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Chapter 8: Problem 16

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 by combining the given pairs of elements are: (a) Barium Fluoride: \(BaF_2\) (b) Cesium Chloride: \(CsCl\) (c) Lithium Nitride: \(Li_3N\) (d) Aluminum Oxide: \(Al_2O_3\)

Step by step solution

01

(Step 1: Determine the charge of each ion)

Using the periodic table, we can determine the charge of each ion in the given pairs of elements. For example, metals in Group 1 have a charge of +1, metals in Group 2 have a charge of +2, and nonmetals in Group 17 have a charge of -1.
02

(a) Barium and Fluorine)

Barium (Ba) is a Group 2 element, so its ion has a charge of +2 (Ba^2+). Fluorine (F) is a Group 17 element, so its ion has a charge of -1 (F^-).
03

(b) Cesium and Chlorine)

Cesium (Cs) is a Group 1 element, so its ion has a charge of +1 (Cs^+). Chlorine (Cl) is a Group 17 element, so its ion has a charge of -1 (Cl^-).
04

(c) Lithium and Nitrogen)

Lithium (Li) is a Group 1 element, so its ion has a charge of +1 (Li^+). Nitrogen (N) is a Group 15 element, so its ion has a charge of -3 (N^3-).
05

(d) Aluminum and Oxygen)

Aluminum (Al) is a Group 13 element, so its ion has a charge of +3 (Al^3+). Oxygen (O) is a Group 16 element, so its ion has a charge of -2 (O^2-).
06

(Step 2: Combine the ions to form ionic compounds)

Now that we have the charges, we can combine each pair of elements in a way that their overall charge is neutral, forming the ionic compound.
07

(a) Barium and Fluorine)

To achieve a neutral charge, we need two fluorine ions for each barium ion: \[Ba^{2+} + 2F^{-} \rightarrow BaF_2\]
08

(b) Cesium and Chlorine)

To achieve a neutral charge, we need one chlorine ion for each cesium ion: \[Cs^{+} + Cl^{-} \rightarrow CsCl\]
09

(c) Lithium and Nitrogen)

To achieve a neutral charge, we need three lithium ions for each nitrogen ion: \[3Li^{+} + N^{3-} \rightarrow Li_3N\]
10

(d) Aluminum and Oxygen)

To achieve a neutral charge, we need two aluminum ions for each three oxygen ions: \[2Al^{3+} + 3O^{2-} \rightarrow Al_2O_3\] So, the ionic compounds formed by combining the given pairs of elements are: (a) Barium Fluoride: \(BaF_2\) (b) Cesium Chloride: \(CsCl\) (c) Lithium Nitride: \(Li_3N\) (d) Aluminum Oxide: \(Al_2O_3\)

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