A Level Chemistry 9701 Paper 11, May/June 2023

Element X has six more protons than element Y. Which statement must be correct? A Atoms of element Y are smaller than atoms of element X. B Element X has a full shell of electrons. C Element X and element Y are in the same group. D Element X and element Y are in the same period.

Which statement explains why calcium has a higher melting point than barium? A Calcium cations are smaller than barium cations and have a stronger attraction to the delocalised electrons. B The structure of calcium is partly giant molecular. C There are more delocalised electrons in calcium than in barium as it has a lower ionisation energy. D There is greater repulsion between barium atoms as they have more complete electron shells than calcium atoms.

Three statements about potassium and chlorine and their ions are listed. 1 The atomic radius of a potassium atom is greater than the atomic radius of a chlorine atom. 2 The first ionisation energy of potassium is greater than the first ionisation energy of chlorine. 3 The ionic radius of a potassium ion is greater than the ionic radius of a chloride ion. Which statements are correct? A 1 only B 2 only C 1 and 3 D 2 and 3

For which equilibrium do both of the equilibrium constants $K_c$ and $K_p$ have no units? A ${\mathrm{H}}_2(\mathrm{g})+{\mathrm{I}}_2(\mathrm{g})\rightleftharpoons 2\mathrm{H}\mathrm{I}(\mathrm{g})$ B ${\mathrm{N}}_2(\mathrm{g})+3{\mathrm{H}}_2(\mathrm{g})\rightleftharpoons 2\mathrm{N}{\mathrm{H}}_3(\mathrm{g})$ C ${\mathrm{N}}_2{\mathrm{O}}_4(\mathrm{g})\rightleftharpoons 2\mathrm{N}{\mathrm{O}}_2(\mathrm{g})$ D $\mathrm{S}{\mathrm{O}}_2(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_2(\mathrm{g})\rightleftharpoons \mathrm{S}{\mathrm{O}}_3(\mathrm{g})$

Calcium carbide, $\mathrm{C}\mathrm{a}{\mathrm{C}}_2$, reacts with water, as shown. The data below the equation show, in $\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$, the standard enthalpies of formation of the compounds involved. $$\begin{array}{ccccccc}\mathrm{C}\mathrm{a}{\mathrm{C}}_2(\mathrm{s})& +& {\mathrm{H}}_2\mathrm{O}(\mathrm{l})& \to & \mathrm{C}\mathrm{a}\mathrm{O}(\mathrm{s})& +& {\mathrm{C}}_2{\mathrm{H}}_2(\mathrm{g})\\ -60& & -286& & -635& & +228\end{array}$$ What is the standard enthalpy change of the reaction shown? A $-753\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ B $-61\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ C $+61\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ D $+753\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

In the sodium chloride lattice the number of chloride ions that surround each sodium ion is called the coordination number of the sodium ions. What are the coordination numbers of the sodium ions and the chloride ions in the sodium chloride lattice?

Histidine is an amino acid. What are the approximate bond angles 1, 2, and 3?

The Contact process takes place at a pressure between $100000\mathrm{P}\mathrm{a}$ and $200000\mathrm{P}\mathrm{a}$. A catalyst is used. Which statement is correct? A ${\mathrm{V}}_2{\mathrm{O}}_5$ catalyst is added to increase the equilibrium yield of the reaction. B Changes in pressure have no effect on the position of equilibrium. C The equilibrium yield of the reaction is very high under the conditions used. D An iron catalyst is added to increase the rate of reaction.

Bromine reacts with aqueous sodium hydroxide at $25{}^{\circ }\mathrm{C}$. reaction 1 $\mathrm{B}{\mathrm{r}}_2(\mathrm{a}\mathrm{q})+2\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}(\mathrm{a}\mathrm{q})\to \mathrm{N}\mathrm{a}\mathrm{B}\mathrm{r}(\mathrm{a}\mathrm{q})+\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{B}\mathrm{r}(\mathrm{a}\mathrm{q})+{\mathrm{H}}_2\mathrm{O}(\mathrm{l})$ The $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{B}\mathrm{r}$ formed is unstable at $25{}^{\circ }\mathrm{C}$ and reacts further. reaction 2 $3\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{B}\mathrm{r}(\mathrm{a}\mathrm{q})\to 2\mathrm{N}\mathrm{a}\mathrm{B}\mathrm{r}(\mathrm{a}\mathrm{q})+\mathrm{N}\mathrm{a}\mathrm{B}\mathrm{r}{\mathrm{O}}_3(\mathrm{a}\mathrm{q})$ Which reactions are disproportionations? A both reaction 1 and reaction 2 B neither reaction 1 nor reaction 2 C reaction 1 only D reaction 2 only

Which statement is correct? A The relative atomic mass of a ${}^{35}\mathrm{C}\mathrm{l}$ atom is 35.5. B The relative formula mass of $\mathrm{C}\mathrm{a}\mathrm{C}{\mathrm{O}}_3$ is 100.1. C The relative isotopic mass of a ${}^{24}\mathrm{M}\mathrm{g}$ atom is 24.3. D The relative molecular mass of ${\mathrm{O}}_2$ is 16.0.

