1. Ch. 12.1 Notes---Ionic Bonding & Ionic Compounds Ionic Bonds Form when ___________ transfer their _____________ electrons to a _______________. The forces of attraction between the ____________ (+) and the _____________ (-) bind the compound together. How to Represent an Ionic Bond (1)Quantum Mechanics (electron configurations): Na 1s 2 2s 2 2p 6 3s 1 Cl 1s 2 2s 2 2p 6 3s 2 3p 5 metalsvalence nonmetal cation anion Na… ___ 3s ↑ Cl… ___ ___ ___ ___ 3s 3p ↓ ↑ ↑ ↑↓↓↓

2. How to Represent an Ionic Bond 2) Bohr Model

3. How to Represent an Ionic Bond 3) Electron Dot Notations: Na + Cl  [ ] [ ] Practice Problems: (1) Draw the electron dot notation for the formation of an ionic compound between sodium and oxygen. (2) Draw the electron configuration notation for the formation of an ionic compound between magnesium and fluorine. Na +1 Cl -1

5. Sodium + Chloride

6. Practice Problems: 3) a) Draw the electron dot notation for a potassium atom. b) Draw the electron dot notation for a potassium ion. (4) a) Draw the electron dot notation for a sulfur atom. b) Draw the electron dot notation for a sulfur ion. K [K +1 ] S [ S -2 ]

7. Properties of Ionic Compounds and Covalent Molecules Ionic:  _______________ of electricity when dissolved water or melted.  formed between __________ and _________________  have _________ melting points  usually ________ soluble in water form ___________________ solids Conductors metalsnonmetals high very crystalline (dissolved salt)

8. Crystalline Patterns

9. Quartz Quartz is the common mineral form of silicon dioxide (SiO2). It is the dominant mineral in most sands and sandstones.

11. Pyrite mineral form of the iron disulfide (FeS2) with a gold-like appearance, making it also known as "fool's gold"

12. Calcite Calcite is a carbonate mineral and the most stable polymorph of calcium carbonate (CaCO3). The shape is Rhombohedron.

13. Galena Galena is the natural mineral form of lead sulfide. (PbS) It is the most important lead ore mineral.

14. Gypsum Gypsum is a very soft mineral composed of calcium sulfate dihydrate, with the chemical formula CaSO4·2H2O.

16. Properties of Ionic Compounds and Covalent Molecules Molecular: ________________ of electricity always formed between two _______________ usually have ________ melting points solubility in water _______: (polar =dissolve; nonpolar = insoluble) For a compound to to conduct electricity it must have: (1) Charged Particles (_________) (2) Particles Free to Move (___________ or __________ phase) Insulators nonmetals low varies ions liquidaqueous

17. Demonstration good conductor poor conductor nonconductor Pure H 2 O great conductor

18. Ch. 6 Notes---Chemical Names & Formulas Ionic Compounds (“________”): – Name or formula starts with a _________ (or NH 4 +, ammonium). – Other quick ways to tell if the compound is ionic: formula uses parentheses Example: ________________ formula contains more than 2 elements (capital letters)‏ Example: ________________ name uses Roman numerals Example: ________________ name ends in “-ate” or “ite”. Example: _________________ salts metal Ca(OH) 2 FeCrO 4 lead(II) chloride barium sulfate

19. Valence Electrons On The Periodic Table 1 234567 8 Sucktastic! Assume 2

20. Charges On The Periodic Table +1 +2+3 +/- 4-3-2 0 Sucktastic!

21. Writing Formulas for Ionic Compounds Step 1-- use your ion sheet and find the ions and their charges. Step 2-- “Cross the charges” if they don’t balance out. Step 3-- Use parentheses around polyatomic ion “chunks”. Practice Problems: Write the formula for each ionic compound. copper(II) bromide ____________________ aluminum nitrite _________________________ barium hydrogen carbonate ___________________________ Cu +2 Br -1 = CuBr 2 …(don’t show 1’s)‏ Al +3 NO 2 -1 = Al(NO 2 ) 3 Ba +2 HCO 3 -1 = Ba(HCO 3 ) 2

22. Naming Ionic Compounds Just use your ion sheet and find the names of the ions. cation name anion name Practice Problems: Name the following ionic compounds. a) NaC 2 H 3 O 2 b) (NH 4 ) 2 CO 3 c) NaCl d) CaO sodium acetate ammonium carbonate sodium chloride calcium oxide