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Question 1 a) This question concerns the theoretical molecule xenon thiotetrafluoride, XeSF4. i) Draw a Lewis diagram in wedge-and-dash form showing the shape of XeSF4. Your diagram must include ALL pairs of electrons. What is the name of this shape? ii) Silicon disulphide, SiS2, can exist as linear molecules with this Lewis structure: S=Si S The Pauling electronegativities of silicon and sulphur are 1.9 and 2.58, respectively. Use this to explain why there are no dipole-dipole interactions between molecules of SiS2. b) Butan-1-ol is very soluble in water: 73g of butanol can be dissolved in one dm³ of water at room temperature. However, at the same temperature, octan-1-ol has a very low solubility in water (0.3 g dm-³). Explain this observation in terms of intermolecular forces. c) Write equations to represent the following processes (state symbols are required) i) the enthalpy of formation of carbon monoxide ii) the enthalpy of (complete) combustion of ethanal iii) the formation of the CH3 (g) radical by the reaction of methane and chlorine gases

Question 1 a) This question concerns the theoretical molecule xenon thiotetrafluoride, XeSF4. i) Draw a Lewis diagram in wedge-and-dash form showing the shape of XeSF4. Your diagram must include ALL pairs of electrons. What is the name of this shape? ii) Silicon disulphide, SiS2, can exist as linear molecules with this Lewis structure: S=Si S The Pauling electronegativities of silicon and sulphur are 1.9 and 2.58, respectively. Use this to explain why there are no dipole-dipole interactions between molecules of SiS2. b) Butan-1-ol is very soluble in water: 73g of butanol can be dissolved in one dm³ of water at room temperature. However, at the same temperature, octan-1-ol has a very low solubility in water (0.3 g dm-³). Explain this observation in terms of intermolecular forces. c) Write equations to represent the following processes (state symbols are required) i) the enthalpy of formation of carbon monoxide ii) the enthalpy of (complete) combustion of ethanal iii) the formation of the CH3 (g) radical by the reaction of methane and chlorine gases

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 1 a) This question concerns the theoretical molecule xenon thiotetrafluoride, XeSF4. i) Draw a Lewis diagram in wedge-and-dash form showing the shape of XeSF4. Your diagram must include ALL pairs of electrons. What is the name of this shape? ii) Silicon disulphide, SiS₂, can exist as linear molecules with this Lewis structure: S: Si S The Pauling electronegativities of silicon and sulphur are 1.9 and 2.58, respectively. Use this to explain why there are no dipole-dipole interactions between molecules of SiS2. b) Butan-1-ol is very soluble in water: 73g of butanol can be dissolved in one dm³ of water at room temperature. However, at the same temperature, octan-1-ol has a very low solubility in water (0.3 g dm-³). Explain this observation in terms of intermolecular forces. c) Write equations to represent the following processes (state symbols are required) i) the enthalpy of formation of carbon monoxide ii) the enthalpy of (complete) combustion of ethanal iii) the formation of the CH3 (g) radical by the reaction of methane and chlorine gases
Transcribed Image Text:Question 1 a) This question concerns the theoretical molecule xenon thiotetrafluoride, XeSF4. i) Draw a Lewis diagram in wedge-and-dash form showing the shape of XeSF4. Your diagram must include ALL pairs of electrons. What is the name of this shape? ii) Silicon disulphide, SiS₂, can exist as linear molecules with this Lewis structure: S: Si S The Pauling electronegativities of silicon and sulphur are 1.9 and 2.58, respectively. Use this to explain why there are no dipole-dipole interactions between molecules of SiS2. b) Butan-1-ol is very soluble in water: 73g of butanol can be dissolved in one dm³ of water at room temperature. However, at the same temperature, octan-1-ol has a very low solubility in water (0.3 g dm-³). Explain this observation in terms of intermolecular forces. c) Write equations to represent the following processes (state symbols are required) i) the enthalpy of formation of carbon monoxide ii) the enthalpy of (complete) combustion of ethanal iii) the formation of the CH3 (g) radical by the reaction of methane and chlorine gases
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