Multiple Choice
Which of the following best explains why successive ionization energies increase for an atom?
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10. Periodic Properties of the Elements
Periodic Trend: Successive Ionization Energies
Multiple Choice
Which of the following chemical equations correctly represents the third ionization of aluminum?
A
Al^{+} ightarrow Al^{2+} + e^{-}
B
Al ightarrow Al^{3+} + 3e^{-}
C
Al^{3+} ightarrow Al^{4+} + e^{-}
D
Al^{2+} ightarrow Al^{3+} + e^{-}
Verified step by step guidance1
Understand what ionization means: Ionization is the process of removing electrons from an atom or ion, resulting in a positively charged ion.
Identify the order of ionizations for aluminum (Al): The first ionization removes one electron from neutral Al to form Al^{+}, the second ionization removes another electron from Al^{+} to form Al^{2+}, and the third ionization removes an electron from Al^{2+} to form Al^{3+}.
Write the general form of the third ionization reaction: It involves removing one electron from the Al^{2+} ion, so the equation should be Al^{2+} \(\rightarrow\) Al^{3+} + e^{-}.
Check the given options against this understanding: The correct third ionization must start with Al^{2+} and produce Al^{3+} plus an electron.
Confirm that the other options do not represent the third ionization: For example, Al \(\rightarrow\) Al^{3+} + 3e^{-} represents the removal of three electrons at once (not stepwise), and Al^{3+} \(\rightarrow\) Al^{4+} + e^{-} is not typical for aluminum as it rarely forms a +4 ion.
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