9701_w20_qp_23 - revisedeck

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The graph shows the first ionisation energies of some of the elements in Group2. first ionisation energy / kJ mol–1 Group 2 element Be Mg Ca Sr Ba Write an equation for the first ionisation energy of Mg. Include state symbols. Explain the observed trend in first ionisation energies down Group2. The second ionisation energy of Be is 1757 kJ mol–1. Explain why the second ionisation energy of Be is higher than the first ionisation energy of Be.

1. Atomic structure → 1.4. Ionisation energy

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Phosphorus, sulfur and chlorine can all react with oxygen to form oxides. Phosphorus reacts with an excess of oxygen to form phosphorus(oxide. Write an equation to show the reaction of phosphorus with excess oxygen. Describe the reaction of phosphorus(oxide with water. State the structure and bonding of solid phosphorus(oxide. The two most common oxides of sulfur are SO2 and SO3. When SO2 dissolves in water, a small proportion of it reacts with water to form a weak Brønsted‑Lowry acid. Explain the meaning of the term weak Brønsted-Lowry acid. Write the equation for the reaction of SO2 with water. SO2 reacts with NO2 in the atmosphere to form SO3 and NO. NO is then oxidised in air to form NO2. SO2 + NO2 → SO3 + NO 2NO + O2 → 2NO2 State the role of NO2 in this two-stage process. Emissions of SO2 from coal-fired power stations can be reduced by mixing the coal with powdered limestone. Limestone is heated to form CaO in reaction1. This then reacts with SO2 and O2 to form CaSO4 in reaction2. reaction 1: CaCO3→ CaO+ CO2reaction 2: CaO+ SO2+ 1 2O2→ CaSO4State the type of reaction occurring in reaction1. Use the data to calculate the enthalpy change of reaction2. compound ∆Hf / kJ mol–1 CaO–635 SO2–297 CaSO4–1434 enthalpy change of reaction2 = kJ mol–1 Chlorine forms several oxides, including Cl 2O, Cl O2 and Cl 2O6. Draw a ‘dot-and-cross’ diagram of Cl 2O. Show outer-shell electrons only. Cl O2 can be prepared by reacting NaCl O2 with Cl 2. Write the oxidation state of chlorine in each species in the boxes provided. 2NaCl O2 + Cl 2 → 2Cl O2 + 2NaCl oxidation state of chlorine: +3 Cl 2O6is produced by the reaction of Cl O2with O3. 2Cl O2+ 2O3Cl 2O6+ 2O2∆H = –216 kJ mol–1 The reaction takes place at 500 K and 100 kPa. State and explain the effect on the yield of Cl 2O6when the experiment is carried out: ● at 1000 K and 100 kPa ● at 500 K and 500 kPa. ElementE is a Period5 element. E reacts with oxygen to form an insoluble white oxide that has a melting point of 1910 °C. The oxide of E conducts electricity only when liquid. E also reacts readily with Cl 2to form a white solid that reacts exothermically with water. The resulting solution reacts with aqueous silvernitrate to form a white precipitate that dissolves in dilute ammonia. Suggest the type of bonding shown by the oxide of E. Explain your answer. Suggest the type of bonding shown by the chloride of E. Explain your answer.

