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- Draw a valid Lewis structure for each compound. a. Ng b. (CH,OH)* (CH;CH2) d. HNNH е. НаBN C.Assign formal charges to each carbon atom in the given species. All lone pairs have been drawn in. нн a. CH2=CH b. H-с-н с. Н-с-н d. H-С-С H H e. -N: f. g. h. :N=N=N: -N=O:Consider tne pairs oI SIruciures snown. H. H. А. and H. CH3 CH3 В. and H. :O: and H3C H. H2C D. CH3CH,* and *CH2CH3 Which structures are resonance structures to each other? pair A pair B pair C nair D :O: C.
- Draw a second resonance structure for each species. a. CH3-C=C-C-CH3 b. CH3-C-CH3 CI: HHH c. H-C=C-CI: HHc. There is a total of five resonance structures (including the original structure). : OHAssign formal charges to each carbon atom in the given species. All lone pairs have been drawn in. нн a. CH2=CH b. н-с-н с. Н-с-н d. H-Ć-Č нн H e. f. N=N=N: g h. or -N=Q:
- Consider the compounds and ions with curved arrows drawn below. When the curved arrows give a second valid resonance structure, draw the resonance structure. When the curved arrows generate an invalid Lewis structure, explain why the structure is unacceptable. c. CH;CH2-CEN: a. b. d.8. Compute for the formal charge (FC) on each atom in the following compounds. a. H3N - BH3 b. [H2CNH2]+ c. H3O+ d. HCO3- 9. Draw Lewis structures for the following compounds, showing an appropriate formal charges. a. [CH3OH2]+ b. [HONH3]+ c. NaBH3CN d. CH3NH3+ 10. For each of the following compounds, draw the important resonance forms. Indicate which structures are major and minor contributors or whether they would have the same energy. a. [CH3OCH2]+ b. H2SO4 c. CO3-2 d. H2C=CH-+CH2 e. [CH3C(OCH3)2 ]+ 11. Draw the complete Lewis structures for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)28. Compute for the formal charge (FC) on each atom in the following compounds. a. H3N - BH3 b. [H2CNH2]+ c. H3O+ d. HCO3- 9. Draw Lewis structures for the following compounds, showing an appropriate formal charges. a. [CH3OH2]+ b. [HONH3]+ c. NaBH3CN d. CH3NH3+ 10. For each of the following compounds, draw the important resonance forms. Indicate which structures are major and minor contributors or whether they would have the same energy. a. [CH3OCH2]+ b. H2SO4 c. CO3-2 d. H2C=CH-+CH2 e. [CH3C(OCH3)2 ]+ 11. Draw the complete Lewis structures for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)2 b. CH3CH2COCN c. (CH3)3CCOCHCH2 d. (CH3CH2)2CO e. (CH3)2CHCH2Cl 12. Draw the line-angle formula for the following condensed structural formulas. a. CH3(CH2)3CH(CH3)2 b. CH3CH2COCN c. (CH3)3CCOCHCH2 d. (CH3CH2)2CO e. (CH3)2CHCH2Cl
- Draw all resonance structures for the following molecules. -S=0 CF3 a. b.Label the resonance structures in each pair as major, minor, or equal contributors to the hybrid. Then draw the hybrid. a. CH3-C-N-CH3 I HH CH3-C=N-CH3 HH b. CHg=c&l, H CH₂-C=CH₂ HProvide all reasonable resonance structures for each molecular structure below. Use curved arrows to show how electrons are moved and dont forget lone pairs. E 1. CH3 CNO E2. CHỌN -1 NCO E3. CHOCN E +1 4. O C S E5. N = N = O E1. CH CNO E2. CH3NCO E3. CH₂OCN E4. O-C-S E5. N-1=N+1=0 E6. CH H₂O