In general, the higher the charge on the ions in an ionic compound, the more favorable is the lattice energy. Why do some stable ionic compounds have + 1 charged ions even though + 4, + 5, and + 6 charged ions would have a more favorable lattice energy?

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Chemistry

Trey

5 November, 10:27

In general, the higher the charge on the ions in an ionic compound, the more favorable is the lattice energy. Why do some stable ionic compounds have + 1 charged ions even though + 4, + 5, and + 6 charged ions would have a more favorable lattice energy?

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Answers (1)

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Leia Davies · Answer 1

The main reason why some stable ionic compounds have + 1 charged ions, even though other higher would have a more favorable lattice energy is because;

1. Energy is required to remove each of the electrons in an atom, and the more more the electrons are removed, the smaller the atom radius becomes, with increasing nuclear attraction between the opposite charges.

Note, it is a bit easy to remove a single electron, when compared to 4, 5 or 6 electrons. hence, the reason why Ionic compounds are more stable with + charged ions than others.

2. The stability of an ionic compound is dependent on his lattice energy. And the ions with large charge will have a greater attraction between the cations and anions, hence have higher lattice energy. However, the distance between the ions and the nucleus of the atom plays a major role in the stability of the ion.