Iodine and propanone react according to the following equation. $${\mathrm{I}}_2(\mathrm{a}\mathrm{q})+\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{C}{\mathrm{H}}_3(\mathrm{a}\mathrm{q})\to \mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{C}{\mathrm{H}}_2\mathrm{I}(\mathrm{a}\mathrm{q})+\mathrm{H}\mathrm{I}(\mathrm{a}\mathrm{q})$$ If the concentration of propanone is increased, keeping the total reaction volume constant, the initial rate of the reaction also increases. What could be the reason for this? A A greater proportion of collisions are successful at the higher concentration. B The particles are further apart at the higher concentration. C The particles have more energy at the higher concentration. D There are more collisions per second between particles at the higher concentration.

Four successive ionisation energies (IE) of element E are shown. Element E is in Period 3 of the Periodic Table.

In which group of the Periodic Table is E? A 14 B 15 C 16 D 17

In this question you should assume that the gas formed behaves as an ideal gas. A $1.7\mathrm{g}$ sample of $\mathrm{M}\mathrm{g}$ reacts with $50.0\mathrm{c}{\mathrm{m}}^3$ of $2.2\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{d}{\mathrm{m}}^{-3}\mathrm{H}\mathrm{C}\mathrm{l}$ at $303\mathrm{K}$ and $110400\mathrm{P}\mathrm{a}$. Which volume of gas is produced, measured under these conditions? A $1.3\mathrm{d}{\mathrm{m}}^3$ B $1.6\mathrm{d}{\mathrm{m}}^3$ C $2.5\mathrm{d}{\mathrm{m}}^3$ D $5.0\mathrm{d}{\mathrm{m}}^3$

Chlorine dioxide, $\mathrm{C}\mathrm{l}{\mathrm{O}}_2$, reacts with aqueous sodium hydroxide to produce water and a mixture of two sodium salts, $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}{\mathrm{O}}_2$ and $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}{\mathrm{O}}_3$. What is the mole ratio of $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}{\mathrm{O}}_2$ to $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}{\mathrm{O}}_3$ in the product mixture? A 1:2 B 3:5 C 1:1 D 5:3

The temperature of a sample of an inert gas is increased. What effect does this have on the number of molecules with the most probable energy and on the number of molecules with higher energy?

For which compound is there the greatest percentage loss of mass on strong heating? A anhydrous calcium carbonate B anhydrous calcium nitrate C anhydrous magnesium carbonate D anhydrous magnesium nitrate

The solids sodium chloride and sodium iodide both react with concentrated sulfuric acid at room temperature. With $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$, the products are $\mathrm{N}\mathrm{a}\mathrm{H}\mathrm{S}{\mathrm{O}}_4$ and $\mathrm{H}\mathrm{C}\mathrm{l}$. With $\mathrm{N}\mathrm{a}\mathrm{I}$, the products are $\mathrm{N}\mathrm{a}\mathrm{H}\mathrm{S}{\mathrm{O}}_4$, $\mathrm{H}\mathrm{I}$, ${\mathrm{I}}_2$, $\mathrm{S}{\mathrm{O}}_2$, ${\mathrm{H}}_2\mathrm{O}$, $\mathrm{S}$ and ${\mathrm{H}}_2\mathrm{S}$. What is the explanation for this difference in products? A Chloride ions will displace iodine from the solution. B Hydrogen chloride is more volatile than hydrogen iodide. C Iodide ions are better reducing agents than chloride ions. D Sulfuric acid is able to act as a dehydrating agent with $\mathrm{N}\mathrm{a}\mathrm{I}$.

$\mathrm{S}\mathrm{i}{\mathrm{O}}_2$ has a melting point of $1713{}^{\circ }\mathrm{C}$. It reacts with hot $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}(\mathrm{a}\mathrm{q})$ to form sodium silicate, $\mathrm{N}{\mathrm{a}}_2\mathrm{S}\mathrm{i}{\mathrm{O}}_3$, and water. No reaction occurs when $\mathrm{S}\mathrm{i}{\mathrm{O}}_2$ is added to hot ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4(\mathrm{a}\mathrm{q})$. What can be deduced from this information?

