[Maximum number: 1]

Manganese and nitrogen can show a range of different oxidation states.
Calculate the sum of the oxidation states of Mn and N in each row of the table.

In which row is this sum the smallest?

manganese-containing species

nitrogen-containing species

$\mathrm{MnCl}_{4}$

$\mathrm{N}_{2}$

$\mathrm{MnCO}_{3}$

$\mathrm{NO}_{2}{ }^{-}$

$\mathrm{K}_{2} \mathrm{MnO}_{4}$

$\mathrm{NH}_{4}{ }^{+}$

$\mathrm{Mn}(\mathrm{OH})_{3}$

$\mathrm{NH}_{2} \mathrm{OH}$

[Maximum number: 1]

Which compound contains two different elements with identical oxidation states?

A

HClO

B

$\mathrm{Mg}(\mathrm{OH})_{2}$

C

$\mathrm{Na}_{2} \mathrm{SO}_{4}$

D

$\mathrm{NH}_{4} \mathrm{Cl}$

[Maximum number: 1]

What is the average oxidation number of sulfur in each compound?

$\mathrm{Ca}\left(\mathrm{HSO}_{3}\right)_{2}$

$\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}$

4

2

4

6

2

6

4

[Maximum number: 1]

In which reaction does an element undergo the largest change in oxidation state?

A

$\mathrm{Cl}_{2}+2 \mathrm{OH}^{-} \rightarrow \mathrm{OCl}^{-}+\mathrm{Cl}^{-}+\mathrm{H}_{2} \mathrm{O}$

B

$3 \mathrm{Cl}_{2}+6 \mathrm{OH}^{-} \rightarrow \mathrm{ClO}_{3}^{-}+5 \mathrm{Cl}^{-}+3 \mathrm{H}_{2} \mathrm{O}$

C

$\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$

D

$3 \mathrm{MnO}_{4}{ }^{2-}+4 \mathrm{H}^{+} \rightarrow \mathrm{MnO}_{2}+2 \mathrm{MnO}_{4}^{-}+2 \mathrm{H}_{2} \mathrm{O}$

(a)

(i)

A sample of Al reacts with an excess of $\mathrm{Cl}_{2}$ .

State the oxidation number of Al in the product of the reaction.
oxidation number of Al

[ 1 ]

(b)

The oxide of silicon reacts with calcium oxide in an addition reaction to produce calcium silicate, $\mathrm{CaSiO}_{3}$ . The oxidation number of calcium in $\mathrm{CaSiO}_{3}$ is +II .

[ 1 ]

(i)

Deduce the oxidation number of silicon in calcium silicate.
oxidation number of silicon

[ 1 ]

[Maximum number: 2]

Copper is used in electrical equipment. It has a melting point of $1085^{\circ} \mathrm{C}$ .

(a)

When KI(aq) is added to $\mathrm{CuSO}_{4}(\mathrm{aq})$ the blue-coloured solution turns brown and a white precipitate of CuI(s) is seen.

The reaction between copper ions and iodide forms only two products.

[ 2 ]

(i)

Complete the equation for this reaction.

\ldots \ldots \ldots . . \mathrm{Cu}^{2+}+\ldots \ldots \ldots . . \mathrm{I}^{-} \rightarrow \ldots \ldots \ldots . . \mathrm{CuI}+\ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots . . . .

[ 1 ]

(ii)

Identify the oxidising agent in this reaction. Explain your answer in terms of electron transfer.

[ 1 ]

(a)

When magnesium is heated in air, magnesium oxide, MgO , is the major product. Smaller amounts of magnesium nitride, $\mathrm{Mg}_{3} \mathrm{~N}_{2}$ , are also made.

[ 2 ]

(i)

Calculate the oxidation number for magnesium and for the nitrogen species in $\mathrm{Mg}_{3} \mathrm{~N}_{2}$ to complete Table 1.1.

Table 1.1

[ 1 ]

(ii)

Identify the type of reaction which takes place between magnesium and nitrogen. Explain your answer.

[ 1 ]

[Maximum number: 3]

Hydrogen iodide, HI, is a colourless gas at room temperature.

(a)

HI reacts with oxygen to form iodine and water.

[ 3 ]

(i)

Construct an equation for the reaction of HI with oxygen.

[ 1 ]

(ii)

Explain, with reference to oxidation numbers, why this reaction is a redox reaction.

[ 2 ]

[Maximum number: 3]

The elements in Group 17 are known as the halogens.

(a)

Sodium chlorate(I), NaClO, oxidises dilute hydrochloric acid to form three products. The products which contain chlorine have chlorine species with oxidation number -1 or 0.

No other species changes its oxidation number during the reaction.
Use this information to complete the ionic equation.

\ldots \ldots . . \mathrm{ClO} \mathrm{O}^{-}+\ldots \ldots . \mathrm{HCl} \rightarrow \ldots \ldots \ldots . . .+\ldots \ldots \ldots . . .+\ldots \ldots . \ldots . .

[ 3 ]

(a)

Gallium is a silver-grey solid. Aluminium and gallium share many similar chemical properties.

[ 2 ]

(i)

Construct an equation for the reaction of gallium when heated in oxygen to form gallium oxide, $\mathrm{Ga}_{2} \mathrm{O}_{3}$ .

[ 1 ]

(ii)

Deduce the oxidation number of gallium in $\mathrm{Ga}_{2} \mathrm{O}_{3}$ .

[ 1 ]