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Chapter 5: Problem 166

Arrange in order of increasing ionic character: \(\mathrm{CsBr}, \mathrm{KBr}, \mathrm{PBr}_{3} \mathrm{MgBr}_{2}\)

Short Answer

Expert verified
The order of increasing ionic character for the given compounds, based on electronegativity differences, is: \(PBr_3 < MgBr_2 < KBr < CsBr\).

Step by step solution

01

List the electronegativity values of the elements involved

Refer to a periodic table or electronegativity chart for the electronegativity values (Pauling scale) of the elements in question: Cesium (Cs): 0.79 Potassium (K): 0.82 Phosphorus (P): 2.19 Magnesium (Mg): 1.31 Bromine (Br): 2.96
02

Calculate electronegativity differences for each compound

Calculate the absolute electronegativity differences for each bond in the given compounds: CsBr: |2.96 - 0.79| = 2.17 KBr: |2.96 - 0.82| = 2.14 PBr₃: |2.96 - 2.19| = 0.77 (P-Br bond) MgBr₂: |2.96 - 1.31| = 1.65
03

Arrange compounds in increasing order of electronegativity difference

Arrange the compounds in order according to the electronegativity differences from step 2, in ascending order (lowest to highest): PBr₃ < MgBr₂ < KBr < CsBr Thus, the order of increasing ionic character is: PBr₃, MgBr₂, KBr, CsBr.

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Most popular questions from this chapter

What is a binary compound? Is atmospheric oxygen an example of a binary compound?

Without knowing the electronegativity values, in what situation can you be absolutely sure that the bonding between two atoms will be purely covalent?

The oxide ion is \(\mathrm{O}^{2-}\). How does this ion differ from the peroxide ion, \(\mathrm{O}_{2}^{2-} ?\) Draw dot diagrams for both.

Classify the bonds in each of the following as ionic, covalent, or polar covalent. Explain each choice. (a) \(\mathrm{Br}_{2}\) (b) \(\mathrm{PCl}_{3}\) (c) LiCl (d) ClF (e) \(\mathrm{MgCl}_{2}\)

Draw dot diagrams for \(\mathrm{Cl}_{2}\) and for \(\mathrm{MgCl}_{2}\) (put \(\mathrm{Mg}\) in the middle) that agree with the type of bonding occurring in each. (That is, show electrons as being shared or transferred, and if they are transferred, show the charges of the resulting ions.)
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