Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 81

How many electrons can each subshell hold before it is considered full?

Short Answer

Expert verified
Each subshell can hold the following maximum number of electrons before being considered full: - s subshell: 2 electrons - p subshell: 6 electrons - d subshell: 10 electrons - f subshell: 14 electrons

Step by step solution

01

Identify the subshells

There are 4 types of subshells, each represented by a different letter and associated with a specific angular momentum quantum number (l): - s subshell (l = 0) - p subshell (l = 1) - d subshell (l = 2) - f subshell (l = 3) In this step, we will find out the maximum number of electrons that can be held by each of these subshells.
02

Determine the maximum number of electrons for each subshell using the formula

Using the formula 2(2l+1), we will calculate the maximum number of electrons each subshell can hold before it is considered full. 1. s subshell (l = 0): \( \text{Electrons}_{s} = 2(2(0)+1) = 2(1) = 2 \) 2. p subshell (l = 1): \( \text{Electrons}_{p} = 2(2(1)+1) = 2(3) = 6 \) 3. d subshell (l = 2): \( \text{Electrons}_{d} = 2(2(2)+1) = 2(5) = 10 \) 4. f subshell (l = 3): \( \text{Electrons}_{f} = 2(2(3)+1) = 2(7) = 14 \)
03

State the maximum number of electrons for each subshell

Now that we have calculated the maximum number of electrons each subshell can hold before being considered full, we can provide the final results for each subshell: - s subshell: 2 electrons - p subshell: 6 electrons - d subshell: 10 electrons - f subshell: 14 electrons

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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 an anion and a cation joining to form a compound. (a) How does knowing the charge of the ions help to determine the formula? (b) What would be the formula of the compound formed from \(\mathrm{Ca}^{2+}\) cations and \(\mathrm{N}^{3-}\) anions?

Of the atoms \(\mathrm{Na}, \mathrm{Cl}, \mathrm{K}, \mathrm{Br}\), which has the largest atomic radius? Which has the largest first ionization energy?

What is the total number of \(p\) -subshell electrons for each of the following atoms: \(\mathrm{P}, \mathrm{Mg}\), Se, \(\mathrm{Zn} ?\)

How can you tell how many electrons a representative metal is likely to lose? What, in general, will be the charge of the cation it forms?

How does the first ionization energy of the alkali metal in a given period compare with the first ionization energy of the halogen in the same period? What is the result in terms of how these elements tend to react with each other?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation

Organic 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.

Sign-up for free