9.2. Periodicity of chemical properties of the elements in Period 3
A subsection of Chemistry, 9701, through 9. The Periodic Table: chemical periodicity
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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. 
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THEORY
2020
Paper 2, Variant 1
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The Period3 elements, Na to S, all react with oxygen to form oxides. State the trend in acid/base behaviour of the oxides of the Period3 elements, from Na to S. State and explain the trend, from Na to S, in the maximum oxidation number of the Period3 elements in their oxides. Sodiumoxide and phosphorus(oxide both react with water. Name the product of each reaction. reaction product sodium oxide with water phosphorus(oxide with water  Explain why phosphorus(oxide has a low melting point of approximately 300 °C but magnesiumoxide has a high melting point of approximately 2850 °C. Aluminiumoxide, Al 2O3, reacts separately with both acids and alkalis. Write an equation for the reaction of aluminiumoxide with excess aqueous hydrochloricacid. Write an equation for the reaction of aluminiumoxide with excess aqueous sodiumhydroxide. Describe the lattice structure of silicon(oxide. Your answer should include reference to the arrangement of the silicon and oxygen atoms and the bonds between them. Sodiumoxide and silicon(oxide react to form sodiumsilicate(, Na2SiO3. Sodiumoxide is obtained from the thermal decomposition of sodiumcarbonate. Write equations for the following reactions: sodiumoxide with silicon(oxide the thermal decomposition of sodiumcarbonate, forming sodiumoxide and carbondioxide. 
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THEORY
2020
Paper 2, Variant 2
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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. 
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THEORY
2020
Paper 2, Variant 3
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