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Periodic Trends
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Periodic Trends
Explain why atomic radius decreases across a period.
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Predict which element has the smaller atomic radius: Mg or Al. Justify your answer based on periodic trends.
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Sodium and chlorine are in the same period. Compare their atomic radii and explain the difference.
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Define first ionization energy.
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Compare the first ionization energies of Li and Na. Justify your answer using effective nuclear charge and electron shielding.
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Explain why the first ionization energy of oxygen is slightly lower than that of nitrogen, despite the general trend.
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Define ionic radiu
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Predict whether a Mg²⁺ ion or a Na⁺ ion will have a smaller ionic radius and justify your answer.
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Explain how the ionic radius changes when sulfur forms an anion.
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Explain the relationship between ionization energy and Coulomb's law.
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Rank the elements Be, B, and Li in order of increasing first ionization energy. Justify your answer.
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Compare the sizes of a Cl⁻ ion and a K⁺ ion, and explain the factors that contribute to the difference.
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Predict whether the trend in ionic radii is consistent across a period for anions and cations. Justify your answer.
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i) A new element X is found in Group 2, Period 5. Predict its ion charge and typical compound type when reacting with fluorine.
ii) Determine, with a reason, whether the percentage of ionic character is higher or lower in the compound formed in part i) compared to magnesium fluoride.
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Compare the expected first ionization energy of element X with that of magnesium. Justify your answer based on periodic trends.
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