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English to be acceptable, so I would not favor just putting it back in as is. But the edit does make the important point that we have little mention of orbital overlap and no mention of the difference between s-s, s-p and p-p direct and lateral overlap, i.e. sigma and pi bonds (though the edit didn't use those terms). So I think we need to insert a revised version of this edit to insert the important points, with the flaws fixed and possibly better integrated into the article. I will try to get to this soon if no one else does first.
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do well to have the difference between cis and trans included in their curiculum. Most people won't want to go on and delve into an article about IUPAC naming rules or about alkenes, and yet they're liable to encounter "trans fat" and "trans double bond" and wish they knew what it meant. The stuff about lipids belongs in an article about lipids or fats, I think.
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better description, or fix it. I am not clueless about chemistry, but I felt like I was, looking at that picture! What do those dashed lines and non-dashed lines mean? And what is the significance of the angles? And, okay, so those arrows are electrons, but...what do they mean??? You got three going one way and one going the other way... --
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used are perp. to each other, so when you rotate it, then there will be at least some orbital overlap. Compare that to a double bond where when you rotate it 90 degrees, then there is no pi overlap at all. That's what I seem to remember from gen chem, but I can't find any notes on it or any external refs either.
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First, I have moved this new section to the bottom of the talk page. From your examples, I think you meant to say that macro-molecular structures CAN have an UNlimited number of atoms, which is correct. Proteins have a large but definite number of atoms - for example all hemoglobin molecules have the
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Does anyone have plans for an
Electron Dot Notation article? A seperate, improved article would be useful. It would need step by step instructions, ect. Alternatively, someone could link the Electron Dot Notation page to this one, but that would be slightly inadequate I'd do it myself, but I'm laking
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I forgot about network covalent which does sound more scientific and more clearly excludes chain macromolecules. A fast Google search gives 17 900 hits for "giant covalent" and "10 900" for "network covalent". More technical papers I suspect would more often favor "network covalent" though I haven't
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Sorry, but this article strikes me as rather poorly written, and, sorry again, I am not the guy to make the corrections. I hope someone more qualified agrees and takes the necessary steps. But that first picture!!--what a useless piece that is! Does ANYONE know what it means? If so, please give it a
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I thought that this was relavant to the article, so I put a couple of sentences in on it. I wanted to make sure with someone else on this before I put it in though: Is a triple bond less rigid than a double bond in terms of rotation? I would think so because in a triple bond, the pi orbitals being
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I don't doubt that there would be a steric issue with a fourth bond, but I still don't see the "left, right, and up" in a triple bond. The two π-bonds are at right angles to each other, so "left" and "right" doesn't make sense to me. I don't understand in what sense the σ-bond is "shunted upwards"
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I encourage you to indulge yourself, but I do think it would be nice to keep a linked mention of cis and trans in there somehow, because people encounter these terms all the time now with "trans fats" in the news, and so I think even somebody who is just at the stage of learning what a bond is would
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This page uses diborane as an example of an electron deficient compound, while the main
Knowledge page on electron deficiency explicitly states it is not. I do not have enough knowledge of the matter to decide which is true, but this conflicting information should be corrected by someone who does.
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Yes, it is true that most (though not all) authors distinguish macromolecular and giant covalent. And I agree that this distinction will be useful to many readers so I will mention the difference in the
Covalent structures section. Also I don't think there is any unanimity about three types (as the
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My school taught us that macro-molecular structure have a limited no. of atoms.For example protein, starch etc. graphite, diamond and quartz should be giant covalent structure which has no end. Am I right? if it's correct I'll change it. PS my chinese username won't show sorreh 13:24, 21 September
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The first sentence of the article currently reads "A covalent bond is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms, and other covalent bonds." So "a covalent bond" is defined (partly) in terms of "other covalent bonds"? That seems circular...
