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Ch.9 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.9 - Periodic Properties of the ElementsProblem 54b
Chapter 9, Problem 54b

Which outer electron configurations would you expect to belong to a metalloid? ns2 b. ns2np6 c. ns2np5 d. ns2np2

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1
Identify the general characteristics of metalloids, which have properties intermediate between metals and nonmetals.
Recall that metalloids are typically found in the p-block of the periodic table, often with partially filled p orbitals.
Analyze each given electron configuration to determine which one corresponds to a partially filled p orbital, characteristic of metalloids.
Consider that ns^2np^2 configuration suggests two electrons in the p orbital, which is partially filled and typical for metalloids.
Conclude that the ns^2np^2 configuration is most likely to belong to a metalloid, as it reflects the intermediate properties of metalloids.

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Key Concepts

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

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented by a series of numbers and letters indicating the energy levels and types of orbitals occupied by electrons. Understanding electron configurations is crucial for predicting an element's chemical properties and behavior, particularly in determining its classification as a metal, nonmetal, or metalloid.
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Metalloids

Metalloids are elements that exhibit properties intermediate between metals and nonmetals. They typically have a mixed set of characteristics, such as being semiconductors of electricity and having a metallic luster. The outer electron configurations of metalloids usually include a combination of s and p electrons, which allows them to form covalent bonds and exhibit variable oxidation states.
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Periodic Table Trends

The periodic table organizes elements based on their atomic number and electron configurations, revealing trends in chemical properties. Elements in the same group often share similar outer electron configurations, influencing their reactivity and bonding behavior. Recognizing these trends helps in predicting which configurations correspond to metalloids, typically found in groups 13 to 16, where the transition from metals to nonmetals occurs.
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Related Practice
Textbook Question

Which outer electron configurations would you expect to belong to a noble gas? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

Textbook Question

Which experience a greater effective nuclear charge: the valence electrons in beryllium or the valence electrons in nitrogen? Why?

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Textbook Question

According to Coulomb's law, rank the interactions between charged particles from lowest potential energy to highest potential energy. a. a 1+ charge and a 1- charge separated by 100 pm b. a 2+ charge and a 1- charge separated by 100 pm c. a 1+ charge and a 1+ charge separated by 100 pm d. a 1+ charge and a 1- charge separated by 200 pm

Textbook Question

Which outer electron configuration would you expect to belong to a reactive nonmetal? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2

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Textbook Question

According to Coulomb's law, which pair of charged particles has the lowest potential energy? a. a particle with a 1- charge separated by 150 pm from a particle with a 2+ charge b. a particle with a 1- charge separated by 150 pm from a particle with a 1+ charge c. a particle with a 1- charge separated by 100 pm from a particle with a 3+ charge

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Textbook Question

Which outer electron configuration would you expect to belong to a reactive metal? a. ns2 b. ns2np6 c. ns2np5 d. ns2np2