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Nov 3, 2016 at 20:32 answer added Roland S. timeline score: 0
Sep 23, 2016 at 23:57 history tweeted twitter.com/StackChemistry/status/779469669803683840
Sep 23, 2016 at 21:36 vote accept R. Mauban
Sep 23, 2016 at 16:05 history edited Martin - マーチン CC BY-SA 3.0
contracted links, minor spell check
Sep 23, 2016 at 16:00 answer added Martin - マーチン timeline score: 10
Sep 23, 2016 at 7:42 comment added Ivan Neretin There was no confusion at all; when you say "dipole moment", you do mean "permanent dipole moment", that's the default assumption. Yes, by the reasons listed above this molecule does have some dipole moment, but I would not be surprised if it is 0.00 when rounded to 2 decimal digits.
Sep 23, 2016 at 6:22 history edited R. Mauban CC BY-SA 3.0
edited title
Sep 23, 2016 at 6:21 comment added R. Mauban Sorry for the confusion, I meant a permanent dipole moment. I will adjust the question to clarify this.
Sep 23, 2016 at 6:08 comment added orthocresol Well, the correct answer to the way you phrased your question is: of course it does have a dipole moment. Whether the dipole moment is significant enough for us to consider the molecule to be polar, is a different matter entirely. But that is not the question asked. The question is "does it have a dipole moment" and the answer is "yes".
Sep 23, 2016 at 5:59 comment added Khan In my thought the dipole moment of 1-bromo-4-chlorobenzene is 0, there is not that much difference in the electronegativity of Chlorine(3.0) and bromine (2.8).
S Sep 23, 2016 at 5:58 history suggested Khan CC BY-SA 3.0
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Sep 23, 2016 at 5:55 review Suggested edits
S Sep 23, 2016 at 5:58
Sep 23, 2016 at 5:52 review First posts
Sep 23, 2016 at 6:56
Sep 23, 2016 at 5:49 history asked R. Mauban CC BY-SA 3.0