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would be a σ-bond and three π-bonds. The σ-bond forms directly between the two carbon atoms, but is shunted upwards by the repulsive force of the two π-bonds to the left and right (hence left, right and up). The third π-bond would have to bend all these bonds excessively, leading to instability. I
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I think that there is some useful material in the new section
Directional Property of the Covalent Bond, added today by editor 1.39.13.71 and deleted a few minutes later by Material Scientist. It is true that the editor is inexperienced and that this edit required revisions to both formatting and
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Maybe the C–C bond 1,1,1-trifluoroethane is a cleaner example? Due to the high electronegativty of F, C1 would be quite δ+, whereas C2 would not be. But by adding partial charges, one could argue that the effective electronegativity of the carbon atoms has changed. Semi-equivalently, one could
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is a bad, or better, a too difficult, example, polarity in that molecule is for a different reason than electrons not being 'shared equally'. Ozone has two resonance structures. But either do not exist, the electrons are equally shared between the bonds (Lewis structures are only a model). The
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Sources are probaly their teachers instead of qualified scientists. The problem comes with the fact that there is no real line bewtween covalent and ionic bonding (there is a formal defination but thats just to make it easier to communicate). Also, how do you define bond strength and what two
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giant covalent are distinguished by their structure. Giant covalent substance's atoms usually form bonds with more than 1 other atom(eg each silicon or diamond(carbon)atom joins to 4 other. each graphite atom joins 3 other. In SiO2, each
Silicon atom joins 4 Oxygen atom,while each oxygen joins
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In the second paragraph, where the types of covalent bond are listed, each type includes a hyperlink to the appropriate
Knowledge page except the words "Metal-to-Metal bonding". I cannot add the edit myself since this page is locked, would someone can please hyperlink the text "Metal-to-Metal
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Many major chemical supply houses sell several noble-gas compounds: anyone with a moderate lab could make some and they have known synthetic uses...no longer really that unique or totally exotic. Please don't confuse "found in nature" with...well with anything that has much meaning about the
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The page for unsaturated bond redirects here.. but this page does not say anything about unsaturated bond. Maybe to chemistry students, this might be obvious, but as a public encyclopedia it should be clear exactly how this page relates to an unsaturated bond. as it is this page gives me no
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The last three noble gases can be "forced" into compounds. I will list these and their electronegativities(just to show what they would be bonding with covalently), however, please note that these compounds do not happen in nature, so are pretty much irrelevent to this article, also, these
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Diborane has always been described as an electron deficient compound because there are 4 "bonds" in the central ring and only 4 electrons. more recently it has been seen as perfectly normal, but the "electron deficient" tag remains. It depends how you define "electron deficient".
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I don't see what this is trying to convey. The two pi bonds are at right angles to each other, looking down the bond axis, and the sigma bond is symmetric about the axis, or straight ahead if you like. Where does "left, right, and up" come from? Which one is the sigma bond?
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is normally described as having a double or maybe triple bond - it isn't explosive, merely unstable. Quadruple and higher bonds get described for esoteric transition metal compounds, but that's it. So, unless someone has good reference sources to show otherwise, I'll chop it
1369:”. This is not common terminology and I cannot find any reputable source which uses it. The IUPAC gold book (and every other colored IUPAC book) has no mention of it. Moreover, it is a gross misnomer, as a “molecular bond” implies a bond between molecules, i.e. it is an
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Bond order as defined currently is usefully general; when defined as the difference between bonding and antibonding electrons it is specific to simple molecular orbital theory. And as written, the mention of sigma and pi bonds is correct, and fits with high school
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I just have a question, maybe you all can help me!..What is an example of a
Covalent Bond and explain what is happening at the atomic level during bonding?.... im doing a chemisrty paper and that is one of the questions, if you know the answer.. please tell mee!
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consider that the bond is really between "the carbon on a methyl group" and "the carbon on a trifluoromethyl group", not just between two carbons, so the electronegativity difference of the group is what matters, not just the specific bonded atoms.
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molecular-bonds, and are never (correctly) referred to as “molecular bonds”. If there is no citation for who calls these molecular bonds, this should be removed to avoid father confusion for new chemists, which is recurring due to this inaccuracy.
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I've just axed it. This article is about covalent bonding, and that was talking very specifically about the bonding in fatty acids. cis and trans is something much more general than that, I don't think that the description there helped much.
331:"Atoms tend to share electrons in such a way that their outer electron shells are filled." Isn't that misleading, given that the stable number of 8 electrons is not the maximum number of electrons that can fit in the third shell and beyond?
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1000°C) are often much higher than macromolecular(~300-600°C). In macromolecular, the structure is basically more like a linear chain of atoms with branches instead of a 3D network. It is a big difference. Maybe consider not mixing them
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In those books, bond order is half the difference of the nuber of electrons in the bonding and those in the antibonding state. Example: A bond order of 1 means: Two electrons in the bonding and none in the antibonding state.
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Actually, the energy gap for the right image should be smaller, since there is poorer size and symmetry overlap between both participating atomic orbitals (as defined by polar covalent). All things being equal, of course.
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I've learned that ionic bonds are stronger than covalent bonds, since the ions have a greater amount of attraction between them. Can the person who stated that covalent bonds are stronger cite their sources?
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No. that's not what I meant. What I meant is that the example in the article may be wrong. Quartz, diamond, graphite are giant covalent NOT macro-molecular. Starch, plastic, protein are macro-molecular.
