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anonymous
 4 years ago
how to tell whether an element is paramagnetic or diamagnetic
anonymous
 4 years ago
how to tell whether an element is paramagnetic or diamagnetic

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0simply by counting their electron if it is even then it is daimagnetic if it is odd then paramagnetic its a trick but here O2 is xception it is paramagnetic

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Do you know molecular orbital theory? We use it is to see if an element is paramagnetic or dia magnetic well odd electron species are always paramagnetic but you can decide for even numbers only by using MOT...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Write the orbitals in MOT and fill them up ans see if there are unpaired electrons if there are it is paramagnetic if not then it is diamagnetic.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i told its a trick not ans

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Whatever, i just told the ans :P

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0but if we have to distinguish between paramagnetic and diamagnetic oxide then?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Could you give an example?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0between Na2o, MgO, BeO

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Take the ion O2 and use MOT it has 18 electrons.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0so why you are not considering electrons in Na and Mg

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Good question i'm not sure :D

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Thats an ionic bond between Na+ and O even if you want to consider Na+ you would consider it seperately. Generally i would think you consider the O2, I;ve not heard of paramagnetic cations...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0well if u are doing ques of oxide as well u have to use MOT by which u can identify and u can use trick but dont use in theoretical xam if u are giving compound or oxide all u have to do is count electrons ok even in oxide same rule is followed.. here u cant convert in ions there is no sense to do so.. in ques they dont as individualy if they give oxide den y r u doing so

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Well Na2O is an ion isn't it? If O2 is paramagnetic then naturally the entire compound would be diamangnetic.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Heena i did not get what you are trying to say...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0O2 is exception wen u rite it by using MOT u ll find that

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0How is O2 is an exception? Na2O magnetic behaviour can be attributed to O2 ion.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0srrry O2 is not the xception O2 is exception..

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0By MOT even O2 is no exception there are two unpaired electrons in the pi* orbitals which lend it a para magnetic charcter.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i agree wat u saying but i m telling the exception acc. to the trick sir..dat i told her

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0For heavens sake please stop using sir.... :D
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