Textbook Question 2D3

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Seraphina Joseph 1C
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Textbook Question 2D3

Postby Seraphina Joseph 1C » Sat Nov 14, 2020 3:42 pm

What makes BaBr2 have primarily ionic bonds and not the rest of them? Does the amount of Br have an effect on whether it has ionic or covalent bonds?

Lea Chamoun 2J
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Re: Textbook Question 2D3

Postby Lea Chamoun 2J » Sat Nov 14, 2020 4:07 pm

If you look at Figure 2D.2 in the textbook, it shows the electronegativity values for the elements. Because the difference in electronegativity is greater between Ba and Br than it is for B and Br or Be and Br, BaBr2 is the most ionic of the three.

Isaac Wen
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Re: Textbook Question 2D3

Postby Isaac Wen » Sun Nov 15, 2020 12:52 am

Seraphina Joseph 1C wrote:What makes BaBr2 have primarily ionic bonds and not the rest of them? Does the amount of Br have an effect on whether it has ionic or covalent bonds?


I don't think the amount of Br matters, at least in this case. The bond between Ba and one Br should be the same as the bond between Ba and the other Br atom. Therefore, we only have to take into account one of these same bonds when calculating the electronegativity difference.

Seraphina Joseph 1C
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Joined: Wed Sep 30, 2020 9:31 pm

Re: Textbook Question 2D3

Postby Seraphina Joseph 1C » Sun Nov 15, 2020 12:37 pm

Thank you this makes a lot of sense now!


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