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Straight- or normal-chain (even-numbered), monoenoic components, i.e. with one double bond, make up a high proportion of the total fatty acids in most natural lipids. Normally the double bond is of the
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Ahem...the picture seems to show a CH4 molecule but says "ethene". Don't want to mess with the picture (I'm not great at graphics) but would some other Most
Honorable Wikipedian care to look after it?
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939:"Some examples of Electron Dot Notation are shown in the following figure. An alternative form, in which bond-forming electron pairs are represented as solid lines, is shown alongside."
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How is it possible for noble gases to bond if their electron shell is full? I know noble gases can form compounds in special conditions, but it has to be impossible! Please answer!
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The kind of material is "network solid" (a redirect), focusing on the overall structure and properties rather than the facts of the bonds within it. That's another : -->
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Not to mention, it could be further defined into polar covalent and apolar covalent bonds, which although are redirected to this article, are in fact not discussed.
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I'm confused... I just studied from the Books of
Pettifor and Suttun. And they seem to define bond order as something very different, thatn what is the article.
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I would personally like to add a section on Lewis structures (aka. electron dot diagrams), polar and apolar covalent bonds, and co-ordinate covalent bonds.
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checked. So I think it is best to mention both names, with network covalent first as it is clearer and also corresponds to the name of another article.
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No one calls covalent bonds “molecular bonds”, and no one should. Please remove this erroneous statement given in the first sentence of this article.
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same structure. Your other examples - starch, graphite, diamond, quartz - do in fact have an unlimited number of atoms, so have no end as you say.
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Covalent bonds are more common between non-metals, whereas ionic bonding is more common between two metal atoms or a metal and a non-metal atom.
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However, most of my resources belong to the
University of Technology, Sydney, Australia. Thus, the resources are unavailable to the public.
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Wether the bond is sigma or pi doesn't have anything to do with bond order, but is determined by the angular momentum across the bond axis.
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I do wish someone who understands organic chemistry would clean this up, because I'd like to understand the solid line figures better.
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molecular-bond, such as hydrogen bonding or pi-pi interactions between neighboring molecules. Whereas covalent bonds are explicitly
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A correct way to say this would be middle, up and down and left and right, π bonds are "surronding" the σ bond at a straight angle.
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I don't know why this article says that covalent bonding is STRONGER than ionic bonding? This is incorrect... Unless Im mistaken
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double bond & triple bond both direct here but this page hardly contains info on these topics. Should they redirect to
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an idea: can we please have some examples of covalent bonds eg. the diatomic molecules of gases, water, carbon dioxide
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I'd like to second that the definition is unhelpful. I would fix it myself, but I came here to learn the definition!
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As there seems to be an article that specializes in talking about Valence bond theory and Molecular orbital theory (
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Also noticed that a page concerning the naming of covalent compounds, and indeed any naming conventions for all of
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What would be an example of an ionic bond between two metal atoms? This would require that a metal form an anion.
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as a student that is studying chemistry, I dont think the definition of the covalent bond is defined clearly.
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either; if it's direction is to be called "up" in a triple bond, it's "up" in a single or double bond too.
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at the time (June 3, 2020). There are suggestions below for improving the article. If you can improve it,
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Does the literature actually call these "giant covalent", or is that just a lay-language description for
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on 28 September 2005. For the contribution history and old versions of the redirected page, please see
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please insert a animated picture of sharing electron and differentiate it from transferring electron
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Okay, I was the one who put that there. I will retract it and talk about the polarity of ozone in
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on Knowledge. If you would like to participate, please visit the project page, where you can join
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article now says) or four types (if giant covalent is added), so I will just say several types.
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on 3 May 2015. For the contribution history and old versions of the redirected page, please see
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am, however, working on an A-level view of how bonds form, so please correct me if I'm wrong.
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Um-- The diagram is BAD considering quantum mechanics. The Bohr model of the atom is dead.
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polarity in this molecule is more the result of the molecule not being linear, but bent. --
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2. The 2nd sentence says "An alternative form... ..is shown alongside" - But it ISN'T!
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information and I am left completely in the dark as to what a unsaturated bond is.
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The three shared orbitals in a triple bond can be imaged as left, right, and up.
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Update: Moved back and converted chemical bonding model to a disambiguation.--
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I do not know any examples of these compounds, if anyone would be so kind...
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1. There's only one figure so it should say "An example" not "Some examples"
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Can u clearly write in the details what exactly you are trying to explain .
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Nobody complaint, so I at least made a stub instead of redirect. Please see
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should be made into real article, like they have it on other wikipedias:
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electronegativities are not very accurate, these are rough estimates...
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bonding" at the beginning of the second paragraph to the article at:
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Does much of anything even exist there? If so, then just link there.
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This seems completely out of place to me. I'm tempted to remove it.
