1. + Ionic Compounds Write down the stuff in red

2. + Atoms vs. Molecules vs. Compounds ATOMS are the smallest particles of any element that is still that element Example: an atom of hydrogen (H) or an atom of calcium (Ca) MOLECULES are groups of 2 or more atoms Example: H 2 or O 2 or H 2 0 or HCl COMPOUNDS are groups of 2 or more atoms of different elements Example: H 2 0, HF, NH 3 or CH 4 2

3. + Forming compounds When atoms move close together, their valence electrons interact A bond will form if the electrons become more stable (become an octet) Electrons become more stable by either: Losing electrons to other atoms and becoming an CATION Gaining electrons from other atoms and becoming an ANIONARING electrons 3

4. + Types of bonding There are two main types of chemical bonding: IONIC BONDING When atoms gain or lose (transfer) electrons to other atoms Example: Na + Cl = NaCl COVALENT BONDING (We’ll get to this later) When atoms share electrons with other atoms Example: H 2 + O = H 2 0 4

5. + Ionic bonding An ionic compound contains a POSITIVE ion (usually a METAL) and a NEGATIVE ion (usually a non-metal) EX: Na + +Cl - = NaCl (positive metal) (negative non-metal)ionic compound In ionic bonding one or more electrons TRANSFERS from each atom of METAL to each atom of NON- METAL 5

6. + Example of an Ionic Compound Sodium (Na) has 1 valence electron Chlorine (Cl) has 7 valence electron Sodium loses its 1 valence electron and gives it to Chlorine Sodium has become less negative (more positive) and now has a +1 charge Chlorine has become more negative and now have a -1 charge 6

7. + NaCl Ionic Bonding A C B 7

8. + Activity Break! Girls on the left side of the classroom (near my desk) You are metals Boys on the right side of the classroom (by the maps) You are non-metals Wait further instructions! Mini marshmallows are your electrons. Metals need to find non-metals to give their electrons to in such a way that you both have full valence shells (0 marshmallows or 8)

9. + Naming Ionic Compounds Ionic compound names have 2 parts to it, one for each ion in it: The positive metal ion is always written FIRST The negative non-metal ion is always written SECOND The non-metal’s name always ends with the suffix “ide” metal non-metal + ion - ion Example: Potassium Iodide (positive metal) (negative non-metal, ending with –ide) 9

10. + Names of Ionic Non-Metals ElementIonic NameSymbol FlourineFlourideF-F- ChlorineChlorideCl - BromineBromideBr - IodineIodideI-I- OxygenOxideO 2- SulfurSulfideS 2- SeleniumSelenideSe 2- NitrogenNitrideN 3- PhosphorusPhosphideP 3- 10

11. + Practice Naming Write down the proper name of the ionic compound formed from the following ions: Magnesium +Phosphorus= Calcium +Bromine= Aluminum + Oxygen= Lithium+Nitrogen= Zinc+Sulfur= 11 Magnesium Phosphide Calcium Bromide Aluminum Oxide Lithium Nitride Zinc Sulfide

12. + Naming Ionic Compounds from Formulas If you just have the formula, how do you name it? Example: CaI 2 1. Identify and name the metal ion in the compound  Ca 2+ is the metal. Its name is calcium. Calcium 2. Identify and name the non-metal ion in the compound  I - is the non-metal. Its name is Iodine. Iodine 3. Change the name of the non-metal so it ends with “ide” Iodide 4. Write the two together to name the ionic compound Calcium Iodide 12

13. + Practice Naming from Formulas Na 3 P 1. Name the positive metal ion 2. Name the negative non-metal ion 3. Change the suffix to “ide” 4. Write out the name 5. Bam! 13 Sodium Phosphorus Phosphide Sodium Phosphide

14. + Writing Formulas for Ionic Compounds Example: Aluminum Flouride 1. Identify the POSITIVE ion and the NEGATIVE ion and list their charges  Aluminum: Al 3+  Flouride: F - 2. Figure out how many of each ion you need to balance out the charges  Al 3+ := + 3  F - : -1 -1 -1 = - 3 3. Notice how many of each ion you needed to balance the charges  1 Al 3+ ion  3 F - ions 4. Write out the formula by listing the ions. Indicate how many of each ion are there by writing the number in a subscript beside it  AlF 3 14

15. + Practice Writing Ionic Formulas Example: magnesium nitride 1. Identify each ion and list its charge 2. Figure out how many of each ion you need to balance the charges 3. Note how many of each ion you needed 4. Write out the formula and indicate how many of each ions are there with a subscripted number 5. Bam! 15 Mg 2+ N 3- Mg 2+ = +2 +2 +2 = +6 N 3- = -3 -3 =-6 3 Mg 2+ Ions 2 N 3- Ions Mg 3 N 2