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Based on the relative likelihood of these possibilities and any other potential structures that YOU can draw, determine the bond order for the first N—N bond.   If your answer is a fraction, use that fraction as the decimal equivalent (i.e. 1 1/4 = 1.25, etc.)

Based on the relative likelihood of these possibilities and any other potential structures that YOU can draw, determine the bond order for the first N—N bond.   If your answer is a fraction, use that fraction as the decimal equivalent (i.e. 1 1/4 = 1.25, etc.)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Based on the relative likelihood of these possibilities and any other potential structures that YOU can draw,

determine the bond order for the first N—N bond.

 

If your answer is a fraction, use that fraction as the decimal equivalent (i.e. 1 1/4 = 1.25, etc.) 

The image contains representations of chemical structures using Lewis dot formulas, showing nitrogen atoms connected by various types of bonds. The dots represent valence electrons. 1. Two nitrogen atoms are triple-bonded to each other, shown as \( \ddot{N} \equiv N \equiv \ddot{N} \). Each nitrogen has a lone pair (two dots) on either side. 2. Three consecutive nitrogen atoms are shown, forming two triple bonds. The structure is \( \ddot{:} N \equiv N \equiv N \equiv N \equiv \ddot{N} \) with a lone pair on the leftmost and rightmost nitrogen. 3. Five nitrogen atoms are depicted in a linear arrangement with alternating double and triple bonds: \( \ddot{N} \equiv N = \dot{N} \equiv N \equiv \ddot{N} \). 4. The structure shows two double bonds and one triple bond among five nitrogen atoms: \( \ddot{N} \equiv N = N = N = \ddot{N} \). Each end nitrogen atom has a lone pair. 5. In this sequence, there is an alternating pattern of triple and single bonds: \( \ddot{N} \equiv N - N \equiv N = \ddot{N} \). Each nitrogen at the ends has a lone pair of electrons. 6. This structure shows three triple-bonded nitrogen atoms: \( \dot{\ddot{N}} \equiv N - N \equiv N - \ddot{N} : \). There are lone pairs at both ends of the chain.
Transcribed Image Text:The image contains representations of chemical structures using Lewis dot formulas, showing nitrogen atoms connected by various types of bonds. The dots represent valence electrons. 1. Two nitrogen atoms are triple-bonded to each other, shown as \( \ddot{N} \equiv N \equiv \ddot{N} \). Each nitrogen has a lone pair (two dots) on either side. 2. Three consecutive nitrogen atoms are shown, forming two triple bonds. The structure is \( \ddot{:} N \equiv N \equiv N \equiv N \equiv \ddot{N} \) with a lone pair on the leftmost and rightmost nitrogen. 3. Five nitrogen atoms are depicted in a linear arrangement with alternating double and triple bonds: \( \ddot{N} \equiv N = \dot{N} \equiv N \equiv \ddot{N} \). 4. The structure shows two double bonds and one triple bond among five nitrogen atoms: \( \ddot{N} \equiv N = N = N = \ddot{N} \). Each end nitrogen atom has a lone pair. 5. In this sequence, there is an alternating pattern of triple and single bonds: \( \ddot{N} \equiv N - N \equiv N = \ddot{N} \). Each nitrogen at the ends has a lone pair of electrons. 6. This structure shows three triple-bonded nitrogen atoms: \( \dot{\ddot{N}} \equiv N - N \equiv N - \ddot{N} : \). There are lone pairs at both ends of the chain.
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