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2).Giant covalent is usually a 3D network and its mp and bp (: -->
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In the para before you present the Lewis diagram, the text says:-
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Diborane: Electron deficient or not? (conflicting information)
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Requesting Hyperlink to Knowledge article on Metallic bonding
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diagram, and I must say it's actually quite well drawn. --
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Giant macromolecular covalent vs simple covalent molecular
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This article states that covalent bonds are “also called…
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Covalent bonding is usually stronger than ionic bonding.
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This usually yields the same result. Think about it. --
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Can you please clarify exactly what you are asking? --
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Covalent structures (macromolecular structure)problems
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I really think the reference to a quadruple bond for C
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Knowledge level-4 vital articles in Physical sciences
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That does seem not-very-useful. I just re-redirected
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Such "step by step instructions" is more suitable at
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1049:i don't understand covalent bonding. Help please.
135:, a collaborative effort to improve the coverage of
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1530:Knowledge vital articles in Physical sciences
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1285:https://en.m.wikipedia.org/Metallic_bonding
676:Could someone make the connection, please?
293:Anyone in favor of semi-locking this page?
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966:Noble gas covalent bonds? ???
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263:its talk page
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253:Covalent bond
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219:
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213:Covalent bond
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27:Covalent bond
25:
18:
17:
1490:
1455:
1411:— Preceding
1407:
1380:— Preceding
1374:
1370:
1366:
1364:
1325:
1288:
1281:
1130:— Preceding
1127:2015 (UTC)
1125:
1105:
1082:— Preceding
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814:— Preceding
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304:
301:'09 Comments
292:
289:'10 Comments
281:Old comments
242:
202:
170:
130:
90:WikiProjects
73:
33:good article
31:
30:
26:
1289:Thank you!
1051:—Preceding
1003:Radon: 2.4
1000:Xenon: 2.6
916:Rifleman 82
904:Rifleman 82
589:Josh Cherry
555:Josh Cherry
399:Josh Cherry
365:Josh Cherry
307:—Preceding
258:its history
218:its history
204:Shared pair
47:renominated
1509:Categories
1347:Officer781
1332:Officer781
627:Sareen eng
247:page were
207:page were
1185:together?
1035:instead?
980:Ronhjones
791:True.
784:Missy1234
680:Mouvement
648:EvilStorm
644:somewhere
485:Chemistry
460:wikibooks
436:Iridium77
420:Iridium77
350:Kosebamse
146:Chemistry
137:chemistry
109:Chemistry
78:is rated
43:please do
1425:contribs
1413:unsigned
1394:contribs
1382:unsigned
1144:contribs
1132:unsigned
1084:unsigned
1053:unsigned
885:Taquito1
816:unsigned
489:Pingveno
475:Pingveno
452:Pingveno
335:No, see
309:unsigned
1308:Dirac66
1293:Pharcsa
1235:Dirac66
1202:Dirac66
1155:Dirac66
1109:Dirac66
1033:pi-bond
611:soon!--
173:on the
80:B-class
1491:Voice
1306:Done.
1252:DMacks
1220:DMacks
1013:DMacks
953:Edetic
864:DMacks
841:Drag-5
767:DMacks
753:Spoon!
699:ideas.
690:Spoon!
602:and Si
537:(talk)
534:romanm
523:(talk)
520:romanm
464:Menchi
408:168...
249:merged
209:merged
86:scale.
1473:Bduke
1438:Bduke
1375:intra
1371:inter
1037:V8rik
734:ozone
391:trans
251:into
211:into
67:This
1497:talk
1477:talk
1462:talk
1442:talk
1421:talk
1390:talk
1351:talk
1336:talk
1312:talk
1297:talk
1256:talk
1239:talk
1224:talk
1206:talk
1191:talk
1174:talk
1159:talk
1140:talk
1113:talk
1092:talk
1061:talk
1041:talk
1017:talk
984:talk
957:talk
920:talk
908:talk
889:talk
868:talk
845:talk
824:talk
751:. --
663:Hi,
514:and
462:. --
317:talk
165:High
1187:榎本徑
1170:榎本徑
1136:榎本徑
858:to
701:Ian
613:Ian
387:cis
372:Ian
1511::
1499:)
1479:)
1464:)
1444:)
1436:--
1427:)
1423:•
1396:)
1392:•
1353:)
1338:)
1314:)
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1258:)
1241:)
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1218:?
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1176:)
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1142:•
1115:)
1094:)
1063:)
1043:)
1019:)
986:)
959:)
922:)
914:--
910:)
891:)
870:)
862:.
847:)
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646:?
510:,
319:)
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843:(
822:(
608:2
604:2
600:2
572:2
339:.
315:(
265:.
225:.
177:.
92::
49:.
Text is available under the Creative Commons Attribution-ShareAlike License. Additional terms may apply.
