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- Using your model of butane (CH3CH2CH2CH3) , complete the following graph of the anglebetween the two Me groups vs. potential energy. a. Label each Newman projection of butane on the graph with the words staggered, eclipsed, gauche, and anti, as appropriate. (Note that some structures will have more than one label.) b. Draw a wedge and dash bond representation of butane in its lowest P.E. conformation.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.name the following compounds. only need part q, j and r
- pls help ASAP! “which term best describes the relationship between the following two molecules?”Molecular formula. Molar mass (g.mol-1). ΔcH0 (kJ.mol-1) Petrol C8H18 * 114 - 5470 Diesel C20H42 * 282 - 8090 Natural gas. CH4 16 - 890 Hydrogen. H2 2 - 286 Methanol. CH3OH 32 - 726 *Petrol and diesel are complex mixtures of hydrocarbons. On average, their properties resemble those of C8H18 and C20H42, respectively. 1.1) Calculate the energy density (in kJ.g-1) for all the fuels in the table above. Use the molar masses supplied in the table. 1.2) Why would you say that Space Shuttles rather use hydrogen as its primary fuel source instead of one of the other fuels in the table? 1.3) Formula 1 racing cars use petrol as their fuel source. In the USA, “Indy cars” use methanol as fuel source and in South Africa farmers use diesel as fuel source for their tractors. If all these motors perform equally optimally, which vehicle is the most fuel efficient? Give a reason for your answer.Between 1865 and 1890, other possible structures were proposed for benzene, such as those shown here. Considering what nineteenth-century chemists knew about benzene, which is a better proposal for benzene’s structure: Dewar benzene or Ladenburg benzene? Why?
- I need to indicate how the first resonance structure (the one with #4 above it) turns into the second one with arrows, but I cannot figure it out.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.Using your general knowledge of periodic trends in electronegativity, predict whether the C=O bond and the C-H bonds in formaldehyde will be strongly polar, weakly polar or nonpolar. Calculate the electronegativity difference ΔχO-C across the C=O bond and the electronegativity difference ΔχC-H to confirm or correct your predictions. For any strongly polar bond(s) on the molecule, draw the bond dipole moment adjacent to the bond in the VSEPR structure above, using crossed arrow notation to show the direction of the positive and negative bond dipoles. Predict whether the overall molecule should be polar or nonpolar. ___________________ Explain your reasoning below. If the overall molecule is polar, draw the net dipole next to the molecule, using crossed arrow notation to indicate the direction of the dipole.
- Construct models of the following generalized formula: a. Model 1: CH4 b. Model 2: CH3Cl c. Model 3: CH2ClBr d. Model 4: CHClBrFWhich of these formulas is(are) not valid for octane? A. C8H18B. C8H20C. C8H16D. CH3CH2CH2CH2CH2CH2CH2CH3E. CH3(CH2)6 CH31. 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.