2. 1. Identify the type of reaction 2. Predict the product(s) using the reaction type as a model 3. Balance it Don’t forget the diatomic elements: ( ClIFHBrON )

3. two substances (generally elements ) combine and form a compound. A + B  AB e.g. 2H 2 + O 2  2H 2 O

4. First: Predict the product(s) Second: Write and balance the equation, using your periodic table Solid Magnesium reacts with oxygen gas Mg (s) + O 2(g)  Sodium metal reacts with chlorine gas Na (s) + Cl 2(g)  Aluminum metal reacts with fluorine gas Al (s) + F 2(g) 

5. Occur when a compound breaks up into the elements or into simpler compounds AB  A + B e.g. 2 H 2 O  2H 2 + O 2

6. e.g. carbonate and chlorate decomposition reactions do not go to elements Carbonates (CO 3 2- ) decompose to carbon dioxide + a metal oxide e.g. CaCO 3  CO 2 + CaO Chlorates (ClO 3 - ) decompose to oxygen gas + a metal chloride e.g. 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2

7. First: Predict the products Second: Write and balance the equation, using your periodic table Solid Lead (IV) oxide decomposes PbO 2(s)  Aluminum nitride decomposes AlN (s) 

8. Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2(g) + O 2(g)  BaCO 3(s)  Co (s) + S (s)  NH 3(g) + H 2 CO 3(aq)  NI 3(s)  (assume Co III) Nitrogen monoxide

9. Occur when one element replaces another in a compound A metal can replace a metal (+ ion) OR a nonmetal can replace a nonmetal (- ion). remember: - the (+) cation always goes first - when H 2 O ionizes, it forms an H + and OH - (not H+ and O -2 )

11. Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zn (s) + HCl (aq)  ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction 2

12. Sodium chloride solid reacts with fluorine gas NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) Note that fluorine replaces chlorine in the compound Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq)  2 2

13. Occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound AB + CD  AD + CB

14. Think about it like “foil”in algebra, first and last ions go together + inside ions go together e.g. AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq)

15. Predict the products. Balance the equation 1. HCl (aq) + AgNO 3(aq)  2. CaCl 2(aq) + Na 3 PO 4(aq)  3. Pb(NO 3 ) 2(aq) + BaCl 2(aq)  4. FeCl 3(aq) + NaOH (aq)  5. H 2 SO 4(aq) + NaOH (aq)  6. KOH (aq) + CuSO 4(aq) 

16. Occur when a hydrocarbon reacts with oxygen gas, also called burning

17. In general: C x H y + O 2  CO 2 + H 2 O The products in combustion are always carbon dioxide and water. (although incomplete burning produces by-products like carbon monoxide)

18. Example C 5 H 12 + O 2  CO 2 + H 2 O Write the products and balance the following combustion reaction: C 10 H 22 + O 2  5 6 8

19. State the type, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4  2. C 6 H 12 + O 2  3. Zn + CuSO 4  4. Cs + Br 2  5. FeCO 3 

20.  Once you write the molecular equation (synthesis, decomposition, etc.), check for reactants and products that are soluble or insoluble.  Usually assume the reaction is in water  Use a solubility table to determine which compounds dissolve in water.  If the compound is soluble, the compound splits into component ions  If the compound is insoluble, then it remains as a compound

22.  Gases only slightly dissolve in water  Strong acids and bases dissolve in water  Hydrochloric, Hydrobromic, Hydroiodic, Nitric, Sulfuric, Perchloric Acids  Group I hydroxides (should be on your chart anyway)  Water slightly dissolves in water! (H+ and OH-)  SrSO 4 is insoluble; BeI 2 and the products are soluble

23. Molecular Equation: K 2 CrO 4 + Pb(NO 3 ) 2  PbCrO 4 + 2 KNO 3 SolubleSolubleInsoluble Soluble Total Ionic Equation: 2 K + + CrO 4 -2 + Pb +2 + 2 NO 3 -  PbCrO 4 (s) + 2 K + + 2 NO 3 -

24.  These are the same as total ionic equations, but you should cancel out ions that appear on BOTH sides of the equation Total Ionic Equation: 2 K + + CrO 4 -2 + Pb +2 + 2 NO 3 -  PbCrO 4 (s) + 2 K + + 2 NO 3 - Net Ionic Equation: CrO 4 -2 + Pb +2  PbCrO 4 (s)

25.  Try this one! Write the molecular, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water. Molecular: Total Ionic: Net Ionic: