If someone were to ask me what are the angles of say, sp3 nitrogen and sp3 oxygen, should I answer that it is ~109°, or should I take into consideration the repulsion between orbitals? In that case, for example, the right answer would be ~107° for nitrogen, and ~104° for oxygen. I'm having trouble undersanding if orbital repulsion happens "before" or "after" bonds are formed. Is the geometry tetrahedrical for both? Or is it pyramidal/bent respectively?
My uni textbook explains it very vaguely and I wanna learn more.
Does anyone know about a good resource for research on this topic?
Thanks a lot:)
I have seen many practice questions involving answers being d orbital answers, such as sp2d, when does this occur and why?
I’m a little confused on the connection between a molecules molecular orbital diagram and it’s individual atomic hybridization. Can anyone help me?
Thank you
I’m so sick and tired of this situation: someone asks a question about hybridization, VBT, etc. and then some smartass invariably in the comments says “VbT iS a LiE, oRbItAls dOnT hYbRiDIzE, MO tHeOrY iS tHe OnLy rEAL tHeOrY”
We get it, you’re really fucking intelligent because you took chemistry courses past orgo II. No one cares. Just answer the question so the student understands, instead of confusing them with a bunch of information about MO theory, group theory, and quantum mechanics they don’t need.
<\rant>
My organic chemistry professor said something in passing that struck me as odd. We were talking about hybridization and he said something along the lines of how it isn’t real. What? So I did a little bit of google research and it looks like hybridization is a tool for understanding what is happening, but is not really what’s going on. Ok, but I can’t figure out what’s really going on. It’s some quantum crap apparently. Can anyone explain what’s really going on with hybridization or the lack thereof?
Do f orbitals hybridize? If they do what hybrid orbitals do they form? Ty in advance
Hello! I'm in general chem 1 and would appreciate all the help I can get!
So I just learned about atomic orbitals and sigma bonds but I'm not really understanding how to approach this question. Like do I use the number of electron groups to see their hybridization? And how do I know if it is even hybridized in the first place?
https://preview.redd.it/wg4xjjjhg0x41.jpg?width=1148&format=pjpg&auto=webp&s=6ec1427432e450a277ad7fffd1c2740c335a58a9
Thanks in advance!
The nature of metal–boron orbital interactions in boron‐bearing intermetallics and its influence on the surface hydrogen adsorption property and catalytic activity aredemonstrated. Several transition‐metal–boron intermetallics are predicted to be efficient hydrogen‐evolving materials with catalytic activity approaching platinum, and among them RuB is confirmed experimentally.
Abstract
A theoretical and experimental study gives insights into the nature of the metal–boron electronic interaction in boron‐bearing intermetallics and its effects on surface hydrogen adsorption and hydrogen‐evolving catalytic activity. Strong hybridization between the d orbitals of transition metal (TM) and the sp orbitals of boron exists in a family of fifteen TM–boron intermatallics (TM:B=1:1), and hydrogen atoms adsorb more weakly to the metal‐terminated intermetallic surfaces than to the corresponding pure metal surfaces. This modulation of electronic structure makes several intermetallics (e.g., PdB, RuB, ReB) prospective, efficient hydrogen‐evolving materials with catalytic activity close to Pt. A general reaction pathway towards the synthesis of such TMB intermetallics is provided; a class of seven phase‐pure TMB intermetallics, containing V, Nb, Ta, Cr, Mo, W, and Ru, are thus synthesized. RuB is a high‐performing, non‐platinum electrocatalyst for the hydrogen evolution reaction.
https://ift.tt/2QmPN24
Be has 2 electrons in its 2s orbital. To form BeH2, I think it needs to hybridize to sp orbitals. What causes the hybridization?
(I’m not learning chemistry in English, so I don’t know some of the technical terms) So, we’re learning about how atoms form molecules through covalent bonds. And I understand how in one orbital (which is defined by n,l and m), there are two electrons with opposite spins. I also know how I describe the electron structure of an atom (for example: 1s^2 2s^2 2p^6 and so on). But when it comes to molecules bonding I don’t understand how I’m supposed to decide whether is a sigma or pi bond. I also don’t understand anything about orbital hybridization. So, I call thee to help!
In NH3 the bond pair of electrons between hydrogen and nitrogen has a dipole moment towards nitrogen but the dipole moment of lone pair of nitrogen atom is away from it. I want to know why this happens ,as the electron is attracted towards the nucleus shouldn't the dipole moment of lone pair be towards the nucleus as the nucleus attracts the electrons.
For example, neon has an electron configuration of 1s2 2s2 3p6.
I’ve viewed the Khan academy videos & gone over my notes for class but the information isn’t clicking. I’d really appreciate if I could get point toward some additional resources to look over/study. Thanks!
Thanks in advance for any help!
I really wonder how C atom hybridize for example sp^3. The carbon is undertaking the electron promotion which one orbital from s orbitals move to empty p orbital. You know it takes energy, but does anyone knows where the energy came from?
I am teaching myself sigma pi hybridization and have some confusion on the topic. I understand that the purpose of hybridization is to combine the orbitals from electron configuration together to achieve energy equivalence among the orbitals. The significance of that comes from a compound like CF*4* having 4 bonds that appear to be equivalent, but the electron configuration of carbon says otherwise. Anyway, my confusion roots from why the shape of the orbitals in hybridization matter. Is it so the two electrons in the covalent bond have the same amount of room to move around?
Thanks for the help!
Hi all, not a homework question, but this is a very simple question that I've crossposted in /r/chemhelp.
I've got a basic question about orbital hybridization. If a 2s and a 2p orbital hybridize, the result will be an sp3 orbital.
Geometrically it will look like an asymmetric p orbital, with one side being much larger than the other. Why does this occur? I assume it has something to do with interference/phase, but I don't quite understand. Thanks.
I know that this doesn't exactly pertain to AP courses, but I thought I could get an answer here.
So yesterday in AP Chemistry, we began a lesson on Hybrid Orbital Theory, Valence Bond Theory, and Isomers. Many of us in the class can't seem to figure out how to find hybrid orbitals. On our lecture, there isn't a slide that clearly explains what these are and our teacher is on leave for the rest of the week. Any help would be appreciated, and thanks in advance!
[Edit]: Finally got some clarification between the post you've made and the wiki. Thanks again for all your help!
http://imgur.com/LBN3lye
I'm having a ton of trouble understanding this section. Can someone please explain how I know how many, I don't even know what they're called, red balloons to draw? Is it based on VSEPR or the number of valence electrons?
I would really appreciate an ELI5 version.
I'm not doing too hot in AP Chem...
