Natural states of elements down a group

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Natural states of elements down a group

Postby 305920501 » Sun Dec 10, 2023 11:37 pm

I know a couple questions have shown up on exams about naturally occurring diatomic elements and their gaseous forms- I was wondering if there's any reason behind or trend to the states that elements prefer to be in. For example, down Group 17, I know F and Cl are diatomic and in a gas state at room temperature. Meanwhile, Br and I, both in the same group just below, are liquid and solid respectively at room temperature but also diatomic. Is there a reason for these changes down the group but but still a consistency of homonuclear diatomic molecules?

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Re: Natural states of elements down a group

Postby Chem_Mod » Tue Dec 12, 2023 3:44 pm

This trend is due to the increasing weight of the halogen as you go down the group! The iodine atom is massive compared to fluorine, and has many many more electrons. So when you have the molecule I2, it is going to have pretty strong Van der Waals disperson forces keeping these molecules together. The molecule is very heavy and there are a lot of electrons that can "slosh" around and create temporary dipoles. So, I2 is a solid. Br2 is lighter than I2, with weaker intermolecular forces, and will be a liquid. Cl2 and F2 are even lighter with even smaller intermolecular forces, so their molecules are free to spread out and make a gas! Since they have the same valence configuration, these atoms will bond in the same way, but their molecules exist in different states due to their differing weights.

I've moved this topic from coordination compounds to the intermolecular forces topic.

Return to “Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)”

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