Talk:Chemical bond

message: Weak chemical bonds are sometimes major players in complex stereochemistry. But for simpler molecules they only effect in the compounds' physical properties. Modern science handles these bonds differently from the other types of bonds (covalent, polar, ionic, metallic). F.e. there is no LCAO (or molecular orbitals) for these. Melianis 13:50, 7 December 2005 
(UTC)  Expanded the article, tried to make it more understandable by classical terms. This article is in serious need of pictures (differences between various bonding types). I have a few ideas but don't know if i'm up to the task. Anyway, i'm not going to bother if they're accurate or not, basic idea should be enough. Melianis 15:17, 9 December 2005 (UTC)
thread_title:  '05 comments 

message: The last half of the 20th century (to first approx) saw MO theory slowly winning out over Pauling, and if the balance has since tipped, when and how and for what problem classes needs to be noted, just as you've done it in the non-math parts of the modern VB article. Try to keep this one non-mathematical, but if you see examples you don't like or that you think are misleading, fix them with replacements. You know enough to do it.  Yeah, I know you don't have time for full rewrite. But please note the tricky way Wikipedia has of drawing out the time of true experts in various fields. Wikipedians write articles which are get better and better until some true expert reads them and says "Gak, that's SORT of right, and I can't STAND the difference between this and true". So you go to the TALK page and complain (see, we suckered  you out of that much of your time). And those who did the rough work then cheer you on to do whatever you can to be WP:BOLD and WP:SOFIXIT. Go for it. Start with the simplest metaphors you can, and work your way up. Compare and contrast methods. Remember you're writing for an audience who's mostly never seen the math function for a wavefunction, so pretend you're Steven Weinberg writing The First Three Minutes. No question you know what you're talking about, but you have to explain it anyway, and give real-world examples (benzene, carotene, graphite). SBHarris 05:24, 26 November 2006 (UTC)
replies: text:  I've made a start on the first couple of sections - it may be too jargon-ridden, feel free to simplify. Rparson 23:00, 26 November 2006 (UTC)
thread_title: =

message: The section on intermolecular bonding is deficient - it omits several types of intermolecular force (e.g. higher order multipole interactions such as dipole-quadrupole or quadrupole quadrupole, and induction forces such as ion-induced dipole.) I could add these in, but I wonder if it's better to just cut thhe entire section, as it's only tangentially related to the subject of the article. The article is about Chemical Bonds, after all, and this section is about interactions that are for the most part not generally referred to as chemical bonds (hydrogen bonds being the exception, perhaps there should just be a section on Hydrogen Bonds and toss out the rest.) Rparson 18:44, 28 November 2006 (UTC)
replies: text: I agree, but first, we need to fix something. I have altered two main article links. Dipole-dipole attraction redirected to Intermolecular force so I altered that. We should have a link there. Instantaneous dipole attraction also directs there. However Van der Waals forces is a quite separate article. I just fixed a small redirect issue with it. Perhaps Van der Waals forces and Intermolecular force need to be merged. I'll look into it but not immediately. --Bduke 21:38, 28 November 2006 (UTC)
thread_title:  Intermolecular Bonding 

message: This article is really improving nicely.  I would suggest adding more references (aim for ten) and add an external links section to “good articles” on chemical bonding.  Keep up the good work: --Sadi Carnot 18:10, 10 December 2006 (UTC)
thread_title: Good work!

message: The article currently gives diborane as an example of banana bonds. I think that this usage of the term "banana bond" is nonstandard, and three-center two-electron bond is a more appropriate term. Banana bond is more commonly used to refer to "bent" bonds in cyclopropane, or to a view of the C=C double bond as a combination of two banana bonds instead of a combination of a sigma bond plus a pi bond. Note that the current version of Diborane doesn't mention bananas at all, and the current version of banana bond doesn't mention diborane at all. I do recognize that the bonding in diborane is sometimes informally called "banana" (and deserves a brief mention in the banana bond article), but it would be more precise to simply call it a three-center two-electron bond. Itub 22:46, 18 December 2006 (UTC)
replies: text: Note: I just expanded banana bond and added a link to three-center two-electron bond, as well as a section about double and triple bonds. Itub 00:47, 19 December 2006 (UTC)
replies: text: Agree. Looks like you fixed the problem nicely, yourself. Isn't it nice when Wikipedia works like that? SBHarris 01:14, 19 December 2006 (UTC)
thread_title:  Banana bond 

