Q3: Draw the Lewis structures for nitromethane (CH3NO2) and methyl nitrite (CH3ONO). Draw at least two resonance forms for each. Determine which form for each is the major resonance contributor.
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- Q3: Draw the Lewis structures for nitromethane (CH3NO2) and methyl nitrite (CH3ONO). Draw at least two resonance forms for each. Determine which form for each is the major resonance contributor. Page 1 of 4 Chem 0310 Organic Chemistry 1 Recitations Q4: Draw the Lewis structures for the cyanate ion (OCN) and the fulminate ion (CNO-). Draw all possible resonance structures for each. Determine which form for each is the major resonance contributor.Q4: Draw the Lewis structures for the cyanate ion (OCN) and the fulminate ion (CNO). Draw all possible resonance structures for each. Determine which form for each is the major resonance contributor.S Shown below is the major resonance structure for a molecule. Draw the second best resonance structure of the molecule. Include all non-zero formal charges. H H = HIN: H C. :0 H /\ H H Click and drag to start drawing a structure. ×
- None-draw the possible resonance structures of IO3^2- ion. -the experimental bond length of P and O bond in PO4^3- ion is in between the bond lengths of P=O and P-O.what is the reason behind this?. -draw the possible resonance structures of C3h3^- ion and on each sructure assign formal charge on each atom.Draw Lewis structures for each of the following ions. One atom in each ion has a formal charge that is not zero.Determine which atom it is, and what the formal charge is. (a) the C2H5 anion; (b) the CH3O cation; (c) the CH6N cation;(d) the CH5O cation; (e) the C3H3 anion (all three H atoms are on the same carbon)
- The resonance structures shown below have all lone pairs drawn in, but are missing formal charges. What is the formal charge on (A) the carbon on the left , (B) the nitrogen on the left (C) the carbon on the right , and (D) the nitrogen on the right A B HC DH C-N C=N H. H. HLewis structure for nitrate ion and sulfur trioxide. Draw F C of each atom.How many resonance structures can be drawn for the AsO4anion (this is a -3 charged anion)? (Hint -- first make absolutely sure you are drawing the Lewis structures with the lowest possible formal charge on the central atom). Group of answer choices 2 5 4 6 3 none
- 1. a)draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula CN- b) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula BrI3Draw the molecules in Problem 1.61 using line structuresCalculating Formal Charge: Formal charge is calculated for each atom in a structure. It provides information about the stability and reactivity of the atom in the molecule. Formal Charge = Valence Electrons - 1/2 Bonding Electrons - Non-bonding Electrons For example, the formal charge on the carbon of methane is calculated here. Carbon has 4 valence electrons. There are 8 bonding electrons around it. Formal Charge4- 12 (8) -0 Calculate the formal charge on the circled atoms in the following structures. formal charge: Incorect formal charge: formal charge: 1 Incomect