Omg, I don’t think you understand how genuinely amazing you are!! You explain everything so so well, in detail but it makes sense!! Thank you so much, I hope you’re really getting something out of posting these videos because I know for a fact I’m getting a lot out of watching them! 😊
Thank you for your kind words! It's definitely very nice to know how useful the videos are 😀 That's the main thing that keeps me wanting to make more! I've made a follow up video to this that's out today about intermolecular forces as well...
OMG! Thankyou so much. You explain so smoothly. In-depth yet so simple and yesss, the actual concept. Thankyou so much. No one has taught me like this.
Great question. I dont yet, no. I'm prioritising AQA and those features aren't really required. I'll be doing a video about the different crystal structures in the next few months, but that doesn't sound quite like the things you mean
Hi sir, do you think this is correct in terms of finding if molecules are polar: > If a non-symmetrical molecule has even one polar bond, it is regarded to have overall polarity > HOWEVER, if the compound is symmetrical (equal bond angles between all bonds and same elements that the central atom is bonded to), even if there are polar bonds, it is regarded to have overall non-polarity because dipoles cancel out in symmetrical molecules
Thank you so much for this video but can i ask, on other sources it says that the electronegativity increases down a group while you are saying it increases UP a group so im not sure which is right!
I have a question related to alkanes but I can't find your video for it so I wil ask here What causes the C-H bond to break? I did a mcq and they said that u light only breaks CL -CL bond so what breaks a C-H bond then ?
That's a great question and your understanding is correct. The answer is that the chlorine free radical breaks the bond. It, along with an H plus 1 Electron from the C-H bond form HCl, leaving the 'CH3 with its unpaired electron. Free radicals are very reactive which is why this can happen, but this reaction specifically happens because the 2 products are slightly more stable than the 2 reactants. That being said, this reaction along with most organic reactions is actually Reversible. Which makes sense, since the CH3 free radical will also be unstable and reactive and so could reverse the process.
Two things: Hydrogen and chlorine are in two separate groups, so direct comparisons are not easy based on the period (row) something is in. Secondly, and most importantly in this comparison, electronegativity is due to the nuclear charge vs atomic radius. Chlorine has 9 protons and 2 energy levels whereas hydrogen only has 1 proton. This pull from the nucleus is 9 times stronger and far outweighs the fact chlorine has 1 extra energy level
@@chemistrytutor then how does electronegativity decreases down the group. How does this make sense I mean like you said chlorine has 2 energy levels than hydrogen so it is more electronegative but chlorine is found below than hydrogen in the periodic table. Ughhh i feel so dumbb!
@miiya468 its confusing for hydrgoen but the rest makes sense after H. Electronegativity increases across a period due to increased nuclear charge. Electronegativity decreases down a group due to increased atomic radius. So Electronegativity increases as you go up and right
@@chemistrytutor okay finally i understood this but I have another confusion that is book says some molecules like CCL4 contain polar bonds but have no polarity because dipole moments cancel each other out. But CHCL3 molecule does not cancel the polarity. How does this happen ?? Do you have any idea about this???
The proof using vectors to show why the dipoles cancel each other out is literal GENIUS. Thank you so much!
😀 Glad you found that useful. So powerful as an explanation!
Omg, I don’t think you understand how genuinely amazing you are!! You explain everything so so well, in detail but it makes sense!! Thank you so much, I hope you’re really getting something out of posting these videos because I know for a fact I’m getting a lot out of watching them! 😊
Thank you for your kind words! It's definitely very nice to know how useful the videos are 😀
That's the main thing that keeps me wanting to make more! I've made a follow up video to this that's out today about intermolecular forces as well...
OMG! Thankyou so much. You explain so smoothly. In-depth yet so simple and yesss, the actual concept. Thankyou so much. No one has taught me like this.
That's really lovely to hear! Thank you for the feedback 😊
I would like to know if you have any videos explaining the rest of the chemical bonding, Lewis diagrams, distortion, resonance etc.
Great question. I dont yet, no. I'm prioritising AQA and those features aren't really required. I'll be doing a video about the different crystal structures in the next few months, but that doesn't sound quite like the things you mean
Thank you so much for posting these sir!! These help alot and make A level less brutal :)
You're very welcome 😀
I'm glad they're useful ☺️
Hi sir, do you think this is correct in terms of finding if molecules are polar:
> If a non-symmetrical molecule has even one polar bond, it is regarded to have overall polarity
> HOWEVER, if the compound is symmetrical (equal bond angles between all bonds and same elements that the central atom is bonded to), even if there are polar bonds, it is regarded to have overall non-polarity because dipoles cancel out in symmetrical molecules
Great description. That's exactly the way of thinking about it that I'd recommend! 😀
Thank you so much for this video but can i ask, on other sources it says that the electronegativity increases down a group while you are saying it increases UP a group so im not sure which is right!
That's really odd. It 100% definitely increases up a group
I have a question related to alkanes but I can't find your video for it so I wil ask here
What causes the C-H bond to break? I did a mcq and they said that u light only breaks CL -CL bond so what breaks a C-H bond then ?
That's a great question and your understanding is correct. The answer is that the chlorine free radical breaks the bond. It, along with an H plus 1 Electron from the C-H bond form HCl, leaving the 'CH3 with its unpaired electron.
Free radicals are very reactive which is why this can happen, but this reaction specifically happens because the 2 products are slightly more stable than the 2 reactants.
That being said, this reaction along with most organic reactions is actually Reversible. Which makes sense, since the CH3 free radical will also be unstable and reactive and so could reverse the process.
@@chemistrytutor rhis makes sense thanks alottt
I am confused how come chlorine is more electronegative than hydrogen if electronegativity decreases down the group? Am i missing something????
Two things: Hydrogen and chlorine are in two separate groups, so direct comparisons are not easy based on the period (row) something is in. Secondly, and most importantly in this comparison, electronegativity is due to the nuclear charge vs atomic radius. Chlorine has 9 protons and 2 energy levels whereas hydrogen only has 1 proton. This pull from the nucleus is 9 times stronger and far outweighs the fact chlorine has 1 extra energy level
@@chemistrytutor then how does electronegativity decreases down the group. How does this make sense I mean like you said chlorine has 2 energy levels than hydrogen so it is more electronegative but chlorine is found below than hydrogen in the periodic table. Ughhh i feel so dumbb!
@miiya468 its confusing for hydrgoen but the rest makes sense after H.
Electronegativity increases across a period due to increased nuclear charge.
Electronegativity decreases down a group due to increased atomic radius.
So Electronegativity increases as you go up and right
@@chemistrytutor okay finally i understood this but I have another confusion that is book says some molecules like CCL4 contain polar bonds but have no polarity because dipole moments cancel each other out. But CHCL3 molecule does not cancel the polarity. How does this happen ?? Do you have any idea about this???
@@samsyy-601 it's to do with symmetry and the polar bonds cancelling out. 9:40 on here
th-cam.com/video/81DFZQTDD2g/w-d-xo.htmlfeature=shared
Amazing videoo
Loved it
I hope u keep uploadingg
Thank you 😊
COGNITOS ENEMY
@nerdyboi2000 there's room for two 😃
Intermolecular forces video to go after this one.
th-cam.com/video/yech6seOtwk/w-d-xo.html
I will watcg this one In Jan when I have to prepare for unit 2 😉
@@Insta_Feed 😎