message: ((EDIT: I wish I knew what was real on this page, and what isn't. -Lindsey)) (added by User:71.65.50.127)
It might help if the anon explained this point. --Bduke 01:18, 12 January 2007 (UTC)
thread_title: Comment moved from article

message: The spelling is now a hybridiz/sation of US and UK--P.wormer 01:01, 24 March 2007 (UTC)
thread_title:  hybridization or hybridisation? 

message: Is there any possibility that we would be able to create such an article? I think it'd be an important distinction to explain the fundamentals of simplified bonding theories in an article away from a general one; stuff such as lewis theory, VSEPR, Ligand-packing and soforth.   ♥♥ ΜÏΠЄSΓRΘΠ€ ♥♥ slurp me! 21:01, 4 April 2007 (UTC)
thread_title:  Proposal to create [[Simple bonding]] ? 

message: There is some kind of confused comment about this now, added by Enormousdude, in the INTRO. It implies that the nature of a bond depends somehow on constructive interference between two electrons. It doesn't. There are plenty of one-electron bonds (eg H2+), and two-electron bonds are NOT 4 times as strong as one-electron bonds. In fact, they are generally less than half as strong, due to electron-electron repulsion. (Example: bond enthalpy in H2+ is about 2.65 eV and in H2 it is 4.0 eV). So I'm going to remove this comment in a few days, unless somebody can convince me otherwise. SBHarris 20:23, 18 April 2007 (UTC)
replies: text: I noticed that too. It is certainly confusing. The article does need a simple explanation of the covalent bond and it needs to be correct. --Bduke 22:30, 18 April 2007 (UTC)

text: I don't think he meant the interference of two electrons, but the interference of the functions that you could use to describe the unbound system (as in sp3 orbital + sp3 orbital -> sigma orbital, with an increased electron density between the two nuclei). --Itub 06:20, 26 April 2007 (UTC)
replies: text: Comment should stay removed, as per Sbharris. I think we have a good-faith edit by a physcics undergrad who hasn't quite undertood all of his or her courses. Physchim62 (talk) 13:22, 26 April 2007 (UTC)
thread_title:  Amplitude addition resulting in charge expansion 

message: I think that perhaps this is a good place to ask for advice, as many Wikipedia articles suffer from this (or in my ignorance, I think they suffer from this). My question is the following: what is the correct use of bind|bound|bound and bond|bonded|bonded when talking about chemical bonds? I mean, is the expression "atoms A and B are unbound" correct, to mean "atoms A and B are not bonded"? To me the former sounds like "the size of the atoms is unbound (i.e. it is unlimited)", yet I see it in many places. Other uses include "binding energy" (which is correct), or "atoms A and B bind together" (how about "atoms A and B bond together", or "atom A bonds atom B" or "atom A binds (to) atom B"). I must confess that after a Ph.D. in chemistry, this silly thing still haunts me (obviously, I am not a native English speaker). — isilanes (talk|contribs) 11:04, 4 June 2007 (UTC)
thread_title:  'Bonded' vs 'bound' 

