1. Assign formal charges to the elements in cach of the structures below. Note: Count oxygen atoms starting from the left for each structure. :0: :0: :0: Formal Charge ö: m ö: <
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- The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.The C=O double bond is called a “carbonyl bond.” Acetone and othercarbonyl compounds are introduced in some texts along with this structure a. Is this an important resonance structure of acetone? Explain. b. Does this structure convey any useful information about acetone? If so, what?
- Which of the following statements concerning the structures below is/are true? Formal charges are not shown. You can select more than one, or none of, these statements. H H- : 0: :Ö: :0: A :Ö: :0: D :O: H -Ö—H HÖ :0: :0: B :Ö: HÔ—s—ö—H :0: -Ö—H E H- :O: :Ö: :0: C The formal charge of S is zero in structure A. The formal charge of S is zero in structure E. On the basis of formal charges, structure A is the most important structure. The formal charge of S is +1 in structure C. In structure D, the formal harge is -1 for the O atom that has a double bond to S. Structure B is unrealistic because there are too many electrons around S. -Ö-HDetermine formal charge of each labeled atom in the following structure d. :0 : :S: e a HCalculating formal charge (co: ) or A student proposes the following Lewis structure for the carbonate ion. .. C=0-0: :0: Assign a formal charge to each atom in the student's Lewis structure. atom formal charge central O right O bottom O :0 : II
- 5. Calculate the formal charges on the indicated atoms in each compound below. :0: - B. С. D. - :CE0: :Cl: А. The formal charge on phosphorous (A) is The formal charge on oxygen (B) is The formal charge on carbon (C) is The formal charge on oxygen (D) isThe structures below are two possible resonance forms for sulfate. 72- 72- :0: :0: :0-S-0: |3| :0: : (a) (b) S. O (single bond) O (double bond), Calculate the formal charge for the atoms in each and write them in the spaces above. Based on formal charge, which is the better (more contributing) structure? Circle the one that has the most preferred formal charges.2. Assign the formal charges of each atom in the structures below. O: C. a. I I H HT H HH O || ZIH N-H H b. d. 0: :Ö=~=0: :0-S-O: .O. :Ö=Z Ö: H C 11 -C C-H =C-H C -H
- central atom underlined: NH3O ICl3 XeO3 C4H4 O.R.-Lewis structure: Remember to always: • Show charge, if present. • Draw at least one more equivalent resonance structure (with «) if present, to describe delocalized covalent bonding. count all lone pairs in LS: polar: Y/N?Determine the formal charge for the atom indicated in the structures below. ASSUME that the structures are drawn correctly and that you do not have to change them due to formal charge issues. The external atom in this structure. :O: :O! Ar 11 :0: The central atom in this structure. = :0: (1 Si = : 0: 2- 1. +1 2. +2 3. +3 4. 0 5. -3 6.-2 7. -15. Write the resonance structure that would result from moving the electrons as the curved arrows indicate. Be sure to include formal charges if needed. (a) ? (b) H. ? H. H. H. (c) H. .N. (d)