# Would an $H_2O$ Molecule actually look like this 3D representation if we could see it?

I'm trying to get a much better grasp on atoms and molecules and I am a visual learner. I found the above image here. This intuitively makes sense to me because I can see how the electron orbitals change from a spherical shape to a tear drop shape after this process:

Now the hydrogen electron clouds have become trapped inside the oxygen atom because they can't overcome the repulsion of the outer oxygen electron clouds.

The exposed hydrogen protons help me understand how H2O is a polar molecule because they give the two "corners" of the molecule a positive charge and the opposite side of the molecule a negative charge, corresponding to this model of H2O:

My question is, does the first model above actually represent the physical layout of the nucleus's and electron clouds of an H2O molecule (as best we understand it currently)?

## Update

It looks like the orbitals in the first picture above may be a bit off on the oxygen molecule since there should be two spherical shells around the oxygen nucleus (1S and 2S) with 2 electrons each and then the other 4 electrons would occupy (but not fill) the 3 2P double-teardrop shells on the X, Y, and Z axis (although I'm not sure why one axis of the 2P shell is smaller than the others). But barring that perceived discrepancy, the 4 valence electrons would exist in the teardrop shaped 2P orbitals, correct? That would make sense to me then how the hydrogen electron orbitals could get trapped behind them.

( I used this electron orbital diagram for oxygen for reference:

)

• Short answer: no. Your first picture is quite misleading on a number of counts. Don't get attached to it. – Emilio Pisanty Jan 4 at 4:31
• without further checking if the depiction of the orbitals is correct, I would definitely answer no to the question in the title. "Observing" is an act of measure and, as such, will cause the reduction of the wavepacket. Your electrons, when you observe them, will appear at a precise location; you will never "see" the orbitals as they are depicted here. You could only recreate it statistically after a large number of observations (if your figure is correct) – Barbaud Julien Jan 4 at 5:11
• Direct observation of orbitals was reported. For example Nature 401 (1999) 49-52 – Dr S T Lakshmikumar Jan 4 at 5:20
• The proton cannot be so isolated. The H-O bond is covalent. So the electron orbitals have to be present near the protons – Dr S T Lakshmikumar Jan 4 at 5:27
• You can't see electron clouds or orbitals, so perhaps you need to reword your question? What do you even mean by seeing a molecule? – Aaron Stevens Jan 4 at 5:29

As part of an undergraduate project I calculated the electron density for various small molecules such as water and ammonia, and the disappointing result is that they are all basically formless blobs with only small bumps where the hydrogen atoms are. They ended up looking much like your last picture of water:

though even that picture exaggerates the bump in the electron density caused by the hydrogen atoms. Sadly I no longer have the results from my calculations, but then they were done in 1983.

So if you could see the water molecule I'm afraid it would just look like a roughly spherical fuzzy blob.

• If I understand OP correctly, s/he wants to dissect that electron cloud into individual components for the different electrons. Which is, of course, impossible; the details are here. – Emilio Pisanty Jan 4 at 5:45
• While this might be impossible when probed from the outside, what would we get if we probed/calculated charge density in the HOH plane? I guess we'd get some noticeable bumps there... – Ruslan Jan 4 at 10:00
• @Ruslan I did calculate the electron density in the HOH plane and even then there were only small bumps due to the hydrogen atoms. Bear in mind that each H atom contributes only 1 electron out of 10 in total, and the electrons are delocalised over the OH bond. Very near the proton you get a spike in electron density, but you wouldn't see that from outside the molecule. It really is just a blob. – John Rennie Jan 4 at 11:59
• This is fascinating thanks. So, the conclusion I'm drawing is that you can't really "sense" the actual orbital shapes (spherical, teardrop/peanut/balloon) of the electrons around the atom so it would never "look" like the first image from my post. However, I'm now wondering if the forces, not the shapes, are accurate in the first image I posted. Is it true that the hydrogen electron (or electron clouds) actually do get "trapped" behind the oxygen electron (or electron clouds) after a water molecule is formed? If the answer is yes, that would at least give me some idea of how things work. – BarrettNashville Jan 4 at 16:20

Although "a picture is worth a thousand words", in some cases explaining what a picture represents requires even more words. This is the case for the graphic representation of electronic density and electronic orbitals.

First of all, the two concepts have not to be confused. Total electronic density may be measured, while theoretical concepts al one-particle orbitals cannot. In many visualizations of electronic states in atoms and molecules the two quantities are mixed. Still they are different (orbitals are complex functions in general, and even if a real representation is selected they carry a sign, while density, being connected to a square modulus is positive by definition).

