Question

In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. lattice energy1 = absolute value of the lattice energy Greatest lattice energy! (strongest bonds) Least lattice energy (weakest bonds) Li, s K,5 Rbs , Nas Ces

Answer 1

The size of ions affects the lattice energy in an ionic compound. Smaller ions have stronger ionic bonds and higher lattice energies.

Step-by-step explanation:

The lattice energy of an ionic compound is influenced by the size of the ions involved. Generally, smaller ions have stronger ionic bonds, which result in higher lattice energies. In the given list of compounds, we can compare the lattice energies based on the sizes of the ions.

K(+) has the smallest ion size, so it is expected to have the highest lattice energy.

Li(+) has the next smallest ion size, so it would have the second highest lattice energy.

Rb(+) is larger than K(+), so it would have a lower lattice energy compared to K(+).

Na(+) is larger than Li(+), so it would have a lower lattice energy compared to Li(+).

Cs(+) is the largest ion, so it would have the lowest lattice energy among all the ions listed.