Element X has the second largest atomic radius in its period. An atom of X has three occupied electron shells only. The oxide of X is shaken with water. What could be the pH of the resulting solution? A 5 B 7 C 9 D 14

Which emission from an internal combustion engine contributes to the erosion of marble statues? A carbon monoxide B nitrogen C nitrogen dioxide D unburnt hydrocarbons

The diagram shows the melting points of eight elements with consecutive atomic numbers. Which element could be sodium? A B C D

The boiling points of $\mathrm{B}{\mathrm{r}}_2$, $\mathrm{I}\mathrm{C}\mathrm{l}$ and $\mathrm{I}\mathrm{B}\mathrm{r}$ are given in the table.

Which row explains: • why the boiling point of $\mathrm{I}\mathrm{C}\mathrm{l}$ is greater than $\mathrm{B}{\mathrm{r}}_2$ • why the boiling point of $\mathrm{I}\mathrm{B}\mathrm{r}$ is greater than $\mathrm{I}\mathrm{C}\mathrm{l}$?

A solution contains both $\mathrm{M}{\mathrm{g}}^{2+}(\mathrm{a}\mathrm{q})$ and $\mathrm{S}{\mathrm{r}}^{2+}(\mathrm{a}\mathrm{q})$ at the same concentration. The solution is divided into two equal portions. Aqueous sodium hydroxide is added dropwise to one portion. Dilute sulfuric acid is added dropwise to the other portion. Which row is correct?

Structural isomerism and stereoisomerism should be considered when answering this question. If a molecule contains two non-identical chiral carbon atoms, four optical isomers exist. How many isomers are there with: • molecular formula ${\mathrm{C}}_7{\mathrm{H}}_{14}\mathrm{O}$ and • a five-membered ring and • a tertiary alcohol group? A 4 B 5 C 9 D 13

Which reagent will react with pentan-3-ol to give a mixture of stereoisomers? A acidified potassium dichromate B concentrated sulfuric acid C ethanoic acid in the presence of a little concentrated ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ D hydrogen chloride

An organic molecule W contains 3 carbon atoms. It requires 4.5 molecules of oxygen for complete combustion. What could W be? A propane B propanoic acid C propanone D propan-1-ol

Which equation represents a reaction that proceeds through initiation, propagation and termination steps? A ${\mathrm{C}}_4{\mathrm{H}}_{10}+\mathrm{C}{\mathrm{l}}_2\to {\mathrm{C}}_4{\mathrm{H}}_9\mathrm{C}\mathrm{l}+\mathrm{H}\mathrm{C}\mathrm{l}$ B ${\mathrm{C}}_5{\mathrm{H}}_{11}\mathrm{B}\mathrm{r}+\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}\to {\mathrm{C}}_5{\mathrm{H}}_{11}\mathrm{O}\mathrm{H}+\mathrm{N}\mathrm{a}\mathrm{B}\mathrm{r}$ C ${\mathrm{C}}_6{\mathrm{H}}_{12}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{C}}_6{\mathrm{H}}_{13}\mathrm{O}\mathrm{H}$ D ${\mathrm{C}}_6{\mathrm{H}}_{13}\mathrm{C}\mathrm{H}\mathrm{O}+\mathrm{H}\mathrm{C}\mathrm{N}\to {\mathrm{C}}_6{\mathrm{H}}_{13}\mathrm{C}\mathrm{H}(\mathrm{O}\mathrm{H})\mathrm{C}\mathrm{N}$

Structural isomerism and stereoisomerism should be considered when answering this question. A set of isomeric hydrocarbons: • all contain 14.3% by mass of hydrogen • all react with bromine by addition, $0.280\mathrm{g}$ of each hydrocarbon reacting with $0.799\mathrm{g}$ of bromine. What is the maximum number of isomeric compounds in the set? A 1 B 3 C 4 D 5

Which row describes the solvent used and type of reaction occurring when bromoethane reacts with $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}$ to form ethene?

Which row describes the type of reaction that occurs when propan-1-ol reacts to form the named carbon-containing product?

Which statement describes what happens when 2-chloro-2-methylpropane is warmed with $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}(\mathrm{a}\mathrm{q})$? A This secondary halogenoalkane reacts by a mixture of an ${\mathrm{S}}_{\mathrm{N}}1$ and an ${\mathrm{S}}_{\mathrm{N}}2$ mechanism. B This secondary halogenoalkane reacts only by an ${\mathrm{S}}_{\mathrm{N}}2$ mechanism. C This tertiary halogenoalkane reacts mostly by an ${\mathrm{S}}_{\mathrm{N}}1$ mechanism. D This tertiary halogenoalkane does not react with hydroxide ions under these conditions.

