The formal charge on carbon in CO 3 2-is. 00000 :0: || 2 ¥ 4 ¥ 0 +2 +4 -4 +1 , where the Lewis structure of the ion is:

COMPARING LEWIS STRUCTURES TO2/S02 | =N = :o: Enter the overall charge for each substance. For a non-zero charge greater than one, enter the number first and then sign. Calculate the overall charge by summing the formal charge on each atom in the species. :ö:

For CH3CH2OH+ and (CH3)3CCH2- a, what are the lewis structures b. where are the formal charges

A student proposes the following Lewis structure for the (PC14) ion. : Cl: - : : Cl P Cl: : | : Cl: Assign a formal charge to each atom in the student's Lewis structure. atom P formal charge left Cl ☐ top Cl ◎ right Cl bottom Cl П

Consider the formate ion, HCO2-, which is the anionformed when formic acid loses an H+ ion. The H and the twoO atoms are bonded to the central C atom. (a) Draw the bestLewis structure(s) for this ion. (b) Are resonance structuresneeded to describe the structure? (c) Would you predict thatthe C¬O bond lengths in the formate ion would be longeror shorter relative to those in CO2?

(c) Write the Lewis structure for SC12, C13+, SOCI2, CIOCIO3(contains Cl-O-CI bond)

A student proposes the following Lewis structure for the carbonate :C10=0 atom :0: Assign a formal charge to each atom in the student's Lewis structure. central O right O bottom O C ww formal charge 1 0 0 X (co-)ion. 5

Use the octet rule and formal charges to select the best Lewis structure for HCP. A H-PEc: в H-C: Р—н—с D H=P=c: E H=C=P P.

A Lewis structure for the carbonate ion is shown here: Which structure is the best resonance structure for the carbonate ion? :0: 0=C-0 • 1-0-0 12- o lö—c=ö–ộ: - o [c=ở–ợ–ộ:|- • :O: :0=C—0: :0:

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on.