OK guys, I need help and loads of it! Snow days aren't good when you don't understand something.
Covalent Bonding (or just bonding, I've been told ionic is still classed as bonding for teaching senior school but it isn't really, not in my eyes).
How do the elecrons pair up?
Are they limited to just the space in which the orbitals overlap so both atoms feel complete?
Do they have to be of the same spin to pair up (I think so but aren't sure)?
Do orbitals have to bend to form pi bonds or do the electrons leave the p shell?
And does the sigma p orbital bonding mean both little arms of the p shell have to bend over to match up? Does that make sense? Not really.
And here's an unrelated one. I comprehend how spin keeps electrons in the same shell from hitting each other, but how do s electrons not hit the electrons in the p orbitals? Because the s shell overlaps all the p shells and d shells and whatnot so how do the electrons not bump into each other. OK they repel each other but does that alter the "shape" of the shell, are electrons less likely to be found at certain points, especially in the s orbital, if there is a chance they could collide? Or is this a really, really stupid question?
And if anyone wants to pass this onto a chemist please feel free. I just don't get this and the lecturer doesn't understand my questions! (Then again, I'm not convinced I do some of the time either.)
sorry Ryn, I know it isnt funny that you dont understand something, but I have NO IDEA what language you just spoke! lol
So I am sorry I cannot help you but I am subbing this anyway cos now I really want to know if those little arms are going to bend or not!!
LOL. I don't have to understand it, which is why the notes and books don't go into enough detail, I just want to! Isn't that what a University education is supposed to be about?
Ryn, I'm currently sitting here tearing up my chemistry degree. I feel like I *should* be able to answer your questions, but I just can't!
The one thing I can comment on - I was initially under the impression that electron orbitals were a "path" that the electrons ran around on. They aren't. They actually kind of buzz around in a "cloud" that's that rough shape. They can even be outside of that orbital shape - there's just a higher probability that they are there.
The bonding questions are hurting my head - if something pops into my brain later on, I'll come back.
Of course, it's over 10 years now (!!!) since I finished uni, so it's entirely possible that everything I learned is now seriously outdated!
*Struggling to remember what I was taught in chemistry at uni* .... I think BW has it fairly right though, they aren't confined to a particular orbital, there is just a higher probability that they will be found in a certain orbital, so the electron cloud is really just a fuzz surrounding the nucleus. Sorry I can't answer your other questions...it's way too early in the morning for chemistry, that and the fact I left uni over 2 years ago! Lol
Atomic bonding question
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!!!) since I finished uni, so it's entirely possible that everything I learned is now seriously outdated!
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