An absolute life saver. Did more in 20 mins than my Chemistry teacher in 2 months. Also, love the visuals and labels, I just screenshot at points for revision during the day in school.
Do we need to know about the structure graphite and diamond and how this relates to its properties as I can’t find it in the spec for this section (2.2.2)?
So are dispersion forces the same as induced dipole-dipole? Since you stated they were also called (London) forces which if you google dispersion forces it states they are also called london forces.
If hydrocarbons are classed as non-polar bc the electromagnetic difference is just so low, then does the same apply when chlorine and oxygen bond together?
no its trigonal plannar because the two lone pairs oppose each other and cancel each other out leaving there to just be a trigonal plannar formation (3 bonded pairs)
An absolute life saver. Did more in 20 mins than my Chemistry teacher in 2 months. Also, love the visuals and labels, I just screenshot at points for revision during the day in school.
You're very welcome!
spent 10 years on this one video 🤣
Do we need to know about the structure graphite and diamond and how this relates to its properties as I can’t find it in the spec for this section (2.2.2)?
Thanks for this mate
You're welcome! Please share the videos, the more people that see them the better!
should we memories the pauling scale values just in case
So are dispersion forces the same as induced dipole-dipole? Since you stated they were also called (London) forces which if you google dispersion forces it states they are also called london forces.
Could someone please explain what exactly a dipole is? I don't understand the difference between a dipole and a polar bond.
If hydrocarbons are classed as non-polar bc the electromagnetic difference is just so low, then does the same apply when chlorine and oxygen bond together?
at 13:05 isn't the molecule with BP = 3 and LP = 2 called T-shape? since a trigonal planar molecule has 3 BP and 0 LP?
no its trigonal plannar because the two lone pairs oppose each other and cancel each other out leaving there to just be a trigonal plannar formation (3 bonded pairs)
@@harjapp 👍
Do we have to know all of those shapes? I'm pretty sure It's only Linear, Trigonal Planar, Tetrahedral, Octahedral, Pyramidal and Non-Linear?
Yes you do!
yes we only got taught them that you mentioned
@@AlleryChemistry i was only taught linear octahedral non linear trigonal pyramidal tetrahedral trigonal planar and linear
Thank you so much
omg im' youre bigist fan❤️❤️❤️😍😍😍😍
No ur not i am
Thank you for your video❤
So so helpful thank you:)
Thank you
Welcome!
Thank you this is so helpful! Just subsribed :)
🙏🙏have a test next period would have failed if not for you 🙏🙏wish me luck😅
Best of luck!
Isn't it a called 'non-linear' when it has 2 BP and 2 LP?
Alternate name
Same thing
Really good video
Did you just say water isn’t polar....?
quite scary no one else mentioned it...
water is a polar molecule
3:54 you stupid feaces
4:15
Is this video for suitable AQA chemistry?
Specifically for OCR
jus go on the AQA one he has