Why are ducks waterproof? It’s because they produce copious amounts of oils from their uropygial glands and spread it across their feathers. In this exercise, we’ll be investigating the molecular structure of one of these preen oils to determine how it keeps ducks dry. D Question 2This molecule is mostly nonpolar overall, butthe electrons are not perfectly evenlydistributed. On the structure of preen oilabove, identify where the electron densitywill most likely be concentrated. Explain howyou know which atoms will have moreelectron density than the rest of themolecule.H2H2H2H2H2H2H2C-CH3H2Molecule AH3CH2H2H2H2H2H2H2 Question 1To investigate preen oil further, you'veisolated two compounds from the uropygialgland of a common wood duck. Preen oilmust be quite non-polar, if it is to repelwater. Of the two molecules you've isolated,which one do you think is more likely to bepreen oil? Explain how you identified thepreen oil compound.H2C-H2H2H2H2H2H2Molecule ACH3H3CH2H2H2H2H2HH2N IHOMolecule BH.fo

Answer 1: since molecule A seems to a large number of non polar hydrocarbon chain so it could be…

Question 1 To investigate preen oil further, you've isolated two compounds from the uropygial gland of a common wood duck. Preen oil must be quite non-polar, if it is to repel water. Of the two molecules you've isolated, which one do you think is more likely to be preen oil? Explain how you identified the preen oil compound. H2 H2 с. H2 H2 H2 H2 H2 H2 .C C-CHS Molecule A H3C H2 H2 H2 H2 H2 H2 H2 H2N. OH Molecule B H fu

Question 1 To investigate preen oil further, you've isolated two compounds from the uropygial gland of a common wood duck. Preen oil must be quite non-polar, if it is to repel water. Of the two molecules you've isolated, which one do you think is more likely to be preen oil? Explain how you identified the preen oil compound. H2 H2 с. H2 H2 H2 H2 H2 H2 .C C-CHS Molecule A H3C H2 H2 H2 H2 H2 H2 H2 H2N. OH Molecule B H fu

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter23: Carbon: Not Just Another Element

Section: Chapter Questions

Problem 66PS

See similar textbooks

Similar questions

Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF Propane, CH3CH2CH3 Heptane, CH3(CH2)5CH3 Propanol, CH3CH2CH2OH Heptanol, CH3(CH2)6OH For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line to show any H-bonding
I need answer for question 2.3 1. Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMFa. Propane, CH3CH2CH3b. Heptane, CH3(CH2)5CH3 c. Propanol, CH3CH2CH2OH d. Heptanol, CH3(CH2)6OH2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line to show any H-bonding.3. For each compound, consider whether or not any polar bonds are presenta. Use a different coloured pen to identify any polar bondsb. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning4. Compare your drawings for propanol and heptanol.a. Which compound has stronger dispersion forces? Explain your answerb. Which compound has a higher boiling point? Explain your answer5. Compare your drawings of heptanes and heptanola. Which compound is more polar? Explain your answerb. Which compound is more soluble in water? Explain your answer
I need helping solving these and their are 2 more questions within this problem as well but I couldn't upload all The last two are: What is the C−C−C bond angle in propene? 109.5° 180° 90° 120° Does propene have an overall two‑dimensional shape or three‑dimensional shape? three‑dimensional two‑dimensional
1. Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF.a. Propane, CH 3 CH 2 CH 3b. Heptane, CH 3 (CH 2 ) 5 CH 3c. Propanol, CH 3 CH 2 CH 2 OHd. Heptanol, CH 3 (CH 2 ) 6 OH2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed lineto show any H-bonding.3. For each compound, consider whether or not any polar bonds are present.a. Use a different coloured pen to identify any polar bondsb. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning4. Compare your drawings for propanol and heptanol.a. Which compound has stronger dispersion forces? Explain your answer.b. Which compound has a higher boiling point? Explain your answer.5. Compare your drawings of heptane and heptanol.a. Which compound is more polar? Explain your answer.b. Which compound is more soluble in water? Explain your answer Analysis:1. Which compound has higher solubility in water?a. A polar compound or a…
Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF Propane, CH3CH2CH3 Heptane, CH3(CH2)5CH3 Propanol, CH3CH2CH2OH Heptanol, CH3(CH2)6OH For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line to show any H-bonding. For each compound, consider whether or not any polar bonds are present Use a different coloured pen to identify any polar bonds Which compounds are polar? Which compounds are nonpolar? Explain your reasoning Compare your drawings for propanol and heptanol. Which compound has stronger dispersion forces? Explain your answer Which compound has a higher boiling point? Explain your answer Compare your drawings of heptanes and heptanol Which compound is more polar? Explain your answer Which compound is more soluble in water? Explain your answer
#3 Solve the problem, please read directions carefully. Thumbs up if you do it correctly.
Question 1: Predict the structures for the following molecule: XeOF2, ClOF3, SOCl2
Give only typing answer with explanation and conclusion Consider the compounds below. First, identify if the compound is covalent or ionic. If covalent, identify the intermolecular forces that compound will have. Then, rank them based on their melting point – with 1 being highest, 5 being lowest. NaBr LiF H2S C2H6 H2O
draw the 3d model of the molecule CH3CH2CH2C[triplebond]CCH2CH2CH3 from the view of the triple bonded C atoms. Not sure if I drew the appropriate hydrogens needed on the Carbons that have the triple bond?
1.) Circle and label all of the non-alkane functional groups in the molecule shown below. Be as specific as possible (use 1o, 2o and 3o to describe amines and amides). 2.) Draw the line angle structure for the molecule in the box.
Which of the following is a non-polar molecule, but contains polar bonds? Group of answer choices H2S CH2F2 NH3 XeCl4
Is the answer to this question II? It cannot be I or III because there are two oxygen molecules, and then it cannot be IV because there are six carbons only, I think - three in the pentagon ring, then plus three more with one pair of carbons double bonded?