2. The Activity Series & Solubility

3. The Activity Series Ranks metals from most to least reactive. –the top are most reactive –the bottom are least reactive Used to predict if a single displacement reaction will take place. K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au

4. Using the Activity Series Identify the Reactants Check the Activity Series –The only way the reaction will occur is if the metal that ’ s by itself is higher on the series than the one in the compound –Ex: CaCl 2 + Na  – NaCl + Ca  K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au

5. Examples: Fe+ CuSO 4  Ni+ NaCl  Li+ ZnCO 3  Al+ CuCl 2  Determine if the reaction occurs If so: Write products and balance the equations If not: write NR for No Reaction Cu + Fe 2 (SO 4 ) 3 Yes, Fe is above Cu NR (no reaction) No, Ni is below Na Zn + Li 2 CO 3 Cu + AlCl 3 Yes, Al is above Cu K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au Yes, Li is above Zn 2Fe + 3Cu SO 4  Fe 2 (SO 4 ) 3 + 3Cu 2Li + ZnCO 3  Li 2 CO 3 + Zn 2Al + 3CuCl 2  3Cu + 2AlCl 3

6. Halogens Like the metals, Halogens have an activity series as well. The halogen activity series simply follows group 17 down the Periodic table –By themselves, halogens are always diatomic. F2F2 Cl 2 Br 2 I2I2

7. Examples 2 NaI + Cl 2  2 LiCl + Br 2  F2F2 Cl 2 Br 2 I2I2 2 NaCl + I 2 N.R. Yes, Cl 2 is above I 2 No, Br 2 is below Cl 2

8. More Problems Predict if each reaction will happen, if so, write the products, if not write NR. Balance any reaction that occurs. HCl + I 2  Ag(NO 3 ) + Ni  Pb + Zn(C 2 H 3 O 2 ) 2  CaBr 2 + F 2  Mg + ZnCl 2  Zn + Fe(SO 4 )  KBr + Cl 2  Mg + Ca(NO 3 ) 2  K Na Li Ca Mg Al Zn Fe Ni Sn Pb H Cu Hg Ag Au F2F2 Cl 2 Br 2 I2I2

9. Solubility Solubility rules tell whether a compound is soluble or not. If a compound is soluble it reacts, if not it does not.

10. Solubility Rules  All compounds containing alkali metal cations and the ammonium ion are soluble.  All compounds containing NO 3 -, ClO 4 -, ClO 3 -, and C 2 H 3 O 2 - anions are soluble.  All chlorides, bromides, and iodides are soluble except those containing Ag +, Pb 2 +, or Hg 2 2+.

11. Solubility Rules Cont.  All sulfates are soluble except those containing Hg 2 2+, Pb 2+, Sr 2+, Ca 2+, or Ba 2+.  All hydroxides are insoluble except compounds of the alkali metals, Ca 2+, Sr 2+, and Ba 2+. 6) All compounds containing PO 4 3-, S 2-, CO 3 2-, and SO 3 2- ions are insoluble except those that also contain alkali metals or NH 4 +.

12. Predict if the Compound reacts Mg(NO 3 ) 2 CaSO 4 CaCl 2 K 2 SO 4 Al 2 S 3 Ba(OH) 2 (NH 4 ) 3 PO 4 Mg(OH) 2 SrCO 3 BeS BaSO 4 CuCl 2

13. Predict the Products & Balance ____Mg(NO 3 ) 2 + ____Al 2 S 3  ____CaSO 4 + ____BeS  ____CaCl 2 + ____Ba(OH) 2  ____K 2 SO 4 + ____(NH 4 ) 3 PO 4  ____SrCO 3 + ____CuCl 2  ____BaSO 4 + ____Mg(OH) 2 

14. Predicting Products 1.Decide what kind of reaction it is (one of the five types) 2.Apply the rules for that type of reaction 3.Balance the equation 4.If you absolutely can ’ t balance the equation, the equation isn ’ t correct!

15. New Problems ___NaCl  ? What kind of reaction will this be? How do you know? So what are the products? ___NaCl  ___Na + ___Cl 2

16. Fe + CuSO 4  ? What kind of reaction will this be? How do you know? Does it react? What are the products? ___Fe + ___CuSO 4  ___FeSO 4 + ___Cu

17. Fe 2 O 3 + HCl  ? What kind of reaction will this be? How do you know? Does it react? What are the products? __Fe 2 O 3 + ___HCl  ___FeCl 3 + __H 2 O

18. C 3 H 8 + O 2  What kind of reaction will this be? How do you know? So what are the products? ___C 3 H 8 + ___O 2  ___CO 2 + ___H 2 O

19. Fe + Cl 2  What kind of reaction will this be? How do you know? So what are the products? Fe + Cl 2  FeCl 3

20. Practice ___H 2 + ___S  ___C 6 H 12 O 6 + ___O 2  ___GeBr 4  ___C + ___Br 2  ___NaFBr  ___Cu + ___H 2 SO 4 

21. More Practice ___Cr(OH) 3 + ___HCl  ___C 3 H 8 + ___O 2  ___Cl 2 O 3  ___B 2 O 3 + ___Al 2 F 6  ___C 12 H 26 O 12 + ___O 2  ___Ba(OH) 2 + ___CO 2  ___Be + ___P 