1. Net Ionic Equations

2. Equations Reactant formulas/symbols  Product formulas/symbols What we’ve done so far Example Fe(s) + 2AgNO 3 (aq)  2Ag(s) + Fe(NO 3 ) 2 (aq)

3. Don’t Forget! Must write state of matter Solid, liquid, gas, aqueous Types of products Check solubility rules Solid product? You have a precipitate

4. Complete Ionic Equation Reactant ions  Product ions Write soluble ionic compounds as individual ions Example Fe(s) + 2AgNO 3 (aq)  2Ag(s) + Fe(NO 3 ) 2 (aq) Fe(s) + 2Ag + (aq) + 2NO 3 - (aq)  2Ag(s) + Fe +2 (aq) + 2NO 3 - (aq)

5. Spectator Ions Present on both sides of the equation Do not change Example Fe(s) + 2Ag + (aq) + 2NO 3 - (aq)  2Ag(s) + Fe +2 (aq) + 2NO 3 - (aq) What did not change? 2NO 3 - (aq)

6. Net Ionic Equation Does not contain spectator ions Example Fe(s) + 2Ag + (aq) + 2NO 3 - (aq)  2Ag(s) + Fe +2 (aq) + 2NO 3 - (aq) Fe(s) + 2Ag + (aq)  2Ag(s) + Fe +2 (aq)

7. Try It! Write the chemical equation, complete ionic equation, and net ionic equation for: Lead(II) nitrate reacts with hydrogen chloride to yield lead(II) chloride and hydrogen nitrate

8. Try It! Answer Chemical Pb(NO 3 ) 2 (aq) + 2 HBr(aq)  PbBr 2 (s) + 2HNO 3 (aq) Complete ionic Pb +2 (aq) + 2NO 3 ‾(aq) + 2H + (aq) + 2Br‾(aq)  PbBr 2 (s) + 2H + (aq) + 2NO 3 ‾(aq) Net ionic Pb +2 (aq) + 2Br‾(aq)  PbBr 2 (s)

9. Practice Makes Perfect Write complete & net ionic equations for all ppt reactions from data table I (don’t forget to balance and include phases)… the 1 st two are: BaCl 2 (aq) + 2AgNO 3 (aq)  2AgCl(s) + Ba(NO 3 ) 2 (aq) Sodium carbonate reacts with silver nitrate to yield sodium nitrate and silver carbonate.

10. Calcium chloride reacts with potassium phosphate to yield calcium phosphate and potassium chloride

11. Classwork / Homework Potassium + water  potassium hydroxide + hydrogen Zinc + hydrogen chloride  zinc chloride + hydrogen Copper(II) sulfate + iron  Nitrogen trihydride (l) + hydrogen sulfate  ammonium sulfate Iron(III) sulfate + barium nitrate  Potassium iodide + chlorine 

12. Rxn QU-EST directions Part 1 Directions: Write a balanced chemical equation for THREE (3) of the following reactions. Note: if no products are listed, you will need to predict them. Be sure to include the PROPER FORMULA, APPROPRIATE STATES/PHASES for each substance, and COEFFICIENTS needed to balance the equation. Also, please identify the TYPE of reaction (combination, decomposition, single replacement, double replacement, and combustion) as well as if the reaction occurs. Please indication the reactions you want graded by circling their numbers. If no reaction occurs, balance the equation and write NR above the reaction arrow. Assume only one product can be solid.

13. Rxn QU-EST directions Part 2 Directions: Write balanced chemical equation for FIVE (5) of the following reactions. Note: if no products are listed, you will need to predict them (keeping cation charges in new compounds). Be sure to include the PROPER FORMULA (with balanced charges if needed), APPROPRIATE STATES/PHASES for each product, and COEFFICIENTS needed to balance the equation. Please indication the reactions you want graded by circling their numbers. If no reaction occurs, balance the equation and write NR above the reaction arrow. Assume only one product can be solid, if any.

14. Rxn QU-EST directions Part 3 Directions: Write a NET IONIC equation for TWO (2) of your previously balanced DOUBLE REPLACEMENT REACTIONS from part 2 so choose wisely because the reaction MUST TAKE PLACE (i.e. NO “no reaction” reactions). You need to first write the COMPLETE IONIC equation along with the ORIGINAL NUMBER.