(a) Write out the ground-state electron configuration (1 s^2 2 s^2,. and so on) for the carbon a

Name: Problem 13, Chapter 29: College Physics
Uploaded: 2021-05-02T07:13:17-08:00
Duration: 3 min 32 s
Channel: Rashmi Sinha
Description: (a) Write out the ground-state electron configuration (1 s^2 2 s^2,. and so on) for the carbon atom. (b) What element of next-larger Z has chemical properties similar to those of carbon? (See Example 29.3.) Give the ground-state electron configuration for this element.

step 1 In this part, first part, we have to determine the ground state electron configuration of carbon

Question

(a) Write out the ground-state electron configuration $\left(1 s^{2} 2 s^{2},\right.$ and so on) for the carbon atom. (b) What element of next-larger $Z$ has chemical properties similar to those of carbon? (See Example 29.3.) Give the ground-state electron configuration for this element.

   (a) Write out the ground-state electron configuration $\left(1 s^{2} 2 s^{2},\right.$ and so on) for the carbon atom. (b) What element of next-larger $Z$ has chemical properties similar to those of carbon? (See Example 29.3.) Give the ground-state electron configuration for this element.

College Physics

Hugh D. Young Philip… 11th Edition

Chapter 29, Problem 13

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Solved by Expert Rashmi Sinha

05/02/2021

Step 1

This means it has 6 electrons in its neutral state. The electron configuration is determined by filling up the energy levels from lowest to highest. The first energy level (1s) can hold up to 2 electrons, the second energy level (2s) can also hold up to 2 Show more…

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(a) Write out the ground-state electron configuration $\left(1 s^{2} 2 s^{2},\right.$ and so on) for the carbon atom. (b) What element of next-larger $Z$ has chemical properties similar to those of carbon? (See Example 29.3.) Give the ground-state electron configuration for this element.

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Key Concepts

Ground-State Electron Configuration

This concept refers to the arrangement of electrons in an atom’s orbitals when the atom is in its lowest energy state. It determines the distribution of electrons among various energy levels and sublevels while obeying the Pauli exclusion principle, Hund’s rule, and the Aufbau principle. Understanding this configuration is fundamental to predicting an element’s chemical and physical properties.

Periodic Trends and Group Similarities

Elements that belong to the same group (vertical column) in the periodic table typically exhibit similar chemical properties because they have similar valence electron configurations. Recognizing these trends allows for the prediction of element behavior in chemical reactions, even if the elements belong to different periods. This concept is crucial for understanding why elements with higher atomic numbers may show properties analogous to lighter elements within the same group.

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