Types+of+Reactions

The following table lists the types of reactions we have studied and the date of each quiz.

Each quiz can include material from any of the previous quizzes.
 * Quiz Number || Date || Types of Reactions || Textbook References ||
 * 1 || August 31, 2012 || Synthesis (Combination) reactions between metals and nonmetals to produce binary salts and the decomposition of hydrogen peroxide || Addison-Wesley section 8.2; Flinn Scientific Chapter 7 ||
 * 2 || September 14, 2012 || Decomposition Reactions of carbonate, such as metallic carbonates (i.e. limestone, which is calcium carbonate), ammonium carbonate, carbonic acid. The decomposition of reactions chlorate and sulfurous acid. || Addison-Wesley section 24.1, page 710; Flinn Scientific Handbook, the decomposition reactions on pages 42 and 43. ||
 * 3 || December 4, 2012 || Combustion of alkanes - methane through decane. || A paragraph and illustration about combustion reactions can be found in Addison Wesley, section 8.2, pages 220 and 221. Also, alkanes are discussed in Addison Wesley, section 25.1 (pages 743 to 751). The table on 745 lists the formulas and names of the alkanes you should memorize. ||
 * 4 || January 25, 2013 || Alkali metals in water and in air. || Addison-Wesley section 24.1, especially page 706. Brown-LeMay section 7.7, page 258. ||
 * 5 || February 8, 2013 || Single replacement reactions of metals. You should memorize that alkali metals are more reactive than alkaline earths, and that transition metals are less reactive than these. The least reactive metals are copper, silver, gold, and platinum. Solutions of copper, silver, or gold ions will dissolve your car (and many other metals). || Brown LeMay, section 7.4, especially pages 131 and 132. Addison-Wesley section 8.2, pages 216 to 218. ||
 * 6 ||  || * Metal oxides in water.
 * Nonmetal oxides in water.
 * (metal) hydrides in water.
 * (metal) nitrides in water. || Examples of these reactions are shown in Brown LeMay, section 7.6, pages 254 and 255. A very detailed discussion of the behavior of the oxide ion in water can be found in Brown LeMay, section 16.5 (middle of page 627). This discussion shows that hydrides and nitrides also form bases in water. ||
 * 7 ||  || Neutralization reactions. Neutralization reactions forming the gases H2S and CO2 are interesting cases. They are described on pages 126 and 127. Neutralization reactions also happen in two other cases: metal oxides in acids and nonmetal oxides in bases. || Brown LeMay, section 4.3, especially pages 124 to 127 explains most neutralization reactions. Also, section 7.6 (pages 254 and 256) shows examples of the metal and nonmetal oxides. ||

Try the following method for memorizing the solubility guidelines. 1. Fold a paper in half. Use one half for the soluble ions and the other half for the insoluble ions. 2. Work on the soluble side first. Write the common ions that form soluble compounds. 3. Work on the insoluble side. 4. Now add the exceptions on the soluble side. Notice that only three ions have exceptions: the halides, sulfate, and sulfide. The exceptions in these cases are caused by two sets of cations:
 * 1) write all the halides except fluoride (chloride, bromide, iodide)
 * 2) write all the ions from column one, including hydrogen.
 * 3) write nitrate, chlorate, and sulfate. **Look at this list - it contains the conjugate ions of the strong acids and the same metal ions that form strong bases.
 * 4) write acetate (CH3COO-) and ammonium (NH4+). Notice that you now have listed to conjugate base of acetic acid and the conjugate acid of ammonia).
 * 1) write hydroxide. Notice that H+ makes compounds soluble while OH- makes them insoluble.
 * 2) write carbonate and phosphate.
 * 3) write sulfide.
 * 1) Ca2+, Sr2+, and Ba2+ are not soluble with sulfate (SO4)2- but are soluble when with sulfide, S2-.
 * 2) Ag+, Pb2+, and (Hg2)2+ are not soluble with sulfate or with the halides.

These are links to some really cool periodic tables: 1. Dynamic periodic table