Chemistry Paper 2 November 2022

1. Aatomisation
2. Bhydration
3. Creduction
4. Dionisation

1. A$1s^22s^22p^4$
2. B$1s^22s^22p^6$
3. C$1s^22s^22p^63s^2$
4. D$1s^22s^22p^63s^23p^6$

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1. A79.0
2. B79.9
3. C80.0
4. D81.0

1. Atowards the positive plate instead, because helium is a noble gas and does not respond to the field.
2. Bless, because its larger mass gives it a smaller charge-to-mass ratio despite its greater charge.
3. Cmore, because its charge is twice as great, and charge dominates completely over mass in electric deflection.
4. Dby exactly the same amount, since both ions carry an overall positive charge and are accelerated identically.

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1. Aat every single electron removed, rising by a constant amount each time.
2. Bonly after all ten electrons have been removed, as a single final jump.
3. Cbetween removal of the electrons in the outer (n=2) shell and those in the inner (n=1) shell.
4. Dimmediately after the very first electron is removed from the ion, before any other large jumps occur at all.

1. Asilver(I) does not form complexes with nitrogen-donor ligands such as ammonia.
2. Bits lattice enthalpy is so large, and $I^-$ such a poor ligand, that complex formation with $NH_3$ cannot release enough energy to overcome it.
3. Ciodide ions react directly with the ammonia molecules in solution to form a completely separate, insoluble compound that simply coats over the AgI crystals.
4. Dammonia is too weak a base to dissolve any silver halide under any conditions at all.

1. Athe number of moles of it shown in the equation
2. Bthe power to which its concentration is raised in the rate equation
3. Cthe number of particles which collide in one step
4. Dthe time taken for its concentration to halve

1. Arate $= k[H_2O_2][I^-][H^+]$
2. Brate $= k[H_2O_2][I^-]$
3. Crate $= k[H_2O_2]^2[I^-]$
4. Drate $= k[H_2O_2][I^-]^2[H^+]^2$

1. Athe concentration of each reactant depended only on the volume of that reactant added
2. Bthe temperature would not change
3. Cthe reaction would go to completion
4. Dthe same apparatus could be used each time

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1. Afirst order with respect to $I^-$, since rate is directly proportional to $[I^-]$.
2. Bsecond order with respect to $I^-$, since halving a concentration always halves the rate regardless of order.
3. Czero order with respect to $I^-$, since the rate change exactly matches the concentration change.
4. Dfirst order overall, regardless of which reactant's concentration was changed in the experiment.

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1. Atitrating the entire reaction mixture with sodium thiosulfate right at the very start, before any reaction occurs.
2. Brecording the temperature rise of the mixture at fixed time intervals throughout the entire reaction.
3. Ctiming how long it takes for a fixed, small amount of iodine to appear (using a starch indicator), then taking 1/time as the relative rate.
4. Dmeasuring the total mass of the whole reaction flask continuously on an electronic balance for the entire duration of the reaction, from start to finish.

1. Aa yellow flame and a brown solid
2. Ba green flame and a white smoke only
3. Ca brilliant white flame and a white ash
4. Da blue flame and a black residue

1. A$Mg(s) + H_2O(g) \rightarrow MgH_2(s) + \frac{1}{2}O_2(g)$
2. B$Mg(s) + 2H_2O(g) \rightarrow Mg(OH)_2(s) + H_2(g)$
3. C$Mg(s) + H_2O(g) \rightarrow MgO(s) + H_2(g)$
4. D$2Mg(s) + H_2O(g) \rightarrow Mg_2O(s) + H_2(g)$

1. Aable to react with water in the stomach
2. Ba stronger base
3. Cmuch cheaper to produce
4. Dfar less soluble, so the suspension is only weakly alkaline

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1. Aa giant covalent (macromolecular) structure, with every carbon and oxygen atom linked in a continuous 3D lattice.
2. Ban ionic lattice structure, with $C^{4+}$ and $O^{2-}$ ions held together by strong electrostatic forces.
3. Ca simple molecular (covalent) structure, held together between molecules only by weak van der Waals forces.
4. Da metallic structure, with delocalised electrons free to move throughout the solid.

1. Aa giant covalent (macromolecular) structure, with each Si atom covalently bonded to 4 O atoms tetrahedrally.
2. Ba layered structure like graphite, with only weak forces holding the layers together.
3. Ca simple molecular structure, with only weak van der Waals forces acting between separate, discrete $SiO_2$ molecules in the solid.
4. Dan ionic lattice, with $Si^{4+}$ and $O^{2-}$ ions arranged in a giant ionic structure.

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1. Aester and amine
2. Bcarboxylic acid and amide
3. Cester and nitro
4. Damide and ketone

1. A4-aminobenzoic acid
2. B4-nitrobenzoic acid
3. Cethyl benzoate
4. Dbenzoic acid

1. A$NaNO_2$ and HCl below 10 °C
2. Bethanol and concentrated $H_2SO_4$ under reflux
3. CSn and concentrated HCl, followed by NaOH
4. Dconcentrated $HNO_3$ and $H_2SO_4$ at 55 °C

1. A4-aminobenzoic acid as its ammonium salt (the $-NH_2$ group protonated to $-NH_3^+Cl^-$).
2. Bethyl 4-aminobenzoate, since only the ester linkage's alkyl group is affected by hydrolysis.
3. C4-nitrobenzoic acid, since the amine group is oxidised back to a nitro group under acidic conditions.
4. Dbenzoic acid only, with the amine group completely removed from the aromatic ring.

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1. Abutan-1-ol, butan-2-ol and methylpropan-2-ol
2. Bbut-1-yne, but-2-yne and cyclobutene
3. Cbut-1-ene, but-2-ene and butane
4. Dbut-1-ene, 2-methylpropene, cyclobutane and methylcyclopropane

1. A$=O$
2. B$-Cl$
3. C$-H$
4. D$-OSO_2Cl$

1. Aa good conductor of heat
2. Bunreactive and an efficient catalyst for the oxidation of exhaust gases
3. Ccheap and easily replaced
4. Dreadily oxidised by exhaust gases

1. Aoxidatively cleaving the $C=C$ double bond and oxidising the $-OH$ and carbonyl groups to carboxylic acids or $CO_2$ as appropriate.
2. Breducing the $C=O$ group to $-OH$, while leaving the $C=C$ double bond and existing $-OH$ group unchanged.
3. Csubstituting the $-OH$ group with a $-Mn$ containing group, with no effect on the $C=C$ or $C=O$ groups.
4. Dpolymerising the entire molecule through addition across its $C=C$ double bond only, leaving both the $-OH$ and $C=O$ groups completely unreacted throughout.

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1. Aseparates proteins according to their solubility
2. Bidentifies the elements present in a sample
3. Cmeasures the mass of DNA in a cell
4. Dproduces a pattern of DNA fragments unique to an individual

1. Atravel further through the gel
2. Btravel less far through the gel
3. Cdo not move at all
4. Dmove towards the negative electrode

1. Ameasuring the pH of blood
2. Bestimating the age of rocks
3. Cdetecting metal ions in water
4. Ddetermining paternity

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1. Athe suspect's bands are a similar colour to the crime-scene sample's bands after staining.
2. Bthe suspect's DNA sample migrates exactly the same total distance through the gel as the crime-scene sample, regardless of the actual band pattern observed.
3. Cthe pattern (number and position) of bands in the suspect's DNA profile aligns exactly with the crime-scene sample's bands.
4. Dthe suspect's DNA sample produces more bands in total than the crime-scene sample.

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