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4) The successive () ionization energies of a certain element are 1, kJ/mol, I, 4900 kJ/mol, L = 6500 kJ/mol, and Is-8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is A) K B) Si C) As D) Ca E) S 5) Which of the following elements has the greatest electron affinity? A) Mg B) Al C) Si D) P E) S 6) Select the series of atoms that are arranged in order of increasing electronegativity. A) S< K

4) The successive () ionization energies of a certain element are 1, kJ/mol, I, 4900 kJ/mol, L = 6500 kJ/mol, and Is-8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is A) K B) Si C) As D) Ca E) S 5) Which of the following elements has the greatest electron affinity? A) Mg B) Al C) Si D) P E) S 6) Select the series of atoms that are arranged in order of increasing electronegativity. A) S< K

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please solve only question 8

### Chemistry Problem Set **1. Which of the following make an isoelectronic pair?** A) \( \text{Ca}^{2+} \) and \( \text{Fe}^{3+} \) B) \( \text{O}^{2-} \) and \( \text{F}^- \) C) \( \text{F}^- \) and \( \text{Cl}^- \) D) \( \text{Cl}^- \) and \( \text{Ca}^{2+} \) E) None of the above **2. Arrange the following ions in order of increasing ionic radius: \( \text{K}^+, \text{P}^{3-}, \text{S}^{2-}, \text{Cl}^- \)** A) \( \text{K}^+ < \text{Cl}^- < \text{S}^{2-} < \text{P}^{3-} \) B) \( \text{K}^+ < \text{P}^{3-} < \text{S}^{2-} < \text{Cl}^- \) C) \( \text{P}^{3-} < \text{S}^{2-} < \text{Cl}^- < \text{K}^+ \) D) \( \text{P}^{3-} < \text{Cl}^- < \text{S}^{2-} < \text{K}^+ \) **3. Which of the elements listed below has the highest first ionization energy?** A) He B) Ne C) Ar D) Kr E) Xe **4. The successive (4) ionization energies of a certain element are \( \text{I}_1 = 589.5 \text{ kJ/mol} \), \( \text{I}_2 = 1145 \text{ kJ/mol} \), \( \text{I}_3 = 4900 \text{ kJ/mol} \), \( \text{I}_4 = 6500 \text{ kJ/mol} \), and \( \text{I}_5 = 8100 \text{ kJ/mol} \). This pattern of ionization energies suggests that the unknown element is:** A) P B) S C) As D) Ca
Transcribed Image Text:### Chemistry Problem Set **1. Which of the following make an isoelectronic pair?** A) \( \text{Ca}^{2+} \) and \( \text{Fe}^{3+} \) B) \( \text{O}^{2-} \) and \( \text{F}^- \) C) \( \text{F}^- \) and \( \text{Cl}^- \) D) \( \text{Cl}^- \) and \( \text{Ca}^{2+} \) E) None of the above **2. Arrange the following ions in order of increasing ionic radius: \( \text{K}^+, \text{P}^{3-}, \text{S}^{2-}, \text{Cl}^- \)** A) \( \text{K}^+ < \text{Cl}^- < \text{S}^{2-} < \text{P}^{3-} \) B) \( \text{K}^+ < \text{P}^{3-} < \text{S}^{2-} < \text{Cl}^- \) C) \( \text{P}^{3-} < \text{S}^{2-} < \text{Cl}^- < \text{K}^+ \) D) \( \text{P}^{3-} < \text{Cl}^- < \text{S}^{2-} < \text{K}^+ \) **3. Which of the elements listed below has the highest first ionization energy?** A) He B) Ne C) Ar D) Kr E) Xe **4. The successive (4) ionization energies of a certain element are \( \text{I}_1 = 589.5 \text{ kJ/mol} \), \( \text{I}_2 = 1145 \text{ kJ/mol} \), \( \text{I}_3 = 4900 \text{ kJ/mol} \), \( \text{I}_4 = 6500 \text{ kJ/mol} \), and \( \text{I}_5 = 8100 \text{ kJ/mol} \). This pattern of ionization energies suggests that the unknown element is:** A) P B) S C) As D) Ca
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