How many structurally isomeric secondary alcohols are there with the molecular formula ${\mathrm{C}}_5{\mathrm{H}}_{12}\mathrm{O}$? A 1 B 2 C 3 D 4

Which reagent: • can confirm the presence of a carbonyl group in an organic compound • does not distinguish between aldehydes and ketones? A acidified ${\mathrm{K}}_2\mathrm{C}{\mathrm{r}}_2{\mathrm{O}}_7$ B 2,4-DNPH reagent C Fehling’s reagent D $\mathrm{L}\mathrm{i}\mathrm{A}\mathrm{l}{\mathrm{H}}_4$

Which compound gives a positive test with alkaline aqueous iodine and does not show optical isomerism? A $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{O}\mathrm{H}$ B $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}\mathrm{H}(\mathrm{O}\mathrm{H})\mathrm{C}\mathrm{H}\mathrm{O}$ C $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{O}\mathrm{C}\mathrm{H}(\mathrm{O}\mathrm{H})\mathrm{C}{\mathrm{H}}_3$ D $(\mathrm{C}{\mathrm{H}}_3{)}_2\mathrm{C}(\mathrm{O}\mathrm{H})\mathrm{C}\mathrm{H}\mathrm{O}$

Two samples of compound X were treated separately with different reagents which were added in excess. The products of these two reactions are shown. Which reagents could be used for reaction 1 and reaction 2?

Which method could produce butanoic acid? A an acid–base reaction involving $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{O}}_2\mathrm{N}\mathrm{a}$ B the hydrolysis of $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{C}\mathrm{N}$ C the acidic hydrolysis of $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}\mathrm{O}\mathrm{O}\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_3$ D the oxidation of $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{O}\mathrm{H}$

Which ester may be hydrolysed to produce two products, one of which may be reduced to the other? A $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{O}}_2\mathrm{C}{\mathrm{H}}_3$ B $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{H}(\mathrm{C}{\mathrm{H}}_3)\mathrm{C}{\mathrm{O}}_2\mathrm{C}{\mathrm{H}}_2\mathrm{C}\mathrm{H}(\mathrm{C}{\mathrm{H}}_3{)}_2$ C $\mathrm{C}{\mathrm{H}}_3\mathrm{C}{\mathrm{H}}_2\mathrm{C}{\mathrm{O}}_2\mathrm{C}\mathrm{H}(\mathrm{C}{\mathrm{H}}_3{)}_2$ D $(\mathrm{C}{\mathrm{H}}_3{)}_2\mathrm{C}\mathrm{H}\mathrm{C}{\mathrm{O}}_2\mathrm{C}\mathrm{H}(\mathrm{C}{\mathrm{H}}_3{)}_2$

Two compounds, X and Y, are mixed and a little concentrated ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ is added. Ester Z is found in the resulting mixture of products. Which two compounds could be X and Y?

The diagram shows a section of a polymer molecule. $$-\mathrm{C}{\mathrm{H}}_2-\mathrm{C}\mathrm{H}=\mathrm{C}\mathrm{H}-\mathrm{C}{\mathrm{H}}_2-\mathrm{C}{\mathrm{H}}_2-\mathrm{C}\mathrm{H}=\mathrm{C}\mathrm{H}-\mathrm{C}{\mathrm{H}}_2-$$ Which monomer will produce this polymer? A $\mathrm{C}{\mathrm{H}}_2=\mathrm{C}{\mathrm{H}}_2$ B $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{H}=\mathrm{C}{\mathrm{H}}_2$ C $\mathrm{C}{\mathrm{H}}_3\mathrm{C}\mathrm{H}=\mathrm{C}\mathrm{H}\mathrm{C}{\mathrm{H}}_3$ D $\mathrm{C}{\mathrm{H}}_2=\mathrm{C}\mathrm{H}-\mathrm{C}\mathrm{H}=\mathrm{C}{\mathrm{H}}_2$

There are two naturally occuring isotopes of bromine. One isotope has 44 neutrons. The other isotope has 46 neutrons. Ignoring fragments, how many peaks are there in the mass spectrum of tribromomethane, ${}^{12}{\mathrm{C}}^1\mathrm{H}\mathrm{B}{\mathrm{r}}_3$? A 2 B 3 C 4 D 6