3. ENERGY INVOLVED IN IONIC BONDING presentation.pdf
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This document discusses the energy involved in the formation of ionic bonds in sodium chloride. It explains the steps of converting the elements to gaseous ions, forming the ionic compound, and combining the steps. It also discusses lattice energies, which is the energy required to break ionic bonds and convert the solid compound into gaseous ions. The document provides examples of using thermochemical data in a Born-Haber cycle to calculate the lattice energy of ionic compounds such as NaCl, MgF2, and Na2O.
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- 2. FORMATION OF SODIUM CHLORIDE
- 3. Formation of NaCl Na(s) NaCl (s) Na(g) Na+ (g) Cl- (g) Cl(g) Cl2 (g)
- 4. Steps Involved 1. Elements (standard state) converted into gaseous atoms 2. Losing or gaining electrons to form cations and anions 3. Combining gaseous anions and cations to form a solid ionic compound 4. Combining all the steps Let’s consider:
- 5. LATTICE ENERGIES lattice energy: energy required to break ionic bonds and sublime (always positive).
- 6. Step 1: Convert from Solid to Gas • The standard enthalpy change of atomisation is the ΔH required to produce one mole of gaseous atoms (enthalpy of Sublimation - from solid to gas)
- 7. Step 1: Convert from Solid to Gas • The standard enthalpy change of atomisation is the ΔH required to produce one mole of gaseous atoms (enthalpy of Sublimation - from solid to gas). NOTE: for diatomic gaseous elements, ΔHo at is equal to half the bond energy (enthalpy)
- 8. Becoming cations • Ionization energy • Enthalpy change for one mole of a gaseous element or cation to lose electrons to form a mole of positively charged gaseous ions
- 9. Step 2: Formation of gaseous ions • Electron Affinity • Enthalpy change when one mole of gaseous atoms or anions gains electrons to form a mole of negatively charged gaseous ions. • For most atoms = exothermic, but gaining a 2nd electron is endothermic due to the repulsion between the anion and the electron
- 10. Lattice Enthalpy • Energy required to convert one mole of the solid compound into gaseous ions. • It is highly endothermic • We cannot directly calculate ΔHo lat , but values are obtained indirectly through Hess’s law for the formation of the ionic compound • We will use the reverse of this lattice energy equation to find the lattice energy
- 11. Introduction to the Born – Haber cycle
- 12. EXAMPLES
- 13. Calculations • Calculate the lattice energy of NaCl(s) using the following: (kJmol-1 ) ΔHf° = Δ Hs°+ Δ HIE°+ Δ Ha°+ Δ Hea°- U
- 14. • Ionisation energy (first and second) • Electron affinity (first and second) • Dissociation energy • Sublimation energy • Enthalpy of formation • Lattice energy • Enthalphy of atomisation
- 15. • Calculate the enthalpy of formation of Magnesium Floride given the following information
- 18. • Calculate the lattice energy of Sodium oxide given the following information • Heat of formation of Na2O = -414 kJ/mol • Atomization energy of sodium = +107 kJ/mol • Ionization energy of sodium = + 496 kJ/mol • Atomization energy of oxygen = +498 kJ/mol • 1st electron affinity for oxygen = -141 kJ/mol • second electron affinity for oxygen = 844 kJ/mol