Explanation The metallic character is related with the chemical properties of metals. These chemical properties are a result of how easily metals tend to lose their electrons in chemical reactions to form cations. The tendency of metals to lose electrons is attributed to their low ionization energies. Metallic character increases on going down the group. It is because the atomic radius increases down the group and effective nuclear charge decreases. This leads to less attraction of electrons by the nucleus; thus, electrons are lost easily as one moves down the group. Metallic character decreases across the period in the periodic table from left to right. It is because the atomic radius decreases on moving across the period and effective nuclear charge increases. The electrons are more tightly held to the nucleus; thus electrons are not lost easily. Following the above trends, the elements in the bottom left corner have the highest metallic character and the ones that lie in the top right corner have the lowest metallic character. S r lies in the bottom left corner; thus it has the highest metallic character. G a and A l belong to the same group, but G a is placed lower to A l

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Chapter 8, Problem 84E

Interpretation Introduction

To arrange: The elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al

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Chapter 8, Problem 83E

Chapter 8, Problem 85E

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Ch. 8 - Prob. 1SAQ Ch. 8 - Q2. Which electron in sulfur is most shielded from...Ch. 8 - Prob. 3SAQ Ch. 8 - Prob. 4SAQ Ch. 8 - Prob. 5SAQ Ch. 8 - Prob. 6SAQ Ch. 8 - Prob. 7SAQ Ch. 8 - Prob. 8SAQ Ch. 8 - Prob. 9SAQ Ch. 8 - Prob. 10SAQ

