Which molecule would you predict to have the strongest...

Which molecule would you predict to have the strongest intermolecular interactions? Skeletal structure Molar mass (g/mol) Density (g/mL) Melting point (°C) Dipole moment (D) A 180.2 1.4 136 6.5 OH CI B 173.6 1.6 105 5.2 OH O-N+O C 173.6 1.05 -7.5 3.85 D F F F S F F F 214.6 6.2 -64 0.0 HO E 152.1 1.1 81 2.6

Transcript

00:01 To determine the strongest intermolecular force that exists between two molecules, it's often helpful to draw the lewis structure.

00:10 If we draw the lewis structure for pf3, it's going to take on a trigonal, pyramidal, molecular geometry, or molecular shape.

00:27 Because of that, with fluorine being highly electronegative, the base of the pyramid, will be negative, the top of the pyramid will be positive.

00:40 Therefore, we will create a dipole.

00:44 So between the molecules, we will have a dipole, dipole, dipole, intermolecular force of attraction.

00:54 For the next molecule, we have c2h6.

01:01 Anytime we have a hydrocarbon, the difference in electronegativity, and the geometry of the hydrocarbon typically results in a non -polarer.

01:13 Molecule.

01:15 Because it is non -polar, we will just have london dispersion or vanderwals forces that occur between the molecules.

01:27 For the third one, we have cl2.

01:31 Its lewis structure is just cl cl.

01:34 So it is linear.

01:36 There is no polarity between the two chlorines because they have the same electronegativity.

01:44 So we also just have dispersion forces.

01:51 And then for the next one, we end up getting a hydrogen directly bonded to an oxygen.

02:02 And any time we have a hydrogen directly bonded to an oxygen, as shown here, we get hydrogen bonding between the molecules...

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