Define transition element.
State how the melting point and density of iron compare with those of calcium.
Define standard cell potential, $E^{\circ}_{\text{cell}}$.
Draw a fully labelled diagram of the equipment that may be used to measure the cell potential of a cell made from a $\text{Cu(II)}/\text{Cu}$ electrode and an $\text{Fe(III)}/\text{Fe(II)}$ electrode. Include all necessary reactants.
The reaction between $\text{S}_2\text{O}_8^{2-}(aq)$ and $\text{I}^-(aq)$ is sped up by adding a few drops of $\text{Fe}^{3+}(aq)$. Use equations to demonstrate the catalytic function of $\text{Fe}^{3+}$ in this reaction.
$\text{Fe}^{3+}(aq)$ can oxidise $\text{I}^-(aq)$, whereas $[\text{Fe(CN)}_6]^{3-}(aq)$ cannot oxidise $\text{I}^-(aq)$. Use $E^{\circ}$ values to account for these observations.
When aqueous solutions of $\text{S}_2\text{O}_8^{2-}$ and tartrate ions are mixed the reaction proceeds very slowly. However, this reaction proceeds quickly in the presence of an $\text{Fe}^{3+}(aq)$ catalyst. Suggest why this reaction is slow without the $\text{Fe}^{3+}$ catalyst.
Use the overall equation to work out the half-equation for the oxidation of tartrate ions, $\text{C}_4\text{H}_4\text{O}_6^{2-}$, to carbon dioxide, $\text{CO}_2$, and methanoate ions, $\text{HCO}_2^-$.
Complete the table below to show the structures of the organic products formed when tartaric acid reacts separately with each reagent. Identify the type of reaction in each case.
Tartaric acid reacts with the amine 1-phenylethylamine, $\text{C}_6\text{H}_5\text{CH(NH}_2)\text{CH}_3$, to produce an ionic salt. Draw the structure of the salt formed in this reaction. Include the charges on the ions.