Chemistry Paper 2 November 2014

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1. AThe chloride ion has one more electron than the chlorine atom, giving it a negative charge.
2. BThe chloride ion has one fewer electron than the chlorine atom, giving it a positive charge.
3. CThe chloride ion has one more proton than the chlorine atom.
4. DThe chloride ion has one more neutron than the chlorine atom.

1. ACCl4 molecules are held together by weak intermolecular forces of attraction, while Ca²⁺ and Cl⁻ ions in CaCl2 are held together by strong electrostatic forces.
2. BCCl4 is made up of ions while CaCl2 is made up of covalent molecules.
3. CCCl4 has a higher boiling point than CaCl2 because its molecules are larger.
4. DCCl4 molecules are held together by strong intermolecular forces of attraction, while ions in CaCl2 are held together by weak electrostatic forces.

1. Aprecipitation
2. Bredox
3. Chydrolysis
4. Dneutralisation

1. A1,92 dm3
2. B2,69 dm3
3. C5,76 dm3
4. D2,88 dm3

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1. A24,67 cm3/min
2. B0,411 cm3/min
3. C0,274 cm3/min
4. D0,400 cm3/min

1. AAtoms of the same element with the same number of protons but different numbers of neutrons.
2. BMolecules with the same molecular formula but different structural formulae.
3. CDifferent structural forms of the same element in the same physical state.
4. DCompounds with the same general formula and similar chemical properties, differing by CH2 between successive members.

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1. Aa metal is deposited as a coating onto another metal by passing an electric current through an electrolyte containing ions of the coating metal, as in electroplating.
2. Ban ionic compound is broken down using heat alone, without an electric current, as happens in thermal decomposition.
3. Can ionic compound is broken down into its elements by passing an electric current through its molten or aqueous solution form.
4. Da covalent compound's molecules move through a porous membrane under an electric field, with no electrode reactions taking place.

1. AThey migrate to the cathode, where they lose electrons and are converted to atoms.
2. BThey migrate to the anode, where they lose electrons and are converted to atoms.
3. CThey migrate to the cathode, where they gain electrons and are converted to atoms.
4. DThey migrate to the anode, where they gain electrons and are converted to atoms.

1. AOxygen gas would be produced at the anode, as OH⁻ ions from water are preferentially discharged instead of chromium dissolving.
2. BChlorine gas would be produced at the anode, as Cl⁻ ions are preferentially discharged.
3. CHydrogen gas would be produced at the anode, as H⁺ ions are preferentially discharged.
4. DChromium metal would continue to be deposited at the anode, as with the chromium electrode.

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1. AFe2Cl3
2. BFeCl2
3. CFeCl3
4. DFeCl

1. AFeCl6
2. BFeCl3
3. CFe3Cl9
4. DFe2Cl6

1. AEach carbon atom is covalently bonded to three other carbon atoms, forming layers of hexagonal rings that can slide over each other.
2. BPositive and negative ions are held together in a rigid lattice by strong electrostatic forces, as in an ionic compound such as sodium chloride.
3. CIndividual molecules are held together by weak forces of attraction between molecules, as in a simple molecular solid such as iodine.
4. DEach carbon atom is covalently bonded to four other carbon atoms in a rigid three-dimensional structure.

1. Agraphite has a lower density than diamond, and materials with lower density conduct electricity better.
2. Bgraphite has delocalised electrons that move freely along its layers, while diamond has no free or delocalised electrons.
3. Cdiamond has delocalised electrons that move freely, while all of graphite's electrons are held in fixed covalent bonds.
4. Dgraphite contains free-moving ions, while diamond contains only covalent bonds.

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1. ATest the gas with a lit splint; it burns with a 'pop' sound, as it does when testing for hydrogen gas.
2. BBubble the gas through limewater; the limewater turns milky, as it does when testing for carbon dioxide gas.
3. CBubble the gas through bromine water; the orange/brown colour is decolourised.
4. DTest the gas with a glowing splint; the splint relights, as it does when testing for oxygen gas.