Inorganic Chemistry Nomenclature A. Anions
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1 Writing Net Ionic Equations and Determination of Spectator Ions Predicting Products and Balancing Total Equation: 1. Given reactants, swap appropriate ions to form product compounds 2. Determine phase of products using Solubility Rule or Solubility Table 3. Place appropriate coefficients in front of compound to balance the Total Equation. Writing out Net Ionic Equation and Determining Spectator Ions: 4. For each of the compound in the balanced total equation: (a) Leave intact if it is solid (s), liquid (l), or gas (g) (b) Break into appropriate ion if it is aqueous (aq) 5. Cancel out identical ions from both sides of the equation. These ions are known as the spectator ions. 6. The remaining ions has the same phase as its parent compound. These ions and compounds form the Net Ionic Equation. Inorganic Chemistry Nomenclature A. Anions carbide C 4 nitride N 3 peroxide O 2 2 fluoride F acetate C 2 H 3 O 2 nitrite NO 2 oxide O 2 chloride Cl carbonate CO 3 2 nitrate NO 3 hydroxide OH hypochlorite ClO oxalate C 2 O 4 2 phosphide P 3 sulfide S 2 chlorite ClO 2 cyanide CN phosphite PO 3 3 sulfite SO 3 2 chlorate ClO 3 phosphate PO 4 3 sulfate 2 perchlorate ClO 4 silicide Si 4 arsenide As 3 selenide Se 2 bromide Br silicate SiO 3 2 arsenite AsO 3 3 selenite SeO 3 2 hypobromite BrO germanide Ge 4 arsenate AsO 4 3 selenate SeO 4 2 bromite BrO 2 germanate GeO 3 2 telluride Te 2 bromate BrO 3 hydrogen carbonate (bicarbonate) HCO 3 hydrogen sulfite (bifulfite) HSO 3 hydrogen sulfate (bisulfate) H chromate CrO 4 2 tellurite TeO 3 2 perbromate BrO 4 tellurate TeO 4 2 iodide I hypoiodite IO iodite IO 2 iodate IO 3 periodate IO 4
2 dichromate Cr 2 O 7 2 permanganate MnO 4 B. Cations Common name IUPAC name Formula or Symbol ammonium ammonium NH 4 + hydronium hydronium H + cuprous copper (I) Cu + cupric copper (II) Cu 2+ mercurous mercury (I) Hg 2 2+ mercuric mercury (II) Hg 2+ ferrous iron (II) Fe 2+ ferric iron (III) Fe 3+ nickelous nickel (II) Ni 2+ nickelic nickel (III) Ni 2+ stannous tin (II) Sn 2+ stannic tin (IV) Sn 4+ The following metal ions have only one oxidation number: 1+ : All group IA metal ions (Li +, Na +, K +, Rb +, Cs +, Fr + ) and Ag + 2+ : All group IIA metal ions (Be 2+, Mg 2+, Ca 2+, Sr 2+, Ba 2+, Ra 2+ ), Zn 2+ and Cd : Al 3+ Solubility Rules 1. All salts of group IA and NH 4 + are soluble. 2. All NO 3, ClO3, ClO4 and C2 H 3 O 2 salts are soluble. 3. All Cl, Br, and I salts are soluble except those of Ag +, Hg 2 2+ and Pb All SO4 2 salts are soluble except those of Ca 2+, Ag +, Pb 2+,Sr 2+ and Ba 2+. (NOTE: Ag 2 SO4 is slightly soluble) 5. All metal oxides are insoluble except those of group IA, Ca 2 + and Sr 2+. Upon dissolving in water these are converted to the hydroxide. 6. All metal hydroxides are insoluble except those of group IA, Ca 2 + and Sr 2+. Ba(OH)2 is slightly soluble. 7. All CO 3 2, PO 4 3 and S 2 salts are insoluble except those of group IA and NH4 +.
