/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 74 For each element, indicate the n... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 6: Problem 74

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) nitrogen, (b) silicon, (c) chlorine.

Short Answer

Expert verified
(a) Nitrogen: 5 valence electrons, 2 core electrons, and 3 unpaired electrons. (b) Silicon: 4 valence electrons, 10 core electrons, and 2 unpaired electrons. (c) Chlorine: 7 valence electrons, 10 core electrons, and 1 unpaired electron.

Step by step solution

01

(a) Nitrogen

: 1. Determine the atomic number: Nitrogen has an atomic number of 7. 2. Write the electron configuration: For Nitrogen, the electron configuration is 1s虏 2s虏 2p鲁. 3. Analyze the electron configuration: - Valence electrons: There are 5 valence electrons in Nitrogen (2 from the 2s orbital and 3 from the 2p orbital). - Core electrons: There are 2 core electrons in Nitrogen (from the 1s orbital). - Unpaired electrons: There are 3 unpaired electrons in Nitrogen (from the 2p orbital).
02

(b) Silicon

: 1. Determine the atomic number: Silicon has an atomic number of 14. 2. Write the electron configuration: For Silicon, the electron configuration is 1s虏 2s虏 2p6 3s虏 3p虏. 3. Analyze the electron configuration: - Valence electrons: There are 4 valence electrons in Silicon (2 from the 3s orbital and 2 from the 3p orbital). - Core electrons: There are 10 core electrons in Silicon (2 from the 1s orbital, 2 from the 2s orbital, and 6 from the 2p orbital). - Unpaired electrons: There are 2 unpaired electrons in Silicon (from the 3p orbital).
03

(c) Chlorine

: 1. Determine the atomic number: Chlorine has an atomic number of 17. 2. Write the electron configuration: For Chlorine, the electron configuration is 1s虏 2s虏 2p6 3s虏 3p5. 3. Analyze the electron configuration: - Valence electrons: There are 7 valence electrons in Chlorine (2 from the 3s orbital and 5 from the 3p orbital). - Core electrons: There are 10 core electrons in Chlorine (2 from the 1s orbital, 2 from the 2s orbital, and 6 from the 2p orbital). - Unpaired electrons: There is 1 unpaired electron in Chlorine (from the 3p orbital).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

(a) What are the similarities of and differences between the \(1 \mathrm{~s}\) and \(2 s\) orbitals of the hydrogen atom? (b) In what sense does a \(2 p\) orbital have directional character? Compare the "directional" characteristics of the \(p_{x}\) and \(d_{x^{2}-y^{2}}\) orbitals. (That is, in what direction or region of space is the electron density concentrated?) (c) What can you say about the average distance from the nucleus of an electron in a \(2 s\) orbital as compared with a \(3 s\) orbital? (d) For the hydrogen atom, list the following orbitals in order of increasing energy (that is, most stable ones first): \(4 f, 6 s, 3 d, 1 s, 2 p\).

(a) According to the Bohr model, an electron in the ground state of a hydrogen atom orbits the nucleus at a specific radius of \(0.53 \AA\). In the quantum mechanical description of the hydrogen atom, the most probable distance of the electron from the nucleus is \(0.53 \AA\). Why are these two statements different? (b) Why is the use of Schr枚dinger's wave equation to describe the location of a particle very different from the description obtained from classical physics? (c) In the quantum mechanical description of an electron, what is the physical significance of the square of the wave function, \(\psi^{2}\) ? \(6.55\) (a) For \(n=4\), what are the possible values of \(l\) ? (b) For \(l=2\), what are the possible values of \(m_{l}\) ? (c) If \(m_{l}\) is 2 , what are the possible values for \(l\) ?

Give the values for \(n, l\), and \(m_{l}\) for (a) each orbital in the \(2 p\) subshell, (b) each orbital in the \(5 d\) subshell.

Arrange the following kinds of electromagnetic radiation in order of increasing wavelength: infrared, green light, red light, radio waves, \(X\) rays, ultraviolet light.

A laser pointer used in a lecture hall emits light at \(650 \mathrm{~nm}\). What is the frequency of this radiation? Using Figure 6.4, predict the color associated with this wavelength.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.