1. IONIC COMPOUNDS

2. STABILITY Relates to nobility Every element’s dream They’ll do what they can to look like a noble gas…pseudo-noble gas configuration Duet Rule Octet Rule Potential Energy

3. Bond Energy The energy required to break a bond The energy is absorbed when the bond is broken, thus…released when formed Stronger bonds are more stable –Require more energy to break them –i.e. ionic bonds Weaker bonds are less stable –Require less energy to break them –i.e. molecular or covalent bonds

4. Achieving Stability Ionic bonds made by transferring electrons Metals will do what? Nonmetals will do what? Once electrons are transferred, the atoms are converted to ions. lose electron(s) gain electron(s)

5. Ions Positively charged ions are called? Negatively charged ions are called? Bond to make an ionic compound or salt cations anions

6. Salts Made of metals and nonmetals or polyatomic ions Solid –Ordered arrangement called crystal lattice Brittle High melting point Electrical conductors in aqueous and molten phases

7. More About Ions Written as a symbol with superscript to the right indicating the charge Charge is written as a number followed by a + or – sign Monatomic ions—”one-atomed” ions Polyatomic ions—”many-atomed” ions

8. Monatomic Ions Use periodic table to determine charges of representative elementsperiodic table Group 1…1+…element name + ion Group 2…2+…element name + ion Group 13…3+…element name + ion Group 14…skip Group 15…3-…ide ending + ion Group 16…2-…ide ending + ion Group 17…1-…ide ending + ion

9. Monatomic Ions For the transition metals, you must memorize the possible charges of the common ions Cr 2+ Chromium (II) ionChromous ion Cr 3+ Chromium (III) ionChromic ion Mn 2+ Manganese (II) ionManganous ion Mn 3+ Manganese (III) ionManganic ion Fe 2+ Iron (II) ionFerrous ion Fe 3+ Iron (III) ionFerric ion

10. Monatomic Ions Co 2+ Cobalt (II) ionCobaltous ion Co 3+ Cobalt (III) ionCobaltic ion Ni 2+ Nickel (II) ionNickelous ion Ni 3+ Nickel (III) ionNickelic ion Cu 1+ Copper (I) ionCuprous ion Cu 2+ Copper (II) ionCupric ion Hg 2 2+ Mercury (I) ionMercurous ion Hg 2+ Mercury (II) ionMercuric ion

11. Monatomic Ions Sn 2+ Tin (II) ionStannous ion Sn 4+ Tin (IV) ionStannic ion Pb 2+ Lead (II) ionPlumbous ion Pb 4+ Lead (IV) ionPlumbic ion Ag 1+ Silver ion Zn 2+ Zinc ion Cd 2+ Cadmium ion

12. Polyatomic Ions Refer to handout Know the formula (that means elements, subscripts, and charge) of each listed

13. Making Ionic Compounds A cation and an anion will bond in order to bring the charge of the compound to zero. A “criss-cross” method is used to determine the number of each ion necessary to balance the charges Always reduce subscripts.

14. Making Ionic Compounds Na 1+ Cl 1- 11 = NaCl = MgCl 2 = AlCl 3 Mg 2+ Cl 1- 12 Al 3+ Cl 1- 13

15. Making Ionic Compounds NaCl MgCl 2 AlCl 3 sodium chloride magnesium chloride aluminum chloride

16. Making Ionic Compounds Na 1+ S 2- 21 = Na 2 S = MgO = Ca 3 P 2 Mg 2+ O 2- 22 Ca 2+ P 3- 32

17. Making Ionic Compounds Na 2 S MgO Ca 3 P 2 sodium sulfide magnesium oxide calcium phosphide

18. Making Ionic Compounds Pb 4+ O 2- 24 = PbO 2 = AgI = Fe 2 O 3 Ag 1+ I 1- 11 Fe 3+ O 2- 23

19. Making Ionic Compounds PbO 2 AgI Fe 2 O 3 iron (III) oxide or ferric oxide silver iodide Lead (IV) oxide or plumbic oxide

20. Making Ionic Compounds Pb 4+ (OH) 1- 14 = Pb(OH) 4 = MgSO 4 = Al 2 (C 2 O 4 ) 3 Mg 2+ (SO 4 ) 2- 22 Al 3+ (C 2 O 4 ) 2- 23

21. Making Ionic Compounds Pb(OH) 4 MgSO 4 Al 2 (C 2 O 4 ) 3 lead (IV) hydroxide or plumbic hydroxide magnesium sulfate aluminum oxalate

22. Crystal Lattice 3-dimensional arrangement of atoms or ions in a solid Simplest part is called a unit cell There are six types of crystal systems –We will focus on the cubic unit cell

23. Cubic Unit Cells Three types: –Simple –Body-centered –Face-centered

24. Simple Cubic Unit Cell P

25. Face-centered Cubic Unit Cell NaCl Cl - ions Na + ions

26. Body-centered Cubic Unit Cell CsCl Cs + ion Cl - ion

27. Now… PRACTICE