2. *Learn Organic Nomenclature Rules *Any compounds that produce ions in solution, should have those written in ionic form WRITE NET IONIC EQUATIONS! *All reactions on AP EXAM DO occur. There are NO no reactions! *Need to balance equations *No requirement to use state symbols *Don’t expect to know all the equations *Can get partial credit; 1 pt. for reactants and two possible for products Have THREE, net ionic equations from sentences and answer a question about the reaction.

3. First step Categorize the equation: 1.Double replacement (Metathesis) 2.Simple Redox 3.Non-simple Redox 4.Hydrolysis 5.Complex Ion Formation 6.Organic

4. 1. Double replacement (Metathesis) Where two ions are substituted….. Usually involve acids, bases and salts.

5. Acids Have H written first and donate ONE H + Organic acids have the H+ written in the COOH group: CH 3 COOH Organic acids are weak! KNOW the strong acids: HCl, HBr, HI and acids where the number of oxygen’s present exceeds the number of hydrogen’s by two or more: HNO 3 H 2 SO 4

6. Acids Strong acids loose only one Hydrogen; H 2 SO 4  H + + HSO 4 - Carbonic acid, H 2 CO 3, is weak and prefers CO 2 + H 2 O. If represented as an acid (on the left side of equation) then: H 2 CO 3  H + + HCO 3 - Sulfurous acid, H 2 SO 3, is written as H 2 SO 3  H + + HSO 3 - (if a reactant) NOT dissociated if written as a product!

7. Bases Formula ends in OH, except Ammonia and organic bases that contain Nitrogen. (has a lone pair of electrons that can be donated) Organic alcohols are NOT bases. KNOW the strong bases: Group I & II hydroxides and ammonium hydroxide. BUT ammonium hydroxide prefers: NH 4 OH  NH 3 + H 2 O

8. Salts Salt is a compound where the hydrogen ion in an acid have been replaced by metal or ammonium ions. KNOW the solubility rules for salts! If they use the term EQUIMOLAR, that means: reactants react in a 1:1 ratio some of the ionizable Hydrogen’s in an acid are being replaced Slightly soluble salts may be written in dissociated or undissociated form

9. Examples of Double Replacement: Solutions of sodium phosphate and calcium Chloride are mixed. 3Ca +2 + 2 PO 4 -3  Ca 3 (PO 4 ) 2 A dilute solution of lithium hydroxide is mixed with dilute hydrobromic acid. H + + OH -  H 2 O Hydrogen sulfide gas is bubbled through a solution of silver nitrate. H 2 S + 2Ag +  2H + + Ag 2 S

10. 2. Simple Redox A reaction where electrons are transferred from one species to another. Single displacement, Combustion, Combination and Decomposition

11. Single Displacement: Halogen displacement, Hydrogen displacement, One metal replacing another in solution. Combustion: organic compounds forming CO 2 & H 2 O, metals burning in air Combination: element & element, non-metal oxide & water(acid), metal oxide & water (base), metal oxide & non-metal oxide (salt)

12. a. Magnesium metal is added to a solution of Iron (III) Chloride. Mg + 2Fe +3  2Fe +2 + Mg +2 Hint: Know that Mg will oxidize Know that Fe +3 goes to Fe +2 Know that Cl - is a spectator ion Question: What color change may be observed? Fe +3 is yellow/brown and Fe +2 is pale green

13. b. Solid magnesium carbonate is heated MgCO 3  MgO + CO 2 Hint: Know that when CO 3 -2 is heated CO 2 gas is made Question: How might one test for the gas produced in this reaction? CO 2 will turn a solution of lime water ‘milky’ Ca(OH) 2

14. 3. Non-Simple Redox A reaction involving the transfer of electrons. In these reactions an oxidizing agent will cause the oxidation of another compound and in the process, itself will be reduced.

15. a. Potassium Manganate(VII) is added to a solution containing acid and bromide ions. 2MnO 4 - + 10Br - + 16 H +  5 Br 2 + 2Mn +2 + 8 H 2 O Hints: If it says it contains acid, add H + Learn the common oxidizing and reducing agents Question: What is the oxidation number of Mn before and after the reaction?

16. b. Aqueous potassium dichromate is added to a solution containing tin(II) nitrate. Cr 2 O 7 -2 + 3Sn +2 + 14H +  3Sn +4 + 2Cr +3 + 7 H 2 O Hints: write the two half-reactions here and balance. That’s where the H + and H 2 O came from. Cr 2 O 7 -2  Cr +3 Sn +2  Sn +4 Question: Which substance is being oxidized in the reaction? Explain.

17. c. Concentrated Hydrochloric acid is added to solid manganese (IV) Oxide. 4H + + 2Cl - + MnO 2  Mn +2 + Cl 2 + 2H 2 O Hints: Know what MnO 2 turns into. Write the acid as separate ions Know that Cl - on one side will oxidize to Cl 2 Question: Which species in the equation is the reducing agent ?

18. 4. Hydrolysis A reaction with water. Examples: Anion of a weak acid + water  Weak acid and OH - Cation of a weak base + water  Weak base + OH - Non-metal Halide + H 2 O  H + + element + combination PCl 3 + 3H 2 O  3H + + 3Cl - + H 3 PO 3 PCl 5 + 4 H 2 O  5H + + 5Cl - + H 3 PO 4

19. a. Solid lithium hydride is added to water LiH + H 2 O  Li + + OH - + H 2 Question: Describe a test for the gas produced in this reaction. b. Phophorous tribromide is added to water PBr 3 + 3H 2 O  3H + + 3Br - + H 3 PO 3 Question: What would be the expected shape of a phosphorous tribromide molecule? Trigonal pyramidal

20. 5. Transition Metal Chemistry A reaction involving a transition metal ion in aqueous solution either undergoing ligand exchange (often with ammonia or hydroxide) or the destruction of complexes with acids. Hints: Aluminum and zinc act like transition metal ions and form complexes Excess often appears in these questions Know complexes and how to name them Most first row transition metal complexes exist in solution as hexaaqua ions. (6 waters)

21. a. A solution of ammonium thiocyanate is added to a solution of iron(III) chloride. [Fe(H 2 O) 6 ] +3 + SCN -  [Fe(SCN - )(H 2 O) 5 ] +2 + H 2 O Question: What type of bond is formed between the ligand and the central transition metal in complexes? Dative Bond b. Excess dilute nitric acid is added to a solution containing tetraamminecadmium (II) ions. 4H+ + [Cd(NH 3 ) 4 ] +2  Cd +2 + 4NH 4 + Question: What type of hybridization is found around the nitrogen atom in the product? sp 3 hybridization

22. 6. Organic Chemistry A reaction where an organic compound is involved. Hints: Most often, combustion or oxidation Addition reactions; breaking a double bond and adding a halogen or hydrogen Substitution; removing hydrogen with something Esterification; Carbon acid + alcohol giving an ester and water Know names and rules for organic compounds.

23. a. methane is mixed with an excess of bromide gas CH 4 + 4Br 2  CBr 4 + 4HBr Question: What type of reaction is taking place? a substitution; H atoms replaced by Br b. 1-propanol is burned completely in air 2CH 3 CH 2 CH 2 OH + 9O 2  6CO 2 + 8 H 2 O Question: If four moles of 1-propanol were burned, how many moles of carbon dioxide would be formed?

24. c. Ethanoic acid is refluxed with ethanol and a catalyst for several hours. CH 3 COOH + C 2 H 5 OH  CH 3 COOC 2 H 5 + H 2 O Question: What is a common use of the organic product in this reaction? Esters are often used as artificial fruit flavors.