Identify each statement as true or false: (a) Ionization energies are always negative quantities. (b) Oxygen has a larger first ionization energy than fluorine. (c) The second ionization energy of an atom is always greater than its first ionization energy. (d) The third ionization energy is the energy needed to ionize three electrons from a neutral atom.

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Select the false statement below.
A. Fluorine has a greater first ionization energy than iodine, andthe reason for this is because fluorine has a greater amount ofshielding of outer electrons by inner electrons than doesiodine.
B. The following process is an endothermic process and representsthe first ionization energy of an atom A:

A(g) ? A1+(g) + e1-
C. The first ionization energy of an atom is smaller than thesecond ionization energy of the same atom.
D. Phosphorus has a greater first ionization energy than magnesium,and the reason for this is because P has a greater effectivenuclear charge (Zeff) than Mg.

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.

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3. Which one of the following statements is false? (a) the first ionization energy of bromine is larger than that of calcium (b) the first ionization energy of barium is smaller than that of magnesium (c) in a given row in the periodic table, the alkali metal always has the largest first ionization energy (d) the melting points of the alkali metals decrease as their atomic weights increase (e) the second ionization energy of an element is always greater than the first ionization energy

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