Ionic Compounds 2D3

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Maggie Doan 1I
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

Ionic Compounds 2D3

Postby Maggie Doan 1I » Mon Nov 12, 2018 7:30 pm

How do you determine which compounds have ionic bonds?
And why is BaBr2 primarily more ionic than BeBr2 and BBr3?

Emma Scholes 1L
Posts: 62
Joined: Fri Sep 28, 2018 12:18 am

Re: Ionic Compounds 2D3

Postby Emma Scholes 1L » Mon Nov 12, 2018 7:40 pm

A rough guideline to determine if something is an ionic bond is to use electronegativity. If the electronegativity difference is greater than 2, it is likely an ionic bond. BaBr2 is more ionic than BeBr2 and BBr3 because the electronegativity difference is greater.

Christopher Tran 1J
Posts: 77
Joined: Fri Sep 28, 2018 12:15 am

Re: Ionic Compounds 2D3

Postby Christopher Tran 1J » Mon Nov 12, 2018 7:44 pm

You can determine which atoms have ionic bonds by looking at their electronegativity differences. A difference of over approximately 2 typically means that there is an ionic bond.

The Ba - Br bond has a larger difference in electronegativity values compared to Be + Br and B + Br.

Br = 2.96, Ba = 0.89, Be = 1.57, B = 2.04

Ba-Br = 2.96-0.89 = 2.07 > 2, most ionic

Be-Br = 2.96-1.57 = 1.39

B-Br = 2.96-2.04 = 0.92


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