How many TOTAL resonance structures are there for sulfate, SO4²? 06 4 02 O 1 (single, solved structure, no other forms)

A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.

Consider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?

Three resonance forms can be drawn for the molecule N2O. Which resonance form is likely to more closely resemble the structure of this molecule? (a) (b) (c)

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?

Draw all possible resonance structures for SO2, SO32-, and SO. Use the resonance structures to solve the problems below. the species  are in order of increasing S-O bond length (shortest bond first). SO< SO2<SO32- (A) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.)SO32-:  ---Select--- 1.00 1.33 1.50 2.00 3.00 bonds between S and O.(B) Match each species with the correct formal charge on the central S atom.SO32-:  ---Select--- -1.00 -0.67 -0.50 0.00 +1.00 +2.00 charge on S.(C) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures.SO32-:  ---Select--- -1.00 -0.67 -0.50 0.00 +1.00 +2.00 average charge on outside O atom.

What possible error(s) exist in the Lewis structure (assume we are trying to represent the best possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)? [:ö==S: N= CO :O: The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with three lone pairs on the sulfur. There are no errors. This is the best possible structure. The Lewis structure above does not minimize formal charges, thus is the not the best possible structure. The nitrogen atom has an expanded octet, and this structure is impossible. The Lewis structure contains the wrong number of electrons, thus this structure is impossible.

what are the resonance structures for ch4n, need 2

Draw the bonding pattern for the third resonance structure of the azide ion, N3. Two of the resonance structures are shown below. (Include double/triple bonds and any formal charges.) Edit Drawing eTextbook and Media N=N_N?²- A How many lone pair electrons are on the central nitrogen atom? # of lone pair electrons on the central nitrogen atom: -Ń=N: B How many lone pair electrons are on the each of the other two nitrogen atoms? # of lone pair electrons on each of the other nitrogen atoms: Why do both bonds of the azide ion have the same length? O The bond lengths are the same because the resonance structure you drew was tetrahedral. O The bond lengths are the same because single, double, and triple bonds are always the same length. O The bond lengths are the same because structures A and B are equivalent and therefore make equal contributions to the hybrid.

up for additional resources #1 :O: || The Lewis structure of ozone (O₂) is shown on the left below with numbers on the corresponding atoms. Choose the correct set of formal charges of the atoms in ascending order of atom number. #2 O: Question 9 of 28 #3 A) #1 = 0 , # 2 = 0, #3 = 0 B) #1 = -1, #2 = 0, #3 = +1 C) #1 = 0, #2 = +1, #3 = -1 D) #1 = + 1, #2 = -1, #3 = 0 E) #1 = -2, # 2 = +1, #3 = +1