A Level Chemistry 9701 Paper 21, May/June 2023

Complete Table 1.1. Table 1.1

Identify the sub-shell in an atom of Te that contains electrons with the lowest energy.

Construct an equation to represent the first ionisation energy of Te.

The radius of Te ions decreases after each successive ionisation. State two factors that are responsible for the increase in the first six ionisation energies of Te.

Sketch a graph in Fig. 1.1 to show the trend in the first seven ionisation energies of Te.

Te reacts with ${\mathrm{F}}_2$ at $150{}^{\circ }\mathrm{C}$ to form ${\mathrm{T}\mathrm{e}\mathrm{F}}_x$. Molecules of ${\mathrm{T}\mathrm{e}\mathrm{F}}_x$ are octahedral with bond angles of ${90}^{\circ }$. Explain why ${\mathrm{T}\mathrm{e}\mathrm{F}}_x$ is octahedral with bond angles of ${90}^{\circ }$.

${\mathrm{T}\mathrm{e}\mathrm{F}}_x$ reacts with water to form tellurium hydroxide and $\mathrm{H}\mathrm{F}$. The oxidation number of tellurium does not change during this reaction. Construct an equation for the reaction of ${\mathrm{T}\mathrm{e}\mathrm{F}}_x$ with water.

Name the type of reaction that occurs when ${\mathrm{T}\mathrm{e}\mathrm{F}}_x$ reacts with water.

Define enthalpy change of neutralisation, $\mathrm{\Delta }{H}_{\text{neut}}$.

An experiment is carried out to calculate $\mathrm{\Delta }{H}_{\text{neut}}$ for the reaction between $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}(\mathrm{a}\mathrm{q})$ and ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})$. $100{\mathrm{c}\mathrm{m}}^3$ of $1.00\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}(\mathrm{a}\mathrm{q})$ is added to $75{\mathrm{c}\mathrm{m}}^3$ of $1.00\mathrm{m}\mathrm{o}\mathrm{l}{\mathrm{d}\mathrm{m}}^{-3}{\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})$ in a polystyrene cup and stirred. Results from the experiment are shown in Table 2.1. Table 2.1

Use equation 1 to calculate the amount, in $\mathrm{m}\mathrm{o}\mathrm{l}$, of ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})$ that is neutralised in the experiment. amount of ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})$ neutralised = .............................. $\mathrm{m}\mathrm{o}\mathrm{l}$

Calculate $\mathrm{\Delta }{H}_{\text{neut}}$ using the results in Table 2.1. Include units in your answer. Assume that: • the specific heat capacity of the final solution is $4.18\mathrm{J}{\mathrm{g}}^{-1}{\mathrm{K}}^{-1}$ • $1.00{\mathrm{c}\mathrm{m}}^3$ of the final solution has a mass of $1.00\mathrm{g}$ • there is no heat loss to the surroundings • full dissociation of ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})$ occurs • the experiment takes place at constant pressure. Show your working. $\mathrm{\Delta }{H}_{\text{neut}}=$ .............................. units ..............................

Complete the equation for the reaction that occurs when a solution of $\mathrm{B}\mathrm{a}(\mathrm{O}\mathrm{H}{)}_2$ is added to aqueous sulfuric acid. Include state symbols. ....... ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4(\mathrm{a}\mathrm{q})+$ ....... $\mathrm{B}\mathrm{a}(\mathrm{O}\mathrm{H}{)}_2(\mathrm{a}\mathrm{q})\to$ ........................................................................................

Suggest why the enthalpy change of neutralisation cannot be determined using the addition of dilute sulfuric acid to aqueous barium hydroxide.

Chlorine reacts with silicon to form silicon(IV) chloride. Describe the appearance of silicon(IV) chloride at room temperature and pressure. State its structure and bonding. appearance ............................................................................................................................... structure and bonding ...............................................................................................................

Samples of magnesium chloride and phosphorus(V) chloride are added to separate beakers of cold water. Complete Table 3.1. Ignore temperature changes when considering observations for these reactions. Table 3.1

State the reagent and conditions required for the formation of sodium chlorate(V) from ${\mathrm{C}\mathrm{l}}_2(\mathrm{g})$.

Explain why the reaction in (c)(i) is described as a disproportionation reaction. Your answer should refer to relevant species and their oxidation numbers.

Chlorine reacts with methane in a series of reactions to produce chloroalkanes. State the conditions required for chlorine to react with methane.

