A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 4 years ago
can anyone pls suggest the reason why,CO2 and SiO2 are not isostructural at 300K???
anonymous
 4 years ago
can anyone pls suggest the reason why,CO2 and SiO2 are not isostructural at 300K???

This Question is Closed

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1When comparing molecules and ions that are isoelectronic, only with the respect to their valance electrons, the expectation of isostructural behaviour may not hold. To take your situation: CO2 and SiO2 at room temperatur and pressure, CO2 is a linear molecule but SiO2 has an extended strcture containing silicon atoms in terahedral environments. An extended solid phase form of CO2 has been made at about 1900 K and 40 gigapascal pressure (If I remember right). This has a quartzlike structure, quartz being a 3dimensional polymorph of SiO2. In the gas phase however we find SiO2 as linear triatomic molecules. A reason for this can be explained saying the vibrational modes may be thermally excited (in a classical interpretation one expresses this by stating that “the molecules will vibrate faster”), but they oscillate still around the recognizable geometry of the molecule.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0does geometry of these molecules takes the major part in this case???

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0overall and simply why they do not exist isostructural at this temperature? is it b'coz of the structural change or any other???

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1kk. Had your lectures about temperature, internal energy, molecular energy and vibrational modes? (perhaps morse potential aswell)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0nw im going through the lectures of internal energy :)

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1Alrightie :) Anyway you know that the energy for the distance between atoms looks like this right?dw:1356793711039:dw

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1Well same idea aplies to angles between atoms  beside they are diffrence from atom to atom (in some cases)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0fine explain more pls....

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1dw:1356793835811:dw

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1The energy levels of the two molecules are diffrence... CO2 is more stable in its linare form at 300 K (room tempture), while SiO2 is not.

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1Sorry my drawings suck..

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0is SiO2 having a constant graph?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0nt abt the drawings it s about the matter we r discussing:)..... i can undestand :) looks gud anyway...

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1dw:1356794123184:dwIt would (without being sure) maybe look like this:

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1Else I can suggest you read about vibrational modes of molecules, I sure belive I will becuase I'm a bit unsure (molecular geometry is not my best :P) :)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i hav no idea abt vibrational modes.... suggest any reading materials... if u can :)

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1What textbook do you use? (might be I have it)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0open university books...

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1In that case I see if I can find some lecture notes here from the University of Copenhagen.

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1That are not in Danish :P

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Bt u explained me some basic ideas... :) thanx alot 4 dat

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1Well I wish i could explain it better, mostly only work with the equations and then make conseqences from that.. Anyway, I can find some good reading in my open lectures, however else take a look at the wiki: http://en.wikipedia.org/wiki/Molecular_vibration

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0im on wiki nw thanx :):)

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1No prob, have a good day and if you are good with organic chemistry please see if you can answer my question :P

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i tried bt couldnt... im jst a beginner:).... if i find anywhere... sure i'll let u knw... :)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Carbon is a lot smaller than silicon. Being that small, it can more readily involve the closerin p valence orbitals to form pi bonds to neighboring oxygen atoms  which gives you the CO2 molecule. Silicon, on the other hand, has a harder time involving the 3p orbitals in pi bonding to its neighbors, so it generally prefers to stick to sigma bonds. That means to satisfy its valence it forms bonds to four  not two  neighboring oxygens, which results in the extended diamondoid structure of silica at 300K. This is one of the illustrations of how the first element in each group often behaves nontrivially different from the others. One of the more significant is that the second row elements, being much smaller, form pi bonds much more readily than the elements in Period 3 and higher. You can see a similar effect in Group 6A: oxygen readily forms the doublebonded O2 molecule and exists as a gas at STP, while sulfur, just below it, instead prefers to form extended rings and chains of single bonds, and exists in the solid state at STP. Same with Group 5A: nitrogen forms the triply bonded N2, while phosphorus exists as the pyramidal P4 and is a solid at STP. No idea what molecular vibrations has to do with anything.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0do u mean the different types bonding of these two plays the key role???

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0No, I mean the size of the atoms plays an important role in the types of bonding each prefers, and that, in turn, explains why they form two different types of oxides.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0fine.... size might be factor... i didnt think abt the size...thanx alot :)

Frostbite
 4 years ago
Best ResponseYou've already chosen the best response.1CarlFarm, your way is way more specific, and also giveing a more actural reason, but the reason i used molecular vibrations is just a matter of approach, however your explination is more specific, what I wrote is only what I have experinced and choosed to see as energy that changes the molecule's 3dimensional geometry.
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.