1 / 19

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.

elia
Télécharger la présentation

Warm Up Review

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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.

More Related