Which element in each of the following pairs has more nonmetallic character?
(a) Se or Te

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Identify the position of Se (Selenium) and Te (Tellurium) on the periodic table.

Recall that nonmetallic character increases as you move from left to right across a period and decreases as you move down a group.

Note that both Se and Te are in the same group (Group 16) of the periodic table.

Since Se is above Te in the same group, it is higher up on the periodic table.

Conclude that Se has more nonmetallic character than Te because nonmetallic character decreases down a group.

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Key Concepts

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

Nonmetallic Character

Nonmetallic character refers to the tendency of an element to exhibit properties typical of nonmetals, such as high electronegativity, poor conductivity, and the ability to gain electrons. Nonmetals are generally found on the right side of the periodic table and are characterized by their ability to form covalent bonds and anions.

Periodic Trends

Periodic trends are patterns observed in the properties of elements across the periodic table. Nonmetallic character increases as you move from left to right across a period and decreases as you move down a group. Understanding these trends helps predict the behavior of elements based on their position in the periodic table.

Group and Period Positioning

Elements are organized in groups (columns) and periods (rows) in the periodic table. Selenium (Se) and tellurium (Te) are both in Group 16, but Se is higher in the group than Te. The position of an element in the periodic table influences its properties, including its nonmetallic character, which typically decreases down a group.

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Related Practice

Consider the six second- and third-row elements in groups 4A–6A of the periodic table:

Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.

(b) Explain why the fluorides of nitrogen and phosphorus have different molecular structures but the fluorides of carbon and silicon have the same molecular structure.

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