1. IONIC COMPOUNDS Formation of Ionic Bonds and their Properties

2. IONIC SOLIDS Exist in the solid state in a crystalline form. Commonly referred to as a salt. Lattice is a regularly repeating three-dimensional array of atoms, molecules, or ions

3. Ionic vs Molecular Compounds In a solid ionic compound, each ion is surrounded by ions of the opposite charge, but is not associated with any particular ion. There are no molecules in an ionic solid. The formula of an ionic compound refers to the formula of the formula unit, the lowest ratio of the positive and negative ions that make up the compound.

4. What are ionic compounds made of? Ionic compounds are formed as a result of the electrostatic attraction between oppositely charged ions – a cation and an anion. Monoatomic Ions e.g. Na +, Ca +2, O -2, or Cl - Polyatomic Ions e.g. NH 4 +1, MnO 4 -, SO 3 -2, or PO 4 -3 Since the number of positive charge equals the number of negative charges, the net compound is neutral.

5. LATTICE ENERGY A measure of the strength of bonds in that ionic compound Energy change or enthalpy of formation For NaCl, the final step to create NaCl (s) would be: Na + (g) + Cl − (g) → NaCl (s) This process is exothermic.

6. Why Exothermic? Coulomb's Law

7. Formation of lithium fluoride (LiF) Li (s)  Li (g) Li (g)  Li + (g) + e - ½ F 2 (g)  F (g) F (g) + e -  F - (g) Li + (g) + F - (g)  LiF (s) _______________________ Li (s) + ½ F 2 (g)  LiF (s)

8. Lattice Energy of Alkali Metals F-F- Cl - Br - I-I- Li + 1036853807757 Na + 923780747704 K+K+ 821715682649 Rb + 785689660630 Cs + 740659631604 The values are energy released when the ionic crystal is formed. The units are kJ/mol. BE ABLE TO EXPLAIN THE TREND!

9. Impact of Charge The stronger the charge on an ion the stronger the attractive force that will result in an ionic lattice. Therefore, 1 +/- ions form compounds with lower lattice enthalpies than 2 +/- ions. Moreover, the Mg +2 ion is smaller than the Na +1 ion. Compound NaCl Na 2 O MgCl 2 MgO Lattice Energy 780 2478 2526 3791 EXPLANATION? Let's Make Sodium!

10. Impact of Ionic Radius In general, the larger the ionic radius the lower the lattice enthalpy as the force of attraction between the ions is smaller and the packing of the ions is less efficient. NaCl780NaF918 KCl711NaCl780 RbCl685NaBr742 CsCl661NaI 705 EXPLANATION? Would you expect the lattice energy of CsI be relatively large or relative small?

11. CHECK FOR UNDERSTANDING For each pair, indicate which bond will have a higher lattice energy. Justify your answer a. NaCl or LiF b. MgO or SrO c. CaO or ScN 788 v 1030 kJ/mol 3795 v 3217 kJ/mol 3414 v 7547 kJ/mol

12. CHECK FOR UNDERSTANDING Two ions with charges of +2 and -2 are separated by a distance of 1.0 angstroms (0.1 nm). By what factor is the potential energy changed when those ions are moved to 4.0 angstroms away? Charles Coulomb By what factor is the potential energy changed when distance is kept constant but the charge of the ions becomes +1 and -1?

13. ELECTROLYSIS ALUMINIUM VIDEO How Is It Made? Let's Make Sodium Again!