One of the products of the reaction is ${\mathrm{C}\mathrm{H}}_2{\mathrm{C}\mathrm{l}}_2$ which reacts further to produce ${\mathrm{C}\mathrm{H}\mathrm{C}\mathrm{l}}_3$. Complete Table 3.2 to show details of the mechanism that forms ${\mathrm{C}\mathrm{H}\mathrm{C}\mathrm{l}}_3$ from ${\mathrm{C}\mathrm{H}}_2{\mathrm{C}\mathrm{l}}_2$. Table 3.2

${\mathrm{C}\mathrm{H}\mathrm{C}\mathrm{l}}_3$ and $\mathrm{H}\mathrm{F}$ are used to form ${\mathrm{C}\mathrm{H}\mathrm{C}\mathrm{l}\mathrm{F}}_2$ in a substitution reaction. Construct an equation for this reaction.

$\mathbf{X}$ is a product of the substitution reaction that occurs when ${\mathrm{C}\mathrm{H}\mathrm{C}\mathrm{l}\mathrm{F}}_2$ reacts with ${\mathrm{B}\mathrm{r}}_2$. There is only one naturally occurring isotope of fluorine, ${}^{19}\mathrm{F}$. The mass spectrum of $\mathbf{X}$ shows molecular ion peaks at $m\mathrm{/}e=164$, $166$ and $168$. Complete Table 3.3 to show all the molecular ions responsible for each peak. Table 3.3

$\mathbf{V}$ reacts with an excess of ${\mathrm{L}\mathrm{i}\mathrm{A}\mathrm{l}\mathrm{H}}_4$ to form $\mathbf{W}$. Draw the structure of $\mathbf{W}$ in the box.

Identify the role of ${\mathrm{L}\mathrm{i}\mathrm{A}\mathrm{l}\mathrm{H}}_4$ in the reaction with $\mathbf{V}$.

$\mathbf{V}$ reacts to form $\mathbf{Z}$ in a single reaction, as shown in Fig. 4.2. Fig. 4.2 Suggest the reagent and conditions needed to form $\mathbf{Z}$ from $\mathbf{V}$.

Deduce the empirical formula of $\mathbf{Z}$.

Complete Table 4.1 to show the number of ${\mathrm{s}\mathrm{p}}^2$ and ${\mathrm{s}\mathrm{p}}^3$ hybridised carbon atoms that are present in a molecule of $\mathbf{V}$. Table 4.1

$\mathbf{Q}$ contains the elements carbon, hydrogen and oxygen only. It is a saturated molecule with no branching in its carbon backbone. $\mathbf{Q}$ contains only one functional group. The relative molecular mass of $\mathbf{Q}$ is $88$. No effervescence is seen when ${\mathrm{N}\mathrm{a}}_2{\mathrm{C}\mathrm{O}}_3$ is added to $\mathbf{Q}$. Effervescence is seen when sodium is added to $\mathbf{Q}$. $\mathbf{Q}$ reacts with alkaline ${\mathrm{I}}_2(\mathrm{a}\mathrm{q})$ to form a yellow precipitate. Draw the structure of $\mathbf{Q}$ in the box.

Molecule $\mathbf{M}$ is present in petrol, a fuel used in cars. $\mathbf{M}$ is a saturated, non-cyclic hydrocarbon. $\mathbf{M}$ contains eight carbon atoms. Construct an equation for the complete combustion of $\mathbf{M}$.

Describe how the composition of products differs when incomplete combustion of $\mathbf{M}$ occurs.

When petrol is burned in an internal combustion engine, oxides of nitrogen are released into the atmosphere. Oxides of nitrogen are responsible for the formation of acid rain. Suggest the conditions required for the production of oxides of nitrogen during combustion of $\mathbf{M}$ in an internal combustion engine. Use an appropriate equation in your answer.

Describe how acid rain is formed in the atmosphere in the presence of oxides of nitrogen and ${\mathrm{S}\mathrm{O}}_2$. Identify the role of the oxides of nitrogen in this process. Include all relevant equations.

State one other type of air pollution that is caused by the production of oxides of nitrogen in an internal combustion engine.

Biodiesel $\mathbf{T}$ is a fuel made from vegetable oil $\mathbf{R}$. Fig. 5.1 shows the production of $\mathbf{T}$ from $\mathbf{R}$ in a two-step process. Fig. 5.1 In step 1 all three ester groups in $\mathbf{R}$ react. Suggest a suitable reagent and conditions for step 1.

Draw the structural formula of $\mathbf{J}$ in the box in Fig. 5.1.

Name the type of reaction that occurs in step 2.

Name organic reagent $\mathbf{G}$ used in step 2.

$\mathbf{L}$ is called decanoic acid. Use systematic nomenclature to deduce the name of $\mathbf{T}$.