1. + Ionic Nomenclature Chemistry 1

2. + Exam Analysis Averages Chemical Bonding (%) Periodic Trends (%) Electrons (%)

3. + The Language of Chemistry Subscripts indicate the number of atoms of an element in a molecule. C 8 H 18 or MgCl 2 How many atoms of each element are in the following? CH 4 SO 2 O 2 P 4 O 10 Pb(NO 3 ) 2

4. + Review What is a cation? What is an anion? What group of elements typically form +1 cations? Why? What group of elements typically form +2 cations? Why? What group of elements typically form -1 anions? Why? What group of elements typically form -2 anions? Why?

5. + Ions and Compounds Monatomic ions (N 3- ) Ions formed from a single atom Polyatomic ions (SO 4 2- ) Ions formed from more than one atom See hand-out (purple) Binary Compounds Made of two elements Ternary Compounds Made of three or more elements (contains polyatomic ion) **When writing chemical formulas for ionic compounds, the overall charge of the compound must be ZERO/NEUTRAL!**

6. + Formula of Ionic Compounds 1) List the cation (positively charged ion) chemical symbol first. 2) List the anion (negatively charged ion) chemical symbol after the cation. 3) If the charges are not the same (sum of the oxidation numbers must equal zero), subscripts must be added to indicate a ratio of positive and negative ions. -The polyatomic ion acts as an individual ion. -Because polyatomic ions act as a unit, NEVER CHANGE SUBSCRIPTS OF ANY ATOM WITHIN THE ION. -Transition metals with more than one oxidation number… the charge is noted using roman numerals!

7. + Let’s Practice Writing Formulas Q: What is the chemical formula for aluminum fluoride? 1. Symbol for aluminum ion = Al 3+ Symbol for fluoride ion = F - 2. Al 3+ F - 3. Least common multiple is. 4. AlF 3 5. Orbital Notation Verification

8. + Practice Writing Formulas Write the correct formula for the following ionic compounds. 1) Potassium and Iodide 2) Magnesium and Chloride 3) Aluminum and Bromide 4) Cesium and Nitride 5) Barium and Sulfide

9. + Practice Writing Formulas With Polyatomic Ions 1) Sodium and Nitrate 2) Calcium and Chlorate 3) Aluminum and Carbonate 4) Potassium and Chromate 5) Magnesium and Carbonate

10. + Naming Ionic Compounds List the name of the cation (watch for transition metals). List the name of the anion, changing the ending to “ide” If you have a polyatomic anion, just list its name after the cation. CaCl 2 = calcium chloride Na 2 S = sodium sulfide

11. + Naming Ionic Compounds With A Transition Metal Work backwards to determine the charge on the transition metal…. Cr 2 O 3 FeONiCl 2 Mn 3 (PO 4 ) 2 Rules To Name Compound: 1. Name the cation 2. Place the charge of the transition metal as a roman numeral 3. Name the anion by changing the ending to “ide”

12. + Review – Binary Compounds Write the correct chemical formula for each of the following compounds. potassium bromide magnesium selenide sodium phosphide tin(IV) chloride aluminum oxide scandium(III) sulfide Give the correct names for each of the following compounds listed below. KF SnI 4 SiF 4 AlBr 3 FeCl 3 ZnO

13. + Review Ternary Compounds Write the chemical formulas for the following names: Iron (III) acetate Gold(III) sulfate Ammonium phosphate Calcium nitrate Write the chemical names for the following chemical formulas: FeC 2 O 4 Pb(CO 3 ) 2 Al(MnO 4 ) 3 Ba(OH) 2

14. + For next time… Complete Unit Packet Part 2 (Part 1 should be completed at this time). Read pages 232-244 (Ch. 7 sections 2 and 3)

15. + Entrance Ticket Write the formula for the following compounds. Hint-look up the charges for each element/ion and then balance the charges Calcium Nitride Rubidium Sulfide Lead (II) Nitrate Iron (III) Oxide Manganese (III) Chlorate Write the name for the following compounds. Cr 3 P 2 Al 2 (SO 4 ) 3 BaO CoN Cu 3 (PO 4 ) 2

16. + Molecular Compounds Nomenclature (Covalent) When naming compounds consisting of two nonmetals, the names of the elements are written in the same order as they appear in the formula. (The more metallic element is written first.) The second element uses the suffix “-ide”. Prefixes are added to the name of each element to indicate the NUMBER of atoms of the element in the molecule. (If the first element’s prefix is mono-, it will be dropped. For example, monocarbon dioxide (CO 2 ) is simply called carbon dioxide.) **Note: the “o” or “a” at the end of a prefix is usually dropped when the word following the prefix begins with another vowel…e.g. monoxide or pentoxide.

17. + Prefixes –Polyatomic Handout PrefixNumber of atoms Mono-1 Di-2 Tri-3 Tetra-4 Penta-5 Hexa-6 Hepta-7 Octa-8 Nona-9 Deca-10

18. + For the following molecular compounds, write the molecular formula: Carbon mononitride Sulfur tribromide Phosphorus triflouride Nitrogen dioxide Carbon tetrachloride Dihydrogen monoxide Sulfur trioxide Dinitrogen hexoxide

19. + For the following molecular formulas, write the compound name: SiO 2 CO 2 SeF 6 N 2 O 5 As 2 O 5 AsI 3 PCl 5 CF 4

20. + Flow Chart Challenge Create a flow chart to use while NAMING Ionic and Covalent Compounds Hints: How do you distinguish between an Ionic and Covalent Compound? Which one uses prefixes? When do you use Roman Numerals in the name? What do you do for naming polyatomic ions?

21. + Individual Practice Unit Packet Part 3 (Omit Acid Naming)