Chem 101 Classifying Chemical Reactions Lectures 17 and 18
Classifying Chemical Reactions Chemical reactions can be divided into five categories: I. Combination or Synthesis Reactions II. Decomposition Reactions III. Single-Replacement Reactions IV.Double-Replacement Reactions V. Neutralization Reactions VI. Combustion Reactions
Combination Reactions (or Synthesis Reactions) Combination reaction, two simpler substances are combined into a more complex compound. Let s take a look at 3 types of combination reactions: metal with oxygen nonmetal with oxygen metal and a nonmetal
Reactions of Metals and Oxygen When a metal is heated with oxygen gas, a metal oxide is produced. metal + oxygen gas metal oxide Example: Magnesium metal produces magnesium oxide. 2 Mg(s) + O 2 (g) 2 MgO(s) Example: Iron metal reacts with oxygen to produce iron(iii) oxide: 4 Fe(s) + 3 O 2 (g) 2 Fe 2 O 3 (s)
Reactions of Nonmetals and Oxygen Oxygen and a nonmetal react to produce a nonmetal oxide. nonmetal + oxygen gas nonmetal oxide Example: Phosphorous produces tetraphosphorous decaoxide. P 4 (s) + 5 O 2 (g) P 4 O 10 (s) Example: Sulfur reacts with oxygen to produce sulfur dioxide gas: S(s) + O 2 (g) SO 2 (g)
Metal + Nonmetal Reactions A metal and a nonmetal react in a combination reaction to give a binary ionic compound. metal + nonmetal binary ionic compound Example: Sodium reacts with chlorine gas to produce sodium chloride: 2 Na(s) + Cl 2 (g) 2 NaCl(s) When a main group metal reacts with a nonmetal, the formula of the ionic compound is predictable. If the compound contains a transition metal, the formula is not predictable.
Decomposition Reactions Decomposition reaction, a single compound is broken down into simpler substances. Heat or light is usually starts a decomposition reaction. Ionic compounds containing oxygen often decompose into a metal and oxygen gas. Example: Heating solid mercury(ii) oxide produces mercury metal and oxygen gas: 2 HgO(s) 2 Hg(l) + O 2 (g)
Carbonate Decomposition Metal hydrogen carbonates decompose to give a metal carbonate, water, and carbon dioxide. Example: nickel(ii) hydrogen carbonate decomposes: Ni(HCO 3 ) 2 (s) NiCO 3 (s) + H 2 O(l) + CO 2 (g) Metal carbonates decompose to give a metal oxide and carbon dioxide gas: Example: calcium carbonate decomposes: CaCO 3 (s) CaO(s) + CO 2 (g)
Activity Series Activity series: A sequence of metals is arranged according to their ability to undergo reaction. When a metal (active) undergoes a replacement reaction, it displaces another metal (less active) from a compound or aqueous solution.
Activity Series Most reactive metals appear first in the activity series. Least reactive metals appear last in the activity series. The relative activity series: K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au
Single-Replacement Reactions Single-replacement reaction, a more active metal displaces a less active metal in a compound. If a metal precedes another in the activity series, it will undergo a single-replacement reaction: Fe(s) + CuSO 4 (aq) FeSO 4 (aq) + Cu(s) If a metal follows another in the activity series, no reaction will occur: Ni(s) + CdSO 4 (aq) NR
Aqueous Acid Displacements Metals that precede (H) in the activity series react with acids and those that follow (H) do not react with acids. More active metals react with acid to produce hydrogen gas and an ionic compound: Fe(s) + 2 HCl(aq) FeCl 2 (aq) + H 2 (g) Metals less active than (H) show no reaction: Au(s) + H 2 SO 4 (aq) NR
Active Metals Active metals, a few metals that are active enough to react directly with water. The active metals are: Li, Na, K, Rb, Cs, Ca, Sr, and Ba. Active metals react with water to produce a metal hydroxide and hydrogen gas: 2 Na(s) + 2 H 2 O(l) 2 NaOH(aq) + H 2 (g) Ba(s) + 2 H 2 O(l) Ba(OH) 2 (aq) + H 2 (g)
Solubility Rules Solubility rules are used to predict if a compound will be soluble in water.
Double-Replacement Reactions Double replacement reaction, two ionic compounds in aqueous solution switch anions and produce two new compounds. AX + BZ AZ + BX If either AZ or BX is an insoluble compound, a precipitate will appear and there is a chemical reaction. If no precipitate is formed, there is no reaction.
Double-Replacement Reactions Aqueous barium chloride reacts with aqueous potassium chromate: BaCl 2 (aq) + K 2 CrO 4 (aq) BaCrO 4 (s) + 2 KCl(aq) This is a double replacement reaction, since BaCrO 4 is insoluble, from the solubility rules. Aqueous sodium chloride reacts with aqueous lithium nitrate: NaCl(aq) + LiNO 3 (aq) NaNO 3 (aq) + LiCl(aq) Both NaNO 3 and LiCl are soluble, so there is no reaction.
Neutralization Reactions Neutralization reaction, is the reaction of an acid and a base. HX + BOH BX + HOH A neutralization reaction produces a salt and water. H 2 SO 4 (aq) + 2 KOH(aq) K 2 SO 4 (aq) + 2 H 2 O(l)
Review 4 ways to understand if a chemical reaction occurred: 1. A gas is detected. 2. A precipitate is formed. 3. A permanent color change is seen. 4. Heat or light is given off. An exothermic reaction gives off heat and an endothermic reaction absorbs heat.
Review There are 7 elements that exist as diatomic molecules: H 2, N 2, O 2, F 2, Cl 2, Br 2, and I 2 When we balance a chemical equation, the number of each type of atom must be the same on both the product and reactant sides of the equation. We use coefficients in front of compounds to balance chemical reactions.
Review In combination reactions, two or more smaller molecules are combined into a more complex molecule. In a decomposition reaction, a molecule breaks apart into two or more simpler molecules. In a single-replacement reaction, a more active metal displaces a less active metal according to the activity series.
Review In a double-replacement reaction, two aqueous solutions produce a precipitate of an insoluble compound. The insoluble compound can be predicted based on the solubility rules. In a neutralization reaction, and acid and a base react to produce a salt and water.