Chapter 5 Preview Multiple Choice Short Answer Extended Response Standardized Test Preparation Chapter 5 Preview Multiple Choice Short Answer Extended Response

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 1. In the modern periodic table, elements are arranged according to A. decreasing atomic mass. B. Mendeleev’s original model. C. increasing atomic number. D. when they were discovered.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 1. In the modern periodic table, elements are arranged according to A. decreasing atomic mass. B. Mendeleev’s original model. C. increasing atomic number. D. when they were discovered.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 2. Group 17 elements, the halogens, are the most reactive of the nonmetal elements because they A. require only one electron to fill their outer energy level. B. have the highest ionization energies. C. have the largest atomic radii. D. are the farthest to the right in the periodic table.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 2. Group 17 elements, the halogens, are the most reactive of the nonmetal elements because they A. require only one electron to fill their outer energy level. B. have the highest ionization energies. C. have the largest atomic radii. D. are the farthest to the right in the periodic table.

Chapter 5 Multiple Choice 3. The periodic law states that Standardized Test Preparation Chapter 5 Multiple Choice 3. The periodic law states that A. the chemical properties of elements can be grouped according to periodicity. B. the properties of the elements are functions of atomic mass. C. all elements in the same group have the same number of valence electrons. D. all elements with the same number of occupied energy levels must be in the same group.

Chapter 5 Multiple Choice 3. The periodic law states that Standardized Test Preparation Chapter 5 Multiple Choice 3. The periodic law states that A. the chemical properties of elements can be grouped according to periodicity. B. the properties of the elements are functions of atomic mass. C. all elements in the same group have the same number of valence electrons. D. all elements with the same number of occupied energy levels must be in the same group.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 4. As you move left to right across Period 3 from Mg to Cl, the energy needed to remove an electron from an atom A. generally increases. B. generally decreases. C. does not change. D. varies unpredictably.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 4. As you move left to right across Period 3 from Mg to Cl, the energy needed to remove an electron from an atom A. generally increases. B. generally decreases. C. does not change. D. varies unpredictably.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 5. Which of the following elements has the highest electronegativity? A. oxygen. B. hydrogen. C. fluorine. D. carbon.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 5. Which of the following elements has the highest electronegativity? A. oxygen. B. hydrogen. C. fluorine. D. carbon.

Chapter 5 Multiple Choice 6. The noble gases have Standardized Test Preparation Chapter 5 Multiple Choice 6. The noble gases have A. high ionization energies. B. high electron affinities. C. large atomic radii. D. a tendency to form both cations and anions.

Chapter 5 Multiple Choice 6. The noble gases have Standardized Test Preparation Chapter 5 Multiple Choice 6. The noble gases have A. high ionization energies. B. high electron affinities. C. large atomic radii. D. a tendency to form both cations and anions.

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 7. Which electron configuration is not correct? A. O2– [He]2s22p6 B. Mg2+ [He]2s22p6 C. V3+ [Ar]3d2 D. Al3+ [Ar]2s22p6

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 7. Which electron configuration is not correct? A. O2– [He]2s22p6 B. Mg2+ [He]2s22p6 C. V3+ [Ar]3d2 D. Al3+ [Ar]2s22p6

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 8. Which two elements are more likely to have the same charge on their ions? A. Se and As B. Sn and Si C. Ca and Rb D. I and Xe

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 8. Which two elements are more likely to have the same charge on their ions? A. Se and As B. Sn and Si C. Ca and Rb D. I and Xe

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 9. Which list ranks the elements Sr, Te, Kr, Ru, and Cs in order of increasing electron affinity? A. Sr < Te < Ru < Cs < Kr B. Te < Ru < Sr < Cs < Kr C. Cs < Sr < Ru < Te < Kr D. Kr < Cs < Sr < Ru < Te

Chapter 5 Multiple Choice Standardized Test Preparation Chapter 5 Multiple Choice 9. Which list ranks the elements Sr, Te, Kr, Ru, and Cs in order of increasing electron affinity? A. Sr < Te < Ru < Cs < Kr B. Te < Ru < Sr < Cs < Kr C. Cs < Sr < Ru < Te < Kr D. Kr < Cs < Sr < Ru < Te

Chapter 5 Short Answer Standardized Test Preparation 10. The second ionization energies for the elements S–Ti are listed in a scrambled order below. Assign the correct IE2 value to each element (Hint: S has IE2 = 2251 kJ/mol, and Ti has IE2 = 1310 kJ/mol.) Explain your reasoning. IE2 values (kJ/mol): 2666, 2297, 3051, 1235, 2251, 1310, and 1145

Chapter 5 Short Answer Standardized Test Preparation 10. The second ionization energies for the elements S–Ti are listed in a scrambled order below. Assign the correct IE2 value to each element (Hint: S has IE2 = 2251 kJ/mol, and Ti has IE2 = 1310 kJ/mol.) Explain your reasoning. IE2 values (kJ/mol): 2666, 2297, 3051, 1235, 2251, 1310, and 1145 Answer: S: 2551 kJ/mol; Cl: 2297 kJ/mol; Ar: 2666 kJ/mol; K: 3051 kJ/mol; Ca: 1145 kJ/mol; Sc: 1235 kJ/mol; Ti: 1310 kJ/mol. For the second ionization, the general trend is for increasing IE2 across the period in Groups 218 with Group 1 having the highest IE2. IE2 decreases going down a group.

Standardized Test Preparation Chapter 5 Short Answer 11. What group most commonly forms 2– ions? Explain your reasoning.

Standardized Test Preparation Chapter 5 Short Answer 11. What group most commonly forms 2– ions? Explain your reasoning. Answer: Group 16 most commonly forms 2– ions, because these elements require only two more electrons to fill their shell (obtain a noble-gas configuration).

Chapter 5 Extended Response Standardized Test Preparation 12. An ordered list of atomic radii for 14 consecutive elements is shown below. Without using the graph in your book, make a graph of these atomic radii versus the element’s atomic number. Explain your reasoning. Atomic radii (pm): 75, 73, 72, 71, 186, 160, 143, 118, 110, 103, 100, 98, 227, and 197.

Chapter 5 Extended Response Standardized Test Preparation 12. An ordered list of atomic radii for 14 consecutive elements is shown below. Without using the graph in your book, make a graph of these atomic radii versus the element’s atomic number. Explain your reasoning. Atomic radii (pm): 75, 73, 72, 71, 186, 160, 143, 118, 110, 103, 100, 98, 227, and 197. Answer: There are eight numbers between the first and second minimum; therefore, these eight elements must either be the second or third period. There are four numbers before the first maximum; hence, these four numbers must be elements in the second row because the first row contains only two elements (H and He). Therefore, the eight elements must be in the third period. The first atomic radius listed must correspond to atomic number 7, which is N. (continued on next slide)

Chapter 5 Extended Response Standardized Test Preparation Chapter 5 Extended Response 12. Answer, continued: Your graph should look like the following: