Chemical Reactions 4.3Single Displacement Reactions

Last Class Identified and predicted the products of synthesis and decomposition reactions

Learning Goals We are learning to… – Identify and predict the products of single displacement reactions

Chemical Reactions Most chemical reactions can be grouped into 4 categories 1.Synthesis 2.Decomposition 3.Single displacement 4.Double displacement

Single Displacement Reaction A reaction in which an element displaces another element in a compound to produce a new compound and the displaced element. General Equation: A + BC  AC + B Example: zinc reacts with copper(II) sulphate Zn(s) + CuSO 4 (aq)  ZnSO 4 (aq) + Cu(s)

The Activity Series of Metals A ranking of the relative reactivity of metals Most reactive metals at the top; least reactive metals at the bottom. Includes H: like metals forms a cation

The Activity Series of Metals We can use the activity series to determine if a reaction will occur Elements can only displace those below it from aqueous compounds The farther away two elements are, the quicker the reaction

The Activity Series of Metals Example: magnesium metal is placed in a solution of copper(II) sulfate.

The Activity Series of Metals 1.Write the chemical formulas of the reactants 2.Identify which metal is higher on the activity series. 3.Determine if a reaction will occur. 4.Determine the products 5.Balance

The Activity Series of Metals Examples: 1.Pb(s) + Zn(NO 3 ) 2 (aq)  2.Mg(s) + AgNO 3 (aq)  3.Li(s) + H 2 SO 4 (aq)  4.Na(s) + H 2 O(l)  5.Hg(l) + H 2 SO 4 (aq) 

The Halogen Activity Series Halogens also participate in single displacement reactions, have their own activity series General equation: A + BC  BA + C Example: Cl 2 (g) + 2KI(aq)  2KCl(aq) + I 2 (aq)

The Halogen Activity Series Examples 1.Br 2 (l) + KI  2.I 2 (aq) + KCl(aq) 

Homework In class: Lab Activity After: Page 169 #2-4 and 9