Structure- Data! Redraw Original Structure and Add Lone Pairs Redraw Original Structure with Lone Pairs and Add Curved Arrows to Neutralize as Many Formal Charges as Possible Draw Resonance Structure That Follows From Curved Arrows Drawn Above Which Resonance Structure is Lower Energy (Original or Yours)? Why? НО. 00 OH CH3 OH OH
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- 1. Add nonbonding electron pairs to each atom where it is implied by the line-angle drawings shown below. 2. Use the curved arrow formalism to generate four additional, valid resonance structures for each compound. 3. Rank your resonance structures in order of increasing contribution to the overall nature of the molecule.Draw the skeletal (line-bond) structure of [CH₃CH₂CHC(O)CH₂CH₂CH₃]⁻. Include all lone pairs and charges as appropriate. What do the brackets and the - exponent mean for this formula?For the following molecules:I. Draw the best Lewis Dot Structures for each of the following molecules. The best structuretakes into consideration resonance structures, calculations of formal charge for each atom,and tries to minimize the overall formal charge for the structure. II. Draw the 3-D VSEPR structures for the following molecules. You may combine these twodrawings (for I and II) into 1 drawing if you wish. III. Label the bond angles. IV. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) foreach molecule. V. State the hybridization around each central atom in the molecule. VI. State whether the overall molecule is polar or nonpolar. VII. For any two of the following molecules, state the strongest intermolecular force betweenmultiple of the same molecule.a. IF2b. H2CO3c. CH3CH2COOHd. N2O4e. PO4^3-f. CH3COCNg. ClO3^-1h. C4H8
- Draw two significant resonance structures for the molecule below (start at the same site of instability for both). Only one lone pair and formal charge are provided; provide any formal charges and lone pairs that are missing on the original structure and on your resonance forms. Make sure to draw curved arrows correctly (starting from a bond/lone pair) and be very clear where the head of the arrow is pointing. Finally, rank them from most stable to least stable and justify your choices. The skeleton for your resonance is provided.Assign the correct formal charge to the oxygen atom in this structure (you may right click on the atom and use the Charge menu, or use the + and - buttons on the graphical toolbar). Once the correct formal charges have been placed, identify all atoms with a reasonable formal charge by setting the map number to 1, and those with an unreasonably large formal charge by setting the map number to 2. HINT: all of the hydrogen atoms are already shown.Which of the following structure(s) have proper formal chargers and the correct number of bonds for each atom?
- Consider this “Dr. Yan’s imaginary” molecule below in line-angle formula. Note that you MAY NOT add or remove lone pairs. How many CH groups are there in the molecule? ____________ b) The formal charge of O is:__________; and the formal charge of N is: ____________________ c) The overall charge of the molecule: ___________Please show all steps and I will upvote if correct. According to the Walsh diagram, why is NH3 pyramidal while BH3 is planar? Which molecule should have the smallest bond angle ~ NH3, PH3, or AsH3? Think of electronegativity differences and the Walsh diagrams of these molecules.Which of the following species (B, C,D) is a valid resonance of A? Use curved arrows to show how A is converted to any valid resonance structure.
- synthesized compound and wants to determine its molecular structure. However, due to the compound's highly reactive nature, it cannot be isolated in pure form for traditional spectroscopic analysis. The chemist decides to perform computational simulations to predict the compound's molecular structure and properties. Discuss the challenges and limitations associated with this approach.Explain the Below fact ? A “better” resonance structure is one that has more bonds and fewercharges.For the following species: a) draw the resonance structures (include in parentheses the total number of reasonable resonance structures); b) show with curved arrows the movement of electrons that occurred in a resonant form to obtain the resonant form that follows c) circle the structure(s) that contribute the most to the hybrid; d) draw the resonance hybrid (please give clear handwritten solution)