* Intermolecular Forces: Iodine (I₂) experiences stronger intermolecular forces than fluorine (F₂). Specifically, iodine exhibits London dispersion forces, which are stronger than the dipole-dipole interactions present in fluorine.
* Atomic Size and Polarizability: Iodine atoms are larger than fluorine atoms, making them more polarizable. This means the electron cloud in iodine is more easily distorted, leading to stronger London dispersion forces.
* Molecular Weight: Iodine has a higher molecular weight than fluorine, which also contributes to stronger intermolecular attractions.
In summary: The stronger intermolecular forces in iodine, due to its larger size, higher polarizability, and greater molecular weight, result in higher melting and boiling points compared to fluorine.
