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I just want to say that your teaching is phenomenal. I don't even play attention to my teacher anymore. I just come here and I know more than the students that pay attention to the teacher. Thank you so much!
no one could make me understand the lewis structure until i get into you video . thanks a tone
+Shawn Dypx I am channelling the ghost of Lewis!
oh wow. ok But i got some confusions on ions with your methods. especially That So4 3-
that is because it is SO4 2- !
Amazing video
Hehe, I thought you were one of my students playing a trick on me! Glad I can help.
5 and 6 charges centers but the IB have only ever asked about trigonal bipyramidal, seesaw, octahedral and square planar for HL
5 bonds will give 10 electrons shared, N needs 8.Plus a pentuple bond has so many repulsive electrons in a small volume it would probably be unstable
ugh. thanks for explaining when my teacher couldnt
thanks for your awesome video
Isn't [CO3]2- at 11:28 a resonance structure?
There are 3 Lewis structures for the CO32-. The average of all these possible resonance structures is the closest to reality.
Thanks, this was really helpful :)
thank you for helping prove my teacher wrong. :-D
Thank you sooooo much ...(thumbs up 👍)
for N2, why can't you have 5 bonds between them? it will have a full valence shell still?
legendery
how can i determine if its a triple or double bond like nitrogen? before i start bonding?
thornley is the goat 🐐🐐
Is it isoelectric or isoelectronic?
Why is H2O an exception? they have 2 and 8 so isn't that the normal octet rule? Thanks
how did I say it was an exception?
CO3 2- has 20 electrons (4+(6x3) - 2), which means it makes 10 electron pairs. On your diagram there are 12 pairs. Why is it so?
CO3 2- has 2 extra electrons not 2 fewer. so (4+(6x3)+2) / 2
Why is Beryllium stable with 4 electrons?
not sure - size is a factor as is the fact that this theory was replaced by molecular orbital theory - which (probably) accounts for this better.
there comes the matter of formal charge
Activstudio and an Activboard
There is no straightforward way, unless you have the name of the molecule.
UNIS
my teacher is using this to teach and im in 9th grade send help
Muuuhhahahaa
![S2.2.3 What is a Dative Covalent bond? [SL IB Chemistry]](http://i.ytimg.com/vi/zLCU9Je7gQ4/mqdefault.jpg)
![S2.2.3 What is a Dative Covalent bond? [SL IB Chemistry]](/img/tr.png)
![S2.2.9 Deduction of intermolecular forces, via structure & chemical formula [SL IB Chemistry]](http://i.ytimg.com/vi/GIcIkBQQrlw/mqdefault.jpg)
![S3.1.4 Describe and explain 5 trends in Group 1 and Group 17 [SL IB Chemistry]](http://i.ytimg.com/vi/-4xKhr8RNjA/mqdefault.jpg)
![S2.2.8 What are Dipole-Dipole Intermolecular Forces? [SL IB Chemistry]](/img/n.gif)
I just want to say that your teaching is phenomenal. I don't even play attention to my teacher anymore. I just come here and I know more than the students that pay attention to the teacher. Thank you so much!
no one could make me understand the lewis structure until i get into you video . thanks a tone
+Shawn Dypx I am channelling the ghost of Lewis!
oh wow. ok But i got some confusions on ions with your methods. especially That So4 3-
that is because it is SO4 2- !
Amazing video
Hehe, I thought you were one of my students playing a trick on me! Glad I can help.
5 and 6 charges centers but the IB have only ever asked about trigonal bipyramidal, seesaw, octahedral and square planar for HL
5 bonds will give 10 electrons shared, N needs 8.
Plus a pentuple bond has so many repulsive electrons in a small volume it would probably be unstable
ugh. thanks for explaining when my teacher couldnt
thanks for your awesome video
Isn't [CO3]2- at 11:28 a resonance structure?
There are 3 Lewis structures for the CO32-. The average of all these possible resonance structures is the closest to reality.
Thanks, this was really helpful :)
thank you for helping prove my teacher wrong. :-D
Thank you sooooo much ...(thumbs up 👍)
for N2, why can't you have 5 bonds between them? it will have a full valence shell still?
legendery
how can i determine if its a triple or double bond like nitrogen? before i start bonding?
thornley is the goat 🐐🐐
Is it isoelectric or isoelectronic?
Why is H2O an exception? they have 2 and 8 so isn't that the normal octet rule? Thanks
how did I say it was an exception?
CO3 2- has 20 electrons (4+(6x3) - 2), which means it makes 10 electron pairs. On your diagram there are 12 pairs. Why is it so?
CO3 2- has 2 extra electrons not 2 fewer. so (4+(6x3)+2) / 2
Why is Beryllium stable with 4 electrons?
not sure - size is a factor as is the fact that this theory was replaced by molecular orbital theory - which (probably) accounts for this better.
there comes the matter of formal charge
Activstudio and an Activboard
There is no straightforward way, unless you have the name of the molecule.
UNIS
my teacher is using this to teach and im in 9th grade send help
Muuuhhahahaa