Textbook Question
Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO32– c. ClO– d. NO2–
Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 5
Use covalent Lewis structures to explain why the compound that forms between nitrogen and hydrogen has the formula NH3 and why NH2 and NH4 are not stable.
Verified step by step guidance1
<insert step 1> Identify the valence electrons for nitrogen and hydrogen. Nitrogen has 5 valence electrons, and hydrogen has 1 valence electron.>
<insert step 2> Determine the total number of valence electrons available for bonding in NH3. Nitrogen contributes 5 electrons, and each hydrogen contributes 1 electron, totaling 8 valence electrons.>
<insert step 3> Draw the Lewis structure for NH3. Place nitrogen in the center and arrange three hydrogen atoms around it. Use pairs of electrons to form single bonds between nitrogen and each hydrogen.>
<insert step 4> Check the stability of NH3 by ensuring that nitrogen has a complete octet (8 electrons) and each hydrogen has a complete duet (2 electrons).>
<insert step 5> Explain why NH2 and NH4 are not stable. NH2 would leave nitrogen with an incomplete octet, and NH4 would require nitrogen to have 9 electrons, exceeding the octet rule.>
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