Lawrie Ryan and Roger Norris Solutions for Chapter: Transition Elements, Exercise 12: EXAM-STYLE QUESTIONS

Define the term complex ion.

Use the subshell notation $\left(1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6, \mathrm{etc}\right)$ to give the electronic configuration of an $\mathrm{Fe}$ atom.

Use the subshell notation $\left(1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6, \mathrm{etc}\right)$ to give the electronic configuration of an ${\mathrm{Co}}^{2+}$ atom.

Use the subshell notation $\left(1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6, \mathrm{etc}\right)$ to give the electronic configuration of an ${\mathrm{Ti}}^{3+}$ atom.

Give the formulae of two iron compounds in which iron has different oxidation states. Give the oxidation states of the iron in each compound.

Explain why complexes of iron compounds are coloured.

Write balanced ionic equations and describe the observations for the reaction that occur when sodium hydroxide solution is added to a solution containing ${\left[\mathrm{Cu}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+} \left(\mathrm{aq}\right)$

Write balanced ionic equations and describe the observations for the reaction that occur when excess concentrated ammonia solution is added to a solution containing ${\left[\mathrm{Cu}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]}^{2+} \left(\mathrm{aq}\right)$.