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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Identify the elements in each compound: NaF consists of sodium (Na) and fluorine (F), while CaO consists of calcium (Ca) and oxygen (O).

Determine the common oxidation states of these elements: Na typically has a +1 charge, F typically has a -1 charge, Ca typically has a +2 charge, and O typically has a -2 charge.

Analyze the compounds to determine the charge of the anions: In NaF, F is the anion and in CaO, O is the anion.

Apply the concept of neutrality in compounds: The total charge in the compound must be zero, so the charge of the anion must balance the charge of the cation.

Conclude the charges of the anions: In NaF, the anion F has a charge of -1 to balance Na's +1. In CaO, the anion O has a charge of -2 to balance Ca's +2.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Isoelectronic Species

Isoelectronic species are atoms, ions, or molecules that have the same number of electrons and, consequently, the same electronic structure. In the case of NaF and CaO, both compounds have ions that achieve a stable electron configuration similar to noble gases, which is crucial for understanding their chemical behavior and bonding.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in chemical bonding. The number of valence electrons determines how an atom interacts with others, including the formation of ions. In NaF, sodium (Na) has one valence electron, while fluorine (F) has seven, leading to the formation of Na+ and F- ions.

Ionic Charges

Ionic charges refer to the positive or negative charge that an atom acquires when it loses or gains electrons. In NaF, sodium loses one electron to become Na+, while fluorine gains one electron to become F-. In CaO, calcium (Ca) loses two electrons to form Ca2+, and oxygen (O) gains two electrons to form O2-, resulting in the respective charges of the anions in each compound.

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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. (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?

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.

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?

Textbook Question

The substances NaF and CaO are isoelectronic (have the same number of valence electrons). (c) Without looking up lattice energies, which compound is predicted to have the larger lattice energy?

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.

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?