Beryllium has that p orbital but there just isn't any electrons in it. That's why he showed the configuration with the 2p0. It's there it just isn't occupied. There is the difference between electrons and orbitals. I might be wrong but that's what I am getting out of it.
Nice explanation, but can somebody help me out with the relavance of making the comparison of a simple H1s- Be sp [hybrid] overlap against the H1s - Be2p overlap? Since Be has no p electrons, why would it undergo hybridization when it has a 2s orbital with two electrons that can overlap with the 1s orbitals of the two H atoms? S orbitals are spherically symmetrical, so there sould be ample overlapping and hence stability. Thanks!
Is this the same as bonding/antibonding ? For example if the question was , sketch the resulting bonding/antibonding orbitals between S and Py orbitals
I understand the answer now. If anyone was confused by this here's the answer. So when the orbitals 'combine' they don't merge they just create a new type of orbital, which didn't exist before. So in the case of SP hybridization you start of with 1 2P orbital and 1 2S orbital and you make 2 new SP orbitals. Each SP orbital is 50 percent S orbital and 50 percent P orbital. So half the S orbital goes into one SP orbital and the other half goes into the other SP orbital.
it is in the 2nd energy level so it technically has a p sublevel that is empty. this is also why we have expanded octets but that occurs with d sublevels.
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Hi - what about the bonding situation in GaF? How do these hybridized orbitals look like?
How can you combine the hybridized sp (2s+2p) orbital when there are no 2p electrons? Why is a hybrid orbital in case even possible?
I am curious about this too. It is almost like he is describing Boron instead of Beryllium.
Beryllium has that p orbital but there just isn't any electrons in it. That's why he showed the configuration with the 2p0. It's there it just isn't occupied. There is the difference between electrons and orbitals. I might be wrong but that's what I am getting out of it.
In the excited state one electron from 2s goes from 2s to 2p
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Nice explanation, but can somebody help me out with the relavance of making the comparison of a simple H1s- Be sp [hybrid] overlap against the H1s - Be2p overlap? Since Be has no p electrons, why would it undergo hybridization when it has a 2s orbital with two electrons that can overlap with the 1s orbitals of the two H atoms? S orbitals are spherically symmetrical, so there sould be ample overlapping and hence stability. Thanks!
2s2 orbital promotes its electron in 2p0 and then 2s1 and 2p1 hybridized
@@faseehniazi1210 but why?How is that energetically beneficial?
Is this the same as bonding/antibonding ? For example if the question was , sketch the resulting bonding/antibonding orbitals between S and Py orbitals
Grace McCarthy Sounds like it :)
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I don't get how you get two SP hybridised orbitals. When you combine 2 orbitals that should make 1 new combined orbital. How do you get 2 ?
I understand the answer now. If anyone was confused by this here's the answer. So when the orbitals 'combine' they don't merge they just create a new type of orbital, which didn't exist before. So in the case of SP hybridization you start of with 1 2P orbital and 1 2S orbital and you make 2 new SP orbitals. Each SP orbital is 50 percent S orbital and 50 percent P orbital. So half the S orbital goes into one SP orbital and the other half goes into the other SP orbital.
why does Be have a 2p orbital, when its electron configuration is 1s2s?
it is in the 2nd energy level so it technically has a p sublevel that is empty. this is also why we have expanded octets but that occurs with d sublevels.
is it weird that im learning this in 6th grade
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