Lattice Energy
Chemistry ⇒ Chemical Bonding and Structure
Lattice Energy starts at 11 and continues till grade 12.
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Arrange the following compounds in order of increasing lattice energy: NaCl, KCl, MgO.
Calculate the lattice energy of an ionic compound if the enthalpy of formation is −800 kJ/mol, the ionization energy is +500 kJ/mol, the electron affinity is −300 kJ/mol, and the sublimation energy is +200 kJ/mol. (Assume all other steps sum to zero.)
Calculate the lattice energy of NaCl if the energy required to form Na+(g) is +496 kJ/mol, the energy to form Cl−(g) is −349 kJ/mol, and the enthalpy of formation of NaCl(s) is −411 kJ/mol. (Assume all other steps sum to zero for simplicity.)
Describe how the lattice energy of an ionic compound can be estimated using the Born-Haber cycle.
Describe the Born-Haber cycle and its use in determining lattice energy.
Describe the effect of lattice energy on the solubility of ionic compounds in water.
Explain how the size of ions affects the lattice energy of an ionic compound.
Explain why lattice energy is considered an exothermic process when forming an ionic solid from gaseous ions.
Explain why lattice energy is higher for ionic compounds with small, highly charged ions.
Explain why the lattice energy of Na2O is higher than that of NaCl.
If the ionic radii of both cation and anion increase, what happens to the lattice energy?
State the relationship between lattice energy and the melting point of an ionic solid.
The lattice energy of MgO is much higher than that of NaCl. Give a reason for this observation.
