5.3.1 Lattice enthalpy

• Lattice enthalpy is the energy released when 1 mole of an ionic compound is formed from its constituent gaseous ions
• Lattice enthalpy is a key factor in determining the stability of ionic compounds

  True
• Arrange the components of the Born-Haber cycle in their correct order:

  1️⃣ Enthalpy of formation

  2️⃣ Atomization enthalpy

  3️⃣ Ionization energy

  4️⃣ Electron affinity

  5️⃣ Lattice enthalpy
• Discrepancies between experimental and theoretical lattice enthalpy values indicate partial covalent character

  True
• What is lattice enthalpy defined as?

  Energy released forming ionic compound
• The Born-Haber cycle is a thermochemical cycle used to relate lattice enthalpy to other energy changes
• What is atomization enthalpy?

  Gaseous atoms from 1 mol
• The Born-Haber cycle is based on Hess's law
• How is lattice enthalpy determined experimentally in the Born-Haber cycle?

  By summing enthalpy changes
• Lattice enthalpy is the energy released when 1 mole of an ionic compound is formed from its constituent gaseous ions
• Applying Hess's law to the Born-Haber cycle allows for the determination of lattice enthalpy


  True
• Steps involved in the Born-Haber cycle

  1️⃣ Atomization enthalpy

  2️⃣ Ionization energy

  3️⃣ Electron affinity

  4️⃣ Lattice enthalpy
• What is ionization energy?

  Energy required to remove electron
• Lattice enthalpy can be determined experimentally using the Born-Haber cycle


  True
• Match the method with its description:

  Experimental (Born-Haber cycle) ↔️ Lattice enthalpy determined by summing enthalpy changes

  Theoretical (Coulomb's law) ↔️ Lattice enthalpy estimated using ionic properties
• Lattice enthalpy represents the strength of ionic bonds in a crystal lattice

  True
• What is enthalpy of formation?

  Energy change forming 1 mol compound
• What is the symbol for lattice enthalpy?

  $\Delta H_{lattice}$
• Lattice enthalpy is the energy released when gaseous ions form an ionic lattice.


  True
• The enthalpy of formation refers to the energy change when 1 mole of a compound is formed from its elements under standard conditions.


  True
• Atomization enthalpy is the energy required to convert 1 mole of a solid element into gaseous atoms
• Steps in the Born-Haber cycle for the formation of NaCl

  1️⃣ Atomization of Na and Cl

  2️⃣ Ionization of Na

  3️⃣ Electron affinity of Cl

  4️⃣ Formation of the NaCl lattice
• The Born-Haber cycle helps to determine or verify the values of lattice enthalpy.
• Ionization energy is the energy required to remove an electron from a gaseous atom.


  True
• Ionization energy is the energy required to remove an electron from a gaseous atom
• The electron affinity is always a negative value.

  False
• The Born-Haber cycle can be used to determine lattice enthalpy experimentally.

  True
• Experimental lattice enthalpies can differ from theoretical values due to partial covalent character in the compound.


  True
• Steps in the Born-Haber cycle for measuring lattice enthalpy

  1️⃣ Atomization enthalpy

  2️⃣ Ionization energy

  3️⃣ Electron affinity

  4️⃣ Formation of ionic lattice
• Discrepancies between experimental and theoretical lattice enthalpies indicate deviations from ideal ionic bonding.

  True
• What does 'e' represent in the context of lattice enthalpy calculations?

  Elementary charge
• \(r\) is the distance between ions
• The Born-Haber cycle is used to measure lattice enthalpy.

  True
• What law is applied to the Born-Haber cycle to determine lattice enthalpy experimentally?

  Hess's law
• Match the method with its description:

  Born-Haber Cycle ↔️ Experimentally determines lattice enthalpy

  Coulomb's Law ↔️ Estimates lattice enthalpy theoretically
• The attractive forces between larger ions are weaker.


  True
• Larger ions have lower lattice enthalpies
• Why does a higher charge on ions increase lattice enthalpy?

  Stronger electrostatic attraction
• Match the ionic charge with its effect on lattice enthalpy:

  Low (e.g., Na⁺, Cl⁻) ↔️ Lower

  High (e.g., Mg²⁺, O²⁻) ↔️ Higher
• How does a higher coordination number affect lattice enthalpy?

  Increases lattice enthalpy