message: :I recently started a page called chemical bonding models a modest page at best which is currently under dispute. I started this page since I considered incorporating segments on Valence shell electron pair repulsion (VSEPR) Theory, Crystal Field Theory (CFT), and Ligand Field Theory (LFT) into chemical bonding along side the discussion of Valence Bond Theory (VBT) and Molecular Orbital (MO) Theory and the well written "Comparison of valence bond and molecular orbital theory". I didn't go this route since chemical bonding seemed bloated and ripe for division into separate pages; especially if I added these segments which don't deserve equal footing with VBT and MO theory.  
:Another example of this bloat is that all the bonds types are listed on equal terms.  The major bonding types or strong chemical bonds as they are referred to on this page are covalent, ionic, and metallic; even coordinate covalent bond is an subcategory of covalent bonding.  The minor bonding types should some how be identified as less significant.  Does there need to be a page dedicated to "types of chemical bonds" to collectively list things like Bent bonds, Polar covalent bond, multi-center multi-electron bonds and the others minor bonds in a single place?  The same idea can be extended to the section on "Intermolecular bonding" while I realize that Cation-pi interaction should be noted as a intermolecular bonding event its not on equal footing with Hydrogen bonding. Should there also be a "List of Intermolecular bonding"?  
:The question I pose is: Does the page simple increase in size to the point where the significant information is diluted by second tier information or do we give the second tier their own venue?  How has this been handled on other pages?--OMCV (talk) 05:05, 19 March 2008 (UTC)
replies: text:  The usual pattern on Wikipedia is indeed that (as information is added from various sources) length increases to the point that it's obvious that some of it must be spun off into a subarticle(s). At that time, somebody with a good overview knowledge has to perform a delicate operation in which less-important and/or more-technical stuff gets spun off, with some semblance of summary of it left behind. Sometimes that summary already exists in the main article. Othertimes not, and it must be written at the time the other stuff goes off.  The real pain happens with the "and/or" above. It's usually the case that some more-technical and lengthy parts that need to be spun off due to length-alone, are actually of higher quality than the more general parts that need to stay. So doing the spin-off subtly decreases the overall quality of the parent article, due to dilution. But there's no help for it. So long as people insist on writing what they know and are interested in, vs. what the encyclopedia NEEDS :), there are going to be problems of unevenness of content. These show up as particularly threadbare patches in the main rug, that become more apparent every time a lovely new Persian throw-rug gets so big that it has to be moved to another room of the house. SBHarris 18:50, 9 October 2008 (UTC)
thread_title:  Page Focus 

message: As I understand it - the overview and introduction are strictly correct.
They however will cause anyone who does not understand the subject to be very confused.
Chemical bonds hold atoms together in various ways, with different strengths, to form molecules and compounds. Everyday objects are all comprised of atoms bound together in several ways. The accurate description of why this happens is complex, and described by the laws of quantum electrodynamics. In practice, simpler approximations are often used.
Simplifying, there are two basic types of bonding, ionic, which involve the sharing or transfer of electrons between atoms, and the usually weaker covalent bonding, which does not.(subtly incorrect)
Something of this sort of length and level of complexity perhaps for the first couple of paragraphs, going on to a simple description of the main sorts?
::I wonder why quantum electrodynamics needs to be mentioned in the lead at all, particularly with the suggestion that instead, quantum mechanics is used as an approximation. Quantum electrodynamics is a more accurate but more complex version of QM (one that takes into account subtle effects caused by quantization of the EM fields themselves), and so it really doesn't have to be mentioned as an "alternative" to QM. All these things are QM. The question is what approximations we want to make. Are the fields to be approximated as "even" with no vacuum polarization into virtual particles? Are the mechanics to be approximated as non-relativistic? Are multi-electron wavefunctions to be approximated as linear combinations of single electron wavefunctions, plus fudging? And so on. I think the LEAD really only needs to mention that QM explains all (so far as we can tell from the very high agreement (11 sig digit) between theory and measurement for simple systems), but approximations are necessary in nearly all complex systems to get answers, as with all engineering problems. I'll write a little suggestion, and others can restore all or part of the present lead, as they like. SBHarris 19:07, 9 October 2008 (UTC)
thread_title: Overview

message: Can someone please write a small section on sulfur/pi interactions? --kupirijo (talk) 17:37, 9 October 2008 (UTC)
thread_title:  Sulfur/pi interactions 

