What intermolecular forces are important for the molecule below? [Check all that apply.] HN, N. CH3 lon-Dipole Hydrogen Bonding O Dipole-Dipole London Dispersion Forces None of these
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![What intermolecular forces are important for the molecule below?
[Check all that apply.]
HN.
CH3
lon-Dipole
Hydrogen Bonding
Dipole-Dipole
London Dispersion Forces
None of these](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fde326383-8b00-4076-b3f6-1f860c5e4029%2Fdc468587-5f13-4617-9361-e55498386b8d%2Ff2j1uvc_processed.png&w=3840&q=75)
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- a.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 answerPick all of the molecules with a permanent net electric dipole : CHCl3, 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?
- Examine 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.It’s not dipole-dipole. Pls helpWhich molecule is expected to have the largest dispersion force? a)C3H8 b)F2 c)N2H4 d)C8H16
- Attraction between atoms to weak. 1. How would you describe the spacing between the atoms? Are the atoms free to move around? 2. What is the likely phase (solid, liquid, or gas) of the substance that is comprised of the atoms you have just described.Hello, I am currently working on intermolecular forces and have a question about a dye experiment I completed in class. In regards to the molecule attached, what is the strongest intermolecular force that it exhbits, and if it is not ion-dipole, why?why rotation across double bond is not possible?
- Hello. What is the difference between antibonding, nonbonding, and bonding molecular orbitals?Select the diatomic molecule below that has the highest boiling point. * F₂ Cl₂ Br₂ I₂Both 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
