AS & A Level Chemistry - 9701 Paper 4 2017 Winter Zone 1

The compound nitrosyl bromide, NOBr, can be formed by the reaction shown.

$$2\text{NO} + \text{Br}_2 \rightleftharpoons 2\text{NOBr}$$

(a) Using oxidation numbers, explain why this reaction is a redox reaction.
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[2]

(b) Nitrosyl bromide contains a trivalent nitrogen atom.

Draw the ‘dot-and-cross’ diagram for NOBr. Show outer electrons only.

[Image: Dot-and-cross diagram]
[2]

(c) The rate of the reaction was measured at various concentrations of the two reactants, NO and Br₂, and the following results were obtained.

[Table_1]

(a) The table lists values of solubility products, $K_{sp}$, of some Group 2 carbonates.
[Table_1]
Use the data in the table to describe the trend in the solubility of the Group 2 carbonates down the group.
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(b) (i) Write an equation to show the equilibrium for the solubility product for MgCO$_3$. Include state symbols.
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(ii) With reference to your equation in (i), suggest what is observed when a few cm$^3$ of concentrated Na$_2$CO$_3$(aq) are added to a saturated solution of MgCO$_3$. Explain your answer.
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(c) Use the data in the table to calculate the solubility of MgCO$_3$ in water at 298 K, in g dm$^{-3}$.
solubility of MgCO$_3$ = ............................. g dm$^{-3}$ [2]

(d) (i) Magnesium nitrate decomposes at a lower temperature than barium nitrate.
Explain why.
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(ii) A sample of barium nitrate was heated strongly until no further change occurred. A white solid was formed.
Write an equation for the action of heat on barium nitrate.
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(iii) When water was added to the white solid produced in (d)(ii), an alkaline solution was produced. Adding sulfuric acid to this solution produced a white precipitate.
Write equations to explain these observations.
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(a) Define the term \textit{standard cell potential}.
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(b) (i) Draw a fully labelled diagram of the experimental set-up you could use to measure the
standard electrode potential of the $\text{Pb}^{2+}(\text{aq})/\text{Pb}(\text{s})$ electrode. Include the necessary chemicals.
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(ii) The $E^\circ$ for a $\text{Pb}^{2+}(\text{aq})/\text{Pb}(\text{s})$ electrode is –0.13 V.
Suggest how the $E$ for this electrode would differ from its $E^\circ$ value if the concentration of $\text{Pb}^{2+}(\text{aq})$ ions is reduced. Indicate this by placing a tick (✓) in the appropriate box in the table.
[Table_1]

Explain your answer.
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(c) Car batteries are made up of rechargeable lead-acid cells. Each cell consists of a negative
electrode made of $\text{Pb}$ metal and a positive electrode made of $\text{PbO}_2$. The electrolyte is $\text{H}_2\text{SO}_4(\text{aq})$.
When a lead-acid cell is in use, $\text{Pb}^{2+}$ ions are precipitated out as $\text{PbSO}_4(\text{s})$ at the negative electrode.
$$\text{Pb}(\text{s}) + \text{SO}_4^{2-}(\text{aq}) \rightarrow \text{PbSO}_4(\text{s}) + 2\text{e}^-$$
(i) Calculate the mass of $\text{Pb}$ that is converted to $\text{PbSO}_4$ when a current of 0.40 A is delivered by the cell for 80 minutes.
mass of Pb = ...................... g [2]
(ii) Complete the half-equation for the reaction taking place at the positive electrode.
$\text{PbO}_2(\text{s}) + \text{SO}_4^{2-}(\text{aq}) + ............. + ............. \rightarrow \text{PbSO}_4(\text{s}) + .............$ [1]

(d) The diagrams show how the voltage across two different cells changes with time when each cell is used to provide an electric current.
Suggest a reason why:
- the voltage of the lead-acid cell changes after several hours,
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- the voltage of the fuel cell remains constant.
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(a) Describe and explain how the density and melting point of cobalt compare to those of calcium.
density of cobalt .....................................................................................................................
explanation ...........................................................................................................................
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melting point of cobalt ..............................................................................................................
explanation ............................................................................................................................
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(b) Transition metals can form complexes.
What is meant by the term \textit{transition metal complex}?
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(c) (i) Cobalt can form the compounds $[ \text{Co(NH}_3)_5\text{Br}]\text{SO}_4$ and $[ \text{Co(NH}_3)_5\text{SO}_4]\text{Br}$. These two compounds are structural isomers.
Define the term \textit{structural isomer}.
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(ii) Draw a three-dimensional diagram to show the structure of the ion $[ \text{Co(NH}_3)_5\text{Br}]^{2+}$. Name its shape.

Compound P contains several functional groups.
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(a) Name the functional groups present in P.
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(b) Compound P can be polymerised.
Draw a section of the polymer of P showing two repeat units. Name the type of polymerisation.
type of polymerisation .................................................................................................................. [2]
(c) Complete the following table to show the structures of the products formed and the type of organic reaction when P reacts with the four reagents.
| reagent | structure(s) of product(s) | type of organic reaction |
|---|---|---|
| excess Br₂(aq) | | |
| excess hot, concentrated, acidified MnO₄^-(aq) | | |
| excess hot HCl(aq) | | |
| excess H₂/Pt catalyst | | |
[8]

(a) 4-nitromethylbenzene can be prepared via an electrophilic substitution reaction as shown.

