Download problem set: atomic structure

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