the colour of a compound is usually attributed to the presence of unpaired electrons in outermost shell of the central element.in the givn q,we have to find out the oxidation states of the metals of the corresponding compounds and then obtain the hybridisation of the respective metal ions considering the effect of the ligands using vbd or crystal field theory. in case the central metal ion present in the compound possesses an unpaired electron after considering the effects of the ligand fields,we can conclude that the compound is coloured.
as explained above,in the compound CuF2,Cu is in +2 state,which has a d9 configuration.in addition,as F is a weak field ligand,it will,under o circumstances,cause pairing up of electrons.in this case,however,d9 configuration makes it impossible for pairing to occur even when strong ligands are present.hence,we can conclude that CuF2 is coloured.
"Many of the things you can count,dont count....
Many of the things you cant count,really do count...."-Albert Einstein
"The important thing in science is not so much to obtain new facts as to discover new ways of thinking about them"-William Bragg
"An inexplicable fact is infinitely preferable to an incomprehensible mystery"-F. Soddy
RISHIPRATIM MAZUMDAR
NIT DURGAPUR
1ST YEAR,ELECTRONICS AND COMMUNICATIONS
Moderation Team
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