QuestionJune 10, 2025

SECTION 6.3 PERIODIC TRENDS 1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium. 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl^- ion to be larger or smaller than an Mg^2+ ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S^2-) is larger than the chloride ion (Cl^-) 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electronegativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form?Explain. 10. Arrange oxygen fluorine, and sulfur in order of increasing electronegativity.

SECTION 6.3 PERIODIC TRENDS 1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium. 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl^- ion to be larger or smaller than an Mg^2+ ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S^2-) is larger than the chloride ion (Cl^-) 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electronegativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form?Explain. 10. Arrange oxygen fluorine, and sulfur in order of increasing electronegativity.
SECTION 6.3 PERIODIC TRENDS 1. Explain why a magnesium atom is smaller than atoms of both sodium and calcium. 2. Predict the size of the astatine (At) atom compared to that of tellurium (Te). Explain your prediction. 3. Would you expect a Cl^- ion to be larger or smaller than an Mg^2+ ion? Explain. 4. Which effect on atomic size is more significant, an increase in nuclear charge across a period or an increase in occupied energy levels within a group? Explain. 5. Explain why the sulfide ion (S^2-) is larger than the chloride ion (Cl^-) 6. Compare the first ionization energy of sodium to that of potassium. 7. Compare the first ionization energy lithium to that of beryllium. 8. Is the electronegativity of barium larger or smaller than that of strontium? Explain. 9. What is the most likely ion for magnesium to form?Explain. 10. Arrange oxygen fluorine, and sulfur in order of increasing electronegativity.

Solution
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Answer

1. Magnesium is smaller than sodium and calcium. ### 2. Astatine is larger than tellurium. ### 3. Cl^{-} is larger than Mg^{2+}. ### 4. Increase in occupied energy levels is more significant. ### 5. S^{2-} is larger than Cl^{-}. ### 6. Sodium has higher ionization energy than potassium. ### 7. Beryllium has higher ionization energy than lithium. ### 8. Barium has lower electronegativity than strontium. ### 9. Magnesium forms a Mg^{2+} ion. ### 10. Sulfur < Oxygen < Fluorine in electronegativity. Explanation 1. Compare Atomic Sizes of Magnesium, Sodium, and Calcium Magnesium is smaller than sodium because it has a higher nuclear charge with the same number of energy levels, pulling electrons closer. Compared to calcium, magnesium has fewer occupied energy levels, making it smaller. 2. Predict Size of Astatine vs. Tellurium Astatine is larger than tellurium because it is located below tellurium in the periodic table, meaning it has more occupied energy levels. 3. Compare Sizes of Cl^{-} and Mg^{2+} Cl^{-} is larger than Mg^{2+} because Cl^{-} gains an electron, increasing electron-electron repulsion, while Mg^{2+} loses electrons, reducing its size. 4. Significant Effect on Atomic Size An increase in occupied energy levels within a group is more significant for atomic size than an increase in nuclear charge across a period, as additional energy levels greatly increase atomic radius. 5. Compare Sizes of S^{2-} and Cl^{-} The sulfide ion (S^{2-}) is larger than the chloride ion (Cl^{-}) because S^{2-} has gained two electrons, increasing electron-electron repulsion more than the single electron gain in Cl^{-}. 6. Compare First Ionization Energies of Sodium and Potassium Sodium has a higher first ionization energy than potassium because it is higher up in the same group, meaning its valence electron is closer to the nucleus and more tightly bound. 7. Compare First Ionization Energies of Lithium and Beryllium Beryllium has a higher first ionization energy than lithium due to its higher nuclear charge and filled 2s subshell, making it harder to remove an electron. 8. Compare Electronegativity of Barium and Strontium Barium has a lower electronegativity than strontium because it is further down the group, with more energy levels, reducing effective nuclear attraction on bonding electrons. 9. Most Likely Ion for Magnesium Magnesium most likely forms a Mg^{2+} ion by losing two electrons to achieve a stable noble gas configuration. 10. Order Oxygen, Fluorine, and Sulfur by Electronegativity Increasing electronegativity order: Sulfur < Oxygen < Fluorine.

Explanation

1. Compare Atomic Sizes of Magnesium, Sodium, and Calcium<br /> Magnesium is smaller than sodium because it has a higher nuclear charge with the same number of energy levels, pulling electrons closer. Compared to calcium, magnesium has fewer occupied energy levels, making it smaller.<br /><br />2. Predict Size of Astatine vs. Tellurium<br /> Astatine is larger than tellurium because it is located below tellurium in the periodic table, meaning it has more occupied energy levels.<br /><br />3. Compare Sizes of $Cl^{-}$ and $Mg^{2+}$<br /> $Cl^{-}$ is larger than $Mg^{2+}$ because $Cl^{-}$ gains an electron, increasing electron-electron repulsion, while $Mg^{2+}$ loses electrons, reducing its size.<br /><br />4. Significant Effect on Atomic Size<br /> An increase in occupied energy levels within a group is more significant for atomic size than an increase in nuclear charge across a period, as additional energy levels greatly increase atomic radius.<br /><br />5. Compare Sizes of $S^{2-}$ and $Cl^{-}$<br /> The sulfide ion ($S^{2-}$) is larger than the chloride ion ($Cl^{-}$) because $S^{2-}$ has gained two electrons, increasing electron-electron repulsion more than the single electron gain in $Cl^{-}$.<br /><br />6. Compare First Ionization Energies of Sodium and Potassium<br /> Sodium has a higher first ionization energy than potassium because it is higher up in the same group, meaning its valence electron is closer to the nucleus and more tightly bound.<br /><br />7. Compare First Ionization Energies of Lithium and Beryllium<br /> Beryllium has a higher first ionization energy than lithium due to its higher nuclear charge and filled 2s subshell, making it harder to remove an electron.<br /><br />8. Compare Electronegativity of Barium and Strontium<br /> Barium has a lower electronegativity than strontium because it is further down the group, with more energy levels, reducing effective nuclear attraction on bonding electrons.<br /><br />9. Most Likely Ion for Magnesium<br /> Magnesium most likely forms a $Mg^{2+}$ ion by losing two electrons to achieve a stable noble gas configuration.<br /><br />10. Order Oxygen, Fluorine, and Sulfur by Electronegativity<br /> Increasing electronegativity order: Sulfur < Oxygen < Fluorine.
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