Very good question! In these diatomic acids, the strength of the acids is governed, not by electronegativity, but by the atomic size of the atom matched with hydrogen. Since iodine is a larger atom than chlorine, iodine's attraction to hydrogen will be weaker, allowing the H-I bond to break more readily than even the H-Cl bond when added to water.
Sir what about fazans rule where if there's a small cation and a large anion it causes polarization and has more covalent character thus making it not lose the H+ every easily. Where am I going wrong sir?
SLAMMED that like buttonn! Great video sir!!
Thanks for that like! And thanks for watching!
That conclusion part really helped me summarizing this topic! Thank you, Mr. Krug! ❤❤🧪
Thanks for your kind words! Hopefully that conclusion helps make sense of all these concepts put together.
Who else feels bad for the strong acid’s conjugate base😭 cmon man it’s trying its best!
You're right... But that poor base couldn't catch a proton to save its life!
For the last section question D, since chlorine is more electronegative, how come iodine is the stronger acid?
Very good question! In these diatomic acids, the strength of the acids is governed, not by electronegativity, but by the atomic size of the atom matched with hydrogen. Since iodine is a larger atom than chlorine, iodine's attraction to hydrogen will be weaker, allowing the H-I bond to break more readily than even the H-Cl bond when added to water.
Thank you, Mr. Krug.
@@JeremyKrugdoes this apply to everything
@@Lee-eb5ge wym🥸
thank you so much 🙏🙏
You're welcome, and thank you for watching!
Sir what about fazans rule where if there's a small cation and a large anion it causes polarization and has more covalent character thus making it not lose the H+ every easily. Where am I going wrong sir?