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Postby madisondesilva1c » Fri Nov 02, 2018 11:23 am

Todays lecture ended with the introduction of Dipole, how do you represent dipole with an arrow if two atoms are very similar in electronegativity? Will this ever be the case or will one always be more electronegative than the other?

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Re: Dipole

Postby melodyzaki2E » Fri Nov 02, 2018 11:27 am

I think one will always be at least slightly more electronegative than the other; if they're the same element (like N2) then there wouldn't be any dipole moments because they would have equal electronegativity, i'm not totally sure though.

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Re: Dipole

Postby 305154707 » Fri Nov 02, 2018 11:52 am

Hi ! This was discussed in relation to polar covalent bonds. In these types of bonds, one atom will always be more electronegative than the other(s), giving a separation of charge. In this case you could draw the arrow showing the direction of the dipole/dipole moment. A nonpolar covalent bond has a very small difference in electronegativity, or no difference at all. An example would be O2. Because the O atoms have the same electronegativity, you couldn't distinguish where the probable "pooling" of electrons would be.

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Re: Dipole

Postby LaurenJuul_1B » Fri Nov 02, 2018 11:55 am

Dipole has to do with polar covalent bonds! This means that one of the atoms will always be more electronegative, and in turn you will be able to draw the arrow without worrying about the atoms being too close in electronegativity.

Danny Elias Dis 1E
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Re: Dipole

Postby Danny Elias Dis 1E » Fri Nov 02, 2018 11:42 pm

Do dipole moments have characteristics of ionic bonds too?

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