Question 1 Item 1 Question 1 Directions: For parts of the free-response question that require calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Examples and equations may be included in your answers where appropriate. Answer the following questions about elements in Group 18 of the periodic table. (a) Using principles of atomic structure, explain why the atomic radius of Xe is less than that of Te. (b) Photoelectron spectroscopy data for the 1s sublevel of Ne and the 1s sublevel of Xe are represented below. In terms of Coulomb’s law and atomic structure, explain why the peak for Ne is positioned so far to the right of the peak for Xe. Three compounds that contain an element from Group 18 are XeOF4, XeO2F2, and XeF4. Possible Lewis electron dot diagrams for the compounds are shown below. (c) Which structure, B, C, or D, minimizes the formal charges for each atom in XeO2F2 ? Justify your choice. (d) A student proposes that the energy of the Xe−to−F bond in the structure in diagram B is equal to that of the Xe−to−F bond in the structure in diagram A. Do you agree or disagree with the student’s claim? Justify your answer. (e) The dipole moment of the XeOF4 molecule (diagram A) is nonzero. Identify its molecular geometry and explain how its geometry and the polarity of its bonds result in a nonzero dipole moment. Question 6 The boiling point of XeF4 (diagram E) is greater than the boiling point of elemental Xe. (f) Identify the type(s) of intermolecular force(s) that the two substances have in common. Question 7 (g) Explain the difference in boiling points based on the types and relative strengths of intermolecular forces. (h) XeOF4 reacts with SiO2 to produce XeO2F2 and SiF4. The unbalanced chemical equation for the reaction appears below. a SiO2 + b XeOF4 → c SiF4+ d XeO2F2 Give the value of each of the following coefficients in the balanced equation. a= b= c= d=