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Chapter 8: Problem 18

Which ionic compound is expected to form from combining the following pairs of elements: (a) barium and fluorine, (b) cesium and chlorine, (c) lithium and nitrogen, (d) aluminum and oxygen?

Short Answer

Expert verified
The ionic compounds formed from the given pairs of elements are: (a) BaF₂, (b) CsCl, (c) Li₃N, and (d) Al₂O₃.

Step by step solution

01

Identify the charges of the ions

Barium (Ba) is in Group 2, so it tends to form a +2 ion (Ba²⁺). Fluorine (F) is in Group 7 (also known as Group 17), so it tends to form a -1 ion (F⁻).
02

Combine the ions to form an ionic compound

To form a stable ionic compound, we need the charges to balance out. In this case, we will need two F⁻ ions to balance the charge of one Ba²⁺ ion. The ionic compound formed will be BaF₂. #b) Cesium and Chlorine#
03

Identify the charges of the ions

Cesium (Cs) is in Group 1, so it tends to form a +1 ion (Cs⁺). Chlorine (Cl) is also in Group 7 (Group 17), so it tends to form a -1 ion (Cl⁻).
04

Combine the ions to form an ionic compound

In this case, the charges of the ions are already balanced. We can directly combine one Cs⁺ ion with one Cl⁻ ion to form the ionic compound CsCl. #c) Lithium and Nitrogen#
05

Identify the charges of the ions

Lithium (Li) is in Group 1, so it tends to form a +1 ion (Li⁺). Nitrogen (N) is in Group 5 (Group 15), so it tends to form a -3 ion (N³⁻).
06

Combine the ions to form an ionic compound

We will need three Li⁺ ions to balance the charge of one N³⁻ ion. The ionic compound formed will be Li₃N. #d) Aluminum and Oxygen#
07

Identify the charges of the ions

Aluminum (Al) is in Group 13, so it tends to form a +3 ion (Al³⁺). Oxygen (O) is in Group 6 (Group 16), so it tends to form a -2 ion (O²⁻).
08

Combine the ions to form an ionic compound

In this case, we will need two Al³⁺ ions to balance the charge of three O²⁻ ions, giving us a compound ratio of 2:3. The ionic compound formed will be Al₂O₃.

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Most popular questions from this chapter

(a) What is meant by the term electronegativity? (b) On the Pauling scale what is the range of electronegativity values for the elements? (c) Which element has the greatest electronegativity? (d) Which element has the smallest electronegativity?

Arrange the bonds in each of the following sets in order of increasing polarity: (a) \(\mathrm{C}-\mathrm{F}, \mathrm{O}-\mathrm{F}, \mathrm{Be}-\mathrm{F} ;\) (b) \(\mathrm{O}-\mathrm{Cl}\), \(\mathrm{S}-\mathrm{Br}, \mathrm{C}-\mathrm{P} ;(\mathrm{c}) \mathrm{C}-\mathrm{S}, \mathrm{B}-\mathrm{F}, \mathrm{N}-\mathrm{O}\)

Consider the following statement: "For some molecules and ions, a Lewis structure that satisfies the octet rule does not lead to the lowest formal charges, and a Lewis structure that leads to the lowest formal charges does not satisfy the octet rule." Illustrate this statement using the hydrogen sulfite ion, \(\mathrm{HSO}_{3}^{-}\), as an example (the \(\mathrm{H}\) atom is bonded to one of the \(\mathrm{O}\) atoms).

Based on Lewis structures, predict the ordering of \(\mathrm{N}-\mathrm{O}\) bond lengths in \(\mathrm{NO}^{+}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\).

The substance chlorine monoxide, \(\mathrm{ClO}(g)\), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has a dipole moment of \(1.24 \mathrm{D}\) and the (a) Determine the magnitude of \(\mathrm{Cl}-\mathrm{O}\) bond length is \(1.60 \mathrm{~A}\). the charges on the \(\mathrm{Cl}\) and \(\mathrm{O}\) atoms in units of the electronic charge, e. (b) Based on the electronegativities of the elements, which atom would you expect to have a negative charge in the ClO molecule? (c) By using formal charges as a guide, propose the dominant Lewis structure for the molecule. Are the formal charges consistent with your answers to parts (a) and (b)? Can you reconcile any differences you find?
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