Ch. 8 - Prob. 11SAQ Ch. 8 - Prob. 12SAQ Ch. 8 - Q13. The ionization energies of an unknown...Ch. 8 - Prob. 14SAQ Ch. 8 - Q15. For which element is the gaining of an...Ch. 8 - 1. What are periodic properties? Ch. 8 - Prob. 2E Ch. 8 - Prob. 3E Ch. 8 - 4. Who is credited with arranging the periodic...Ch. 8 - 5. Explain the contributions of Meyer and Moseley...Ch. 8 - Prob. 6E Ch. 8 - Prob. 7E Ch. 8 - Prob. 8E Ch. 8 - Prob. 9E Ch. 8 - 10. What is penetration? How does the penetration...Ch. 8 - 11. Why are the sublevels within a principal level...Ch. 8 - 12. What is an orbital diagram? Provide an...Ch. 8 - Prob. 13E Ch. 8 - Prob. 14E Ch. 8 - Prob. 15E Ch. 8 - Prob. 16E Ch. 8 - Prob. 17E Ch. 8 - Prob. 18E Ch. 8 - Prob. 19E Ch. 8 - Prob. 20E Ch. 8 - 21. Describe the relationship between an element’s...Ch. 8 - 22. Which of the transition elements in the first...Ch. 8 - 23. Describe how to write the electron...Ch. 8 - Prob. 24E Ch. 8 - Prob. 25E Ch. 8 - Prob. 26E Ch. 8 - 27. What is effective nuclear charge? What is...Ch. 8 - Prob. 28E Ch. 8 - Prob. 29E Ch. 8 - Prob. 30E Ch. 8 - Prob. 31E Ch. 8 - Prob. 32E Ch. 8 - 33. What is ionization energy? What is the...Ch. 8 - 34. What is the general trend in the first...Ch. 8 - 35. What are the exceptions to the periodic trends...Ch. 8 - Prob. 36E Ch. 8 - Prob. 37E Ch. 8 - Prob. 38E Ch. 8 - 39. Write a general equation for the reaction of...Ch. 8 - Prob. 40E Ch. 8 - 41. Write the full electron configuration for each...Ch. 8 - 42. Write the full electron configuration for...Ch. 8 - 43. Write the full orbital diagram for each...Ch. 8 - 44. Write the full orbital diagram for each...Ch. 8 - 45. Use the periodic table to write an electron...Ch. 8 - 46. Use the periodic table to determine the...Ch. 8 - 47. Use the periodic table to determine each...Ch. 8 - 48. Use the periodic table to determine each...Ch. 8 - 49. Name an element in the fourth period (row) of...Ch. 8 - 50. Name an element in the third period (row) of...Ch. 8 - 51. Determine the number of valence electrons in...Ch. 8 - Prob. 52E Ch. 8 - 53. Which outer electron configuration would you...Ch. 8 - Prob. 54E Ch. 8 - 55. According to Coulomb’s law, which pair of...Ch. 8 - 56. According to Coulomb’s law, rank the...Ch. 8 - 57. Which of the following will experience a...Ch. 8 - 58. Arrange the atoms according to decreasing...Ch. 8 - 59. If core electrons completely shielded valence...Ch. 8 - Prob. 60E Ch. 8 - 61. Choose the larger atom from each pair. a. Al...Ch. 8 - Prob. 62E Ch. 8 - 63. Arrange these elements in order of increasing...Ch. 8 - 64. Arrange these elements in order of decreasing...Ch. 8 - 65. Write the electron configuration for each...Ch. 8 - 66. Write the electron configuration for each...Ch. 8 - 67. Write orbital diagrams for each ion and...Ch. 8 - Prob. 68E Ch. 8 - 69. Which is the larger species in each pair? a....Ch. 8 - 70. Which is the larger species in each pair? a....Ch. 8 - 71. Arrange this isoelectronic series in order of...Ch. 8 - Prob. 72E Ch. 8 - 73. Choose the element with the higher first...Ch. 8 - Prob. 74E Ch. 8 - 75. Arrange these elements in order of increasing...Ch. 8 - Prob. 76E Ch. 8 - 77. For each element, predict where the “jump”...Ch. 8 - 78. Consider this set of ionization...Ch. 8 - 79. Choose the element with the more negative...Ch. 8 - Prob. 80E Ch. 8 - 81. Choose the more metallic element from each...Ch. 8 - Prob. 82E Ch. 8 - 83. Arrange these elements in order of increasing...Ch. 8 - Prob. 84E Ch. 8 - Prob. 85E Ch. 8 - Prob. 86E Ch. 8 - Prob. 87E Ch. 8 - Prob. 88E Ch. 8 - Prob. 89E Ch. 8 - Prob. 90E Ch. 8 - Prob. 91E Ch. 8 - Prob. 92E Ch. 8 - Prob. 93E Ch. 8 - Prob. 94E Ch. 8 - Prob. 95E Ch. 8 - Prob. 96E Ch. 8 - Prob. 97E Ch. 8 - Prob. 98E Ch. 8 - 99. Consider these elements: N, Mg, O, F, and...Ch. 8 - Prob. 100E Ch. 8 - Prob. 101E Ch. 8 - Prob. 102E Ch. 8 - Prob. 103E Ch. 8 - Prob. 104E Ch. 8 - Prob. 105E Ch. 8 - 106. The electron affinity of each group 5A...Ch. 8 - 107. The elements with atomic numbers 35 and 53...Ch. 8 - Prob. 108E Ch. 8 - Prob. 109E Ch. 8 - Prob. 110E Ch. 8 - Prob. 111E Ch. 8 - 112. The first ionization energy of sodium is 496...Ch. 8 - 113. Consider the elements: B, C, N, O, F. a....Ch. 8 - Prob. 114E Ch. 8 - 115. Consider the densities and atomic radii of...Ch. 8 - 116. As you have seen, the periodic table is a...Ch. 8 - 117. Consider the metals in the first transition...Ch. 8 - 118. Imagine a universe in which the value of ms...Ch. 8 - Prob. 119E Ch. 8 - Prob. 120E Ch. 8 - Prob. 121E Ch. 8 - Prob. 122E Ch. 8 - 123. Unlike the elements in groups 1A and 2A,...Ch. 8 - 124. Using the data in Figures 8.15 and 8.16,...Ch. 8 - 125. Even though adding two electrons to O or S...Ch. 8 - Prob. 126E Ch. 8 - 127. The heaviest known alkaline earth metal is...Ch. 8 - Prob. 128E Ch. 8 - Prob. 129E Ch. 8 - Prob. 130E Ch. 8 - 131. Imagine that in another universe atoms and...Ch. 8 - 132. The outermost valence electron in atom A...Ch. 8 - 133. Determine whether each statement regarding...Ch. 8 - Prob. 134E Ch. 8 - Prob. 135E Ch. 8 - Prob. 136QGW Ch. 8 - Prob. 137QGW Ch. 8 - Prob. 138QGW Ch. 8 - Prob. 139QGW Ch. 8 - Prob. 140QGW Ch. 8 - Prob. 141DIA

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