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In lecture we discussed that the reasoning behind the physical states of these molecules was based off of the strength of their dispersion forces. The dispersion forces of F2 and Cl2 are weaker, seeing that they are relatively smaller and less polarizable. Because of this, they remain in the gas phase, with no particles strictly bound close together. On the other hand, Br2 is a solid seeing that its dispersion forces are a little stronger in comparison with F2 and Cl2. This holds the particles somewhat together, but without any definite shape. Lastly, I2 is a solid at room temperature because of the fact that its dispersion forces are the strongest, holding its particles tightly together.
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