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Chapter 13: Q67E (page 554)

Question: Some of the pollutants in the atmosphere are ozone, sulphur dioxide, and sulfur trioxide. Draw Lewis structures for these three molecules. Show all resonance structures.

Short Answer

Expert verified

Answer

The given pollutants are O3, SO2, and SO3. These are triatomic molecules with symmetricity around the central atom.

Step by step solution

01

Drawing Lewis structure and resonance structure O3 

The homogenous molecule has a symmetrical structure. The molecule contains one double bond. Ozone has two O atoms with a positive partial charge.

02

Drawing Lewis structure and resonance structure SO2 

SO2 is an sp2 hybridized. Two O and S combined to produce molecules. The molecule has a planar structure.

03

Drawing Lewis structure and resonance structure SO3 

This compound has two covalent S-O bonds represented by an arrow line in the diagram. In molecule, S does not have lone pair it is completely donated to two O atoms.

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Most popular questions from this chapter

Question: Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structures for the reactants and products in the reactions described below.

a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide.

b. Boron trihydride accepts a pair of electrons from ammonia, forming

NH3BH3.

Give a possible explanation for why these two reactions occur.


Think of forming an ionic compound as three steps (this is a simplification, as with all models):(1)removing an electron from the metal,(2)adding an electron to the nonmetal, and(3)allowing the metal cation and nonmetal anion to come together.

a. What is the sign of the energy change for each of these three processes?

b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer.

c. What must be the sign of the sum of the three processes?

d. Given your answer to part c, why do ionic bonds occur?

e. Given your explanations to part dwhy is NaClstable but not Na2Cl2and Nacl2? What about MgOcompared to MgO2and Mg2O?

Question: Nitrous oxide (N2O) has these possible Louis structure:

Given the following bond lengths,

N-N167pmN=O115pmN=N120pmN-O147pmN≡N110pm

Rationalize the observations that the N-N bond length in N2O isand that the N-O bond length is 119 Pm. Assign formal charges to the resonance structures on the basis of formal charges? Is this consistent with observation?

Question: SF6, CIF5 , and XeF4 are three compounds whose central atoms do not follow the octet rule. Draw Lewis structures for these compounds.

Which of the following molecules have net dipole moments? For the polar molecules, indicate the polarity of each bond and the direction of the net dipole moment of the molecule.

a.CH2Cl2,CHCl3,CCl4b.CO2,N2Oc.PH3,NH3
See all solutions

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