the table lists the lattice energies of some compounds.\n| compound | lattice energy (kj/mol) |\n|--|--|\n|…

the table lists the lattice energies of some compounds.\n| compound | lattice energy (kj/mol) |\n|--|--|\n| lif | -1,036 |\n| licl | -853 |\n| naf | -923 |\n| kf | -821 |\n| nacl | -786 |\nwhich statement about crystal lattice energy is best supported by the information in the table?\nthe lattice energy increases as cations get smaller, as shown by lif and kf.\nthe lattice energy increases as the cations get larger, as shown by lif and licl.\nthe lattice energy decreases as cations get smaller, as shown by nacl and naf.\nthe lattice energy decreases as the cations get smaller, as shown by naf and kf.

the table lists the lattice energies of some compounds.\n| compound | lattice energy (kj/mol) |\n|--|--|\n| lif | -1,036 |\n| licl | -853 |\n| naf | -923 |\n| kf | -821 |\n| nacl | -786 |\nwhich statement about crystal lattice energy is best supported by the information in the table?\nthe lattice energy increases as cations get smaller, as shown by lif and kf.\nthe lattice energy increases as the cations get larger, as shown by lif and licl.\nthe lattice energy decreases as cations get smaller, as shown by nacl and naf.\nthe lattice energy decreases as the cations get smaller, as shown by naf and kf.

Answer

Explanation:

Step1: Analyze ion - size relationship

In ionic compounds, lattice energy is related to ion - size. Smaller ions can get closer to each other, resulting in stronger electrostatic attractions and higher lattice energy.

Step2: Compare LiF and KF

Li⁺ has a smaller ionic radius than K⁺. The lattice energy of LiF (- 1036 kJ/mol) is more negative (higher in magnitude) than that of KF (- 821 kJ/mol), indicating that as cations get smaller, the lattice energy increases.

Step3: Analyze other options

  • For LiF and LiCl, the anion changes (F⁻ vs Cl⁻), not just the cation size effect.
  • For NaCl and NaF, the anion changes (Cl⁻ vs F⁻), not just the cation size effect.
  • For NaF and KF, the correct trend is that as the cation (Na⁺ is smaller than K⁺) gets smaller, the lattice energy increases, not decreases.

Answer:

The lattice energy increases as cations get smaller, as shown by LiF and KF.