1. MOLECULAR, (TOTAL) IONIC AND NET IONIC EQUATIONS 1.Sodium chloride and silver nitrate → sodium nitrate and silver chloride NaCl + AgNO 3 → NaNO 3 + AgCl(s) The AgCl is labeled with (s) because it is insoluble and forms a precipitate.

2. IONIC EQUATION Na + + Cl - + Ag + + NO 3 - → Na + + NO 3 - + AgCl(s) All substance are dissociated except for the insoluble AgCl(s)

3. NET IONIC EQUATION The ions not involved in forming the precipitate (Na + and NO 3 - ) are called "Spectator Ions" and are eliminated to form the net ionic equation. Ag + + Cl - → AgCl(s) Any source of silver ions and chloride ions would result in the same net ionic equation. Sodium chloride substitutes contain potassium chloride.

4. 2. Copper(II) chloride + sodium sulfide → copper(II)sulfide and sodium chloride CuCl 2 + Na 2 S → CuS + NaCl CuCl 2 + Na 2 S → CuS (s) + 2 NaCl Cu 2+ + 2Cl - + 2Na + + S 2- → CuS(s) + 2Na + + 2Cl - The spectator ions are Na + and Cl - Cu 2+ + S 2- → CuS(s)

5. 3. Calcium chloride + sodium carbonate  calcium carbonate and sodium chloride CaCl 2 + Na 2 CO 3 → CaCO 3 (s) + 2NaCl Ca 2+ + 2Cl - + 2Na + + CO 3 2- → CaCO 3 (s) + 2Na + + 2Cl - The spectator ions are Na + and Cl - Ca 2+ + CO 3 2- → CaCO 3 (s)

6. 4. Barium nitrate + sodium phosphate → barium phosphate and sodium nitrate Ba(NO 3 ) 2 + Na 3 PO 4 → Ba 3 (PO 4 ) 2 (s) + NaNO 3 3 Ba(NO 3 ) 2 + 2 Na 3 PO 4 → Ba 3 (PO 4 ) 2 (s) + 6 NaNO 3 3Ba 2+ + 6NO 3 - + 6Na + + 2PO 4 3- → Ba 3 (PO 4 ) 2 (s) + 6Na + + 6NO 3 - The spectator ions are Na + and NO 3 - 3Ba 2+ + 2PO 4 3- → Ba 3 (PO 4 ) 2 (s)

7. 5. Chromium(III) chloride + silver nitrate → chromium(III) nitrate and silver chloride CrCl 3 + 3AgNO 3 → Cr(NO 3 ) 3 + 3AgCl(s) Cr 3+ + 3Cl - + 3Ag + + 3NO 3 - → Cr 3+ + 3NO 3 - + 3AgCl(s) 3Ag + + 3Cl - → 3AgCl(s) Ag + + Cl - → AgCl(s)