IB Chemistry SL 3.1.6 Oxidation States

Practise assigning oxidation states in neutral compounds, polyatomic ions and coordination species by applying charge rules consistently. Use signed notation correctly and…

Exam points

calculate an unknown oxidation state so the signed values sum to the species charge
write oxidation states as +3 or III rather than confusing them with ionic charge notation
identify the element reduced or oxidised and state its initial and final oxidation states

[Maximum number: 2]

Chlorine undergoes many reactions.

2.67 g of manganese(IV) oxide was added to $200.0 \mathrm{~cm}^{3}$ of $2.00 \mathrm{moldm} \mathrm{m}^{-3} \mathrm{HCl}$ .

\mathrm{MnO}_{2}(\mathrm{~s})+4 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{MnCl}_{2}(\mathrm{aq})

State the oxidation state of manganese in $\mathrm{MnO}_{2}$ and $\mathrm{MnCl}_{2}$ .
$\mathrm{MnO}_{2}:$ $\mathrm{MnCl}_{2}$ :

$\mathrm{MnO}_{2}:+4$ $\mathrm{MnCl}_{2}:+2$

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3.1.6—Oxidation states question 1