Covalent Bonds - Revision history

Entr0py at 14:37, 2 December 2024

2024-12-02T14:37:01Z

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	[[https://drive.google.com/file/d/1J4DUDLtbsgmnibLhhBHSVXHsUFseuIqD/view?usp=sharing\|Thumb\|A table of common covalent bonds and their bond energies, found in https://openstax.org/books/chemistry-atoms-first-2e/pages/9-4-strengths-of-ionic-and-covalent-bonds]]		[[https://drive.google.com/file/d/1J4DUDLtbsgmnibLhhBHSVXHsUFseuIqD/view?usp=sharing\|Thumb\|A table of common covalent bonds and their bond energies, found in https://openstax.org/books/chemistry-atoms-first-2e/pages/9-4-strengths-of-ionic-and-covalent-bonds]]

			The potential energy associated with a covalent bond follows the familiar shape derived from applying quantum theory to [[Molecules]].

			[[File:Cov_Pot.gif]]

	===A Computational Model===		===A Computational Model===

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History

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	==History==		==History==

	While it was not coined as covalent bonding until 1919 by Irving Langmuir, the theory of the ability for two atoms to share a pair of electrons can be traced back to Gilbert N. Lewis in 1916, who proposed that atoms would bond to each other in order to fill empty energy shells, thus causing them to no longer have any valence electrons. It was also Lewis who created dot notation, commonly used to indicate how many electrons an atom has and how many of those electrons are alone rather than being part of a pair. Much later, in 1927, Walter Heitler and Fritz London proposed the first quantum explanation for covalence, arguing that the bonds are created by the overlapping of electron orbitals.		While it was not coined as covalent bonding until 1919 by Irving Langmuir, the theory of the ability for two atoms to share a pair of electrons can be traced back to Gilbert N. Lewis in 1916, who proposed that atoms would bond to each other in order to fill empty energy shells, thus causing them to no longer have any valence electrons. It was also Lewis who created dot notation, commonly used to indicate how many electrons an atom has and how many of those electrons are alone rather than being part of a pair. He also studied thermodynamics and the law of conservation of energy. Much later, in 1927, Walter Heitler and Fritz London proposed the first quantum explanation for covalence, arguing that the bonds are created by the overlapping of electron orbitals.

	== See also ==		== See also ==

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References

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	https://openstax.org/books/chemistry-atoms-first-2e/pages/9-4-strengths-of-ionic-and-covalent-bonds		https://openstax.org/books/chemistry-atoms-first-2e/pages/9-4-strengths-of-ionic-and-covalent-bonds

			https://www.youtube.com/watch?v=IrSnJfc94pg

Eapalkova3: /* Further reading */

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Eapalkova3: /* Further reading */

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Connectedness

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	==Connectedness==		==Connectedness==
	#How is this topic connected to something that you are interested in?		#How is this topic connected to something that you are interested in?
	* I personally have always been fascinated with ~~genetics~~ and how ~~it could~~ be ~~altered~~, ~~and since~~ the ~~different nucleotides are all very similar in their chemical makeup~~, ~~I hope~~ that ~~our~~ understanding of ~~how to cause the formation or destruction of these~~ bonds ~~can eventually allow~~ us to ~~alter nucleotides, and thus alter someone's genetic code, for example to cure a form of cancer~~.		* I personally have always been fascinated with pharmaceuticals and how so many different and useful drugs can be created through the simple breaking and forming of covalent bonds. For example, the everyday drug that we use as a painkiller, acetaminophen is actually a fairly basic organic compound that can be created by forming and phenol group and an amide with a covalent bond. Also, better understanding of breaking covalent bonds could help us further chemotherapy related drugs to better target only cancerous cells.

	#How is it connected to your major?		#How is it connected to your major?
	* The bonding of different atoms together can greatly alter their chemical and physical properties, and thus is responsible for much of the world around us and the events we witness within it. For example, "hydrogen bonding" between water molecules, that being how they attract and repel each other when at different orientations due to their polarity, greatly affects the pattern into which it solidifies, in this specific case causing ice, the solid form of water, to actually be less dense than liquid water. Not only is this an abnormal physical characteristic, it is also likely a major reason complex life was able to develop on Earth, since only the surface of the oceans would freeze during ice ages rather than their entirety, allowing life to grow under the insulating layer.		* The bonding of different atoms together can greatly alter their chemical and physical properties, and thus is responsible for much of the world around us and the events we witness within it. For example, "hydrogen bonding" between water molecules, that being how they attract and repel each other when at different orientations due to their polarity, greatly affects the pattern into which it solidifies, in this specific case causing ice, the solid form of water, to actually be less dense than liquid water. Not only is this an abnormal physical characteristic, it is also likely a major reason complex life was able to develop on Earth, since only the surface of the oceans would freeze during ice ages rather than their entirety, allowing life to grow under the insulating layer.

