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Ch.9 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 5th Edition
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Tutti i libri di testoTro 5th EditionCh.9 - Periodic Properties of the ElementsProblema 79
Capitolo 9, Problema 79

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

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Step 1: Understand the concept of metallic character. Metallic character refers to how easily an element can lose electrons to form positive ions (cations). Elements with higher metallic character are typically found on the left side and towards the bottom of the periodic table.
Step 2: Locate the elements on the periodic table. Chlorine (Cl) is in Group 17 (halogens) and Period 3, while Oxygen (O) is in Group 16 and Period 2.
Step 3: Compare their positions. Metallic character decreases across a period from left to right and increases down a group. Since both Cl and O are nonmetals, we need to determine which is less nonmetallic (or more metallic) based on their positions.
Step 4: Analyze the trend. Oxygen is higher up in the periodic table compared to chlorine, which means it is less metallic. Chlorine, being lower in the same group, is more metallic than oxygen.
Step 5: Conclude which element is more metallic. Based on their positions and the trend of metallic character, chlorine (Cl) is more metallic than oxygen (O).

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Metallic Character

Metallic character refers to the tendency of an element to lose electrons and form positive ions. Elements with high metallic character are typically good conductors of heat and electricity, and they exhibit properties such as malleability and ductility. As you move down a group in the periodic table, metallic character increases, while it generally decreases across a period from left to right.
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Metallic Character Example

Periodic Trends

Periodic trends are patterns observed in the properties of elements as you move across or down the periodic table. 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 positions in terms of reactivity and bonding.
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Periodic Trends

Halogens vs. Chalcogens

Halogens (Group 17) and chalcogens (Group 16) are two groups of nonmetals in the periodic table. Halogens, such as chlorine (Cl), are more reactive and have higher electronegativities compared to chalcogens like oxygen (O). While both groups are nonmetals, halogens are generally considered to have less metallic character than chalcogens, making it essential to compare their properties when determining metallic character.
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Halogenation Reactions
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