1. Naming Ionic Compounds & Ions

2. Names  Why do we name ionic compounds & ions?  Universal names  Everyone on the same page

3. Ions  Oxidation # is the charge of the ion  2 types of ions…  Monoatomic Ion  Ion formed from a single atom  Na +, Cl -  Polyatomic Ion  Ion formed from a group of atoms  NH 4 +, CH 3 COO -

4. How do we name Ions?  Different for cations and anions 1.Cations (a.k.a.Positive Ions)  Name of atom followed by ion.  K + = Potassium Ion  Na + = Sodium Ion  Ca 2+ = calcium Ion 2.Anions (a.k.a. Negative Ions)  Drop the suffix and add “-ide” followed by ion  F - = Fluoride Ion  O 2- = Oxide Ion

5. Putting them together in an ionic compound…  Cation listed first, followed by the appropriately named anion.  NaCl = “Sodium chloride”  K 2 O = “Potassium oxide”

6. Compounds  Binary Compound  Compound made of 2 different elements ionically bonded.  Total electrical charge is neutral  +’s & -’s cancel each other

7. Chemical Formulas  Group of chemical symbols, superscripted and subscripted numbers  How do we write these???  Write the elements and their oxidation numbers as superscripts  Use subscripts to balance charges Mg 2+ Br -- + Mg 2 Br (1) Al 3+ O 2- + Al 3 O 2 Magnesium Bromide Aluminum Oxide

8. Comparing Molecules Molar Mass and Avogadro’s Number

9. Atomic Mass WWWWhat unit of measurement do we use????? AAAAtomic Mass Units: AMU CCCCompares quantities of mass to small to see. 1111 amu = 0.00000000000000000000000166g 1111.66 x 10-24g

10. Molar Mass  Finding mass of molecules?  Use atomic mass  Count atoms and add masses  C 6 H 12 O 6 (this is our trusty glucose molecule) CCCCCC CCCCCCHHHHHHHHHHHHOOOOOO

11. Finding Molar Mass  C 6 H 12 O 6  N 2 O 4 180.18 amu’s 92.02 amu’s 12.01 1.01 16 14.01 16

12. QUESTION!  Now that we can find the relative mass of a molecule, can we find the number of molecules in a certain amount of a substance?

13. Measurements  How many molecules are in 180.18g of C 6 H 12 O 6 ?  A mole  What is a mole?  Term to describe a certain number of items.

14. MOLE AAAAvogadro’s Number 666602,000,000,000,000,000,000,000 6666.02 x 1023

15. Comparison Nampa Population 71,282 Idaho Population 1,293,593 U.S. Population 292,731,592 World population 6,252,380,471 Mole 602,000,000,000,000,000,000,000

16. Moles and AMU’s  Molar Mass of C 6 H 12 O 6 = 180.18 amu  180.18g of C 6 H 12 O 6 has 6.02 x 10 23 molecules  #AMU’s  #Grams  1 Mole

17. Practice 10 lbs each 100 lbs each 20 lbs total 200 lbs total 2 cats Couple 110 lbs total 10 + 100

18. 7 amu 10 amu 8 amu 6 amu 4 amu 10 amu25 amu

19. 10 amu 25 amu 6.02 x 10 23 = 10 grams = 25 grams

20. Practice  CO 2  C 6 H 12 O 6  H 2 O  CH 4   44 AMU   180 AMU   18 AMU   16 AMU Determine the atomic mass of the following molecules. Determine the atomic mass of the following molecules.

21. Activity: Formulas Lab  Use the sheet on page 8 of your packet  Get a sheet of ion tiles  Color the cations (+ ions) one color, color the anions (- ions) another color  Cut out the tiles  Combine them in ratios that match up the number of +’s and –’s  Write as many formulas as possible

22. Activity: Formulas Lab  Example:  Aluminum has a 3+ charge  You can combine it with 3 Chloride ions to form AlCl 3  or you can use a single Phosphate ion (PO 4 3- ) and make AlPO 4  Do this as many times as you can until you fill your lab sheet. There are about 60 combinations so go wild and see how many you can make.

23. Activity 1. A package has 60 eggs, how many dozen eggs are there? 2. A carton of 6 eggs is how many dozen? 3. How many molecules are in 18.02g of H 2 O? 4. How many molecules are in 216g of O 2 ? 5. How many molecules are in 19.48kg of NaCl? 6. If an amount of material contained 9.03 x 10 23 molecules, how many moles would that be?