Describe the octet rule in the Lewis model.

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Problem 5E Chapter 9

Chemistry: A Molecular Approach | 3rd Edition

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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

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Problem 5E

Describe the octet rule in the Lewis model.

Step-by-Step Solution:

Solution 5E Step 1 of 3 In the periodic table of elements, only noble gases can be considered “stable” because they have a complete electronic configuration, even in the inner Energy shells and in the outer one (called Valence Shell). The other elements, since they don’t have a complete electronic configuration in their Valence shell, must bond together in order to resemble the noble gases; on doing that, elements can share their electrons (as it happens in covalent bond) or they can tranfer electrons one to another (as it happens in ionic bond) When two elements bond together, the outer shell must contain eight electrons to be considered “complete”. This is the octet rule proposed by Lewis. In Lewis’ structures, we need to represent only the electrons of the valence shell. Every electron can be represented as a dot. Thus we need to know the electronic configuration of every element. Step 2 of 3 Example electron configuration of sodium (Na) is electron configuration of fluorine (F)is Sodium has only one electron in the valence shell; Fluorine has seven valence electrons, thus sdium and fluorin can be represented as follows:

Step 3 of 3

Chapter 9, Problem 5E is Solved
Textbook: Chemistry: A Molecular Approach
Edition: 3rd
Author: Nivaldo J. Tro
ISBN: 9780321809247

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