Textbook Problem 2D.3

[MinjooPark_3I]

I honestly do not know if this fits into this topic but I needed help with
Which of these compounds has bonds that are primarily ionic? (a) BBr3; (b) BaBr2; (c) BeBr2.

I thought we were just supposed to see how far away the two elements were to see the largest difference in electronegativity, but I am not quite sure. Thank you for any help!

[Q Scarborough 1b]

Hi,
You are correct in that you are supposed to find the largest difference in electronegativity. For this question, that largest electronegativity difference would be BaBr2, making it the most ionic.

[Thomas Vu 1A]

One shortcut you can take to determine which molecules are primarily ionic are to just say that Be and Ba are metals while Br is a nonmetal which fits the definition for ionic. Boron on the other hand is a nonmetal and 2 nonmetals cannot make an ionic molecule.

[Jaclyn Dang 3B]

You are right in the fact that you look at how far away they are. I had trouble with this one too they they seem almost the same. Hope this helps.

[MinjooPark_3I]

I'm sorry, but I still do not quite understand how we measure the difference in electronegativity. Do we have to count the amount of elements in between them? or do we compare the sizes of the elements? Thank youu for any help!

[MinjooPark_3I]

I'm sorry, but I still do not quite understand how we measure the difference in electronegativity. Do we have to count the amount of elements in between them? or do we compare the sizes of the elements? Thank youu for any help!

Oh. I just realized I could just look at the electronegativity chart... OOPS ahaha. Will the electronegativity chart be provided during the exam if there is a question like this? Thank you for everyone that clarified!!