IGCSE/GCSE/O & A Level/IB/University Student Forum

Qualification => Subject Doubts => GCE AS & A2 Level => Sciences => Topic started by: AN10 on June 08, 2010, 02:33:52 pm

Title: chem doubt
Post by: AN10 on June 08, 2010, 02:33:52 pm

Which of the following would behave most like an ideal gas at room temperature?
A carbon dioxide
B helium
C hydrogen
D nitrogen

Y helium y not hydrogen?

Title: Re: chem doubts
Post by: CHEMMASTER6000 on June 08, 2010, 02:42:21 pm

first , argon exist as an atom so it does not have bonds

second helium has a full octet structure so there are no intermolecular bonding

Title: Re: chem doubts
Post by: AN10 on June 08, 2010, 02:49:33 pm

Quote from: CHEMMASTER6000 on June 08, 2010, 02:42:21 pm

first , argon exist as an atom so it does not have bonds

second helium has a full octet structure so there are no intermolecular bonding

ok Thanks :)...i got da frst 1 so i deleted it!

Title: Re: chem doubt
Post by: Chingoo on June 08, 2010, 02:57:49 pm

You cannot say helium has NO intermolecular forces; intermolecular forces don't depend on electronic configuration as such. It is monoatomic, however, and is inert. It is not polar because it consists of single atoms alone and hence is less polarizable. Hydrogen is diatomic and has the same number of electrons (the complete molecule) as compared to a He, and due to its ability to be polarized (two atoms present), it's less ideal than Helium.

Title: Re: chem doubt
Post by: AN10 on June 08, 2010, 03:37:19 pm

Finally someone gave me a good explanation to this question....asked so many ppl but nobody could answer it well....so THANKS!