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The azide ion, N3-, is a symmetrical ion, all of whose

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro ISBN: 9780321809247 1

Solution for problem 108E 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 108E

The azide ion, N3-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.

Step-by-Step Solution:

Solution 108E Step 1 of Azide ion is formed by three Nitrogen atoms and a negative charge because it’s a negative monovalent ion. The total electrons can be calculated by applying this formula Total electrons= 3(Valence electrons of N) + charge of the ion= 3(5) + 1= 16 We can assume that the terminal Nitrogens carry two lone pairs each other, while the central Nitrogen forms a double bond with the left N and a single bond with the right N, like this Step 2 If we calculate the formal charge for each N in this structure Left N Formal charge= Valence electrons - lone pairs electrons - ½ bonding electrons=5-4-2= - 1 Central N Formal charge= Valence electrons - lone pairs electrons - ½ bonding electrons=5-2-3= 0 Right N Formal charge= Valence electrons - lone pairs electrons - ½ bonding electrons=5-4-1=0 This structure, however, is not so stable because The right Nitrogen doesn’t reach the octet

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Chapter 9, Problem 108E is Solved
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Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

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