ionic bonds

[emmaferry2D]

Which of these compounds has bonds that are primarily ionic? (a)
BBr3;(b) BaBr2;(c) BeBr2
the answer in the textbook is BaBr2 and i was wondering why it is not BeBr2, the two seem to be the same distance away from Br on the periodic table so I assumed they would have almost the same difference in electronegativity

[KhanTran3K]

Hey!
The answer would be BaBr2, since the difference in electronegativity would be much higher than BeBr2. By looking at the trends, Ba is much lower than Be in column 2, meaning it has a much larger radius, and therefore, less electronegativity. This would result in a higher difference in electronegativity between the Ba and the Br. Feel free to correct me if I am wrong. Hope this helps!

[Namratha Gujje]

Electronegativity decreases as we go down a period and Ba is much lower in group 2 meaning that it has a lower eneg than Be. Because of this, the electronegativuty difference would be greater in BaBr2 making it the one that is the most ionic.

[AmyHo2K]

Electronegativity is lower down a group so there would be more of difference between Ba and Br.

[Lung Sheng Liang 3J]

BaBr2 would be the most ionic compound b/c it has less electronegativity than BeBr2 since it is further down the period.

[305607822]

Ba is way further down the period table on the left side so it has a big radius and thus lower electronegativity.

[Acharya Ranawat 3E]

Ba and Br have the greatest difference in electro negativity which means it is most likely to be ionic. This is becasue ionic bonds are formed when there is the great difference in electro negativity. Hope this helps!

[305561744]

Since Ba is so far down the periodic table, it has a great deal of electron shielding, meaning it is not very electronegative. This results in the ionic bond.

[Hannah Thornton 1F]

BaBr2 would be the most ionic because it has the greatest electronegativity. Since electronegativity decreases as we go down a period, and Ba is lower down than Br on the periodic table, this compound would be very electronegative.

[Alexis Rempillo 3B]

Generally speaking with trends, Ba would have a lower electronegativity than Be since it's closer to the bottom-left (where electronegativity is low). With the data from the interweb, Ba has an electronegativity of 0.89 compared to Be's electronegativity of 1.57. There would be a greater difference in electronegativity between BaBr2 than BeBr2 because of Ba's low electronegativity. Meaning, BaBr2 is more ionic.

[haryn Shin 1H]

Considering the trends in the periodic table, the electron affinity, and thus the electronegativity is lower towards the bottom of the periodic table, which results in greater difference in electronegativity for BaBr2 than BeBr2. Greater difference in electronegativity means that the compound is more ionic. Hope this helps!

[Maddie Klee 3K]

To determine which one has bonds that are primarily ionic you need to find the difference in electronegativity between the two atoms. By looking at the periodic trend of electronegativity, we can see that electronegativity increase as you move up a group and across a period. Since electronegativity decreases as we go down a period and Ba is much lower in group 2 than Be, it has a lower electronegativity. Due to this, the electronegativity difference would be greater in BaBr2 than in BeBr2, making it the one that is the most ionic out of the compounds.

[Mahima Manoj 1F]

As electronegativity decreases down a group, Ba has a lower electronegativity than Be, which means that the difference of electronegativity between BaBr2 is greater than the difference between BeBr2. So BaBr2 would be more ionic

[madelyn kelly 1I]

The trend in the periodic table conveys that F is the most electronegative element, so moving diagonally right towards F would lead to higher electronegativity. On the other hand, moving down a group would decrease electronegativity. Because Ba and Br would have a higher difference in electronegativity based on the trend, it would be more ionic.