Use the References to access important values ifmee IA BA 2A 3A 4A SA 6A 7A Ge R
ID: 590335 • Letter: U
Question
Use the References to access important values ifmee IA BA 2A 3A 4A SA 6A 7A Ge Rs Se Br Kr Rt Rn The boiling point of IC1(97 C) is higher than the boiling point of Br (59 °C) because induced dipole forces are much stronger for ICI than for Br the molecular weight ofICI is 162.4, while that of Br, is 159.8. ICI is an ionic compound, while Br, is a molecular compound there is hydrogen bonding in ICL, but not in Br ICl is polar, while Bry is nonpolar Retry Eatire Group 2 more group attempts remaining ChExplanation / Answer
The boiling point of bromine is 58.8 C; the boiling point of ICl is 97.4 C, so the difference is fairly dramatic. In the bromine molecule, however, only dispersion forces operate. Dispersion forces also operate in ICl, and these would be expected to be greater in that the iodine atom, has a larger more polarizable electron cloud. In addition, in ICl there would be some degree of bond polarity in that chlorine is certainly more electronegative than iodine, and would tend to polarize electron density towards itself.
We could represent the resultant dipole as +ICl, and these dipoles would tend to align in such a way that tends to maximize intermolecular interaction:
+ICl+ICl+ICl
No such intermolecular interaction is available for BrBr, as this necessarily has a non-polar bond. And thus both bond polarity, and dispersion forces conspire to make the interhalogen less volatile. So the correct answer is A and E
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