2. Catalyst Write the Molecular, Total Ionic, and Net Ionic Reactions for the chemical reactions below: a)AgSO 4 + K 3 PO 4  a)Reacting Magnesium Sulfate and Lithium Fluoride

3. GRADE!

4. Catalyst Pick up Papers from the front Calculate the actual yield of Potassium Sulfate if you started with 15 g of Silver (II) Sulfate and excess Potassium Phosphate, which produced Potassium Sulfate at a 75% yield. Use the following equation: AgSO 4 + K 3 PO 4  Ag 3 (PO 4 ) 2 + K 2 SO 4

5. BIG GOAL

6. Explosion! (3 MINUTES)

7. Explosion Questions 1.What is the formula for density? 2.Give an example of a chemical property. 3.Give an example of a physical property. 4.What is the law of conservation of mass? 5.What is the law of definite proportions? 6.What is the law of multiple proportions? 7.Who discovered the electron? 8.What are the three types of radiation? 9.Which particle is the biggest? 10.Which is the smallest? 11.Who is Ernest Rutherford? 12.How do you find the number of neutrons? 13.What is an isotope? 14.What is the formula for Nitrite? 15.What is the formula for Perchlorate? 16.What is the formula for Hyposulfite? 17.What is the empirical formula? 18.What is the molecular formula? 19.What is the limiting reagent? 20.What is the excess reagent? 21.What is the % yield? 22.What is % composition? 23.What does it mean to be aqueous? 24.Name 3 strong acids 25.Name 3 Strong bases

8. How to Remember Solubility RULES! Always Soluble: CASH – N – GIA C: Chlorates A: Ammonium S: Sulfates – CBS/PBS H: Halogens – F: CBS-PM Cl/Br/I: HAPpy N: Nitrates GIA: Group 1A

9. How to Remember Solubility RULES! Always Soluble: kNights can take on anything Acetate : the Ace I ClBr except Silver Lead and Mercury C: Chlorates A: Ammonium S: Sulfates – CBS/PBs H: Halogens – F: CBS-PM Cl/Br/I: HAPpy N: Nitrates GI: Group 1 A: Acetates

10. Acid/Base Reactions

11. Acid/Base Reactions: form a SALT and WATER as the only products HA + BOH  BA + H 2 O Bronsted Lowry Acid Definition: Proton donor Base Definition: Proton Acceptor

12. MUST REMEMBER: STRONG electrolytes (acids and bases) dissociate completely, weak electrolytes Do NOT! ALWAYS WRITE THESE EQUATIONS IN NET IONIC REACTION FORM!

13. Example Equations: Hydrochloric Acid reacts with Sodium Hydroxide Remember: Write the NET IONIC Equation!

14. Identify the Type of Reaction below: 1) Does your reaction have oxygen as one of it's reactants and carbon dioxide and water as products? If yes, then it's a combustion reaction 2) Does your reaction have two (or more) chemicals combining to form one chemical? If yes, then it's a synthesis reaction 3) Does your reaction have one large molecule falling apart to make several small ones? If yes, then it's a decomposition reaction 4) Does your reaction have any molecules that contain only one element? If yes, then it's a single displacement reaction 5) Does your reaction have water as one of the products? If yes, then it's an acid-base reaction 6) If you haven't answered "yes" to any of the questions above, then you've got a double displacement reaction

15. Identify the Type of Reaction below: List what type the following reactions are: 1) NaOH + KNO 3 --> NaNO 3 + KOH 2) CH 4 + 2 O 2 --> CO 2 + 2 H 2 O 3) 2 Fe + 6 NaBr --> 2 FeBr 3 + 6 Na 4) CaSO 4 + Mg(OH) 2 --> Ca(OH) 2 + MgSO 4 5) NH 4 OH + HBr --> H 2 O + NH 4 Br 6) Pb + O 2 --> PbO 2 7) Na 2 CO 3 --> Na 2 O + CO 2

16. Identify the Type of Reaction below: List what type the following reactions are: 1) double displacement 2) combustion 3) single displacement 4) double displacement 5) acid-base 6) synthesis 7) decomposition

17. Acid/Base Reaction Calculations

18. Steps to perform Acid-Base Reaction Calculations or any precipitation reaction 1.List the compounds present before the reaction occurs 2.Write the balanced net ionic equation 3.Calculate the moles of reactants (may use volume and molarity) 4.Determine the limiting reactant 5.Calculate the moles of the required reactant or product 6.Convert to grams or volume as required

19. Example 1: When aqueous solutions of Na 2 SO 4 and Pb(NO 3 ) 2 are mixed. Calculate the mass of Lead (II) Sulfate formed when 1.25 L of 0.0500 M Lead (II) Nitrate and 2.00 L of 0.250 M Sodium Sulfate are mixed. Is this a precipitation or Acid/Base reaction?

20. Example 2: What volume of a 0.100 M HCl solution is needed to neutralize 25.0 mL of 0.350 M NaOH? Is this a precipitation or Acid/Base reaction?

21. Example 3: In a certain experiment, 28.0 mL of 0.250 M HNO3 and 53.0 mL of 0.320 M KOH are mixed. Calculate the amount of water formed in the resulting reation. What is the concentration of H + or OH - ions in excess after the reaction goes to completion?

22. Acid/Base Reaction Titrations

23. We use this technique for Volumetric Analysis! Buret  Titrant  Analyte  Endpoint: when the solution changes color in a titration

24. Buret  Titrant  Analyte  Endpoint: when the solution changes color Equivalence Point: point where enough titrant has been added to react exactly with the amount of analyte (no limiting reagent)

25. Practice Problems

26. Redox Reactions (aka Oxidation Reduction Reactions)

27. Oxidation-Reduction Reactions/Redox Reactions – when one or more electrons are transferred Oxidation States/Oxidation numbers - Table 4.2 Rules of Assigning oxidation states… ** the sum of the oxidation states must add to the original ion charge

28. Oxidation State Assignments:

29. Practice Assigning Oxidation States:

30. If an element is oxidized…it LOST electrons Oxidation involves an increase in oxidation state If an element is reduced…it GAINED electrons Reduction involves a decrease in oxidation state

31. In other words… Oxidizing agent means the Reduction means to GAIN electrons LEO the lion goes…GER OR OIL RIG (Oxidation is loss/Reduction is gain)

32. Oxidizing Agent – A compound that accepts electrons Reducing Agent – A compound that donates electrons whereas… An ELEMENT (within that compound) can be oxidized or reduced!

33. Balancing Redox Reactions!