Jmdonev: 1 revision imported

2026-08-04T20:43:53Z

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energy>Jmdonev at 05:27, 30 July 2026

2026-07-30T05:27:06Z

← Older revision		Revision as of 05:27, 30 July 2026
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	[[Category:Done ~~2017~~-07-01]]		[[Category:Done 2026-08-01]]
	[[File:3D_model_hydrogen_bonds_in_water.png\|250px\|thumb\|Figure 1. A depiction of hydrogen bonding between water molecules. <ref>Wikimedia Commons [Online], Available: https://commons.wikimedia.org/wiki/File:3D_model_hydrogen_bonds_in_water.svg</ref>]]		[[File:3D_model_hydrogen_bonds_in_water.png\|250px\|thumb\|Figure 1. A depiction of hydrogen bonding between water molecules. <ref>Wikimedia Commons [Online], Available: https://commons.wikimedia.org/wiki/File:3D_model_hydrogen_bonds_in_water.svg</ref>]]

	<onlyinclude>A '''hydrogen bond''' is an attraction between [[molecule]]s (an ''~~intermolecular~~ attraction''). Hydrogen bonds can form between molecules that have C-H, N-H, Cl-H, and F-H [[chemical bond\|bonds]]. </onlyinclude>		<onlyinclude>A '''hydrogen bond''' is an attraction between [[molecule]]s (an '''''inter'''molecular attraction''). Hydrogen bonds can form between molecules that have N-H, O-H, F-H, and Cl-H [[chemical bond\|bonds]]. </onlyinclude>

	A hydrogen bond is not a "bond" in the same sense as the [[chemical bond]]s that hold the atoms in a molecule together. They are about 10-100 times weaker than a covalent bond<ref>Silberberg et al., "Chemistry: The Molecular Nature of Matter and Change, 2nd Canadian Ed.", McGraw Hill, 2016.</ref> ~~(although~~ stronger than other attractions ~~between molecules)~~. A hydrogen bond can occur between molecules when the molecules are ''polar'' (they have an [[electric dipole]]) and the dipole involves a ~~bond to~~ a ~~hydrogen~~ atom. The slight positive and slight negative ~~of the dipoles~~ in two different molecules attract the molecules to each other.		A hydrogen bond is '''not''' a "bond" in the same sense as the [[chemical bond]]s that hold the atoms in a molecule together. They are about 10-100 times weaker than a covalent bond (an ''intra''molecular bond),<ref>Silberberg et al., "Chemistry: The Molecular Nature of Matter and Change, 2nd Canadian Ed.", McGraw Hill, 2016.</ref> but they are stronger than other ''inter''molecular attractions. A hydrogen bond can occur between molecules when the molecules are ''polar'' (they have an [[electric dipole]]) and the dipole involves a hydrogen atom covalently bonding with a very electronegative atom such as Nitrogen, Oxygen, or Fluorine. The slight positive and slight negative dipole moments in two different molecules attract the molecules to each other, as seen in Figure 1.

	Compared to compounds that cannot hydrogen bond, compounds that do hydrogen ~~bond~~ with each other will have higher [[boiling point]]s and [[melting point]]s. ~~The presence of~~ strong ~~hydrogen bonds in [[water]] explains many of its unique properties - it is~~ a [[~~liquid]~~] ~~at room [[temperature~~]~~], when most other~~ molecules ~~of a similar size are [[gas]]es~~.		Compared to compounds that cannot hydrogen bond, compounds that do participate in hydrogen bonding with each other will have higher [[boiling point]]s and [[melting point]]s. These higher boiling and melting points are due to the strong ''inter''molecular forces, which translate to a higher [[specific heat capacity]] because those stronger forces between the molecules require more energy to overcome.

	To learn more about hydrogen bonds, see the [https://chem.libretexts.org/Textbook_Maps/General_Chemistry_Textbook_Maps/Map%3A_Chem1_(Lower)/07%3A_Solids_and_Liquids/7.03%3A_Hydrogen-Bonding_and_Water Chemistry LibreText] page.		The presence of strong hydrogen bonds in [[water]] explains many of its unique properties. Water is a [[liquid]] at room [[temperature]], when most other molecules of a similar size are [[gas]]es. It also exhibits a high specific heat capacity, which explains its ability to regulate temperature.

			To learn more about hydrogen bonds, see the [https://chem.libretexts.org/Textbook_Maps/General_Chemistry_Textbook_Maps/Map%3A_Chem1_(Lower)/07%3A_Solids_and_Liquids/7.03%3A_Hydrogen-Bonding_and_Water Chemistry LibreText] page about hydrogen-bonding and water.

			== For Further Reading ==

			* [[Molecule]]
			* [[Electric dipole]]
			* [[Specific heat capacity]]
			* [[Water]]
			* [[Chemical bond]]
			* Or explore a [[Special:Random\|random page]]

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

Jmdonev: 1 revision imported

2017-08-29T01:47:39Z

1 revision imported

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Jmdonev at 00:26, 28 August 2017

2017-08-28T00:26:34Z

New page

[[Category:Done 2017-07-01]]
[[File:3D_model_hydrogen_bonds_in_water.png|250px|thumb|Figure 1. A depiction of hydrogen bonding between water molecules. <ref>Wikimedia Commons [Online], Available: https://commons.wikimedia.org/wiki/File:3D_model_hydrogen_bonds_in_water.svg</ref>]]

<onlyinclude>A '''hydrogen bond''' is an attraction between [[molecule]]s (an ''intermolecular attraction''). Hydrogen bonds can form between molecules that have C-H, N-H, Cl-H, and F-H [[chemical bond|bonds]]. </onlyinclude>

A hydrogen bond is not a "bond" in the same sense as the [[chemical bond]]s that hold the atoms in a molecule together. They are about 10-100 times weaker than a covalent bond<ref>Silberberg et al., "Chemistry: The Molecular Nature of Matter and Change, 2nd Canadian Ed.", McGraw Hill, 2016.</ref> (although stronger than other attractions between molecules). A hydrogen bond can occur between molecules when the molecules are ''polar'' (they have an [[electric dipole]]) and the dipole involves a bond to a hydrogen atom. The slight positive and slight negative of the dipoles in two different molecules attract the molecules to each other.

Compared to compounds that cannot hydrogen bond, compounds that do hydrogen bond with each other will have higher [[boiling point]]s and [[melting point]]s. The presence of strong hydrogen bonds in [[water]] explains many of its unique properties - it is a [[liquid]] at room [[temperature]], when most other molecules of a similar size are [[gas]]es.

To learn more about hydrogen bonds, see the [https://chem.libretexts.org/Textbook_Maps/General_Chemistry_Textbook_Maps/Map%3A_Chem1_(Lower)/07%3A_Solids_and_Liquids/7.03%3A_Hydrogen-Bonding_and_Water Chemistry LibreText] page.

==References==
{{reflist}}

Hydrogen bond - Revision history

Jmdonev: 1 revision imported

energy>Jmdonev at 05:27, 30 July 2026

Jmdonev: 1 revision imported

Jmdonev at 00:26, 28 August 2017