The document discusses net ionic equations, which involve writing molecular and ionic equations and identifying spectator ions. A molecular equation shows all species as whole units, while an ionic equation shows dissolved species as free ions. To write a net ionic equation, the molecular equation is first written and balanced, then molecules are broken into ions. Spectator ions that are present on both sides of the reaction are then canceled to give the net ionic equation. The document also discusses what substances will ionize or dissociate into ions in solution based on their type (salt, acid, base) and whether they are considered strong electrolytes.

1. Net Ionic Equations

2. Stuff you already know! Solute Solvent Solution Homogeneous Mixture Mixture Dissolve

3. Stuff you want to learn today. Molecular Equation Ionic Equation Net Ionic Equation Spectator Ions Electrolytes Salts Strong Acid Strong Base Hi, I’m Ion the spectator

4. Stuff you are learning right now! Molecular Equation Equation in which the formulas of the compounds are written as though all species existed as molecules or whole units. Ionic Equation An equation that shows dissolved species (soluble salts, acids, or bases) as free ions.

5. Molecular Vs. Ionic Equations Molecular Equation: CaCl 2(aq) + Na 2 CO 3(aq)  CaCO 3(s) + 2NaCl (aq) Ionic Equation: Ca +2 (aq) + 2Cl -1 (aq) + 2Na +1 (aq) + CO 3 -2 (aq)  CaCO 3 (s) + 2 Na +1 (aq) + 2 Cl -1 (aq)

6. Molecular vs. Ionic Equations Na + Na + Cl - Cl - Cl - Na + H + OH -1 OH -1 H + H + 3 NaCl 3 H 2 O OH -1

7. Writing Net Ionic Equations Write & Balance the molecular Equation You need same # of atoms on of each element on both sides Use Solubility table to determine the solubility of the salts Poorly soluble salts do NOT ionize (break apart)

8. Writing Net Ionic Equations continued 3 Break molecules into ions Write Proper charges Use Coefficients to balance atom count Do NOT break up polyatomic ions (SO 4 -2 , CO 3 -2 , PO 4 -3 ) 4 Cancel Spectator Ions & Rewrite

9. Spectator Ions Ions present on product & reactant side that stay the same and are not directly involved in the chemical reaction. Molecular Equation: CaCl 2(aq) + Na 2 CO 3(aq)  CaCO 3(s) + 2 NaCl (aq) Ionic Equation: Ca +2 (aq) + 2Cl -1 (aq) + 2Na +1 (aq) + CO 3 -2 (aq)  CaCO 3 (s) + 2Na +1 (aq) + 2 Cl -1 (aq) Net Ionic Equation Ca +2 (aq) + CO 3 -2 (aq )  CaCO 3 (s)

10. What Ionizes? READ THE FINE PRINT Phase Labels: Solid – (s) Liquid – (l) Gas – (g) Aqueous – (aq) * Solids, Liquids, & Gases do not break into ions!!!

11. Will it Ionize? Salts? – Use solubility Table Acids? - Are they Strong? Bases? - Are they Strong

12. SALTS The Solubility Table p. 344 Ion Solubility Exceptions NO 3 – soluble none ClO 4 – soluble none Cl – soluble except Ag + , Hg 2 2+ , *Pb 2+ I – soluble except Ag + , Hg 2 2+ , *Pb 2+ SO 4 2- soluble except Ca 2+ , Ba 2+ , Sr 2+ , Hg 2+ , Pb 2+ , Ag + CO 3 2- insoluble except Group IA and NH 4 + PO 4 3- insoluble except Group IA and NH 4 + OH – insoluble except Group IA, *Ca 2+ , Ba 2+ , Sr 2+ S 2- insoluble except Group IA, IIA and NH 4 + Na + soluble none K + soluble none NH 4 + soluble none

13. Acids (HNm) Strong Acids Acids formed from the group VIIA Nonmetals Br, Cl, I are strong Examples: HBr, HCl, HI Acids where the # of oxygen atoms minus the # of hydrogen atoms is 2 or greater are strong.

14. Will it “completely” Ionize aka Is it a Strong Acid? HBr HI H 2 S H 2 SO 4 HC 2 H 3 O 2 HClO 3 HClO 2 HNO 3 C 2 Br 6

15. Bases (MOH) Strong Bases Bases formed from group IA & IIA Metals are strong w/ the exceptions of Be, Mg, & Fr.

16. Will it “completely” Ionize aka Is it a Strong Base? NaOH KOH Mg(OH) 2 Al(OH) 3 Be(OH) 2 Ca(OH) 2