1. Ch. 6 Bonding 6.3 Ionic Bonding

2. Ionic Compounds ionic bonds do NOT form molecules chemical formulas for ionic compounds represent the simplest ratio of ion types made of anions and cations

3. Ionic Compounds combined so that positive charges balance negative charges crystalline solid formula of ionic compound depends of the charges of the ions combined

4. Binary Ionic Compounds Because positive charges must balance negative charges, use criss-cross method to make formulas. Write the formula for aluminum oxide.

5. Binary Ionic Compounds If you don’t like criss-cross, use algebra. Write the formula for barium sulfide.

6. Formation attractive forces: – oppositely charged ions (main attraction) – nuclei and electron clouds of adjacent ions repulsive forces: – like-charged ions (main repulsion) – electrons of adjacent ions

7. Formation distance between the ions creates a balance between those forces ions minimize their PE by combining in an orderly arrangement called a crystal lattice

8. Formation Specific lattice pattern created depends on: charges of ions – determines number of electrons transferred – determines the ratio of ions size of ions – larger ions need more space

9. Lattice Energy energy released when separate gaseous ions bond to form ionic solid or the energy absorbed to break the bonds between ions the larger the amount of energy, the stronger the bond more electrons transferred or smaller ions leads to a larger lattice energyNaCl-787.5NaBr-751.4 CaF 2 -2634.7 CaO-3385 LiCl-861.3 MgO-3760 KCl-715

10. In each of the following pairs of compounds, identify the one with the higher lattice energy KCl, CaS LiF, NaCl Fe 2 O 3, MnO 2 CaO, CaCl 2