1. Chapter 7 Ionic Bonds

2. Ionic Bonds Video

3. Chemical Bonds force that holds two atoms together (either by sharing or transferring electrons)

4. Ionic Bonds bond composed of charged particles (formed by losing or gaining electrons) that are electrostatically held together

5. Properties of Ionic Bonds ions are held together in a crystal lattice (3D geometric arrangement of particles) solids high melting and boiling points will conduct electricity when dissolved in water Video- crystal lattice Video

6. Ions charged particle (from losing or gaining electrons) Cation:positively charged particles formed by losing electrons Anion:negatively charged particles formed by gaining electrons

7. What are cations afraid of? Dogions. Ha.Ha.Ha.Ha.Ha.

8. Monoatomic Ion = ion made of one type of atom Ex. Na + O -2 Polyatomic Ion = ion made of more than one type of atom Ex. CO 3 -2

9. Oxidation Number the charge on the atoms or group of atoms Group 1 = +1 Group 2 = +2 Group 13 = +3 Group 16 = -2 Group 17 = -1

10. Chemical Formula Combination of symbols that represent the composition of a compound (compound – chemical combination of two or more elements) -shows relative number of atoms of each element and types of elements involved. Subscript = # of atoms of that element

11. Writing ionic formulas 1. Find the oxidation numbers of both ions (chart or p. 218-221) and symbols 2. Add atoms so that the total charge adds up to zero (may have to use least common multiple)

12. 3. Combine symbols and subscripts together, cation first then anion (use parentheses around polyatomics and NO roman numerals after lead, iron, copper and tin) 4. Sodium and chlorine love story Sodium and chlorine love story

13. Sodium oxide Na= +1O = -2 You need two +1 sodium ions to add up to the –2 charge on the oxygen ion to make the compound add up to zero Na +1 O -2 Na 2 O

14. Iron (III) sulfate Fe = +3 SO 4 = -2 -Least common multiple = 6 -Need 2 iron ions, 3 sulfate ions Fe +3 SO 4 -2 Fe 2 (SO 4 ) 3

15. Aluminum sulfide Barium chloride Lead (II) nitrate Ammonium phospate Al 2 S 3 BaCl 2 Pb(NO 3 ) 2 (NH 4 ) 3 PO 4

16. Naming Ionic Compounds 1. Name the cation as it is written on the periodic table (except ammonium) 2. Add roman numeral in parentheses if lead, iron, copper or tin.

17. 3. Anion- Monoatomic –change ending to –ide (Ex. Oxygen => oxide) Polyatomic – keep ending as written. (Ex. Carbonate) 4. Common acids don’t follow these rules.

18. MgI 2 Magnesium iodide

19. SnCO 3 Tin (II) carbonate