Lawrie Ryan and Roger Norris Solutions for Chapter: Redox Reactions, Exercise 1: BEFORE YOU START

Write down as many definitions of oxidation and reduction as you can.

Write an oxidation-reduction (redox) equation and explain which compound or element has been oxidised and which has been reduced.

Make a list of few oxidising agents and reducing agents.

Write down any qualitative tests for the presence of oxidising agents and reducing agents.

Balance the given chemical equation by hit and trial method:

$\mathrm{Al}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{ }{\to }{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)$

 Construct a balanced ionic equation for this reaction, using the two half equations below:

$2{{\mathrm{IO}}_3}^{-}+12{\mathrm{H}}^{+}+10{\mathrm{e}}^{-}\stackrel{ }{\to }{\mathrm{I}}_2+6{\mathrm{H}}_2\mathrm{O}$

$\mathrm{Zn}\stackrel{ }{\to }{\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}$

Write down a list of few compounds that include oxidation numbers as Roman numerals, e.g., ($\mathrm{II}$), ($\mathrm{IV}$), etc.