Textbook Question
Arrange these compounds in order of increasing magnitude of lattice energy: KCl, SrO, RbBr, CaO.
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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.
Related Practice
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Write the Lewis structure for each molecule or ion. a. H3COH d. O22-
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Open Question
Is this question formulated correctly? If not, please fix it and return the output as a JSON of the form: {'question': 'question text'}. Here is the question: Calculate ΔH° for the reaction H2(g) + Br2(g) → 2 HBr(g) using bond energy values. The ΔH°f of HBr(g) is not equal to one-half of the value calculated. Account for the difference.
Textbook Question
Write the electron configuration for N. Then write the Lewis symbol for N and show which electrons from the electron configuration are included in the Lewis symbol.
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