![]() ![]() Heating an oxysalt produces a metal oxide plus a nonmetal oxide or a metal salt plus oxygen, or some combination of these two decomposition reactions. (Al(C 2H 3O 2) 3 and Pb(NO 3) 2 are both soluble)Ĩ. Some combinations of salts may give oxidation-reduction reactions (see (11) below), but most do not.ĬaCl 2(aq) + K 2CO 3(aq) CaCO 3(s) + KCl(aq)ĪgNO 3(aq) + FeCl 3(aq) AgCl(s) + Fe(NO 3) 3(aq)Īl(NO 3) 3(aq) + Pb(C 2H 3O 2) 2(aq) no reaction To make a prediction as to whether a reaction will take place or not, you must know the solubility rules for common salts (Ebbing 4/e, page 104 lab manual, Appendix 7). Whether or not a precipitate forms depends on the exact combination of salts used. Reaction of solutions of two soluble salts with one another can give a precipitate of an insoluble salt formed by a double replacement reaction (also called a metathesis). Normally, these reactions do not involve oxidation or reduction.īaCO 3(s) + HBr(aq) BaBr 2(aq) + H 2O(l) + CO 2(g) The best-known examples of this type of reaction involve carbonates, bicarbonates, sulfides, and sulfites, but many other examples are known as well. This is especially true if the nonmetal oxide is a compound of limited solubility in water such as SO 2, CO 2, or the nitrogen oxides. In many cases, the weak acid produced is unstable and decomposes to give the oxide of a nonmetal and water (see (2) above). The cation in the salt formed as the product comes from the weak acid salt the anion in the product salt comes from the strong acid. The original salt of the weak acid may be either a pure solid or in aqueous solution. This is another example of an acid-base reaction, in addition to the ones given in (4) and (5) above. Reaction of the salt of a weak acid (that is, a compound containing the anion of a weak acid) with a strong acid produces the weak acid and a salt. Either or both of the reactants may be a pure material or in aqueous solution. This is essentially the reverse of one of the reaction types mentioned in (4) above. Ammonium salts react with metal hydroxides and oxides in an acid-base reaction to produce ammonia. The oxidation states of the anion of the acid and cation of the base normally remain unchanged. The acid and/or base may be pure solids, liquids, or gases, or in aqueous solution. The base may be a metal hydroxide, a metal oxide, or a weak base such as NH 3. The cation in the salt comes from the base the anion comes from the acid. Reaction of an acid with a base gives a salt plus water. ![]() This combination reaction occurs only if no water is present in the presence of water, the nonmetal and metal oxides react with the water to produce acid and hydroxide, respectively (as shown in (2) above), then these react as in (4) below.Ĥ. This is essentially a reaction of the O 2- or OH - in the metal compound with the molecular nonmetal oxide. Reaction of a metal oxide with a nonmetal oxide gives an oxysalt reaction of a metal hydroxide with a nonmetal oxide produces a "hydrogen" oxysalt. Metal hydroxides decompose on heating to give the metal oxide and water, and oxyacids decompose on heating to give water and the nonmetal oxide in the appropriate oxidation state.ģ. ![]() Both of these are combination reactions, and both can be reversed by heating the products. Reaction of a nonmetal oxide with water produces an oxyacid in which the nonmetal is in the same oxidation state as in the oxide you started with. Reaction of a metal oxide with water produces a metal hydroxide that is, a strong base. You may wish to balance the reactions in the handout as an exercise.)Ģ. ![]() They, like the others in this handout, are meant only to show the correct formulae for the reactants and products. ( NOTE: The above reactions are not balanced, nor were they intended to be. (exact product depends on relative amounts of I 2 and Cl 2) I 2 + Cl 2 ICl, ICl 3, or ICl 5 (covalent) Some pairs of elements may react only slowly and require heating for significant reaction to occur. If two nonmetals react, the product is a molecule with polar covalent bonds, with a formula consistent with the normal valences of the atoms involved. If a metal and a nonmetal react, the product is ionic with a formula determined by the charges on the ions the elements form. When two elements react, a combination reaction occurs (think: could any other type of reaction occur?), producing a binary compound (that is, one consisting of only two types of atoms). ![]()
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