''.</onlyinclude> Valence electrons are the farthest from the positive [[charge]] (the [[proton]]s) and thus tend to be easier to remove than core electrons; this means that it takes them less [[energy]] to move far away from the atom. This difference comes from the [[electric force]] being an [[inverse square law]]. Removing an electron (any of them) from a neutral atom turns the atom into an [[ion]].		<onlyinclude>'''Valence electrons''' are the electrons orbiting the nucleus in the outermost atomic shell of an atom. Electrons that are closer to the nucleus are in filled orbitals and are called '''core electrons'''.</onlyinclude> Valence electrons are the farthest from the positive [[charge]] (the [[proton]]s) and thus tend to be easier to remove than core electrons; this means that it takes them less [[energy]] to move far away from the atom. This difference comes from the [[electric force]] being an [[inverse square law]]. Removing an electron (any of them) from a neutral atom turns the atom into an [[ion]].

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	==References==		==References==

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

J.williams: 1 revision imported

2015-08-26T21:31:46Z

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J.williams at 17:00, 12 August 2015

2015-08-12T17:00:27Z

New page

[[Category:Done 2015-06-01]]
[[File:Valence.png|thumbnail|300px|right|Figure 1: The two yellow electrons on the outermost oval are the '''valence electrons'''; the other 10 electrons are '''core electrons'''.<ref>This image was created by part of the [[Who_we_are| Energy Education team]].</ref> This picture does not address the [[quantum mechanics]] of electrons around atoms.]]
Electrons exist in [[orbital]]s around a [[nucleus]]. These orbitals and the associated energy needed to remove each of these electrons are set by [[quantum mechanics]]. Each of these orbitals serves to create a shell of [[electron]]s in the [[atom]].
<onlyinclude>'''Valence electrons''' are the electrons orbiting the nucleus in the outermost atomic shell of an atom. Electrons that are closer to the nucleus are in filled orbitals and are called '''core electrons'''.</onlyinclude> Valence electrons are the farthest from the positive [[charge]] (the [[proton]]s) and thus tend to be easier to remove than core electrons; this means that it takes them less [[energy]] to move far away from the atom. This difference comes from the [[electric force]] being an [[inverse square law]]. Removing an electron (any of them) from a neutral atom turns the atom into an [[ion]].

Valence electrons also tend to be the electrons that specifically participate in a [[chemical bond]], like ionic bonds or covalent bonds.

For more information about valence electrons, core electrons and how they related to [[chemical reaction]]s please see UC Davis's [http://chemwiki.ucdavis.edu/Wikitexts/UC_Davis/UCD_Chem_124A%3A_Kauzlarich/ChemWiki_Module_Topics/Valence_and_Core_Electrons chem wiki].

==References==

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