message: The intro in the article electromagnetic force states correctly that: It is the electromagnetic force that holds electrons and protons together in atoms, and which hold atoms together to make molecules. This is the basis of the covalent "bond". The electromagnetic force is also the basis for the other chemical bonds. But this central fact is not present in this article on the chemical bond. I found that my chemistry course book is also very unclear on this so cannot give a good reference. I would say something like: 
All chemical bonds are examples of coulomb attraction in particular configurations of atoms. In particular this is the case for the covalent bond. When two or more atoms are in the vicinity of each other there is a complex interaction between all the electrons and all the nuclei. There are certain configurations in terms of distances and angles that form local optima (small changes from these configurations require addition of energy from outside the system). Detailed descriptions and motivations of this are possible only by use of quantum mechanical models. For a particular element there is a typical number of directions and angles between directions where other atoms are to be placed for a stable configuration to be formed. The distance depends on relations between the atoms in the pair. When two atoms take part in such a configuration they are said to bond with each other. In this perspective, the bond can be said to be the relation between two of the atoms in such a configuration. The bond is not an entity in itself. But each bond has a relation to a particular electron that "wanders" close to both the atoms that are bonded. The bond is similar to the relation between me and earth. It is the thing that makes me mostly stay in place instead of floating around. The main difference is that may bond to the earth is a way of viewing an interplay between gravitation and electromagnetism, while the chemical bond involves only electromagnetism. --Ettrig (talk) 10:10, 18 October 2008 (UTC)
replies: text: My bad, this is described well under the headline "Overview". --Ettrig (talk) 12:20, 18 October 2008 (UTC)
thread_title:  Basics are missing

message: I was looking at the bond energies table, and it gives the oxygen-hydrogen bond as being equal to 366 kJ/mol. I think this is wrong. I did the calculation for the oxidation of hydrogen to give water, and by my working, assuming this releases 572kJ per mole of oxygen molecules, and using the other bond energies in the table, the OH bond should be 486 kJ/mol. I appreciate that these are approximate values that depend on the entire molecule etc, but I would assume that they wouldn't vary by 30%, and so the 366 value is a typo that should read 466.
Mathemancer (talk) 07:25, 27 December 2008 (UTC)
replies: text: Hmm, yes, there's a problem there, and the figure is correctly taken from the source so the problem is in the source. The dissociation enthalpy of the O–H bond in water is 542.8 kJ/mol, according to NIST data (although I know where you got your slightly lower figure from). A very weak O–H bond would be that in hydrogen peroxide, which has a dissociation enthalpy of 356.2 kJ/mol (from gass phase H2O2, slightly more from the liquid); an in-between example is methanol, with a bond dissociation enthalpy of 474±4 kJ/mol. It looks like that table (and section) needs some work doing on it, not least in checking. Physchim62 (talk) 17:45, 27 December 2008 (UTC)
thread_title:  OH bond energy 

message: I was just wondering whether anyone could help me with cleaning the article up a tad? I took out the long intro, which repeated a large amount of information in the article and replaced it with a brief (maybe too brief?) summary.
just another couple of points about this article:
*Does anyone else think the history section looks too long?
*There is a section for valence bond theory; why is there not one for MO theory? could the valence section be shortened?
*Could the comparision of these two theories and their explanations be combined into one section on "Bond Theories" for example?
*Should the theories be moved to after the explanation of bonds?
of course, all this could just be pointless rubbish, if anyone has any input, please say! it would be nice to promote this article eventually
Thecurran91 (talk) 20:54, 21 September 2009 (UTC)
replies: text: Yes, you shortened it too much. The original intro may have been too long, but that was because somebody had the idea of putting all the non-technical "overview" material which originally began the article, up into the LEAD. Some of this is actually NOT repeated anywhere in the article (why DO a bunch of random nuclei and electrons stick together? In small words.). And of course, LEAD material is supposed to repeat, at the same time it stands alone.  As it it is, your lead is two paragraphs for a very long article, which is not enough. 4 paragraphs are recommended at minimum. So now we have an article which doesn't have a lead long enough to explain why a chemical bond forms, but you have to slog through the entire rest of the article to get that (and good luck).  So try again. Don't delete, improve. Don't delete material in a too-long lead, but put it back in an up-front overview, which is where it was before. SBHarris 22:32, 21 September 2009 (UTC)
replies: text: Hmm. well I reverted my edit as all the stuff was commented. I still don't think the bits about covalent and ionic bonds are short enough for the intro, you agree? and you could also try to sound a bit nicer to newbies like me in future. Thecurran91 (talk) 10:05, 22 September 2009 (UTC)

