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![What intermolecular forces are important for the molecule below?
[Check all that apply.]
CH3F
London Dispersion Forces
Dipole-Dipole
None
Hydrogen Bonding
lon-Dipole](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fde326383-8b00-4076-b3f6-1f860c5e4029%2Fbf289c39-a53a-4548-9061-c5c31b8444a9%2Flnk824s_processed.png&w=3840&q=75)
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- Identify what type of intermolecular forces exist between the following pairs. ( I already anwer it but I am not sure with my answers Please check my answer and correct it if it wrong. Thank you!) HBr and H₂S Answer: Dipole-dipole Cl₂ and CBr₄ Answer: London dispersion forces I₂ and NO₃¹⁻ Answer: Dipole-induced dipole NH₃ and C₆H₆ Answer: Ion- induced dipoleAttraction 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.Pick all of the molecules with a permanent net electric dipole : CHCl3, I2
- Which compound(s) exhibit(s) dipole-dipole forces? (hint: draw the lewis structures) 1. BCl3 3. NF3 2. XeF2 4. OCl2 a. 3 only b. 2, 3, and 4 c. 1 and 2 d. 3 and 4Rank the forces overall of methane, methanol and water (IMF: dispersion, dipole-dipole, hydrogen-bonding)TRUE OR FALSE 1. molecules with temporary dipole moment tend to align with opposite polarities in the solid phase for maximum attractive attraction. 2.the boiling point of compounds containing elements in the same periodic group is inversely proportional to the elements molar mass. 3.when adhesion is greater than cohesion, a convex appearance of the liquid in a tube is evident. 4.when cohesion is greater than adhesion, a concave appearance of the liquid in tube is evident.
- I need help with this question please. Also, my other question was, What intermolecular forces does Phosphorous Trifluoride (PF3) exhibit?Which molecule(s) will experience the Hydrogen Bonding force? Select all that apply. Group of answer choices: A) H2O B) NH3 C) H2 D) N2the strongest IMF present between molecules of each compound. CS2 [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion CH2O [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion HF [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion MgF2 [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion
- 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.Which of the following will show lowest surface tension? A. CH3CH2CH2OH B. CH3OH C. OHCH2CH2OH D. CH3CH2Br E. CH3CH2CH2CH2CH3What is the strongest interparticle force in each of the following substances?a) CH3Clhydrogen bondingdipole―dipoledispersion(b) CH3CH3dipole―dipoledispersionhydrogen bondingc) NH3hydrogen bondingdispersiondipole―dipole