Chemistry, 20.02.2020 09:02 Cassandoo

Explain how you would expect the strength of
the ionic bonds in potassium bromide (KBr) to compare with that of the
bonds in lithium bromide (LiBr).

Answers: 2

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Answer from: mydoggy152

The comparison of the strength of the ionic bonds in potassium bromide KBr to that of the

bonds in lithium bromide (LiBr);. The strength of the ionic bonds in Potassium bromide (KBr) is weaker than the bonds in Lithium bromide (LiBr).

Although, Lithium and Potassium are elements I. the group 1 of the periodic table as a result of their +1 Valency.

While comparing the ionic radius of Lithium and Potassium, it is evident that the ionic radius of Lithium is smaller and hence,

Lithium has a greater electrostatic attraction between its nucleus and Valence electron.

Since, the strength of an ionic bond is inversely proportional to the distance between the nucleus of the constituent elements.

The ionic bond strength in LiBr is stronger than that in Potassium bromide, KBr.

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Answer from: kenzie5889

You should expect that the ionic bond in LiBr is stronger than the bond in KBr.

Explanation:

The ionic bonds are formed by the electrostatic attraction between the ions, cations and anions.

In KBr the cation is K⁺ and the anion is Br⁻.

In LiBr the cation is Li⁺ and the anion is Br⁻.

You must expect that the bond strength depends mainly on the charges present on each ion and the distance between them.

Nevertheless, the effect of the distance between the radius dominate the trendency of the bond strength, which makes that the ionic strength trend be related to the ionic radius trend.

Lithium is a smaller ion than Potassium (both are in the same group and Lithium is above Potassium).

Thus, you should expect that the Li ion is closer to the Br ion than what the K ion is to the Br ion and expect that the bond between a Li ion and the Br ion be stronger than the bond between the K ion and the Br ion.

Answer from: Quest

The mass has escaped into a gas which you can not see so the law stays true.

Answer from: Quest

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Explain how you would expect the strength of
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