Classify the following compounds based on the type of intermolecular interactions: hydrogen  bond/London dispersion force/dipole-dipole interaction  H2O _______________________  CH4 _______________________  CH3CH2OH ________________________

List the molecules in decrease strength of intermolecular forces. (So the strongest intermolecular forces should be matched to 1 and the weakest to 4).      CH4     He     NH3     H2CO

1. Which of the following exhibit hydrogen bonding? a. HI b. H₂ c. H₂O₂ wing infor 93.17 mm Hg

match with following Highest vapor pressure2nd highest vapor pressure2nd lowest vapor pressureLowest vapor pressure   PH3CO2CH3CH2OHC5H12

Consider the following experimental boiling points: CH4: -162°C C3Hg: -42°C C6H14: 69°C C9H20: 151°C Which of the following statements is correct for this set of compounds and supported by the data given? Select as many as applicable Select one or more: The molecule with the strongest intermolecular forces is C9H20 The C-C bond is the strongest covalent bond among the four molecules The dominant effect behind this trend is the strength of dipole/dipole forces OCH4 is the most polarizable molecule of the four C9H₂0 is the most polarizable molecule of the four The dominant effect behind this trend is the strength of dispersion forces

Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.Group of answer choices C4H10 CCl4 CH3NH2 NaBr CH2Br2

Looking at the structure of the following molecule determine which intermolecular forces it exhibits. H | CH3 H | | H-C-C-C-H | | | HH H London Forces Dipole-Dipole Hydrogen Bonding lonic Attractions

Decide which intermolecular forces act between the molecules of each compound in the table below. compound 1₂ iodine water CHA methane carbon monoxide intermolecular forces (check all that apply) dispersion dipole hydrogen-bonding ▬ L 0 X

Identify the main intermolecular attraction in the following molecule: (attached file) ionic bonding dipole-dipole ion-dipole hydrogen bonding London dispersion

Bromine (Br2) is a liquid at room temperature. What is the attractive force that exists among Br2 molecules in the liquid? Hydrogen bond attraction dipole-dipole rejections London dispersion forces dipole-dipole attractions O O O