Eduqas A-Level Chemistry: Inorganic Chemistry overview quiz quiz

Hydrochloric acid is far too weak an acid to provide enough hydrogen ions here

Sulfuric acid is a stronger oxidising agent than the manganate(VII)

Chloride ions would be oxidised by the manganate(VII), giving a false titre

Hydrochloric acid would reduce the iron(II) ions back to the metal

At the very start, before any thiosulfate is added from the burette

After the end point has already been clearly reached

Starch is not used at any stage in this titration

Near the end point, when the solution is pale straw

$-1$ and $+1$

$0$ and $-1$

$+1$ and $+5$

$-1$ and $+5$

It increases, because the atoms get larger and gain electrons more easily

It decreases, because the atom gains an electron less readily

It stays roughly constant all the way down the group

It increases, because the shielding of the outer shell decreases

Chloride

Iodide

Bromide

Fluoride

$\text{Br}_2 + 2\text{Cl}^- \rightarrow 2\text{Br}^- + \text{Cl}_2$

$\text{Cl}_2 + \text{Br}_2 \rightarrow 2\text{BrCl}$

$\text{Cl}^- + \text{Br}^- \rightarrow \text{ClBr}^{2-}$

$\text{Cl}_2 + 2\text{Br}^- \rightarrow 2\text{Cl}^- + \text{Br}_2$

Always forming colourless 2+ ions only

Forming coloured ions in aqueous solution

Showing several different variable oxidation states

Acting as a catalyst in many industrial reactions

The water ligands are themselves intrinsically blue and they pass that colour straight on to the surrounding aqueous solution itself

An electron is promoted across split d orbitals (a d-d transition), and the complementary colour of the absorbed light is seen

Copper has a completely full 3d sub-shell, and full sub-shells always absorb red light and transmit a blue colour

The complex adopts a tetrahedral shape, and all tetrahedral copper complexes are blue because of their symmetry

Redox, in which copper changes oxidation state

Disproportionation of the copper(II) ion into two states

Ligand substitution

Precipitation of an insoluble copper salt

$0.0160\ \text{mol dm}^{-3}$

$0.400\ \text{mol dm}^{-3}$

$0.0400\ \text{mol dm}^{-3}$

$0.0800\ \text{mol dm}^{-3}$