Understanding the Relationship Between Ions and Dipoles: Debunking the Myth

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SUMMARY

Ions can possess dipoles, contrary to the misconception that they cannot because they are not compounds. The acetate ion, for example, demonstrates this phenomenon due to the presence of an extra electron in its carboxylate group, creating an electric gradient and resulting in a dipole moment. Additionally, even monoatomic ions can exhibit transient dipoles, which are temporary imbalances of charge. This discussion highlights the importance of understanding polyatomic ions and their dipole characteristics in chemistry.

PREREQUISITES
  • Understanding of polyatomic ions and their structures
  • Familiarity with dipole moments and electric gradients
  • Knowledge of intermolecular forces, specifically London dispersion forces
  • Basic concepts of ionic and covalent bonding
NEXT STEPS
  • Research the properties and examples of polyatomic ions
  • Study the concept of dipole moments in detail, focusing on induced and transient dipoles
  • Explore intermolecular forces, particularly London dispersion forces and their implications
  • Review the structure and behavior of common ions, such as acetate and nitrate
USEFUL FOR

Chemistry students, educators, and anyone interested in deepening their understanding of ionic compounds and dipole interactions.

Stalker23
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Can ions have dipoles?

ive had a really long argument with a teacher who says ions can't have dipoles because ions are not compounds...

can anyone clarify this for me please
 
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Ions can certainly have dipoles, since ions are not restricted to being monoatomic like the chloride anion or the lithium cation.

Consider the acetate ion (see attached figure). The acetate ion consists of a methyl group directly connected to a carboxylate group.

An oxygen atom in the carboxylate group contains an extra electron, which causes the carboxylate group to be negatively charged. Because the extra electron is localized on the carboxylate group, an electric gradient across the molecules is set up; which causes the dipole moment.

Perhaps your teacher, for the sake of the class, wanted to emphasize that the ions you will be dealing with ions which are strictly monoatomic; and because of spherical symmetry, wouldn't have a dipole moment. :smile:
 

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awsome
i think she's just stupid...at one point she said NF3 had no dipole. and i specifically asked her why NO3- wouldn't have one and she gave me that BS reson (ions arent compounds...)
thanks a lot
 
Last edited:
Even monoatomic ions can have transient dipoles.
 
really?

never heard of those...in AP Chemistry in HS
 
Never? I took AP Chemistry last year; transient dipoles are simply temporary imbalances of charge, which can exist among molecules or separate atoms.

Recall this from the "(London) dispersion forces" section in the chapter on intermolecular forces. (though, I don't know what textbook you are using)

...at one point she said NF3 had no dipole. and i specifically asked her why NO3- wouldn't have one and she gave me that BS reson (ions arent compounds...)
thanks a lot

Remind her of that common term, "polyatomic ions" :wink:
 
Last edited:
ha

im using Zumdahl, which my tacher warships like a god.

thanks again
 
Stalker23 said:
really?

never heard of those...in AP Chemistry in HS


maybe you haven't learned about it yet...?

i took that course last year and learned aboot them
 
well if its what i think your talking about, we call them tomporary dipoles or induced dipoles

:-p
 

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