3 Example 1 Given: AgNO 3 (aq) + NaCl (aq) Ag + Cl Na+ NO 3 AgNO 3 (aq) + NaCl (aq) AgCl + NaNO 3 AgNO 3 (aq) + NaCl (aq) AgCl (s) + NaNO 3 (aq) Also balance the equation with appropriate coefficients. Ag + NO 3 Na + Cl AgCl Na + NO 3 Ag + NO 3 Na + Cl AgCl Na + NO 3 Spectator ions: NO 3, Na + Net ionic equation: Ag + (aq) + Cl (aq) AgCl (s) Example 2 Given: BaCl 2 (aq) + H 2 (aq) Ba 2+ 2 H + Cl BaCl 2 (aq) + H 2 (aq) Ba + HCl BaCl 2 (aq) + H 2 (aq) Ba + HCl BaCl 2 (aq) + H 2 (aq) Ba + 2 HCl
4 Ba 2+ 2 Cl 2 H + 2 Ba 2 H + 2 Cl Ba 2+ 2 Cl 2 H + 2 Ba 2 H + 2 Cl Spectator ions: Cl, H + Net ionic equation: Ba 2+ (aq) + 2 (aq) BaSO4 (s) Example 3 Given: (NH 4 ) 2 (aq) + KOH (aq) + NH 4 OH 2 K + 2 (NH 4 ) 2 (aq) + KOH (aq) NH 4 OH + K 2 (NH 4 ) 2 (aq) + KOH (aq) NH 4 OH (aq) + K 2 (aq) (NH 4 ) 2 (aq) + 2 KOH (aq) 2 NH 4 OH (aq) + K 2 (aq) NH 4 SO4 2 K + 2 OH + 2 NH 4 2 OH 2 K NH 4 SO4 2 K + 2 OH + 2 NH 4 2 OH 2 K + 2 Spectator ions: NH 4 +, OH, K +, SO4 2 Net ionic equation: none Note: If all species are aqueous (aq), then all ions are spectator ions and there will be no net ionic equation.
5 Example 4 (This example has the products and their phases already given.) Given: (NH 4 ) 2 (aq) + KOH (aq) NH 3 (g) + H 2 O (l) + K 2 (aq) (NH 4 ) 2 (aq) + 2 KOH (aq) 2 NH 3 (g) + 2 H 2 O (l) + K 2 (aq) NH 4 SO4 2 K + 2 OH 2 NH 3 2 H 2 O 2 K NH 4 SO4 2 K + 2 OH 2 NH 3 2 H 2 O 2 K + 2 Spectator ions: K +, 2 Net ionic equation: 2 NH 4 + (aq) + 2 OH (aq) 2 NH3 (g) + 2 H 2 O (l) Better net ionic equation: NH 4 + (aq) + OH (aq) NH3 (g) + H 2 O (l) Example 5 Given: Na 3 PO 4 (aq) + Ca(NO 3 ) 2 (aq) 3 Ca PO 4 Na + NO 3 Na 3 PO 4 (aq) + Ca(NO 3 ) 2 (aq) Ca 3 (PO 4 ) 2 + NaNO 3 Na 3 PO 4 (aq) + Ca(NO 3 ) 2 (aq) Ca 3 (PO 4 ) 2 (s) + NaNO 3 (aq) 2 Na 3 PO 4 (aq) + 3 Ca(NO 3 ) 2 (aq) Ca 3 (PO 4 ) 2 (s) + 6 NaNO 3 (aq) 6 Na PO 4 3 Ca 2+ 6 NO 3 Ca 3 (PO 4 ) 2 6 Na + 6 NO 3
6 6 Na + 2 PO Ca 2+ 6 NO 3 Ca 3 (PO 4 ) 2 6 Na + 6 NO 3 Spectator ions: Na +, NO 3 Net ionic equation: 2 PO 4 3 (aq) + 3 Ca 2+ (aq) Ca3 (PO 4 ) 2 (s).
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