Just found your channel. You're criminally underrated. Keep up the cool videos! They're very informative, especially for someone who only understands basic chemistry.
I was wondering about the halogens, are they Bronsted-Lowry acids? It's weird to see they're Lewis bases. Is it because they are ions, conjugate to their hydride acids?
From my understanding, halogens themselves (F-, Cl-, Br-, I-) are actually Bronsted-Lowry bases because, as you said, they are conjugate bases to their protonated acids (ex: in the Bronsted-Lowry definition, I- is considered a base, albeit extremely weak, because HI is a strong acid. F- is considered a weak base, significantly stronger than I-, because its conjugate acid, HF, is a weak acid). Bronsted-Lowry definitions of acids just require that a compound can donate protons to water (or another base), and all protonated halogens (HF, HCl, HBr, HI) are therefore acids. Their ions cannot be Bronsted-Lowry acids because they don't have any protons to donate. Interestingly, you can also use hard-soft acid-base theory to determine how strong of a Bronsted-Lowry acid a protonated halogen is. H+ is considered a hard Lewis acid, and so the harder the Lewis base the halogen anion is, the stronger the bond between the two, and thus the weaker it is as a Bronsted-Lowry acid. Of HF, HCl, HBr, and HI, HF is the weakest Bronsted-Lowry acid, and HI is the strongest (I- is the softest base of the halogen anions). I'll probably make a video about this soon, because it's a pretty cool topic. Thanks for your question!
The molecular forms of the hydrogen halides are BL acids because they are eager to donate their proton. Once they do, the halide ion is then the conjugate base, while the proton acceptor becomes the conjugate acid. Lewis acids and bases on the other hand are electron acceptors or donors, respectively. By and large, the two theories agree on what constitutes acids and bases -- at least under aqueous conditions. I recommend theses short articles for a better picture of what's going on. en.wikipedia.org/wiki/Br%C3%B8nsted%E2%80%93Lowry_acid%E2%80%93base_theory en.wikipedia.org/wiki/Lewis_acids_and_bases
@@FoolishChemist That's actually a brilliant idea for a video, I don't think I've found anything describing that on YT that wasn't part of a loooooong lecture on multiple other concepts too.
I think the solid formed from that reaction would be aluminum hydroxide, which is very insoluble and would precipitate out of solution if that's what you're asking
0:15 you're mixing up Phosphine (PH₃) with Phosgene (COCl₂). Phosgene was used as a chemical warfare agent in WW1, not Phosphine. Edit: Thanks a lot for wasting my time correcting you.
Clarification on mistake at 3:37: "3Cl-" should be "PO43-", so that our net ionic equation is "Al3+ + PO43- --> AlPO4"
Loving the amount of info in these videos brother
Thanks man 🙏 love your videos
Just found your channel. You're criminally underrated. Keep up the cool videos! They're very informative, especially for someone who only understands basic chemistry.
Thank you! That's the goal 😁
I feel like that word play was a fantastic example of why wording maters in chemistry
Sir are you talking about chemistry or cooking 😅
Hello, im watching a lot of chemical videos lately and im very glad u are making a lot explenations for preparative and theoretical stuff :D
To your example at 1:17 I have another good one
Help jack off the horse
Help jack, off the horse
I was wondering about the halogens, are they Bronsted-Lowry acids? It's weird to see they're Lewis bases.
Is it because they are ions, conjugate to their hydride acids?
From my understanding, halogens themselves (F-, Cl-, Br-, I-) are actually Bronsted-Lowry bases because, as you said, they are conjugate bases to their protonated acids (ex: in the Bronsted-Lowry definition, I- is considered a base, albeit extremely weak, because HI is a strong acid. F- is considered a weak base, significantly stronger than I-, because its conjugate acid, HF, is a weak acid). Bronsted-Lowry definitions of acids just require that a compound can donate protons to water (or another base), and all protonated halogens (HF, HCl, HBr, HI) are therefore acids. Their ions cannot be Bronsted-Lowry acids because they don't have any protons to donate.
Interestingly, you can also use hard-soft acid-base theory to determine how strong of a Bronsted-Lowry acid a protonated halogen is. H+ is considered a hard Lewis acid, and so the harder the Lewis base the halogen anion is, the stronger the bond between the two, and thus the weaker it is as a Bronsted-Lowry acid. Of HF, HCl, HBr, and HI, HF is the weakest Bronsted-Lowry acid, and HI is the strongest (I- is the softest base of the halogen anions).
I'll probably make a video about this soon, because it's a pretty cool topic. Thanks for your question!
The molecular forms of the hydrogen halides are BL acids because they are eager to donate their proton. Once they do, the halide ion is then the conjugate base, while the proton acceptor becomes the conjugate acid. Lewis acids and bases on the other hand are electron acceptors or donors, respectively. By and large, the two theories agree on what constitutes acids and bases -- at least under aqueous conditions. I recommend theses short articles for a better picture of what's going on.
en.wikipedia.org/wiki/Br%C3%B8nsted%E2%80%93Lowry_acid%E2%80%93base_theory
en.wikipedia.org/wiki/Lewis_acids_and_bases
@@FoolishChemist That's actually a brilliant idea for a video, I don't think I've found anything describing that on YT that wasn't part of a loooooong lecture on multiple other concepts too.
I also like to use the double sided arrows for ion attractions now, nice representation
FIRST ALSO IM GLAD YOUR BACK!!!
Hey man, you look so much like one of my Chemsitry AP classmates I was genuienly stunned for a moment :c
Great video!
Nicely explained
If aluminum phosphide mix with water and make phosphine gas then will its solid powder become inactive ?
I think the solid formed from that reaction would be aluminum hydroxide, which is very insoluble and would precipitate out of solution if that's what you're asking
3:40 - fix the error!
Whoops! Thanks for catching this
Lol i like the aluminium phosphide part
bro died 💀
The algorithm brought me here.
W algorithm
dude u r a chemist and you should at least know how to write aluminium before making videos about it (:
0:15 you're mixing up Phosphine (PH₃) with Phosgene (COCl₂). Phosgene was used as a chemical warfare agent in WW1, not Phosphine.
Edit: Thanks a lot for wasting my time correcting you.