4 Course Handouts
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Periodic Table
Periodic Table (PDF)
Significant Figures & Rounding
Significant Figures & Rounding (.doc file)
Strong Acids and Bases to Memorize
Strong Acids
- HCl (hydrochloric acid)
- HBr (hydrobromic acid)
- HI (hydroiodic acid)
- HNO3 (nitric acid)
- H2SO4 (sulfuric acid)
- HClO4 (perchloric acid)
- HClO3 (chloric acid)
- HBrO4 (perbromic acid)
- HClO3 (chloric acid)
- HIO4 (periodic acid)
- HClO3 (iodic acid)
If the acid in question is not on this list, you may assume it is weak for this class.
Strong Bases
- LiOH (lithium hydroxide)
- NaOH (sodium hydroxide)
- KOH (potassium hydroxide)
- RbOH (rubidium hydroxide)
- CsOH (cesium hydroxide)
- Ca(OH)2 (calcium hydroxide)
- Sr(OH)2 (strontium hydroxide)
- Ba(OH)2 (barium hydroxide)
If the base in question is not on this list, you may assume it is weak for this class.
Polyatomic ions
Ions with more than one atom. (You should know the name, formula, and charge!)
| Charge | Name | Formula |
|---|---|---|
| -1 | Acetate | C2H3O2– |
| -1 | Chlorate | ClO3– |
| -1 | Chlorite | ClO2– |
| -1 | Nitrate | NO3– |
| -1 | Nitrite | NO2– |
| -1 | Cyanide | CN– |
| -1 | Hydroxide | OH– |
| +1 | Ammonium | NH4+ |
| -2 | Chromate | CrO42- |
| -2 | Carbonate | CO32- |
| -2 | Sulfate | SO42- |
| -2 | Sulfite | SO32- |
| -3 | phosphate | PO43- |
| -3 | phosphite | PO33- |
Solubility Tables
Soluble
| Contains these Ions | Soluble | Exceptions |
|---|---|---|
| Li+, Na+, K+, Rb+, Cs+, NH4+ | Most salts (ionic compounds) containing alkali metals (Group 1) and ammonium are soluble. | none |
| NO3– | Most salts containing nitrate are soluble | |
| Cl–, Br–, I– | Most salts containing halogen anions (Main Group 7) are soluble. (Chloride, bromide, and iodide salts) | Salts containing Cu+, Ag+, Pb2+, and Hg22+ |
| SO42- | Many salts containing sulfate are soluble. | Salts containing Sr2+, Ba2+, Pb2+, and Hg22+ |
Insoluble
| Contains these Ions | Insoluble | Exceptions |
|---|---|---|
| OH– and S2- | Most salts containing hydroxide or sulfide anions are insoluble. | Salts containing alkali metals (Li+, Na+, K+, Rb+, and Cs+), and the “heavy” alkaline earth metals (Ca2+, Sr2+, and Ba2+) |
| CO32-, PO43- | Most salts containing carbonate or phosphate anions are insoluble. | Salts containing alkali metals (Group 1) and ammonium are soluble. (Li+, Na+, K+, Rb+, Cs+, NH4+) |
| SO42- | Many salts containing sulfate and cations with charges greater than or equal to 2 are insoluble, including salts containing Sr2+, Ba2+, Pb2+, and Hg22+. | Salts containing Cu+, Ag+, Pb2+, and Hg22+ |
| SO42- | Many salts containing sulfate are soluble. | Salts containing alkali metals (Group 1) and ammonium are soluble. (Li+, Na+, K+, Rb+, Cs+, NH4+), and Mg2+ |
Oxidation Number Rules
- For pure elements, the oxidation numbers are equal to zero (0).
- ex: Mg0 H20 O20 Cu0
- For monatomic ions, the oxidation number is equal to the charge on the ion.
- ex: Mg2+ Ca2+ Na+ Cu+
- F in compounds is always F– (ox # = -1)
- O in compounds is almost always O2- (ox # = -2) (exceptions include peroxides, such as H2O2)
- Metals in group 1A are always +1 (ox # = +1)
- ex: Na+ K+
- Metals in group 2A are always +2 (ox # = +2)
- ex: Mg2+ Ca2+
- H in compounds is usually +1, (unless bonded to a metal, then -1, such as in H-storage materials)
H2O H+
exception: LiBH4 (H is -1) - The sum of the oxidation numbers for all atoms in the compound must equal the overall charge of the compound. The sum of the oxidation numbers for all atoms in a polyatomic ion must equal the overall charge of the ion.