/*! 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 11 Consider the element silicon, Si... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 11

Consider the element silicon, Si. (a) Write its electron configuration. (b) How many valence electrons does a silicon atom have? (c) Which subshells hold the valence electrons?

Short Answer

Expert verified
The electron configuration of Silicon (Si) is \(\mathrm{1s^2 2s^2 2p^6 3s^2 3p^2}\). Silicon has 4 valence electrons, which are found in the 3s and 3p subshells.

Step by step solution

01

Writing the electron configuration of Silicon (Si)

Silicon is the element with atomic number 14, which means it has 14 electrons. To write its electron configuration, we can follow the Aufbau principle, which suggests filling the orbitals in the order of increasing energy levels. The order is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 4f, 5d, 6s, 5f, 6d, 7s, 6f, 7d, 7f, 8s, ... Filling in each orbital with the given 14 electrons, we get: 1s虏, 2s虏, 2p鈦�, 3s虏, 3p虏 So, the electron configuration for Silicon is \(\mathrm{1s^2 2s^2 2p^6 3s^2 3p^2}\).
02

Determining the number of valence electrons

Valence electrons are the electrons found in the outermost energy level of an atom. In the case of Silicon, the outermost energy level is n=3. We have 2 electrons in the 3s subshell and 2 electrons in the 3p subshell. Therefore, Silicon has a total of 2 + 2 = 4 valence electrons.
03

Identifying the subshells holding the valence electrons

As mentioned in Step 2, the valence electrons are in the outermost energy level, which is n=3 for Silicon. These valence electrons are found in two subshells: the 3s subshell and the 3p subshell. So, the subshells that hold the valence electrons of Silicon are 3s and 3p.

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

Consider the formate ion, \(\mathrm{HCO}_{2}^{-}\), which is the anion formed when formic acid loses an \(\mathrm{H}^{+}\)ion. The \(\mathrm{H}\) and the two \(\mathrm{O}\) atoms are bonded to the central \(\mathrm{C}\) atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? (c) Would you predict that the \(\mathrm{C}-\mathrm{O}\) bond lengths in the formate ion would be longer or shorter relative to those in \(\mathrm{CO}_{2}\) ?

Consider the following statement: "For some molecules and ions, a Lewis structure that satisfies the octet rule does not lead to the lowest formal charges, and a Lewis structure that leads to the lowest formal charges does not satisfy the octet rule." Illustrate this statement using the hydrogen sulfite ion, \(\mathrm{HSO}_{3}{ }^{-}\), as an example (the \(\mathrm{H}\) atom is bonded to one of the O atoms).

Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to \(\mathrm{C}\) ), (b) \(\mathrm{H}_{2} \mathrm{O}_{2}\), (c) \(\mathrm{C}_{2} \mathrm{~F}_{6}\) (contains a \(\mathrm{C}-\mathrm{C}\) bond), (d) \(\mathrm{AsO}_{3}{ }^{3-}\), (e) \(\mathrm{H}_{2} \mathrm{SO}_{3}\) ( \(\mathrm{H}\) is bonded to \(\mathrm{O}\) ), (f) \(\mathrm{NH}_{2} \mathrm{Cl}\).

(a) Triazine, \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}_{3}\), is like benzene except that in triazine every other \(\mathrm{C}-\mathrm{H}\) group is replaced by a nitrogen atom. Draw the Lewis structure(s) for the triazine molecule. (b) Estimate the carbon-nitrogen bond distances in the ring.

An ionic substance of formula MX has a lattice energy of \(6 \times 10^{3} \mathrm{~kJ} / \mathrm{mol}\). Is the charge on the ion M likely to be \(1+, 2+\), or \(3+\) ? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

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.