Even if one confines the attention to graphic representations of electron density, again some care is required to interpret pictures:

• some of them are intended as purely qualitative, while others come from quantitative calculations;
• there are many ways to represent graphically a 3D density. The most common used in the case of electronic density visualization are: iso-density surface plots and clouds of dots, both with some pros and cons.
• in some (most of the) cases only the electron density corresponding to single or to the highest orbitals are shown, in other (few) cases the total density is shown.

Furthermore, the image one can get from an iso-density surface can vary a lot depending on the chosen value of density, which is intrinsically quite an arbitrary value.

After all these words of caution, I should add that probably the best strategy is to use more than one visualization method in order to get a visual understanding of the electronic configuration, always keeping in mind that electronic density is an average quantity.

does the first model above actually represent the physical layout of the nucleus's and electron clouds of an H2O molecule (as best we understand it currently)?

The first picture looks quite difficult to understand to me. Of course there is no quantitative indication. But even qualitatively, there are a few suspicious features: i) those sharp points; ii) a very unphysical spherical shape around oxygen; iii) the presence and the position of four tear-like sall blobs. I would not assign a high degree of reliability to this icture as a faithful representation of the real electron density. It was probably intended as a purely qualitative representation of a linear combination of atomic orbitals without any claim of connection to the electron density of the molecule.

As far as the more symmetric blob shown also by John Rennie, it looks more reasonable, but only if one is representing the valence charge density. The real charge density of the water molecule would appear very different, by taking into account that oxygen conributes to the total density with 8 electrons,while each hydrogen with only one.

• Thanks for the insight. It helps to know that there is probably no real way of "visualizing" atoms and molecules using one particular model without missing some key concepts. – BarrettNashville Jan 4 at 16:09

Depending on the meaning of "if we could see". If force microscopy can be considered as seeing (personally I think yes if we can reasonably sort an image out of observed data, e.g. x ray diffraction or electronic microscopy as more known techniques) then this paper is one among others that report direct molecular/atomic/bond images:

https://www.nature.com/articles/ncomms8766

Note that in a molecule not all "parts" are equally "seen" by the AFM tip. For instance they can be spatially inaccessible or more/less chemically affine to it. Combining different layers can bring out details and/or enhance contrast, a bit like HDR technique in photography if I can use a loose analogy.

Moreover the assignment of specific features to specific orbitals/bonds can eventually be achieved by comparing the various images and calculations - although and with the limits mentioned above the final picture is depicting the molecule as whole.

More specifically to your answer: the water molecule would likely look as in the second plot. To date all molecular pictures turned out to be striking similar to what was sketched well before using any imaging techniques but just calculations or even based on chemical properties, reactions and products formation ^.

All images are almost superimposable to orbital and charge density plots as well as to the graphs which serve as frame and are known as molecular structural formulae. The latter were in use already in the 19th century!

To the question can we see a single orbital? Not the single electron of course, but this is why the notion of orbital emerged. The latter can indeed be seen at least through its corresponding charge density at some given discriminatory level, like in calculation s.

Perhaps technicalities and reactivity prevented to date the imaging of a single H atom but in principle an image could be obtained as for the TPDCA molecule taken as example above.

It will be a more or less fuzzy sphere - we can be confident on that.

^physical properties played a big role, too. For instance the existence of enantiomers suggested a tetrahedral geometry around C atoms.

edit after I found a basically identical question with valuable answers. While the discussion of afm and x-ray diff. are already in my A, there is a link to a spectacular results rendering H orbital in 3-D!

https://chemistry.stackexchange.com/questions/57784/has-anyone-even-taken-a-picture-of-a-molecule-to-confirm-the-geometry-predicted

• Even through its corresponding charge density, looking at a single orbital does not appear either theoretically sound nor experimentally feasible. – GiorgioP Jan 4 at 15:01
• @GiorgioP. What would be the very same kind of image of an H atom or that of H2 adsorbed on silicon? It is the more physical representation of what you would plot imposing a threshold value while in this case the experimental details would do. The empty orbitals want play much role without much theoretical discussion. – Alchimista Jan 4 at 15:24
• The cases of H or H$_2$ are exceptional since there is only one valence orbital. But in general, how could you select contributions from a particular orbital to the total electron density? – GiorgioP Jan 4 at 15:32
• This is the kind of thing I was hoping to see for a water molecule. Thanks for sharing. I guess the best we can "see" really are just blobs, but it is interesting to actually see those blobs and know that you can actually see their shapes and positions. The other image in that same Nature article of a molecule of Perylenetetracarboxylic dianhydride (PTCDA) is just as fascinating to me. Thanks. – BarrettNashville Jan 4 at 16:15
• @BarrettNashville glad it helped. Things of that sorts are the best images of atoms and molecules we have. Consider accepting the answer if not better ones come. – Alchimista Jan 4 at 16:45