Dipole-Dipole forces

(Polar molecules, Non-polar molecules, etc.)

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Lauryn Shinno 2H
Posts: 59
Joined: Fri Sep 28, 2018 12:24 am

Dipole-Dipole forces

Postby Lauryn Shinno 2H » Sun Nov 18, 2018 8:56 am

Does everything have dipole-dipole forces unless atoms of the same element are arranged symmetrically around the central atom?

Samantha Kwock 1D
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

Re: Dipole-Dipole forces

Postby Samantha Kwock 1D » Sun Nov 18, 2018 10:02 am

No, it depends on the electronegativity differences between the atoms involved in the bond. If the electronegativity difference between the two atoms involved in the bond is small, then the bond is non-polar and its arrangement around the central atom does not matter.

Hannah Padilla 1H
Posts: 29
Joined: Fri Sep 28, 2018 12:19 am

Re: Dipole-Dipole forces

Postby Hannah Padilla 1H » Sun Nov 18, 2018 10:30 am

However, the the bonds are polar, and the either the atoms are arranged symmetrically or in another way that the dipole forces cancel out, then the molecule is considered nonpolar.

George Ghaly 2L
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Re: Dipole-Dipole forces

Postby George Ghaly 2L » Sun Nov 18, 2018 1:47 pm

Dipole-dipole forces occur when their a great difference between the electronegativity of two atoms. When determining the dipole forces it is important to consider if they cancel or not because then polarity can be inferred.

Aiden Atoori 1C
Posts: 67
Joined: Fri Sep 28, 2018 12:24 am

Re: Dipole-Dipole forces

Postby Aiden Atoori 1C » Sun Nov 18, 2018 1:50 pm

Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces have strengths that range from 5 kJ to 20 kJ per mole. They are much weaker than ionic or covalent bonds and have a significant effect only when the molecules involved are close together (touching or almost touching).

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