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Sean Phen
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Postby Sean Phen » Sun Nov 22, 2020 8:58 pm

How can you tell if a molecule is dipole-dipole interaction?

Bailey Giovanoli 1L
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Re: Dipole-Dipole

Postby Bailey Giovanoli 1L » Sun Nov 22, 2020 9:00 pm

If the molecules interacting are dipoles independently of one another, then there is a dipole-dipole interaction. An example of this is two HF molecules interacting.

Katie Lam 2J
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Re: Dipole-Dipole

Postby Katie Lam 2J » Sun Nov 22, 2020 9:03 pm

You can tell if there is an electronegativity difference between the atoms. This electronegativity difference helps you determine whether a bond is polar, and dipole-dipole interactions can only occur between polar molecules. Hope this helps!

Nicole Bruno Dis 1B
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Re: Dipole-Dipole

Postby Nicole Bruno Dis 1B » Sun Nov 22, 2020 9:11 pm

You look at an atom's electronegativity. If the difference is in the range between 0.4 and 1.7, then the molecule is considered polar and if a molecule is polar, it is likely caused by a dipole-dipole interaction. Polar molecules contain polar bonds that create dipoles caused by a positive/negative charge difference.

Elena Chen 2E
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Re: Dipole-Dipole

Postby Elena Chen 2E » Sun Nov 22, 2020 9:20 pm

Molecules that are polar contain dipole moments, which means atoms within the molecule have significant differences in electronegativity. If two molecules interacting are both polar, then it is likely that there is a dipole-dipole interaction.

Taha 2D
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Re: Dipole-Dipole

Postby Taha 2D » Sun Nov 22, 2020 9:22 pm

They both should have dipoles independant of each other and need to have a significant difference electronegativity to form dipole interactions.

Kelly Ha 1K
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Re: Dipole-Dipole

Postby Kelly Ha 1K » Sun Nov 22, 2020 9:43 pm

Polar molecules have dipole moments due to the unequal distribution of electrons, so a dipole-dipole interaction consists of attraction between two or more polar molecules. You can usually tell if there is a dipole-dipole interaction if you can identify if the molecules involved are polar (for example, drawing out the Lewis structure and checking for asymmetry). You can also look at the electronegativity differences- if the difference is between 0.4 and 1.7, then it is a polar bond.

Hailey Qasawadish 2J
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Re: Dipole-Dipole

Postby Hailey Qasawadish 2J » Sun Nov 22, 2020 10:01 pm

As a general rule, polar molecules have dipole dipole interactions because there is an unequal sharing of electrons causing a dipole moment. Hope this helps!

Melissa Solis 1H
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Re: Dipole-Dipole

Postby Melissa Solis 1H » Sun Nov 22, 2020 10:04 pm

First thing you should know is that a dipole-dipole interactions is that they occur between stationary polar molecules. Additionally, it's an interaction between two electron dipoles; like partial charges repel and opposite charge attract. They have a significant effect only when they are very close to one another.

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Re: Dipole-Dipole

Postby AntonioZarich2E » Sun Nov 22, 2020 10:05 pm

Dipole-Dipole bonds are formed when each is a polar molecule, independent of the other one.

Joanna Huang
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Re: Dipole-Dipole

Postby Joanna Huang » Sun Nov 22, 2020 10:24 pm

Dipole dipole interaction are between two molecule with oppositely charged ends. You can tell when they are oppositely charged when the atoms in the molecule have different electronegativities. This means that one of the atom in the molecule has a greater tendency to attract electrons, thus even though they are connected by a covalent bond, the electrons tend to be attracted closer to the atom with greater electronegativity. Have two of these types of molecules together, and that's a dipole dipole interaction.

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