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PROBLEM SET: ATOMIC STRUCTURE -2010/11 Write clear, concise answers for the following questions. Write no more than two sentences for any question. Include electron configuration, orbital filling diagrams, and mathematical formulas where they will support your answers. 1)Explain each of the following observations about ionization energies using the principles of atomic structure: a) As you move from left to right across a row on the periodic table, the first ionization energy of the elements increase. b) Magnesium has a higher first ionization energy than Aluminum c) Phosphorus has a higher first ionization energy than Sulfur d) Potassium has a higher second ionization energy than Calcium 2) Explain each of the following observations about atomic size using the principles of atomic structure. a) A Boron atom is larger than a Nitrogen atom b) A Potassium atom is larger than a Sodium atom c) The ionic radius of the sulfide ion is bigger than the chloride ion d) Ca2+ ion is smaller than a Cl- ion. 3) Explain each of the following about periodic trends using the principles of atomic Structure: a) The electron affinity of Fluorine is more negative than Oxygen. b) The electron affinity of Magnesium is a positive value. c) The electron affinity for Phosphorus is less negative than Silicon. d) The electron affinity of Neon is a positive value. 4) a) Describe what you would see if you added: i)a piece of zinc to a test tube filled with hydrochloric acid. ii)a piece of copper to a test tube filled with hydrochloric acid b) Explain how the activity series of metals allows you to make this prediction. c) Write a balanced net ionic equation for an reaction(s) that occur. d) In a separate experiment, a piece of copper is added to a container with nitric acid. i)Describe what you would see happening. ii) Write the balanced net ionic equation for this reaction. iii) Explain why you would obtain different results when adding the copper to nitric acid