(i) This reaction also forms an isomer of 4-nitromethylbenzene as a by-product. Draw the structure of this by-product. [1]
(ii) Write an equation for the reaction between HNO₃ and H₂SO₄ that forms the electrophile for this reaction. [1]
(iii) Describe how the structure and bonding of the six-membered ring in intermediate T differs from that in methylbenzene. [3]

(b) Benzocaine is used as a local anaesthetic. It can be synthesised from 4-nitromethylbenzene by the route shown.

(i) Give the systematic name of compound W. [1]
(ii) Suggest the reagents and conditions for steps 1–5.
step 1 ............................................................................................................
step 2 ............................................................................................................
step 3 ............................................................................................................
step 4 ............................................................................................................
step 5 ............................................................................................................ [6]
(c) Suggest how the basicity of benzocaine would compare to that of ethylamine. Explain your answer. [2]

(d) A sample of benzocaine, shown below, was analysed by proton NMR and carbon-13 NMR spectroscopy.

(i) Predict the number of peaks that would be seen in the carbon-13 NMR spectrum. [1]
(ii) Benzocaine was dissolved in CDCl₃ and the proton NMR spectrum of this solution was recorded.

Suggest why CDCl₃ and not CHCl₃ is used as the solvent when obtaining a proton NMR spectrum. [1]
(iii) Use the Data Booklet and the spectrum in (d)(ii) to complete the table for the proton NMR spectrum of benzocaine. The actual chemical shifts, δ, for the four absorptions have been added.
[Table_1]
δ / ppm | group responsible for the peak | number of ¹H atoms responsible for the peak | splitting pattern
1.2 | | |
3.5 | | |
5.5 | | |
7.1–7.4 | | | multiplet [4]
(iv) Explain the splitting pattern for the absorption at δ1.2 ppm. [1]
(v) The proton NMR spectrum of benzocaine dissolved in D₂O was recorded. Suggest how this spectrum would differ from the spectrum in (d)(ii). Explain your answer. [1]

(e) Benzocaine can also be used to synthesise the dyestuff S by the following route.

(i) Suggest the reagents used for step 1. [1]
(ii) Suggest structures for compounds R and S and draw them in the boxes. [2]

(a) Complete the following electronic structures.

• the iron atom, Fe 1s²2s²2p⁶ ...................................

• the iron(III) ion, Fe³⁺ 1s²2s²2p⁶ ....................................

(b) Solutions of iron(III) salts are acidic due to the equilibrium shown.

$[\text{Fe(H}_2\text{O)}_6]^{3+}(\text{aq}) \rightleftharpoons [\text{Fe(H}_2\text{O)}_5(\text{OH})]^{2+}(\text{aq}) + \text{H}^+(\text{aq}) \quad K_a = 8.9 \times 10^{-4} \text{mol dm}^{-3}$

Calculate the pH of a $0.25 \text{mol dm}^{-3}$ FeCl₃ solution.

pH = ................................

(c) The table shows numerical values of the stability constants for the following equilibrium where M can be one of the metal ions listed and L one of the ligands which replaces one H₂O molecule.

$[\text{M(H}_2\text{O)}_6]^{n+}(\text{aq}) + \text{L}^-(\text{aq}) \rightleftharpoons [\text{M(H}_2\text{O)}_5\text{L}]^{(n-1)+}(\text{aq}) + \text{H}_2\text{O}(l)$

[Table_1]

(i) What is meant by the term stability constant, $K_{stab}$?

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(ii) Use the data in the table to predict the formula of the complex formed in the greatest amount when

• a solution containing equal concentrations of both F^- and SCN^- ions is added to Fe³⁺(aq),

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• a solution containing equal concentrations of both Fe³⁺ and Hg²⁺ ions is added to Cl^-(aq).

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(d) The complex [Fe(ed^2-)₂Cl₂]^3- can be formed according to the equation shown.

$[\text{Fe(H}_2\text{O)}_4\text{Cl}_2]^+(\text{aq}) + 2\text{ed}^{2-}(\text{aq}) \rightleftharpoons [\text{Fe(ed)}_2\text{Cl}_2]^{3-}(\text{aq}) + 4\text{H}_2\text{O}(l)$

Write the expression for the equilibrium constant, $K_{stab}$, and state its units.

$K_{stab} = $ ................................ units ................................

(e) [Fe(ed^2-)₂Cl₂]^3- shows geometrical and optical isomerism.

(i) Complete the three-dimensional diagrams to show the three stereoisomers of [Fe(ed^2-)₂Cl₂]^3-.

You may use -O O- to represent ed^2-.



(ii) Give the letters of two isomers of [Fe(ed^2-)₂Cl₂]^3- which are geometrical isomers of each other.

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(iii) Give the letters of the two isomers of [Fe(ed^2-)₂Cl₂]^3- which show optical isomerism.

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(iv) Give the letter of the isomer which has no dipole moment.

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