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Solution: What is the maximum number of electrons that can

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 90P Chapter 9

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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1
Problem 90P

PROBLEM 90P

What is the maximum number of electrons that can occupy the n = 4 quantum shell?

Step-by-Step Solution:

Solution 90P

Step 1:

The fourth shell has 4 subshells(s, p, d, f). The s subshell, which has 1 orbital with 2 electrons, the p subshell, which has 3 orbitals with 6 electrons, and the d subshell, which has 5 orbitals with 10 electrons, f subshell has 7 orbital , which has 14 electrons. For a total of 16 orbitals and 32 electrons.

Step 2 of 2

Chapter 9, Problem 90P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “What is the maximum number of electrons that can occupy the n = 4 quantum shell?” is broken down into a number of easy to follow steps, and 16 words. The full step-by-step solution to problem: 90P from chapter: 9 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 90P from 9 chapter was answered, more than 312 students have viewed the full step-by-step answer. This full solution covers the following key subjects: electrons, maximum, occupy, quantum, shell. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.

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