State the precipitate's formula and colour.
Finish the equation to show the reaction between $\text{MBr}_2$ and $\text{AgNO}_3$. $\ldots\,\text{MBr}_2 + \ldots\,\text{AgNO}_3 \rightarrow \ldots$
A $0.250\,\text{g}$ sample of pure $\text{MBr}_2$ contains $8.415 \times 10^{-4}\,\text{mol}$ of $\text{MBr}_2$. Calculate the relative formula mass, $M_r$, of $\text{MBr}_2$. Use the result to identify $\text{M}$. Show your working.
Describe what is observed when chlorine gas is bubbled into an aqueous solution of $\text{MBr}_2$.
Name the type of reaction that takes place when $\text{MBr}_2$ reacts with chlorine gas.
Compound $Y$ is a pure insoluble solid that contains halide ions. One reagent is added straight to compound $Y$ to find out which halide ion is present. Identify the reagent added. State the observation that would confirm $Y$ contains bromide ions.
Three separate $1.0\,\text{g}$ samples of different magnesium salts are tested so that the anion in each sample can be identified. Explain how heating is used to identify which sample is: • $\text{MgCO}_3$ • $\text{Mg(NO}_3)_2$ • $\text{MgO}$
Complete the electron configuration for the magnesium cation in these salts. $1s^2\,\ldots$
A sample of $\text{MgCO}_3(s)$ is told apart from a sample of $\text{Mg(OH)}_2(s)$ by adding a small amount of each solid to $\text{HCl(aq)}$. State one similarity and one difference in these two reactions.