Concept:Intermolecular forces in perfectly non-polar molecules rely solely on the random, temporary movement of electron clouds.
Formula:Not applicable.
Solution:- Iodine (\( \text{I}_2 \)) is a homonuclear diatomic molecule. Because both iodine atoms share the electrons equally, the molecule is perfectly symmetrical and non-polar, possessing a net dipole moment of zero.
- At any given instant, the large electron cloud can randomly shift to one side, creating a temporary, instantaneous dipole.
- This temporary dipole distorts the electron cloud of a neighboring \( \text{I}_2 \) molecule, creating an "induced" dipole.
- The resulting electrostatic attraction is called an Instantaneous dipole-induced dipole force (formally known as London Dispersion Forces).
Why other options are incorrect:Dipole-dipole forces require permanent polarity, which iodine lacks. Dipole-induced dipole forces require a mixture of polar and non-polar substances.
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