text: Agree, we should not BITE each other, newbies or not. The question really comes down to "what do we want in this article?" Straight away, and reading from the top, I wouldn't classify a chemical bond as a "process", I would classify it as a situation. I don't think the reference to QED is useful either, as current theories of chemical bonding only use QED as a perturbation in the calculations, and then only in the most precise of calculations. If someone else  with more experience in the area would like to correct me, I would be grateful. My main question is: "what do editors want in this article?" we could ask at WT:CHEM for more opinions. Physchim62 (talk) 13:41, 22 September 2009 (UTC)
replies: text: Hi, thanks for the good advice! I was wondering, having taken SBHarris' advice, I have lengthened the intro in a sandbox a little more, giving a bit more detail. Maybe there should be some info about the theories in the lead but I don't have the knowledge to do this; Maybe SBHarris would care to lend a hand? Anyway, if you could give me some constructive criticism about my sandbox I would be very grateful! Thecurran91 (talk) 14:53, 22 September 2009 (UTC)
replies: text:  Sorry that sounded gruff. I should have looked to see how new you were. We all assume that somebody who looks like they know what they're doing insofar as the basic moves (like knowing how to pipelink to a policy link as you did below with BITE), has been around enough to have read the WP:MOS and so on. Anyway, welcome. ;) Yes, the present LEAD is indeed too long, and I (for one) am not happy with it. I didn't make it that long. Again, that happened due to a summary section getting put up there by somebody else. I did help with the summary. We have to do something or other more general before diving into a long history, but the question is: what? I'll be happy to comment on your sandbox stuff. Of course I don't feel I WP:OWN this article (notice I didn't revert you but let you think and others comment); I just feel the need to warn against drastic change which delete text and leave an impoverished lead which isn't long enough. Some compromise is needed.  And (BTW) I also surely think QED is silly to mention here (another issue of somebody else), anymore than relativity in a car crash. Nobody uses QED to calculate atomic bonds-- it's a higher energy thing for far higher order corrections (Lamb shift, etc) which are totally lost in the noise of having to do with messy non-linear multi-body problems. Ab initio calculation of bond strengths are lucky to be acurate to one part in 1000, if I read the literature right. QED at atomic electron binding energies introduces corrections on the order of (what?) 10 parts in a million for Z=1,and maybe something more interesting for heavier elements. SBHarris 02:58, 23 September 2009 (UTC)
thread_title:  Improvements for a GA? 

message: Can we put something about how long bonding takes?  The latest research from Canada places bromine molecule breakup at around 200 femtoseconds.  Does anybody have times for the converse process -- bonding itself?  —Preceding unsigned comment added by 65.50.1.50 (talk) 20:22, 16 September 2010 (UTC)
thread_title: Time Taken

message: Huckels rule regarding aromatic bond - gives benzene as an example with n=4, whereas it should be n=1, Huckels rule applies to the pi electrons only. Huckels rule article is correct.  — Preceding unsigned comment added by 85.95.101.151 (talk) 14:43, 5 December 2012 (UTC)
thread_title:  Huckels Rule - benzene example incorrect 

