Questions: Understanding periodic trends in atomic ionizability Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization energy required He -> He+ + e- ? Tl -> Tl+ + e- ? Sb -> Sb+ + e- ? ionization energy required He -> He+ + e- ? O -> O+ + e- ? Ra -> Ra+ + e- ? 1 (least) 2 3 3 (most)

Understanding periodic trends in atomic ionizability Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization energy required He -> He+ + e- ? Tl -> Tl+ + e- ? Sb -> Sb+ + e- ? ionization energy required He -> He+ + e- ? O -> O+ + e- ? Ra -> Ra+ + e- ? 1 (least) 2 3 3 (most)
Transcript text: Understanding periodic trends in atomic ionizability Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. \begin{tabular}{|l|l|} \hline ionization & \multicolumn{1}{|c|}{\begin{tabular}{c} energy \\ required \end{tabular}} \\ \hline $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$ & $?$ \\ \hline $\mathrm{Tl} \rightarrow \mathrm{Tl}^{+}+e^{-}$ & $?$ \\ \hline $\mathrm{Sb} \rightarrow \mathrm{Sb}^{+}+e^{-}$ & $?$ \\ \hline \end{tabular} \begin{tabular}{|l|l|} \hline \multicolumn{1}{|c|}{ ionization } & \multicolumn{1}{c|}{\begin{tabular}{c} energy \\ required \end{tabular}} \\ \hline $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$ & $?$ \\ \hline $\mathrm{O} \rightarrow \mathrm{O}^{+}+e^{-}$ & $?$ \\ \hline $\mathrm{Ra} \rightarrow \mathrm{Ra}^{+}+e^{-}$ & $\checkmark ?$ \\ \hline & \begin{tabular}{l} 1 (least) \\ 2 \\ 3 \end{tabular} \\ \hline & 3 (most) \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Understanding Ionization Energy Trends

Ionization energy is the energy required to remove an electron from an atom. It generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. This is because atoms on the right side of the periodic table have more protons, which increases the nuclear charge and holds electrons more tightly. Conversely, atoms lower in a group have electrons further from the nucleus, which are easier to remove.

Step 2: Analyzing the First Set of Ionizations

For the first set of ionizations:

  • He (Helium) is a noble gas with a very high ionization energy due to its full outer shell.
  • Tl (Thallium) is in group 13 and period 6, with a relatively low ionization energy compared to helium.
  • Sb (Antimony) is in group 15 and period 5, with an ionization energy higher than thallium but lower than helium.

Order by increasing ionization energy:

  1. $\mathrm{Tl} \rightarrow \mathrm{Tl}^{+}+e^{-}$
  2. $\mathrm{Sb} \rightarrow \mathrm{Sb}^{+}+e^{-}$
  3. $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$
Step 3: Analyzing the Second Set of Ionizations

For the second set of ionizations:

  • He (Helium) again has the highest ionization energy.
  • O (Oxygen) is in group 16 and period 2, with a high ionization energy but lower than helium.
  • Ra (Radium) is in group 2 and period 7, with the lowest ionization energy among these elements.

Order by increasing ionization energy:

  1. $\mathrm{Ra} \rightarrow \mathrm{Ra}^{+}+e^{-}$
  2. $\mathrm{O} \rightarrow \mathrm{O}^{+}+e^{-}$
  3. $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$

Final Answer

For the first set of ionizations:

  • $\mathrm{Tl} \rightarrow \mathrm{Tl}^{+}+e^{-}$: \(\boxed{1}\)
  • $\mathrm{Sb} \rightarrow \mathrm{Sb}^{+}+e^{-}$: \(\boxed{2}\)
  • $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$: \(\boxed{3}\)

For the second set of ionizations:

  • $\mathrm{Ra} \rightarrow \mathrm{Ra}^{+}+e^{-}$: \(\boxed{1}\)
  • $\mathrm{O} \rightarrow \mathrm{O}^{+}+e^{-}$: \(\boxed{2}\)
  • $\mathrm{He} \rightarrow \mathrm{He}^{+}+e^{-}$: \(\boxed{3}\)
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