In the following Lewis structure of [SiF6], every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). : Ë : :ד: :ד: Si ட்::ட்: F :F: 0 0 0 2- 2+

1) Don't forget to show formal charges where necessary Draw the resonance hybrid for the following ion based upon the given resonance structures. C=CH₂ CH₂ Os. -CH₂

Would you mind to check all the answer on this table because I try to understand the line bond structure and re-draw structure my homework? Could you help me with this question CS2?

For the species below draw additional resonance structures (where all atoms have access to an octect of electrons) for species A, B, C, and D. Determine the bond order of the bond from the underlined C to underlined O for the lowest energy structure(s). You may need to evaluate the formal charge of the additional species you draw. These are species in an aprotic solvent, so only electrons may be moved, not hydrogen atoms. For each lettered structure below, input the bond order as an integer (1,2,etc) or improper fraction (4/3, 5/4, etc). A Structure Bond Order A HO: (f) H B B С Which structure A-D has the longest underlined C-O bond? :N=C=0: D D

2) (cont.) In the box below each Lewis drawing, PRINT one of the three following ABBREVIATIONS to characterize that Lewis drawing's relevance to the molecule's ACTUAL structure. i) CRS (Contributing Resonance Structure) ii) RS (Resonance Structure but not a CRS) iii) NRS (Not a Resonance Structure)

Two resonance structures are possible for the anion shown. One resonance form is given, but it is incomplete. Complete the given structure by adding nonbonding electrons and formal charges. Draw the remaining resonance structure, including nonbonding electrons and formal charges. Omit curved arrows. Structure A: complete the structure by adding Structure B: draw the remaining resonance structure, nonbonding electrons and formal charges. including nonbonding electrons and formal charges. Rings Erase Select Draw Rings More Erase Select Draw More H // C H. H

What is delocalization energy? How is it related to resonance energy? Answer by selecting all true statements. 00 Resonance energy is a term used in VB theory. Resonance energy and delocalization energy are term that describe different conditions. Resonance energy is a term used in MO theory. Resonance energy and delocalization energy are essentially the same thing. Resonance energy and delocalization energy represent the additional stability associated with a spreading out of electron density. Delocalization energy is a term used in VB theory. Delocalization energy is a term used in MO theory. Resonance energy and delocalization energy represent the additional stability associated with concentrating electron density.

3. For each molecule below, draw two additional resonance reasonable structures. Be show sure to show how the resonance structures are related using formal arrow pushing. Rank the resonance structures from most stable to least stable (if they are the same stability rank them the same). Finally, draw the hybrid. ΝΗ G yg

1. For each of the following compounds and ions, draw the complete Lewis structure. All formal charges should be on the atoms that possess that formal charge. CH4 H3CBr CH3CH₂OH H₂S H₂SO4 (sulfuric acid) H³0+ CH3* 2. Convert the following condensed formulas into bond-line structures, making sure to draw in zig-zag formation. CH3CH₂CH₂CH₂CH₂CH₂CH₂CH3 FCH₂CH₂I H₂C=CHCH₂OH (CH3)2CHCOOH

a) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges.  b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges. c) Select the three TRUE statements from those provided below. The molecule on the right (Molecule B) is planar (all atoms lie within the same plane). The molecule on the left (Molecule A) is planar (all atoms lie within the same plane). The molecule on the right (Molecule B) has polar bonds. The molecule on the left (Molecule A) has polar bonds. We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.