message: The phrase "the electrons spend more time between nuclei, than anywhere else in space" is incorrect. They spend more time near the nuclei than anywhere else. The electron density between nuclei however increases on bond formation over the situation of two non-interacting atoms. I leave it to others to rewrite that section. --Bduke  (Discussion) 21:56, 28 May 2013 (UTC)
replies: text: I also don't like this statement. At the moment, I can't think of a good way of editing it. Maybe just get rid of it for now. It's not really necessary. I would be careful with the nuclei comment. While electron wavefunctions for atomic systems are typically high at the nucleus, their probability density is not. The probability density will be peaked at some distance away from the nuclei, depending on the number of electrons and the nuclear charge. For example, an electron in a hydrogen atom has its peak electron density at a value of r = a0. Sirsparksalot (talk) 17:36, 4 June 2013 (UTC)
replies: text: The peak at r = a0 is saying that a0 is the most probable radius - i.e the probability of finding the electron in the volume element 4 pi r**2 delta r. This volume element increases as r increases. However if you look at the probability of finding the electron in equal volumes - (delta x) (delta y) (delta z) the probability is greatest at the nucleus. Several texts plot the electron density in molecules. The peaks are always at the nucleus. The density is the square of the wave function. You are confusing it with the radial density which is density times 4 pi r**2. --Bduke  (Discussion) 21:41, 4 June 2013 (UTC)
replies: text:  Yep. Probabily volumetric density dP/dV = psi^2. So the straight differential probability dP is psi^2 dV = psi^2 (4piR^2dR). So RADIAL DENSITY dP/dR = Psi^2 (4piR^2). To see where that function is maximum, you must differentiate yet again WRT R, finding dP^2/dR^2, and set that to zero. The extra differentiation (psi^2 is here a simple exponential in terms of a, the Bohr radius) gives a function of two terms set to zero, and solving that gives an R for P(R)max and that's the Bohr radius.  Going to the original complaint above, since our wavefunctions in molecules are stationary states that are time-independent, it's better not to speak of where the electron spends "most time", as the wavefunction doesn't change with time. Best to speak of electron density in space, like some charged jelly that doesn't move in time but does change in density from place to place in SPACE. That motionless jelly has a radial density (as above) that is maximal on a plane somewhere between two atoms in the bonding molecular orbital (MO) of a chemical bond (in a bond between atoms of the same element in a diatomic molecule, of course it's exactly between them). For an antibonding MO, there's a node in that plane, so the electron is least likely there. The radial increase in density between atoms defines a bonding orbital, and the node an antibonding one.  If you work out where the electron density is (you have to sum it for more than one electron), then simple electrostatics gives the force with which the bond holds the atoms together (Feynman first realized this in an early paper in 1939). It sounds like a classical not quantum answer, but it's merely the classical outcome of a quantum calculation, as force is just the distance-derivative of potential, and the electron-density lines up along potentials, so you can integrate expectation-forces right along with potentials and electron densities. This calculation explains the electrostatic force you have to overcome to start to separate two bonded atoms, but doesn't entirely explain what force keeps them apart in opposition to their wholey electrostatic attraction. Still, the attractive part of a bond is what we are interested in.  It's true that even the radial probability is not much affected for inner electrons of atoms that participate in a bond (so these electrons have about equal probability of being between atoms as not, and do have almost their summed probability associated with just one atom). But we just ignore these electrons as inner electrons that effectively don't participate in the bond. It is the outer electrons with warped orbitals that brings their charge-density more into the space beteen atoms than the space that isn't between atoms, that are responsible for the attractive part of a covalent chemical bond.SBHarris 22:19, 4 June 2013 (UTC)
replies: text: The increasing volume element as a function of r is precisely what I was referring to. Wouldn't "near" the nucleus imply the electron's proximity to the nucleus or, in other words, the radius? Similarly, what does it mean to be "between" the nuclei as opposed to near the nuclei? Sirsparksalot (talk) 19:52, 25 June 2013 (UTC)

text: Maybe my inquiry is a moot point since the text has been removed from the article. I understand where the electrons are, but I still have trouble with the semantics of the comparison of "between" nuclei as opposed to "near" the nuclei. An electron can be both between and near. If the between classification is used, then the argument should be that the integrated probability density is higher between the nuclei as opposed to outside of the nuclei (although I don't necessarily think "outside" is the best choice of terms). Also, I don't like the term "near" the nuclei because, in my opinion, it specifically implies the radial distance between a nucleus and an electron. In this case, due to the larger volume element of the radial distribution function, the electron is more likely to be located away from the nucleus as opposed to "near" the nucleus, despite the wavefunction being peaked there and regardless of the fact that a chemical bond is involved. Am I making sense? Sirsparksalot (talk) 15:38, 26 June 2013 (UTC)
thread_title:  Where are electrons most? 

