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Ch.9 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook
All textbooksTro 5th EditionCh.9 - Periodic Properties of the ElementsProblem 80
Chapter 9, Problem 80

Choose the more metallic element from each pair. a. Sb or Pb b. K or Ge c. Ge or Sb d. As or Sn

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1. The metallic character of an element is determined by its position on the periodic table. As you move from left to right across a period, the metallic character decreases. As you move down a group, the metallic character increases.
2. For pair a (Sb or Pb), both elements are in the p-block of the periodic table. Sb (Antimony) is in the 5th period while Pb (Lead) is in the 6th period. Since metallic character increases as you move down a group, Pb is more metallic than Sb.
3. For pair b (K or Ge), K (Potassium) is in the s-block (4th period) and Ge (Germanium) is in the p-block (4th period). Since metallic character decreases as you move from left to right across a period, K is more metallic than Ge.
4. For pair c (Ge or Sb), both elements are in the p-block of the periodic table. Ge (Germanium) is in the 4th period while Sb (Antimony) is in the 5th period. Since metallic character increases as you move down a group, Sb is more metallic than Ge.
5. For pair d (As or Sn), As (Arsenic) is in the p-block (4th period) and Sn (Tin) is also in the p-block but in the 5th period. Since metallic character increases as you move down a group, Sn is more metallic than As.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Metallic Character

Metallic character refers to the tendency of an element to lose electrons and form positive ions. It increases down a group in the periodic table and decreases across a period from left to right. Elements with higher metallic character are typically more conductive, malleable, and ductile, which are characteristic properties of metals.
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Periodic Trends

Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, ionization energy, electronegativity, and metallic character. Understanding these trends helps predict the behavior of elements in chemical reactions and their relative metallic character.
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Comparison of Elements

When comparing elements, it is essential to consider their positions in the periodic table. Elements in the same group share similar properties, while those in the same period exhibit varying characteristics. By analyzing their locations, one can determine which element is more metallic based on their tendency to lose electrons and their physical properties.
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Related Practice
Textbook Question

Choose the element with the more negative (more exothermic) electron affinity from each pair. a. Na or Rb

Textbook Question

Consider this set of ionization energies. IE1 = 578 kJ/mol IE2 = 1820 kJ/mol IE3 = 2750 kJ/mol IE4 = 11,600 kJ/mol To which third-period element do these ionization values belong?

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Textbook Question

Arrange these elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al.

Textbook Question

Arrange these elements in order of increasing metallic character: Fr, Sb, In, S, Ba, Se.

Textbook Question

Choose the more metallic element from each pair. c. Cl or O