## Section 5.8: Classification of Reactions **Classify each of the following reactions. More than one of the five basic classifications may apply.** ### Reactions a) \( \text{W(CO)}_6 \rightarrow \text{W(CO)}_5 + \text{CO} \) b) \( \text{[Co(CN)}_5\text{]^{2-}} + \text{I}^- \rightarrow \text{[Co(CN)}_5\text{I]}^{3-} \) c) \( \text{[PdCl}_4\text{]^{2-}} + \text{C}_2\text{H}_4 \rightarrow \text{[PdCl}_3\text{(C}_2\text{H}_4)]^- + \text{Cl}^- \) d) \( \text{IrBr(CO)(PPh}_3\text{)}_2 + \text{HBr} \rightarrow \text{IrBr}_2\text{(CO)H(PPh}_3\text{)}_2 \) e) \( \text{[Co(NH}_3\text{)}_5(\text{H}_2\text{O})]^{3+} + \text{[Cr(H}_2\text{O)}_6]^{2+} \rightarrow \text{[Co(NH}_3\text{)}_5(\text{H}_2\text{O})]^{2+} + \text{[Cr(H}_2\text{O)}_6]^{3+} \) ### Analysis For each reaction, consider the types of reactions that may apply, such as: 1. **Decomposition Reaction** - A single compound breaks down into two or more simpler substances. 2. **Combination Reaction** - Two or more substances combine to form a single compound. 3. **Single Replacement Reaction** - One element replaces another element in a compound. 4. **Double Replacement Reaction** - Exchange of ions between two compounds. 5. **Redox Reaction** - Change in oxidation states between reactants and products, involving electron transfer. **Graphical or Diagram Information** No graphs or diagrams are present in this section.

Wouldn't the charge of [Ru(H2O)3(CN)3] be +1 because Br would have a charge of -1?

Circle all of the following species that exhibit geometric isomers. (a) [Rh(en)2 I2]I (b) [Pd(CO)2(CN)2](CN)2 (c) [Ni(C2O4)3]Cl4 Circle all of the following species that exhibit optical isomerism. (a) [Rh(en)2 I2]I (b) [Pd(CO)2(CN)2](CN)2 (c) [Ni(C2O4)3]Cl4

[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Explain why the addition of water changes the equilibrium position even though the concentration of water is essentially constant and normally not included in the equilibrium constant expression. What are two functions that water performs in this reaction?