1. Review of Ionic and Molecular Formula Writing:

2. Chapter 8 Outline 8.1 – Chemical Equations The symbols and formulas used to represent reactants and products

3. Reading and Writing Chemical Equations: 1.Represent the Facts 2.Use correct formulas for compounds -Ionic – SWAPPING -Molecular – PREFIXES -Diatomics – AUTOMATICALLY get a subscript “2”

4. Diatomics: Silly Phrase: Hairy Ninjas Often Fight Clean Bright Italians

5. Reading and Writing Chemical Equations: Metals are the symbol only: Magnesium metal = Mg Copper metal = Cu **No numbers or charges!!*

6. Reading and Writing Chemical Equations: 3.Law of Conservation of Mass: Nature balances the reactions, so we must too! We will use COEFFICIENTS which match what nature does.

7. Types of Equations Word Equation -Shows reactants and products in WORDS -For now these will be given to you Example: Methane Gas + Oxygen Gas -> Carbon dioxide + Water

8. Types of Equations Formula Equation -Uses Formulas Example: CH 4 + O 2 -> CO 2 + H 2 O

9. Types of Equations Balanced Equation -Number of each atom on the left matches the number on the right -THIS IS WHAT NATURE DOES! Example: CH 4 + 2O 2 -> CO 2 + 2H 2 O

10. Other Symbols s=solid l=liquid g=gas aq=aqueous=dissolved in water Reversible Reaction Add Heat

11. Significance of an Equation -Will give us information about the amounts of reactants and products -That’s Chapter 9! Reversible Reactions – Can proceed in either direction.

12. Balancing Reactions Most can be done by inspection STEPS 1.Write the WORD EQUATION (for now given) Ex. Water -> Hydrogen Gas + Oxygen Gas (this is called the Electrolysis of Water) 2. Replace words with formulas

13. Water -> Hydrogen Gas + Oxygen Gas H2OH2O->H2H2 + O2O2

14. 3.Balancing -Balance one atom at a time -Start with elements that are on each side one time only -Balance polyatomics (like NO 3 ) as an entire group when possible -Balance O and H last

15. Water -> Hydrogen Gas + Oxygen Gas H2OH2O O2O2 -> + H2H2 H O Count atoms to check!

16. Electrolysis of Water

17. Practice Problems

18. More Practice Problems

20. 8.2 – Types of Reactions 1.Synthesis -Combining 2 or more reactants to form one product A + X -> AX Example: Magnesium + Oxygen Gas -> Magnesium oxide

21. 8.2 – Types of Reactions 2.Decomposition -Breaking down 1 reactant into 2 or more products AX -> A + X Example: Hydrogen peroxide -> Water + Oxygen gas

22. 8.2 – Types of Reactions 3. Single Displacement -One element replacing another in a compound A + BX -> B + AX -A replaces the one it is most similar to! Example: aluminum + iron (III) oxide -> iron + aluminum oxide

23. Single Displacement Honors must be able to predict products. Examples: 1.copper (II) nitrate + zinc -> 2.Sodium chloride + fluorine gas ->

24. 8.2 – Types of Reactions 4. Double Displacement -Two elements switch places in compounds AX + BY -> AY + BX Example: Sodium chloride+Silver(I) nitrate->Sodium nitrate+Silver(I) chloride 4 Types of Reactions Review: (Stop after Dbl Disp)

25. 8.2 – Types of Reactions 4. Double Displacement -You must be able to predict products for this type of reaction! Example: Iron (II) sulfide + Hydrogen chloride ->

26. Activity Series Activity = Ability to react Activity Series = List of elements by activity High on the list means the element can replace those below it Helps us determine whether a reaction will or will not happen

27. Activity Series Li K Ca Na Mg Al Zn Fe Co Ni Sn Pb Cu Hg Ag Most active on this list Least active on this list

28. Activity Series Li K Ca Na Mg Al Zn Cr Fe Co Ni Sn Pb Cu Hg Ag For a single displacement reaction to occur, the SINGLE REACTANT must be HIGHER than the one in the compound Example: 2Al + 3ZnCl 2 -> 3Zn + 2AlCl 3 Example: Co + 2NaCl -> CoCl 2 + 2Na

29. Solubility Solubility = Ability to dissolve Soluble = Dissolves In Water = Aqueous – aq Insoluble = Does NOT Dissolve Solid = s = precipitate

30. Solubility Solubility Rules (these will be given to you on test): –Group 1 and Ammonium compounds ARE soluble –Acetate, Nitrate, and chlorate compounds ARE soluble –Group 17 (other than F) ARE soluble EXCEPT when with Ag, Hg2+2, and Pb –Sulfates ARE soluble EXCEPT when with Ba, Sr, Pb, Ca, Ag, Hg2+2 –Carbonates, Hydroxides, Oxides, Sulfides, Phosphates, Oxalates are INSOLUBLE **Start at the top and work down. STOP when you hit the first rule that applies to ANY PART of you compound**

31. Solubility Examples: Cu(NO 3 ) 2 = Silver nitrate + sodium chloride ->