For each molecule, or ion, write the name, then draw the Lewis structure. Next to each of these molecules, draw resonance structures, when necessary. If resonance structures exist, draw all resonance structures connected with a double arrow (+) to indicate that the actual structure is an average of the resonance structures. Give the formal charge and oxidation number of the central atom on each. 25. SCI4 30. ХeF: 31. NH,OH CO(NH2)2 26. *HCO; 27. PO3- 32. 28. SO;- 33. SO2 34. CINO 35. BrOs', all possible resonance with expanded octets 29. In exercises 27-29, be sure to try at least one double bond to lower formal charges.

Draw the lewis structure with formal charges. If the lewis structure has resonance please show all possible resonance structures. 1. CH3NO2 2. HNO3 (H is bonded to one of the O's)

2,2,2-trifluoroethanol, CF₃CH₂OH. is used industrially as a solvent for nylon. Draw the Lewis structure of CF₃CH₂OH. In your final structure, please make sure the elements are in the order they are provided.

a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of SO4. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of POC13. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge:

Draw the Lewis structure for SiO₂. Be sure to include all resonance structures that satisfy the octet rule.

Write a Lewis symbol for atom or ion. Mg2+

Draw the Lewis structures (with formal charges) of each of the species in the indicated pair and use the lewis stucture to answer which has the longer bond? and which has the stronger bond? 1.) O2 or O2^2+  2.) NO- or NO^3-  3.) F2 or F2^2+  4. NO2+ or NO2^3-  5.) OF2 or FO+

11) Use the chemical equation and the table of average bond energies to answer the following questions. C3H4+4 0₂3 CO₂ + 2 H₂O a. Draw Lewis structures for all four species represented in the reaction above. b. Calculate the enthalpy change, AHns that occurs in this reaction.

2. Draw the lewis structures for both resonance structures of the OCBr+ ion and select the statement that is true a. The molecule sometimes looks like one resonances structure, and at other times it looks like the other resonance structure b. In one resonance structure, the carbon is in the center, and in the other one, the oxygen is in the center c. The bond between carbon and oxygen would best be described as 2.5 bonds (halfway between a double and a triple bond) d. In one resonance structure the positive charge is on the bromine, and in the other, it is on the carbon.

An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of zero. H Н—N—С- -о—с—Н H H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges. Click and drag to start drawing a structure.