	#Is there an interesting industrial application?		#Is there an interesting industrial application?
	* The ability to trigger the formation of covalent bonds has allowed researchers to synthesize artificial DNA.		* The ability to trigger the formation of covalent bonds has allowed researchers to synthesize artificial DNA.
			* Covalent bonds can also be applied to gases and petroleum. Gas is held together by covalent bonds and our world runs on the use of gases and petroleum.

	==History==		==History==

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Difficult

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 ===Difficult===
-Calculate the enthalpy change 2C2H6+5O2->4CO2+6H2O
+Calculate the enthalpy change 2C2H6+7O2->4CO2+6H2O
 ==Connectedness==

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Difficult

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	===Difficult===		===Difficult===
	Calculate the enthalpy change ~~H2O(l)~~->~~H2O(g)~~		Calculate the enthalpy change 2C2H6+5O2->4CO2+6H2O
	~~H20(l) has~~

	==Connectedness==		==Connectedness==

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Difficult

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	===Difficult===		===Difficult===
	~~calculate~~ the enthalpy~~...~~		Calculate the enthalpy change H2O(l)->H2O(g)
			H20(l) has

	==Connectedness==		==Connectedness==

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	== See also ==		== See also ==
			Covalent bonds also tie into the subject of molecules because these bonds are found within molecules, specifically between the atoms. This is all on the atomic level so this can also tie into atomic and quantum theory as well as energy levels.
	~~Are there related topics or categories in this wiki resource for~~ the ~~curious reader to explore? How does~~ this ~~topic fit~~ into ~~that context?~~

	[https://www.physicsbook.gatech.edu/Molecules/ Molecules]		[https://www.physicsbook.gatech.edu/Molecules/ Molecules]

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	===Further reading===		===Further reading===
			These readings delve into intermolecular and intramolecular forces and how these forces have further types with varying strengths based on components such as the types of atoms in the molecule and the electronegativity.
	https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/03%3A_Compounds/3.09%3A_Intramolecular_forces_and_intermolecular_forces		https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/03%3A_Compounds/3.09%3A_Intramolecular_forces_and_intermolecular_forces
	https://www.masterorganicchemistry.com/2010/10/01/how-intermolecular-forces-affect-boiling-points/#:~:text=There%20are%20four%20major%20classes,of%20%E2%80%9Copposite%20charges%20attract%E2%80%9D.&text=The%20four%20key%20intermolecular%20forces,Van%20der%20Waals%20dispersion%20forces.		https://www.masterorganicchemistry.com/2010/10/01/how-intermolecular-forces-affect-boiling-points/#:~:text=There%20are%20four%20major%20classes,of%20%E2%80%9Copposite%20charges%20attract%E2%80%9D.&text=The%20four%20key%20intermolecular%20forces,Van%20der%20Waals%20dispersion%20forces.
	These readings delve into intermolecular and intramolecular forces and how these forces have further types with varying strengths based on components such as the types of atoms in the molecule and the electronegativity.

	===External links===		===External links===

← Older revision		Revision as of 22:43, 24 July 2022
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	https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/03%3A_Compounds/3.09%3A_Intramolecular_forces_and_intermolecular_forces		https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/03%3A_Compounds/3.09%3A_Intramolecular_forces_and_intermolecular_forces
	https://www.masterorganicchemistry.com/2010/10/01/how-intermolecular-forces-affect-boiling-points/#:~:text=There%20are%20four%20major%20classes,of%20%E2%80%9Copposite%20charges%20attract%E2%80%9D.&text=The%20four%20key%20intermolecular%20forces,Van%20der%20Waals%20dispersion%20forces.		https://www.masterorganicchemistry.com/2010/10/01/how-intermolecular-forces-affect-boiling-points/#:~:text=There%20are%20four%20major%20classes,of%20%E2%80%9Copposite%20charges%20attract%E2%80%9D.&text=The%20four%20key%20intermolecular%20forces,Van%20der%20Waals%20dispersion%20forces.
			These readings delve into intermolecular and intramolecular forces and how these forces have further types with varying strengths based on components such as the types of atoms in the molecule and the electronegativity.

	===External links===		===External links===