one the very last example how would the methanol take the hydrogen (it would make it almost just like the molecule it took it from) or, wouldn't H2O break apart from the methyl group? or the hydrogen break away from the H2O? or since its not the main reactant it just doesn't matter?? someone plz help I need to understand
On the second example, wouldn't the water just leave resulting in an alkene and therefore, an elimination reaction? I'm confused. I thought for SN1 reactions, the leaving group had to be a weaker base than the nucleophile attacking it?
kay so sometimes I keep catching him say "the more stable, the more reactive." Isn't the opposite? Why is it that sometimes it's the opposite and he changes his words?
2ndintelligentWorld I'm no expert at chemistry but what I think he means is that if something is more reactive, then it must hold onto electrons more closely/expel electrons more easily. This means that it must be more stable in it's ion form (seeing as it is reactive in the first place as it really wants that electron/doesn't want it). Thus it's more stable if it's more reactive originally. This might all be horribly wrong.... oh well!
+2ndintelligentWorld SN1 needs stable carbocation. After leaving group leaves, you need stable cation otherwise cation will not be formed. thus no cation . thus no sn1 reaction.
I took this course nine months ago. I totally have forgotten most of it. I don't understand why I am never able to remember chemistry materials for the long amount of time.
Oxygen (Periodic Table) has 6 valence electrons, 1 lone pairs (2 electrons) and three bonded electrons: 1) 1 bonded together with the carbocation and 2) 2 bonded together with each hydrogen and we know that in a covalent bond each atom 'owns' 1/2 of that bond. So oxygen has 2 electrons plus 3 electrons (from the covalent bonds with carbon and hydrogen) = 5 valence electrons when according to the Periodic Table it is supposed to own 6. So therefore, it lacks an electron and therefore bears a positive charge.
Thanks this is helpful
good vid
instead of one more molecule of methanol why can't the cl take the hydrogen to form hcl?
U helped me alot thanks alot
Sabreena James Cameron Diaz
one the very last example how would the methanol take the hydrogen (it would make it almost just like the molecule it took it from) or, wouldn't H2O break apart from the methyl group? or the hydrogen break away from the H2O? or since its not the main reactant it just doesn't matter?? someone plz help I need to understand
he attac
but most importanty
he nucleophile
i don't know why i feel this video wasn't as organize as other ones from khan. maybe it was the used of only yellow color to explain.
Agreed.
On the second example, wouldn't the water just leave resulting in an alkene and therefore, an elimination reaction? I'm confused. I thought for SN1 reactions, the leaving group had to be a weaker base than the nucleophile attacking it?
where do all the cl's go? aren't they supposed to be +cl- at the end of the product? I'm confused.
Yes I guess they forgot to write that
Estrella Solimar yes but that part is implied... some just don’t write it... my teacher does the same
can some one explain to me what he meant by "we have to think about the acid/base reaction as well at 9:03" ?
he means like consider the nucleophile like a Lewis base and the electrophile a Lewis acid.
kay so sometimes I keep catching him say "the more stable, the more reactive." Isn't the opposite? Why is it that sometimes it's the opposite and he changes his words?
2ndintelligentWorld I'm no expert at chemistry but what I think he means is that if something is more reactive, then it must hold onto electrons more closely/expel electrons more easily. This means that it must be more stable in it's ion form (seeing as it is reactive in the first place as it really wants that electron/doesn't want it). Thus it's more stable if it's more reactive originally. This might all be horribly wrong.... oh well!
+2ndintelligentWorld SN1 needs stable carbocation. After leaving group leaves, you need stable cation otherwise cation will not be formed. thus no cation . thus no sn1 reaction.
Riken Maharjan totally correct
I took this course nine months ago. I totally have forgotten most of it. I don't understand why I am never able to remember chemistry materials for the long amount of time.
Chill happens with everyone...trust me ik
Why does the O get a positive charge after it connects to the carboncation? HELP
Oxygen (Periodic Table) has 6 valence electrons, 1 lone pairs (2 electrons) and three bonded electrons: 1) 1 bonded together with the carbocation and 2) 2 bonded together with each hydrogen and we know that in a covalent bond each atom 'owns' 1/2 of that bond. So oxygen has 2 electrons plus 3 electrons (from the covalent bonds with carbon and hydrogen) = 5 valence electrons when according to the Periodic Table it is supposed to own 6. So therefore, it lacks an electron and therefore bears a positive charge.
Because it loses an electron to the carbocation.
Because it donates an electron to the carbocation.
The first two reactions are not an example of solvolysis? Why not?
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