I appreciate these videos more than anything in the world right now. Thank you for everything you’re doing, and having it for anyone to watch for free. You are amazing!
Good question, and yes they do. Vapor pressure is often assessed as part of a gas law question, and since this concept pops up throughout the course from time to time, I wanted to introduce it here. Thanks for watching!
Molecular solids are common molecules (water, carbon dioxide, almost any molecular compound) when it's in the solid form (ice, dry ice, etc.) These have forces holding them together to maintain their solid form. Covalent network solids are associated by a much stronger force, and you don't have to know very many of these for AP (SiO2, graphite, diamond are the main examples). CNS have melting/boiling points that are usually even higher than ionic compounds. Great question!
Can we say that both CO2 and SiO2 have London dispersion forces, but SiO2 has more electrons, and the more electrons a molecule has, the more polarizable it is and the stronger it is, and the more stronger molecule's LDFs, the higher boiling points?
We could say that, but the difference in boiling point between CO2 and SiO2 is so great that there's another force here. SiO2 is a covalent network solid; each Si atom has bonds with O atoms in multiple directions; this is the main reason SiO2 has such a high b.p. compared to CO2.
For AP Chem, there are really only a very limited number of covalent network solids you're expected to know: diamond, graphite, SiO2, and SiC. The trick is knowing that covalent network solids have bonds spread in multiple dimensions. Any molecular/covalent compound can be a molecular solid if we get the temp cold enough.
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I appreciate these videos more than anything in the world right now. Thank you for everything you’re doing, and having it for anyone to watch for free. You are amazing!
I'm glad you're able to make use of my videos. I have lots more on the way!
These videos are so amazing! Keep it up Jeremy!
Thanks for the kind words. I have lots more videos on the way!
You are truly wonderful, Sir 🎉🥼!
Thank you so much for your kind words!
I haven’t seen vapour pressure in the 3.2 AP videos. Do they come up on the exam?
Good question, and yes they do. Vapor pressure is often assessed as part of a gas law question, and since this concept pops up throughout the course from time to time, I wanted to introduce it here. Thanks for watching!
Amazing videos
Thanks for watching!
could you differentiate between molecule solids and covalent network solids? thanks
Molecular solids are common molecules (water, carbon dioxide, almost any molecular compound) when it's in the solid form (ice, dry ice, etc.) These have forces holding them together to maintain their solid form. Covalent network solids are associated by a much stronger force, and you don't have to know very many of these for AP (SiO2, graphite, diamond are the main examples). CNS have melting/boiling points that are usually even higher than ionic compounds. Great question!
Can we say that both CO2 and SiO2 have London dispersion forces, but SiO2 has more electrons, and the more electrons a molecule has, the more polarizable it is and the stronger it is, and the more stronger molecule's LDFs, the higher boiling points?
We could say that, but the difference in boiling point between CO2 and SiO2 is so great that there's another force here. SiO2 is a covalent network solid; each Si atom has bonds with O atoms in multiple directions; this is the main reason SiO2 has such a high b.p. compared to CO2.
❤❤❤❤
how do you know if a molecule is a covalent network solid vs just a molecular solid?
For AP Chem, there are really only a very limited number of covalent network solids you're expected to know: diamond, graphite, SiO2, and SiC. The trick is knowing that covalent network solids have bonds spread in multiple dimensions. Any molecular/covalent compound can be a molecular solid if we get the temp cold enough.
amazing video❤❤unit exam tomorrow😢😢😢
You will do great on your exam!
🤓💀