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Warm Up Review

Warm Up Review. Classify the type of reaction AgNO 3 + NaCl  AgCl + NaNO 3 2 PbO 2  2 PbO + O 2 3. 2 Al + 3 CuSO 4  Al 2 (SO 4 ) 3 + 3 Cu Predict the products of the following reactions: Zn + 2 AgNO 3  MgCl 2 + Ca(OH) 2  2Mg + O 2 . Warm Up Review.

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Warm Up Review

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  1. Warm Up Review Classify the type of reaction • AgNO3 + NaCl AgCl + NaNO3 • 2 PbO2  2 PbO + O2 3. 2 Al + 3 CuSO4 Al2(SO4)3 + 3 Cu Predict the products of the following reactions: • Zn + 2 AgNO3  • MgCl2 + Ca(OH)2  • 2Mg + O2 

  2. Warm Up Review Classify the type of reaction • AgNO3 + NaCl AgCl + NaNO3 double displacement • 2 PbO2  2 PbO + O2 decomposition 3. 2 Al + 3 CuSO4 Al2(SO4)3 + 3 Cu single displacement Predict the products of the following reactions: • Zn + 2 AgNO3  Zn(NO3)2 + 2Ag • MgCl2 + Ca(OH)2  Mg(OH)2 + CaCl2 • 2Mg + O2  2MgO

  3. Quiz on Friday 8.2…… Study 8.3 Reactions in Aqueous Solution

  4. H2O • Water is a combination of two ions H+ and OH- • The reaction of ionic compounds in water (aqueous solution) allows the ionic compounds to disassociate in the solution. • (aq) indicates that in solution the ions are formed AgNO3(aq) Ag+ (aq) and NO3- (aq)

  5. Some ions combine in solutions to form insoluble solids. • These insoluble solids are called precipitates. • Precipitates are indicated by (s) • They do not dissolve in solution to form ions Ag+ + Cl- AgCl (s)

  6. Precipitates

  7. Writing Complete Ionic Equations • An equation that shows the dissolved ionic compounds (ie. The ions) Mg(NO3)2(aq)  +  Na2CO3(aq)MgCO3 (s)  +  2 NaNO3(aq)

  8. Writing Complete Ionic Equations • An equation that shows the dissolved ionic compounds (ie. The ions) Mg(NO3)2(aq)  +  Na2CO3(aq)MgCO3 (s)  +  2 NaNO3(aq) Mg2+ (aq)  ** Your turn- try to complete the rest of ionic eqaution!

  9. Writing Complete Ionic Equations • An equation that shows the dissolved ionic compounds (ie. The ions) Mg(NO3)2(aq)  +  Na2CO3(aq)MgCO3 (s)  +  2 NaNO3(aq) Mg2+ (aq)  +  2 NO3¯ (aq)  +  2 Na+ (aq)  +  CO32- (aq)   MgCO3 (s)  +  2 Na+ (aq)  +  2 NO3¯ (aq)

  10. Ions that appear on both sides of the equation are not directly involved in the reaction. • They are called spectator ions Mg(NO3)2(aq)  +  Na2CO3(aq)MgCO3 (s)  +  2 NaNO3(aq) Mg2+ (aq)  +  2 NO3¯ (aq)  + 2 Na+ (aq) +  CO32- (aq)   MgCO3 (s)  +  2 Na+ (aq) + 2 NO3¯ (aq)

  11. The equation can be re-written with out the spectator ions. This is called a Net ionic equation. Mg(NO3)2(aq)  +  Na2CO3(aq)MgCO3 (s)  +  2 NaNO3(aq) Mg2+ (aq)  +  2 NO3¯ (aq)  +  2 Na+ (aq)  +  CO32- (aq)  MgCO3 (s)  +  2 Na+ (aq)  +  2 NO3¯ (aq) Mg2+ (aq) +  CO32- (aq)  MgCO3 (s)

  12. Predicting the formation of a Precipitate • Write the ions formed by your reactants • Identify how the ions (cations and anions) will rearrange • Look at table 8.3 (pg. 227) to see if the newly formed products are soluble • If they are soluble, that means they will dissolve into ions • If they are insoluble, they will be solids (precipitates)

  13. Predicting the Formation of a Precipitate: Example SrBr2 (aq)  +  K2SO4 (aq)   First: Identify the Ions formed Sr2+ (aq)  +  2 Br¯ (aq)  +  2 K+ (aq)  +  SO42- (aq)

  14. Predicting the Formation of a Precipitate: Example SrBr2 (aq)  +  K2SO4 (aq)   First: Identify the Ions formed Sr2+ (aq)  +  2 Br¯ (aq)  +  2 K+ (aq)  +  SO42- (aq) Second: Identify how the ions will rearrange SrSO4 and KBr 

  15. Predicting the Formation of a Precipitate: Example SrBr2 (aq)  +  K2SO4 (aq)   First: Identify the Ions formed Sr2+ (aq)  +  2 Br¯ (aq)  +  2 K+ (aq)  +  SO42- (aq) Second: Identify how the ions will rearrange SrSO4 and KBr Third: Look at Table 8.3 to identify which compounds are soluble. • Notice the rule for sulfates (SO4); soluble except when in compounds of Pb, Ag, Hg, Ba, Sr, and Ca • Notice the rule for salts of alkali metals and ammonia (they are soluble)

  16. Predicting the Formation of a Precipitate: Example SrBr2 (aq)  +  K2SO4 (aq)   First: Identify the Ions formed Sr2+ (aq)  +  2 Br¯ (aq)  +  2 K+ (aq)  +  SO42- (aq) Second: Identify how the ions will rearrange SrSO4 (s) and KBr (aq)   Third: Look at Table 8.3 to identify which compounds are soluble. • Notice the rule for sulfates (SO4); soluble except when in compounds of Pb, Ag, Hg, Ba, Sr, and Ca • Notice the rule for salts of alkali metals and ammonia (they are soluble)

  17. Lets re-write the net ionic equation using this information! Sr2+ (aq)  +  2 Br¯ (aq)  +  2 K+ (aq)  +  SO4(aq)    SrSO4 (s)  +  2 K+ (aq)  +  2 Br¯ (aq) Sr2+ (aq)  +  SO42- (aq)      SrSO4 (s)

  18. The End! Begin HW so that I am able to help you during class.

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