9. The Periodic Table: chemical periodicity → 9.2. Periodicity of chemical properties of the elements in Period 3

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

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The reducing agent LiAl H4 can be synthesised by reacting aluminiumchloride with lithiumhydride, LiH. At 200 °C, aluminiumchloride exists as Al 2Cl 6. Draw the structure of Al 2Cl 6, showing fully any coordinate (dative covalent) bonds in the molecule. At 1000 °C, aluminiumchloride exists as Al Cl 3. State the bond angle in Al Cl 3. ° Lithiumhydride contains the ions Li+ and H–. State the electronic configuration of these two ions. Li+ H– LiAl H4 decomposes slowly to form LiAl and H2. LiAl H4→ LiAl + 2H2LiAl shows metallic bonding. Describe metallic bonding. LiAl H4 cannot be used in aqueous solution because it reacts with water to produce LiOH, H2and a white precipitate which is soluble in excess sodiumhydroxide. Identify the white precipitate. Two students try to prepare 2‑hydroxybutanoic acid in the laboratory. O 2-hydroxybutanoic acid OH OH Both students oxidise butane‑1,2‑diol to form P in reaction1. One student then reduces P using LiAl H4. Q is formed. The other student reduces P using NaBH4. R is formed. butane-1,2-diol OH OH P O OH O [O] reaction 1 reaction 2 LiAl H4 reaction 3 NaBH4 Q R State the reagents and conditions required for reaction1. Only one of the students successfully prepares 2‑hydroxybutanoic acid. Identify which of Q or R is 2‑hydroxybutanoicacid and explain the difference between reactions2 and 3. A third student prepares 2‑hydroxybutanoicacid using propanal as the starting material. In step1 the student reacts propanal with a mixture of NaCN and HCN. C H C S H CN O C2H5 OH C2H5 C H COOH OH C2H5 step 1 NaCN / HCN step 2 HCl / reflux Draw the mechanism for the reaction of propanal with the mixture of NaCN and HCN to form S. ● Identify the ion that reacts with propanal. ● Draw the structure of the intermediate of the reaction. ● Include all charges, partial charges, lone pairs and curly arrows. C H C S H CN O C2H5 OH C2H5 Complete the equation for the reaction in step 2, when S is heated under reflux with HCl . C2H5CH(OH)CN + → C2H5CH(OH)COOH + The infrared spectrum of an organic compound is shown. The organic compound is either S or 2‑hydroxybutanoicacid. transmittance % wavenumber / cm–1 Deduce the identity of the compound. Give two reasons for your answer. In your answer, identify any relevant absorptions above 1500 cm–1 in the spectrum and the bonds that correspond to these absorptions.

16. Hydroxy compounds → 16.1. Alcohols

17. Carbonyl compounds → 17.1. Aldehydes and ketones

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Iodine is used in many inorganic and organic reactions. State and explain the trend in volatility of the halogens, from chlorine to iodine. Explain why HI is the least thermally stable of HCl, HBr and HI. The table shows the electronegativity values for hydrogen, fluorine and iodine. element electronegativity value H 2.1 F 4.0 I 2.5 Explain, in terms of intermolecular forces, why HI has a lower boiling point than HF. Iodine reacts with hot concentrated aqueous sodium hydroxide in the same way as chlorine. Write an equation for the reaction of iodine and hot aqueous sodiumhydroxide. Iodoalkanes contain carbon-iodine bonds. The simplest iodoalkane is CH3I. CH3I can be made from methanol, CH3OH. Identify a reagent that can convert CH3OH to CH3I. 1,2‑diiodoethane, CH2ICH2I, can be made by bubbling ethene into liquid iodine. Fully name the type of mechanism shown in this reaction. J reacts with NaOH, forming different products dependent on the conditions used. I J Name J. J reacts with NaOHto form K. OH K Fully name the mechanism of the reaction of J with NaOHto form K. J reacts with NaOH dissolved in ethanol to form a mixture of two alkenes, L and M. AlkeneL is shown. I NaOH in ethanol and L J M In the box provided, draw the structure of M. Explain why L does not show geometrical (cis-trans) isomerism. L reacts with hot concentrated acidified KMnO4to form propanone and one other organic product. Identify the other organic product. Propanone reacts with excess alkaline aqueous iodine. Complete and balance the equation for this reaction. CH3COCH3 + I2 + OH– CH3COO– + H2O + I– + State one observation that can be made in the reaction in .

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

14. Hydrocarbons → 14.2. Alkenes

11. Group 17 → 11.4. The reactions of chlorine

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