Which of the following alkali metal halides has the largest lat-tice energy? Explain. (a) (b) (c)

검증된 단계별 안내

Identify the alkali metals and halides involved in each option (a), (b), and (c).

Understand that lattice energy is influenced by the charge of the ions and the distance between them. The greater the charge and the smaller the ionic radii, the stronger the lattice energy.

Recall that in the periodic table, as you move down a group, the ionic radius increases. This means that for alkali metals, the ionic radius increases from Li to Cs.

Similarly, for halides, the ionic radius increases as you move down the group in the periodic table, from F to I.

Compare the alkali metals and halides in each option based on their positions in the periodic table to determine which combination has the smallest ions with the highest charges, as this will likely have the largest lattice energy.

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Lattice Energy

Lattice energy is the amount of energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. Higher lattice energy indicates stronger ionic bonds, which typically results from smaller ionic radii and higher charges on the ions.

Ionic Size and Charge

The size of the ions involved in the formation of an ionic compound significantly affects lattice energy. Smaller ions can pack more closely together, leading to stronger electrostatic attractions and higher lattice energy. Additionally, the charge of the ions plays a crucial role; ions with higher charges will produce greater lattice energy due to stronger interactions.

Trends in Alkali Metal Halides

In alkali metal halides, lattice energy trends can be analyzed based on the alkali metal and halide involved. As you move down the group of alkali metals, the ionic size increases, leading to lower lattice energies. Conversely, halides with higher electronegativity (like fluorine) tend to form compounds with higher lattice energies due to their smaller ionic size compared to other halides.