message: Section headings, per WP manual of style, should be in sentence case, with only the first letter capitalized. 
https://en.wikipedia.org/wiki/Wikipedia:Manual_of_Style#Section_headings
Kortoso (talk) 22:51, 16 December 2013 (UTC)
thread_title:  Sentence case 

message: the last sentence in the second paragraph reads:  
This phenomenon limits the distance between nuclei and atoms in a bond.
that doesn't sound right.  ?
Would one of the follow be better?:
This phenomenon limits the distance between a nucleus and the other nucleus in a bond.
versus
This phenomenon limits the distance between nuclei and electrons in a bond.
____
:I think what was meant is the distance between a nucleus and the other nucleus in a bond. We could change it, but that would just repeat the thought of the previous sentence, so instead I have just deleted the incorrect sentence. Dirac66 (talk) 20:06, 24 April 2017 (UTC)
thread_title:  Minor Clarification; possible typo 

message: How to avoid silly mistakes. 
 Uddipansinha2 (talk) 17:35, 6 July 2017 (UTC)
thread_title:  Psychology  

message: An editor has asked for a discussion to address the redirect Association (chemistry). Please participate in the redirect discussion if you have not already done so.  Shhhnotsoloud (talk) 11:36, 9 April 2018 (UTC)
thread_title:  Association (chemistry) listed at [[Wikipedia:Redirects for discussion|Redirects for discussion]] 

message: Currently, the See also section is empty. Should it be deleted or filled in?--Adûnâi (talk) 22:35, 13 July 2019 (UTC)
replies: text: The empty section was removed in November. I have now restored the section with a list of 11 items based on the French article, although in alphabetical order. Dirac66 (talk) 00:51, 4 April 2020 (UTC)
thread_title:  The empty "See also section" 

message: dimensions 197.211.59.54 (talk) 13:52, 21 February 2021 (UTC)
thread_title:  physics 

message: Chemical bonds to artificial atoms formed by quantum corrals have been measured. I suggest to include this into the description of chemical bonds, see
https://science.sciencemag.org/content/early/2021/05/12/science.abe2600 132.199.97.70 (talk) 12:21, 14 May 2021 (UTC)
replies: text: Not done: it's not clear what changes you want to be made. Please mention the specific changes in a "change X to Y" format and provide a reliable source if appropriate. ScottishFinnishRadish (talk) 12:26, 14 May 2021 (UTC)
thread_title:  Semi-protected edit request on 14 May 2021 

message: Re the twin chemical diagrams towards the end of section "Strong chemical bonds" both show 3 H atoms bonded to a single N atom. Each bond is different.
I came to this page specifically to learn about what bond is associated with what symbol. It seems to me that such information ought to be prominently displayed in the introductory section  of the article.
While I learned some chemistry in the late 1960s this symbology was not then in common use, if indeed, it was in use at all. Pawprintoz (talk) 04:26, 5 February 2023 (UTC)
replies: text: The bonds in :File:NH3-BF3-adduct-bond-lengthening-2D.png look different but they are chemically identical. The meaning is explained to an extent at Skeletal formula#Stereochemistry. I used these different representations of covalent bonds to show  has a staggered conformation. Ben (talk) 10:48, 5 February 2023 (UTC)
replies: text: I have now added a summary of the meaning to this article, with a link to Skeletal formula#Stereochemistry for more detail including pictorial definitions of the terms wedged bond and dashed bond. Dirac66 (talk) 12:28, 5 February 2023 (UTC)
thread_title:  Missing info on diagrams 

message: 4 ways to maintain a healthy tooth 154.160.0.65 (talk) 21:49, 22 February 2024 (UTC)
thread_title:   Interested Science