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Ch.8 - Basic Concepts of Chemical Bonding
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All textbooksBrown 14th EditionCh.8 - Basic Concepts of Chemical BondingProblem 23b

Chapter 8, Problem 23b

The substances NaF and CaO are isoelectronic (have the same number of valence electrons). (b) What are the charges of each of the anions in each compound?

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Hey everyone. Our question here is asking us to determine the charges of the ions in the ISO electronic substances. Our first one being magnesium sulfide and the second one being potassium chloride. For our first one magnesium sulfide, we know that we have magnesium with a plus two charge and sulfur with a minus two charge. Since it's in our group +68 and are an ion in this case is going to be sulfur and magnesium is going to be our caddy on. Moving on to potassium chloride. We know that potassium has a plus one charge since it's in our group one a And Chlorine is in our group seven a with a -1 charge. Again, chlorine is are an ion since it has that negative charge And the charge is going to be a -1. So I hope this made sense. And let us know if you have any questions.
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Related Practice
Textbook Question

NaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (a) The lattice energies of NaCl and KF are given in Table 8.1. Based on the lattice energies, would you expect the Na─Cl or the K─F distance to be longer?

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Textbook Question

NaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (b) Use the ionic radii given in Figure 7.8 to estimate the Na─Cl and K─F distances.

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Textbook Question

The substances NaF and CaO are isoelectronic (have the same number of valence electrons). (a) What are the charges on each of the cations in each compound?

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Textbook Question

The substances NaF and CaO are isoelectronic (have the same number of valence electrons). (d) Using the lattice energies in Table 8.1, predict the lattice energy of ScN.

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Textbook Question

(a) Does the lattice energy of an ionic solid increase or decrease (i) as the charges of the ions increase, (ii) as the sizes of the ions increase?

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Textbook Question

Consider the ionic compounds KF, NaCl, NaBr, and LiCl. (a) Use ionic radii (Figure 7.8) to estimate the cation–anion distance for each compound.

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