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- Create 3 different lewis structures that are not resonance structures for a compound. Note that the compound much have 4 carbon atoms, 1 oxygen atom, 1 nitrogen atom, 6-10 hydrogen atoms. The formula for the 3 compounds do not need to be exactly the same. Consider also: 1st compound: There must be 1 carbon atom with tetrahedral geometry around it. 2nd compound: There must be 1 carbon with trigonal planar geometry 3rd compound: There must be 1 carbon with linear geometry around it. Encircle those carbons mentioned. Make sure that lone pairs are visible.2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction, Preferred Molecular Compound Electron Dipole Reason Geometry Moment (Polarity) geometry SF4 BRF3 XeF4 3. Using the Lewis structure predict the geometrical structures of the following ions and state the hybridization of the central atom. Ion Electron Geometry Molecular Formal Charge Central Atom Geometry of Central Hybridization Atom CO32- NO3- BF44. Draw the complete Lewis structures showing all valence electrons, all atoms, all charges, all resonance forms for the molecules or species where appropriate. Show the best structure based on formal charge considerations. Supply the information requested. Water Ethanol (CH3CH₂OH) H-O-H Bond Angle Electronic Geometry of O atom Formate Ion (HCO₂¹) Carbon dioxide Electronic Geometry of C atom Hybridization of the C
- 2. Consider the resonance structures below may only A C. yongary] B C D a. On each structure (A-D) show all lone pair electrons. b. Provide arrows that show electron movement from A to B, B to C, and C to D. Which is the "most contributing” resonance form (A, B, C, or D)? Explain your choice. d. Draw the resonance hybrid for this molecule (use “delta” 8+ or - to show partial charges).Fill in the table. Central atom is listed first. A. Write the number of valence electrons below the formulaB. Draw the Lewis structureC & D. Write the Electron Group Geometry and Molecular Shape NamesE. Write the bond angleF. Write the molecular polarity. "P" for polar and "NP" for nonpolar. SpeciesValenceElectrons(1 pt.) LewisStructure(2 pt.) Electron PairGeometryName(1 pt.) Molecular ShapeName (1 pts.) BondAngle (1 pt.) Molecular Polarity(1 pt.) PO43- NOBr UploadQuestions 6a, b, c, d is linked to one another and focus on the molecule shown below. H ба) Before we can start assigning hybridization, we need to correctly assign our VSEPR electron-pair geometries to each central atom. For each of the chosen central atom, match it with it's corresponding electron-pair geometry. Drag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE V C1 trigonal planar c C2 linear O N1 tetrahedral C trigonal pyramidal N 01 tetrahedral N trigonal planar o Bent O tetrahedral O :0: :0= II II I-0 - -I I-z: I
- Draw Lewis structures and assign formal charges for the following compounds and ions. Note any resonance forms and explain which resonance form is the most important. Make a note of any other unusual features (such as "this one doesn't work" and why- what are the shortcomings of the model.) CO3²- CO NO₂ CNO (include isomers) Al₂Cl6 B₂H6 O2 (paramagnetic) H3O+ LiF IF78. 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
- For the formula CH2CF2, "draw the Lewis structure in your work (.. PAfter drawing the complete Lewis structure, type in the shape, bond angle, etc. for each blank. What is the molecular shape or geometry for the carbon on the left (the C in CH2)? trigonal planer What is the molecular shape or geometry for the carbon on the right (the C in CF2)? trigonal planer What is the bond angle for the carbon on the left (the C in CH2)? Type in a plain number, but include a "<" sign in front of the number if applicable. What is the bond angle for the carbon on the right (the C in CF2)? Type in a plain number, but include a "<" sign in front of the number if applicable. What is the hybridization for the carbon on the left (the C in CH2)? Type this in without any superscript, for instance sp3 would be typed as "sp3". What is the hybridization for the carbon on the right (the C in CF2)? Type this in without any superscript, for instance sp would be typed as "sp3". Is the molecule overall polar or…Rank the three bonds, A (carbon-carbon), B (oxygen-hydrogen) and C (carbon- hydrogen) indicated by the arrows in the structure below in order of increasing bond dissociation energy (not all H atoms are included in the line-angle structure). Hint: Comparing C-H and O-H the difference is electronegativity, comparing C-H and C- C is the difference in atomic size. A H3C. H3C H A8. Draw all resonance structures of the following compounds. Show electron-pushing arrows. For each, which resonance structure contributes the most to the resonance hybrid? NHSEE MORE QUESTIONS