9701_s17_qp_22 - revisedeck

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The composition of atoms and ions can be determined from knowledge of atomic number, nucleon number and charge. Complete the table. atomic number nucleon number number of electrons number of protons number of neutrons symbol 6Li+ Boron occurs naturally as a mixture of two stable isotopes, 10B and 11B. The relative isotopic masses and percentage abundances are shown. isotope relative isotopic mass abundance / % 10B 10.0129 19.78 11B to be calculated 80.22 Define the term relative isotopic mass. Calculate the relative isotopic mass of 11B. Give your answer to six significant figures. Show your working.

1. Atomic structure → 1.1. Particles in the atom and atomic radius

2. Atoms, molecules and stoichiometry → 2.1. Relative masses of atoms and molecules

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Nitrogen gas, N2, is very unreactive. Explain why nitrogen gas is so unreactive. Despite the low reactivity of N2, oxides of nitrogen occur in the atmosphere through both natural and man-made processes. Explain why oxides of nitrogen can be produced by internal combustion engines. State and explain, using a suitable equation, how oxides of nitrogen produced by internal combustion engines can be prevented from reaching the atmosphere. State the role of nitrogen dioxide, NO2, in the formation of acid rain by oxides of sulfur. Write suitable equations to explain this role. role equation 1 equation 2 Suggest an equation to show how NO2 can contribute directly to acid rain. Explain how the uncontrolled use of nitrate fertilisers on land can lead to a severe reduction in water quality in rivers.

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

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The hydrogen halides, HCl, HBr and HI, can undergo thermal decomposition. In a sealed container an equilibrium is established according to the equation shown. 2HXH2+ X2(where X = Cl, Br or Some bond energies are shown in the table. bond energy / kJ mol–1 H–Br H–H Br–Br Use these data to calculate a value for the enthalpy change, ΔH, for the thermal decomposition of hydrogen bromide, HBr, according to the equation shown. ΔH = kJ mol–1 At a temperature of 700 K a sample of HBr is approximately 10% decomposed. Changing the temperature affects both the rate of decomposition of HBr and the percentage that decomposes. The Boltzmann distribution for a sample of HBr at 700 K is shown. Ea represents the activation energy for the reaction. proportion of molecules with a given energy molecular energy Ea Using the same axes, sketch a second curve to indicate the Boltzmann distribution at a higher temperature. With reference to the curves, state and explain the effect of increasing temperature on the rate of decomposition of HBr. The decomposition of HBr is endothermic. State the effect of increasing temperature on the percentage of HBr that decomposes. Use Le Chatelier’s principle to explain your answer. At 700 K HBr is approximately 10% decomposed but hydrogen iodide, HI, is approximately 20% decomposed. Explain this difference with reference to bond strengths and the factors that affect them. At temperatures above 1500 K, HCl will decompose. A sample of 0.300 mol of HCl decomposed in a sealed container. The resulting equilibrium mixture was found to contain 1.50 × 10–2 mol of Cl 2. Calculate the amounts, in mol, of H2 and HCl present in the equilibrium mixture. H2 = mol HCl = mol Calculate the mole fraction of each gas in the equilibrium mixture. mole fraction of HCl = mole fraction of H2 = mole fraction of Cl 2 = In another experiment under different conditions, an equilibrium mixture was produced with mole fractions for each species as shown. species mole fraction HCl 0.88 H2 0.06 Cl 2 0.06 Write the expression for the equilibrium constant, Kp, for the decomposition of HCl. 2HCl H2+ Cl 2Kp = Explain why the total pressure of the system does not need to be known for Kp to be calculated for this experiment. Calculate the value of Kp for this experiment. Kp =

11. Group 17 → 11.2. The chemical properties of the halogen elements and the hydrogen halides

8. Reaction kinetics → 8.2. Effect of temperature on reaction rates and the concept of activation energy

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The hydrocarbons A, C4H10, and B, C4H8, are both unbranched. A does not decolourise bromine. B decolourises bromine and shows geometrical isomerism. Draw the skeletal formula of A. A The hydrocarbon A, C4H10, has a branched isomer. Suggest why unbranched A has a higher boiling point than its branched isomer. Give the structural formula of B. Explain why B shows geometrical isomerism. Draw the mechanism of the reaction of B with bromine, Br2. Include all necessary charges, dipoles, lone pairs and curly arrows. Explain the origin of the dipole on Br2 in this mechanism. The alcohols C and D are isomers of each other with molecular formula C4H10O. Both isomers are branched. When C is heated under reflux with acidified potassium dichromate(no colour change is observed. When D is heated under reflux with acidified potassium dichromate(the colour of the mixture changes from orange to green and E, C4H8O2, is produced. E reacts with aqueous sodium carbonate to form carbon dioxide gas. Identify C, D and E. C D E Write the equation for the reaction between E and aqueous sodium carbonate. The isomers F and G, C5H10O, both form an orange precipitate when reacted with 2,4-DNPH. F is unbranched and reacts with alkaline aqueous iodine to produce a yellow precipitate. G does not react with alkaline aqueous iodine. It contains a chiral centre and produces a silver mirror when warmed with Tollens’ reagent. Name the yellow precipitate produced by the reaction between F and alkaline aqueous iodine. Give the structural formula of F and of G. F G Explain the meaning of the term chiral centre. H and I are isomers with molecular formula C2H4O2. The infra-red spectra of isomers H and I are shown. percentage transmittance percentage transmittance wavenumber / cm–1 H wavenumber / cm–1 I Identify the bonds responsible for the principal peaks above 1500 cm–1 in each spectrum. spectrum of H spectrum of I Name H and I. H I

15. Halogen compounds → 15.1. Halogenoalkanes

14. Hydrocarbons → 14.2. Alkenes

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