why is the boiling point of F2 lower than that of I2?

Question

somethign related to the trends in the periodic table?

Answer 1

The boiling point of a liquid substance depends on the strength of the intermolecular forces. The stronger these interactions the more energy you need to provide to break them so that the molecules go into the gaseous phase. As Teroy mentioned in this case you have only London forces, that is induced dipole-induced dipole forces. Iodine is more polarizable because it is bigger, thus induced dipoles are more readily formed, which results in stronger intermolecular interactions and finally in higher boiling point.

Answer 2

Fluorine Boiling Point

Answer 3

In the UK we tend to call these weak attractive forces between all molecules van der Waal's forces, but the principle is the same - their size depends on the number of electrons in the molecule, which is much bigger with iodine than with fluorine.

Answer 4

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You need to distinguish between intermolecular and intramolecular bonding. The intermolecular bonding of the halogens increases as you go down the group (and increase in size)

Answer 5

this two molecules is nonpolar and so the only intermolecular force acting on it is London force... with such IMFA the boiling point will depend only on the molecular weight of the molecules. since Iodine is heavier than fluorine then it will have higher boiling point.

best answer?

Answer 6

This may help. Very detailed answer

http://perfectpracticemakesperfect.org/2014/01/03/the-melting-points-of-alkali-metals-decrease-from-li-to-cs-in-contrast-the-melting-points-of-halogens-increase-from-f2-to-i2-why-what-is-the-expected-trend-in-the-melting-points-of-the-compounds-l/

Answer 7

erm... u only got it wrong cos u missed out At, astatine, which is even higher than Iodine. should be At>I>Br>Cl>F