1. Net Ionic Equations Review Grade lab reports Notes on Net ionic equations Guided Practice Homework

2. Write, predict, balance 1. Sulfur dioxide reacts with water.

3. Grading of Lab Reports Using the provided rubric grade the lab report you are provided. Discuss their thinking and conclusions.

4. Date: Net Ionic Equations I

5. Electrolytes Many times the reactants of DR rxns are in aqueous solutions. This means that the compound (ionic salt) actually separates into its cation and anion in water They become electrolytes. Able to conduct electricity Observe: strong, weak and non-electrolytes

6. All important product, AIP In order for a double replacement reaction to occur, it must create: precipitate(solid) water gas

7. Example Problem AgNO 3 + NaCl  AgCl + NaNO 3 Using the solubility chart, determine the state of matter of each compound. This is the MOLECULAR EQUATION Which is the all important product? Rewrite the equation, separating each aqueous compound into its cation and anion.

8. Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq)  AgCl (s) + Na + (aq) + NO 3 - (aq) This is the COMPLETE IONIC EQUATION Omit matching ions from both sides of the equation; these are the spectator ions, they only watched the chemistry take place – they were not a part of it. Scratch NO 3 - (aq) and Na + (aq)

9. What remains is the NET IONIC EQUATION, the actual chemistry that took place. Ag + (aq) + Cl - (aq)  AgCl (s)

10. BaCl 2 + MgSO 4  MgCl 2 + BaSO 4 Ba +2 (aq) + SO 4 -2 (aq)  BaSO 4(s)

11. Sr(C 2 H 3 O 2 ) 2 +Na 2 SO 4  SrSO 4 + 2NaC 2 H 3 O 2 Sr +2 (aq) + SO 4 -2 (aq)  SrSO 4(s)

12. LiOH + HCl  LiCl + H 2 O OH - (aq) + H + (aq)  H 2 O (l)

13. Na 2 CO 3 + HI CO 3 -2 (aq) + 2H + (aq)  H 2 O (l) + CO 2(g)