ON O N=0 H N=0 i i Add the missing lone pair electrons to all atoms, then draw the curved arrow notation to form next structure. + 56 120 H C :Ë: N ON O S F P
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- 11. Add curved arrows to the following structures to show how electron pairs must be moved to interconvert the structures, and locate any formal charges. This is the nitrate ion and it has three resona onance structures (RS). וך- :ó: :0: 1. supply formal charges 1. supply formal charges 2. draw e pushing arrows draw third RS here 2. draw e¯ pushing arrows that make second RS to make third RSla. Draw Kekule structures for the following lb. Draw a Line-Bond structures (to the right)for the following H3C CH3 C-CH3 H3C. CH HC FCH HCEC- -CH22. Identify and state any formal charges in the following structures. CH3 - CECH (I) 3. Draw any dipoles in the following structure. Draw your answers in question. 2. above. AH! 4-0 ㅍ CH3 on the structures shown
- The actual structure of SF4 places the lone pair in only one of two possible sites. To discuss the stability of the observed structures, we need only consider bond angles LP/LP ii. BP/BP >> LP/BP > LP/LP LP/BP > BP/BP >> LP/LP LP/LP >>> LP/BP > BP/BP LP/LP = LP/BP = BP/BP ii. iv. V.Q3. Circle the following pairs of structures that do not constitute resonance structures. H3C.CH3 H3C-N-CH3 a) b) H,C=C=CH2 H3C-CECH c) d) H3C CH2 H3C FCH2 OH e) H3C CH3 H,CCH2Pick the one reaction whose products don't match the given arrows. Assume lone pairs and formal charges are correct. A B C D H 07:0 H : OCH 3 :F: H-CI: 61: HO. :OCH 3 :ךד: + F: 어 HOT
- Name the following molecule. =D0Draw all possible resonance structures by copying the skeleton shown. Edit bonds and charges to complete each resonance structure. DOC NN [1] A Submit 7 H 1²D EXP. L [10] [10] [10] [1] [7] L CONT. 1 [2] 121 Previous Answers Request Answer [3] [6] [3] [6] [3] [6] [4] ? [5] [4] [5] [4] [5] [10] [10] [10] 191 [7] [7] 121 [3] [6] [3] [6] [3] [6] [4] [5] [4] [5] [4] [5] H N S Br | P FWrite the best Lewis or Kekulé structure (showing all lone pairs of electrons, formal charges, and appropriate geometry – use wedge-dash where needed) for each of the following species given as condensed formulas: a) NH2- b) PO3H3 c) H2COH+ d) NaBH3CN e) C6H5MgBr f) CH3AlCl2
- 4. Circle the following pairs of structures that do not constitute resonance structures. For the proper resonance pairs, draw curved arrows to convert the first structure to the second. Draw in all lone pairs of electrons. H3C-CH3 „CH3 HgC-N' a) b) H2C=C=CH2 H3C-CECH FCH2 d) H3C' CH2 H H3C7. >., Draw three concise arrows in the structure below and then draw the resulting resonance structure.Curved arrows are used to illustrate the flow of electrons. Using the provided resonance structures, draw the curved electron-pushing arrows to show the interconversion between resonance hybrid contributors. Be sure to account for all bond- breaking and bond-making steps. Drawing Arrows :S: | :N:O KO Ø