1. Unit 9: Reactions Types & Net Ionic Equations John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall, Inc. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

2. Redox Reactions: Decomposition AB → A + B1 → 2 (+/– → 0 0) Combustion C x H y + O 2 → CO 2 + H 2 O (–/+ 0 → +/– +/–) Single Replacement AB + C → A + CB (+/– 0 → 0 +/–) Synthesis A + B → AB2 → 1 (0 0 → +/–) Reactions Types Double Replacement AB + CD → AD + CB (+/– +/– → +/– +/–) NOT Redox

3. Balanced Net Ionic Equations 1.Complete molecular equation. 2.Dissociate all strong electrolytes (aq). 3.Cross out spectators (same charge & state) 4.Net Ionic Equation with remaining species. 5.Balance it. (if REDOX: O H E BALANCE U) comp – diss – cross – net – bal (SA’s, SB’s, & Soluble salts) Group I NH 4 + NO 3 –

4. BaSO 4 + NH 4 NO 3 Balanced Net Ionic Equations 1)(NH 4 ) 2 SO 4 + Ba(NO 3 ) 2 → 2)HCl (aq) + NaOH (aq) → 3)HF (aq) + KOH (aq) → comp – diss – cross – net – bal +2–2+––+ Ba 2+ + SO 4 2– → BaSO 4 NaCl (aq) + H 2 O ( l ) +–+––+ H + + OH – → H 2 O Strong Acid and Strong Base Precipitation KF (aq) + H 2 O ( l ) + – –+ HF + OH – → F – + H 2 O Weak Acid and Strong Base Double Replacement

5. Gas-Forming Reactions Single Rep: Metal + Acid Metal Ion + H 2 4) Zn (s) + H 2 SO 4 (aq) ZnSO 4 (aq) + H 2 (g) NIE: Zn (s) + 2 H + (aq) Zn 2+ (aq) + H 2 (g) (M 0 )(H + )(M + )(gas) +2– 2+2– Double Rep: Acid + Carbonate Salt + 5) HCl (aq) + CaCO 3 (s) CaCl 2 (aq) + H 2 O (l) + CO 2 (g) NIE: 2 H + (aq) + CaCO 3 (s) Ca 2+ (aq) + H 2 O (l) + CO 2 (g) (or Bicarbonate) (HCO 3 – ) (CO 3 2– ) (H + ) CH 3 COOH + NaHCO 3  CH 3 COONa +H 2 O + CO 2 H 2 CO 3 (aq) H 2 O (l) + CO 2 (g) (decomposes immediately) (gas)

6. Activity Series of Metals increasing ease of oxidation Cannot displace H + from acid to make H 2 (g)