I am needing help with a through c, please. Sodium azide, NaN3, is commonly used in automobile airbags, since it decomposes explo-sively to form nitrogen gas.a. Complete the skeleton structure shown below for the azide ion, N₁, and any otherresonance structures that may be applicable.b. Use formal charge to determine which resonance structure is most important.c. Use VSEPR theory to predict the molecular shape (linear or bent).N N N

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World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section12.3: Lewis Structures

Problem 4RQ

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a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.
G. N. Lewis developed a model for chemical bonding that you have learned in this chapter. His theory was extremely successful and is used today at all levels of chemistry, from the introductory class to the research laboratory. Why was Lewis theory so successful?
The chemistry of the nitrite ion and HNO2: (a) Two resonance structures are possible for NO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. (b) In forming the acid HNO2 an H+ ion attaches to the O atom and not the N atom of NO2. Explain why you would predict this result. (c) Two resonance structures are possible for HNO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. Is either of these structures strongly preferred over the other?
The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing) underground CO2produced at power plants so as to diminish the: greenhouse effect. Draw all resonance structures of the CO2molecule.
1. For the species listed above, write two valid and likely Lewis structures. 2. Calculate formal charges on all atoms in each structure. Apply the criteria mentioned above to select the “best” Lewis structure. Label your chosen Lewis structure for each species as “BEST”.
What determines which atoms are the central atoms? How do you adjust the number of electrons to form a cation? What about an anion? What causes some molecules with the same number of electron domains to have different shapes? Would they cause the real bond angle to be larger or smaller? Why? Which of the following elements should you expect to form an incomplete octet: H, He, Be, B, C, O? Why? Which of the following elements are good candidates to form an expanded octet: N, F, Ne, P, S, Cl, Ar? Why? What things must you consider when determining if a molecule is polar or non-polar?
25. A skeletal structure for SO₂Cl₂ is shown below. Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms.
1) Discuss the advantages and disadvantages of using the molecular models (ball and stick) as learning aids. Recommend an alternative to using this method for modeling molecules. 2) Build C6H6 as a ring. What do you notice about the placement of the bonds? This is an example of resonance. What is a resonant Lewis structure? 3) Explain how a diminished and expanded octet can be formed.
A common form of elemental phosphorus is the tetrahedralP4 molecule, where all four phosphorus atoms areequivalent: At room temperature phosphorus is a solid. (a) Are there anylone pairs of electrons in the P4 molecule? (b) How manyP¬P bonds are there in the molecule? (c) Draw a Lewisstructure for a linear P4 molecule that satisfies the octet rule.Does this molecule have resonance structures? (d) On thebasis of formal charges, which is more stable, the linear moleculeor the tetrahedral molecule?
A common form of elemental phosphorus is the tetrahedralP4 molecule, where all four phosphorus atoms areequivalent:At room temperature phosphorus is a solid. (a) Are there anylone pairs of electrons in the P4 molecule? (b) How manyP¬P bonds are there in the molecule? (c) Draw a Lewisstructure for a linear P4 molecule that satisfies the octet rule.Does this molecule have resonance structures? (d) On thebasis of formal charges, which is more stable, the linear moleculeor the tetrahedral molecule?
Consider the SO 3 molecule. How many valence electrons does the molecule have? How many lone pairs of electrons are on the central atom? How many lone pairs of electrons in total are on the substituent atoms? How many resonance structures can be drawn for the molecule? If the ion doesn't exhibit resonance, indicate "1" as only one structure can be drawn for the molecule.
Using BEST Lewis structures and the VSEPR model, match each molecular formula with the molecular geometry that describes it.

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