What intermolecular forces are important for the molecule below? [Check all that apply.] XeF4 Dipole-Dipole Hydrogen Bonding None of these lon-Dipole O London Dispersion Forces
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![What intermolecular forces are important for the molecule below?
[Check all that apply.]
XeF4
Dipole-Dipole
Hydrogen Bonding
None of these
lon-Dipole
London Dispersion Forces](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fde326383-8b00-4076-b3f6-1f860c5e4029%2F52c26403-c5b3-4815-9ad5-c641a6f3aa57%2F00w76ra_processed.png&w=3840&q=75)
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- Pick all of the molecules with a permanent net electric dipole : CHCl3, I2a.draw a wedge and dashed wedge structure (picture) of CH3Cl that best illustrates the geometry about the central atom shown in the picture. In the other box, draw another picture of the model from a different angle (viewpoint). b.In CH3Cl, are the three hydrogen atoms equivalent (i.e., do they have identical environments with respect to the other atoms adjacent to themselves)? Briefly explain the evidence for your answerBoth NH3, NCl3, and NF3 are all polar. Here is a data table with some additional information: Name Melting Point (°C) Boiling Point (°C) Molecular Geometry Nitrogen trihydride (ammonia) -77.7 -33.3 Trigonal Pyramidal Nitrogen trichloride -40.0 71.0 Trigonal Pyramidal Nitrogen trifluoride -207 -129 Trigonal Pyramidal Considering intermolecular forces, for what reason would nitrogen trichloride have such a high boiling point? choose one: 1.The molecular geometry makes it the most polar of the compounds 2.The larger mass and larger electron cloud means stronger LDF 3.It can participate in H-bonding 4.Unlike the other substances, it is polar. 5.The small mass means it takes less energy to break the IMF
- Which molecule is expected to have the largest dispersion force? a)C3H8 b)F2 c)N2H4 d)C8H16What types of intermolecular interactionsdoes chloroform (CH3Cl) exhibit?I) London dispersionII) dipole-dipoleIII) hydrogen bondingIV) covalent bondingRecall that chloroform is tetrahedralelctronic geometry with C as the central atom.1. II only2. II and III only3. II and IV only4. I and II only5. I, II, and III only1. 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
- 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…Select the diatomic molecule below that has the highest boiling point. * F₂ Cl₂ Br₂ I₂Answer each question and justify your answer by doing ALL of the following: • Identify the type of substance and important interparticle force(s) for both substances. − Explain how you know (substances and forces). − For each molecular substance, fully justify how you know if it is polar or nonpolar. Provide a Lewis structure, a geometry sketch, calculation of |ΔEN| values, and a discussion of symmetry. • Identify which of the two substances has stronger interparticle forces. If they have the same type of interparticle force, explain how you know which is stronger. • Answer the question by connecting the property asked about to strength of interparticle forces. • Use complete sentences, write all words out (no abbreviations) and be specific and complete with all explanations. Do not refer to any actual data. 10-3. Does CH4O or CH3F have the higher boiling point? 10-5. Does BaSO4 or KCN have the lower melting point?
- PLEASE ANSWER THHS ASAP Find the geometry, hybridization, polarity, and intermolecular forces in each molecule for those two molecules. 1. CBr4 and 2. SPFExamine the elements in the second row of the periodic table. Note that HF, H2O, NH3 and CH4 are sp3 hybridized. The first three are all capable of hydrogen bonding. Methane, however, is not capable of hydrogen bonding. Explain.For each determine… 1. Are these molecules non polar or polar? How did you determine this? 2. Draw any molecule dipoles in all structures if any .
